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
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The answer is Option a)
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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,
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