Non-metals

The only non-metal that is in liquid form at room temperature is bromine.

Carbon and phosphorus are the examples of non-metals in solid form. Hydrogen is an example of a gaseous non-metallic element.

Carbon does not react with dilute hydrochloric acid because:

i. Carbon is a non-metal.

ii. Non-metals are electron acceptors.

iii. Hence, they are not able to remove the hydrogen present in acids.

iv. Thus, the effect of dilute hydrochloric acid on carbon is not observed.

Among the given oxides, N₂O is of neutral nature:

i. When non-metal combines with oxygen, it forms oxide.

ii. A neutral oxide is an oxide which neither reacts with an acid nor with a base.

iii. Nitrous oxide (N₂O) is an example of neutral oxide (an oxide which is neutral in nature)

iv. Other examples of neutral oxides are H₂O and CO (carbon monoxide).

Dihydrogen gas (H₂) is insoluble in water whereas carbon dioxide, sulphur dioxide and ammonia are soluble in water.

Sulphuric acid is called king of chemicals because:

i. It is a very important industrial chemical.

ii. It is widely used to prepare other chemicals.

iii. It is used in the production of fertilizers, paints, soaps, detergents, synthetic fibres etc.

Dihydrogen gas is combustible. It is very stable and it reacts with air without burning.

Haber’s process:

i. Production of ammonia gas is carried out by Haber’s process.

ii. In this process, dihydrogen and dinitrogen are mixed together.

iii. They are passed over iron (Fe) catalyst to form ammonia.

iv. The reaction takes place given below:

Note: A catalyst is a substance which can change the speed of reaction without itself undergoing any change.

(a-2) Extraction of sulphur is done by Frasch method

(b–4) Production of nitric acid is done by Ostwald’s method.

(c-1) Production of sulphuric acid is done by the Contact process

(d-3) Production of ammonia gas is done by Haber’s Process.

(a – 2)

Sulphuric acid is a strong dehydrating agent.

i. It means sulphuric acid has a property to remove water from any substance.

ii. For example: If sulphuric acid falls on sugar, paper, wood etc., it removes water from it and burns it.

iii. Hence, utmost care is taken while using it.

(b – 4)

Sulphur is used in the preparation of fire crackers.

(c – 1)

Sulphur is used in the bleaching of wooden pulp in the paper industry. Thus, it is a weak bleaching agent.

(d – 3)

Dihydrogen (H₂) gas is much lighter than air and also lighter than all other gases. So, it is the lightest gas among all.

(a-3)

The chemical formula of sulphurous acid is H₂SO₃.

The structure of sulphurous acid is:

(b-4)

The chemical formula of sulphuric acid is H₂SO₄.

The structure of sulphuric acid is:

(c-2)

Oleum is also known as fuming sulphuric acid. The chemical formula of oleum is H₂S₂O₇.

The structure of oleum is:

(d-1)

The chemical formula of phosphoric acid is H₃PO₄.

The structure of phosphoric acid is:

Two examples of non-metallic elements which are in solid form are:

i. Carbon

ii. Sulphur

Two examples of non-metallic elements which are in gaseous form are:

i. Hydrogen

ii. Oxygen

Note: Some other examples of non-metals in gaseous form are nitrogen, chlorine etc.

The gaseous mixture of carbon monoxide and dihydrogen gas is known as water gas.

Two substances which are used as promoters in manufacture of ammonia gas by Haber’s process are:

i. Aluminium oxide (Al₂O₃)

ii. Potassium oxide (K₂O)

They are added to increases the efficiency of the catalyst. Hence, they are called promoters.

The concentrated solution of ammonia is called liquor ammonia. The chemical formula of liquor ammonia is NH₄OH.

Some elements exist in two or more forms having different physical properties (different arrangement of atoms) and same chemical properties. This property of an element is called allotropy.

The allotropic forms of that element are called allotropes.

There are two allotropic forms of sulphur which are:

i. Rhombic sulphur- It is stable at temperature lower than 369K and has an octahedral structure.

ii. Monoclinic sulphur - It is stable at temperature higher than 369K and has a needle like structure.

The effect of litmus paper on aqueous solution of ammonia:

i. Dry ammonia gas does not show any effect on litmus paper.

ii. But aqueous solution turns red litmus paper into blue.

iii. This indicates that aqueous solution of ammonia shows basic nature.

i. P₄(s) + 5O₂(g) → P₄O₁₀(s)

It is a reaction in which non-metallic element combines with dioxygen gas to form oxide.

ii. SO₂(g) + H₂O(l) → H₂SO₃ (l)

This is a type of synthesis reaction. This reaction is used in the preparation of sulphurous acid

iii. P₄(s) + 6Cl₂(g) → 4PCl₃(g)

The above reaction is a type of synthesis reaction. This reaction is used in the preparation of phosphorus trichloride.

iv. O₂(g) + 2H₂(g) → 2H₂O (l)

It is a reaction in which non-metallic element reacts with dihydrogen gas to form stable hydride compounds.

v. Mg(s) + H₂O(g) → MgO (s) + H₂ (g)

It is a reaction in which a less active metal reacts with water to form dihydrogen gas. The other less active metals are zinc and iron.

vi. 3Fe(s) + 4H₂O(g) → Fe₃O₄(s) + 4H₂(g)

It is also a reaction in which a less active metal reacts with water to form dihydrogen gas.

vii. CO (g) + H₂O(g) → CO₂ (g) + H₂ (g)

This is a reaction in which mixture of water gas (CO₂ and H₂) is passed with water vapour to produce excess dihydrogen gas and to remove carbon monoxide.

viii. 3NO₂ (g) +H₂O(l) → 2HNO₃ (l) + NO(g)

The above reaction is a part of Ostwald process.

ix. S(s) +6HNO₃(aq) → H₂SO₄(aq) + 6NO₂(g) + 2H₂O(l)

It is a reaction in which sulphur reacts with nitric acid to form sulphuric acid, nitrogen dioxide and water.

x. SO₃(g) + H₂SO₄(aq) → H₂S₂O₇(l)

The above reaction is a type of synthesis reaction. This reaction is used in the preparation of oleum (H₂S₂O₇) which is also known as fuming sulphuric acid.

xi. C₁₂H₂₂O₁₁(s)+ Con H₂SO₄(l) → 12C (s) +11H₂O(l)

The above reaction is a type of dehydration reaction. The sulphuric acid acts as a dehydrating agent. It removes the water from sugar (C₁₂H₂₂O₁₁) and burn it.

xii. CaCO₃(s) + dil H₂SO₄(aq) → CaSO₄(aq) + CO₂(g) + H₂O(l)

The above reaction is a type of dehydration reaction. The sulphuric acid will act as a dehydrating agent. It produces calcium sulphate, carbon dioxide and water.

(i) SO₃(g) + H₂O(l) H₂SO₄(aq)

Sulphur trioxide gas reacts with water to form sulphuric acid with very corrosive fumes.

(ii) S(s) + O₂(g) → SO₂(g)

Sulphur reacts with dioxygen gas to form sulphur dioxide (non-metallic oxide). This oxide is acidic in nature.

(iii) CO₂ + H₂O(l) H₂CO₃ (aq)

Carbon dioxide reacts with water to form carbonic acid (H₂CO₃). This means carbon dioxide is an acidic oxide i.e., an oxide which is acidic in nature.

(iv) S(s) + H₂(g) → H₂S (g)

Sulphur (non-metallic element) reacts with dihydrogen gas to form hydrogen sulphide that is a stable hydride compound.

(v) 2Na(s) + 2H₂O (l) → 2NaOH(aq) + H₂(g)

When active metal like Na reacts with water, it produces sodium hydroxide and liberates dihydrogen gas.

(vi) Zn(s) + H₂O(g) → ZnO(s) + H₂(g)

Less active metal like Zn reacts with water vapour to form zinc oxide and dihydrogen gas.

(vii)

In this process, methane mixed with water over nickel catalyst to form a mixture of carbon monoxide and dihydrogen gas.

This mixture is called water gas.

(viii) CuO(s) + H₂(g) → Cu(s) + H₂O(g)

Dihydrogen gas is a good reducing agent. It reduces easily the metallic oxides.

(ix) H₂(g) + 2K(s) → 2KH(s)

When dihydrogen gas reacts with metal, it forms the metallic hydride of that element.

(x) MgSO₄(aq) + NH₄OH (aq) → Mg(OH)₂(s) + (NH₄)₂SO₄(aq)

Ammonium hydroxide (NH₄OH) forms magnesium hydroxide (Mg(OH)₂)

(xi).

SO₂ reacts with H₂S in the presence of Fe₂O₃ catalyst to form

sulphur. It is one of the methods for the extraction of sulphur.

(xii).

On reaction of sulphur dioxide gas with dioxygen gas in the presence of vanadium catalyst (V₂O₅), sulphur trioxide gas is formed.

(xiii) CuSO₄5H₂O(s) + con. H₂SO₄(l) → CuSO₄

Addition of sulphuric acid to copper sulphate, the water is removed. Because sulphuric acid is a dehydrating agent. It removes all the water present in the substance.

Physical properties of non-metallic elements are:

i. They are non-lustrous except iodine which is lustrous in appearance.

ii. They are brittle, hard or soft.

iii. They are poor conductors of electricity except graphite which is a good conductor of electricity.

iv. They combine with oxygen to form metallic oxides.

v. Metallic oxides are either acidic or neutral in nature.

Physical properties of dihydrogen gas are:

i. It is colourless, odourless and tasteless gas.

ii. It is insoluble in water.

iii. It is much lighter than air and also lighter than all other gases.

iv. Hence, it is the lightest gas.

v. It is a neutral gas.

Uses of dihydrogen gas are:

i. It is used in the production of ammonia in Haber’s process.

ii. It is used in welding of metals.

iii. It is used as fuel in rockets.

iv. It is also used as fuel cell for the production of electricity.

v. It is an important source of energy in future.

Physical properties of ammonia gas are:

i. It is a colourless gas.

ii. It is lighter gas than air.

iii. It gets completely dissolve in water this means it is highly soluble in water.

iv. It has a very unpleasant smell which can cause irritation to eyes and nose.

v. Aqueous solution of ammonia acts as a weak base.

Ostwald’s process:

i. Ammonia gas is used in the preparation of nitric acid by this method.

ii. First, ammonia and dioxygen gas react together over platinum catalyst to form nitric oxide (NO)

iii. Now, nitric oxide formed above combines with oxygen to form fumes of nitrogen dioxide (NO₂)

2NO + O₂→ 2NO₂

iv. The nitrogen dioxide reacts with water to form nitric acid.

NO₂ + H₂O → HNO₃

Nitric acid

Uses of ammonia gas:

i. It is used in the preparation of baking soda and washing soda.

ii. It is used in the preparation of nitric acid by Ostwald’s method.

iii. The important use of ammonia is that; it is used in the preparation of number of fertilizers.

iv. It is used to prepare dyes, explosives etc.

v. It is also used in the preparation of medicines like folic acid etc.

Physical properties of sulphur:

i. It is a yellow coloured solid substance.

ii. It has two allotropes which are rhombic sulphur and monoclinic sulphur.

iii. It is insoluble in water.

iv. But it is soluble in organic solvents like carbon disulphide, toluene, ethanol etc.

v. It has low melting point.

Reactionof sulphur with acids:

i. Sulphur reacts with hot concentrated sulphuric acid to form sulphur dioxide. The reaction is:

S + 2H₂SO₄→ 2H₂O + 3SO₂

ii. Sulphur reacts with concentrated nitric acid to form sulphuric acid. The reaction is:

S + 6HNO₃→ H₂SO₄→ 6NO₂ + 3H₂O

Reactionof sulphur with dihydrogen gas (H₂):

Sulphur reacts with dihydrogen gas to form hydrogen sulphide. The reaction is:

S + 2H₂→ 2H₂S

Reaction with carbon element:

Sulphur reacts carbon element to form carbon disulphide. The reaction is:

C+ 2S → CS₂

Uses of sulphur are:

i. It is used in the manufacture of sulphuric acid.

ii. It is used in the production of solvent like carbon disulphide (CS₂)

iii. It acts as an antiseptic for skin disease.

iv. It is used in the preparation of fire crackers.

v. It is also used in the preparation of insecticides.

Physical properties of sulphur dioxide gas are:

i. It is a colourless gas.

ii. It has unpleasant smell that causes coughing and suffocation.

iii. It is an oxide of non-metals that is sulphur.

iv. It is acidic in nature.

v. It is highly toxic and non-inflammable gas.

Uses of sulphur dioxide gas are:

i. It is used in the manufacture of sulphuric acid.

ii. It is a weak bleaching agent.

iii. It prevents the growth of bacteria.

iv. Hence, it is used as an antiseptic.

v. It is also used as a preservative in fruits juice, in jam and drying of fruits.

Uses of sulphuric acid:

i. It is used in identification of organic compounds in labs.

ii. It is used in the production of fertilizers.

iii. It is also used in the production of daily thig we use which are plastic, fibre, dyes, paints, detergents etc.

iv. It is used to prepare HCl, HBr from their salts.

v. It is also used to prepare explosives and drugs.

Difference between concentrated sulphuric acid and dilute sulphuric acid:

The hydrogen gas can be prepared by the reaction of metal with dilute acid or water.

Preparation of hydrogen gas from zinc metals with dilute acid:

i. In labs, pieces of zinc metals are taken in a flask.

ii. Dilute sulphuric acid or dilute hydrochloric acid is added to the flask.

iii. When the reaction takes place, a solution of zinc sulphate is formed and hydrogen gas is produced. The reaction is:

Zn + H₂SO₄→ ZnSO₄ + H₂

iv. The gas formed is collected in a jar by downward displacement of water.

v. Because H₂ is a gas lighter than air.

Industrial production of dihydrogen gas:

i. In industries, the production of gas is carried out from methane (natural gas).

ii. In this process, methane mixed with water over nickel catalyst to form a mixture of carbon monoxide and dihydrogen gas.

iii. This mixture is called water gas.

iv. By reaction of water gas again with water, excess dihydrogen gas is formed and carbon monoxide is removed.

CO + H₂O → CO₂ + H₂

v. To separate H₂ gas from this mixture, it is passed through water.

vi. This way it can be collected in gas jar.

Haber’s process:

i. Production of ammonia gas is carried out by Haber’s process:

ii. In this process, dihydrogen and dinitrogen are mixed together.

iii. They are passed over iron (Fe) catalyst to form ammonia.

iv. Two substances are used as promoters which are aluminium oxide (Al₂O₃) and potassium oxide (K₂O)

v. They are added to increases the efficiency of the catalyst. Hence, they are called promoters.

vi. By cooling the reaction mixture at temperature lower than 273K, ammonia can be separated from N₂ and H₂ gases.

vii. The reaction takes place given below:

Flow chartfor the manufacture of ammonia gas

Sulphur has two allotropes:

Rhombic Sulphur

i. It is stable at temperature lower than 369K.

ii. It possesses octahedral structure.

iii. It is insoluble in water but soluble to some extent in benzene and alcohol.

iv. It is quickly soluble in CS₂.

Monoclinic Sulphur

i. It is stable at temperature higher than 369K.

ii. It possesses needle-like structure.

iii. It is insoluble in water.

iv. It is soluble in CS₂.

Contact process:

i. In this process, first sulphur is burnt in air to form sulphur dioxide.

S + O₂→ SO₂

ii. Sulphur dioxide gas with excess air is passed over V₂O₅

catalyst so that sulphur trioxide is formed.

iii. When sulphur trioxide is dissolved in concentrated sulphuric acid, it forms fuming sulphuric acid or oleum.

SO₃ + H₂SO₄→ H₂S₂O₇

Oleum

iv. Oleum is diluted with water.

v. As a result, desired concentration of sulphuric acid can be obtained.

H₂S₂O₇ + H₂O → H₂SO₄

Chemical properties of dilute sulphuric acid:

i. When reacted with metal, dilute sulphuric acid produces metal sulphates and hydrogen gas. For examples:

ii. When dilute sulphuric acid reacts with oxides, hydroxides or carbonates of metal, it produces metal sulphates, CO₂ and water. For examples:

Oxide: ZnO + H₂SO₄→ ZnSO₄ + H₂O

Hydroxide: NaOH + H₂SO₄→ Na₂SO₄ +2H₂O

Carbonate: CaCO₃ + H₂SO₄→ CaSO₄ +H₂O + CO₂

iii. When dilute sulphuric acid reacts with sodium carbonate and sodium bicarbonate, it forms sodium sulphate and carbon dioxide.

Chemical properties of non-metallic elements are:

Reactionof metal with dioxygen gas:

Non-metallic elements combine with dioxygen to form oxides.

C + O₂→ CO₂

Carbon dioxide

S + O₂→ SO₂

Sulphur dioxide

i. CO₂ and SO₂ are acidic oxides.

ii. CO and H₂O are neutral oxides.

Reactionof non-metal with acid:

i. Non-metals are electron acceptors.

ii. Hence, they are not able to remove the hydrogen present in acids.

iii. Thus, the effect of dilute hydrochloric acid on carbon is not observed.

Reactionof non-metal with dihydrogen:

Non-metallic elements react with dihydrogen gas to form stable hydride compounds.

For examples:

N₂ + H₂→ 2NH₃

O₂ + 2H₂→ 2H₂O

C + 2H₂→ CH₄

chemical properties of dihydrogen gas are:

Reaction with dioxygen gas:

When dihydrogen gas reacts with dioxygen gas, it forms water

2H₂ + O₂→ 2H₂O

i. Dihydrogen gas forms an explosive mixture with dioxygen gas.

ii. A large amount of heat is produced by this reaction.

Reaction with Metal oxide:

i. Dihydrogen gas is a good reducing agent.

ii. It reduces easily the metallic oxides.

For example: CuO + H₂→ Cu + H₂O

Reaction with active metals:

Dihydrogen gas combines with active metals like Na, K, Ca and forms the metallic hydride of that metal.

H₂ + 2Na → 2NaH

H₂ + 2K → 2KH

H₂ + Ca → CaH₂

Frasch method:

i. Frasch method is used for the extraction of sulphur from the core of the earth.

ii. This method is based on the low melting point of sulphur.

iii. Three concentric pipes are passed below in the soil so that they touch the layer of the sulphur.

iv. Superheated water vapour is passed at 443K temperature in the soil through the outermost cylinder.

v. As a result, sulphur melts because of its low melting point.

vi. Then, air is passed through the innermost cylinder so that sulphur and water in the central cylinder come out on the surface and gets cooled.

vii. Sulphur is insoluble in water. Hence, it can easily separated from the solution.

Chemical properties of sulphur dioxide gas are:

Reaction with gas:

i. When sulphur dioxide gas is passed through the solution of sodium hydroxide, sodium sulphite is formed.

SO₂ + NaOH → Na₂SO₃ + H₂O

Sodium

sulphite

ii. When sulphur dioxide gas is passed through the lime water, lime water becomes milky and calcium sulphite is formed.

SO₂ + Ca(OH)₂→ CaSO₃ + H₂O

LimeCalcium

watersulphite

Reaction with dioxygen gas:

When sulphur dioxide gas is passed through dioxygen gas in the presence of V₂O₅ catalyst, sulphur trioxide is formed.

2SO₂ + O₂→ 2SO₃

Sulphur trioxide

Reaction with hydrogen sulphide gas (H₂S) :

When sulphur dioxide gas is passed through hydrogen sulphide gas, sulphur is formed.

2SO₂ + H₂S → 3S + 2H₂O

Sulphur