Question

Statement 1 : To obtain effective $p\pi-d\pi$ overlap, the size of the $d$-orbital must be similar to the size of the $p$-orbital. So for chlorine $p\pi-d\pi$ bonding is strongest in their oxoanions.
Statement 2 : On moving a period from left to right in the periodic table, the nuclear charge is increased and more $s$ and $p$-electrons are added. Since these $s$ - and $p$-electrons shield the nuclear charge incompletely, the size of the atom and that of the $d$-orbitals decreases. This leads to progressively stronger $p\pi-d\pi$ bonding.

• A. If both Statement $1$ and Statement $2$ are true and the statement $2$ is the correct explanation of the statement $1$
• B. If both Statement $1$ and Statement $2$ are true but statement $2$ is not the correct explanation of the statement $1$
• C. If Statement $1$ is true but Statement $2$ is false
• D. If Statement $1$ is false but Statement $2$ is true

Answer 1

Answer: (A)

Both the statements are true and the Statement $2$ is the correct explanation for the Statement $1$.