The increasing order of the first ionisation enthalpies of the elements B, P, S and F (lowest first) is
A
F < S < P < B
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B
P < S < B < F
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C
B < P < S < F
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D
B < S < P < F
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Solution
The correct option is D B < S < P < F Element:BSPFI.E.(eV):8.310.411.017.4 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(1s22s22p63s23p3) has a stable half filled electronic configuration than S(1s22s22p63s23p4). For this reason, ionisation enthalpy of P is higher than S.