Multiple Choice
Given a molecule in which the antimony atom forms three sigma bonds and has one lone pair, what is the hybridization of the antimony atom?
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12. Molecular Shapes & Valence Bond Theory
Hybridization
Multiple Choice
Which type of hybridization is exhibited by the oxygen atoms in the nitrate ion (NO_3^-)?
A
sp^2
B
sp^3
C
sp
D
none (oxygen atoms are not hybridized)
Verified step by step guidance1
Step 1: Understand the structure of the nitrate ion (NO_3^-). It consists of one nitrogen atom centrally bonded to three oxygen atoms, with resonance structures distributing the double bond among the oxygens.
Step 2: Recall that hybridization depends on the steric number, which is the number of atoms bonded plus the number of lone pairs on the atom in question. For oxygen in NO_3^-, consider its bonding and lone pairs.
Step 3: Each oxygen atom in NO_3^- is bonded to nitrogen with a single or partial double bond (due to resonance) and has two lone pairs of electrons. This means each oxygen has three regions of electron density (1 bond + 2 lone pairs).
Step 4: Using the steric number of 3, determine the hybridization of oxygen atoms. A steric number of 3 corresponds to sp^2 hybridization.
Step 5: Conclude that the oxygen atoms in the nitrate ion exhibit sp^2 hybridization because they have three electron regions around them, consistent with trigonal planar electron geometry.
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