Predict the hybridization of the oxygen atom in water, H2O. Draw a picture of its three-dimensional structure, and explain why its bond angle is 104.5°.

Ch.1 - Structure and Bonding

Wade9th EditionOrganic ChemistryISBN: 9780135213728당신이 사용하는 게 아니라요?교과서 변경

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Wade 9th Edition

Ch.1 - Structure and Bonding

문제 16a

1장, 문제 16a

Predict the hybridization of the oxygen atom in water, H₂O. Draw a picture of its three-dimensional structure, and explain why its bond angle is 104.5°.

검증된 단계별 안내

Identify the central atom in the molecule. In water (H2O), the central atom is oxygen.

Determine the number of valence electrons for the oxygen atom. Oxygen has 6 valence electrons.

Consider the bonding and lone pairs around the oxygen atom. In H2O, oxygen forms two sigma bonds with hydrogen atoms and has two lone pairs of electrons.

Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the hybridization. The steric number (number of sigma bonds + lone pairs) for oxygen in H2O is 4, indicating sp³ hybridization.

Explain the bond angle. The ideal bond angle for sp³ hybridization is 109.5°, but the presence of lone pairs, which exert greater repulsion than bonding pairs, reduces the bond angle to approximately 104.5°.

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주요 개념

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Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for pairing electrons to form chemical bonds. In water (H2O), the oxygen atom undergoes sp3 hybridization, which involves the mixing of one s orbital and three p orbitals, resulting in four equivalent sp3 hybrid orbitals. This hybridization explains the tetrahedral arrangement of electron pairs around the oxygen atom.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. In water, the geometry is bent or V-shaped due to the two lone pairs on the oxygen atom, which repel the hydrogen atoms, resulting in a bond angle of 104.5°. This angle is less than the ideal tetrahedral angle of 109.5° due to the greater repulsion exerted by lone pairs compared to bonding pairs.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the shape of molecules based on electron pair repulsions. According to VSEPR theory, electron pairs around a central atom will arrange themselves to minimize repulsion. In H2O, the two lone pairs on oxygen push the hydrogen atoms closer together, resulting in a bond angle of 104.5°, which is characteristic of a bent molecular shape.