Which of the following is/are correct order?

Acidic strength:

H C l O < H B r O < H I O

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Basic strength:

N a_{2} O > M g O > A l_{2} O_{3} > S i O_{2}

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Electron affinity:

I < B r < F < C l

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Ionization energy:

C l^{-} < C l < C l^{+}

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Solution

The correct option is D Ionization energy: $C l^{-} < C l < C l^{+}$
(a) The correct acidic order is:
$H C l O > H B r O > H I O$
With increase in electronegativity of the central atom, acidic nature of oxyacids increses.

(b) As we move from left to right, basic nature of the oxide decreases. So the correct order of basic strength is:
$N a_{2} O > M g O > A l_{2} O_{3} > S i O_{2}$

c) Electron affinity decreases down the group due to increase in the atomic radius down the group. However, $C l$ has greater electron affinity than $F$ , because, due to smaller size of $F$ atom, inter electronic repulsion in $F$ is considerably high.

(d) The energy required to remove the most loosely bound electron from an isolated gaseous atom is called the ionization energy. $C l^{+}$ has highest ionization energy since the effective nuclear charge on the outermost electron will be highest in this case as one electron is removed already and oppositely $C l^{-}$ will have lowest ionization energy.

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