Question

44. The correct order in which the 0-0 bond
length increases in the following:
1) H20,< 0, < O3 2) O2 < H2O2< 02
3) 02 < H202 < 03; 4) 02, < 03, < H,202
ANSWER WITH EXPLAINATION PLZZZZ​

Answer 1

Answer:

Explanation:

first find where it is having better over lapping

extent of overlapping is inversely proportional to n1+n2

where n1 is shell number of atom 1 and n2 is shell no. of 2

and if n1+n2 is same find more directional orbitals

and which has more directional orbitals has better overlapping

in h2o2 and o2

o2 has less bond length bcoz double bond character

and in h2o2 there is no double character so more bond length

and in o3

there are equivalent resonating structures

so bond length of all are same and that is average of all so it should be greater than 1

so h2o2 has more bond length and o3

so option d

Answer 2

$\huge \: \red \star \: { \large \pink { \underline\mathcal{ANSWER}} } \: \red\star \: </p><p></p><p> \:$

• option ( 4 ) is correct answer

$\\ \green{concept}$

• Here :- MOT ( molecular orbital theory)
• see explanation for other concepts

$\\ \green{ \text{factors affecting bond length} }$

• bond length inversly proportinal to electronegativity difference.

• $\footnotesize{d_{A-B } =r_A + r_B - 0.09 \times \underline \land \: EN }$
• bond length inversly proportinal to bond order. ( use MOT class 11 )
• bond length inversly proportinal to percentage s character.
• here h202 has all single bond in its structure. or we can say bond order is 1 .
• for o2 bond order is 2 as o2 form double bond
• 03 also have partial double bond character but not complete double bond . also not complete single bond. so it is in intermediate.

hope it helps