Question

The decreasing values of bond angles from NH₃ (106º) to
SbH₃ (101º) down group-15 of the periodic table is due to
(a) decreasing lp-bp repulsion
(b) decreasing electronegativity
(c) increasing bp-bp repulsion
(d) increasing lp-bp repulsion

Answer 1

The answer is Option a)

Thanks❤

Answer 2

Decreasing electronegativity is the cause.

Explanation:

• The compounds given here are NH3, PH3, AsH3, SbH3.

• The central atoms are the nitrogen, phosphorous, arsenic and antimony.

• All these atoms belong to group 15 of the periodic table.

• As we know, due to increase in size of an atom, the electronegativity increase as we go down the group.

• So trend of electronegativity here is N >P>As>Sb.

• And the electronegativity gives the size of the bond.

• So, the bond size being lower, gives the bond pair bond pair repulsion.

• As we go down, size of atom increase, giving less bp bp repulsion.

• So the hydrogens come closer.

For more information about electronegativity,

https://brainly.in/question/8270445

What is electronegativity?explain why halogens possess highest electronegativity?

https://brainly.in/question/2321200

What is electronegativity?how does it compare with electron affinity