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Question

Which of the following trend is/are correct?

A
ClO2>SO2>CO2>P2O5 (acidic nature)
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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
C S>Se>Te>O (electron affinity)
D H3PO2>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.

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