what is the bond order of the s - o bonds in the following?\na. 1.00\nb. 1.33\nc. 1.50\nd. 1.75\ne. 2.00
what is the bond order of the s - o bonds in the following?\na. 1.00\nb. 1.33\nc. 1.50\nd. 1.75\ne. 2.00
Answer
Explanation:
Step1: Identify resonance structures
There are 3 resonance - contributing structures for the $SO_{3}^{2 - }$ ion shown.
Step2: Calculate bond order formula
The formula for bond order in case of resonance is $\text{Bond Order}=\frac{\text{Total number of bonding pairs}}{\text{Number of equivalent bonds}}$. In the resonance structures of $SO_{3}^{2 - }$, the total number of bonding pairs between S and O is 4 (counting all the double - bond and single - bond contributions in the resonance forms), and the number of equivalent S - O bonds is 3.
Step3: Calculate bond order
$\text{Bond Order}=\frac{4}{3}\approx1.33$.
Answer:
B. 1.33