Question

Consider the trichlorostannanide (SnCl^-_3) anion. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the angle between the tin-chlorine bonds? Compared to the ideal angle, you would expect the actual angle between the tin-chlorine bonds to be

Answer 1

The central atom in the trichlorostannanide (SnCl^-_3) anion is tin (Sn). There is one lone pair of electrons around the central tin atom. The angle between the tin-chlorine bonds is 120°.

Step-by-step explanation:

The central atom in the trichlorostannanide (SnCl-3) anion is tin (Sn).

There is one lone pair of electrons around the central tin atom.

The angle between the tin-chlorine bonds is 120°.

Compared to the ideal angle of 120°, we would expect the actual angle between the tin-chlorine bonds to be 120°.

Answer 2

In the trichlorostannanide ion, tin (Sn) is the central atom with one lone pair of electrons, and the angle between the tin-chlorine bonds is approximately 95° due to lone pair-bonding pair repulsion, which is smaller than the ideal 120° of a trigonal planar arrangement.

Step-by-step explanation:

In the trichlorostannanide ion (SnCl-3), the central atom is tin (Sn). Based on the geometry described, this anion has a bent molecular shape, similar to SO2, with a lone pair of electrons on the tin atom. There are three electron groups around the central atom: two bonding groups (the chlorine atoms) and one lone pair of electrons, which is consistent with an AX2E designation. The ideal angle in a trigonal planar arrangement is 120°, but due to the lone pair occupying more space and pushing the tin-chlorine bonds closer together, the Cl-Sn-Cl bond angle is reduced to approximately 95°. This angle is smaller than the ideal angle because of the increased repulsion between the lone pair and bonding pairs of electrons.