Question

Which of the following statements concerning SO₂ is (are) true?

a. The central sulfur atom is sp² hybridized.

b. One of the sulfur–oxygen bonds is longer than the other(s).

c. The bond angles about the central sulfur atom are about 120 degrees.

d. There are two bonds in SO₂.

e. There are no resonance structures for SO₂.

Short answer

Sulfur dioxide is formed by two oxygen molecules and one central sulfur atom which are bonded with two sigma and two pie bonds. As sulfur has one lone pair also it will exhibit sp² hybridization. It can form two resonating structures, due to which the bond length of both sulfur oxygen is same.

Step-by-step solution

(a) Hybridisation

To calculate hybridization, we have to add a number of sigma bonds and a number of lone pairs. In SO₂, sulfur atom forms two sigma bond and have one lone pair. So, the hybridization will become sp².

(b) Bond length

The bond length of both the sulfur-oxygen bonds is the same due to the phenomenon of resonance, it has a partial positive charge on sulfur and a partial negative charge on oxygen.

(c) Bond angle

The sulfur has formed two sigma and two pie bonds and also it consists of a lone pair, due to which it will repel the bond pair of sulfur and oxygen and forms 109.5 degrees of bond angle.

(d)

The sigma bond in a molecule is represented by a single bond whereas a double and triple bond is considered as pie bond. So, in SO ₂there are two single bonds and thus have two sigma bonds.

(e) Resonance structure

Resonance structure shows the delocalization of electrons around the atoms. In SO₂, there are two resonating structures possible as shown below:

It is an incorrect answer.