Question

Assertion (A) : First ionisation enthalpy of N is higher than 0.
Reason (R) : Extra stability of half-filled 2p subshell of O atom.
Assertion (A) : Second IE of all elements are always higher than first IE.
Reason (R): IE of noble gas elements are highest in their respective period.
Assertion (A) : IE of Alkali metals are lowest in a period.
Reason (R): The size of Alkali metals are largest in any period.
OR
Assertion (A): IE in a period increases as we go from left to right.
Reason (R): In period left to right Zeff decreases and geff increases.


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Answer 1

First ionisation enthalpy of N is higher than 0.

Reason (R) : Extra stability of half-filled 2p subshell of O atom.

Assertion (A) : Second IE of all elements are always higher than first IE.

Reason (R): IE of noble gas elements are highest in their respective period.

Assertion (A) : IE of Alkali metals are lowest in a period.

Reason (R): The size of Alkali metals are largest in any period.

OR

Assertion (A): IE in a period

Answer 2

A) In reality, the first ionisation energy of nitrogen is greater than the first ionisation energy of oxygen because nitrogen, in a stable half filled orbital state, is comparatively more stable than oxygen.

A) So, second ionization enthalpy is always higher than the first ionisation enthalpy for every element. Solution : Electron is more tightly bound by the nucleus in an cation (i.e M+) as the number of proton remains the same as in neutral atom whereas number of electron is one less than the proton.

A) On the periodic table, first ionization energy generally increases as you move left to right across a period. This is due to increasing nuclear charge, which results in the outermost electron being more strongly bound to the nucleus.

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