Question

Statement 1: The molecule $S{{O}_{2}}$ has a net dipole.
Statement 2: Oxygen has a higher electronegativity than sulphur.
(A) Both statement 1 and statement 2 are correct and statement 2 is the correct explanation of the statement 1.
(B) Both statement 1 and statement 2 are correct, but statement 2 is NOT the correct explanation of statement 1.
(C) Statement 1 is correct, but statement 2 is not correct.
(D) Statement 1 is not correct, but statement 2 is correct.

Answer 1

The dipole moment in any compound is directed towards the more electronegative atom of the compound. The lone pair-lone pair repulsion is much greater than the lone pair-bond pair and bond pair-bond pair repulsion.

Complete step by step answer:
$S{{O}_{2}}$ has a net dipole moment. This is because there is an appreciable difference of electronegativity between Sulphur and Oxygen atoms. Since Oxygen is more electronegative, the electrons on the sulphur atoms are attracted toward the oxygen atom, creating a net dipole moment. Also $S{{O}_{2}}$ has two lone pairs on the central atom, which cause lone pair-lone pair repulsion, which bents the structure of $S{{O}_{2}}$, therefore, the dipole moment have a non zero value.

So, the correct answer is “Option A”.

Note: Dipole moment is any compound that arises when there is separation of charges. Dipole moment can arise in ionic compounds and covalent compounds. Dipole moments occur due to the difference in the electronegativity of the two bonded atoms. A dipole moment is a measure of the polarity of a chemical bond between two atoms in a molecule.