Question

which is the correct order number for bond length of C-O in CO, CO3^2- and Co2 ?
(A)CO2 <CO3^2-<CO
(B) CO <CO3^2- <CO2
(C )CO<CO2<CO3^2-
(D)CO3^2-<CO2 <CO​

Answer 1

Answer:

May be... option (C)

CO < CO2 < CO3^2-

Answer 2

hi friend,

here is your answer

Answer:

(c) co<co2<co3^2-

Explanation:

CO<CO2<CO3^2- is the increasing bond length order because

CO has triple bond so bond length minimum and CO2 has double bond so its bond length maximum then CO and CO32- has partial single bond characters due to resonance so it has maximum bond length .

step by step explanation

Method (1) Bond-multiplicity increases bond-length.

Thus,

(i) C≡)→ has least bond-length.

(ii) O=C+O→ next to C=O.

(iii)

Hence, increasing order of bond-length is CO<CO

2

<CO

3

2−

Method (2)

(i) More be the value of bond-order smaller be the bond-length and more be the bond-energy.

(ii) Bond-order (BO)=

Total number of canonical forms

Total number of bonds associated between two atoms in all structure

(a) CO→C≡O→BO=

1

3

=3

(b) CO

2

→O=C=C→BO=

2

4

=2

Hence, order of bond-length CO<CO

2

<CO

3

2−

Epimer is used to designate diastereomers that differ in configuration at only one chiral centre.

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