Explain the following question (based on ionisation energy):
(a) Why `IE_(1)` of `N` is higher than that of `O` atom ?
(b) Why `IE_(1)` of `Mg` is higher than that of `Al` atom?
(c ) Why `IE_(1)` of `C` is greater than that of `B` atom whereas `IE_(2)` is reverse ?
(d) In general, `IE` increases along the period `(rarr)`. Explain why the `IE_(2)` of `Cr` is higher than that of `Mn` (Manganese)?
(e) The `IE_(1)` and `IE_(2)` of `K` are `420` and `3050 kJ mol^(-1)` respectively and those of `Ca` are `560` and `1140 kJ mol^(-1)` respectively. Compare their values and comment on the differences.
(f) The `IE` of `Li`, `Be` and `C` are `5.5, 9.3` and `11.3 eV`. What would be the case and explain.
i. `K, Ca,Se` , ii. `N,O,F`
iii. `K^(o+), Ar,Cl^(ɵ)` , iv `Fe, Fe^(2+), Fe^(3+)`
v. `C,N,O` , vi. `Cu,Ag,Au`
vii. `K, Rb, Cs` , viii `Be, B, C`
ix. `Na, Mg, Al`
(h) Explain why `Fe^(2+)` is more easily oxidised to `Fe^(3+)` than `Mn^(2+)` to `Mn^(3+)`.
(i) Explain whether `IE_(1)` of two isotopes of same element would be same or different.
(j) What are the factors on which `IE` of main group elements tends to decrease douwn the group `(darr)`.