Question

choose the number of lone pairs or atoms to complete each description below. a molecule that has a trigonal - planar shape has lone pair(s). a molecule that has a bent shape and a trigonal - planar electron domain shape has lone pair(s). a molecule that has a trigonal - pyramidal shape has atom(s) and lone pair(s) around the central atom. done

Explanation:

Step1: Recall trigonal - planar shape

A molecule with a trigonal - planar shape has 0 lone pairs around the central atom. The three bonding domains are arranged in a plane at 120 - degree angles.

Step2: Recall bent shape with trigonal - planar electron - domain

A molecule with a bent shape and a trigonal - planar electron - domain shape has 1 lone pair. The presence of one lone pair on the central atom causes the bond angles to be less than 120 degrees, resulting in a bent shape.

Step3: Recall trigonal - pyramidal shape

A molecule with a trigonal - pyramidal shape has 3 bonding atoms and 1 lone pair around the central atom. The lone pair exerts a greater repulsion than bonding pairs, causing the bond angles to be less than the tetrahedral angle of 109.5 degrees.

Answer:

A molecule that has a trigonal - planar shape has 0 lone pair(s).
A molecule that has a bent shape and a trigonal - planar electron domain shape has 1 lone pair(s).
A molecule that has a trigonal - pyramidal shape has 3 atom(s) and 1 lone pair(s) around the central atom.