Select the correct order with respect to acidic nature of the given compounds.

A l_{2} O_{3} < I n_{2} O_{3} < T l_{2} O < B_{2} O_{3}

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T l_{2} O < I n_{2} O_{3} < A l_{2} O_{3} < B_{2} O_{3}

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A l_{2} O_{3} < B_{2} O_{3} < I n_{2} O_{3} < T l_{2} O

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T l_{2} O < A l_{2} O_{3} < B r_{2} O_{3} < I n_{2} O_{3}

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Solution

The correct option is B $T l_{2} O < I n_{2} O_{3} < A l_{2} O_{3} < B_{2} O_{3}$
As we move from top to bottom in a group, metallic character increases and so the acidic nature of the oxides decreases.
Therefore, $B_{2} O_{3}$ is acidic in nature, $A l_{2} O_{3}$ and $G a_{2} O_{3}$ are amphoteric in nature, whereas $I n_{2} O_{3}$ and $T l_{2} O$ are basic in nature.

Hence, the correct order with respect to acidic nature of compounds is as follows:
$T l_{2} O < I n_{2} O_{3} < A l_{2} O_{3} < B_{2} O_{3}$

Hence, option $B$ is correct.

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(a) Classify following oxides as neutral, acidic, basic or amphoteric:

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(b)Write suitable chemical equations to show their nature.

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