Question

i) Give reason: Ionic radius of F (fluoride ion) is more than atomic radius of F (fluorine atom).
ii) How does ionization enthalpy varies down the group?
iii) Ionization enthalpy of nitrogen is more than that of oxygen. Give reason.​

Answer 1

Answer:

(1)As the number of electrons is increased, the nuclear force of attraction is decreased. Thus, the radius of fluoride ions is larger than that of fluorine atoms. F and are smaller and they have less shells. Between F and ,has one more electron, which causes the radius to be bigger.

(2)Ionization enthalpy decreases down the group. Reason: This is because atomic size increases down the group due to the increase in number of shells. The shielding effect increases and hence effective nuclear charge decreases.

(3)An atom is highly stable when its valence orbital is completely filled or half-filled and in nitrogen, the valence p orbital is exactly half filled. ... So, the ionization energy of nitrogen is more than that of oxygen.

Explanation:

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