In which of the following cases, the former change would require lesser energy than the latter?
A
Be+(g)→Be2+(g)+e−;Be(g)→Be+(g)+e−
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B
Na(g)→Na+(g)+e−;Cl−(g)→Cl(g)+e−
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C
Ag(g)→Ag+(g)+e−;Au(g)→Au+(g)+e−
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D
O−(g)→O(g)+e−;S−(g)→S(g)+e−
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Solution
The correct options are CAg(g)→Ag+(g)+e−;Au(g)→Au+(g)+e− DO−(g)→O(g)+e−;S−(g)→S(g)+e− (A) For all elements, IE1<IE2<IE3
(B) The minimum value of IE for an element in periodic table (Na) is also greater than the maximum value of ΔHeg for an element in periodic table (Cl) (w.r.t. magnitude only).
(C) Due to poor shielding effect of 4f electrons, IE for Au>IE for Ag.
(D) ΔHeg for S>ΔHeg for oxygen because of small size of oxygen (w.r.t. magnitude only).