Compare the properties of a metal and a non-metal on the basis of the following:
(b) Nature of oxides

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Solution

Property
Metals
Non-metals
Nature of oxides
Generally, they form basic oxides, and if soluble in water, form an alkaline solution.
Examples
$\underset{calcium}{2 Ca (s)} + \underset{gas}{\underset{oxygen}{O_{2} (g)}} \to \underset{Oxide}{\underset{calcium}{2 CaO (s)}}$
$\underset{oxide}{\underset{calcium}{2 CaO (s)}} + \underset{water}{2 H_{2} O (l)} \to \underset{hydroxide}{\underset{calcium}{2 Ca {(OH)}_{2} (aq)}}$ .
Exception: ${Cr}_{2} O_{3}$ is an acidic oxide. $ZnO$ , $PbO$ and ${Al}_{2} O_{3}$ are amphoteric oxides.
Generally, they form acidic oxides or neutral. When combined with water, they form acids.
For example they form acidic or neutral. When combined with water, they form acids.
Examples
$\underset{carbon dioxide}{{CO}_{2} (g)} + \underset{water}{H_{2} O (l)} \to \underset{carbonic acid}{H_{2} {CO}_{3} (aq)}$
$\underset{dinitrogen pentoxide}{N_{2} O_{5} (g)} + \underset{water}{H_{2} O (l)} \to \underset{nitric acid}{2 {HNO}_{3} (g})$ .
${CO}_{2}$ and $N_{2} O$ are neutral oxides. whereas $N_{2} O_{4}, {SO}_{2}$ etc are acidic in nature.

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Property	Metals	Non-metals
Nature of oxides	Generally, they form basic oxides, and if soluble in water, form an alkaline solution. Examples $\underset{calcium}{2 Ca (s)} + \underset{gas}{\underset{oxygen}{O_{2} (g)}} \to \underset{Oxide}{\underset{calcium}{2 CaO (s)}}$ $\underset{oxide}{\underset{calcium}{2 CaO (s)}} + \underset{water}{2 H_{2} O (l)} \to \underset{hydroxide}{\underset{calcium}{2 Ca {(OH)}_{2} (aq)}}$ . Exception: ${Cr}_{2} O_{3}$ is an acidic oxide. $ZnO$ , $PbO$ and ${Al}_{2} O_{3}$ are amphoteric oxides.	Generally, they form acidic oxides or neutral. When combined with water, they form acids. For example they form acidic or neutral. When combined with water, they form acids. Examples $\underset{carbon dioxide}{{CO}_{2} (g)} + \underset{water}{H_{2} O (l)} \to \underset{carbonic acid}{H_{2} {CO}_{3} (aq)}$ $\underset{dinitrogen pentoxide}{N_{2} O_{5} (g)} + \underset{water}{H_{2} O (l)} \to \underset{nitric acid}{2 {HNO}_{3} (g})$ . ${CO}_{2}$ and $N_{2} O$ are neutral oxides. whereas $N_{2} O_{4}, {SO}_{2}$ etc are acidic in nature.