The increasing order of the first ionisation enthalpies of the elements B, P, S and F (lowest first) is.
The increasing order of the first ionisation enthalpies of the elements B, P, S and F (lowest first) is
(a) F < S < P < B
(b) P < S < B < F
(c) B < P < S < F
(d) B < S < P < F.
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(d) : Element: B S P F
I.E. (eV): 8.3 10.4 11.0 17.4
In general as we move from left to right in a period, the ionisation enthalpy increases with increasing atomic number. The ionisation enthalpy decreases as we move down a group. P(1s2 2s2 2p6 3s2 3p3 ) has a stable half filled electronic configuration than S (1s2 2s2 2p6 3s2 3p4 ). For this reason, ionisation enthalpy of P is higher than S.
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