Question:
Nitrogen form N2, but phosphorous form P2, it's at a time convert in P4, reason is
Nitrogen form N2, but phosphorous form P2, it's at a time convert in P4, reason is
Updated On: Apr 17, 2024
- Triple bond present between phosphorous atom
- pπ – pπ bonding is weak
- pπ – pπ bonding is strong
- Multiple bond form easilly
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The Correct Option is B
Solution and Explanation
The correct option is(B): pπ – pπ bonding is weak.
Phosphorus cannot form pπ−pπ bonds due to its larger atomic size. Consequently, P atoms connect with each other through three sigma bonds. In contrast, Nitrogen forms triple bonds, consisting of one sigma bond and two pi bonds (1−σ and 2−π bonds), leading to its existence as diatomic molecules.
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Concepts Used:
Group 15 Elements
Group 15 elements are also known as nitrogen group elements or nitrogen family.
It consists of:
- Nitrogen (N)
- Phosphorus (P)
- Arsenic (As)
- Antimony (Sb)
- Bismuth (Bi)
- Moscovium (Mc)
They are present on the right side of the periodic table. All the elements are arranged based on their atomic weight. The elements with similar properties reside in a column called the group.
All Group 15 elements have the electron configuration ns2np3 in their outer shell, where n is the principal quantum number.
Periodic Trends in Group 15 Elements
