in PO4 3- iron , the formal charge on each oxygen atom and P-O bond order respectively are
Answers
Answer:
0.75,1.25
Explanation:
In PO
4
3−
, the formal charge on each oxygen atom and the P−O bond order are −0.75,1.25 respectively.
⎣
⎢
⎢
⎡
O−
O
∣∣
P
∣
O
−O
⎦
⎥
⎥
⎤
3−
↔
⎣
⎢
⎢
⎡
O−
P
∣
P
∣
O
=O
⎦
⎥
⎥
⎤
3−
⎣
⎢
⎢
⎡
O−
O
∣
P
∣∣
O
−O
⎦
⎥
⎥
⎤
3−
↔
⎣
⎢
⎢
⎡
O=
P
∣
P
∣
O
−O
⎦
⎥
⎥
⎤
3−
Bond order =
Number of Resonating structures
Number of bonds
=
4
5
=1.25
In a given resonance structure, the O atom that forms double bond has formal charge of 0 and the remaining 3 O atoms have formal charge of -1 each.
In the resonance hybrid, a total of -3 charge is distributed over 4 O atoms. Thus the formal charge of each O atom is
4
−3
=−0.75.
Note:
To calculate the formal charge, the following formula is used.
Formal Charge = [Number of valence electrons on atom] – [non-bonded electrons + number of bonds]
For O atom that forms double bond with P atom,
Formal Charge = 6] – [4 +2] = 0.
For O atom that forms single bond with P atom,
Formal Charge = 6] – [6 +1] =− 1.
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