Question

8.64 Draw the Lewis structures for each of the following molecules or ions. Identify instances where the octet

rule is not obeyed; state which atom in each compound does not follow the octet rule; and state how many
electrons surround these atoms:
a. NO,
b. BF,.
c. ICL₂,
d. OPBr, (the P is the central atom),
e XeF..

Answer 1

This answer explains how to draw Lewis structures for the given molecules or ions, identifies instances where the octet rule is not obeyed, and states which atoms do not follow the octet rule and how many electrons surround them.

Step-by-step explanation:

Lewis Structures and Octet Rule

a. NO: The Lewis structure for NO has a single bond between the N and O atoms. Nitrogen is surrounded by 8 electrons and oxygen is surrounded by 7 electrons, so neither atom follows the octet rule.

b. BF: The Lewis structure for BF has a single bond between the B and F atoms. Boron is surrounded by 6 electrons and fluorine is surrounded by 8 electrons, so boron does not follow the octet rule.

c. ICL₂: The Lewis structure for ICL₂ has a single bond between the I and Cl atoms. Iodine is surrounded by 10 electrons and chlorine is surrounded by 8 electrons, so iodine does not follow the octet rule.

d. OPBr: The Lewis structure for OPBr has a double bond between the O and P atoms and a single bond between the P and Br atoms. Phosphorus is surrounded by 8 electrons, so it follows the octet rule.

e. XeF: The Lewis structure for XeF has a single bond between the Xe and F atoms. Xenon is surrounded by 12 electrons, so it does not follow the octet rule.