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(a) Use the noble-gas notation and write the ground-state electronic configurations of the following ions:
(i) S2- (ii) Sn4+ (iii) Mn2+
(b) Write the equation representing the 2nd ionization energy
(c) The electron affinity of Cs is 45 kJ/mol. Write the equation for which this is the energy change.
(d) Each of the following oxides reacts with water to produce an acid or a base, depending on whether the oxide is an acidic or a basic oxide. Give the formula of the product of this reaction.
(i) Cl2O3 (ii) Na2O (iii) N2O5
1) S2- - [Ne] 3s2, 3p6
2) Sn4+ - 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10
OR [Kr] 4d10
3) Mn2+ - [Ar] 3d5
Co(g) -----> Co(g) + e- (first ionization)
Co+(g) -----> Co2+(g) + e- (second ionization)
Cs + 1e- -----> Cs- , H = 45 KJ/mol
Cl2O3 + H2O ----> 2HClO2 (acid)
Na2O + H2O ----> 2NaOH (base)
N2O5 + H2O ---> 2HNO3 (acid)
(a) Use the noble-gas notation and write the ground-state electronic configurations of the following ions: (i)...
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