Question

Give examples of oxides that are neutral and acidic oxides.

Answer 1

Hint: Oxides are chemical compounds with one or more oxygen atoms combined with another element (example-$L{i}_{2}O$) . Oxides are binary compounds of oxygen with another element, example-$C{O}_2,S{O}_2,CaO,CO,ZnO,Ba{O}_2,H_{2}O$ etc. Oxides can be generated with multiple reactions.

Complete answer:
Oxides are called because here, oxygen is in combination with only one element. Based on their acid-base characteristics oxides are classified as acidic, basic, amphoteric and neutral:
$$1.$$ An oxide that combines with water to give an acid is termed as an acid oxide.
$2.$ The oxide that gives a base in water is known as basic oxide.
$3.$ An amphoteric solution is a substance that can chemically react as either acid or base.
$4.$ However, it is also possible for an oxide to be neither acidic nor basic, but is a neutral oxide.
There are different properties which help distinguish between the three types of oxide. The term anhydride (without water) refers to compounds that assimilate$H_{2}O$ to form either an acid or a base upon the addition of water.
Acidic oxide: Acidic oxide are the oxides of non-metals and these acid anhydride form acid with water.
$\bullet$ Sulfurous acid- $S{O}_2+H_{2}O\to H_{2}S{O}_3$
$\bullet$ Sulfuric acid- $S{O}_3+H_{2}O\to H_{2}S{O}_4$
$\bullet$ Carbonic acid- $C{O}_2+H_{2}O\to H_{2}C{O}_3$
Acidic oxides are known as acid anhydrides (example- sulfur dioxide is sulfurous anhydride and sulfur trioxide is sulfuric anhydride) and when combined with bases, they produce salts, example-$Cu(OH{)}_2\stackrel{\mathrm{\Delta }}{\to }CuO+H_{2}O$$4.$$4.$
$S{O}_2+2NaOH\to N{a}_{2}S{O}_3+H_{2}O$
Neutral oxide- Neutral oxide show neither basic nor acidic properties and hence do not form salts when reacted with acids and bases, example- carbon monoxide $(CO)$, nitrous oxide $(N_{2}O)$, nitric oxide $(NO)$, etc. are neutral oxides.
Preparation of Oxides:
$\bullet$ By direct heating of an element with oxygen:
$2Mg+O_2\stackrel{heat}{\to }2MgO$
$2Ca+O_2\stackrel{heat}{\to }2CaO$
$S+O_2\stackrel{heat}{\to }S{O}_2$
$P_4+O_2\stackrel{heat}{\to }2P_2{O}_5$
$\bullet$ By reaction of oxygen with compounds at higher temperature:
$1.$ sulfides are usually oxidized when heated with oxygen.
$2PbS+3O_2\stackrel{\mathrm{\Delta }}{\to }2PbO+2S{O}_2$
$2ZnS+3O_2\stackrel{\mathrm{\Delta }}{\to }2ZnO+2S{O}_2$
$2.$ When heated with oxygen, compounds contained carbon and hydrogen are oxidized.
$C_2{H}_{5}OH+3O_2\to 2C{O}_2+3H_{2}O$
$3.$ By thermal decomposition of certain compounds like hydroxides, carbonates. And nitrates
$CaC{O}_3\stackrel{\mathrm{\Delta }}{\to }CaO+C{O}_2$
$2Cu(N{O}_3{)}_2\stackrel{\mathrm{\Delta }}{\to }2CuO+4N{O}_2+O_2$
$Cu(OH{)}_2\stackrel{\mathrm{\Delta }}{\to }CuO+H_{2}O$
$$4.$$ By oxidation of some metals with nitric acid
$$2Cu+8HN{O}_3\stackrel{heat}{\to }2CuO+8N{O}_2+4H_{2}O+O_2$$
$$Sn+4HN{O}_3\stackrel{heat}{\to }Sn{O}_2+4N{O}_2+2H_{2}O$$
$$5.$$ By oxidation of some nonmetallic with nitric acid.
$$C+4HN{O}_3\to C{O}_2+4N{O}_2+2H_{2}O$$

Note:
The oxide of elements in a period becomes progressively more acidic as one goes from left to right in a period of the periodic table. Metal oxide on the left side of the periodic table produces a basic solution in water (example- $N{a}_{2}O$). Nonmetallic oxides on the right side of the table produce an acidic solution (example- $C{l}_{2}O$).