# Carboxylation and Decarboxylation of Aluminum Oxide Nanoparticles Using Bifunctional Carboxylic Acids and Octylamine

Authors: Shirin Alexander; Virginia Gomez; Andrew R. Barron
Journal: Journal of Nanomaterials
 (2016)

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## Abstract

The carboxylation of alumina nanoparticles (NPs), with bifunctional carboxylic acids, provides molecular anchors that are used for building more complexed structures via either physisorption or chemisorption. Colloidal suspensions of the NPs may be prepared by covalently bonding a series of carboxylic acids with secondary functional groups (HO2C-R-X) to the surface of the NPs: lysine (X = NH2),p-hydroxybenzoic acid (X = OH), fumaric acid (X = CO2H), and 4-formylbenzoic acid (X = C(O)H). Subsequent reaction with octylamine at either 25°C or 70°C was investigated. Fourier transform IR-attenuated reflectance spectroscopy (FTIR-ATR), thermogravimetric analysis (TGA), and scanning electron microscopy (SEM) along with energy dispersive X-ray (EDX) analysis were used to characterize the bifunctionalized monolayers and/or multilayer corona surrounding the alumina NPs and investigate the reaction mechanism of octylamine with the functional groups (X) of the NPs. Except for the fumaric functionalized NPs, addition of octylamine to the functionalized NPs leads to removal of excess carboxylic acid corona from the surface via an amide formation. The extent of the multilayer is dependent on the strength of the acid⋯acid interaction.


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## Body

## 1. Introduction

Metal oxide-based nanoparticles (NPs) are among the most commercially important nanoparticles with a wide range of applications, including fillers [1], preceramic materials allowing for controlled morphology and porosity [2, 3], biological and biomedical applications [4–10], organic based electronic devices [11], coatings [12], water purification membranes [13–17], and enhanced oil recovery (EOR) [18, 19]. To use oxide NPs in most of these applications, the particles need to be combined with organic moieties (resins, polymers, acids, etc.) in order to provide functionalized groups (molecular anchors) for further reactivity and miscibility with particular solvent systems for processing. In the case of aluminum oxide and iron oxide NPs, the most readily accessible and flexible organic functionality involves reaction of the surface with carboxylic acids (HO2CR). As such the carboxylate-oxide NP interactions have been extensively studied with some even produced commercially [20–22]. The identity of the organic substituents (R) on the carboxylate group controls the physical properties of the functionalized NP. For example, simple aliphatic hydrocarbon and fluorocarbon chains (R = CnH2n+1CnF2n+1) can be used for the creation of hydrophobic surfaces [20, 23–25], while protic substituents (i.e., OH, NH2, and SO3H) can be used to create hydrophilic surfaces [13], enhance solubility [26], and facilitate further reactivity [27, 28].We have shown that aluminum oxide wafers can be functionalized by different multifunctional acids [29], and self-assembled monolayer (SAM) or multilayers are formed depending on the type of acid used. It was also shown that octylamine coupling layers are created with the SAMs by either physisorption or chemisorption. Physisorption occurs via hydrogen bonding between the functional group of octylamine and the SAMs, thus leading to a pH dependency. In this work, however, we show the effect of octylamine on the carboxylic acid functionalized alumina NP as a decarboxylating agent rather than a coupling layer.


## 2. Materials and Methods

### 2.1. Materials

All the carboxylic acids and the amine shown in Figure1 and the aluminum oxide nanoparticles (under the trade name of Aeroxide-Alu C) were obtained from Sigma Aldrich and were used as received. The unfunctionalized NPs are fluffy, white powders with specific surface area of 100
±
15 m2·g−1 and average particle diameters of 12 nm.Figure 1
Carboxylic acids with various functional groups: (a) lysine (p
K
a: 2.18, 8.95, 10.53), (b)p-hydroxybenzoic acid (p
K
a: 4.57, 9.46), (c) fumaric acid (p
K
a: 3.03, 4.38), (d) 4-formylbenzoic acid (p
K
a: 3.84), and (e) octylamine (p
K
a: 10.65).
(a)
(b)
(c)
(d)
(e)


### 2.2. Characterization

Scanning electron microscopy (SEM) and associated energy dispersive X-ray (EDX) measurements were performed with a Hitachi Field Emission S-4800 scanning microscope. Samples were attached to a metal mount using carbon tape. Thermogravimetric/differential thermal analysis (TGA/DTA) experiments were conducted on a TA Instrument SDT Q600 using open alumina crucible under static airflow. The heating profile was equilibrated at 50°C and then ramped at 20°C min−1. Fourier transform infrared (FTIR) measurements were carried out by Thermoscientific i510, recording spectra in the 400–4000 cm−1 region with 32 scans. Zeta potential measurements (triplicate) and dynamic light scattering (DLS) were carried out using a Malvern Zetasizer Nanoseries instrument at room temperature. Particles were dispersed using an ultrasonic bath before each measurement and acidity and basicity were adjusted using 0.1 M of HNO3 and KOH as required. Nuclear magnetic resonance (1H-NMR) spectrum was recorded on a 500 MHz Bruker machine at 25°C in deuterated methanol (MeOD).


### 2.3. Synthesis of Carboxylated Alumina Nanoparticles

In a modification of the literature procedures [7, 29], the aluminum oxide nanoparticles were refluxed overnight in aqueous solutions (100 mL) of the individual carboxylic acids (1 : 2 aluminum oxide to carboxylic acid mole equiv.). Lysine is readily soluble in water; however, in order to increase the solubility of the rest of the acids, the solution’s pH was altered to above the p
K
a of each acid (see Figure 1) [30]. The functionalized particles were then washed with water, ethanol, and ether (3 × 10 mL each) to remove unreacted carboxylic acids and oven dried at 80°C overnight.


### 2.4. Reaction of Carboxylated Nanoparticles with Octylamine

The carboxylated aluminum NPs were stirred in solutions of octylamine (1 : 1.5 of acids on the surface, calculated using TGA data, to octylamine mole equiv.) in methanol (50 mL) and left stirring overnight either under refluxing conditions or at room temperature. The particles were then filtered out and were washed with pH 11 aqueous solutions (2 × 10 mL) and dried in air. Both products (prepared at room temperature or under refluxing conditions) were analyzed by TGA, IR, and EDX. In the case of the lysine functionalized NPs, the soluble side product was characterized by IR and1H-NMR spectroscopy.


## 2.1. Materials

All the carboxylic acids and the amine shown in Figure1 and the aluminum oxide nanoparticles (under the trade name of Aeroxide-Alu C) were obtained from Sigma Aldrich and were used as received. The unfunctionalized NPs are fluffy, white powders with specific surface area of 100
±
15 m2·g−1 and average particle diameters of 12 nm.Figure 1
Carboxylic acids with various functional groups: (a) lysine (p
K
a: 2.18, 8.95, 10.53), (b)p-hydroxybenzoic acid (p
K
a: 4.57, 9.46), (c) fumaric acid (p
K
a: 3.03, 4.38), (d) 4-formylbenzoic acid (p
K
a: 3.84), and (e) octylamine (p
K
a: 10.65).
(a)
(b)
(c)
(d)
(e)


## 2.2. Characterization

Scanning electron microscopy (SEM) and associated energy dispersive X-ray (EDX) measurements were performed with a Hitachi Field Emission S-4800 scanning microscope. Samples were attached to a metal mount using carbon tape. Thermogravimetric/differential thermal analysis (TGA/DTA) experiments were conducted on a TA Instrument SDT Q600 using open alumina crucible under static airflow. The heating profile was equilibrated at 50°C and then ramped at 20°C min−1. Fourier transform infrared (FTIR) measurements were carried out by Thermoscientific i510, recording spectra in the 400–4000 cm−1 region with 32 scans. Zeta potential measurements (triplicate) and dynamic light scattering (DLS) were carried out using a Malvern Zetasizer Nanoseries instrument at room temperature. Particles were dispersed using an ultrasonic bath before each measurement and acidity and basicity were adjusted using 0.1 M of HNO3 and KOH as required. Nuclear magnetic resonance (1H-NMR) spectrum was recorded on a 500 MHz Bruker machine at 25°C in deuterated methanol (MeOD).


## 2.3. Synthesis of Carboxylated Alumina Nanoparticles

In a modification of the literature procedures [7, 29], the aluminum oxide nanoparticles were refluxed overnight in aqueous solutions (100 mL) of the individual carboxylic acids (1 : 2 aluminum oxide to carboxylic acid mole equiv.). Lysine is readily soluble in water; however, in order to increase the solubility of the rest of the acids, the solution’s pH was altered to above the p
K
a of each acid (see Figure 1) [30]. The functionalized particles were then washed with water, ethanol, and ether (3 × 10 mL each) to remove unreacted carboxylic acids and oven dried at 80°C overnight.


## 2.4. Reaction of Carboxylated Nanoparticles with Octylamine

The carboxylated aluminum NPs were stirred in solutions of octylamine (1 : 1.5 of acids on the surface, calculated using TGA data, to octylamine mole equiv.) in methanol (50 mL) and left stirring overnight either under refluxing conditions or at room temperature. The particles were then filtered out and were washed with pH 11 aqueous solutions (2 × 10 mL) and dried in air. Both products (prepared at room temperature or under refluxing conditions) were analyzed by TGA, IR, and EDX. In the case of the lysine functionalized NPs, the soluble side product was characterized by IR and1H-NMR spectroscopy.


## 3. Results and Discussion

### 3.1. Carboxylation of Nanoparticles

The extent of functionalization of the as-prepared carboxylic acid functionalized alumina NPs was determined by TGA (Figure2). The as-received alumina NPs show no significant mass loss <800°C (Figure 2(a)); however, after functionalization with carboxylic acids, changes began at approximately 250°C with rapid weight loss occurring in the range 300–400°C (Figure 2(b–e)). The surface coverage (molecules per nm2) of the acids was calculated for the functionalized NPs (based on their weight loss) and is given in Table 1.Table 1
Thermogravimetric analysis of the functionalized NPs.
Sample
Wt% loss250–700°C
Residue@700°C
Grafting density(nm−2)
Lysine NPs
28.0
72.0
16.0
p-Hydroxybenzoic NPs
26.5
73.5
15.7
Fumaric NPs
47.8
52.2
47.5
4-Formylbenzoic NPs
5.8
94.2
2.5Figure 2
TGA of (a) unfunctionalized alumina NPs and alumina NPs functionalized with (b) 4-formylbenzoic acid, (c)p-hydroxybenzoic acid, (d) lysine, and (e) fumaric acid.As can be seen from the data in Table1, the fumaric acid NPs showed a grafting density significantly higher than the other acids. Based upon a theoretical grafting density this result is consistent with the formation of self-assembled multilayers through the -CO2H functionality. Such a multilayer assembly was also observed on alumina wafers [29]. Derakhshan et al. also observed similar behavior on the interaction of fumaric acid and boehmite particles [22]. Fibrous structures of fumarate-boehmite got linked “in plane” to each other through their fumarate linkages and further multilayer structures led to the formation of cubic structures.In order to confirm the covalent functionalization of the carboxylate moieties on the surface of the NPs, FTIR-ATR was performed and the data are shown in Figure3. In all cases, after reaction of acids with the NP surface, the C=O stretching band of the carboxylic acid (ca. 1700 cm−1 in Figure 3(a)) [22] is reduced and/or replaced by bands at 1425 cm−1 and 1590 cm−1 due to the symmetric and asymmetric stretches of carbonyls in bidentate bridging mode (Figure 3(b)) [22, 31]. The broad band at 3464 cm−1 of the unfunctionalized alumina NPs (Figure 3(b)) is due to the presence of hydrogen bonded OH groups on the nanoparticle surfaces [22], which is decreased upon reaction with the carboxylic acid and replaced by concomitant increase in the aliphatic/aromatic C-H stretches at around 2800 cm−1 to 3200 cm−1 as is shown in Figure 3(b).Figure 3
FTIR-ATR spectra of (a) neat carboxylic acids and (b) unfunctionalized alumina NPs, NPs functionalized with lysine,p-hydroxybenzoic acid, fumaric acid, and 4-formylbenzoic acid from top to bottom, respectively.
(a)
(b)Additional characterization of functionalized particles with carboxylic acids was undertaken by EDX analysis. The EDX analysis, shown in Table2, indicates that the surface of the unfunctionalized particles on average is composed of aluminum (30.9%) and oxygen (66.1%) and small percentage of adventitious carbon (2.9%). The Al : O ratio (0.47) is consistent with the hydrated nature of the NPs observed in the IR spectrum (Figure 3(b)). As would be expected, functionalization of the NPs with the acids increases the carbon composition with a decrease in the aluminum content (Table 2). The smallest increase in carbon % is obtained for 4-formylbenzoic NPs with only 1.3 C% increase, which correlates with the TGA data that showed the smallest grafting density for these NPs. There is also a small increase in the C : Al ratio (0.14) as compared to the unfunctionalized NPs (0.09).Table 2
Energy dispersive X-ray (EDX) analysis (atom%  ±1.5) of native and carboxylic acid functionalized NPs.
Surface
C
Al
O
N
C : Al
Alumina NP
2.9
30.9
66.1
—
0.09
Lysine NPs
16.2
24.6
56.2
3.0
0.65
p-Hydroxybenzoic acid NPs
31.7
20.5
47.8
—
1.54
Fumaric acid NPs
31.0
20.6
47.9
—
1.50
4-Formylbenzoic acid NPs
4.2
30.1
65.7
—
0.14The surface charge of the nanoparticles and their calculated isoelectric points (IEP) were achieved using zeta potential measurements. Figure4 shows a plot of zeta potential versus pH for the four functionalized alumina NPs and the native alumina NPs. The data can be used to determine the approximated isoelectric point (IEP) of the particles. Generally, if the IEP is <7 the surface is considered acidic and over pH 7 the surface is basic [32]. As expected, the reference alumina NPs show an IEP value of pH 9.0 close to the values obtained for pseudoboehmite [33]. Figure 4 shows that lysine NPs, p-hydroxybenzoic acid NPs, and 4-formylbenzoic acid NPs have isoelectric points between pH 8 and 10. On the other hand, the fumaric acid functionalized surfaces show a significant change in their surface behavior being more acidic than alumina NPs. These particles have an isoelectric point close to pH 5 due to the presence of an additional negatively charged carboxylic group on their surfaces. A similar effect in the IEP behavior has been observed by Meder et al. when functionalizing alumina NPs with carboxylic acids [5].Figure 4
Zeta potential values of the different NPs versus pH in aqueous suspensions.As pH increases, the particle size for carboxylated particles increases. This is due to the agglomeration and seeded particle growth [34]. The dissolution of aluminium oxides is at its minimum in the neutral pH range [32]; thus the hydrodynamic diameter of the functionalized nanoparticles was measured at pH range 4-5 to avoid dissolution processes. Figure 5 shows differences in the agglomeration state of the samples due to their differences in particle surface behavior. All the nanoparticles showed hydrodynamic diameter distributions around 100 nm at pH values between 4 and 5. The fumaric acid functionalized NPs show agglomeration in this pH range and this is because this pH is close to the isoelectric point as defined by the zeta potential results (Figure 4).Figure 5
Hydrodynamic diameter distributions of the different NPs in aqueous suspensions at pH range 4-5.


### 3.2. Addition of the Octylamine to the Functionalized Nanoparticles

In our recent work we showed that the carboxylated surfaces could undergo further reactivity via their surface functional groups [29]. Two methods (immersing and refluxing) were used for further coating of the aluminum surfaces and the analysis results confirmed that the coupling self-assembled layer is pH responsive and reversible at lower pH under the first method and mainly irreversible under the second method based on the outer functional group of the self-assembled layers. The same experiments were carried out on the carboxylic acid functionalized alumina NPs; however, the results were unexpected. The TGA data, shown in Table 3, revealed that upon reaction of the NPs with octylamine (Figure 1(e)) the weight loss is smaller in all cases apart from fumaric acid NPs, whose weight loss is larger. The EDX analysis of the NPs after reaction with octylamine is consistent with the appropriate TGA data. Apart from the fumaric acid NPs, the carbon content decreases, regardless of the reaction temperature; see Table 4; however, the decrease in C% is higher for the products of the reaction at 70°C as compared to those reacted at 25°C. Clearly, the NPs are not reacting in an analogous manner to that observed for alumina surfaces [29].Table 3
Thermogravimetric analysis of the functionalized NPs reacted with octylamine at 25°C and 70°C.
Sample
Reaction temp.(°C)
Wt% loss250–700°Ca
Residue@700°Ca
Lysine NPs
25
17.4
82.6
70
9.9
90.1
p-Hydroxybenzoic NPs
25
18.1
81.9
70
18.1
81.9
Fumaric NPs
25
48.0
52.0
70
48.5
51.5
4-Formylbenzoic NPs
25
6.6
93.4
70
6.8
93.2
aCompare to values for carboxylate NPs given in Table 1.Table 4
Energy dispersive X-ray (EDX) analysis (atom% ±1.5) of the various carboxylic acid functionalized NPs after reaction with octylamine.
Reaction
Temp. (°C)
C
Al
O
N
C : Al
Lysine NPs + octylamine
25
28.8
26.1
44.5
0.5
1.1
70
4.9
31.9
60.9
0.5
0.15
p-Hydroxybenzoic acid NPs + octylamine
25
10.4
28.7
60.7
0.1
0.36
70
7.7
30.8
60.7
0.6
0.25
Fumaric acid NPs + octylamine
25
32.0
20.4
47.1
0.5
1.56
70
31.8
19.0
48.9
0.6
1.67
4-Formylbenzoic acid NPs + octylamine
25
2.9
41.12
55.9
—
0.07
70
2.8
31.1
66.3
0.4
0.09To have a better understanding of the NPs functionalization (or defunctionalization) after the addition of octylamine the particles were studied by FTIR. Figure6 shows the IR spectra of all the functionalized NPs after addition of octylamine. Based on the TGA and EDX results, fumaric acid NPs are the only particles that did not lose their functional groups upon addition of octylamine and this was confirmed by FTIR. Comparing Figure 6 with Figure 3(b) shows that two characteristic peaks of carboxylic acids bidentate modes at 1425 cm−1 and 1590 cm−1 reduced significantly upon reaction with octylamine for all the samples, except for fumaric acid NPs. There are peaks in all cases that feature octylamine, for example, three defined peaks at 2853, 2919, and 2953 cm−1 characteristic of symmetric and asymmetric -CH2 and asymmetric -CH3 stretches and the broad peaks at 3094–3410 cm−1 due to the presence of the secondary amide/N-H stretches [7, 11, 35]. This indicates that primary role of the octylamine is to remove the majority of the carboxylic acid groups adsorbed on the surface but it secondarily reacts with the surface functional groups of the carboxylic acids via chemical reaction and/or hydrogen bonding as was seen for the alumina wafers [29].Figure 6
FTIR-ATR spectra of all the functionalized NPs, reacted with octylamine (refluxed).Carboxylic acids and amines react together to form salts, and strong heating (to remove water) of these salts leads to amide formation [36, 37]. There are various factors influencing the yield of the reaction, including stirring conditions, temperature, solvent, and reagent’s concentration [38]. The removal of the carboxylate from the surface of the NPs suggests that the reaction with excess of octylamine may lead to formation of an amide. To confirm this proposal the filtrate solutions of the lysine NPs reacted with octylamine were analyzed by FTIR and NMR and are shown in Figures 7 and 8, respectively.Figure 7
The FTIR spectra of the pure lysine and the filtrate solutions of the lysine NPs reacted with octylamine.Figure 8
1H-NMR profile for byproduct of the lysine NPs reacted with octylamine. Peak assignment is as follows: δ (ppm) 0.86 [3H, t, -CH
3], 1.3–1.7 (18H, m, aliphatic C-H), 2.75 (2H, m, -CH
2-NH2-), and 3.28 (2H, m, -CH
2-NH-). The numbers on top of each peak represent the atom on the shown structure.The lysine IR spectrum is compared with the reaction by-product in Figure7. As can be seen, there is evidence of both lysine and amide in the solutions (rather than just unreacted octylamine). Peaks at 3169, 3320, and 3360 cm−1 are due to secondary amide N-H stretches as well as primary amine N-H stretches, and the strong peak at 1568 cm−1 is characteristic of amide N-H bending. It should be noted that the small peak is at 1620 cm−1; this peak is due to amide C=O stretches that partially overlap the N-H bending mode. The NMR spectrum from the filtrate (Figure 8) shows the presence of the amide N-H at 3.28 ppm. If there was only amide present in the solution the peak should have had the integral of 2; however, from the integral of 1.72, we can determine that around 80% of the product is related to amide and the rest is excess octylamine. Details of peak assignments and integrations are given in the legend of Figure 8.Based upon the forgoing, we propose that the following process is present. Upon the initial reaction of the carboxylic acids with the preformed alumina NPs there is surface functionalization in the manner described previously for both organometallic clusters [39] and alumina nanoparticles prepared directly from boehmite [20, 33]. However, unlike these systems, the presence of secondary functionality results in a greater than monolayer reaction, that is, a larger grafting density than calculated from the ideal surface coverage [39]. While this excess carboxylic acid corona is bound via hydrogen bonding, the interaction is sufficiently strong that it is not removed with repeating washing.The extent of the excess carboxylic acid corona around the NP appears to be dependent on the strength of the acid⋯acid interaction. Based upon TGA data (Table1) and the calculated grafting density as compared to an ideal surface coverage we can estimate the extent of the corona. Thus, the 4-formylbenzoic NPs appear to be close to monolayer coverage, while lysine NPs andp-hydroxybenzoic NPs show defined multilayer corona consistent with stronger N-H⋯O and O-H⋯O hydrogen bonding associated with amine⋯carboxylic acid or phenol⋯carboxylic acid interactions [40, 41]. The greater strength of the carboxylic acid dimer involving cyclic dimers with two strong C=O⋯H-O hydrogen bonds [42, 43] results in an extensive multilayer structure for the fumaric acid derivative.Upon addition of octylamine to the 4-formylbenzoic, lysine, andp-hydroxybenzoic derivatives the excess acid is removed by the formation of soluble ammonium carboxylic acid salts or amides. What remain are the covalently bound carboxylate moieties, to which excess octylamine reacts through either hydrogen bonding. In the case of the 4-formylbenzoic derivative heating the reaction mixture results in hydration and the formation of the appropriate amide. A schematic representation of this process is shown in Figure 9. We note that carboxylic acids have been shown to react with amine terminated functionalized metal oxide NPs [44], and the coupling represented herein signifies the observed reaction.Figure 9
Schematic representation of the reaction of carboxylic acids with preformed alumina nanoparticles and their subsequent reaction with octylamine.


## 3.1. Carboxylation of Nanoparticles

The extent of functionalization of the as-prepared carboxylic acid functionalized alumina NPs was determined by TGA (Figure2). The as-received alumina NPs show no significant mass loss <800°C (Figure 2(a)); however, after functionalization with carboxylic acids, changes began at approximately 250°C with rapid weight loss occurring in the range 300–400°C (Figure 2(b–e)). The surface coverage (molecules per nm2) of the acids was calculated for the functionalized NPs (based on their weight loss) and is given in Table 1.Table 1
Thermogravimetric analysis of the functionalized NPs.
Sample
Wt% loss250–700°C
Residue@700°C
Grafting density(nm−2)
Lysine NPs
28.0
72.0
16.0
p-Hydroxybenzoic NPs
26.5
73.5
15.7
Fumaric NPs
47.8
52.2
47.5
4-Formylbenzoic NPs
5.8
94.2
2.5Figure 2
TGA of (a) unfunctionalized alumina NPs and alumina NPs functionalized with (b) 4-formylbenzoic acid, (c)p-hydroxybenzoic acid, (d) lysine, and (e) fumaric acid.As can be seen from the data in Table1, the fumaric acid NPs showed a grafting density significantly higher than the other acids. Based upon a theoretical grafting density this result is consistent with the formation of self-assembled multilayers through the -CO2H functionality. Such a multilayer assembly was also observed on alumina wafers [29]. Derakhshan et al. also observed similar behavior on the interaction of fumaric acid and boehmite particles [22]. Fibrous structures of fumarate-boehmite got linked “in plane” to each other through their fumarate linkages and further multilayer structures led to the formation of cubic structures.In order to confirm the covalent functionalization of the carboxylate moieties on the surface of the NPs, FTIR-ATR was performed and the data are shown in Figure3. In all cases, after reaction of acids with the NP surface, the C=O stretching band of the carboxylic acid (ca. 1700 cm−1 in Figure 3(a)) [22] is reduced and/or replaced by bands at 1425 cm−1 and 1590 cm−1 due to the symmetric and asymmetric stretches of carbonyls in bidentate bridging mode (Figure 3(b)) [22, 31]. The broad band at 3464 cm−1 of the unfunctionalized alumina NPs (Figure 3(b)) is due to the presence of hydrogen bonded OH groups on the nanoparticle surfaces [22], which is decreased upon reaction with the carboxylic acid and replaced by concomitant increase in the aliphatic/aromatic C-H stretches at around 2800 cm−1 to 3200 cm−1 as is shown in Figure 3(b).Figure 3
FTIR-ATR spectra of (a) neat carboxylic acids and (b) unfunctionalized alumina NPs, NPs functionalized with lysine,p-hydroxybenzoic acid, fumaric acid, and 4-formylbenzoic acid from top to bottom, respectively.
(a)
(b)Additional characterization of functionalized particles with carboxylic acids was undertaken by EDX analysis. The EDX analysis, shown in Table2, indicates that the surface of the unfunctionalized particles on average is composed of aluminum (30.9%) and oxygen (66.1%) and small percentage of adventitious carbon (2.9%). The Al : O ratio (0.47) is consistent with the hydrated nature of the NPs observed in the IR spectrum (Figure 3(b)). As would be expected, functionalization of the NPs with the acids increases the carbon composition with a decrease in the aluminum content (Table 2). The smallest increase in carbon % is obtained for 4-formylbenzoic NPs with only 1.3 C% increase, which correlates with the TGA data that showed the smallest grafting density for these NPs. There is also a small increase in the C : Al ratio (0.14) as compared to the unfunctionalized NPs (0.09).Table 2
Energy dispersive X-ray (EDX) analysis (atom%  ±1.5) of native and carboxylic acid functionalized NPs.
Surface
C
Al
O
N
C : Al
Alumina NP
2.9
30.9
66.1
—
0.09
Lysine NPs
16.2
24.6
56.2
3.0
0.65
p-Hydroxybenzoic acid NPs
31.7
20.5
47.8
—
1.54
Fumaric acid NPs
31.0
20.6
47.9
—
1.50
4-Formylbenzoic acid NPs
4.2
30.1
65.7
—
0.14The surface charge of the nanoparticles and their calculated isoelectric points (IEP) were achieved using zeta potential measurements. Figure4 shows a plot of zeta potential versus pH for the four functionalized alumina NPs and the native alumina NPs. The data can be used to determine the approximated isoelectric point (IEP) of the particles. Generally, if the IEP is <7 the surface is considered acidic and over pH 7 the surface is basic [32]. As expected, the reference alumina NPs show an IEP value of pH 9.0 close to the values obtained for pseudoboehmite [33]. Figure 4 shows that lysine NPs, p-hydroxybenzoic acid NPs, and 4-formylbenzoic acid NPs have isoelectric points between pH 8 and 10. On the other hand, the fumaric acid functionalized surfaces show a significant change in their surface behavior being more acidic than alumina NPs. These particles have an isoelectric point close to pH 5 due to the presence of an additional negatively charged carboxylic group on their surfaces. A similar effect in the IEP behavior has been observed by Meder et al. when functionalizing alumina NPs with carboxylic acids [5].Figure 4
Zeta potential values of the different NPs versus pH in aqueous suspensions.As pH increases, the particle size for carboxylated particles increases. This is due to the agglomeration and seeded particle growth [34]. The dissolution of aluminium oxides is at its minimum in the neutral pH range [32]; thus the hydrodynamic diameter of the functionalized nanoparticles was measured at pH range 4-5 to avoid dissolution processes. Figure 5 shows differences in the agglomeration state of the samples due to their differences in particle surface behavior. All the nanoparticles showed hydrodynamic diameter distributions around 100 nm at pH values between 4 and 5. The fumaric acid functionalized NPs show agglomeration in this pH range and this is because this pH is close to the isoelectric point as defined by the zeta potential results (Figure 4).Figure 5
Hydrodynamic diameter distributions of the different NPs in aqueous suspensions at pH range 4-5.


## 3.2. Addition of the Octylamine to the Functionalized Nanoparticles

In our recent work we showed that the carboxylated surfaces could undergo further reactivity via their surface functional groups [29]. Two methods (immersing and refluxing) were used for further coating of the aluminum surfaces and the analysis results confirmed that the coupling self-assembled layer is pH responsive and reversible at lower pH under the first method and mainly irreversible under the second method based on the outer functional group of the self-assembled layers. The same experiments were carried out on the carboxylic acid functionalized alumina NPs; however, the results were unexpected. The TGA data, shown in Table 3, revealed that upon reaction of the NPs with octylamine (Figure 1(e)) the weight loss is smaller in all cases apart from fumaric acid NPs, whose weight loss is larger. The EDX analysis of the NPs after reaction with octylamine is consistent with the appropriate TGA data. Apart from the fumaric acid NPs, the carbon content decreases, regardless of the reaction temperature; see Table 4; however, the decrease in C% is higher for the products of the reaction at 70°C as compared to those reacted at 25°C. Clearly, the NPs are not reacting in an analogous manner to that observed for alumina surfaces [29].Table 3
Thermogravimetric analysis of the functionalized NPs reacted with octylamine at 25°C and 70°C.
Sample
Reaction temp.(°C)
Wt% loss250–700°Ca
Residue@700°Ca
Lysine NPs
25
17.4
82.6
70
9.9
90.1
p-Hydroxybenzoic NPs
25
18.1
81.9
70
18.1
81.9
Fumaric NPs
25
48.0
52.0
70
48.5
51.5
4-Formylbenzoic NPs
25
6.6
93.4
70
6.8
93.2
aCompare to values for carboxylate NPs given in Table 1.Table 4
Energy dispersive X-ray (EDX) analysis (atom% ±1.5) of the various carboxylic acid functionalized NPs after reaction with octylamine.
Reaction
Temp. (°C)
C
Al
O
N
C : Al
Lysine NPs + octylamine
25
28.8
26.1
44.5
0.5
1.1
70
4.9
31.9
60.9
0.5
0.15
p-Hydroxybenzoic acid NPs + octylamine
25
10.4
28.7
60.7
0.1
0.36
70
7.7
30.8
60.7
0.6
0.25
Fumaric acid NPs + octylamine
25
32.0
20.4
47.1
0.5
1.56
70
31.8
19.0
48.9
0.6
1.67
4-Formylbenzoic acid NPs + octylamine
25
2.9
41.12
55.9
—
0.07
70
2.8
31.1
66.3
0.4
0.09To have a better understanding of the NPs functionalization (or defunctionalization) after the addition of octylamine the particles were studied by FTIR. Figure6 shows the IR spectra of all the functionalized NPs after addition of octylamine. Based on the TGA and EDX results, fumaric acid NPs are the only particles that did not lose their functional groups upon addition of octylamine and this was confirmed by FTIR. Comparing Figure 6 with Figure 3(b) shows that two characteristic peaks of carboxylic acids bidentate modes at 1425 cm−1 and 1590 cm−1 reduced significantly upon reaction with octylamine for all the samples, except for fumaric acid NPs. There are peaks in all cases that feature octylamine, for example, three defined peaks at 2853, 2919, and 2953 cm−1 characteristic of symmetric and asymmetric -CH2 and asymmetric -CH3 stretches and the broad peaks at 3094–3410 cm−1 due to the presence of the secondary amide/N-H stretches [7, 11, 35]. This indicates that primary role of the octylamine is to remove the majority of the carboxylic acid groups adsorbed on the surface but it secondarily reacts with the surface functional groups of the carboxylic acids via chemical reaction and/or hydrogen bonding as was seen for the alumina wafers [29].Figure 6
FTIR-ATR spectra of all the functionalized NPs, reacted with octylamine (refluxed).Carboxylic acids and amines react together to form salts, and strong heating (to remove water) of these salts leads to amide formation [36, 37]. There are various factors influencing the yield of the reaction, including stirring conditions, temperature, solvent, and reagent’s concentration [38]. The removal of the carboxylate from the surface of the NPs suggests that the reaction with excess of octylamine may lead to formation of an amide. To confirm this proposal the filtrate solutions of the lysine NPs reacted with octylamine were analyzed by FTIR and NMR and are shown in Figures 7 and 8, respectively.Figure 7
The FTIR spectra of the pure lysine and the filtrate solutions of the lysine NPs reacted with octylamine.Figure 8
1H-NMR profile for byproduct of the lysine NPs reacted with octylamine. Peak assignment is as follows: δ (ppm) 0.86 [3H, t, -CH
3], 1.3–1.7 (18H, m, aliphatic C-H), 2.75 (2H, m, -CH
2-NH2-), and 3.28 (2H, m, -CH
2-NH-). The numbers on top of each peak represent the atom on the shown structure.The lysine IR spectrum is compared with the reaction by-product in Figure7. As can be seen, there is evidence of both lysine and amide in the solutions (rather than just unreacted octylamine). Peaks at 3169, 3320, and 3360 cm−1 are due to secondary amide N-H stretches as well as primary amine N-H stretches, and the strong peak at 1568 cm−1 is characteristic of amide N-H bending. It should be noted that the small peak is at 1620 cm−1; this peak is due to amide C=O stretches that partially overlap the N-H bending mode. The NMR spectrum from the filtrate (Figure 8) shows the presence of the amide N-H at 3.28 ppm. If there was only amide present in the solution the peak should have had the integral of 2; however, from the integral of 1.72, we can determine that around 80% of the product is related to amide and the rest is excess octylamine. Details of peak assignments and integrations are given in the legend of Figure 8.Based upon the forgoing, we propose that the following process is present. Upon the initial reaction of the carboxylic acids with the preformed alumina NPs there is surface functionalization in the manner described previously for both organometallic clusters [39] and alumina nanoparticles prepared directly from boehmite [20, 33]. However, unlike these systems, the presence of secondary functionality results in a greater than monolayer reaction, that is, a larger grafting density than calculated from the ideal surface coverage [39]. While this excess carboxylic acid corona is bound via hydrogen bonding, the interaction is sufficiently strong that it is not removed with repeating washing.The extent of the excess carboxylic acid corona around the NP appears to be dependent on the strength of the acid⋯acid interaction. Based upon TGA data (Table1) and the calculated grafting density as compared to an ideal surface coverage we can estimate the extent of the corona. Thus, the 4-formylbenzoic NPs appear to be close to monolayer coverage, while lysine NPs andp-hydroxybenzoic NPs show defined multilayer corona consistent with stronger N-H⋯O and O-H⋯O hydrogen bonding associated with amine⋯carboxylic acid or phenol⋯carboxylic acid interactions [40, 41]. The greater strength of the carboxylic acid dimer involving cyclic dimers with two strong C=O⋯H-O hydrogen bonds [42, 43] results in an extensive multilayer structure for the fumaric acid derivative.Upon addition of octylamine to the 4-formylbenzoic, lysine, andp-hydroxybenzoic derivatives the excess acid is removed by the formation of soluble ammonium carboxylic acid salts or amides. What remain are the covalently bound carboxylate moieties, to which excess octylamine reacts through either hydrogen bonding. In the case of the 4-formylbenzoic derivative heating the reaction mixture results in hydration and the formation of the appropriate amide. A schematic representation of this process is shown in Figure 9. We note that carboxylic acids have been shown to react with amine terminated functionalized metal oxide NPs [44], and the coupling represented herein signifies the observed reaction.Figure 9
Schematic representation of the reaction of carboxylic acids with preformed alumina nanoparticles and their subsequent reaction with octylamine.


## 4. Conclusions

Functionalization of alumina NPs with various bifunctional carboxylic acids results in chemically bonded multilayers whose extent depends on the surface functional groups. For example, fumaric acid functionalized NPs undergo reaction with at least a 4-fold excess of fumaric acid to create a stable corona. There have previously been reports of the significance of protein corona about NPs [45, 46]; however, little has been investigated for simpler functionality. We have shown that the carboxylic acid corona can be partially or fully removed by using an amine (octylamine) as a reagent wash, under certain temperature, stirring condition, and concentration. This is in contrast to the results obtained for thin films, where a simple pH responsive coupling layer was formed via a hydrogen bonding between the amine and the outer layer of the functionalized wafers [29]. The only functionalized NPs unaffected were fumaric acid NPs, which retained their functionality as well as gaining some interaction with octylamine. As such the treatment of bifunctional carboxylic acid (HO2C-R-X) functionalized alumina NPs with an amine, such as octylamine, should be a routine process for the purification of the functionalized NPs to ensure the removal of excess carboxylic acid. We note, however, that this appears to be limited by the acid⋯acid interaction, since, as in the case of fumaric acid, removal of the functional groups does not happen and/or hardly happens.



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