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}\xrightarrow{\Delta }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:
$2Mg + {O_2}\xrightarrow{{heat}}2MgO$
$2Ca + {O_2}\xrightarrow{{heat}}2CaO$
$S + {O_2}\xrightarrow{{heat}}S{O_2}$
${P_4} + {O_2}\xrightarrow{{heat}}2{P_2}{O_5}$
$ \bullet $ By reaction of oxygen with compounds at higher temperature:
$1.$ sulfides are usually oxidized when heated with oxygen.
$2PbS + 3{O_2}\xrightarrow{\Delta }2PbO + 2S{O_2}$
$2ZnS + 3{O_2}\xrightarrow{\Delta }2ZnO + 2S{O_2}$
$2.$ When heated with oxygen, compounds contained carbon and hydrogen are oxidized.
${C_2}{H_5}OH + 3{O_2} \to 2C{O_2} + 3{H_2}O$
$3.$ By thermal decomposition of certain compounds like hydroxides, carbonates. And nitrates
$CaC{O_3}\xrightarrow{\Delta }CaO + C{O_2}$
$2Cu{(N{O_3})_2}\xrightarrow{\Delta }2CuO + 4N{O_2} + {O_2}$
$Cu{(OH)_2}\xrightarrow{\Delta }CuO + {H_2}O$
\[4.\] By oxidation of some metals with nitric acid
\[2Cu + 8HN{O_3}\xrightarrow{{heat}}2CuO + 8N{O_2} + 4{H_2}O + {O_2}\]
\[Sn + 4HN{O_3}\xrightarrow{{heat}}Sn{O_2} + 4N{O_2} + 2{H_2}O\]
\[5.\] By oxidation of some nonmetallic with nitric acid.
\[C + 4HN{O_3} \to C{O_2} + 4N{O_2} + 2{H_2}O\]

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- $C{l_2}O$).