The increasing order of the first ionization enthalpies of the elements B,P,S and F (lowest first) is:

Options

A. `F lt S lt P lt B`
B. `P lt S lt B lt F`
C. `B lt P lt S lt F`
D. `B lt S lt P lt F`

Answer

D

Explanation

`{:("Element":,B,S, P, F),(I.E.(kJ mol^(-1)):,801,1000,1011,1681):}`
In general as we move from left to right in a period, the ionization enthalpy increases with increasing atomic number. The ionization enthalpy decreases as we move down a group. `P (1s^(2), 2s^(2),3s^(2), 3p^(3))` has a stable half filled electronic configuration than `S(1s^(2), 2s^(2), 2p^(6), 3s^(2), 3p^(4))`. For this reason, ionization enthalpy of `P` is greater than `S.`