# Moringa oleifera Leaf Extract-Mediated Green Synthesis of Nanostructured Alkaline Earth Oxide (MgO) and Its Physicochemical Properties

Authors: Archana Venkatachalam; Joseph Prince Jesuraj; kalainathan Sivaperuman
Journal: Journal of Chemistry
 (2021)

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## Abstract

The magnesium oxide nanoparticles (MgO NPs) were prepared fromMoringa oleifera leaf extract. Phytochemicals are derived from plant extract which are served as stabilizing and capping agents. This green route has been attracted owing to speed, reliable, and eco-friendly and cost-effective one. The synthesized magnesium oxide nanoparticles were taken into three different calcination temperatures (500, 600, and 700°C). The powder X-ray diffraction (PXRD) study shows a pure phase of face-centered cubic structure. Periclase MgO nanoparticles were prepared. The optical band gap of MgO nanoparticles is 4.5 eV, and its absorption in the UV region was observed by UV-visible spectroscopy (UV-Vis). Photoluminescence spectra have exhibited multicolor emissions were being at UV and visible region due to defect centers (F centers) of MgO nanoparticles. EDX (energy dispersive X-ray spectrum) has given the stoichiometric ratio of Mg and O. The functional groups have been studied by Fourier transformed infrared spectroscopy (FTIR), surface morphology transformation has been identified by scanning electron microscopy (SEM) studies, and VSM measurements have given the information of diamagnetic nature of MgO nanoparticles. H-R TEM micrographs have confirmed that particles were in nanorange matched with XRD report. Polycrystalline nature has been observed pattern information. TG-DSC characterization revealed phase transition and weight loss information. D-band and G-band of MgO nanoparticles are studied by micro-Raman analysis. Dielectric analysis has proven that MgO nanoparticles will be a promising candidate for linear dielectric ceramics, thermistor. The present resent studies have revealed that MgO powder will be an economical and promising candidate in superconductor, optoelectronic device, and energy storage applications.


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## Body

## 1. Introduction

Metal oxides are widely employed as catalysts, optical devices, sensors, thermal conductivity enhancers, and energy conversion devices [1–10]. Engineered nanomaterials have unique properties which can be tailored with shape and size, and morphology leads to outstanding properties which are limited to bulk materials. A variety of different structured metal oxides are nanoparticles, wires, tubes, fibers, whiskers, films, layers, triangles, and tetra pods which are most desired structures widely used in technical applications, and its unique structural features are large surface-to-volume ratio, cations with valence states, anions with deficiencies, and depletion of carriers [1]. Magnesium oxides are alkaline earth-based oxide metal is attraction owing to its high economical availability, toxicity, and eco-friendly nature, has been used as inorganic phosphor for optoelectronic devices, biosensors, catalyst. Owing to their defect-induced luminescent property is widely used as solid-state devices [1]. MgO is the wide band gap insulator and smooth surface features due to this property, and it has been used as sensors, refractory, paint, toxic waste remediation, and superconductors [1].Phytochemical-mediated synthesis is a green route which has great attention due to novel strategies and alternative to physical and chemical methods [11]. In this type of bottom-up approach, where the phytochemicals are stabilized and capped with the metal oxide nanoparticles, the reducing agents involved in nanoparticle synthesis are alkaloids, phenolic compounds, terpenoids, and coenzymes [12]. Biosynthesis route employs simple prokaryotic bacteria to eukaryotes such as fungi, plants, and biogreen synthesis which have a better advantage while comparing microorganisms wherein plant-mediated synthesis is the one-step synthesis, but owing to mutation microorganisms over time, they may lose their ability to synthesize nanoparticles and it is very laborious and time-consuming [13]. Plant-mediated synthesis is the one-step protocol and safe; hence, research on plants has expanded rapidly [11, 14, 15]. Plants as a biological agent served as reducing and capping agents involved in the synthesis process and are eco-friendly [16, 17]. Every part of the plant can be used for nanoparticle synthesis such as leaves of the plant, stem, straw, flower, and root [16–22]. Here, extracellular methods had been used for the synthesis of nanoparticles which include the use of leaf extract prepared by boiling or crushing of leaves [23–25]. Nanoparticle synthesis using a plant system is the current scenario. Plant-mediated synthesis is not only used for environmental impact but also used to produce large quantities of contaminated free nanoparticles with well-defined morphology and size [26]. The characteristics of the nanoparticles have been influenced by the source of the plant extract because different extracts contain different concentrations and combinations of organic reducing agents, a plant extract-mediated bioreduction involves mixing the aqueous extract with an aqueous solution of the relevant metal salt at room temperature, and it has been completed within a few minutes [12, 27, 28].Biogreen MgO nanoparticles which had been synthesized from various leaves, fruit, and seed have been reported here. Magnesium oxide nanoparticles were synthesized fromClitoria ternatea leaf extract [29], orange fruit waste [30], citrus lemon leaf extract [31], Brassica oleracea and Punica granatum peels [32], Swertia chirayita [33], neem leaf extract [34], Aloe vera extract [35], seeds of Lepidium sativum [36], aqueous leaf extracts of Psidium guajava (P. guajava) [37], Nephelium lappaceum L. peel extract [38], Amaranthus tricolor, Andrographis paniculata and Amaranthus blitum [39], aqueous leaf extracts of betel [30], Artemisia abrotanum herb water extract [40], Parthenium plant extract [41], and fruit extract (Emblica officinalis) [42]. Biosynthesis of magnesium oxide nanoparticles using leaf extract in the present scenario has been reported here. The aqueous magnesium ions when exposed to Moringa oleifera leaf extract are reduced, and magnesium oxide nanoparticles formed. The plant is belonging to the Moringaceae family, and it is distinguished by parietal placentation, 3-valved fruit, elongated, nondehiscent berry and winged seeds, and a medium-sized tree. The botanical name of the tree is Moringa oleifera Lam., and the family consists of the single genus Moringa [43]. It is widely available in India, and it is an essential dietary ingredient of Indian food. The plant contains minerals, proteins, vitamins, amino acids, and phenolics and provides a rich and rare combination of zeatin, quercetin, β-sitosterol, caffeoylquinic acid, and kaempferol. The leaves contain concentrations of ascorbic acid, oestrogenic substances [44], iron, calcium, phosphorus, copper, vitamins A, B, and C, α-tocopherol, riboflavin, nicotinic acid, folic acid, pyridoxine, β-carotene, protein, and in particular essential amino acids such as methionine, cysteine, tryptophan, and lysine [45]. Silver, nickel, and zinc oxide metal nanoparticles had been synthesized from Moringa oleifera leaf extract. Magnesium oxide nanoparticles have not been reported so as per our knowledge. Herein, a simple and economical procedure has adopted for synthesizing nanostructured MgO using an aqueous leaf extract of Moringa oleifera. To the best of our knowledge, this is the first report to use of an aqueous leaf extract of Moringa oleifera for synthesis of MgO nanoparticles. The prepared MgO nanoparticles are characterized using spectroscopic and microscopic techniques. The thermal, magnetic, and dielectric properties of the prepared MgO nanoparticles have also been studied.


## 2. Materials and Methods

### 2.1. Material Collection

Homely grownMoringa oleifera leaves had been collected. All the chemicals were purchased from Merck that can be used without further purification (MgCl2.6H2O, and NaOH). The chemicals were used here with AR grade with 98% of purity. All aqueous solutions were prepared with double distilled water.


### 2.2.Moringa oleifera Leaf Extract Preparation Method

Freshly collectedMoringa oleifera leaves were washed thoroughly with double distilled water to remove dust particles, weighed, and transferred into the round bottom flask, and it was mixed with water and refluxed for 40 minutes at 70 degrees at the heating mantle. Then, the extract was filtered by Whatman filter paper (No.1) with several times and kept in sterile bottles under refrigerated conditions for the future use. Moringa oleifera leaves and extract are shown in Figures 1(a) and 1(b).Figure 1
Moringa oleifera leaves (a) and aqueous Moringa oleifera leaf extract (b).
(a)(b)


### 2.3.Moringa oleifera Leaf Extract-Mediated Preparation of MgO NPs

In phytochemical-mediated synthesis of MgO NP fabrication, the extract ofMoringa oleifera leaf extract (capping and stabilizing agent) was added to the aqueous solution of MgCl2.6H2O and stirred vigorously at room temperature, and then few drops of NaOH are added under stirring for maintaining appropriate PH which could be acted as a precipitating agent. The transparent solution changed to yellowish color. After 6 hours, the stirred process was completed, precipitation obtained which was yellowish color colloidal particles at the bottom of the flash which indicates the formation of Mg (OH)2 is shown in Figures 2(a) and 2(b). Then, the colloidal solution was centrifuged several times at 4000 rpm for 15 minutes and washed several times with double distilled water and ethanol to remove impurities. After the washing process, the supernatant was collected and dried overnight in a hot air oven at 70-degree Celsius. The dried samples of Mg (OH)2 were crushed and grounded by mortar and pestle. The grounded samples were calcinated in a muffle furnace at different temperatures at 500, 600, and 700°C for three hours for dehydration, the impurities were removed, and finally, white-colored MgO nanoparticles were obtained as shown in Figure 2(c). The mechanism of synthesis of MgO nanoparticles is illustrated in Figure 3.Figure 2
Mg (OH)2 nanoparticle (a, b) and MgO nanopowder (c).
(a)(b)(c)Figure 3
Mechanism of synthesis of MgO nanoparticles.


## 2.1. Material Collection

Homely grownMoringa oleifera leaves had been collected. All the chemicals were purchased from Merck that can be used without further purification (MgCl2.6H2O, and NaOH). The chemicals were used here with AR grade with 98% of purity. All aqueous solutions were prepared with double distilled water.


## 2.2.Moringa oleifera Leaf Extract Preparation Method

Freshly collectedMoringa oleifera leaves were washed thoroughly with double distilled water to remove dust particles, weighed, and transferred into the round bottom flask, and it was mixed with water and refluxed for 40 minutes at 70 degrees at the heating mantle. Then, the extract was filtered by Whatman filter paper (No.1) with several times and kept in sterile bottles under refrigerated conditions for the future use. Moringa oleifera leaves and extract are shown in Figures 1(a) and 1(b).Figure 1
Moringa oleifera leaves (a) and aqueous Moringa oleifera leaf extract (b).
(a)(b)


## 2.3.Moringa oleifera Leaf Extract-Mediated Preparation of MgO NPs

In phytochemical-mediated synthesis of MgO NP fabrication, the extract ofMoringa oleifera leaf extract (capping and stabilizing agent) was added to the aqueous solution of MgCl2.6H2O and stirred vigorously at room temperature, and then few drops of NaOH are added under stirring for maintaining appropriate PH which could be acted as a precipitating agent. The transparent solution changed to yellowish color. After 6 hours, the stirred process was completed, precipitation obtained which was yellowish color colloidal particles at the bottom of the flash which indicates the formation of Mg (OH)2 is shown in Figures 2(a) and 2(b). Then, the colloidal solution was centrifuged several times at 4000 rpm for 15 minutes and washed several times with double distilled water and ethanol to remove impurities. After the washing process, the supernatant was collected and dried overnight in a hot air oven at 70-degree Celsius. The dried samples of Mg (OH)2 were crushed and grounded by mortar and pestle. The grounded samples were calcinated in a muffle furnace at different temperatures at 500, 600, and 700°C for three hours for dehydration, the impurities were removed, and finally, white-colored MgO nanoparticles were obtained as shown in Figure 2(c). The mechanism of synthesis of MgO nanoparticles is illustrated in Figure 3.Figure 2
Mg (OH)2 nanoparticle (a, b) and MgO nanopowder (c).
(a)(b)(c)Figure 3
Mechanism of synthesis of MgO nanoparticles.


## 3. Material Characterization and Instrumentation

The calcinated MgO nanoparticles were analyzed with PAN analytical X’Pert PRO powder X-ray diffractometer with a CuKα radiation operated at 40 kV and 30 mA and the wavelength of λ = 1.54060 Å in the range 2θ = 10–80°. The photoluminescence spectra of MgO nanoparticles studied with 300–700 nm regions were recorded with Varian Cary Eclipse photoluminescence spectra photometer at room temperature with an excitation wavelength of 320 nm. UV-visible spectroscopic studies have been done by a Shimadzu dual-beam spectrometer. The size of the nanoparticle has been determined by transmission electron microscope (TEM) (FEI Tecnai 20) accelerated at 200 kv, morphology of the MgO was studied by using scanning electron microscope (SEM) (JEOL JSM 6390), and elemental analysis was done by energy dispersive X-ray analysis (EDS) which is attached with SEM X-ray column along with SEM images of nanoparticles. The functional groups were found by the Fourier transform infrared spectrum (FTIR) spectrophotometer (PerklinElmer spectrometer) using KBr pellets in the spectral range 4000–400 cm−1. Magnetic properties were investigated and performed at room temperature where the vibrating sample magnetometer model is employed and here applied magnetic field sleeping from −15000 to +15000 (Lakeshore, USA, model 740 equipped with magnetic field 2.17 T). Thermal properties were analyzed by thermal analyzer NETZSCH STA 449 F3 Jupiter which performs simultaneous TG-DSC measurement on the sample. Dielectric properties were characterized by an AC impedance spectroscopy and dielectric analysis using HIOKI 3532–50 LCR Hi TESTER meter in the frequency range of 50 Hz–5 MHz.


## 4. Results and Discussion

### 4.1. Structural Analysis-Powder X-Ray Diffraction (PXRD)

The PXRD technique is used for the identification of crystal structure, purity, and crystallinity. The MgO nanoparticles have been synthesized and then air-dried at a hot air oven, it was calcinated to different temperatures (500, 600, and 700°C), and then it was characterized by PXRD. The patterns of XRD were affirmed that it belongs to the cubic phase of periclase with the Fm3m space group. All peaks were indexed according to the ICDD reference number (01-075-0447). The PXRD patterns clearly show that there were no peaks that had disappeared and had not found any additional peaks were observed, shown in Figure4. So, we affirmed that the prepared MgO nanoparticles did not have any impurity phases which means that pure MgO nanoparticles have been obtained by green extract-mediated synthesis.Figure 4
PXRD patterns of MgO nanoparticles at different calcination temperatures (500, 600, and 700°C).The average crystallite size of MgO nanoparticles has been calculated where Debye–Scherrer’s formula was employed, shown as follows:(1)D=K.λ/β.cosθ,where D is the crystallite size, λ is the X-ray wavelength for Cukα radiation (1.5406A°), θ is Bragg’s diffracting angle, β is the full-width half maximum (FWHM) strain broadening, and K is the shapeless factor.


### 4.2. William–Hall Method and UDM (Uniform Deformation Model)

The W–H method had been used to find the microstrain of the nanopowder and crystallite size where the strain was considered to be uniform in all crystallographic directions which means consideration of the isotropic nature of crystals.The lattice strain and crystallite size can be obtained from the following formalism:(2)β.Cosθ=K.λ/D+4εsin,where ε is the lattice strain, D is the crystallite size, β is the strain broadening, k is the dimensionless shape factor (0.9), λ is the X-ray wavelength for Cukα radiation (1.5406A°), and θ is Bragg’s diffracting angle.The graph was plotted betweenβ cosθ vs 4sinθ at Y- and X-axis, respectively, and fitted linearly. The lattice strain could be calculated from the slope (gradient), and crystallite was calculated from the intercept (K.λ/D). The W–H plot showed that there were positive and negative slopes (strain) due to the existence of compression and tensile strain on the lattice. The W–H plot is shown in Figure 5.Figure 5
William–Hall plot of MgO nanoparticles at 500°C, 600°C, and 700°C (a, b, and c).
(a)(b)(c)The lattice constant (a) and volume of the unit cell (V), and dislocation density of MgO nanoparticles have been found using the following formulae [46, 47]:(3)a=h2+K2+l2×d2,where d is the interplanar spacing and h, k, and l are the miller indices,(4)V=1a3,where a is the lattice constant,(5)δ=1/D2,where D is the crystallite size.The crystallite size was calculated from Debye–Scherrer’s method and the W–H plot method.The calculated crystallite size and lattice parameters, dislocation density, and lattice strain are shown in Table1.Table 1
Calculated crystallite size and lattice parameters, dislocation density, and lattice strain.
Temperature (°C)Average crystallite size (D)Lattice constant (A°)(a)Unit cell volume (A°)3(V)Dislocation density (δ ×10−3)Lattice strain W–H (×10−3) (UDM model)Debye method (nm)W–H method (nm)50014134.246772.704−160010304.247769.7723.6270019354.257775.1731.08Debye’s method and W–H method. Crystallite size was found to an increasing trend while increasing temperature. The crystallite size was found by both methods which are not in the same size but the same increasing trend of in size while temperature increases. The lattice constant has also increased with temperature, but unit cell volume was found to decrease. The lattice strain found by the W–H method having positive and negative slope values due to having tensile and compress stress and in deeply the negative slope value of strain implicitly meant that there was no strain with 500°C calculations [45]. The unit cell volume decreases with increasing calcination temperature. Dislocation density is high while calcination with 600°C with strain. All the values are shown in Table 1.


### 4.3. Morphological Surface Analysis

#### 4.3.1. Scanning Electron Microscope (SEM) Imaging Techniques

The calcined MgO nanopowder morphology was exhibited in low-resolution SEM micrographs which are shown in Figure6. Calcination-dependent morphology transformation was obtained. The MgO nanopowder has distinct morphology during each stage of calcination temperature which is exhibited in micrographs. The MgO nanopowder was calcined at 500°C, and the cubic in shape morphology was observed whereas at 600°C and 700°C nanobar, hexagonal in shape morphology has been observed. Figures 6(a) and 6(d) illustrate cubic, nanobar, and hexagonal morphology. All the shapes were irregular, clustered, and aggregated, and shapes were dependent on calcination. Shape transformation was attained by the influence of temperature, and size was enlarged during the increase of temperature and modified the shapes.Figure 6
SEM images of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c, d).
(a)(b)(c)(d)


#### 4.3.2. High-Resolution Transmission Electron Microscope Imaging Analysis (HR-TEM)

To study particle size, morphology, and nature of particles, HR-TEM analysis was employed and the crystalline nature of materials was studied by SAED (selected area electron diffraction) pattern. MgO nanopowder was dispersed in ethanol on a carbon-coated copper grid, and taken HR-TEM micrographs are shown in Figures7(a), 7(b), 7(d), 7(e), 7(g), and 7(h). The micrographs of HR-TEM illustrated that MgO nanoparticles were aggregated and morphological transformation was observed owing to influences of temperature. The nanoparticles were nano in size (1–100 nm) range, and particle size was matched with XRD crystallite size. The SAED (selected area electron diffraction) patterns of MgO nanoparticles are shown in Figures 7(c), 7(f), and 7(i). Here, we have observed that in all the three calcination temperatures, there were distinct multiple rings with discrete tiny bright spots which are make up the ring which could be implied the nanoparticle were polycrystalline in nature and nano in size. The bright field of HR-TEM images was clearly illustrated, and the nanoparticles were cubic in shape at 500°C, nanobar at 600°C, hexagonal in shape at 700°C. The d-spacing found by the SAED pattern is matched with the XRD report. To reduce the total surface energy of the system, the nanoparticles were got aggregated. HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a, b, c), 600°C (d, e, f), and 700°C (g, h, i) were clearly illustrated in the micrographs.Figure 7
HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a–c), 600°C (d–f), and 700°C (g–i).
(a)(b)(c)(d)(e)(f)(g)(h)(i)


#### 4.3.3. Elemental Composition Analysis-Energy Dispersive X-ray Spectroscopy (EDX)

The chemical concentration of MgO nanoparticles could be estimated by the energy dispersive X-ray spectroscopy (EDX) characterization technique with fresh dispersion of nanopowder. Energy dispersive X-ray spectroscopy (EDX) spectrum is shown in Figures8(a) and 8(b). The spectrum consists of Mg and O element only, and there was no evidence of impurities along with Mg and O. The atomic percentage of Mg and O was indicted in the energy dispersive X-ray spectroscopy (EDX) spectra table (shown in Figure 8(c) and we observed that it has a good stoichiometric ratio of Mg and O.Figure 8
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


### 4.4. Vibrational Characterization

#### 4.4.1. FTIR (Fourier Transform Infrared) Analysis

The phytochemicals were confirmed by functional group analysis which has an important role in the formation of nanoparticles which were acted as stabilizing and capping agents [48]. The functional groups which were absorbed on the surface have been identified with FTIR characterization. FTIR spectra were recorded in the range of 400–4000 cm−1 as shown in Figure 9. Aqueous extract of Moringa oleifera leaf FTIR spectra had four intense peaks, among them, 3433 cm−1 and 3452 cm−1 bands attributed to –OH stretching vibrations owing to the presence of ester, alcohol, carboxylic acid, and ether groups, and peak 1636 cm−1 assigned to –OH bending vibration [49]. The band belongs to 1034 cm−1 is aromatic stretching bands of various bioactive compounds and proteins. The band at 1034 cm−1 corresponds to the aromatic stretching of various bioactive compounds and proteins. The transformation occurred from enol form to keto form due to the presence of flavonoids and phenols. This mechanism reduces the metal ions and forms nanoparticles since it releases reactive H atoms and forms the O-H group since the phenol group has electron-donating ability [48]. The metal oxide characteristic absorption band arises below 1000 cm−1 to form interatomic vibrations. Biosynthesized MgO particle characteristic band exhibited at 442 cm−1 and 438 cm−1 which are assigned to the stretching mode of MgO [50–52].Figure 9
FTIR spectra of calcined MgO nanoparticles andMoringa oleifera leaf extract.


#### 4.4.2. Micro-Raman Scattering

Raman spectroscopy is the vibrational technique used to identify crystal structural information, differentiate the multiple phases in metal oxides, changes in metal-oxygen bond, bond lengths, metal oxidation state, lattice disorder, and distortions, and study the intramolecular and lattice vibrations [53]. Raman spectrum of the cubic phase of periclase with the Fm3m space group has not been identified much in the literature. Limited papers have done the Raman investigation for this cubic phase of MgO NPs. Raman spectra recorded for MgO in the range of 100 cm−1 to 3000 cm−1 are given in Figure 10. MgO NPs possess a high-ordered lattice NaCl structure with cubic space group O5h with cubic structure (Fm3m) symmetry. The vibration modes of MgO nanoparticles which are expected have been written by group theory analysis. It has four Raman active modes and one IR active mode:(6)Γopt=A1gR+EgR+F1gsilent+2FgR+4F1uIR+F2usilent,where 4F1u is the infrared active modes and A1g + Eg+ 2Fg are the Raman active modes [54, 55]. The room temperature Raman spectra recorded for MgO nanoparticles in the range of 100 cm−1 to 3000 cm−1 are exhibited in Figure 10. MgO nanoparticles have Raman active vibrational mode with major Raman band 447 cm−1, 850 cm−1, 1084 cm−1, 1495 cm−1, 1923 cm−1, and 2322 cm−1. There are no vibrational bands which have been observed at cubic morphology at 500°C. Raman vibrations are observed only when increasing the calcination temperature to 600° and 700°C, and the intensity of the peak increases and the spectra show the characteristic peak of MgO at 447 cm−1, 850 cm−1, and 2322 cm−1 [54, 56]. The Raman bands are observed in the range of 200–600 cm−1 for metal oxide minerals [57]. The band belongs to 1084 cm−1 appears owing to TO-LO surface phonon modes, and G-band and D-band peaks were observed. The peaks observed below 1500 cm−1 were attributed to D-band and above 1500 cm−1 were assigned a to G-band [58]. The peaks found under the 300 cm−1 are attributed to lattice modes. The twisting and stretching modes are found in the midfrequency region. The peaks are found at 579, 719, and 1096 cm−1 since the MgO particle has a size between 10 and 30 nm [54]. The IR active mode was observed at 850 cm−1 due to contributions coming from F1 (angle bond O–Mg–O, stretching bond O–O). It describes the octahedral breathing‐type vibrations [55]. The F1u IR active mode observed at 850 cm−1 occurs on the repulsive force between O–O and bending force O–Mg–O for angle bond [54]. The band at 1084 cm−1 corresponds to TO-LO surface phonon modes. The peaks appear below 1500 cm−1 attributed to D-band is known as breathing mode, and the peaks above 1923 cm−1 and 2322 cm−1 are assigned to G-band [59]. The ratio between D-band and G-band gives the information about crystallite size and surface defects, and the peaks with strong intensities indicate the cubic structure [59].Figure 10
Micro-Raman spectra of MgO nanoparticles.


### 4.5. Optical Property Analysis

#### 4.5.1. UV-Visible Absorption Spectroscopy Characterization (before Calcination-as Prepared)

UV-Vis absorbance spectroscopy has revealed the optical property and electronic structure of nanoparticles. The absorbance spectrum was recorded in the range of 200 nm to 800 nm. The UV-visible absorption spectrum of MgO NPs is shown in Figures11(a) and 11(b). The absorption band edge was found at 273 nm (4.5 eV). The absorbance of MgO nanoparticles at the UV region was 273 nm due to surface plasmon resonance. The UV region absorption band at 273 nm (4.5 eV) is found with the excitation of 3-fold coordinated O2− anions in the edges and corners and defects on the surface (F centers), respectively [51, 60, 61]. The energy band gap (Eg) could be found from Tauc plot, and the formula employed is given as follows:(7)α=Ah√−Egn/h√,where α is the absorption coefficient, Eg is the absorption band gap, A is a constant, h√ is the energy of the photon, and n is the nature of transitions. The band gap value could be determined from the intercept of the straight line with the h√. The Tauc plot is shown in Figure 11(b). The computed optical band gap value 4.5 eV was considered as a lower band gap of the MgO NPs due to the presence of 3-coordinated surface anions at the corners whereas the bulk MgO material has band gap of 7.8 eV owing to the existence of 6-coordinated surface anions. The computed band gap value of MgO NPs well matches with previous reports [62–67].Figure 11
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


#### 4.5.2. UV-Vis Spectroscopy in Reflectance Mode (after Calcination)

The optical properties of MgO NPs after calcination have been studied from the reflectance spectrum, and also it was recorded in the range of 200 nm to 800 nm in reflectance mode where diffuse reflectance spectrometer was employed. The optical band gap energy of MgO NPs at different calcination temperatures was calculated by Kubelka–Munk function:(8)FR=1−R2/2R,where R is the reflectance. The graph has been plotted between (F(R) hν) 2 and hν. The energy band gap value at different calcination temperatures has been calculated by extrapolation of the linear part of the (F(R) hν) 2 at the X-axis plot to the intersection with hν at Y-axis. The energy band gap value computed is 5.2 eV, 5.1 eV, and 4.9 eV for 500°, 600°, and 700°C which is illustrated in Figure 11(c). The band gap value has been decreased with increasing temperature which was observed owing to the growth of particles and crystallinity and the value is well-matched with previous reports, and the smallest band gap was observed when calcined at 700°C [68–71].


### 4.6. Photoluminescence Spectroscopy Analysis

#### 4.6.1. Room Temperature Emission Spectroscopy

The PL spectrum of MgO nanoparticles was recorded at room temperature with a Xe lamp as an excitation light source at excitation wavelength 320 nm. Photoluminescence emission spectra are depicted in Figure12. Holes from the valence band and electrons from the electronic states recombine with each other, and this is responsible for the emission behavior of transition metals. The recombination of photoexcited electron and hole pairs at the energy states would induce the photoemission. The nature of the defects causes light emission. Photoluminescence gives the information about the impurities and defects in nanoparticles [61, 72]. The defect centers create different electronic states in the wide band gap of the material such as such F- and F2-type centers (F, F+, F21+, F22+, and F23+), cationic vacancies (VMg−2), Schottky defect (VMg0+V∘0), and interstitial oxygen atom (Oi0, Oi−1, and Oi−2), and those are responsible for multicolor emission [73]. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles shown in Tables 2 and 3. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles. It has arisen at UV-visible region. UV (359 nm), violet (377 nm, 378 nm), blue (491 nm), green (518), and orange (593 nm) emissions were found in PL spectra. Luminescence of MgO nanoparticles arises at UV region (359 nm) due to oxygen vacancies (surface defects). If defect is high, intensity will also be high. Green emission has aroused due to F centers. The green emission arises around 518 nm due to oxygen vacancies that is excitation of F (V∘0) centers [9, 10, 11]. Red orange emission arises due to relaxation luminescence of defect centers F21+ created by mechanical stress. The orange emission arises at 593 nm due to relaxation luminescence of defect centers F21+ (or V∘+1+V∘0) created by mechanical stress [9–11]. Violet emission arises due to F+ centers. The violet emissions arise due to F+ (or V∘+1) centers. Blue emission was raised by hole trapped at Mg vacancy, and it was assigned to F2 center. The blue emission around 491 nm arises due to hole trapped at Mg ion vacancy, and it was assigned to F2 center [61, 77, 78]. Multicolor emission observed in wide band gap of materials due to different electronic states there [61, 77, 78]. Multicolor emissions are observed in wide band gap materials due to different electronic states. PL optical study has given the physical property of the materials. So, according to the above study, MgO NPs will be used as potential material for optoelectronic applications.Figure 12
Photoluminescence emission spectra of MgO nanoparticles (a).Table 2
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Temperature (°C)Wavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)Emission500359UV378–413Violet491Blue518–538Green593Orange600359UV377–411Violet491Blue518–538Green593Orange700359UV377–438Violet491Blue518–538Green593OrangeTable 3
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Metal oxide NPsPeak position wavelength (observed in nm)EmissionEnergy (eV)AttributionReferencesMgO nanoparticles359UV3.45Surface defects[31, 74]378Violet3.2Defect band transition. F+ (or V∘+1) centers[31, 33, 54, 55, 75]4113.0141334382.83491Blue2.52Recombination of electrons with oxygen vacancies[31, 33, 34, 75]518Green2.39Oxygen vacancies (Vo)[31, 33, 48, 52, 53, 74, 76]538Green2.30593Orange2Relaxation luminescence of defect centers F21+created by mechanical stress[31, 48, 52, 53, 74, 76]


### 4.7. Thermal Analysis

#### 4.7.1. Thermogravimetric (TG), Differential Scanning Calorimetric (DSC), and Differential Thermal Analysis (DTA)

The thermal decomposition behavior of samples as prepared was studied by TG and DSC thermographs. The change of weight of the sample concerning temperature measure is TGA. Changes in sample composition and thermal stability can be studied with weight loss of the sample. The TGA DTA and DSC thermographs of MgO nanoparticles are shown in Figures13(a) and 13(b). The weight loss which occurs has been observed at 200- to 450-degree Celsius by exothermic peaks of DTA and DSC from the graph due to decomposition owing to absorption or removal H2O molecules and second weight loss due to the decomposition of bioactive compounds which is from the plant extract [79, 80]. The DSC curve has one endothermic peak at 660°C where maximum weight loss occurs which implies phase transition of Mg (OH)2 to MgO. Hence, the pure MgO nanoparticles have obtained with pure phase at 700°C and the obtained results are well consistent with previous reports [79, 81–87].Figure 13
TGA DTA of MgO nanoparticles and TG-DSC of MgO nanoparticles (a, b).
(a)(b)


### 4.8. Electrical Properties

#### 4.8.1. Real Part of Dielectric Constant (ε′)

The calcinated MgO nanopowder had pelletized by hydraulic pressure, and silver paste was coated on the surface to create better conduction. Frequency dependence of dielectric properties was studied with different temperatures from RT to 180°C (30°C, 80°C, and 130°C and 180°C). We design an energy storage device that needs to study the dielectric constant and dielectric breakdown strength which are the important parameters to calculate the energy density of the dielectrics. Dielectric loss is an important parameter for capacitor performance. The capacitance loss factor has been measured by the parallel plate capacitor method using an LCR meter for the frequency range between 100 Hz and 5 MHz for different temperatures (30°C, 80°C, and 130°C and 180°C).The dielectric constant could be calculated by the relation (1) given as follows:(9)εr=Cp×t/ε0×A,where ε0 is the permittivity of the free space (8.85 × 10–12 farad per meter (F/m), Cp is the capacitance in farad, A is an area of the cross section of pellet, and t is the thickness of pellet.The four type polarization namely space, charge, dipolar, ionic, electronic might be the reason for the dielectric nature of materials, and dielectric constant depends on these parameters. When frequency is applied from 100 Hz to 5 MHz, the Dielectric constant increases rapidly along with frequency which increases due to space charge polarization and interfacial polarization along with temperature increases from room temperature, as shown in Figures14(a)–14(c). When applied frequency increases, the dielectric constant decreases its value gradually, and at the high-frequency range, its value is constant along with different temperatures; the same trend has happened, and it obeys Koop’s theory owing to Maxwell–Wagner type interfacial polarization. At the high-frequency range, the same trend has followed at all the temperatures, the dielectric constant was found constant and merged due polarization decreases, and oxygen vacancies and grain boundaries were might be the reason for a large value of dielectric constant at lower frequency range [88, 89]. Dielectric constant value is high at low-frequency range and low at high-frequency range because of different types of polarization as said above explanation, when at high-frequency range, the electric dipoles cannot follow the frequency of applied field and dipoles cannot shift their orientation sufficiently fast when frequency is high [90, 91]. The dielectric medium has conducting grains which operate at higher frequencies and poor conducting grain boundaries which are operating at lower frequencies, while frequency applied the charge carriers are assembled at grain boundaries, so polarization occurs with high dielectric constant and polarization decreases while frequency value increases, so it has constant value at high frequency since the springing of electrons cannot cope with AC fields.Figure 14
Dielectric constant of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


### 4.9. Imaginary Part of Dielectric Constant (ε′′)

The tan loss decreased with frequency increases, the same trend has followed at all the temperatures due to thermal-activated charges accumulated of charge carriers and space charge polarization. The imaginary part of the dielectric constant value is large at the low-frequency range as shown in Figures15(a)–15(c). The polarization mechanism, defects, and thermally activated mobile ion conduction might be the reason for the fast-rising trend of the imaginary part of dielectric constant at lower frequencies with the thermally activated conduction of mobile ions [89].Figure 15
Dielectric loss of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


### 4.10. Tan Loss

The tan loss is high at low frequency and low at high frequency due to surface polarization has reached constant value and electrons were unable to follow AC signal, so value is high at low frequency, and at high frequency, it has disappeared. The tan loss is shown in Figures16(a)–16(c). At moderate and low frequencies, polarization is high, whereas at high frequencies, charges could not follow the AC signals [88]. Due to the domination of conducting grains, the resistivity comes down, so the loss arises and saturated at high frequency, and it obeys Koop’s law. The tan loss is given by the relation (2):(10)Tan loss=ε′/ε″.Figure 16
Tan loss of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


#### 4.10.1. AC Conductivity Studies

The frequency-dependent AC conductivity of MgO nanopowder has been studied for all the three samples, and the graph has been plotted between frequency and conductivity as shown in Figures17(a)–17(c). The AC conductivity is maximum at higher temperatures with high frequency, and the same trend has been followed by all the samples of MgO nanoparticles due to charge carrier and hopping electrons also increases [92]. Moreover, it obeys the Maxwell–Wagner two-layer model according to this conductivity increases gradually along with frequency [93]. Due to polarization effects at electrode and electrolyte interface at low frequency, the variation of conductivity has occurred and all the values have merged at lower frequency owing to grains and grain boundaries which are more active, at low temperature fewer charge carriers are available, and less hoping electrons might be the reason for low conduction at low frequency [92, 93].Figure 17
AC conductivity of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)AC conductivity was calculated using the relation given as follows:(11)σ=2πfεε0tanδ,where ε0 is the permittivity of free space (8.854 × 10−12 F/m).


### 4.11. Complex Spectroscopy and Impedance Analysis

#### 4.11.1. Impedance Analysis (Z′ andZ″)

Complex impedance (Z∗=Z′+i⋅Z″″) has been analyzed at different temperatures on both sides of the relaxation peak. The frequency and temperature dependence of real part of impedance (z’) and imaginary part of impedance has been studied using the formulism given as follows:(12)Z′=g/Cp2ω2+G2Z″=Cpω/Cp2ω2+G,where ω is the 2 π f, G is the conductance, and Cp is the static capacitance of materials.


### 4.12. Real Part of Impedance (Z′)

The increasing trend of frequency and temperature decreases the real part of impedance value owing to space charge effect and the values saturated at high frequency as shown in supplementary information FiguresS1a, S1c, and S1e, which has meant an increase of conductivity with frequency. At high frequency, the part of impedance value has merged due to the release of space charge and owing to the reduction of barrier properties or accumulation of charges at the electrode surface along with the rise of temperature [75, 94]. The decreasing trend of Z′ value at high frequency is almost low in all the samples.


### 4.13. Imaginary Part of Impedance (z”)

Oxygen vacancies in metal oxides and relaxation processes of materials are being the reason for the frequency-dependent imaginary part of impedance shifted to a higher frequency with an increase in temperature. When high temperatures are met, all the values are saturated and merged at higher frequency [75, 94]. The imaginary part of impedance is shown in supplementary information Figures S1b, S1d, and S1f.


### 4.14. Cole–Cole Plot or Nyquist Plot

The graph was drawn between the real part of impedance (Z′) and the imaginary part of impedance (Z″) as shown in supplementary information Figures S2a, S2b, and S2c. From Figure S2, it can be seen that slightly semicircle with distinct radii appears at the low frequency due to grain boundaries [75, 93, 94]. Semicircle decreases with increasing temperature due to the negative temperature coefficient of materials which are promising materials for thermistor applications.


### 4.15. Complex Electric Modulus Analysis

The real part of the electric modulus and imaginary part of electric modulus are shown in supplementary information FiguresS3 and S4a, S4b, S4c, S4d and S4e, and S4f, and all are frequency-dependent. This technique quite uses full to find the relaxation time and relaxation mechanism at the metal oxides.


### 4.16. Real Part of Electric Modulus

Electric modulus values are high at a higher frequency and at almost zero at the lower frequency which implies that electronic polarization is none [92]. The real part of the electric modulus is shown in supplementary information Figures S3a, S3b, and S3c.


### 4.17. Imaginary Part of Electric Modulus

This imaginary part of electric modulus was studied, and it explains about high conduction loss owing to electric modulus increases with the increasing trend of frequency. Peaks appearing here shifted to a higher frequency because the charge carriers transported from long-range to short-range mobility with the increase of temperature [92]. Moreover, M″ peaks shifted to higher frequencies, so we conclude that it depends on temperature and obeys hopping type mechanism for electrical conduction [92]. The imaginary part of the electric modulus spectra is shown in supplementary information Figures S4d, S4e, and S4f.


### 4.18. Complex Electric Modulus (M′ vs M″)

The complex electric modulus spectra are shown in supplementary information FiguresS5g, S5h, and S5i with different temperatures (30–230°C). From the graph, we could observe that semicircles have been formed because the grain and grain boundaries might be the reason for the conduction of the materials. At the higher frequencies and temperature, the semicircle has been disappeared on account of hopping of ions [75, 92–94].


### 4.19. M–H Loop Characterization (Magnetic Property)

Room temperature magnetization measurements were carried out where vibrating sample magnetometer (VSM) was employed for analysis. Magnetic property of MgO nanoparticles studied from M–H curves is shown in Figure18, and it is observed that all the MgO nanoparticles exhibited room temperature diamagnetism at 500 and 600°C and room temperature; week or dilute ferromagnetism has been observed from the sample while annealed at 700°C. It is diamagnetic in nature at room temperature for the two samples of MgO nanopowder due to decreased number of oxygen vacancies [52, 74]. While increasing calcination temperature, the oxygen vacancies can be improved; hence, the defect sides at the surface of the MgO nanoparticles have been increased. Panchakarla et al. and Pathak et al. have reported previously that the diamagnetic nature oxides exhibit RTFM due to defects (oxygen vacancies) present at the surface of the nanoparticles grains [95, 96]. Many reports have suggested that the room temperature ferromagnetism has been observed at the nanoscale nonmagnetic metal oxides due to anionic or cationic vacancy or size of the nanoparticles or annealing and anisotropy nature of nanomaterials [97–101]. Herein, the nanoparticles at the annealed temperature 700°C show very week ferromagnetic nature at ambient conditions with saturation magnetization value (Ms) of 57.004 E−3 emu/g and coercivity value (Hci) is 1604.5 Oe owing to the oxygen vacancies (F+ centers) have been increased with increasing annealing temperature, and while comparing with photoluminescence spectra of MgO nanoparticles, it has strong green, blue, and violet emissions. The violet and blue emissions occur on the surface of the MgO nanoparticles due to oxygen vacancies (Vo); hence, room temperature ferromagnetism (RTFM) has been observed in diamagnetic oxides owing to defect-induced magnetism. Rao et al. and Hu et al. have reported that the oxygen vacancy (F+) is the major responsible for presence of hysteresis and it shows FM or dilute magnetism in MgO nanoparticles, while temperature increases, it increases the F2+ centers which could be the reason for arising FM in MgO nanoparticles [96, 100, 102, 103].Figure 18
M–H curve of MgO nanoparticles at the room temperature.


## 4.1. Structural Analysis-Powder X-Ray Diffraction (PXRD)

The PXRD technique is used for the identification of crystal structure, purity, and crystallinity. The MgO nanoparticles have been synthesized and then air-dried at a hot air oven, it was calcinated to different temperatures (500, 600, and 700°C), and then it was characterized by PXRD. The patterns of XRD were affirmed that it belongs to the cubic phase of periclase with the Fm3m space group. All peaks were indexed according to the ICDD reference number (01-075-0447). The PXRD patterns clearly show that there were no peaks that had disappeared and had not found any additional peaks were observed, shown in Figure4. So, we affirmed that the prepared MgO nanoparticles did not have any impurity phases which means that pure MgO nanoparticles have been obtained by green extract-mediated synthesis.Figure 4
PXRD patterns of MgO nanoparticles at different calcination temperatures (500, 600, and 700°C).The average crystallite size of MgO nanoparticles has been calculated where Debye–Scherrer’s formula was employed, shown as follows:(1)D=K.λ/β.cosθ,where D is the crystallite size, λ is the X-ray wavelength for Cukα radiation (1.5406A°), θ is Bragg’s diffracting angle, β is the full-width half maximum (FWHM) strain broadening, and K is the shapeless factor.


## 4.2. William–Hall Method and UDM (Uniform Deformation Model)

The W–H method had been used to find the microstrain of the nanopowder and crystallite size where the strain was considered to be uniform in all crystallographic directions which means consideration of the isotropic nature of crystals.The lattice strain and crystallite size can be obtained from the following formalism:(2)β.Cosθ=K.λ/D+4εsin,where ε is the lattice strain, D is the crystallite size, β is the strain broadening, k is the dimensionless shape factor (0.9), λ is the X-ray wavelength for Cukα radiation (1.5406A°), and θ is Bragg’s diffracting angle.The graph was plotted betweenβ cosθ vs 4sinθ at Y- and X-axis, respectively, and fitted linearly. The lattice strain could be calculated from the slope (gradient), and crystallite was calculated from the intercept (K.λ/D). The W–H plot showed that there were positive and negative slopes (strain) due to the existence of compression and tensile strain on the lattice. The W–H plot is shown in Figure 5.Figure 5
William–Hall plot of MgO nanoparticles at 500°C, 600°C, and 700°C (a, b, and c).
(a)(b)(c)The lattice constant (a) and volume of the unit cell (V), and dislocation density of MgO nanoparticles have been found using the following formulae [46, 47]:(3)a=h2+K2+l2×d2,where d is the interplanar spacing and h, k, and l are the miller indices,(4)V=1a3,where a is the lattice constant,(5)δ=1/D2,where D is the crystallite size.The crystallite size was calculated from Debye–Scherrer’s method and the W–H plot method.The calculated crystallite size and lattice parameters, dislocation density, and lattice strain are shown in Table1.Table 1
Calculated crystallite size and lattice parameters, dislocation density, and lattice strain.
Temperature (°C)Average crystallite size (D)Lattice constant (A°)(a)Unit cell volume (A°)3(V)Dislocation density (δ ×10−3)Lattice strain W–H (×10−3) (UDM model)Debye method (nm)W–H method (nm)50014134.246772.704−160010304.247769.7723.6270019354.257775.1731.08Debye’s method and W–H method. Crystallite size was found to an increasing trend while increasing temperature. The crystallite size was found by both methods which are not in the same size but the same increasing trend of in size while temperature increases. The lattice constant has also increased with temperature, but unit cell volume was found to decrease. The lattice strain found by the W–H method having positive and negative slope values due to having tensile and compress stress and in deeply the negative slope value of strain implicitly meant that there was no strain with 500°C calculations [45]. The unit cell volume decreases with increasing calcination temperature. Dislocation density is high while calcination with 600°C with strain. All the values are shown in Table 1.


## 4.3. Morphological Surface Analysis

### 4.3.1. Scanning Electron Microscope (SEM) Imaging Techniques

The calcined MgO nanopowder morphology was exhibited in low-resolution SEM micrographs which are shown in Figure6. Calcination-dependent morphology transformation was obtained. The MgO nanopowder has distinct morphology during each stage of calcination temperature which is exhibited in micrographs. The MgO nanopowder was calcined at 500°C, and the cubic in shape morphology was observed whereas at 600°C and 700°C nanobar, hexagonal in shape morphology has been observed. Figures 6(a) and 6(d) illustrate cubic, nanobar, and hexagonal morphology. All the shapes were irregular, clustered, and aggregated, and shapes were dependent on calcination. Shape transformation was attained by the influence of temperature, and size was enlarged during the increase of temperature and modified the shapes.Figure 6
SEM images of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c, d).
(a)(b)(c)(d)


### 4.3.2. High-Resolution Transmission Electron Microscope Imaging Analysis (HR-TEM)

To study particle size, morphology, and nature of particles, HR-TEM analysis was employed and the crystalline nature of materials was studied by SAED (selected area electron diffraction) pattern. MgO nanopowder was dispersed in ethanol on a carbon-coated copper grid, and taken HR-TEM micrographs are shown in Figures7(a), 7(b), 7(d), 7(e), 7(g), and 7(h). The micrographs of HR-TEM illustrated that MgO nanoparticles were aggregated and morphological transformation was observed owing to influences of temperature. The nanoparticles were nano in size (1–100 nm) range, and particle size was matched with XRD crystallite size. The SAED (selected area electron diffraction) patterns of MgO nanoparticles are shown in Figures 7(c), 7(f), and 7(i). Here, we have observed that in all the three calcination temperatures, there were distinct multiple rings with discrete tiny bright spots which are make up the ring which could be implied the nanoparticle were polycrystalline in nature and nano in size. The bright field of HR-TEM images was clearly illustrated, and the nanoparticles were cubic in shape at 500°C, nanobar at 600°C, hexagonal in shape at 700°C. The d-spacing found by the SAED pattern is matched with the XRD report. To reduce the total surface energy of the system, the nanoparticles were got aggregated. HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a, b, c), 600°C (d, e, f), and 700°C (g, h, i) were clearly illustrated in the micrographs.Figure 7
HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a–c), 600°C (d–f), and 700°C (g–i).
(a)(b)(c)(d)(e)(f)(g)(h)(i)


### 4.3.3. Elemental Composition Analysis-Energy Dispersive X-ray Spectroscopy (EDX)

The chemical concentration of MgO nanoparticles could be estimated by the energy dispersive X-ray spectroscopy (EDX) characterization technique with fresh dispersion of nanopowder. Energy dispersive X-ray spectroscopy (EDX) spectrum is shown in Figures8(a) and 8(b). The spectrum consists of Mg and O element only, and there was no evidence of impurities along with Mg and O. The atomic percentage of Mg and O was indicted in the energy dispersive X-ray spectroscopy (EDX) spectra table (shown in Figure 8(c) and we observed that it has a good stoichiometric ratio of Mg and O.Figure 8
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


## 4.3.1. Scanning Electron Microscope (SEM) Imaging Techniques

The calcined MgO nanopowder morphology was exhibited in low-resolution SEM micrographs which are shown in Figure6. Calcination-dependent morphology transformation was obtained. The MgO nanopowder has distinct morphology during each stage of calcination temperature which is exhibited in micrographs. The MgO nanopowder was calcined at 500°C, and the cubic in shape morphology was observed whereas at 600°C and 700°C nanobar, hexagonal in shape morphology has been observed. Figures 6(a) and 6(d) illustrate cubic, nanobar, and hexagonal morphology. All the shapes were irregular, clustered, and aggregated, and shapes were dependent on calcination. Shape transformation was attained by the influence of temperature, and size was enlarged during the increase of temperature and modified the shapes.Figure 6
SEM images of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c, d).
(a)(b)(c)(d)


## 4.3.2. High-Resolution Transmission Electron Microscope Imaging Analysis (HR-TEM)

To study particle size, morphology, and nature of particles, HR-TEM analysis was employed and the crystalline nature of materials was studied by SAED (selected area electron diffraction) pattern. MgO nanopowder was dispersed in ethanol on a carbon-coated copper grid, and taken HR-TEM micrographs are shown in Figures7(a), 7(b), 7(d), 7(e), 7(g), and 7(h). The micrographs of HR-TEM illustrated that MgO nanoparticles were aggregated and morphological transformation was observed owing to influences of temperature. The nanoparticles were nano in size (1–100 nm) range, and particle size was matched with XRD crystallite size. The SAED (selected area electron diffraction) patterns of MgO nanoparticles are shown in Figures 7(c), 7(f), and 7(i). Here, we have observed that in all the three calcination temperatures, there were distinct multiple rings with discrete tiny bright spots which are make up the ring which could be implied the nanoparticle were polycrystalline in nature and nano in size. The bright field of HR-TEM images was clearly illustrated, and the nanoparticles were cubic in shape at 500°C, nanobar at 600°C, hexagonal in shape at 700°C. The d-spacing found by the SAED pattern is matched with the XRD report. To reduce the total surface energy of the system, the nanoparticles were got aggregated. HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a, b, c), 600°C (d, e, f), and 700°C (g, h, i) were clearly illustrated in the micrographs.Figure 7
HR-TEM images and SAED patterns of MgO nanoparticles at 500°C (a–c), 600°C (d–f), and 700°C (g–i).
(a)(b)(c)(d)(e)(f)(g)(h)(i)


## 4.3.3. Elemental Composition Analysis-Energy Dispersive X-ray Spectroscopy (EDX)

The chemical concentration of MgO nanoparticles could be estimated by the energy dispersive X-ray spectroscopy (EDX) characterization technique with fresh dispersion of nanopowder. Energy dispersive X-ray spectroscopy (EDX) spectrum is shown in Figures8(a) and 8(b). The spectrum consists of Mg and O element only, and there was no evidence of impurities along with Mg and O. The atomic percentage of Mg and O was indicted in the energy dispersive X-ray spectroscopy (EDX) spectra table (shown in Figure 8(c) and we observed that it has a good stoichiometric ratio of Mg and O.Figure 8
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


## 4.4. Vibrational Characterization

### 4.4.1. FTIR (Fourier Transform Infrared) Analysis

The phytochemicals were confirmed by functional group analysis which has an important role in the formation of nanoparticles which were acted as stabilizing and capping agents [48]. The functional groups which were absorbed on the surface have been identified with FTIR characterization. FTIR spectra were recorded in the range of 400–4000 cm−1 as shown in Figure 9. Aqueous extract of Moringa oleifera leaf FTIR spectra had four intense peaks, among them, 3433 cm−1 and 3452 cm−1 bands attributed to –OH stretching vibrations owing to the presence of ester, alcohol, carboxylic acid, and ether groups, and peak 1636 cm−1 assigned to –OH bending vibration [49]. The band belongs to 1034 cm−1 is aromatic stretching bands of various bioactive compounds and proteins. The band at 1034 cm−1 corresponds to the aromatic stretching of various bioactive compounds and proteins. The transformation occurred from enol form to keto form due to the presence of flavonoids and phenols. This mechanism reduces the metal ions and forms nanoparticles since it releases reactive H atoms and forms the O-H group since the phenol group has electron-donating ability [48]. The metal oxide characteristic absorption band arises below 1000 cm−1 to form interatomic vibrations. Biosynthesized MgO particle characteristic band exhibited at 442 cm−1 and 438 cm−1 which are assigned to the stretching mode of MgO [50–52].Figure 9
FTIR spectra of calcined MgO nanoparticles andMoringa oleifera leaf extract.


### 4.4.2. Micro-Raman Scattering

Raman spectroscopy is the vibrational technique used to identify crystal structural information, differentiate the multiple phases in metal oxides, changes in metal-oxygen bond, bond lengths, metal oxidation state, lattice disorder, and distortions, and study the intramolecular and lattice vibrations [53]. Raman spectrum of the cubic phase of periclase with the Fm3m space group has not been identified much in the literature. Limited papers have done the Raman investigation for this cubic phase of MgO NPs. Raman spectra recorded for MgO in the range of 100 cm−1 to 3000 cm−1 are given in Figure 10. MgO NPs possess a high-ordered lattice NaCl structure with cubic space group O5h with cubic structure (Fm3m) symmetry. The vibration modes of MgO nanoparticles which are expected have been written by group theory analysis. It has four Raman active modes and one IR active mode:(6)Γopt=A1gR+EgR+F1gsilent+2FgR+4F1uIR+F2usilent,where 4F1u is the infrared active modes and A1g + Eg+ 2Fg are the Raman active modes [54, 55]. The room temperature Raman spectra recorded for MgO nanoparticles in the range of 100 cm−1 to 3000 cm−1 are exhibited in Figure 10. MgO nanoparticles have Raman active vibrational mode with major Raman band 447 cm−1, 850 cm−1, 1084 cm−1, 1495 cm−1, 1923 cm−1, and 2322 cm−1. There are no vibrational bands which have been observed at cubic morphology at 500°C. Raman vibrations are observed only when increasing the calcination temperature to 600° and 700°C, and the intensity of the peak increases and the spectra show the characteristic peak of MgO at 447 cm−1, 850 cm−1, and 2322 cm−1 [54, 56]. The Raman bands are observed in the range of 200–600 cm−1 for metal oxide minerals [57]. The band belongs to 1084 cm−1 appears owing to TO-LO surface phonon modes, and G-band and D-band peaks were observed. The peaks observed below 1500 cm−1 were attributed to D-band and above 1500 cm−1 were assigned a to G-band [58]. The peaks found under the 300 cm−1 are attributed to lattice modes. The twisting and stretching modes are found in the midfrequency region. The peaks are found at 579, 719, and 1096 cm−1 since the MgO particle has a size between 10 and 30 nm [54]. The IR active mode was observed at 850 cm−1 due to contributions coming from F1 (angle bond O–Mg–O, stretching bond O–O). It describes the octahedral breathing‐type vibrations [55]. The F1u IR active mode observed at 850 cm−1 occurs on the repulsive force between O–O and bending force O–Mg–O for angle bond [54]. The band at 1084 cm−1 corresponds to TO-LO surface phonon modes. The peaks appear below 1500 cm−1 attributed to D-band is known as breathing mode, and the peaks above 1923 cm−1 and 2322 cm−1 are assigned to G-band [59]. The ratio between D-band and G-band gives the information about crystallite size and surface defects, and the peaks with strong intensities indicate the cubic structure [59].Figure 10
Micro-Raman spectra of MgO nanoparticles.


## 4.4.1. FTIR (Fourier Transform Infrared) Analysis

The phytochemicals were confirmed by functional group analysis which has an important role in the formation of nanoparticles which were acted as stabilizing and capping agents [48]. The functional groups which were absorbed on the surface have been identified with FTIR characterization. FTIR spectra were recorded in the range of 400–4000 cm−1 as shown in Figure 9. Aqueous extract of Moringa oleifera leaf FTIR spectra had four intense peaks, among them, 3433 cm−1 and 3452 cm−1 bands attributed to –OH stretching vibrations owing to the presence of ester, alcohol, carboxylic acid, and ether groups, and peak 1636 cm−1 assigned to –OH bending vibration [49]. The band belongs to 1034 cm−1 is aromatic stretching bands of various bioactive compounds and proteins. The band at 1034 cm−1 corresponds to the aromatic stretching of various bioactive compounds and proteins. The transformation occurred from enol form to keto form due to the presence of flavonoids and phenols. This mechanism reduces the metal ions and forms nanoparticles since it releases reactive H atoms and forms the O-H group since the phenol group has electron-donating ability [48]. The metal oxide characteristic absorption band arises below 1000 cm−1 to form interatomic vibrations. Biosynthesized MgO particle characteristic band exhibited at 442 cm−1 and 438 cm−1 which are assigned to the stretching mode of MgO [50–52].Figure 9
FTIR spectra of calcined MgO nanoparticles andMoringa oleifera leaf extract.


## 4.4.2. Micro-Raman Scattering

Raman spectroscopy is the vibrational technique used to identify crystal structural information, differentiate the multiple phases in metal oxides, changes in metal-oxygen bond, bond lengths, metal oxidation state, lattice disorder, and distortions, and study the intramolecular and lattice vibrations [53]. Raman spectrum of the cubic phase of periclase with the Fm3m space group has not been identified much in the literature. Limited papers have done the Raman investigation for this cubic phase of MgO NPs. Raman spectra recorded for MgO in the range of 100 cm−1 to 3000 cm−1 are given in Figure 10. MgO NPs possess a high-ordered lattice NaCl structure with cubic space group O5h with cubic structure (Fm3m) symmetry. The vibration modes of MgO nanoparticles which are expected have been written by group theory analysis. It has four Raman active modes and one IR active mode:(6)Γopt=A1gR+EgR+F1gsilent+2FgR+4F1uIR+F2usilent,where 4F1u is the infrared active modes and A1g + Eg+ 2Fg are the Raman active modes [54, 55]. The room temperature Raman spectra recorded for MgO nanoparticles in the range of 100 cm−1 to 3000 cm−1 are exhibited in Figure 10. MgO nanoparticles have Raman active vibrational mode with major Raman band 447 cm−1, 850 cm−1, 1084 cm−1, 1495 cm−1, 1923 cm−1, and 2322 cm−1. There are no vibrational bands which have been observed at cubic morphology at 500°C. Raman vibrations are observed only when increasing the calcination temperature to 600° and 700°C, and the intensity of the peak increases and the spectra show the characteristic peak of MgO at 447 cm−1, 850 cm−1, and 2322 cm−1 [54, 56]. The Raman bands are observed in the range of 200–600 cm−1 for metal oxide minerals [57]. The band belongs to 1084 cm−1 appears owing to TO-LO surface phonon modes, and G-band and D-band peaks were observed. The peaks observed below 1500 cm−1 were attributed to D-band and above 1500 cm−1 were assigned a to G-band [58]. The peaks found under the 300 cm−1 are attributed to lattice modes. The twisting and stretching modes are found in the midfrequency region. The peaks are found at 579, 719, and 1096 cm−1 since the MgO particle has a size between 10 and 30 nm [54]. The IR active mode was observed at 850 cm−1 due to contributions coming from F1 (angle bond O–Mg–O, stretching bond O–O). It describes the octahedral breathing‐type vibrations [55]. The F1u IR active mode observed at 850 cm−1 occurs on the repulsive force between O–O and bending force O–Mg–O for angle bond [54]. The band at 1084 cm−1 corresponds to TO-LO surface phonon modes. The peaks appear below 1500 cm−1 attributed to D-band is known as breathing mode, and the peaks above 1923 cm−1 and 2322 cm−1 are assigned to G-band [59]. The ratio between D-band and G-band gives the information about crystallite size and surface defects, and the peaks with strong intensities indicate the cubic structure [59].Figure 10
Micro-Raman spectra of MgO nanoparticles.


## 4.5. Optical Property Analysis

### 4.5.1. UV-Visible Absorption Spectroscopy Characterization (before Calcination-as Prepared)

UV-Vis absorbance spectroscopy has revealed the optical property and electronic structure of nanoparticles. The absorbance spectrum was recorded in the range of 200 nm to 800 nm. The UV-visible absorption spectrum of MgO NPs is shown in Figures11(a) and 11(b). The absorption band edge was found at 273 nm (4.5 eV). The absorbance of MgO nanoparticles at the UV region was 273 nm due to surface plasmon resonance. The UV region absorption band at 273 nm (4.5 eV) is found with the excitation of 3-fold coordinated O2− anions in the edges and corners and defects on the surface (F centers), respectively [51, 60, 61]. The energy band gap (Eg) could be found from Tauc plot, and the formula employed is given as follows:(7)α=Ah√−Egn/h√,where α is the absorption coefficient, Eg is the absorption band gap, A is a constant, h√ is the energy of the photon, and n is the nature of transitions. The band gap value could be determined from the intercept of the straight line with the h√. The Tauc plot is shown in Figure 11(b). The computed optical band gap value 4.5 eV was considered as a lower band gap of the MgO NPs due to the presence of 3-coordinated surface anions at the corners whereas the bulk MgO material has band gap of 7.8 eV owing to the existence of 6-coordinated surface anions. The computed band gap value of MgO NPs well matches with previous reports [62–67].Figure 11
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


### 4.5.2. UV-Vis Spectroscopy in Reflectance Mode (after Calcination)

The optical properties of MgO NPs after calcination have been studied from the reflectance spectrum, and also it was recorded in the range of 200 nm to 800 nm in reflectance mode where diffuse reflectance spectrometer was employed. The optical band gap energy of MgO NPs at different calcination temperatures was calculated by Kubelka–Munk function:(8)FR=1−R2/2R,where R is the reflectance. The graph has been plotted between (F(R) hν) 2 and hν. The energy band gap value at different calcination temperatures has been calculated by extrapolation of the linear part of the (F(R) hν) 2 at the X-axis plot to the intersection with hν at Y-axis. The energy band gap value computed is 5.2 eV, 5.1 eV, and 4.9 eV for 500°, 600°, and 700°C which is illustrated in Figure 11(c). The band gap value has been decreased with increasing temperature which was observed owing to the growth of particles and crystallinity and the value is well-matched with previous reports, and the smallest band gap was observed when calcined at 700°C [68–71].


## 4.5.1. UV-Visible Absorption Spectroscopy Characterization (before Calcination-as Prepared)

UV-Vis absorbance spectroscopy has revealed the optical property and electronic structure of nanoparticles. The absorbance spectrum was recorded in the range of 200 nm to 800 nm. The UV-visible absorption spectrum of MgO NPs is shown in Figures11(a) and 11(b). The absorption band edge was found at 273 nm (4.5 eV). The absorbance of MgO nanoparticles at the UV region was 273 nm due to surface plasmon resonance. The UV region absorption band at 273 nm (4.5 eV) is found with the excitation of 3-fold coordinated O2− anions in the edges and corners and defects on the surface (F centers), respectively [51, 60, 61]. The energy band gap (Eg) could be found from Tauc plot, and the formula employed is given as follows:(7)α=Ah√−Egn/h√,where α is the absorption coefficient, Eg is the absorption band gap, A is a constant, h√ is the energy of the photon, and n is the nature of transitions. The band gap value could be determined from the intercept of the straight line with the h√. The Tauc plot is shown in Figure 11(b). The computed optical band gap value 4.5 eV was considered as a lower band gap of the MgO NPs due to the presence of 3-coordinated surface anions at the corners whereas the bulk MgO material has band gap of 7.8 eV owing to the existence of 6-coordinated surface anions. The computed band gap value of MgO NPs well matches with previous reports [62–67].Figure 11
Energy dispersive X-ray spectroscopy (EDX) spectra of MgO nanoparticle (a, b) and atomic percentage of Mg and O (c).
(a)(b)(c)


## 4.5.2. UV-Vis Spectroscopy in Reflectance Mode (after Calcination)

The optical properties of MgO NPs after calcination have been studied from the reflectance spectrum, and also it was recorded in the range of 200 nm to 800 nm in reflectance mode where diffuse reflectance spectrometer was employed. The optical band gap energy of MgO NPs at different calcination temperatures was calculated by Kubelka–Munk function:(8)FR=1−R2/2R,where R is the reflectance. The graph has been plotted between (F(R) hν) 2 and hν. The energy band gap value at different calcination temperatures has been calculated by extrapolation of the linear part of the (F(R) hν) 2 at the X-axis plot to the intersection with hν at Y-axis. The energy band gap value computed is 5.2 eV, 5.1 eV, and 4.9 eV for 500°, 600°, and 700°C which is illustrated in Figure 11(c). The band gap value has been decreased with increasing temperature which was observed owing to the growth of particles and crystallinity and the value is well-matched with previous reports, and the smallest band gap was observed when calcined at 700°C [68–71].


## 4.6. Photoluminescence Spectroscopy Analysis

### 4.6.1. Room Temperature Emission Spectroscopy

The PL spectrum of MgO nanoparticles was recorded at room temperature with a Xe lamp as an excitation light source at excitation wavelength 320 nm. Photoluminescence emission spectra are depicted in Figure12. Holes from the valence band and electrons from the electronic states recombine with each other, and this is responsible for the emission behavior of transition metals. The recombination of photoexcited electron and hole pairs at the energy states would induce the photoemission. The nature of the defects causes light emission. Photoluminescence gives the information about the impurities and defects in nanoparticles [61, 72]. The defect centers create different electronic states in the wide band gap of the material such as such F- and F2-type centers (F, F+, F21+, F22+, and F23+), cationic vacancies (VMg−2), Schottky defect (VMg0+V∘0), and interstitial oxygen atom (Oi0, Oi−1, and Oi−2), and those are responsible for multicolor emission [73]. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles shown in Tables 2 and 3. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles. It has arisen at UV-visible region. UV (359 nm), violet (377 nm, 378 nm), blue (491 nm), green (518), and orange (593 nm) emissions were found in PL spectra. Luminescence of MgO nanoparticles arises at UV region (359 nm) due to oxygen vacancies (surface defects). If defect is high, intensity will also be high. Green emission has aroused due to F centers. The green emission arises around 518 nm due to oxygen vacancies that is excitation of F (V∘0) centers [9, 10, 11]. Red orange emission arises due to relaxation luminescence of defect centers F21+ created by mechanical stress. The orange emission arises at 593 nm due to relaxation luminescence of defect centers F21+ (or V∘+1+V∘0) created by mechanical stress [9–11]. Violet emission arises due to F+ centers. The violet emissions arise due to F+ (or V∘+1) centers. Blue emission was raised by hole trapped at Mg vacancy, and it was assigned to F2 center. The blue emission around 491 nm arises due to hole trapped at Mg ion vacancy, and it was assigned to F2 center [61, 77, 78]. Multicolor emission observed in wide band gap of materials due to different electronic states there [61, 77, 78]. Multicolor emissions are observed in wide band gap materials due to different electronic states. PL optical study has given the physical property of the materials. So, according to the above study, MgO NPs will be used as potential material for optoelectronic applications.Figure 12
Photoluminescence emission spectra of MgO nanoparticles (a).Table 2
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Temperature (°C)Wavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)Emission500359UV378–413Violet491Blue518–538Green593Orange600359UV377–411Violet491Blue518–538Green593Orange700359UV377–438Violet491Blue518–538Green593OrangeTable 3
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Metal oxide NPsPeak position wavelength (observed in nm)EmissionEnergy (eV)AttributionReferencesMgO nanoparticles359UV3.45Surface defects[31, 74]378Violet3.2Defect band transition. F+ (or V∘+1) centers[31, 33, 54, 55, 75]4113.0141334382.83491Blue2.52Recombination of electrons with oxygen vacancies[31, 33, 34, 75]518Green2.39Oxygen vacancies (Vo)[31, 33, 48, 52, 53, 74, 76]538Green2.30593Orange2Relaxation luminescence of defect centers F21+created by mechanical stress[31, 48, 52, 53, 74, 76]


## 4.6.1. Room Temperature Emission Spectroscopy

The PL spectrum of MgO nanoparticles was recorded at room temperature with a Xe lamp as an excitation light source at excitation wavelength 320 nm. Photoluminescence emission spectra are depicted in Figure12. Holes from the valence band and electrons from the electronic states recombine with each other, and this is responsible for the emission behavior of transition metals. The recombination of photoexcited electron and hole pairs at the energy states would induce the photoemission. The nature of the defects causes light emission. Photoluminescence gives the information about the impurities and defects in nanoparticles [61, 72]. The defect centers create different electronic states in the wide band gap of the material such as such F- and F2-type centers (F, F+, F21+, F22+, and F23+), cationic vacancies (VMg−2), Schottky defect (VMg0+V∘0), and interstitial oxygen atom (Oi0, Oi−1, and Oi−2), and those are responsible for multicolor emission [73]. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles shown in Tables 2 and 3. The emission spectrum shows emission at different wavelengths due to different color centers on the MgO nanoparticles. It has arisen at UV-visible region. UV (359 nm), violet (377 nm, 378 nm), blue (491 nm), green (518), and orange (593 nm) emissions were found in PL spectra. Luminescence of MgO nanoparticles arises at UV region (359 nm) due to oxygen vacancies (surface defects). If defect is high, intensity will also be high. Green emission has aroused due to F centers. The green emission arises around 518 nm due to oxygen vacancies that is excitation of F (V∘0) centers [9, 10, 11]. Red orange emission arises due to relaxation luminescence of defect centers F21+ created by mechanical stress. The orange emission arises at 593 nm due to relaxation luminescence of defect centers F21+ (or V∘+1+V∘0) created by mechanical stress [9–11]. Violet emission arises due to F+ centers. The violet emissions arise due to F+ (or V∘+1) centers. Blue emission was raised by hole trapped at Mg vacancy, and it was assigned to F2 center. The blue emission around 491 nm arises due to hole trapped at Mg ion vacancy, and it was assigned to F2 center [61, 77, 78]. Multicolor emission observed in wide band gap of materials due to different electronic states there [61, 77, 78]. Multicolor emissions are observed in wide band gap materials due to different electronic states. PL optical study has given the physical property of the materials. So, according to the above study, MgO NPs will be used as potential material for optoelectronic applications.Figure 12
Photoluminescence emission spectra of MgO nanoparticles (a).Table 2
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Temperature (°C)Wavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)EmissionWavelength (nm)Emission500359UV378–413Violet491Blue518–538Green593Orange600359UV377–411Violet491Blue518–538Green593Orange700359UV377–438Violet491Blue518–538Green593OrangeTable 3
Photoluminescence emission spectra at different temperatures of MgO nanoparticles.
Metal oxide NPsPeak position wavelength (observed in nm)EmissionEnergy (eV)AttributionReferencesMgO nanoparticles359UV3.45Surface defects[31, 74]378Violet3.2Defect band transition. F+ (or V∘+1) centers[31, 33, 54, 55, 75]4113.0141334382.83491Blue2.52Recombination of electrons with oxygen vacancies[31, 33, 34, 75]518Green2.39Oxygen vacancies (Vo)[31, 33, 48, 52, 53, 74, 76]538Green2.30593Orange2Relaxation luminescence of defect centers F21+created by mechanical stress[31, 48, 52, 53, 74, 76]


## 4.7. Thermal Analysis

### 4.7.1. Thermogravimetric (TG), Differential Scanning Calorimetric (DSC), and Differential Thermal Analysis (DTA)

The thermal decomposition behavior of samples as prepared was studied by TG and DSC thermographs. The change of weight of the sample concerning temperature measure is TGA. Changes in sample composition and thermal stability can be studied with weight loss of the sample. The TGA DTA and DSC thermographs of MgO nanoparticles are shown in Figures13(a) and 13(b). The weight loss which occurs has been observed at 200- to 450-degree Celsius by exothermic peaks of DTA and DSC from the graph due to decomposition owing to absorption or removal H2O molecules and second weight loss due to the decomposition of bioactive compounds which is from the plant extract [79, 80]. The DSC curve has one endothermic peak at 660°C where maximum weight loss occurs which implies phase transition of Mg (OH)2 to MgO. Hence, the pure MgO nanoparticles have obtained with pure phase at 700°C and the obtained results are well consistent with previous reports [79, 81–87].Figure 13
TGA DTA of MgO nanoparticles and TG-DSC of MgO nanoparticles (a, b).
(a)(b)


## 4.7.1. Thermogravimetric (TG), Differential Scanning Calorimetric (DSC), and Differential Thermal Analysis (DTA)

The thermal decomposition behavior of samples as prepared was studied by TG and DSC thermographs. The change of weight of the sample concerning temperature measure is TGA. Changes in sample composition and thermal stability can be studied with weight loss of the sample. The TGA DTA and DSC thermographs of MgO nanoparticles are shown in Figures13(a) and 13(b). The weight loss which occurs has been observed at 200- to 450-degree Celsius by exothermic peaks of DTA and DSC from the graph due to decomposition owing to absorption or removal H2O molecules and second weight loss due to the decomposition of bioactive compounds which is from the plant extract [79, 80]. The DSC curve has one endothermic peak at 660°C where maximum weight loss occurs which implies phase transition of Mg (OH)2 to MgO. Hence, the pure MgO nanoparticles have obtained with pure phase at 700°C and the obtained results are well consistent with previous reports [79, 81–87].Figure 13
TGA DTA of MgO nanoparticles and TG-DSC of MgO nanoparticles (a, b).
(a)(b)


## 4.8. Electrical Properties

### 4.8.1. Real Part of Dielectric Constant (ε′)

The calcinated MgO nanopowder had pelletized by hydraulic pressure, and silver paste was coated on the surface to create better conduction. Frequency dependence of dielectric properties was studied with different temperatures from RT to 180°C (30°C, 80°C, and 130°C and 180°C). We design an energy storage device that needs to study the dielectric constant and dielectric breakdown strength which are the important parameters to calculate the energy density of the dielectrics. Dielectric loss is an important parameter for capacitor performance. The capacitance loss factor has been measured by the parallel plate capacitor method using an LCR meter for the frequency range between 100 Hz and 5 MHz for different temperatures (30°C, 80°C, and 130°C and 180°C).The dielectric constant could be calculated by the relation (1) given as follows:(9)εr=Cp×t/ε0×A,where ε0 is the permittivity of the free space (8.85 × 10–12 farad per meter (F/m), Cp is the capacitance in farad, A is an area of the cross section of pellet, and t is the thickness of pellet.The four type polarization namely space, charge, dipolar, ionic, electronic might be the reason for the dielectric nature of materials, and dielectric constant depends on these parameters. When frequency is applied from 100 Hz to 5 MHz, the Dielectric constant increases rapidly along with frequency which increases due to space charge polarization and interfacial polarization along with temperature increases from room temperature, as shown in Figures14(a)–14(c). When applied frequency increases, the dielectric constant decreases its value gradually, and at the high-frequency range, its value is constant along with different temperatures; the same trend has happened, and it obeys Koop’s theory owing to Maxwell–Wagner type interfacial polarization. At the high-frequency range, the same trend has followed at all the temperatures, the dielectric constant was found constant and merged due polarization decreases, and oxygen vacancies and grain boundaries were might be the reason for a large value of dielectric constant at lower frequency range [88, 89]. Dielectric constant value is high at low-frequency range and low at high-frequency range because of different types of polarization as said above explanation, when at high-frequency range, the electric dipoles cannot follow the frequency of applied field and dipoles cannot shift their orientation sufficiently fast when frequency is high [90, 91]. The dielectric medium has conducting grains which operate at higher frequencies and poor conducting grain boundaries which are operating at lower frequencies, while frequency applied the charge carriers are assembled at grain boundaries, so polarization occurs with high dielectric constant and polarization decreases while frequency value increases, so it has constant value at high frequency since the springing of electrons cannot cope with AC fields.Figure 14
Dielectric constant of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


## 4.8.1. Real Part of Dielectric Constant (ε′)

The calcinated MgO nanopowder had pelletized by hydraulic pressure, and silver paste was coated on the surface to create better conduction. Frequency dependence of dielectric properties was studied with different temperatures from RT to 180°C (30°C, 80°C, and 130°C and 180°C). We design an energy storage device that needs to study the dielectric constant and dielectric breakdown strength which are the important parameters to calculate the energy density of the dielectrics. Dielectric loss is an important parameter for capacitor performance. The capacitance loss factor has been measured by the parallel plate capacitor method using an LCR meter for the frequency range between 100 Hz and 5 MHz for different temperatures (30°C, 80°C, and 130°C and 180°C).The dielectric constant could be calculated by the relation (1) given as follows:(9)εr=Cp×t/ε0×A,where ε0 is the permittivity of the free space (8.85 × 10–12 farad per meter (F/m), Cp is the capacitance in farad, A is an area of the cross section of pellet, and t is the thickness of pellet.The four type polarization namely space, charge, dipolar, ionic, electronic might be the reason for the dielectric nature of materials, and dielectric constant depends on these parameters. When frequency is applied from 100 Hz to 5 MHz, the Dielectric constant increases rapidly along with frequency which increases due to space charge polarization and interfacial polarization along with temperature increases from room temperature, as shown in Figures14(a)–14(c). When applied frequency increases, the dielectric constant decreases its value gradually, and at the high-frequency range, its value is constant along with different temperatures; the same trend has happened, and it obeys Koop’s theory owing to Maxwell–Wagner type interfacial polarization. At the high-frequency range, the same trend has followed at all the temperatures, the dielectric constant was found constant and merged due polarization decreases, and oxygen vacancies and grain boundaries were might be the reason for a large value of dielectric constant at lower frequency range [88, 89]. Dielectric constant value is high at low-frequency range and low at high-frequency range because of different types of polarization as said above explanation, when at high-frequency range, the electric dipoles cannot follow the frequency of applied field and dipoles cannot shift their orientation sufficiently fast when frequency is high [90, 91]. The dielectric medium has conducting grains which operate at higher frequencies and poor conducting grain boundaries which are operating at lower frequencies, while frequency applied the charge carriers are assembled at grain boundaries, so polarization occurs with high dielectric constant and polarization decreases while frequency value increases, so it has constant value at high frequency since the springing of electrons cannot cope with AC fields.Figure 14
Dielectric constant of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


## 4.9. Imaginary Part of Dielectric Constant (ε′′)

The tan loss decreased with frequency increases, the same trend has followed at all the temperatures due to thermal-activated charges accumulated of charge carriers and space charge polarization. The imaginary part of the dielectric constant value is large at the low-frequency range as shown in Figures15(a)–15(c). The polarization mechanism, defects, and thermally activated mobile ion conduction might be the reason for the fast-rising trend of the imaginary part of dielectric constant at lower frequencies with the thermally activated conduction of mobile ions [89].Figure 15
Dielectric loss of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


## 4.10. Tan Loss

The tan loss is high at low frequency and low at high frequency due to surface polarization has reached constant value and electrons were unable to follow AC signal, so value is high at low frequency, and at high frequency, it has disappeared. The tan loss is shown in Figures16(a)–16(c). At moderate and low frequencies, polarization is high, whereas at high frequencies, charges could not follow the AC signals [88]. Due to the domination of conducting grains, the resistivity comes down, so the loss arises and saturated at high frequency, and it obeys Koop’s law. The tan loss is given by the relation (2):(10)Tan loss=ε′/ε″.Figure 16
Tan loss of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)


### 4.10.1. AC Conductivity Studies

The frequency-dependent AC conductivity of MgO nanopowder has been studied for all the three samples, and the graph has been plotted between frequency and conductivity as shown in Figures17(a)–17(c). The AC conductivity is maximum at higher temperatures with high frequency, and the same trend has been followed by all the samples of MgO nanoparticles due to charge carrier and hopping electrons also increases [92]. Moreover, it obeys the Maxwell–Wagner two-layer model according to this conductivity increases gradually along with frequency [93]. Due to polarization effects at electrode and electrolyte interface at low frequency, the variation of conductivity has occurred and all the values have merged at lower frequency owing to grains and grain boundaries which are more active, at low temperature fewer charge carriers are available, and less hoping electrons might be the reason for low conduction at low frequency [92, 93].Figure 17
AC conductivity of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)AC conductivity was calculated using the relation given as follows:(11)σ=2πfεε0tanδ,where ε0 is the permittivity of free space (8.854 × 10−12 F/m).


## 4.10.1. AC Conductivity Studies

The frequency-dependent AC conductivity of MgO nanopowder has been studied for all the three samples, and the graph has been plotted between frequency and conductivity as shown in Figures17(a)–17(c). The AC conductivity is maximum at higher temperatures with high frequency, and the same trend has been followed by all the samples of MgO nanoparticles due to charge carrier and hopping electrons also increases [92]. Moreover, it obeys the Maxwell–Wagner two-layer model according to this conductivity increases gradually along with frequency [93]. Due to polarization effects at electrode and electrolyte interface at low frequency, the variation of conductivity has occurred and all the values have merged at lower frequency owing to grains and grain boundaries which are more active, at low temperature fewer charge carriers are available, and less hoping electrons might be the reason for low conduction at low frequency [92, 93].Figure 17
AC conductivity of MgO nanoparticles at 500°C (a), 600°C (b), and 700°C (c) with different temperatures.
(a)(b)(c)AC conductivity was calculated using the relation given as follows:(11)σ=2πfεε0tanδ,where ε0 is the permittivity of free space (8.854 × 10−12 F/m).


## 4.11. Complex Spectroscopy and Impedance Analysis

### 4.11.1. Impedance Analysis (Z′ andZ″)

Complex impedance (Z∗=Z′+i⋅Z″″) has been analyzed at different temperatures on both sides of the relaxation peak. The frequency and temperature dependence of real part of impedance (z’) and imaginary part of impedance has been studied using the formulism given as follows:(12)Z′=g/Cp2ω2+G2Z″=Cpω/Cp2ω2+G,where ω is the 2 π f, G is the conductance, and Cp is the static capacitance of materials.


## 4.11.1. Impedance Analysis (Z′ andZ″)

Complex impedance (Z∗=Z′+i⋅Z″″) has been analyzed at different temperatures on both sides of the relaxation peak. The frequency and temperature dependence of real part of impedance (z’) and imaginary part of impedance has been studied using the formulism given as follows:(12)Z′=g/Cp2ω2+G2Z″=Cpω/Cp2ω2+G,where ω is the 2 π f, G is the conductance, and Cp is the static capacitance of materials.


## 4.12. Real Part of Impedance (Z′)

The increasing trend of frequency and temperature decreases the real part of impedance value owing to space charge effect and the values saturated at high frequency as shown in supplementary information FiguresS1a, S1c, and S1e, which has meant an increase of conductivity with frequency. At high frequency, the part of impedance value has merged due to the release of space charge and owing to the reduction of barrier properties or accumulation of charges at the electrode surface along with the rise of temperature [75, 94]. The decreasing trend of Z′ value at high frequency is almost low in all the samples.


## 4.13. Imaginary Part of Impedance (z”)

Oxygen vacancies in metal oxides and relaxation processes of materials are being the reason for the frequency-dependent imaginary part of impedance shifted to a higher frequency with an increase in temperature. When high temperatures are met, all the values are saturated and merged at higher frequency [75, 94]. The imaginary part of impedance is shown in supplementary information Figures S1b, S1d, and S1f.


## 4.14. Cole–Cole Plot or Nyquist Plot

The graph was drawn between the real part of impedance (Z′) and the imaginary part of impedance (Z″) as shown in supplementary information Figures S2a, S2b, and S2c. From Figure S2, it can be seen that slightly semicircle with distinct radii appears at the low frequency due to grain boundaries [75, 93, 94]. Semicircle decreases with increasing temperature due to the negative temperature coefficient of materials which are promising materials for thermistor applications.


## 4.15. Complex Electric Modulus Analysis

The real part of the electric modulus and imaginary part of electric modulus are shown in supplementary information FiguresS3 and S4a, S4b, S4c, S4d and S4e, and S4f, and all are frequency-dependent. This technique quite uses full to find the relaxation time and relaxation mechanism at the metal oxides.


## 4.16. Real Part of Electric Modulus

Electric modulus values are high at a higher frequency and at almost zero at the lower frequency which implies that electronic polarization is none [92]. The real part of the electric modulus is shown in supplementary information Figures S3a, S3b, and S3c.


## 4.17. Imaginary Part of Electric Modulus

This imaginary part of electric modulus was studied, and it explains about high conduction loss owing to electric modulus increases with the increasing trend of frequency. Peaks appearing here shifted to a higher frequency because the charge carriers transported from long-range to short-range mobility with the increase of temperature [92]. Moreover, M″ peaks shifted to higher frequencies, so we conclude that it depends on temperature and obeys hopping type mechanism for electrical conduction [92]. The imaginary part of the electric modulus spectra is shown in supplementary information Figures S4d, S4e, and S4f.


## 4.18. Complex Electric Modulus (M′ vs M″)

The complex electric modulus spectra are shown in supplementary information FiguresS5g, S5h, and S5i with different temperatures (30–230°C). From the graph, we could observe that semicircles have been formed because the grain and grain boundaries might be the reason for the conduction of the materials. At the higher frequencies and temperature, the semicircle has been disappeared on account of hopping of ions [75, 92–94].


## 4.19. M–H Loop Characterization (Magnetic Property)

Room temperature magnetization measurements were carried out where vibrating sample magnetometer (VSM) was employed for analysis. Magnetic property of MgO nanoparticles studied from M–H curves is shown in Figure18, and it is observed that all the MgO nanoparticles exhibited room temperature diamagnetism at 500 and 600°C and room temperature; week or dilute ferromagnetism has been observed from the sample while annealed at 700°C. It is diamagnetic in nature at room temperature for the two samples of MgO nanopowder due to decreased number of oxygen vacancies [52, 74]. While increasing calcination temperature, the oxygen vacancies can be improved; hence, the defect sides at the surface of the MgO nanoparticles have been increased. Panchakarla et al. and Pathak et al. have reported previously that the diamagnetic nature oxides exhibit RTFM due to defects (oxygen vacancies) present at the surface of the nanoparticles grains [95, 96]. Many reports have suggested that the room temperature ferromagnetism has been observed at the nanoscale nonmagnetic metal oxides due to anionic or cationic vacancy or size of the nanoparticles or annealing and anisotropy nature of nanomaterials [97–101]. Herein, the nanoparticles at the annealed temperature 700°C show very week ferromagnetic nature at ambient conditions with saturation magnetization value (Ms) of 57.004 E−3 emu/g and coercivity value (Hci) is 1604.5 Oe owing to the oxygen vacancies (F+ centers) have been increased with increasing annealing temperature, and while comparing with photoluminescence spectra of MgO nanoparticles, it has strong green, blue, and violet emissions. The violet and blue emissions occur on the surface of the MgO nanoparticles due to oxygen vacancies (Vo); hence, room temperature ferromagnetism (RTFM) has been observed in diamagnetic oxides owing to defect-induced magnetism. Rao et al. and Hu et al. have reported that the oxygen vacancy (F+) is the major responsible for presence of hysteresis and it shows FM or dilute magnetism in MgO nanoparticles, while temperature increases, it increases the F2+ centers which could be the reason for arising FM in MgO nanoparticles [96, 100, 102, 103].Figure 18
M–H curve of MgO nanoparticles at the room temperature.


## 5. Conclusion

Eco-friendly, surfactant-free, low-cost MgO nanoparticles were prepared successfully from the green route at different annealing temperatures. Phase purity was observed by PXRD with rising calcination temperatures where the crystal phase has not a significant change. Heat treatment has revealed that phase transition and weight loss occur due to the reduction of the hydroxyl group. FTIR studies have confirmed the formation of MgO nanoparticles. Diamagnetism property has been observed in MgO nanoparticles. Dielectric dispersion has been observed due to space charge polarization due to grain boundaries, and linear variation in dielectric constant and dielectric loss leads to MgO is a good linear dielectric ceramic and potential candidate for capacitor applications, and it is explained with the Maxwell–Wagner model. Complex impedance analysis and AC conductivity of samples rise trend with increasing frequency due to grain resistant better matches with CBH (correlated barrier hopping) model, and Nyquist plot and Complex modulus plot exhibit non-Debye relaxation type. SEM and TEM studies showed the less aggregated, polycrystalline nature of nanoparticles which were nano in size with distinct morphology with different calcination temperatures. Photoluminescence studies have revealed that the MgO nanoparticles exhibited multicolor emission in UV and Visible regions due to various defect centers (F centers), so it could be a potential candidate in optoelectronic devices and UV detectors since absorbance at UV region and it was a wide band gap material.



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