Be sure to answer all parts. The sulfate ion can be represented with four S―O bonds or with two S―O and two S═O bonds. (a) Which

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Be sure to answer all parts. The sulfate ion can be represented with four S―O bonds or with two S―O and two S═O bonds. (a) Which

representation is better from the standpoint of formal charges? four S―O bonds two S―O bonds and two S═O bonds (b) What shape is the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding? bent tetrahedral trigonal planar trigonal pyramidal spmdn where m = and n = (c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O? sulfur: 3d 3p 2p 3s oxygen: 3p 2p 2s 3s

Chemistry

1 answer:

Anarel [2.9K] · Answer 1 · 2026-03-14T11:35:20+03:00

Response:

a) Representation - (in attachment)

b) The geometry is tetrahedral

c) $sp^{3}$ hybrid orbitals involve sigma bonding.

$\pi$ orbitals arise from the overlap of sulfur's d-orbitals with the p-orbitals of oxygen.

Clarification:

a)

Representation in attachment.

The total charge in both structures is -2. Structure (b) is preferred according to the resonance forms since the formal charges within the species are preserved.

Thus, structure (b) represents the sulfate ion more accurately.

b) In the sulfate ion, the sulfur atom forms connections with four distinct oxygen atoms. Using VSEPR theory, the sulfate ion is tetrahedral in shape.

There are four sigma bonds and no lone pairs surrounding the central atom.

Consequently, the sulfur atom's hybridization is $sp^{3}$

c)

The s and p orbitals of sulfur undergo hybridization to form sigma bonds. The orbitals involved in $\pi$ bonding are

Therefore, $\pi$ bonds result from the overlapping of sulfur's d-orbitals with the p-orbitals of oxygen.