Assertion (A) : The ionisation energy of N is more than that of O
Reason (R ) : Electronic configuration of N is more stable due to half - fillied `2p` orbitals

Assertion: The first ionisation energy of Be is greater than that of B . Reason: 2p-orbital is lower in energy than 2s-orbital.

Assertion: The first ionisation energy of Be is greater than that of B . Reason: 2p-orbital is lower in energy than 2s-orbital.

Assertion: The first ionisation energy of Be is greater than that of B . Reason: 2p-orbital is lower in energy than 2s-orbital.

Assertion (A) : The first IE of Be is greater than that of B Reason (R ) : 2p orbitals is lower in energy than 2s

Assertion (A): The second ionisation energy of 'O' is greater than that of 'N' Assertion (R): The half flled p-orbitals cause greater stability.

Assertion: ionisation energy of sulphur is less than that of phosphorus. Reason: Half filled p-orbitals have extra stability.

Statement-1: First ionisation energy of O^(+)(g) is greater than that of N(g) whereas vice versa is true for the first ionisation energy of N^(+)(g) and N(g) respectively. Statement-2: Electronic configuration of N(g) is more stable than that of N^(+)(g) .

Assertion (A) : Ionisation potential of Be (atomic number 4 ) is more than B (atomic number 5) Reason (R ) : The first electron released fromm Be is of p orbitals but that from B is of s orbitals.