Antimony forms a compound with hydrogen that is called...

Antimony forms a compound with hydrogen that is called stibine. Its formula is $\mathrm{SbH}_{3}$ and the $\mathrm{H}-\mathrm{Sb}-\mathrm{H}$ bond angles are $91.3^{\circ} .$ Which kinds of orbitals does $S b$ most likely use to form the $\mathrm{Sb}-\mathrm{H}$ bonds: pure $p$ orbitals or hybrid orbitals? Explain your reasoning.

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Key Concepts

Orbital Hybridization

Orbital hybridization is the process where atomic orbitals mix to form new, equivalent orbitals that can effectively overlap with orbitals on another atom to form bonds. In many light elements, hybridization (such as sp³) leads to bond angles that are larger than 90°. However, in heavier elements, the energy cost of hybridizing can be significant, and sometimes the atom forms bonds using orbitals that are closer to their pure form.

Molecular Geometry and Bond Angles

Bond angles provide important clues about the type of orbitals used in bonding. Pure p orbitals intersect at right angles (approximately 90°), whereas hybrid orbitals, such as sp³, tend to have bond angles around 109.5°. Observing bond angles near 90° in a molecule suggests that the bonds are likely formed by unhybridized or minimally hybridized p orbitals.

Inert Pair Effect

The inert pair effect is a phenomenon observed in heavier p-block elements where the s electrons are less likely to participate in bonding due to relativistic and electron correlation effects. This leads to the use of mainly p orbitals for bond formation, which is consistent with the observed near-90° bond angles.

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