Advertisements
Advertisements
Question
Account for the following :
N − N single bond is weaker than P − P single bond.
Advertisements
Solution
N-N single bond is weaker than P-P bond due to smaller size of N as compared to P. Smaller size of N leads to smaller N-N bond length. As a result, the lone pair of electrons on the both the N atoms repel each other leading to unstability or weakening of N-N bond.
APPEARS IN
RELATED QUESTIONS
Nitrogen does not form pentahalide.
Discuss the general characteristics of Group 15 elements with reference to their electronic configuration.
Give reasons for the following:
E⁰ value for (Mn3+|Mn2+) is highly positive than that for (Cr3+|Cr2+) couple.
Maximum covalency of nitrogen is ______.
Which of the following group 15 elements forms metallic bonds in an elemental state?
The p-block element of group 15 that forms predominantly basic oxide is _____________.
Which of the following statements is wrong?
In \[\ce{PCl5}\], phosphorus is in sp3d hybridised state but all its five bonds are not equivalent. Justify your answer with reason.
Account for the following:
Zinc is a comparatively a soft metal, iron and chromium are typically hard.
In which one of the following arrangements the given sequence is not strictly according to the properties indicated against it?
