# Chain Length and Thermal Sensitivity of the Infrared Spectra of a Homologous Series of Anhydrous Silver(I)n-Alkanoates

Authors: Peter N. Nelson
Journal: International Journal of Spectroscopy
 (2016)

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## Abstract

The thermal and chain length sensitivity of the infrared spectra of some solid state anhydrous silver(I) salts (n-octanoate ton-eicosanoate, inclusive) are discussed. At ambient temperature, the tilted alkyl chains, anchored to the metal planes via chelating bidentate coordination to the silver ions, are crystallized in the fully extendedall-trans conformation. Interestingly, though all compounds are crystallized in a monoclinic crystal system, their lateral chain packing,van der Waals effects, and hence vibrational features are chain length-dependent. This is a direct result of electrostatic effects of the COO group in addition to vibrational coupling between CH2, CH3, and COO modes, an effect which varies significantly with chain length. Variable temperature infrared measurements indicate significant irreversible changes in the metal-carboxyl coordination sphere, most likely due to bond fission. For long chain adducts (nc>12), thermally induced crystal system switching, monoclinic to triclinic, indicates greater thermal sensitivity of their alkyl chains. During heating, the regions of the hydrocarbon chains, furthest from the COO, become increasingly molten and mobile as the stepwise melt advances towards the solid COO moieties. This solid-liquid melting behaviour is responsible for mesophase formation in metal carboxylate systems.


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## Body

## 1. Introduction

The ability of metal carboxylates to form three-dimensional self-assembled layered structures in addition to diverse coordination modes, in the solid state, is some of their most fascinating structural attributes. However, for most long chain adducts, single crystal data is sparse due to their low molecular symmetries which caused the significant flexibility of the alkyl chains; hence, they usually solidify as thin needle-like or twinned plate-lake crystals, unsuitable for single crystal diffraction. Nonetheless, crystal structures for various short chain homologues have been published [1–3]. For example, crystal structures for both silver(I) acetate [4] and propanoate [5] show carboxylate groups coordinated in asyn-syn type bridging bidentate mode to silver ions, forming dimeric units, held together via extensive interdimer electrostatic forces. Silver-silver distances in these units allowed for extensive metal-metal interactions and possibly bonding. However, though both crystal structures agreed on the type of metal-carboxyl bonding, their molecular and lattice packing were different. For instance, silver acetate was triclinic withP1 symmetry whilst the monoclinic propanoate was ofP21/a Bravais lattice. Indeed, this difference shows clearly that their molecular packing is chain length dependent but their coordination to the central metal ion is physically isostructural. Though further structural changes for longer chain adducts might be gradual, the sensitivity of vibrational spectroscopy to lattice packing provides an invaluable tool for assessing such changes. Surely, the industrial importance of silvern-alkanoates stemming from their wide spread use as low angle calibrants for neutron diffraction instruments [6] and as silver sources in photothermogravimetry (PTG) and photography [7–10], makes relevant a detailed study of their molecular and lattice packing, based on a method, nondestructive to sensitive intermolecular interactions. Furthermore, given the difficulties associated with obtaining single crystals for the long chain adducts, in addition to the destructive nature of X-rays, vibrational features associated with different molecular packing and intralattice interactions are significant. Also, since, like many amphiphilic systems, silver carboxylates exhibit various premelting phases when heated from the room temperature solid to the melt, some of which have been described as liquid crystalline [11], the effect on temperature on their lattice packing is of interest. For example, Nelson [12–14] and Binnemans et al. [11] showed that for silver carboxylates (AgC4⋯C28) the number of premelting phases increases with increasing chain length, the melt being at highest temperature, as is common for these compounds. However, the suggestion by Binnemans that more than one liquid crystalline phases were present in the phase sequences for some silver compounds was questioned by Nelson, based on high temperature microscopy data, but not totally ruled out. The difficulty associated with characterizing the phases of these compounds stems from the fact that they decompose at the melt-to-yield nanoclusters [15]. This suggests that they could possibly be applied in the solid state thermal synthesis of nanoparticles for various applications. Therefore, it is clear that the evolution of their structural features with chain length and temperature is of importance. Furthermore, since it has been recently proven by Berson and coworkers [16] that it is possible to electrochemically influence the growth of a silver nanowires on the surface of carboxyl terminated alkyl silane self-assembly monolayers in the absence of moisture, it is also clear that silver-carboxyl interactions are of significant technological importance.Therefore, in this paper, the vibrational features of some anhydrous silver carboxylates (AgC8⋯C20) are discussed in detail and are correlated with their respective molecular and lattice packing interactions. Their structural evolution is also assessed as a function of chain length and temperature.


## 2. Experimental

The white microcrystalline solids were prepared by metathesis, that is, reaction of the sodium salt of then-alkanoic acids (Aldrich, 95+%), in ethanol, with an excess of aqueous silver nitrate (Aldrich, 99.9%) atca. 343 K. The sodium salts were prepared by dissolving the relevantn-alkanoic acid inca. 50 cm3 of ethanol which was then combined withca. 50 cm3 of ethanol containing a stoichiometric amount of sodium hydroxide (Aldrich, 99.9%) whilst stirring. Subsequent to stirring the aforementioned mixture for a 30 min., an aqueous solution of silver nitrate was added, drop-wise with stirring, to the as prepared sodiumn-alkanoate solution. This resulted in immediate precipitation of a white solid. After stirring for a further 30 min., at ambient temperature, the precipitate was collected by filtration, washed thrice with a solution of 1 : 1 acetone-methylene chloride mixture, and vacuum dried for 24 h. The compounds were then stored in the dark (because of their sensitivity to light), in a desiccator over silica gel. Calculated yields were in excess of 90%. C-H analysis, reported elsewhere [12], proves that the compounds are of high purity.Infrared spectra were recorded from ground samples, deposited on a germanium window of a Bruker Tensor 37 AT-FT IR spectrometer in the range of 4000–500 cm−1 at a resolution of ±1 cm−1. Variable temperature measurements were made using a specially constructed devise which was calibrated for temperature control prior to each measurement.


## 3. Results and Discussion

### 3.1. Room Temperature FT-Infrared Spectroscopy

The infrared spectra for all compounds are typical for metal carboxylates; that is, they are composed of low, high, and medium intensity bands, distributed between 3500 and 500 cm−1. In fact, their spectra can be divided into three main regions: the methyl and methylene group stretching region (2840–2980 cm−1), the carboxylate region (1565–1470 cm−1), and the low frequency region between 1470 and 500 cm−1, generally termed as the “methylene progression region.” However, this region represents more than just the CH2 progression and is very important (vide infra).Vibrations associated with the asymmetric (νas) and symmetric (νs) carboxyl (COO) stretching modes (Figure 1(a)) are located in the regions of ~1565 and ~1420 cm−1, respectively. These bands, formed as a result of complete resonance in the carboxyl moieties due to coordination with the metal, show significant structural sensitivity; hence, they are extensively used in the literature for the characterization of metal-carboxyl coordination and symmetry [11–15]. For example, the difference in stretching frequencies between these two vibrations, Δν=νas-νs, is related to the type of metal-carboxyl bonding; that is, if Δν≈100 cm−1, chelating coordination is indicated but for those in the region of 150 to 170 cm−1, bridging bidentate bonding is likely [17–19]. However, values in excess of 200 cm−1 indicate that the C-O bonds are highly asymmetric; thus coordination is monodentate. The presence of extensive intermolecular interactions in the vicinity of the carboxyl group reduces the accuracy of this type analysis [20]. Hence, though Δν for silver carboxylates is in the range of 97–101 cm−1, crystal structure data, for the short adducts, show that metal-carboxyl bonding is bridging bidentate with extensive intercarboxyl interactions [5]. Interestingly, X-ray powder data showed that their coordination is independent of chain length [12]; that is, they are isostructural where metal-carboxyl bonding is concerned. The greater intensity of the νasCOO relative to the νsCOO band is indicative of nonequivalent C-O bonds, possibly due to different degrees of interaction with the metal ion; that is, metal-carboxyl bonding is asymmetric. Surely, such bonding arrangement at the carboxyl groups would result in chain tilting as was concluded by Binnemans et al. [11], based on synchrotron data and Nelson [12, 14] and based on X-ray diffraction.Figure 1
(a) Carboxyl stretching (νasCOO and νsCOO) and methylene bending mode (δCH2) for AgC11. (b) The methylene twisting, rocking, and progression regions for AgC11.
(a)
(b)Splitting of the carboxyl bands, as observed, is indicative of reduced COO symmetry; hence, energetic separation of degenerate COO vibrational modes persists as the selection rules governing the excitation of these vibrational modes break down. Indeed, this effect is also encouraged by coupling interactions between the C-O vibrations and the stretching mode of the adjacent carbon-carbon bond (C-COO) which bears significant double bond character as a result of resonance in the adjacent carboxyl group. In addition to the νasCOO and νsCOO bands, this region also consists of another structure sensitive vibration in the form of a sharp medium intensity peak, centered atca. 1472 cm−1, associated with methylene (δCH2) bending mode. For instance, splitting of this band due to intermolecular interactions between closely spaced alkyl chains is observed for monoclinic packing whilst a sharp band is indicative of triclinic arrangement where such interactions are less significant [17, 21]. Interestingly, for the compounds discussed here, this band is not split (Figure 1) but is quite broad (Full width half maximum, FWHM: >10 cm−1) with a low frequency shoulder. This indicates that the silver salts reported here are most likely monoclinic as previously reported based on X-ray powder diffraction data [12, 22].The neighboring region, ~1400 to 700 cm−1, consists of several bands associated with the combination vibrations of the polymethylene chain. These bands are highly sensitive to alkyl chain structure and packing; hence, a detailed description of their most informative features is presented (vide infra). Furthermore, since the phase properties of metal carboxylates and other amphiphilic systems are controlled by chain packing and structure, a basic knowledge of the features of these bands is of high importance [23–25]. Subdivision of this region reveals the methylene twisting-rocking, τ-δCH2 (1175–1300 cm−1) and rocking-twisting (700–1060 cm−1) modes, henceforth referred to as the twisting and rocking modes, respectively, to avoid confusion. This region also consists of the CH2 wagging bands: 1170–1370 cm−1. However, unliken-paraffins, where intensity alternation allows for differentiation between the overlapping wagging and twisting modes, the bands of this region are of very low intensities; hence, they are difficult to characterize for silver(I)n-carboxylates. Indeed, similar observations were reported by Snyder and Schachtschneider [26], for long chainn-paraffins; however, some amount of characterization was still possible. The array of methylene twisting vibrations (Figure 2(b)), for silver carboxylates, shows decreased frequencies with increased chain length, a change which is more drastic for shorter chain adducts and for the high frequency bands of this region. This is possibly due to the gradual decrease in alkyl chains polarization. Hence, for shorter chain compounds, where the chains are more polar due to closer proximity of the CH2 groups to the COO, that is, larger COO : CH2 ratios, alkyl chain vibrations are more dependent on the structure of the carboxyl group. Such vibrational interference between the COO and CH2 modes can alter -CH2-CH2- coupling and, hence, lattice packing. However, assuming that this effect is minute and that the CH2 groups behave like linearly coupled identical oscillators (m) with a single degree of freedom, the simple coupled oscillator theory (SCO) can be applied as was possible forn-paraffins [26]. This model shows that the phase difference between adjacent oscillators (φk) is given by φk=kπ/m+1, k=1,2,3,…,m. Hence, the vibration frequencies (υk) of δ-τCH2 motions are controlled primarily by φk; therefore, assigning values of k such that all bands fit to a similar curve yields Figure 2(a) which gives information about CH2-CH2 coupling changes with chain length. Interestingly, the bands for all compounds fit to separate curves unlike forn-paraffins where a single curve was observed. This suggest that the addition of a single methylene group to the alkyl chain results in significant changes in their coupled vibrations and hence molecular packing. This effect is reflected in their total molar enthalpies where the CH2 contribution is exponentially related to the number of methylene groups [14]. The presence of the COO group significantly affects the polarity of the alkyl chains and hence the observed changes in their vibrational frequencies and coupling interactions with increased chain length. Such significant chain length dependence of this effect is strongly reflected in φk; hence, it is different for all compounds (Figure 2(a)). Clearly, the phase differences are more significant for longer chain adducts most likely because the CH2 groups are less affected by the carboxyl group and are therefore more independent in their vibrational motions. This assertion is supported by the convergence of φk above 1280 cm−1 where the COO group influence is quite significant. Furthermore, solid state 13C-NMR data [12] shows clearly that the electron density distribution (polarity) of silver carboxylates is highly chain length-dependent; that is, the influence of the COO group decreases with increased chain length.Figure 2
(a) Frequency phase curves for the methylene twisting-rocking (τ-δCH2) modes for all chain lengths (AgC8⋯C20, inclusive) at room temperature. (b) Room temperature array of the methylene twisting-rocking bands (τ-δCH2) bands for silver(I)n-alkanoates (AgC8⋯C20, inclusive).
(a)
(b)The carbon-carbon stretching (νC-C) bands, for silver carboxylates, atca. 1115 cm−1, are among the most intense in this region, occurring at a frequency similar to that for lead(II) [27], 1128 cm−1, and cerium(III) [28], 1106–1112 cm−1,n-alkanoates. Interestingly, for silvern-eicosanoate, this band exists as a sharp singlet, atca. 1114.8 cm−1, but becomes increasingly broad with decreasing chain length; that is, a low frequency shoulder centered atca. 1108 cm−1 begins to emerge for nc<18. At nc=16, this band is completely split with components at ~1115 and ~1099 cm−1. This is a clear indication of changes in the alkyl chain electron density distribution and hence structure and packing with chain length. However, such subtle changes were not observed in reported X-ray data [12]. However, solid state 13C-NMR results showed clear changes in their electron densities with increased chain length; that is, the long chain homologues were composed of more carbons that were electronically indistinguishable compared to the shorter chain adducts.The region of 700–1060 cm−1 consists of several low intensity bands, primarily associated with the rocking mode of the methylene groups (ρCH2). However, it should be noted that none of these bands can be completely designated as purely rocking since there is always contamination from the twisting modes, an effect which decreases monotonically with decreasing frequency. Hence, the band of highest intensity, centered atca. 718 cm−1, present for polymethylene chains with more than four successive CH2 groups, represents the purest form of ρCH2 motion and is commonly referred to as the CH2 rocking band [29]. This vibration is highly sensitive to chain packing and is therefore often used in the accurate prediction of crystal packing. For example, splitting or excessive broadening caused by close packing of adjacent alkyl chains in the lattice, as observed for silvern-carboxylates, suggests monoclinic or orthorhombic packing whilst a sharp band correlates with a triclinic or hexagonal crystal system [30]. Interestingly, the four additional bands associated with the CH2 rocking-twisting motion, in this region, show no obvious trend with chain length. However, according to Snyder [21], (n-1)/2 and (n-2)/2 bands are allowed for odd and even chainn-paraffins having n carbon atoms, respectively, whilst for silvern-alkanoates a similar relationship is observed but only for the τ-δCH2 bands in the region of 1175–1300 cm−1. For instance, (n/2)+1 and (n+1)/2 bands are allowed for odd and even chain silvern-carboxylates, respectively. This indicates that though the general vibrational behaviours of metaln-carboxylates andn-paraffins are similar, they are not identical; that is, the presence of the COO group and the metal significantly alters their vibrational features. Also, it should be noted that, liken-paraffins where the CH2/CH3 ratio affects the frequencies of these bands, for silver salts this effect is more significant since, in addition to this ratio, the CH2/COO ratio has a similar effect. This shows clearly that the spectral features for hydrocarbon type molecules can be significantly altered by the presence of different substituents. In fact, it was shown that structural manipulations as simple as the geographic location of a triple bond, in unsaturated zinc(II)n-alkanoates, resulted in significant changes in their liquid crystalline and spectral features [31].Other sensitive bands associated with alkyl chain packing are located in the region of 2800–3000 cm−1. This region consists of four main bands ascribed to the symmetric (νs) and asymmetric (νas) stretching modes of the hydrogens attached to the methyl (νasCH3) and methylene carbons (νasCH2). The sensitivity of these bands to alkyl chain symmetry and intermolecular interactions are manifested as odd-even alternation in the νasCH3, atca. 2955 cm−1, discussed in [12]; that is, lower frequencies were observed for odd chain compounds as a result of greatervan der Waals interactions caused by more intimate interplanar packing of the alkyl chains. It was proposed, as supported by density data, that the vertical interlayer spacing was less for odd chain adducts; hence, the closely packed methyl groups are more polarized and facilitative of methyl-methylene carbon-hydrogen electrostatic interactions which reduced the C-H bond order [12–14]. This effect is also reflected in the shape of the νasCH3 band where the FWHM and peak areas for odd chain adducts are only ~50% of those for the even chain homologues. This is due to increased overlapping of the vibrational frequencies associated with the CH3 hydrogen(s) that are polarized parallel (2962 cm−1) and perpendicular (2955 cm−1) to the hydrocarbon plane. Similar frequency values, adduced from single crystals, were reported for both C-H polarization directions inn-paraffins [32]. The other bands in this region are associated with the νasCH2 and νsCH2 modes, atca. 2849 and 2917 cm−1, respectively [33–35]. Integration of these bands yields a constant relative area (νasCH2/νsCH2) of ~2.3 which is in reasonably good agreement with that for crystallinen-hexane andn-heptane where a value of 3.0±0.4 was adduced based on a “simple Raman bond moment model” for tetrahedral CH2 geometry [36]. This indicates that the CH2 groups of silver(I)n-alkanoates are tetrahedral as expected. Comparison of the CH2 stretching frequencies for crystallinen-alkanes in theall-trans conformation (νasCH2~2847 and νsCH2~2916 cm−1) to those for silvern-alkanoates shows that their alkyl chains are ~99.95%all-trans, at ambient temperature, and are therefore fully extended. Interestingly, like the methyl asymmetric stretching band, νasCH2 is also quite broad, bearing a shoulder on both its high and low frequency sides (Figure 3(a)). The shoulder on the low frequency side corresponds accurately to the first overtone of the CH2 bending, intensified by fermi resonance with the νasCH2 vibration. However, the high frequency shoulder is probably due to correlation splitting common for orthorhombic or monoclinic crystal systems and should be accompanied by a second weaker band of a different polarization, similar to observations reported forn-paraffins [37, 38].Figure 3
(a) Typical methyl and methylene group stretching region for AgC20. (b) Typical carboxyl stretching region for long (nc>12; AgC20) and (c) short (nc<12; AgC9) chain silver(I)n-carboxylate at different temperatures.
(a)
(b)
(c)


### 3.2. Variable Temperature FT-Infrared Spectroscopy

Super-ambient FT-Infrared measurements show,inter alia, increased stretching frequencies, reduced intensities, disappearance, and even the emergence of new bands in the spectra for these silver(I)n-alkanoates. For example, the carboxyl stretching region shows significant changes with increased temperature; that is, progressive decrease in both νasCOO and νsCOO bands is observed, especially for long chain adducts (Figure 3(b)). However, beyond 338 K there is no further decrease in the intensity of the νsCOO band though the νasCOO peak has almost completely disappeared at this temperature (Figure 3(b)). Interestingly, simultaneous with the decrease in intensity of the low frequency component of the νasCOO vibration, there is significant increase in the intensity of the band at 1560 cm−1, the high frequency component of this vibrational mode. Surely, this is indicative of significant bonding and symmetry changes in the metal-carboxyl coordination sphere. Furthermore, since Δν has increased, it is reasonable to propose that metal-carboxyl bonding tends towards monodentate coordination with increased temperature. This idea is also supported by the significant reduction and near disappearance of the νsCOO band, a change which correlates with reduced coordination number of the metal. However, though short chain adducts also show noteworthy changes in their COO vibrations (Figure 3(c)) and eventually decompose at the melt [11–14], the fact that both COO stretching modes are preserved, with intensities similar to room temperature, even at 360 K, it is clear that their degradation mechanisms and/or energetics are different from the long chain homologues. It is possible that, for these chain lengths, metal-carboxyl interaction is more rigid as is common for the short chain compounds; hence, their bonding changes occur at higher temperatures as do their melts [11, 12, 15].These observations correlate with reports, by various authors [11, 15], showing that on heating, long chain silver carboxylates undergo significant irreversible changes. Such changes eventually lead to decomposition at the melt-to-yield silver nanoclusters [15]. Indeed, this indicates that they could find application as precursors in the solid state thermal synthesis of nanoparticles for various applications. Furthermore, if methods reported by Hermans and coworkers [39] for the synthesis of dimetal carboxylates are employed, the formation of silver dimetal salts of the form RCOOAgyMx could be possible, thermal decomposition of which could yield mixed metal quantum dots. Also, since long and short chain silver carboxylates behave differently at elevated temperatures, it is possible that their decomposition products are different. Unfortunately, there are no comprehensive reports where the decomposition mechanism and kinetics of a homologous series of silver carboxylates are clearly established.In addition to changes in the carboxyl absorptions, the methylene bending mode, at 1472 cm−1, shows a significant decrease in intensity with increased temperature, for both long and short chain adducts (Figures 3(b) and 3(c)). This is indicative of significant changes in their lattice packing as the hydrocarbon chains become increasingly molten andgauche-trans isomerization becomes more pronounced. This assertion is supported by significant reduction in the intensities of CH2, wagging, twisting, and rocking bands, all of which nearly disappearances completely above 350 K. The C-C stretching bands at ~1114 and 1096 cm−1 also show significant reduction in their intensities as well as complete disappearance of at least one component without coalescence. In fact, at high temperatures, the 1114 cm−1 band becomes increasingly broad, indicating that even at high temperatures there is still distinct carbon environment present in the alkyl chain as discussed (vide supra). The principal CH2 rocking band centered at ~719 cm−1 shows a ~97% decrease in intensity (Figure 4(b)), in addition to disappearance of the shoulder observed at room temperature for long chain adducts but for short chain compounds its shape is preserved. This suggests that the melting behaviour for long and short chain compounds is not identical; hence, different numbers of phase transitions have been reported for them [13]. The decrease in intensity of the CH2 rocking band is also an indication of reduced crystalline order but interestingly, the fact that the features of this band which correlates with monoclinic packing (splitting), at ambient temperature, changed to that for triclinic packing (no splitting); it is clear that the melting mechanism, for long chain compounds, involves structural transition from a monoclinic to a thermally induced triclinic state. However, for short chain compounds this transitions is not present; that is, their room temperature structures are more stable than for the long chain homologues. Extrapolation of the intensity-temperature variation of this peak shows that it should be almost zero at 370 K, a temperature corresponding to the range for the first transition for compounds with 8 to 15 carbon atoms, inclusive. This indicates that the first transition for these short chain compounds is associated, mainly, with alkyl chain melting and reduced crystal system order. However, for long chain adducts, at this temperature, the monoclinic arrangement and crystal system order are almost totally lost due to their greater thermal sensitivity.Figure 4
(a) Typical methyl and methylene stretching region and (b) methylene progression region at different temperatures. (c) Methylene asymmetric : symmetric stretching band intensity ratios versus temperature (equation:y=0.0113x-2.2597, R2=0.9843). (d) von t’ Hoff plot for the effect of temperature on the trans⇄gauche interconversion equilibrium constant K (equation: y=-3727.5x-9.0684, R2=0.9927).
(a)
(b)
(c)
(d)The high frequency bands ascribed to the C-H symmetric and asymmetric stretching vibrations of the CH2 and CH3 groups also show significant temperature sensitivity (Figure 4(a)). For instance, both νsCH3 and νasCH3 bands, atca. 2874 and 2955 cm−1, respectively, decrease simultaneously in intensity with increased temperature, indicating increased rotational freedom of the methyl and methylene groups due to reducevan der Waals interactions as the alkyl chains become increasingly molten. Coalescence of the parallel and perpendicularly polarized methyl νasC-H modes correlate with polarization isotropy and reduced interplanarvan der Waals interactions due to increased CH3 rotational freedom. Similar changes in the CH2 stretching bands with increased temperature provide significant insights into the thermally induced structural and conformational evolution of the methylene group population and hence the alkyl chains. For example, increased temperature results in marked reduction of both νasCH2 and νsCH2 intensities due to reduce conformation order of the alkyl chains. Interestingly, intensity ratios of these peaks, in Raman, associated with the C-H stretching vibrations, are known to be sensitive to the alkyl chain conformational order and environment [40–43]. Hence, a basic quantitative model allowing assessment of the lateral chain packing order(S) of alkyl chain was defined: S=r-0.7/1.5, where r is the intensity ratio of CH2 asymmetric (I−) : symmetric (I+) stretching modes, so that S is unity for crystalline alkyl chains and zero for those in the liquid state [44]. This method has been applied in the structural studies of cholesteric liquid crystals [40] and biomembranes [41, 42]. However, for these compounds, a plot S versus temperature gave a positive slope which would indicate that the alkyl chains become more orderly with increased temperature, an obviously incorrect result. This indicates that the model does not hold true for silver carboxylates. Nonetheless, since the ratio of CH2 (I−/I+) increases with temperature (Figure 4(c)), it is clear that the percentagegauche conformation in the methylene group assembly follows the same trend, as expected, and hence the observed increased asymmetric stretching probability.Based on Figure4(c), the intensities of both bands should be equal atca. 289 K; that is, lateral packing is optimum in this temperature range: the alkyl chains are 100%all-trans. The slope of this plot represents the temperature coefficient of lateral chain packing order: ∂S/∂T=1.13×10-2 K−1 or the thermal sensitivity of chain packing. The magnitude of this parameter describes the strength of the intermolecular forces associated with lattice stability; that is, larger values should result for low melting point alkyl chain assemblies: weak interchainvan der Waals forces; hence, this value should be much smaller for short chain compounds. In addition to reduced intensities, these bands also show changes in their frequencies; that is, with increased temperature both νasCH2 and νsCH2 bands shift to higher frequencies. This is due to increasedgauche conformation population and hence chain kinking. Indeed, thegauche population can be assessed at different temperatures by comparing the stretching frequencies ofall-trans crystallinen-alkanes to these compounds. Therefore, if Trans⇆Gauche isomerization is viewed as a reversible equilibrium, then an estimation of the equilibrium constant (K) at different temperatures based on (1)K=1-n-alkane/νsCH2n-alkane/νsCH2is possible. Therefore, a plot of lnK versus 1/T (K−1) (Figure 4(d)) gives the average isomerization enthalpy and entropy as 30.99 kJ mol−1 and 75.39 J mol−1 K−1, respectively. Surely, these values are not identical over different segments of the melting process as result of heat capacity changes in the methylene group assembly, especially during phase transitions where the density of the lattice changes significantly due to reduce chain packing order. This type of assessment is only valid over small temperature intervals. It is also worthy of note that the magnitude of such energy changes is affected by intermolecular forces of interactions in the lattice. By the fact that these values are large relative to those reported for sodium and potassium carboxylates [14, 22, 24], greatervan der Waals interactions are indicated. However, higher melting temperatures for sodium and potassium carboxylates are due to greater electrostatic forces associated with the metal-carboxyl bonding.Infrared measurements collected on cooling the samples show considerable changes at room temperature. For instance, though the methylene rocking band, centered atca. 720 cm−1, at room temperature, returns to its original intensity, there is a slight shift to lower frequency (~717 cm−1). The C-C stretching and methylene twisting bands also show considerable changes; coalescence and broadening are most obvious, along with reduced intensities. Surely, this confirms that, on heating, even without reaching the melt, the structures of these compounds are permanently changed especially where metal-carboxyl coordination is concerned. For example, both COO modes, on cooling, do not reappear; that is, the changes observed on heating are permanent. Reemergence of the methyl and methylene C-H stretching bands on cooling, though not totally, indicates that despite significant changes in the metal-carboxyl coordination sphere, the alkyl chains remain intact up to 360 K. However, it is imaginable that as temperature tends towards the melt, the aforementioned changes will become more significant as proven by García and coworkers [23], for potassiumn-carboxylates.


## 3.1. Room Temperature FT-Infrared Spectroscopy

The infrared spectra for all compounds are typical for metal carboxylates; that is, they are composed of low, high, and medium intensity bands, distributed between 3500 and 500 cm−1. In fact, their spectra can be divided into three main regions: the methyl and methylene group stretching region (2840–2980 cm−1), the carboxylate region (1565–1470 cm−1), and the low frequency region between 1470 and 500 cm−1, generally termed as the “methylene progression region.” However, this region represents more than just the CH2 progression and is very important (vide infra).Vibrations associated with the asymmetric (νas) and symmetric (νs) carboxyl (COO) stretching modes (Figure 1(a)) are located in the regions of ~1565 and ~1420 cm−1, respectively. These bands, formed as a result of complete resonance in the carboxyl moieties due to coordination with the metal, show significant structural sensitivity; hence, they are extensively used in the literature for the characterization of metal-carboxyl coordination and symmetry [11–15]. For example, the difference in stretching frequencies between these two vibrations, Δν=νas-νs, is related to the type of metal-carboxyl bonding; that is, if Δν≈100 cm−1, chelating coordination is indicated but for those in the region of 150 to 170 cm−1, bridging bidentate bonding is likely [17–19]. However, values in excess of 200 cm−1 indicate that the C-O bonds are highly asymmetric; thus coordination is monodentate. The presence of extensive intermolecular interactions in the vicinity of the carboxyl group reduces the accuracy of this type analysis [20]. Hence, though Δν for silver carboxylates is in the range of 97–101 cm−1, crystal structure data, for the short adducts, show that metal-carboxyl bonding is bridging bidentate with extensive intercarboxyl interactions [5]. Interestingly, X-ray powder data showed that their coordination is independent of chain length [12]; that is, they are isostructural where metal-carboxyl bonding is concerned. The greater intensity of the νasCOO relative to the νsCOO band is indicative of nonequivalent C-O bonds, possibly due to different degrees of interaction with the metal ion; that is, metal-carboxyl bonding is asymmetric. Surely, such bonding arrangement at the carboxyl groups would result in chain tilting as was concluded by Binnemans et al. [11], based on synchrotron data and Nelson [12, 14] and based on X-ray diffraction.Figure 1
(a) Carboxyl stretching (νasCOO and νsCOO) and methylene bending mode (δCH2) for AgC11. (b) The methylene twisting, rocking, and progression regions for AgC11.
(a)
(b)Splitting of the carboxyl bands, as observed, is indicative of reduced COO symmetry; hence, energetic separation of degenerate COO vibrational modes persists as the selection rules governing the excitation of these vibrational modes break down. Indeed, this effect is also encouraged by coupling interactions between the C-O vibrations and the stretching mode of the adjacent carbon-carbon bond (C-COO) which bears significant double bond character as a result of resonance in the adjacent carboxyl group. In addition to the νasCOO and νsCOO bands, this region also consists of another structure sensitive vibration in the form of a sharp medium intensity peak, centered atca. 1472 cm−1, associated with methylene (δCH2) bending mode. For instance, splitting of this band due to intermolecular interactions between closely spaced alkyl chains is observed for monoclinic packing whilst a sharp band is indicative of triclinic arrangement where such interactions are less significant [17, 21]. Interestingly, for the compounds discussed here, this band is not split (Figure 1) but is quite broad (Full width half maximum, FWHM: >10 cm−1) with a low frequency shoulder. This indicates that the silver salts reported here are most likely monoclinic as previously reported based on X-ray powder diffraction data [12, 22].The neighboring region, ~1400 to 700 cm−1, consists of several bands associated with the combination vibrations of the polymethylene chain. These bands are highly sensitive to alkyl chain structure and packing; hence, a detailed description of their most informative features is presented (vide infra). Furthermore, since the phase properties of metal carboxylates and other amphiphilic systems are controlled by chain packing and structure, a basic knowledge of the features of these bands is of high importance [23–25]. Subdivision of this region reveals the methylene twisting-rocking, τ-δCH2 (1175–1300 cm−1) and rocking-twisting (700–1060 cm−1) modes, henceforth referred to as the twisting and rocking modes, respectively, to avoid confusion. This region also consists of the CH2 wagging bands: 1170–1370 cm−1. However, unliken-paraffins, where intensity alternation allows for differentiation between the overlapping wagging and twisting modes, the bands of this region are of very low intensities; hence, they are difficult to characterize for silver(I)n-carboxylates. Indeed, similar observations were reported by Snyder and Schachtschneider [26], for long chainn-paraffins; however, some amount of characterization was still possible. The array of methylene twisting vibrations (Figure 2(b)), for silver carboxylates, shows decreased frequencies with increased chain length, a change which is more drastic for shorter chain adducts and for the high frequency bands of this region. This is possibly due to the gradual decrease in alkyl chains polarization. Hence, for shorter chain compounds, where the chains are more polar due to closer proximity of the CH2 groups to the COO, that is, larger COO : CH2 ratios, alkyl chain vibrations are more dependent on the structure of the carboxyl group. Such vibrational interference between the COO and CH2 modes can alter -CH2-CH2- coupling and, hence, lattice packing. However, assuming that this effect is minute and that the CH2 groups behave like linearly coupled identical oscillators (m) with a single degree of freedom, the simple coupled oscillator theory (SCO) can be applied as was possible forn-paraffins [26]. This model shows that the phase difference between adjacent oscillators (φk) is given by φk=kπ/m+1, k=1,2,3,…,m. Hence, the vibration frequencies (υk) of δ-τCH2 motions are controlled primarily by φk; therefore, assigning values of k such that all bands fit to a similar curve yields Figure 2(a) which gives information about CH2-CH2 coupling changes with chain length. Interestingly, the bands for all compounds fit to separate curves unlike forn-paraffins where a single curve was observed. This suggest that the addition of a single methylene group to the alkyl chain results in significant changes in their coupled vibrations and hence molecular packing. This effect is reflected in their total molar enthalpies where the CH2 contribution is exponentially related to the number of methylene groups [14]. The presence of the COO group significantly affects the polarity of the alkyl chains and hence the observed changes in their vibrational frequencies and coupling interactions with increased chain length. Such significant chain length dependence of this effect is strongly reflected in φk; hence, it is different for all compounds (Figure 2(a)). Clearly, the phase differences are more significant for longer chain adducts most likely because the CH2 groups are less affected by the carboxyl group and are therefore more independent in their vibrational motions. This assertion is supported by the convergence of φk above 1280 cm−1 where the COO group influence is quite significant. Furthermore, solid state 13C-NMR data [12] shows clearly that the electron density distribution (polarity) of silver carboxylates is highly chain length-dependent; that is, the influence of the COO group decreases with increased chain length.Figure 2
(a) Frequency phase curves for the methylene twisting-rocking (τ-δCH2) modes for all chain lengths (AgC8⋯C20, inclusive) at room temperature. (b) Room temperature array of the methylene twisting-rocking bands (τ-δCH2) bands for silver(I)n-alkanoates (AgC8⋯C20, inclusive).
(a)
(b)The carbon-carbon stretching (νC-C) bands, for silver carboxylates, atca. 1115 cm−1, are among the most intense in this region, occurring at a frequency similar to that for lead(II) [27], 1128 cm−1, and cerium(III) [28], 1106–1112 cm−1,n-alkanoates. Interestingly, for silvern-eicosanoate, this band exists as a sharp singlet, atca. 1114.8 cm−1, but becomes increasingly broad with decreasing chain length; that is, a low frequency shoulder centered atca. 1108 cm−1 begins to emerge for nc<18. At nc=16, this band is completely split with components at ~1115 and ~1099 cm−1. This is a clear indication of changes in the alkyl chain electron density distribution and hence structure and packing with chain length. However, such subtle changes were not observed in reported X-ray data [12]. However, solid state 13C-NMR results showed clear changes in their electron densities with increased chain length; that is, the long chain homologues were composed of more carbons that were electronically indistinguishable compared to the shorter chain adducts.The region of 700–1060 cm−1 consists of several low intensity bands, primarily associated with the rocking mode of the methylene groups (ρCH2). However, it should be noted that none of these bands can be completely designated as purely rocking since there is always contamination from the twisting modes, an effect which decreases monotonically with decreasing frequency. Hence, the band of highest intensity, centered atca. 718 cm−1, present for polymethylene chains with more than four successive CH2 groups, represents the purest form of ρCH2 motion and is commonly referred to as the CH2 rocking band [29]. This vibration is highly sensitive to chain packing and is therefore often used in the accurate prediction of crystal packing. For example, splitting or excessive broadening caused by close packing of adjacent alkyl chains in the lattice, as observed for silvern-carboxylates, suggests monoclinic or orthorhombic packing whilst a sharp band correlates with a triclinic or hexagonal crystal system [30]. Interestingly, the four additional bands associated with the CH2 rocking-twisting motion, in this region, show no obvious trend with chain length. However, according to Snyder [21], (n-1)/2 and (n-2)/2 bands are allowed for odd and even chainn-paraffins having n carbon atoms, respectively, whilst for silvern-alkanoates a similar relationship is observed but only for the τ-δCH2 bands in the region of 1175–1300 cm−1. For instance, (n/2)+1 and (n+1)/2 bands are allowed for odd and even chain silvern-carboxylates, respectively. This indicates that though the general vibrational behaviours of metaln-carboxylates andn-paraffins are similar, they are not identical; that is, the presence of the COO group and the metal significantly alters their vibrational features. Also, it should be noted that, liken-paraffins where the CH2/CH3 ratio affects the frequencies of these bands, for silver salts this effect is more significant since, in addition to this ratio, the CH2/COO ratio has a similar effect. This shows clearly that the spectral features for hydrocarbon type molecules can be significantly altered by the presence of different substituents. In fact, it was shown that structural manipulations as simple as the geographic location of a triple bond, in unsaturated zinc(II)n-alkanoates, resulted in significant changes in their liquid crystalline and spectral features [31].Other sensitive bands associated with alkyl chain packing are located in the region of 2800–3000 cm−1. This region consists of four main bands ascribed to the symmetric (νs) and asymmetric (νas) stretching modes of the hydrogens attached to the methyl (νasCH3) and methylene carbons (νasCH2). The sensitivity of these bands to alkyl chain symmetry and intermolecular interactions are manifested as odd-even alternation in the νasCH3, atca. 2955 cm−1, discussed in [12]; that is, lower frequencies were observed for odd chain compounds as a result of greatervan der Waals interactions caused by more intimate interplanar packing of the alkyl chains. It was proposed, as supported by density data, that the vertical interlayer spacing was less for odd chain adducts; hence, the closely packed methyl groups are more polarized and facilitative of methyl-methylene carbon-hydrogen electrostatic interactions which reduced the C-H bond order [12–14]. This effect is also reflected in the shape of the νasCH3 band where the FWHM and peak areas for odd chain adducts are only ~50% of those for the even chain homologues. This is due to increased overlapping of the vibrational frequencies associated with the CH3 hydrogen(s) that are polarized parallel (2962 cm−1) and perpendicular (2955 cm−1) to the hydrocarbon plane. Similar frequency values, adduced from single crystals, were reported for both C-H polarization directions inn-paraffins [32]. The other bands in this region are associated with the νasCH2 and νsCH2 modes, atca. 2849 and 2917 cm−1, respectively [33–35]. Integration of these bands yields a constant relative area (νasCH2/νsCH2) of ~2.3 which is in reasonably good agreement with that for crystallinen-hexane andn-heptane where a value of 3.0±0.4 was adduced based on a “simple Raman bond moment model” for tetrahedral CH2 geometry [36]. This indicates that the CH2 groups of silver(I)n-alkanoates are tetrahedral as expected. Comparison of the CH2 stretching frequencies for crystallinen-alkanes in theall-trans conformation (νasCH2~2847 and νsCH2~2916 cm−1) to those for silvern-alkanoates shows that their alkyl chains are ~99.95%all-trans, at ambient temperature, and are therefore fully extended. Interestingly, like the methyl asymmetric stretching band, νasCH2 is also quite broad, bearing a shoulder on both its high and low frequency sides (Figure 3(a)). The shoulder on the low frequency side corresponds accurately to the first overtone of the CH2 bending, intensified by fermi resonance with the νasCH2 vibration. However, the high frequency shoulder is probably due to correlation splitting common for orthorhombic or monoclinic crystal systems and should be accompanied by a second weaker band of a different polarization, similar to observations reported forn-paraffins [37, 38].Figure 3
(a) Typical methyl and methylene group stretching region for AgC20. (b) Typical carboxyl stretching region for long (nc>12; AgC20) and (c) short (nc<12; AgC9) chain silver(I)n-carboxylate at different temperatures.
(a)
(b)
(c)


## 3.2. Variable Temperature FT-Infrared Spectroscopy

Super-ambient FT-Infrared measurements show,inter alia, increased stretching frequencies, reduced intensities, disappearance, and even the emergence of new bands in the spectra for these silver(I)n-alkanoates. For example, the carboxyl stretching region shows significant changes with increased temperature; that is, progressive decrease in both νasCOO and νsCOO bands is observed, especially for long chain adducts (Figure 3(b)). However, beyond 338 K there is no further decrease in the intensity of the νsCOO band though the νasCOO peak has almost completely disappeared at this temperature (Figure 3(b)). Interestingly, simultaneous with the decrease in intensity of the low frequency component of the νasCOO vibration, there is significant increase in the intensity of the band at 1560 cm−1, the high frequency component of this vibrational mode. Surely, this is indicative of significant bonding and symmetry changes in the metal-carboxyl coordination sphere. Furthermore, since Δν has increased, it is reasonable to propose that metal-carboxyl bonding tends towards monodentate coordination with increased temperature. This idea is also supported by the significant reduction and near disappearance of the νsCOO band, a change which correlates with reduced coordination number of the metal. However, though short chain adducts also show noteworthy changes in their COO vibrations (Figure 3(c)) and eventually decompose at the melt [11–14], the fact that both COO stretching modes are preserved, with intensities similar to room temperature, even at 360 K, it is clear that their degradation mechanisms and/or energetics are different from the long chain homologues. It is possible that, for these chain lengths, metal-carboxyl interaction is more rigid as is common for the short chain compounds; hence, their bonding changes occur at higher temperatures as do their melts [11, 12, 15].These observations correlate with reports, by various authors [11, 15], showing that on heating, long chain silver carboxylates undergo significant irreversible changes. Such changes eventually lead to decomposition at the melt-to-yield silver nanoclusters [15]. Indeed, this indicates that they could find application as precursors in the solid state thermal synthesis of nanoparticles for various applications. Furthermore, if methods reported by Hermans and coworkers [39] for the synthesis of dimetal carboxylates are employed, the formation of silver dimetal salts of the form RCOOAgyMx could be possible, thermal decomposition of which could yield mixed metal quantum dots. Also, since long and short chain silver carboxylates behave differently at elevated temperatures, it is possible that their decomposition products are different. Unfortunately, there are no comprehensive reports where the decomposition mechanism and kinetics of a homologous series of silver carboxylates are clearly established.In addition to changes in the carboxyl absorptions, the methylene bending mode, at 1472 cm−1, shows a significant decrease in intensity with increased temperature, for both long and short chain adducts (Figures 3(b) and 3(c)). This is indicative of significant changes in their lattice packing as the hydrocarbon chains become increasingly molten andgauche-trans isomerization becomes more pronounced. This assertion is supported by significant reduction in the intensities of CH2, wagging, twisting, and rocking bands, all of which nearly disappearances completely above 350 K. The C-C stretching bands at ~1114 and 1096 cm−1 also show significant reduction in their intensities as well as complete disappearance of at least one component without coalescence. In fact, at high temperatures, the 1114 cm−1 band becomes increasingly broad, indicating that even at high temperatures there is still distinct carbon environment present in the alkyl chain as discussed (vide supra). The principal CH2 rocking band centered at ~719 cm−1 shows a ~97% decrease in intensity (Figure 4(b)), in addition to disappearance of the shoulder observed at room temperature for long chain adducts but for short chain compounds its shape is preserved. This suggests that the melting behaviour for long and short chain compounds is not identical; hence, different numbers of phase transitions have been reported for them [13]. The decrease in intensity of the CH2 rocking band is also an indication of reduced crystalline order but interestingly, the fact that the features of this band which correlates with monoclinic packing (splitting), at ambient temperature, changed to that for triclinic packing (no splitting); it is clear that the melting mechanism, for long chain compounds, involves structural transition from a monoclinic to a thermally induced triclinic state. However, for short chain compounds this transitions is not present; that is, their room temperature structures are more stable than for the long chain homologues. Extrapolation of the intensity-temperature variation of this peak shows that it should be almost zero at 370 K, a temperature corresponding to the range for the first transition for compounds with 8 to 15 carbon atoms, inclusive. This indicates that the first transition for these short chain compounds is associated, mainly, with alkyl chain melting and reduced crystal system order. However, for long chain adducts, at this temperature, the monoclinic arrangement and crystal system order are almost totally lost due to their greater thermal sensitivity.Figure 4
(a) Typical methyl and methylene stretching region and (b) methylene progression region at different temperatures. (c) Methylene asymmetric : symmetric stretching band intensity ratios versus temperature (equation:y=0.0113x-2.2597, R2=0.9843). (d) von t’ Hoff plot for the effect of temperature on the trans⇄gauche interconversion equilibrium constant K (equation: y=-3727.5x-9.0684, R2=0.9927).
(a)
(b)
(c)
(d)The high frequency bands ascribed to the C-H symmetric and asymmetric stretching vibrations of the CH2 and CH3 groups also show significant temperature sensitivity (Figure 4(a)). For instance, both νsCH3 and νasCH3 bands, atca. 2874 and 2955 cm−1, respectively, decrease simultaneously in intensity with increased temperature, indicating increased rotational freedom of the methyl and methylene groups due to reducevan der Waals interactions as the alkyl chains become increasingly molten. Coalescence of the parallel and perpendicularly polarized methyl νasC-H modes correlate with polarization isotropy and reduced interplanarvan der Waals interactions due to increased CH3 rotational freedom. Similar changes in the CH2 stretching bands with increased temperature provide significant insights into the thermally induced structural and conformational evolution of the methylene group population and hence the alkyl chains. For example, increased temperature results in marked reduction of both νasCH2 and νsCH2 intensities due to reduce conformation order of the alkyl chains. Interestingly, intensity ratios of these peaks, in Raman, associated with the C-H stretching vibrations, are known to be sensitive to the alkyl chain conformational order and environment [40–43]. Hence, a basic quantitative model allowing assessment of the lateral chain packing order(S) of alkyl chain was defined: S=r-0.7/1.5, where r is the intensity ratio of CH2 asymmetric (I−) : symmetric (I+) stretching modes, so that S is unity for crystalline alkyl chains and zero for those in the liquid state [44]. This method has been applied in the structural studies of cholesteric liquid crystals [40] and biomembranes [41, 42]. However, for these compounds, a plot S versus temperature gave a positive slope which would indicate that the alkyl chains become more orderly with increased temperature, an obviously incorrect result. This indicates that the model does not hold true for silver carboxylates. Nonetheless, since the ratio of CH2 (I−/I+) increases with temperature (Figure 4(c)), it is clear that the percentagegauche conformation in the methylene group assembly follows the same trend, as expected, and hence the observed increased asymmetric stretching probability.Based on Figure4(c), the intensities of both bands should be equal atca. 289 K; that is, lateral packing is optimum in this temperature range: the alkyl chains are 100%all-trans. The slope of this plot represents the temperature coefficient of lateral chain packing order: ∂S/∂T=1.13×10-2 K−1 or the thermal sensitivity of chain packing. The magnitude of this parameter describes the strength of the intermolecular forces associated with lattice stability; that is, larger values should result for low melting point alkyl chain assemblies: weak interchainvan der Waals forces; hence, this value should be much smaller for short chain compounds. In addition to reduced intensities, these bands also show changes in their frequencies; that is, with increased temperature both νasCH2 and νsCH2 bands shift to higher frequencies. This is due to increasedgauche conformation population and hence chain kinking. Indeed, thegauche population can be assessed at different temperatures by comparing the stretching frequencies ofall-trans crystallinen-alkanes to these compounds. Therefore, if Trans⇆Gauche isomerization is viewed as a reversible equilibrium, then an estimation of the equilibrium constant (K) at different temperatures based on (1)K=1-n-alkane/νsCH2n-alkane/νsCH2is possible. Therefore, a plot of lnK versus 1/T (K−1) (Figure 4(d)) gives the average isomerization enthalpy and entropy as 30.99 kJ mol−1 and 75.39 J mol−1 K−1, respectively. Surely, these values are not identical over different segments of the melting process as result of heat capacity changes in the methylene group assembly, especially during phase transitions where the density of the lattice changes significantly due to reduce chain packing order. This type of assessment is only valid over small temperature intervals. It is also worthy of note that the magnitude of such energy changes is affected by intermolecular forces of interactions in the lattice. By the fact that these values are large relative to those reported for sodium and potassium carboxylates [14, 22, 24], greatervan der Waals interactions are indicated. However, higher melting temperatures for sodium and potassium carboxylates are due to greater electrostatic forces associated with the metal-carboxyl bonding.Infrared measurements collected on cooling the samples show considerable changes at room temperature. For instance, though the methylene rocking band, centered atca. 720 cm−1, at room temperature, returns to its original intensity, there is a slight shift to lower frequency (~717 cm−1). The C-C stretching and methylene twisting bands also show considerable changes; coalescence and broadening are most obvious, along with reduced intensities. Surely, this confirms that, on heating, even without reaching the melt, the structures of these compounds are permanently changed especially where metal-carboxyl coordination is concerned. For example, both COO modes, on cooling, do not reappear; that is, the changes observed on heating are permanent. Reemergence of the methyl and methylene C-H stretching bands on cooling, though not totally, indicates that despite significant changes in the metal-carboxyl coordination sphere, the alkyl chains remain intact up to 360 K. However, it is imaginable that as temperature tends towards the melt, the aforementioned changes will become more significant as proven by García and coworkers [23], for potassiumn-carboxylates.


## 4. Conclusion

Fourier transform infrared studies on a homologous series of anhydrous solid state silver(I)n-carboxylates show clearly that at room temperature their methylene groups are crystallized in theall-trans conformation; hence, the alkyl chain is fully extended. The monoclinic crystal system is composed of tilted alkyl chains anchored to silver ions via bridging bidentate coordination. All bands associated with the methylene and carboxyl group vibrations show significant sensitivity to temperature, whilst the effects of chain length are mainly observable in the methylene group vibrations. Increased temperature results in reduced lateral chain packing order due to increased concentration of alkyl chaingauche conformers; that is, chain kinking arises and crystal system order diminishes. In addition to these events, there are significant irreversible bonding changes in the metal-carboxyl coordination sphere; that is, rearrangements in the bonding structure and or bonding breaking occur with increased temperature. However, the effects of temperature on lattice packing, crystalline order and metal-carboxyl bonding are somewhat different for the short chain adducts (<12 carbons); that is, as chain length decreases, their thermal stability increases. Based on these results, it is clear that the molecular packing for anhydrous silver(I)n-alkanoates changes with increased chain length; hence, compounds of different chain length are similar but not identical.



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*Source: 3068430-2016-02-29.xml*