The late F.H. Allen from the Cambridge Crystallographic Data Center has written a LOT about H-bonding in the solid state.  One example of his work can be found at  https://www.ccdc.cam.ac.uk/Community/crystalformconsortium/casestudies/hydrogenbondingpreferences/     There are a lot of papers by him talking about h-bonding motifs.

Dear Apramata,

In 1999, Isaacs et al. showed from interpretations of the anisotropies in the Compton profile of ordinary ice that the hydrogen bond is partly covalent. Some NMR data on hydrogen bonds in proteins also indicate covalent bonding.

Most generally, the hydrogen bond can be viewed as a metric-dependent electrostatic scalar field between two or more intermolecular bonds. This is slightly different from the intramolecular bound states of, for example, covalent or ionic bonds; however, hydrogen bonding is generally still a bound state phenomenon, since the interaction energy has a net negative sum. The initial theory of hydrogen bonding proposed by Linus Pauling suggested that the hydrogen bonds had a partial covalent nature. This remained a controversial conclusion until the late 1990s when NMR techniques were employed by F. Cordier et al. to transfer information between hydrogen-bonded nuclei, a feat that would only be possible if the hydrogen bond contained some covalent character. While much experimental data has been recovered for hydrogen bonds in water, for example, that provide good resolution on the scale of intermolecular distances and molecular thermodynamics, the kinetic and dynamical properties of the hydrogen bond in dynamic systems remain unchanged.

The dynamics of hydrogen bond structures in water can be probed by the IR spectrum of OH stretching vibration. In terms of hydrogen bonding network in protic organic ionic plastic crystals (POIPCs), which are a type of phase change materials exhibiting solid-solid phase transitions prior to melting, variable-temperature infrared spectroscopy can reveal the temperature dependence of hydrogen bonds and the dynamics of both the anions and the cations. The sudden weakening of hydrogen bonds during the solid-solid phase transition seems to be coupled with the onset of orientational or rotational disorder of the ions.

Hydrogen bonds can vary in strength from very weak (1–2 kJ mol−1) to extremely strong (161.5 kJ mol−1 in the ion HF−

2).Typical enthalpies in vapor include:

F−H…:F (161.5 kJ/mol or 38.6 kcal/mol)

O−H…:N (29 kJ/mol or 6.9 kcal/mol)

O−H…:O (21 kJ/mol or 5.0 kcal/mol)

N−H…:N (13 kJ/mol or 3.1 kcal/mol)

N−H…:O (8 kJ/mol or 1.9 kcal/mol)

HO−H…:OH+

3 (18 kJ/mol or 4.3 kcal/mol; data obtained using molecular dynamics as detailed in the reference and should be compared to 7.9 kJ/mol for bulk water, obtained using the same molecular dynamics.).

References:

Isaacs, E.D.; et al. (1999). "Covalency of the Hydrogen Bond in Ice: A Direct X-Ray Measurement". Physical Review Letters 82 (3): 600–603. Bibcode:1999PhRvL..82..600I. doi:10.1103/PhysRevLett.82.600.

Cordier, F; Rogowski, M; Grzesiek, S; Bax, A (1999). "Observation of through-hydrogen-bond (2h)J(HC') in a perdeuterated protein". J Magn Reson. 140 (2): 510–2.

Cowan ML; Bruner BD; Huse N; et al. (2005). "Ultrafast memory loss and energy redistribution in the hydrogen bond network of liquid H2O". Nature 434 (7030): 199–202. Bibcode:2005Natur.434..199C. doi:10.1038/nature03383. PMID 15758995.

Luo, Jiangshui; Jensen, Annemette H.; Brooks, Neil R.; Sniekers, Jeroen; Knipper, Martin; Aili, David; Li, Qingfeng; Vanroy, Bram; Wübbenhorst, Michael; Yan, Feng; Van Meervelt, Luc; Shao, Zhigang; Fang, Jianhua; Luo, Zheng-Hong; De Vos, Dirk E.; Binnemans, Koen; Fransaer, Jan (2015). "1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells". Energy & Environmental Science 8 (4): 1276. doi:10.1039/C4EE02280G

Larson, J. W.; McMahon, T. B. (1984). "Gas-phase bihalide and pseudobihalide ions. An ion cyclotron resonance determination of hydrogen bond energies in XHY- species (X, Y = F, Cl, Br, CN)". Inorganic Chemistry 23 (14): 2029–2033. doi:10.1021/ic00182a010.

 Emsley, J. (1980). "Very Strong Hydrogen Bonds". Chemical Society Reviews 9 (1): 91–124. doi:10.1039/cs9800900091.

Markovitch, Omer and Agmon, Noam (2007). "Structure and energetics of the hydronium hydration shells". J. Phys. Chem. A 111 (12): 2253–2256. doi:10.1021/jp068960g. PMID 17388314.

Hoping this will be helpful,

Rafik

The structure of H-bind in the solid states is governed somewhat with the crystal packing, while in the liquid state the H-bond is not under forced. Therefore the strength of H-bond in the solid state and in liquid phase may be quite different. This difference is much more pronounced for the intermolecular H-bonded systems than for intramolecular one. On the other hand for intermolecular hydrogen bond in non polar solvents all or at least part of the hydrogen bonded systems disappear. 

Thank you for your responses.

Joseph , I actually wanted a comparison of the nature of hydrogen bonding in solid state to that of liquid state. Rafik ...thanks a lot for the references.

Sayyed, what do you mean that the H-bond is not under forced? Is it weaker or do you mean that it has more freedom of choice? Could you point to some references?

Apramita,   the articles by Allen actually do a lot of comparison between solid state and the theoretical and experimental structures supposed in the liquid state.  

But see also the paper by Ghanty et al. (JACS, 122, 1210-1214 (2000)) showing that the interpretation of the Compton scattering results in the paper by Isaacs et al. was incorrect.

Thank you all for this valuable input.