Ozone (O3) is composed of three oxygen atoms. To determine the number of lone pairs on the oxygen atoms, we need to understand its Lewis structure. In O3, one oxygen atom is bonded to another by a double bond, and the third oxygen is bonded to the central oxygen by a single bond, resulting in resonance structures. Each oxygen atom follows the octet rule, aiming for eight electrons in the outer shell.
Step-by-step Breakdown:
Each oxygen atom has 6 valence electrons.
In the resonance structures of ozone, the central oxygen atom (oxygen #2) is bonded to two other oxygen atoms (oxygen #1 and #3).
Oxygen #1 forms a double bond with the central oxygen atom, using 2 bonding pairs (4 electrons) and has 2 lone pairs (4 electrons).
The central oxygen atom has one lone pair and forms a single and a double bond (6 electrons used for bonding and 2 in a lone pair).
Oxygen #3 is singly bonded to the central oxygen atom, using 1 bonding pair (2 electrons) and has 3 lone pairs (6 electrons).
Addition of Lone Pairs:
Oxygen #1: 2 lone pairs
Oxygen #2: 1 lone pair
Oxygen #3: 3 lone pairs
Total lone pairs = 2 + 1 + 3 = 6.
Therefore, the total number of lone pairs on the oxygen atoms of ozone is 6, which falls within the specified range of 6,6.
