Explain the deviation in ionisation enthalpy of some elements from the general trend by using given figure.

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Solution

Ionisation enthalpy increases in a period with an increase in atomic number. The graph shows a few exceptions and not the linear relationship. Ionisation enthalpy of Be is greater than that of B due to filled s-orbital in Be $B e = 1 s^{2} 2 s^{2}, a n d B = 1 s^{2} 2 s^{2} 2 p^{1}$ .

Ionisation enthalpy of N is greater than that of O due to half-filled/?-orbitals in nitrogen. $N = 1 s^{2} 2 s^{2} 2 p^{3} a n d O = 1 s^{2} 2 s^{2} 2 p^{4}$ .

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The first ionization enthalpy values (in kJ $m o l^{- 1}$ ) of group 13 elements are :

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The first ionization enthalpy values (in kJmol^–1) of group 13 elements are :

B	Al	Ga	In	Tl
801	577	579	558	589

How would you explain this deviation from the general trend?

(K J {m o l}^{- 1})

Define ionisation enthalpy. Discuss the factors affecting ionisation enthalpy of the elements and its trends in the periodic table.

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