`text(Definition :)` A binary compound of oxygen with another element is called oxide.
`=>` Oxygen reacts with most of the elements of the periodic table to form oxides.
`=>` In many cases one element forms two or more oxides.
`=>` The oxides vary widely in their nature and properties.
`=>` Oxides can be simple (e.g., `color{red}(MgO, Al_2O_3)` ) or mixed (`color{red}(Pb_3O_4, Fe_3O_4)`).
`=>` Simple oxides can be classified on the basis of their acidic, basic or amphoteric character.
● An oxide that combines with water to give an acid is termed acidic oxide (e.g., `color{red}(SO_2, Cl_2O_7, CO_2, N_2O_5)` ). For example, `color{red}(SO_2)` combines with water to give `color{red}(H_2SO_3)`, an acid.
`color{red}(SO_2+H_2O → H_2SO_3)`
● As a general rule, only non-metal oxides are acidic but oxides of some metals in high oxidation state also have acidic character (e.g., `color{red}(Mn_2O_7, CrO_3, V_2O_5)`).
● The oxides which give a base with water are known as basic oxides (e.g., `color{red}(Na_2O, CaO, BaO)`). For example, `color{red}(CaO)` combines with water to give `color{red}(Ca(OH)_2)`, a base.
`color{red}(CaO+H_2O → Ca (OH)_2)`
● In general, metallic oxides are basic.
● Some metallic oxides exhibit a dual behaviour. They show characteristics of both acidic as well as basic oxides. Such oxides are known as amphoteric oxides. They react with acids as well as alkalies.
● There are some oxides which are neither acidic nor basic. Such oxides are known as neutral oxides. Examples of neutral oxides are `color{red}(CO, NO)` and `color{red}(N_2O)`. For example, `color{red}(Al_2O_3)` reacts with acids as well as alkalies.
`color{red}(Al_2O_3 (s) + 6HCl (aq) +9H_2O (l) → 2 [ Al (H_2O)_6]^(3+) (aq) +6Cl^(-) (aq))`
`color{red}(Al_2O_3 (s) +6NaOH(aq) +3H_2O (l) → 2Na_3 [Al (OH)_6] (aq))`
`text(Definition :)` A binary compound of oxygen with another element is called oxide.
`=>` Oxygen reacts with most of the elements of the periodic table to form oxides.
`=>` In many cases one element forms two or more oxides.
`=>` The oxides vary widely in their nature and properties.
`=>` Oxides can be simple (e.g., `color{red}(MgO, Al_2O_3)` ) or mixed (`color{red}(Pb_3O_4, Fe_3O_4)`).
`=>` Simple oxides can be classified on the basis of their acidic, basic or amphoteric character.
● An oxide that combines with water to give an acid is termed acidic oxide (e.g., `color{red}(SO_2, Cl_2O_7, CO_2, N_2O_5)` ). For example, `color{red}(SO_2)` combines with water to give `color{red}(H_2SO_3)`, an acid.
`color{red}(SO_2+H_2O → H_2SO_3)`
● As a general rule, only non-metal oxides are acidic but oxides of some metals in high oxidation state also have acidic character (e.g., `color{red}(Mn_2O_7, CrO_3, V_2O_5)`).
● The oxides which give a base with water are known as basic oxides (e.g., `color{red}(Na_2O, CaO, BaO)`). For example, `color{red}(CaO)` combines with water to give `color{red}(Ca(OH)_2)`, a base.
`color{red}(CaO+H_2O → Ca (OH)_2)`
● In general, metallic oxides are basic.
● Some metallic oxides exhibit a dual behaviour. They show characteristics of both acidic as well as basic oxides. Such oxides are known as amphoteric oxides. They react with acids as well as alkalies.
● There are some oxides which are neither acidic nor basic. Such oxides are known as neutral oxides. Examples of neutral oxides are `color{red}(CO, NO)` and `color{red}(N_2O)`. For example, `color{red}(Al_2O_3)` reacts with acids as well as alkalies.
`color{red}(Al_2O_3 (s) + 6HCl (aq) +9H_2O (l) → 2 [ Al (H_2O)_6]^(3+) (aq) +6Cl^(-) (aq))`
`color{red}(Al_2O_3 (s) +6NaOH(aq) +3H_2O (l) → 2Na_3 [Al (OH)_6] (aq))`