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HandWiki. Chemical Bonding of H2O. Encyclopedia. Available online: https://encyclopedia.pub/entry/29914 (accessed on 23 September 2026).
HandWiki. Chemical Bonding of H2O. Encyclopedia. Available at: https://encyclopedia.pub/entry/29914. Accessed September 23, 2026.
HandWiki. "Chemical Bonding of H2O" Encyclopedia, https://encyclopedia.pub/entry/29914 (accessed September 23, 2026).
HandWiki. (2022, October 18). Chemical Bonding of H2O. In Encyclopedia. https://encyclopedia.pub/entry/29914
HandWiki. "Chemical Bonding of H2O." Encyclopedia. Web. 18 October, 2022.
Chemical Bonding of H2O
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The content is sourced from: https://handwiki.org/wiki/Chemistry:Chemical_bonding_of_H2O

Water (H2O) is a simple triatomic bent molecule with C2v molecular symmetry and bond angle of 104.5° between the central oxygen atom and the hydrogen atoms. Despite being one of the simplest triatomic molecules, its chemical bonding scheme is nonetheless complex as many of its bonding properties such as bond angle, ionization energy, and electronic state energy cannot be explained by one unified bonding model. Instead, several traditional and advanced bonding models such as simple Lewis and VESPR structure, valence bond theory, molecular orbital theory, isovalent hybridization, and Bent's rule are discussed below to provide a comprehensive bonding model for H2O, explaining and rationalizing the various electronic and physical properties and features manifested by its peculiar bonding arrangements.

chemical bonding molecular symmetry molecular orbital

References

  1. Levine, I. N. (1991). Quantum Chemistry (4th ed.). Prentice-Hall. p. 475. ISBN 978-0-7923-1421-9. 
  2. "The MO Diagram of H2O". http://www.huntresearchgroup.org.uk/teaching/teaching_MOs_year2/L2_Notes_2015_web.pdf. 
  3. "Molecular Orbitals in Inorganic Chemistry: Hunt Research Group, Imperial College London". http://www.huntresearchgroup.org.uk/teaching/year2_mos.html. 
  4. "Molecular Orbitals in Inorganic Chemistry". http://www.huntresearchgroup.org.uk/teaching/teaching_MOs_year2/L2_Slides_2015_web_viewing.pdf. 
  5. Laing, Michael (1987). "No rabbit ears on water. The structure of the water molecule: What should we tell the students?". Journal of Chemical Education 64 (2): 124. doi:10.1021/ed064p124. Bibcode: 1987JChEd..64..124L.  https://dx.doi.org/10.1021%2Fed064p124
  6. "Chem 216: Honors General Chemistry : The Lee Group Solid State Chemistry in the Lee Group". http://leelab.chem.cornell.edu/courses/chem-216-honors-general-chemistry/. 
  7. "Home" (in en). http://www.roaldhoffmann.com/. 
  8. Hoffmann, Roald; Shaik, Sason; Hiberty, Philippe C. (2003-10-01). "A Conversation on VB vs MO Theory: A Never-Ending Rivalry?". Accounts of Chemical Research 36 (10): 750–756. doi:10.1021/ar030162a. ISSN 0001-4842. PMID 14567708.  https://dx.doi.org/10.1021%2Far030162a
  9. "Contrasting MO and VB theory" (in en-US). Chemistry LibreTexts. 2013-10-02. https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Chemical_Bonding/General_Principles_of_Chemical_Bonding/Contrasting_MO_and_VB_theory. 
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