Silacyclohexanes, Sila(hetero)cyclohexanes and Related Compounds: Structure and Conformational Analysis.

Conformational analysis of Si-mono- and Si,Si-disubstituted silacyclohexanes as well as their analogues with a heteroatom(s) in the ring is reviewed with the focus on the recent results. Experimental measurements in the gas phase (gas electron diffraction, GED) and low temperature NMR spectroscopy (LT NMR) on 1H, 13C and 29Si nuclei are described along with theoretical calculations at the DFT and MP2 levels of theory. Structural and conformational specific features are shown to be principally different from those of the carbon predecessors - the corresponding cyclohexanes, oxanes, thianes and piperidines. The role of various effects (steric, hyperconjugation, stereoelectronic, electrostatic) is demonstrated.

1. Introduction

Conformational analysis of cyclohexanes is an inalienable part of organic chemistry that is familiar to all organic chemists, even to those whose interests lie outside this specific area. In going from cyclohexanes to their N-, O-, or S-heteroanalogues, no dramatic changes occur in the structure or conformational preferences of the substituents, which may give an illusion that this is true for all other heterocyclohexanes. However, this is not always so, as it became clear in the last 15 years, when a large number of silacyclohexanes with different groups at silicon, as well as having one or more other heteroatoms in the six-membered ring, such as N, O, S, have been synthesized. The only review on the topic was that of 2004 [1] reporting a few compounds known at that time: silacyclohexane, 1,4-disila- and 1,3,5-trisilacylohexanes and their Si-alkyl derivatives. Since then only two reports published by the present author and reviewing specific questions appeared [2,3]. The nowadays state of the problem is unique in that, on the one hand, it still allows discussing all main findings in the field in one review, and, on the other hand, making solid conclusions based on ample experimental evidences. The studies using various experimental techniques, such as GED, LT NMR, Raman and IR spectroscopy and quantum chemical calculations showed a remarkable difference in the structure and conformational behavior between sila(hetero)cyclohexanes and cyclohexanes, piperidines, oxanes, or thianes. The present review summarizes the results of experimental and theoretical conformational studies on the title compounds in different aggregate states, and is focused on recent works in this field. All these issues will be addressed in the proposed review providing the reader with the answers to the raised questions. The list of references contains 93 items including those of 2019 year, most of them referring to the last decade.

2. General Features of Sila(hetero)cyclohexanes

The three main issues in conformational analysis of cyclohexanes and all their derivatives are the ring conformation, the ratio of the conformers, and the barrier to their interconversion. As will be shown below, these three characteristics of sila(hetero)cyclohexanes drastically differ from those of cyclohexanes, piperidines, oxanes, or thianes.

As to the ring conformation, an important difference is a smaller angle of folding between the C2C3C5C6 plane of the ring and the C2SiC6 plane with respect to the C3C4C5 plane as depicted in Figure 1. The same is true for the nitrogen, oxygen or sulfur-containing heterocycles, in which atom C4 is replaced by the corresponding heteroatom [4].

Figure 1

Lower degree of folding at silicon in the six-membered ring.

The ratio of the conformers is also dramatically different. It is determined by the relative conformational energies, , defined for the ax ⇆ eq equilibrium as = −ΔG° = Gax − Geq. For cyclohexanes, piperidines, oxanes, or thianes the values are always positive. For substituents at silicon they are much smaller and even may become negative. Most striking examples are practically equal values for Me and Ph groups at silicon (0.23 [5] and 0.25 kcal/mol [6]), whereas in the cyclohexane series they are strongly different (1.76 and 2.87 kcal/mol [7]), and the value of for very bulky but, at the same time, highly electronegative substituent CF3, which is positive and very large when it is attached to carbon (2.50 kcal/mol [8]) but becomes negative for CF3 at silicon falling in the range from −0.2 to +0.5 kcal/mol [9]. The ring inversion barriers in silacyclohexanes and their analogues are much lower than those in the carbon predecessors. Normally, they are as low as 4.5–5.5 kcal/mol, in comparison to 10–14 kcal/mol in cyclohexanes, piperidines, oxanes, or thianes. Such small barriers can be measured by NMR only by using special NMR probes working at very low temperatures, down to the interval from −180 to −190 °C, and solvents, which are not frozen at these temperatures (mixtures of freons). Such low barriers are due to the flattened structure of sila(hetero)cyclohexanes (Figure 1), which is closer to the transition state structurally and, according to the Hammond postulate, energetically, and, hence, needs less energy to reach it.

Other differences of sila(hetero)cyclohexanes, like additivity of conformational effects versus nonadditivity in cyclohexanes, or opposite conformational preferences in gas and solution, having no precedents in classical conformational analysis, will be discussed below.

3. Silacyclohexanes

The conformational equilibrium of monosubstituted 1-X-silacyclohexanes 1 in Figure 2 can be shifted either to the axial or to the equatorial conformer, depending on the nature of substituent X. Therefore, the conformational energy of X, (X)Si = −ΔG = −(Geq − Gax) = RT log([eq]/[ax]), can be either positive or negative, in contrast to the corresponding cyclohexanes, in which (X)C is always positive, that is, the substituent always prefers the equatorial position. The available values for both series are summarized in Table 1.

Figure 2

Conformational equilibrium of monosubstituted silacyclohexanes.

Table 1

Conformational energies (kcal/mol) for different substituents at C and Si atoms.

X	A(X)C	A(X)Si
F	0.36	−0.28 [10]
Cl	0.53	−0.43 [11]
Br	0.48	−0.82 [12]
I	0.49	−0.59 [13]
OH	0.6–1.0	0.03 [14]
SiH3	0.33 a	0.05 [15]
Me	1.76	0.23 [5]
CF3	2.50	0.40 [9]
Ph	2.87	0.25 [6]
t-Bu	4.7	1.30 [16]

a Calculated from eq:ax = 90:10 at 75 C [17].

The following conclusions can be made from analysis of the data in Table 1. First, a drastic decrease of all values in going from cyclohexanes to silacyclohexanes implies a minor, subordinate role of steric effects in silacyclohexanes. Second, inversion of the sign (X = halogen) or sharp decrease (X = CF3) of the values of these electronegative groups is indicative of the determining role of electrostatic effects in the latter series. This is owing to the presence of strongly electropositive silicon atom in the molecule and is clearly manifested not only in the position of the equilibrium between the conformers but also in the lengths of the Si-C bonds. Thus, the Si-CF3 bond in trifluoromethylsilacyclohexane is elongated by ~0.08 Å relative to the Si-CH2 because of repulsion of the positively charged Si and CF3 carbon atoms.

The same is true for the Si-CF3 (1.934 Å) and Si–Me bond in 1-methyl-1-silacyclohexane (1.862 Å). The relative importance of steric, hyperconjugation and electrostatic effects was evaluated and discussed in detail in the author’s review [3]. A minor role of steric effects not veiled by the effect of strongly electronegative groups (halogen, CF3) can be followed on the example of X = SiH3. Low in silylcyclohexane (0.33) is, evidently, due to the long C–Si bond (~1.85 Å). Further lengthening in 1-silylsilacyclohexane [e.g., in (t-BuSi)2 the length of the Si–Si bond is 2.69 Å) makes the steric effect negligible ( = 0.05 kcal/mol). The only substituent, for which steric effect could be significant in silacyclohexanes is t-butyl group, but until recently the only available compound of this type was the simplest representative, 1-t-butylsilacyclohexane. Very recently we have synthesized 1-t-butyl-1-phenylsilacyclohexane and investigated its conformational equilibrium (vide infra).

Introduction of a second substituent to silicon rises two interrelated questions in conformational analysis of geminally 1,1-disubstituted silacyclohexanes 2: (i) qualitative applicability of individual values of substituents X and Y for prediction of the position of conformational equilibrium in Figure 3, and (ii) quantitative prediction of the conformer ratio on the basis of monosubstituted compounds (additivity or nonadditivity of conformational energies).

Figure 3

Conformational equilibrium of geminally 1,1-disubstituted silacyclohexanes.

It makes sense to compare the conformational behavior of geminally substituted cyclohexanes and silacyclohexanes. As is clearly seen from Table 2, there is neither quantitative nor even qualitative agreement between the conformational preferences in the mono and disubstituted cyclohexanes. The mean deviation ΔΔG° of the experimental free energy difference ΔG°ax–eq from that calculated by the additive scheme ΔG°add for the presented selection of cyclohexanes is >1 kcal/mol, which is very large for conformational equilibria. The pairs of substituents for which the experimental and calculated values of ΔG° have different sign, that is, the observed conformational preferences are opposite to those predicted from values for monosubstituted compounds, deserve special mention. The most striking example is 1-methyl-1-phenylcyclohexane, which, in view of the much larger conformational energy of the Ph as compared to Me group must exist exclusively as a MeaxPheq conformer.

Table 2

Nonadditivity of conformational effects in cyclohexanes.

X	Y	ΔG°ax–eq	ΔG°add	ΔΔG°	Ref.
Me	F	0.86	1.60	−0.74	[18]
Me	CF3	0.53	1.31	−0.78	[18]
Me	Ph	0.32	−1.11	1.43	[19,20]
Me	NMe2	−0.4	0.21	−0.61	[21]
Ph	NMe2	−0.5	1.34	−1.84	[22]
Me	OH	0.31	0.73	−0.42	[23,24]
Ph	OH	0.5	1.86	−1.36	[25]

However, as was found experimentally, the equilibrium of 1-methyl-1-phenylcyclohexane is substantially shifted to the MeeqPhax conformer (72:28, ΔG°ax–eq = 0.32, Table 2) [26]. The reasons of such behavior have been clarified using high level quantum chemical calculations [20]. In the MeaxPheq conformer, both Ph-‘orthogonal’ and Ph-‘horizontal’ rotamers are destabilized by repulsive interactions of ortho-protons with either the Me group or α-CHeq protons, while in the Ph-‘horizontal’ rotamer of the MeeqPhax conformer the latter destabilization is avoided. For the sake of fairness, it should be noted that there are examples of additivity of conformational effects in cyclohexanes [27,28], but in general, the conclusion about the absence of additivity of the values in geminally disubstituted cyclohexanes made ten years ago [18] is undoubtedly true.

At that time it was too bold to say anything about additivity or nonadditivity in silacyclohexane series because there only available examples were Si(Me,F)- and Si(Me,CF3)-silacyclohexanes. Nevertheless, in the same work, Arnason et al. stated that for silacyclohexanes the model works remarkably well for this limited selection of substituents [18]. Since then, a good deal of studies devoted to conformational preferences in sila(hetero)cyclohexanes have seen the light, as summarized in Table 3. The analysis of Table 3 clearly shows that, if to exclude some specific cases with endocyclic N and O atoms in the ring (No. 10, 12 13, given in bold, which will be discussed below), averaging of other ΔΔG° values results in the mean value of 0.1 kcal/mol for other 12 pairs of conformers, or more than one order of magnitude less than in Table 2 for cyclohexanes.

Table 3

Additivity of conformational effects in silacyclohexanes and sila(hetero)cyclohexanes.

No.	X	Y	Z	ΔG°ax–eq	ΔG°add	ΔΔG°	Ref.
1	CH2	Me	F	0.32	0.51	−0.19	[18]
2	CH2	Me	CF3	0.61	0.49	0.12	[18]
3	CH2	Me	Cl	0.36	0.36	0.00	[29]
4	CH2	Me	Ph	0.11	0.02	0.09	[6]
5	CH2	Ph	F	0.46	0.53	−0.07	[8]
6	CH2	Ph	Cl	0.53	0.68	−0.15	[8]
7	CH2	Ph	OR	0.20	(0.20)	0.00	[9]
8	CH2	Ph	t-Bu	1.1 a	1.05	0.05	a
9	NR	Me	Ph	0.10–0.24	(0.02)	(−0.08–(−0.22))	[30]
10	NR	Me	OR	−0.21	(0.20)	(−0.41)	[31]
11	O	Me	Ph	0.16	(0.02)	(0.14)	[32]
12	O	Me	OR	0.02	(0.20)	(−0.18)	[33]
13	O	Me	F	0.37(gas)>1.4(solution)	0.510.51	0.14>0.9	[34][34]
14	S	Me	Ph	0.15	0.25	−0.10	[6]
15	S	Me	F	−0.78	−0.79	0.01	[35]

a Lower limit of Phaxt-Bueq:Pheqt-Buax = 92(7):8(7) (GED, 337 K; our unpublished results).

Therefore, the additivity model does work for silacyclohexanes without exceptions, and also for sila(hetero)cyclohexanes, unless the latter contain strongly electronegative atom or group in the ring. The exceptions deserve separate consideration, which allowed to reveal the influence of stereoelectronic and electrostatic effects in these specific cases.

Large deviations from additivity in 1,3-dimethyl-3-isopropoxy-3-silapiperidine (No. 10, Table 3) were assigned to the repulsion of the two unidirectional axially oriented dipoles of the nitrogen lone pair and the highly polar Si-O bond (Figure 4, left), destabilizing the MeeqORax conformer and making the MeaxOReq conformer predominant (the ratio was measured as 2:1) [31]. This effect is especially important in Si-alkoxy or Si-hydroxy-3-silapiperidines because of a large dipole moment of the Si-O bond and the higher basicity of nitrogen in α-silylamines relative to organic amines [36,37,38].

Figure 4

Orientation of the N and O lone pairs with respect to the O–Si dipole in 1,3-dimethyl-3-isopropoxy-1,3-azasilinane (left) and 3-isopropoxy-3-methyl-1,3-oxasilinane (right).

In 3-isopropoxy-3-methyl-1,3-oxasilinane (No. 12, Table 3), the MeeqORax:MeaxOReq ratio is 1:1, so, the deviation from additivity is smaller. The observed shift of the conformational equilibrium toward the MeeqORax conformer is explained by orientation of the oxygen atom lone pair in the C-O-C plane [39], as shown in Figure 4, which reduces the repulsion between the two dipoles, as compared to that in the molecule of 1,3-dimethyl-3-isopropoxy-1,3-azasilinane.

Very recently, we have synthesized 1-methylthio-1-phenyl-1-silacyclohexane and performed its conformational analysis using GED, LT NMR, and quantum chemical calculations [40]. It should be said that this was the first compound of this family that contained the exocyclic sulfur-containing group at silicon. It was prepared in 55% yield by the replacement of chlorine in 1-chloro-1-phenyl-1-silacyclohexane with MeSNa. The results are summarized in Figure 5.

Figure 5

Ratio of 1-methylthio-1-phenyl-1-silacyclohexane conformers by different methods.

As follows from Figure 5, all methods clearly show the predominance of Pheq conformer, slightly larger in solution than in gas phase and in nice agreement with theoretical calculations. It must be said that LT NMR spectra were taken not only for 1H and 13C but also for 29Si (Figure 6) [40]. Until 2019, 29Si NMR was not used for conformational analysis of silacyclohexane or any other compounds. The first example was reported in our recent work at the same time (vide infra).

Figure 6

29Si-NMR spectrum of 1-methylthio-1-phenyl-1-silacyclohexane 1 at 98 K.

4. Thiasilacyclohexanes

The largest family of silaheterocyclohexanes is 3- and 4-silathianes including their S-functional derivatives (Figure 7).

Figure 7

1,3- and 1,4-thiasilacyclohexanes and their S-functional derivatives.

Smaller conformational energies are inherent not only to substituents at silicon, but, because of longer C−Si and C−S bonds, also to the groups attached to the endocyclic carbon atoms. For example, while the value of Me is 1.76 kcal/mol (Table 1), the measured ratio of 2-Meeq:2-Meax conformers in the molecule of 2,3,3-trimethyl-3-silathiane is 60:40, that corresponds to ΔGo = 0.35 kcal/mol, coinciding with the calculated value of 0.36 kcal/mol [41]. The analogues of the latter compound with 2-Me3Si [41] and 2-Ph substituents [42] exist as single 2-eq conformers due to the large conformational energy of the Ph (2.87 kcal/mol, Table 1) and SiMe3 group (experimental 2.5 kcal/mol, [43], theoretical 2.05 kcal/mol [44].

An interesting effect of the ring silicon atom was found when analyzing 3-silathiane S-oxides. The predominant existence of cyclic sulfoxides in the SOax conformation is well known [45]. Introduction of substituents at the 3-position to sulfur either in thiane or 3-silathiane destabilizes the SOax form, and both 3,3-dimethylthiane 1-oxide [46,47] and 3,3-dimethyl-3-silathiane S-oxide [46] exist in solution completely in the SOeq form.

The situation becomes more complicated when another substituent is introduced into the ring. Thus, the molecule of 2,3,3-trimethyl-3-silathiane S-oxide having two chiral centers (atoms C-2 and S), can exist as two diastereomers. Indeed, oxidation of 2,3,3-trimethyl-3-silathiane gives rise to the cis/trans diastereomeric mixture of the corresponding S-oxides in 1:2 ratio. The trans-isomer can adopt only the eq-eq form, but for the cis-isomer the MeeqSOax and MeaxSOeq are in equilibrium (Figure 8) with the ratio MeeqSOax:MeaxSOeq equal to 1:1 at room temperature or 5:1 at −120 °C. This is consistent with the large Me value (1.76 kcal/mol) and a small negative value of SO (−0.18 kcal/mol). Although the presence of silicon in the ring lowers the Me value and makes the SO value positive, the MeeqSOax conformer is still preferable at low temperatures [48].

Figure 8

Conformational equilibria in the trans and cis isomers of 3-silathiane S-oxides.

In 4-silathiane S-oxides, the situation is different (Figure 9). The conformational equilibrium in solution is shifted to the equatorial conformer, the SOeq:SOax being 63:37, which is comparable with the 55:45 ratio found for thiane S-oxide [47].

Figure 9

Predominance of the SOeq conformer for 4-silathiane S-oxide.

Interestingly, theoretical DFT calculations showed the SOax conformer to be more stable by 0.93 kcal/mol [49], which seems to contradict the experiment. However, due to a larger dipole moment of SOeq (5.41 vs. 4.21 D in SOax) the use of the PCM in CHCl3 as the solvent led to the inversion of the relative stability and the SOeq conformer was found to be 0.19 kcal/mol more stable [49]. This gives the ratio SOeq:SOax of 70:30 in excellent agreement with the experiment.

Theoretical studies of 4-silathiane S-oxides posed an interesting question about their molecular structure. Usually, sila(hetero)cyclohexanes adopt chair conformation. However, in the presence of one or two halogen atoms at silicon, the boat conformer may become a local minimum on the potential energy surface due to intramolecular S=O∙∙∙Si coordination, as shown in Figure 10.

Figure 10

‘Scorpionoid’ boat structure of axial 4-silathiane S-oxides bearing halogens at silicon.

For these structures, we coined the term ‘scorpionoids’, in which the silicon atom resembles the head and the sulfoxide oxygen atom the stinging tail. The relative stability of the chair and boat forms of 4-silathiane S-oxides with one or two halogens at silicon was analyzed in [50] (see also references cited therein). In the pentacoordinate motif around the silicon atom, the O···Si distance for various pairs of halogens (X, Y = H, F, Cl, Br) fall in the range of 2.05–2.15 Å, and is much less than the sum of the vdW radii of the two atoms (3.62 Å). Penta-coordination is also confirmed by the close to planar CCX equatorial arrangement around silicon, and by longer axial bond Si-Y than the equatorial bond Si-X in the bipyramidal silicon coordination knot [50]. We know only one example of the S=O···Si coordination in which the trigonal bipyramidal structure was proved experimentally [51].

4-Silathiane S-sulfimides, which are isoelectronic analogues of 4-silathiane S-oxides (Figure 7), also have very low activation barriers from 4.4 to 4.7 kcal/mol [52]. For N-phenylsulfonyl-4-silathiane S-sulfimide (Figure 7) the conformational equilibrium is almost degenerate (1:1), whereas in N-triflyl-4-silathiane S-sulfimide the equilibrium is shifted to the axial conformer (~55:45) due to electronegative CF3 group [52]. It should be mentioned, that in addition to the ax and eq conformers of the sulfimide motif, two rotamers, namely, with the “inward” or “outward” CF3 group may exist [53].

It also deserves mentioning that the value of Me in 3-methyl-3-silathiane is 0.35 kcal/mol [35], that is, larger than in the absence of sulfur atom in the ring (0.23 kcal/mol, Table 1). A detailed analysis allowed us to conclude that the conformational preferences are governed not only by the values of the substituents at the silicon atom, but the donor-acceptor interactions between the orbitals of the vicinal bonds play the decisive role; the degree of these interactions was evaluated by the use of the NBO analysis [35].

5. Azasilacyclohexanes (azasilinanes) and Related Compounds

The structures, for which the conformational analysis was done, are given in Figure 11. The results of this analysis should be compared to those for the structures in Figure 7, to determine the effect of the nature of the heteroatom in the ring, and to the silicon-free analogues, like morpholines and piperidines.

Figure 11

Structurally and conformationally studied azasilacyclohexanes (azasilinanes).

The barriers to ring inversion in 4-alkyl-2,2,6,6-tetramethyl-1,4,2,6-oxaazadisilinanes amount to 8.1 ± 0.4 kcal/mol [54], which is less than 11.1 kcal/mol in N-methylmorpholine without α-methyl groups to oxygen [55,56]. Again, this is due to the longer Si–C than C–C bonds and less folded SiOSi part of the molecule.

The strongly electron acceptor triflyl group at the nitrogen atom makes it planar, but still two rotamers with the ‘inward’ or ‘outward’ CF3 group differing in energy by 1.1 kcal/mol in favor of the latter may exist. According to the X-ray analysis, in the crystal the compound exists as the single ‘outward’ rotamer [57] (Figure 12).

Figure 12

‘Inward’ rotamer of 2,2,6,6-tetramethyl-4-triflyl-1,4,2,6-oxazadisilinane.

For N-triflyl-4-silapiperidine, the MP2 calculated ΔE is 0.6 kcal/mol in favor of the ‘outward’ rotamer, corresponding to the ratio of 95:5. The LT 13C-NMR spectroscopy showed the presence of two conformers in the ratio 98:2, which excellently coincides with calculations [57].

The experimental barriers to ring inversion in the N-triflyl compounds in Figure 11 are 12.9 ± 0.2 kcal/mol. An intriguing question is why the barriers in the molecules with almost planar nitrogen are higher than in non-planar N-alkyl derivatives? The answer is that these barriers refer to the interconversion between the outward and inward rotamers, rather than to the ring inversion. Since the total reaction rate cannot be larger than the rate of its limiting step, the overall barrier must be equal to that for the slowest step of the process. The conversion of rotamers of N-triflyl heterocycles is characterized by the barriers of 12–14 kcal/mol [58,59,60].

The crystal structure of a series of N-arylated N-hydroxy-1,3-azasilinanes (4-aryl-4-hydroxy-4-silapiperidines) was determined by Tacke et al. who reached the conclusion that the energy difference between the isomers of silapiperidines is notably smaller than in the corresponding piperidines [61,62,63,64,65]. In 1,4,2-oxaazasilinanes with different substituents at nitrogen in Figure 11, the ring inversion barriers decrease in the order 8.85 (R = Me) > 7.7 (R = Bn) > 4.8 (R = Ph) kcal/mol [66], that means, with increased conjugation of NLP with R. Their quaternization by MeI allowed to prepare the corresponding salts and to investigate them by LT NMR; for the N,N-dimethyl salt, the degenerate conformational equilibrium is too fast even at 103 K, but for the Me,Bn-salt it was frozen and the barrier of interconversion of the conformers equal to 6.1 kcal/mol and the conformational ratio MeaxBneq:MeeqBnax = 60:40 were found [66].

In solution, the simplest representative of 1,3-dimethyl-1,3-azasilinanes (X = H, Y = R = Me) gives an equilibrium mixture SiMeax:SiMeeq = 1:2 (33:67 or 30:70 from 1H- or 13C- LT NMR) [65]. However, in gas phase the axial conformer predominates and the ratio inverts to 2:1 [66]. This corresponds to the Gibbs free energy difference of –0.21 kcal/mol, which is lower than in 1,3-dimethylpiperidine (−1.6 kcal/mol [67]) but almost equal to that in 1-methyl-1-silacyclohexane (−0.23 kcal/mol [5]). Thus, the influence of the nitrogen atom on the barrier to ring inversion in 1,3-dimethylpiperidine (1.60 versus 1.76 kcal/mol in methylcyclohexane) is low (~10%) but measurable, while in silaheterocyclohexanes it is practically zero (0.02 kcal/mol).

1,3,3-Trimethyl-1,3-azasilinane was the first Si,N-heterocycle for which the gas phase structure was obtained [68]. The angle of folding between the C2Si3C4 plane and the N1C2C4C5 plane was found to be ~40° and the angle between the C6N1C2 and C2Si3C5C6 planes − ~60°.

For the Si-chiral 1,3-azasilinanes in Figure 11 (X = Me, Y = Ph, R = Me or i-Pr), the equilibrium is not degenerate, and the conformer ratio was measured as 67:33 (R = Me) [30] or 58.5:41.5 (R = i-Pr) [69], in both cases in favor of the Pheq,Meax conformers. The ring inversion barriers were determined to be equal to 9.0 kcal/mol for R = Me [30] or 8.25 kcal/mol for R = i-Pr [69].

Among the investigated Si,N,O-heterocycles, an interesting object was the silicon analogue of quinolizidine, (3,3,7,7-tetramethylhexahydro-1H-[1.4.2]oxazasilino[4,5-d][1.4.2]oxaazasilin-9a-yl)-methanol, which was prepared by the reaction of aminoalcohol H2NC(CH2OH)3 with (chloromethyl)(methoxy)dimethylsilane [70] (Figure 13).

Figure 13

Synthesis of (3,3,7,7-tetramethylhexahydro-1H-[1.4.2]oxazasilino[4,5-d][1.4.2]oxaazasilin-9a-yl)-methanol by condensation/cyclization of 2-amino-2-(hydroxymethyl)propane-1,3-diol with ClCH2SiMe2OMe.

X-Ray analysis proved the trans,trans-fused structure in the crystal (Figure 14), but the molecule was conformationally flexible and the barrier for interconversion of the conformers was only 5.8 kcal/mol [70].

Figure 14

X-ray structure of 3,3,7,7-tetramethylhexahydro-1H-[1.4.2]oxazasilino[4,5-d][1.4.2]oxaaza-silin-9a-yl)methanol.

Such a flexibility might be suggestive of the cis-fused structure of the two rings in solution, because in decalin the ring inversion is possible only in the cis-isomer, whereas the structure of the trans isomer is rigid. This seeming discrepancy can be rationalized by the fact that in N-fused compounds, such as quinolizidine, inversion at nitrogen atom is possible, as shown in Figure 15.

Figure 15

Conformational flexibility of 3,3,7,7-tetramethylhexahydro-1H-[1.4.2]oxazasilino[4,5-d][1.4.2]oxaazasilin-9a-yl)methanol due to nitrogen pyramid inversion.

Quaternization of the nitrogen atom prevents N-inversion and the isomeric ammonium salts do not suffer interconversion. When treated with methyl iodide, 9a-R-substituted quinolizidines almpost quantitatively give the corresponding salts (Figure 16) existing as the cis/trans isomeric mixtures, in which the molar fraction of the trans isomer decreases in the following order: H > CN > CH3 > CH2OH > CH2NO2 [70].

Figure 16

Isomeric salts formed upon quaternization of 3,3,7,7-tetramethylhexahydro-1H-[1.4.2]oxazasilino[4,5-d][1.4.2]oxaazasilin-9a-yl)methanol.

6. Oxasilacyclohexanes (Silatetrahydropyrans)

Some oxygen-containing silacyclohexanes with the endocyclic oxygen as the second heteroatom in the ring (3-silatetrahydropyrans) have been considered above (see Figure 4 and [32,33,34]. They include disubstituted at silicon compounds with (Me, F), (Me, OPr-i) and (Me, Ph) pairs of substituents. The simplest Si-chiral compound of this series, 3-methyl-3-silatetrahydropyran, was synthesized by the base-catalyzed cyclization followed by dephenylation and reduction [71] as shown in Figure 17. The problem was that it is the most volatile compound as compared to other analogues having boiling point of 62 °C at 104 mm Hg and is easily lost with the solvent during isolation.

Figure 17

Synthesis of 3-methyl-3-silatetrahydropyran.

In freons mixture solution at 103 K, 13C-NMR showed decoalescence of the SiMe, C4 and C5 signals and allowed to measure the conformational ratio and the ring interconversion barrier. As expected, due to small conformational energy Si(Me) of 0.23 kcal/mol the Meax:Meeq ratio was 35:65. The activation barrier was very small, 4.6 kcal/mol [71]. In gas phase the Meax conformer slightly predominates (54:46). The low energy difference between the conformers was in agreement with the theoretically calculated by most of the used DFT and MP2 methods [71].

The Si-phenyl analogue of the above compound, 3-phenyl-3-silatetrahydropyran, and the corresponding silanol, 3-hydroxy-3-phenyl-3-silatetrahydropyran, have been studied by 13C LT NMR and theoretical calculations. Both compounds were synthesized by partial dephenylation from 3,3-diphenyl-3-silatetrahydropyran, as shown in Scheme 1 [72].

Scheme 1

Synthesis of 3-phenyl-3-silatetrahydropyran and 3-hydroxy-3-phenyl-3-sila-tetrahydropyran.

Unfortunately, no decoalescence of the 13C signals was reached for 3-hydroxy-3-phenyl-3-silatetrahydropyran at the lowest temperature, so, the conformational equilibrium could not be measured experimentally. There could be because of too low coalescence temperature (<100 K) or completely one-sided conformational equilibrium. From our experience, both reasons are hardly probable, so the only feasible reason seems to be a small Δδ(13C) between the conformers. For 3-phenyl-3-silatetrahydropyran, however, the equilibrium was frozen and the ratio Phax:Pheq was measured as 17.1:82.9, corresponding to K = 4.59 and ΔG° = −0.31 kcal/mol [72].

7. Si-X-silacyclohexanes (X = Hlg, CN, OMe)

Si-Halogenated silacyclohexanes were conformationally studied by I. Arnason et al. (Hlg = F [10], Cl, Br, I [73]). The results are compiled in Table 4. For comparison, the recently published data for 1-cyano- [74] and 1-methoxy-1-silacyclohexane [75] as well as disubstituted silacyclohexanes with the phenyl group and Hlg = F, Cl [76] or other electronegative groups at silicon are included. Note, that 1-bromo-1-phenylsilacyclohexane has also been synthesized [77] but, because of low stability, its conformational analysis could not be performed.

Table 4

Conformational preferences of Si-halogenated silacyclohexanes (CH2)5Si(R,Hlg).

R	X	Xax Conformer
		Gas	Solution	Ref.
H	F	63.0	64.2	[10]
	Cl	62.5	83.0	[73]
	Br	70.5	85.7	[73]
	I	54.0	85.7	[73]
	CN	84	35	[74]
	OMe	59	− *	[75]
Ph	F	40	76	[76]
	Cl	79	82	[76]

* No decoalescence in NMR. Slight predominance of the ax conformer according to Raman spectroscopy.

As follows from Table 4, for R = H, all electronegative substituents prefer axial locations in the gas phase, the prevalence of the ax conformer varying from 54 to 84%. For X = Hlg, the same is true in solution; for X = OMe, no decoalescence was observed in the NMR spectra, but low-temperature Raman spectroscopy also suggested slight predominance of the ax conformer. An interesting exception is strong predominance of CNeq in solution, that is, practically the same as in its carbon predecessor, cyanocyclohexane C5H11CN, exists predominantly (37:63%) as proved by GED in gas and by dynamic NMR in solution [78]. The dramatically different conformational behavior of 1-cyano-1-silacyclohexane in solution was assigned by the authors to a strong solvation effect. The conclusion was made based on the NBO analysis that the equatorial conformer is favored by the conjugation and steric effects rather than electrostatic effect. However, steric effect of the cyano group is negligible, so it was reasonably concluded that studying of Si-CN containing compounds “remains a challenging mystery” and deserve further investigation.

For R = Ph, predominance of conformer PheqClax in all phases and of PheqFax in solution is in agreement with equatorial preference of the more bulky phenyl group and axial preference of more electronegative halogen atom. In light of this, the predominance of PhaxFax, though small, is puzzling. To rationalize the observed conformational ratios, the energy partitioning analysis was employed [76].

8. Solution vs. Gas Conformational Preferences in Miscellaneous Silacyclohexanes

As stated above, silacyclohexanes may show inversion of conformational preferences in going from gas to solution, which is not observed for their carbon predecessors. One of the first examples was 1,3-dimethyl-1,3-azasilinane existing predominantly as SiMeeq conformer (2:1) in solution but as SiMeax (with the same predominance) in gas phase [66]. Replacement of nitrogen atom in the ring by oxygen (in 3-methyl-3-silatetrahydropyran [71]) or by sulfur (in 3-methyl-3-silathiane [35,79]) does change this trend – in all these heterocyclohexanes the conformational preference is inverted in going from gas to solution. Note, that in the absence of heteroatom, the Meeq conformer predominates in both aggregate states [5]. Similar conformational behavior was found for 1-phenylsilacyclohexane, for which strong preference of Pheq conformer was found in solution (78%) [6] and somewhat less predominance was measured in gas phase (62 ± 10%) [80].

1-Methyl-1-phenyl-1-silacyclohexane containing both methyl and phenyl substituents at silicon was studied first by low-temperature NMR in solution and showed the PheqMeax:PhaxMeeq ratio of 63:37% at 103 K [6]. In gas phase, the ratio inverted being (42 ± 15):(58 ± 15)%. Therefore, the analysis of conformational preferences in this and related compounds allows to conclude that in gas phase at room temperature, the methyl group in the Me/Ph geminally substituted compounds shifts the conformational equilibrium towards the Phax conformers, from Pheq:Phax = 100:0 in phenylcyclohexane [7] to 28:72 in 1-methyl-1-phenylcyclohexane [19] and from 62:38 in 1-phenylsilacyclohexane [80] to 42:58 in 1-methyl-1-phenyl-1-silacyclohexane [81]. Introduction of oxygen atom into the latter molecule gives 3-methyl-3-phenyl-3-silatetrahydropyran and increases the Phax/Pheq ratio in the gas phase from 1.38 to 1.63, which was assigned to H···O interaction in the Phax conformer, similar to that in 3-phenyltetrahydropyran [82] (Figure 18).

Figure 18

Structure of 3-methyl-3-phenyl-3-silatetrahydropyran [32] (left) and 3-phenyltetrahydropyran [82] (right).

This assumption is in agreement with the change of the conformer ratio of 1-methyl-1-phenyl-1-silacyclohexane in solution in favor of the Pheq conformer because the oxygen lone electron pair in solution is involved in H-bonding with more acidic protons of the solvent (CHCl3, CH2Cl2, freons); weak specific interaction H···O does not play any role and the prevalence of the Pheq conformer is determined by somewhat larger conformational energy of Ph relative to Me.

Our recent studies [72], [83] on 1-hydroxy-1-phenyl- and 1-methoxy-1-phenylsilacyclohexane, synthesized as described in [84], allow one to compare the gas vs. solution conformational preference of these compounds. Unfortunately, no decoalescence of the 13C signals could be reached for 1-hydroxy-1-phenylsilacyclohexane in solution, but for 1-methoxy-1-phenylsilacyclohexane a significant predominance of the Pheq conformer (Phax:Pheq = 31.2:68.8) was measured at 103 K [72]. In gas phase, close to equimolar ratio (~50:50) of the two conformers for 1-hydroxy-1-phenylsilacyclohexane and a strong predominance of the Phax conformer for 1-methoxy-1-phenylsilacyclohexane (Phax:Phax = 70:30) were measured by GED [83]. While the predominance of Pheq in solution is anticipated being in compliance with all rules governing the conformational preferences, the gas phase measurements are unexpected and extremely surprising. Both axial preference of more electronegative OH or OMe group and steric effects are in favor of the Pheq conformer in both compounds. However, if to consider the relative polarities of the C-Ph and C-O bonds by comparing charge differences Δq = qSi − qCipso, it turns out that ΔΔq = Δq(Phax) − Δq(Pheq) only slightly (<0.01 e) varies in all used methods [83]. In contrast, the polarity of the Si–O bonds calculated as Δq = qSi − qO is more sensitive to the location of the OH or OMe group, and the value of ΔΔq reaches >0.07 e. A general trend is that in both compounds the Si-O bond is more polarized in the Pheq than in the Phax conformer. Also, in 1-methoxy-1-phenylsilacyclohexane, the Si-O bond is more polarized than in the corresponding conformers of 1-hydroxy-1-phenylsilacyclohexane. To resolve the contradiction stemming from the axial preference for more electronegative OH or OMe group, we assumed that steric factors outweigh small difference in the electronic effects in the molecules under investigation [83]. Sterically, the OMe group creates more hindrances than OH group, as is proved by the larger barriers to rotation in 1-methoxy-1-phenylsilacyclohexane (2.3 and 1.6 kcal/mol) than in 1-hydroxy-1-phenylsilacyclohexane (1.5 and 0.3kcal/mol). This may explain the observed Phax predominance in the former (70:30) over that in the latter case (1:1).

9. Miscellaneous Silacyclohexanes and Related Compounds

An interesting type of molecular motion was found in 1-dimethylamino-1-phenyl-silacyclohexane possessing two bulky groups, Ph and Me2N, at silicon. The compound was synthesized in 56% yield as shown in Scheme 2. The compound is rather unstable and is gradually hydrolyzed with time to siloxane with the rupture of the Si-N bond [84].

Scheme 2

Synthesis of 1-dimethylamino-1-phenylsilacyclohexane.

The conformational equilibrium of 1-(Me2N)-1-Ph-1-silacyclohexane was studied by GED, 13C LT NMR and theoretical calculations [85]. The prevalence of Phax conformer in gas phase (Pheq:Phax = 20:80%) is close to that estimated theoretically. In contrast, in solution low temperature 13C-NMR spectroscopy showed the predominance of the Pheq conformer, Pheq:Phax = 77:23. However, the validity of this conclusion depends on whether the assignment of the signal is correct or not. It should be said, that the predominance of Phax conformer in the gas phase is in agreement with MP2 but not with DFT calculations. In solution, the assignment of signals in the 13C-LT NMR spectra is not unequivocal, either. By comparing with the spectra of 1-Ph and 1-Ph,1-X-silacyclohexanes (X = Me, OMe, F, Cl) after decoalescence [6,72,76], all experimental and theoretically calculated chemical shifts, except those for C-1,5 signal, argue for 1-Ph.

The potential energy surface profile for the Ph and NMe2 group rotation about the Si-CPh and Si-N bonds showed the presence of several conformers. In all of them, because of steric repulsion between the the ortho-protons and methyl hydrogen atoms, the NMe2 group rotation induces rotation of the Ph group, and vice versa. In Figure 19, the corresponding correlation plots are shown for the Phax and Pheq conformers. As is clearly seen, rotation of the two groups is strongly correlated, which is typical for gear motion in molecular motors. ‘Vertical’ lines in the left picture appear because for two scanned angles of the NMe2 group differing by 5° the geometry optimization of the axial Ph group leads the system to two different local minima, causing a ‘jump’ of energy [85].

Figure 19

Correlation between dihedral angles C1-Si-Cipso-Cortho and C4-Si-N-Me in the Phax (left) and Pheq conformers (right) of 1-(dimethylamino)-1-phenylsilacyclohexane.

Due to the aforementioned subordinate role of steric effects in silacyclohexanes, Pheq conformers predominate in nearly all studied 1-phenylsila(hetero)cyclohexanes [6,71]. The only exception was our recent study revealing the predominance of Phax in 1-hydroxy-1-phenylsilacyclohexane [72]. Despite a progress in the conformational analysis of the sila(hetero)cyclohexanes having the Ph group at silicon, the question of the possibility of their existence as Phax conformers has remained open. To fill this gap, we investigated (1,1′-phenyl-1,1′-silacyclohex-1-yl)-disiloxane. The target compound was synthesized by hydrolysis of 1-chloro-1-phenylsilacyclohexane and its 13C-LT NMR spectra were registered [86]. Possible conformers are shown in Figure 20.

Figure 20

Optimized geometry (M062X/6-311G**) of possible conformers of (1,1′-phenyl-1,1′-silacyclohex-1-yl)-disiloxane. ‘ax’ and ‘eq’ refer to the position of the phenyl group.

Theoretical conformational analysis showed a slight energetic preference of the Phax conformers (Phax,Phax > Phax,Pheq > Pheq,Pheq) in spite of higher values for the bulkier phenyl group. This was explained by a larger energy gain from shortening of the Si–O bonds in the Phax conformers, which outweighed steric destabilization. Unfortunately, low-temperature 1H or 13C NMR studies showed the conversion of the conformers to be still fast on the NMR timescale at 100 K, so, further quantification could not be accomplished.

The answer to the question of conformational equilibrium of the studied siloxane was obtained from the 29Si-LT NMR spectra, which contained the signals of all three conformers [87]. This allowed to determine the ratio of the conformers and to assign them in accordance with the relative stability using the theoretically calculated 29Si chemical shifts at the GIAO/B3LYP/6-311++G(d,p)//B3LYP/6-311++G(d,p) level. The calculated shifts are reliable because (i) they lie in the interval of 2.3 ppm, which is well consistent with the experiment (2.6 ppm); (ii) the highest signal in the spectrum in Figure 21 is the most upfield one; the calculated signal for the most stable and, hence, most abundant ax–ax conformer also lies the most high field; (iii) the signal of lowest intensity is the most downfield one (Figure 21) and corresponds to the least stable eq–eq conformer; (iv) two signals of equal intensity appear between them and, judged from the relative energies of conformers in Figure 19, belong to the ax–eq conformer.

Figure 21

29Si-NMR spectra of (1,1′-phenyl-1,1′-silacyclohex-1-yl)disiloxane at 113 K (above) and at 103 K (below).

The ring inversion barrier ΔG# measured from the temperature of decoalescence Tc and the value of Δδ of the ax–ax and eq–eq conformers was found to be one of the lowest ever measured for six-membered rings, 4.8 kcal/mol [87].

It deserves to be mentioned that the spectrum in Figure 21 represents the first example of application of the low temperature 29Si-NMR spectroscopy in conformational analysis [87] (cf. also Figure 6 and the text above).

Interesting analogues of sila(hetero)cyclohexanes are sila(hetero)cyclohexenes. The first sulfur-containing silacyclohexene, 4,4-dimethyl-3,4-dihydro-2H-1,4-thiasiline, was obtained as shown in Scheme 3, in 66% yield by the rearrangement of 4,4-dimethyl-1,4-thiasilinane 1-oxide, using trifluoroacetic anhydride (R = CF3) [88].

Scheme 3

Pummerer rearrangement of 4,4-dimethyl-1,4-thiasilinane S-oxide

3,4-Dihydro-2H-1,4-thiasilines are interesting heterocycles for conformational analysis, but till our studies there were no information on the conformational preferences even of their monoheteroatomic predecessors—silacyclohexenes or 3,4-dihydro-2H-thiopyrans—not to mention thiasilacyclohexenes. Moreover, due to different chains linking the silicon and sulfur atoms (Figure 22), the molecule is chiral. However, the conformational equilibrium of the synthesized 4,4-dimethyl-3,4-dihydro-2H-1,4-thiasiline is fast on the NMR timescale even at 103 K, assumingly, due to higher flexibility, by analogy with very flexible cyclohexene ring (ΔG≠ = 5.37 kcal/mol, [89]) as compared to the cyclohexane ring (ΔG≠ = 10.3 kcal/mol, [90]). So, we had to limit our study to theoretical computational analysis [91].

Figure 22

Conformational equilibrium of 4,4-dimethyl-3,4-dihydro-2H-1,4-thiasiline

Calculations, however, did not prove a higher flexibility of the ring in Figure 22. Averaged barrier to the ring interconversion calculated by various methods was 5.7 kcal/mol, that coincides with that calculated by the most precise method MP2/6-311G**//MP2/cc-pVTZ [91].

Presuming that the phenyl groups to silicon would stabilize the compound and increase the barrier of interconversion we have synthesized 4,4-diphenyl-3,4-dihydro-2H-1,4-thiasiline by the same procedure as was used for the 4,4-dimethyl containing analogue [88]. The synthesis, however, was not a simple replica since some transformations were different and required a search for special reaction conditions. Full synthetic scheme, starting from diphenyl(divinyl)silane, is shown in Scheme 4.

Scheme 4

Synthetic sequence for preparation of 4,4-diphenyl-3,4-dihydro-2H-1,4-thiasiline.

Note, that the synthesized 3,4-dihydro-2H-1,4-thiasilines are the first silicon-containing cyclic vinyl sulfides. Although the target compound, indeed, turned out to be more stable chemically than its dimethylated analogue, still, no decoalescence of the signals in the NMR spectra was reached on cooling.

The higher chemical stability and the presence of sulfur atom in the molecule prompted us to synthesize S-functionalized derivatives of the final compound in Figure 23 [92]. Another reason was very few data available even on linear S-functional derivatives of β-silylated vinyl sulfides, to say nothing of cyclic ones. The reaction of oxidation with m-chloroperbenzoic acid (m-CPBA) gives the corresponding sulfoxide in 52% isolated yield. Further oxidation to sulfone was performed using a larger excess of the oxidant in up to 60% yield (Scheme 5). We have also attempted to prepare the corresponding sulfonimide by the reaction with chloramine B. The formation of the target product was proved by the appearance of two new doublets of the SiCH= and SCH= protons, different from those in other compounds in Scheme 5, as well as by the presence of two multiplets of diastereotopic SiCH2 protons, as in the case of the related sulfoxide. Since sulfonimides are the least stable among the S-functional derivatives, we failed to isolate the product in the analytically pure form, because the reaction is followed by generation of a large amount of nonidentified polysiloxanes. Nevertheless, the spectral data unequivocally prove its formation.

Figure 23

Total synthesis of 4,4-diphenyl-3,4-dihydro-2H-1,4-thiasiline.

Scheme 5

Synthesis of S-functional derivatives of 4,4-diphenyl-3,4-dihydro-2H-1,4-thiasiline.

Much lower stability of 4,4-dimethyl-3,4-dihydro-2H-1,4-thiasiline is characteristic also for its S-functional derivatives. During oxidation with m-CPBA, the compound, usually containing >10% of siloxane, gives a mixture of the sulfoxide, sulfone, and open-chain siloxanes containing the sulfoxide or sulfonyl groups [93].

Finally, the last investigated conformationally silacyclohexane was 1-t-butyl-1-phenyl-1-silacyclohexane, containing two voluminous substituents at silicon (our unpublished results). Both Ph and t-Bu groups are anancomeric in cyclohexanes, but in silacyclohexanes, only the t-Bu group has the value large enough to be fully located in the equatorial position (Table 1). The synthesis of the target compound was challenging and each stage had to be optimized. After cyclization of PhSiCl3 with the di-magnesium derivative of 1,5-dibromopentane, BrMg(CH2)5MgBr, and subsequent treatment of the formed 1-chloro-1-phenyl-1-silacyclohexane with t-BuLi in pentane, the target product was obtained in 43% yield.

The conformational analysis was performed experimentally by GED and theoretically using DFT and MP2 calculations in gas phase. Three conformers were analyzed, as shown in Figure 23.

From the quantum chemical calculations, the Phax and Pheq_90 conformations are most stable, the ΔG value of the Pheq_90 conformer being higher by 1.20–1.91 kcal/mol (cf. with the difference t-Bu–Ph of 1.05 kcal/mol in Table 1). The calculated molar fraction of the Phax conformer varies within 88–96%, being in nice agreement with the GED experimentally measured ratio Phax:Pheq_90 = 92(7):8(7)%. It can be concluded, that in the series of 1-Ph-1-X-silacyclohexanes for X = H, CH3, t-Bu, the contribution of the Phax conformer increases from 38(10) to 58(15) and 92(8)% with increasing the X group size.

To summarize, the specific features of the structure and conformational properties of various sila(hetero)cyclohexanes and some of their derivatives are analyzed in comparison to the carbon predecessors and with an accent on the recent studies in the field. In brief, they are: (i) the determining role of electrostatic as well as stereoelectronic effects due to the presence of a highly electropositive silicon atom and strongly polarized Si-X bonds; (ii) subordinate role of steric effects due to large covalent radius of Si; (iii) much lower conformational energies of the substituents at Si; (iv) much lower barriers to ring interconversion due to substantially planarized Si-containing fragment of the ring; (v) strong dependence on the aggregate state, in many cases resulting in the inversion of conformational preferences in going from gas to the solution.

The performed analysis can be useful for studying other heterocycles containing either ‘tetrel’ elements (Ge, Sn, Pb) or the silicon atom neighbors (P, As, S, Se, etc.).