Aluminium exhibits +3 oxidation state. As we move down the group, +1 oxidation state gets more stable. This is a consequence of

Question

Aluminium exhibits +3 oxidation state. As we move down the group, +1 oxidation state gets more stable. This is a consequence of (A) increasing size of the atom (B) inert pair effect (C) electron deficient nature (D) pπ - pπ bonding

Tardigrade Admin · Accepted Answer

The atoms of group 13 elements have 3 valence electrons, two in s subshell and one in p subshell. The +1 oxidation state becomes more stable as we move down to the group due to inert pair effect. After the removal of 1 electron from p orbital, the remaining ns 2 electrons behave like stable noble gases due to inert pair effect and do not take part in compound formation. The two electrons present in the s-shell are strongly attracted by the nucleus and do not participate in bonding. This inert pair effect becomes more and more prominent on moving down the group. Hence, the +1 oxidation state gets more stable as we move down the group.

Q. Aluminium exhibits $+ 3$ oxidation state. As we move down the group, $+ 1$ oxidation state gets more stable. This is a consequence of

increasing size of the atom

inert pair effect

electron deficient nature

$p π - p π$ bonding

Q. Aluminium exhibits +3 oxidation state. As we move down the group, +1 oxidation state gets more stable. This is a consequence of

increasing size of the atom

inert pair effect

electron deficient nature

pπ−pπ bonding

Q. Aluminium exhibits $+ 3$ oxidation state. As we move down the group, $+ 1$ oxidation state gets more stable. This is a consequence of

$p π - p π$ bonding