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B
Na>Si>Al>Mg(second I. P.)
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C
S>Se>Te>O(electron affinity)
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D
H3PO2>H3PO3>H3PO4(Ka1)
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Solution
The correct options are CS>Se>Te>O(electron affinity) DH3PO2>H3PO3>H3PO4(Ka1) More the electronegativity of the central atom more will be the acidic nature of the compound. Here CO2 will be less acidic than P2O5. So, option (a) is incorrect. Si+ has configuration of [Ne]3s23p1 Al+ has configuration of [Ne]3s2 Al+ has fully filled 3s subshell whereas Si+ has an electron in 3p subshell. So, the second ionisation energy of Si+ will be less than Al+. Hence, option (b) is also incorrect. E.A. of O is least in its group due to its small size and high electron density. Option (c) is correct.
Due to cross conjugation in (2); 1 is weaker base than 2 so H3PO2 is stronger acid than H3PO3, similarly relate H3PO4 for option (b) refer e− configuration & effective nuclear charge order is: Na>Al>Si>Mg.