Column l Electronic configuration | Column ll Electron gain enthalpy/ \[\mathbf{kJ}\,\mathbf{mo}{{\mathbf{l}}^{\mathbf{-1}}}\] |
(1) \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\] | (a) ? 53 |
(2) \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{1}}\] | (b) ? 328 |
(3) \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}2{{p}^{5}}\] | (c) ? 141 |
(4) \[1{{s}^{2}}2{{s}^{2}}2{{p}^{4}}\] | (d) + 48 |
Answer:
(i - d)
Intert gases \[(2{{n}^{2}}n{{p}^{6}})\]
have positive electron gain enthalpy because addition of electron is not easily
possible.
(ii - a)
Alkali metals have very low
electron gain enthalpy.
(iii - b)
Halogens (chlorine) have very
large negative electron gain enthalpy.
(iv - c)
Oxygen has electron gain
enthalpy, next to (chlorine) halogens because oxygen is also an electron
deficient element.
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