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Matter, Metal and Compounds

MATTER IN OUR SURROUNDING ❖ It is the competition between

Matter is anything which has mass and molecular interaction energy and
occupies space. All solids, liquids, and thermal energy that decides whether
gases around us are made of matter. a given substance under given
Scientists believe that matter is made of conditions will be a solid, liquid, or
tiny particles that clump together. A gas.
substance is a pure kind of matter having ❖ Thermal or heat energy can convert
only one kind of constituent particle one state of matter into another
(atom or molecule). Water, iron, gold, state. Thus, a particular state of
copper, aluminium and oxygen are matter depends on both
examples of substances. All substances intermolecular force and the thermal
are matter, but all forms of matter are not energy that basically depends upon
substances. temperature.
Matter can ordinarily exist in three Solid: We are surrounded by
states—solid, liquid, and gas. These three innumerable solid objects. A piece of
states of matter have different wood, a stone, a pencil, a pen, and a
properties. Water exists in all the three computer all are examples of solid's. A
states namely steam or water vapour solid has a definite size and shape which
(gas), water at room temperature do not change on their own.
(liquid), and ice (solid). This is the only Liquid: Water is a liquid. Mustard oil and
substance that exists naturally in all the kerosene oil are other examples of
three states. liquids. Can you think of some more
Matter can be classified in many ways. examples? A liquid has a definite volume.
However, the following are the two main However, a liquid does not have a definite
ways of classifying the matter: shape. It takes the shape of its container.
A liquid can flow. You can pour a liquid or
1. By the physical state of matter as
spill it. Liquids have properties
a solid, liquid, or gas.
intermediate between solids and gases.
2. By the chemical composition of The intermolecular forces in liquids are
matter as an element, a weaker than solids but stronger than
compound, or a mixture. gases. In liquids, the constituent particles
We shall discuss these classifications do not occupy fixed position as in solids,
in the next section. but they have freedom of movement as
Classification of matter based on physical in gases.
states. Matter can ordinarily exist in three Gases: A gas occupies the entire volume
states-1. Solid, 2. Liquid and 3. Gas. of the container irrespective of its size. In
Water exists in all the three states gases, molecules move freely because
namely steam or water vapour (gas), the intermolecular forces are very weak
water at room temperature (liquid) and and are unable to keep the gas molecules
ice (solid). This is the only substance that together in bulk. We cannot see gases,
exists naturally in all the three states. but they are all around us. We can feel
❖ The characteristic properties of the presence of air when the wind blows.
different states of matter depend on The wind is moving air and is a mixture
intermolecular forces. The forces of many gases like oxygen, nitrogen,
holding molecules together are called argon, carbon dioxide, and others.
intermolecular forces. Intermolecular Plasma: The fourth state of matter is
forces try to keep molecules called plasma. This state contains jonised
together, but thermal energy always gas with super energetic and super
tries to keep them far apart. excited particle.

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Different Characteristics of the Three States of Matter

State Volume Density Shape Fluidity Corn- Inter-

of pressibility molecular
Matter Forces
Solid Fixed High Definite Does not Negligible Very
Shape flow strong
Liquid Fixed Lower It takes Flows Very small Weak
When the smoothly when
com- shape of compared
pared container to solid
to solid
Gas Has no Low Has no Flows Highly com- Very weak
Fixed definite smoothly pressible
Volume shape

Classification of Matter According to Mixture: These are obtained by mixing

Chemical Composition two or more substances in any
proportion.
Pure Substance Mixtures can be divided into two
Elements: A chemical element is a pure categories:
substance, and it consists of one type of 1. Homogenous Mixture: They
atom distinguished by its atomic number.
have uniform composition
Examples of some elements are: helium,
throughout like sugar solution, air,
carbon, iron, gold, silver, copper, true solutions.
aluminium, hydrogen, oxygen, etc.
2. Heterogeneous: They have non-
Elements are the building blocks of the
uniform composition like a mixture
Universe. In total, 118 elements have
of salt and sugar in unknown
been listed so far. Out of the total 118
concentration, colloidal solutions.
known elements, about 94 occur
naturally on earth, and the remaining
have been synthesized artificially by Colloidal Solution: These kinds of
nuclear reactions. solutions are heterogeneous in nature
and contain two phases, i.e., dispersed
Elements in Earth's Crust and Human phase and dispersed medium. They can
Body scatter light because of the presence of
large solute particles, i.e., they show
Compound: These contain more than
one kind of atoms. These cannot be
separated into constituent atoms by Tyndall effect and Brownian
simple physical methods. movement. (Blue colour of the sky is
Example: C6H12O6 (glucose), NaC1 also due to scattering of light by dust
(salt), SiO2 (silica). particles suspended in air).
❖ Colloidal solutions are purified by
Impure Substance dialysis.
A substance is said to be impure, if all the ❖ They are of following types on the basis
constituent particles of that substance of dispersed phase and dispersed
are not same in their chemical nature. medium.

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Type of Colloid Dispersed Dispersed Example

Phase Medium
Emulsion Liquid Liquid Milk
Aerosol Liquid Gas Fog clouds
Gel Liquid Solid Jelly, cheese
Aerosol (solid) Solid Gas Smoke, automobile
Sol Solid Liquid Milk of magnesia
Solid sol Solid Solid Coloured gemstone
Foam Gas Liquid Shaving cream
Foam Gas Solid Foam rubber

Separation of Mixture: Some important 2. Boiling Point: It is a temperature at

chemical and physical methods are which vapour pressure of a liquid
discussed further: becomes equal to atmospheric
1. Distillation: It is a method of pressure and at which a substance
separating mixtures based on converts from its liquid state to
difference in volatilities of gaseous state. Atmospheric pressure
compounds in a boiling liquid usually decreases with height;
mixture. hence, at high altitudes, the boiling
2. It is used to separate liquids having point of the water is less than 100°C.
very less difference in their boiling 3. Evaporation: It is the process of
points. For example, a mixture of conversion of a liquid into vapours at
acetone (329 K) and methyl alcohol any temperature below its boiling
(338 K). point. It increases with increase in
3. Crystallisation: It is used to surface area.
separate a mixture of inorganic 4. Condensation: It is the process of
solids with the help of a suitable conversion of gas into liquid. Solid,
solvent; their examples include liquid, and gases are interconvertible
separation of a mixture of sugar and by changing the condition of
salt by using ethyl alcohol. temperature and pressure.
4. Vacuum Distillation: It is also
known as distillation under reduced METAL AND THEIR COMPOUNDS
pressure. It is used to obtain glycerol hose elements which can donate
and H2O and to concentrate electrons and form cations are called
sugarcane juice in sugar industry. metals, like Na, Ca, and Mg.
5. Steam Distillation: It is used to
separate a steam volatile compound Physical Properties of Metals
from non-volatile or non-steam 1. Metals are good conductors of heat
volatile compounds. It is used to and electricity.
purify sandwood oil, aniline, 2. They are ductile in nature.
nitrobenzene, etc. 3. They have lustre.
6. Chromatography: It is the modern 4. They are solid at room temperature
technique used for separation and (only Hg Mercury is liquid in nature
purification of organic compounds. It at room temperature).
is used for the separation of coloured 5. They all have high values of boiling
pigments from a plant. point and melting point.
6. They all have high density (only
Properties of Matter sodium and potassium have low
1. Melting Point: It is a temperature density).
at which a substance converts from 7. Metals are sonorous in nature
its solid state to liquid state. After (means they produce sound).
adding impurities, the melting point 8. Metals have high tensile strength.
decreases.

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Chemical Properties of Metals ❖ Borex-sodium Tetra Borate Deca

1. Produce many compound after Hydrate (Na2B407.10H20): This is a
reaction with no-metals. white crystalline solid that is soluble
2. They form cation after losing an in water.
electron.
3. They produce metal oxide after MAGNESIUM
reaction with oxygen, and metal Symbol: Mg, Atomic Number—12, Mass
oxides are basic in nature. Number—24
4. They produce metal hydroxide after Physical and Chemical Properties:
adding water in them. The metal magnesium doesn't exist in
nature in free state, because it is highly
SODIUM reactive. This is a white and extremely
Symbol: Na, Atomic Number—11, Mass glazed metal like silver. The metal
Number—23 magnesium is malleable and ductile;
Sodium is a highly reactive metal in that's why it can easily be transformed
periodic table and found in Earths crust into a thin wire or ribbon.
(2.27% of total metals); sodium is a soft The boiling point and melting point of this
metal and can easily be cut with knife. metal is 650°C and 110°C.
Uses: The metal magnesium is used in
Occurrence and Extraction: Due to making flash light ribbon, in photography
highly reactive element, it does not exist and in fire crackers, in the composition of
freely in nature, but it is found in the form alloys, etc.
of ores of chloride, nitrate, carbonate, Alloys:
borate, etc. Magnalium—Mg + Al + Cu + Fe
Duralumin—Al + Cu + Mg
Physical and Chemical Properties: Elektron—Mg + Zn + Cu
Sodium is white like silver, but it is very
soft and light, so it can be cut through 1. Magnesia (MgO): The
knife and floats in water. Due to a highly magnesia4Mg0) is also called milk of
reactive nature, sodium is kept inside the magnesia, which is a white coloured
kerosene oil (K-oil). But sodium is soluble powder. This is slightly soluble in
in benzene and ether. water, it is fluorescent to the light and
Uses: As a reducing agent, in synthetic it is fused at a very high temperature;
reactions, and in making tetraethyl lead therefore, magnesia is used in layer
(anti-knocking) compound by the use of lining of blast furnace.
an alloy of sodium-lead.
2. Magnesium Sulphate (MgSO4):
This compound naturally occurs in the
Compounds of Sodium
form of epsomite in epsome, which
❖ Sodium Hydroxide (NaOH): The are abundantly found in hot water
compound NaOH is called caustic spring. This is a colourless crystalline
soda, which is used as a petroleum solid substance. This is frequently
purifier, in manufacturing of soaps, to used in cotton industry, in the
produce glazing in pulp paper, cotton manufacturing of soap, paint, etc.
cloth, etc., and in the production of This is also used as a catalyst with
the artificial silk. platinum in the manufacturing or
❖ Sodium Bicarbonate (NaHCO3): It is production of sulphuric acid (H2SO4).
also called edible soda, and breads 3. Magnesium Alva [Mg
get such exposer by an emergent gas (OH)2.MgCO3.3H2O]: This
CO2. compound is used in removing the
❖ Sodium Chloride (NaCI): This is called acidity from the human stomach and
common salt or ordinary salt, which is it is used as an antacid tablet.
prepared by the vaporization process
of sea water.

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ALUMINIUM is a good conductor of heat and

Symbol: Al, Atomic Number—12, Mass electricity, and it is malleable and ductile.
Number—24 Its melting point and boiling point are
Physical and Chemical Properties: 659.8°C and 2,200°C.
Aluminium doesn't occur in nature in free Uses: This metal (aluminium) and its
state but occurs in the forms of alloys are frequently used in aircrafts,
compounds like bauxite (Al 2O3.2H2O), motor vehicle industries. The cooking
Corundum (Al2O3), Diaspore (Al2O3.H2O). utensils are manufactured by the alloys of
Al is a white glazing metal like silver. This it and by the metal itself.

Alloys of Aluminium
Alloys Composition
Aluminium bronze Al + Cu
Magnelium Al + Mg + Cu + Fe
Nickelloy Al + Ni + Cu
Duralium Mn + Mg

Compounds of Aluminium The boiling point and melting point of

this metal are 851°C and 1439°C.
Aluminium Chloride (A1C13): This is Uses: This metal is used in removing
used as a catalyst in Friedel Craft reaction water which is present in small amounts
which occurs on an extensive level. This in alcoholic solution. It is also used in
is also used as a catalyst in the production removing elements like nitrogen, sulphur,
of Gasoline. It is also used in cracking of and oxygen. which are present in small
petroleum anhydrous AlC13. amounts during the process of metal
Potash Alum extraction.
[K2SO4.A1(SO4)3.24H2O]: This is a
double salt that appears as a colourless Compounds of Calcium
crystalline solid. This is also used in pulp- Calcium Oxide (CaO): This is also called
paper and leather industries, as an quick lime. This is basically a white
antiseptic and as a germicide after porous solid substance that reacts rapidly
shaving, as a germicide for purification of with water and calcium hydroxide is
water, etc. formed.
Aluminium Hydroxide [Al(OH)3]: This Calcium Hydroxide [Ca(OH)2]:
is a white amorphous powder insoluble in This is also called slaked lime, and it is
water, and it is a covalent compound. obtained by reacting quick lime (CaO)
This is used in making fire proof and with water.
water proof clothes; in the name of Calcium Chloride (CaC12): This
aluminium gel, it is used as a drying occurs in a very small amount in sea
agent, freshly precipitated Al(OH)3 water and ocean. It is basically a
absorbs colouring matter forming colourless, crystalline solid substance in
insoluble lakes. which each molecule has six crystals of
water.
CALCIUM Bleaching Powder [Ca(OCI)C1]:
Symbol: Ca, Atomic Number—20, Mass This is an oxychloride of calcium, and it is
Number—40 produced on large scale by Hasen
Physical and Chemical Properties: Clever's process. It is an extremely
This is a white metal like silver and it is temporary compound used in bleaching
soft when compared with the other action of paper and cloth or garment. This
metals but hard when compared with is also used as an insecticide or a
lead, whose relative density is 1.55. This germicide, as a water purifier, and as an
metal also exhibits the phenomenon of anti-infective agent.
malleability and ductility.

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Iron 2,450°C. It is a transition metal and

Symbol: Fe, Atomic Number—26, Mass ferromagnetic, and it is attracted by the
Number—56 magnet. Fe is a transition metal, and it
Physical and Chemical Properties doesn't occur in nature in free state, but
of Iron: Pure iron is like a silver white, it is found in the form of ore. In nature, it
soft, ductile, and malleable metal. The is also found abundantly in green
specific gravity of iron is 9.85, its melting vegetables and in the haemoglobin of the
point and boiling point are 1,533°C and blood.

Alloys of Iron

Steel Other Element Special Feature Uses

with Fe or Properties
Stainless Cr Very hard and Used in making cooking
steel strong, doesn't utensils, surgical instruments,
form rust. blades, etc.
Nickel Ni Very hard and Used in making axles,
Steel elastic, free from electric wire, aircraft, auto
rusting. Parts, etc.
Tungsten W Very hard and Used in making spring,
steel strong. magnets, saws, axles, and
cutting gools.

Compounds of Iron and garment. as an insecticide, as a

Ferrous Sulphate (FeSO4): The reducing agent in the laboratory.
hydrated ferrous sulphate is called green
vitriol (FeSO4.4H2O). This is a light green COPPER
crystalline solid highly soluble in water. Symbol: Cu, Atomic Number—29, Mass
Ferric Chloride (FeCI3): It is used Number—64
as a laboratory reagent in the production Physical and Chemical Properties:
of blood coagulating medicines. Mohr's This is a tough, reddish colour metal
Salt [FeSO4.(NH4)2SO4.6H201(CaC12): whose specific gravity is 8.95, and its
This is a green colour crystalline solid melting point and boiling point are
soluble in water but insoluble in alcohol. 1083°C and 2310°C. It is malleable and
This is used in volume synthesis, in ductile. This is a good conductor of heat
making blue ink, in colouration of leather, and electricity.

Alloys of Copper
Alloys Composition Uses

Brass Cu + Zn Used in making idols, household

utensils, etc.
German silver Cu+ Zn + Ni Used in making idols and utensils.
Bell metal Cu + Sn Used in making bells, utensils, idols,
coins, etc.
Delta metal Cu +, Zn Used in making propellers of ships, as
resistant of sea water.

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Compounds of Copper cyanide (KCN) and sodium aurocyanide

Cupric Sulphate (CuSO)4: This is the and potassium aurocyanide are formed.
main compound of copper, and it is also Uses of Gold: This is used in making
called blue vitriol (CuSO)4.5H2O. This is ornaments, coins, salt photograph of
basically a solid crystalline substance of gold, in electroplating, and in sugar
blue colour in water. A mixture of industries. Thin layers of gold are used in
CuSO4.5H2O and Ca(OH)2 is called pharmaceutical industries.
Bordeaux Mixture, and it is used as a
fungicide. Compounds of Gold
Cuprous Oxide (Cu2O): This is a red Auric Chloride (AuCl3): This is a green
colour solid substance, insoluble in water. powder insoluble in water, and, on
It is obtained as a red precipitate by heating, it explodes violently. That's why
heating CuSO4 with glucose and NaOH it is called fulminating gold. Thus, it is
solution. used as a detonator.
Rold Gold (Cu + Al): This is called
SILVER artificial form of gold, which resembles
Symbol: Ag, Atomic Number—47, Mass like gold, and it is used in making cheap
Number—108 ornaments.
Physical and Chemical Properties: Silver Nitrate (AgNO3): This is used
This is a white, shining, solid metallic as a laboratory reagent, in making hair
substance, malleable and ductile. This is dyes, in electroplating of silver
the best conductor of heat and electricity. compounds, in making special ink which
The relative density of it is 10.47, while is used by washerman in clothes marking,
its melting point and boiling point are and as a voter-marker on the finger of the
960°C and 1,955°C. hand.
Uses of Silver: Silver is used in
making ornaments, utensils, coins, silver PLATINUM
pt. alloy in filling of tooth cavities, silver Symbol: Pt, Atomic Number—78, Mass
plating, etc. Number—195
Uses of Platinum: This is used in
Compounds making ornaments, laboratory equipment
Silver Chloride (AgC1): This is called and devices, electrodes, alloys, and as a
Horn silver, which is frequently used in catalyst in Oswald's process.
making photochromic glass.
Silver Iodide (AgI): It is used in ZINC Symbol: Zn, Atomic Number—30,
producing artificial rains. Mass Number—65
Silver Nitrate (AgNO3): This is used as Physical and Chemical Properties:
a laboratory reagent in making hair dyes, This is a bluish white, hard, and brittle
in electroplating of silver compounds, in metallic substance. At a normal
making special ink which is used by temperature, it is neither malleable nor
washerman in clothes marking, and as a ductile. It is a good conductor of heat and
voter-marker on the finger of the hand. electricity.
GOLD The melting point, boiling point, and
Symbol: Au, Atomic Number—79, Mass specific density of the zinc are 419.5°C,
Number—197 907°C, and 7.1 kg/dm3 respectively.
Physical and Chemical Properties
of Gold: This is a golden, yellowish solid Uses of Zinc: This is used in the
substance insoluble in the acids like HCL, laboratory in the preparation of H2 gas;
HNO3, and H2SO4. But soluble in aqua it is also used in the galvanization of iron
regia and NaCN solution. It is the most sheets to protect iron from rusting,
malleable metal, ductile, and good buckets, boxes, and many household
conductor of heat and electricity. It articles are made from these sheets.
doesn't react with air but dissolves in
sodium cyanide (NaCN) and potassium

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Compounds of Zinc Physical and Chemical Properties of

Lead: Lead is a soft, bluish grey metal
Zinc Sulphate (ZnSO4): This is used in with a bright lustre, and it is used as a
textile industry for soaking cotton threads paper marker. It doesn't react with dry air
before spinning, in making preserver of but reacts with moist air and forms the
wood and hides, in manufacturing of layer of hydroxide first and then of
lithopone white pigment, and in Calico carbonate.
printing and dyes industries. It also reacts with Conc. H2SO4 in
Zinc Sulphide (ZnS): This occurs in which SO2 gas is emerged out. When/ it
nature in the form of zinc blende. It is a reacts with dil.HNO3,then nitric oxide is
white solid that is insoluble in water. This formed, while with conc. HNO3,/ HNO3,
exhibits the virtue of phosphorescence, NO2 gas is formed in the form of a
and, therefore, it is used in making brownish smoke.
phosphorescent screens. Uses of Lead: Lead is a very useful
Zinc Chloride (ZnCl2): Anhydrated metal, and it is used in making alloys,
zinc chloride compound acts as a water lead accumulators, lead shots (bullet)
absorber. The electroplating of ZnC12 is and coverings of electric cables, lead
done to protect the costly wooden chambers, lead pipes, lead-arsenic
furnitures from germs or insects. bullets, in nuclear research, etc.

MERCURY Compounds of Lead

Lead Dioxide (PbO2): It is used in
Symbol: Hg, Atomic Number—80, Mass
Match Industry for making ignition
Number—200
surface of match boxes, used for
Physical and Chemical Properties: preparation of KMnO4.
Mercury is a white, shining metal like Lead Acetate [Pb(CH3COO)2]: This
silver which occurs in the liquid state at is also called SUGAR OF LEAD, and it is
an ordinary temperature. a white crystalline sugar like substance
Uses of Mercury: Mercury is a very soluble in water, and its crystals are
useful liquid metal used in making sweet in taste.
mercury thermometer, barometer, and Lead Tetra Ethyl [Pb(C2H5)4]: It is
used as a contact liquid in electrical a colourless mobile liquid having a special
industrial preparation of vermillion. smell soluble in petrol.

Compounds of Mercury URANIUM

Mercurous Chloride (Hg2Cl2): This is Symbol: U, Atomic Number—92, Mass
also called calomel. It is a white, Number—238
crystalline powder which is insoluble in Physical and Chemical Properties:
water and dil. acids. This is a lustrous, white metal, and it is
malleable and too ductile but an impure
Mercuric Chloride (HgC12): This is
brittle metal. This is the most radioactive
also called corrosive sublimate which is a
element which occurs naturally. This is
deadly poison. This is a colourless,
paramagnetic and has a relative density.
crystalline solid, which is moderately
Uranium is also called metal of hope.
soluble in cold water but extremely
Melting point and Boiling point are
soluble in hot water.
19.05, 1850°C and 3500°C respectively.
Mercuric Sulphide (HgS): This is Isotopes of Uranium: There are
also called vermillion, which is a red three isotopes of uranium—92U234, 92U235,
colour solid crystalline substance. and 92U238. The most abundantly
occurring uranium in nature is 92U238
LEAD (99.28%), while 92U235 (0.71%) and
92U (0.006%) occur in very 92 small
234
Symbol: Pb, Atomic Number—82, Mass
Number—207 amounts. The isotope 92U235 is used in
nuclear (atomic) reactor as a nuclear fuel.

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NON-METALS 3. Ordinary Water (H2O): This is a

In modern periodic table, there are 22 compound whose pure form is
non-metals, in which there are 11 gases, neutral, and its pH is 7. Pure water is
1 liquid, and 10 solids. Bromine occurs in a bad conductor of electricity, but an
the state of liquid, while hydrogen, acidic water is a good conductor of
nitrogen, oxygen, chlorine, etc. are in electricity. At 4°C, the density of the
gaseous state. water is maximum and its volume is
minimum. The ordinary water
HYDROGEN transforms into ice at 0°C. The rainy
Symbol: H, Atomic Number—1, Mass water is the purest form of the water,
Number—1 and 97% parts of the entire water are
assumed to be confined in ocean
Uses of Hydrogen: This is used as a surroundings, while the rest 3% is
fuel (liquid hydrogen) in the rocket, in the only assumed to be confined in the
production of ammonia (NH3) by Haber's pure form. The conversion of water
process, in the manufacturing of into the ice and into the water vapour
vegetable ghee, in the production of are examples of physical changes.
Gasolene, in filling the balloons, etc.
Various forms of Hydrogen Types of Water
Nascent Hydrogen: In the process of Hard Water: Hard water is not good for
chemical reaction, a suddenly emerged drinking because its taste is not good,
hydrogen gas is called atomic hydrogen. and it is harmful for the health. In it
Isotopes of Hydrogen: There are chloride, sulphate and bicarbonate of
three isotopes of hydrogen—Protium calcium and magnesium salts are
(1H1), deuterium (1H2), and tritium (1H3). dissolved. Also, washing soap doesn't
1. Protium (1H1): It has equal atomic produce leather with hard water.
number and mass number, and it is Soft Water: Soft water is good for
equal to 1. drinking because its taste is good, and its
2. Deuterium (1H2): This is called is not harmful for the health. Washing
heavy hydrogen and it has atomic soap produces leather with soft water.
number = 1, mass number = 2. It was Hardness of Water: The hardness
invented by Urey Brickwedde and of water is of two types:
Murphy in 1931. It is used in
explaining the mechanism of organic 1. Permanent Hardness: The
reaction and as a bombarding particle existence of the hardness of water
of the nuclear reactions. due to the chloride and sulphate of
3. Tritium (1H3): Tritium (1H3) is a the Calcium and Magnesium salts is
rarely occurring isotope of hydrogen, called permanent hardness of water.
and it is a beta emitter and a The permanent hardness of water is
radioactive substance. Atomic removed by mixing sodium
number and mass number of it is 1 carbonate in it, and, sometimes, it is
and 3, respectively, while its half-life also removed by boiling the hard
period is 12.4 years. water by the means of distillation.
Compounds of Hydrogen and its 2. Temporary Hardness: The
Isotopes existence of the hardness of water
1. Heavy Water (D2O): The density of due to the bicarbonates of calcium
heavy water (D2O) is more than and magnesium salts is called
ordinary water (H2O). temporary hardness of water. The
2. Hydrogen Peroxide (H2O2): This is temporary hardness of water can be
a light bluish dense liquid without any removed by boiling it. If sodium
smell, and, due to presence of carbonate is mixed up to the water
Hydrogen bonding, it (H202) looks and boiled, then both permanent and
like an ordinary water (H20) and is an temporary types of hardness can be
associated liquid. removed.

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SILICON urea, in cleaning, in the production of

Symbol: Si, Atomic Number—14, Mass nitric acid (HNO3) by Oswald's process
Number—28 and in the production of sodium
Occurrence and uses of Silicon: carbonate (Na2CO3) by Solvay's process,
Silicon occurs in nature abundantly in the in the production of hydrogen, etc.
form of sand and stone but never found
in free state. This is a non-metallic PHOSPHORUS
element, which also exhibits the Symbol: P, Atomic Number—15, Mass
characteristic of allotropy. The hydride of Number—31
the silicon is called Silane. Occurrence and Extraction" of
Phosphorus: Phosphorus is a very
NITROGEN reactive non-metal and easily catches fire
Symbol: N, Atomic Number—7, Mass in air in nature and that's why phosphate.
Number—17 Animal bones contain nearly 58% calcium
Occurrence and uses of Nitrogen: phosphate, while it is found in small
Nitrogen is the main component of the amounts in blood and urine of the animals
atmospheric air, and, in the form of as well as in the plants. There are various
compound, it is also found as ammonia, ores of phosphorus existing in nature,
as ammonium compounds, and in nitrate and a few of them are phosphorite
forms. There are no allotropes of nitrogen [Ca3(PO4)2], chloraphite
like carbon, and, according to the [Ca3(PO4)2CaC12], and redonda
volume, it is 78% in atmospheric air. phosphate (A1PO4).
Nitrogen is also used in the electric
bulbs and thermometer for measuring the OXYGEN
high temperature. It is also used in the Symbol: O2 (molecule formula—O2)
artificial pregnancy of cows for which the Atomic Number—8, Mass Number—16
sperm of bull is kept in it. Element — P-block
Occurrence and Preparation of
Fixation of Nitrogen: The process of Oxygen Gas: Oxygen gas was firstly
transformation of atmospheric nitrogen invented by a Sweden based scientist
by the bacteria in the roots of useful Scheele in 1772. It is a colourless,
nitrogenous compounds is called fixation odourless gas, which is slightly heavier
of nitrogen. The fixation of nitrogen takes than atmospheric air. It reduces into a
place both naturally and artificially. deep blue liquid on cooling, it doesn't
Symbiotic Bacteria namely rhizobium burn itself but favours the process of
take part in the nitrogen fixation process combustion. A mixture of helium and
in the joints of the roots of the hydrogen gas is used in the artificial
leguminous plants. The process of inhalation. There are three isotopes of
transformation of nitrogenous oxygen—8O16, 8O17, and, 8O18.
compounds into nitrogen is called
denitrification. Such process is performed SULPHUR
by certain bacteria called denitrifying Symbol: S, Atomic Number—16, Mass
bacteria. Also, in the process of Number—32
denitrification, released nitrogen by its Allotropes of Sulphur:
compounds directly goes to the 1. Crystalline Allotropic Forms:
atmosphere. (a) Rhombic or Octahedral or a-
sulphur.
Compounds of Nitrogen (b) Prismatic or Monoclinic or 13-
Ammonia (NH3): Ammonia is sulphur.
manufactured at industrial level by
2. Non-crystalline Allotropic Forms:
Haber's process.
(a) Plastic sulphur
Liquefied ammonia is used in freezing
(b) White sulphur
ice in the refrigerators, ammonia is used
(c) Milky sulphur
in the production of ammonium salts and

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Compounds of Sulphur used as an external application of pain

1. Sulphur Dioxide (SO2): During reliever medicine of bone injuries. This is
volcanic eruption, the main gas which also used in the manufacturing of several
releases is sulphur dioxide, and it is a dyes and drugs, and in the preparation of
colourless, suffocating, and a gas of photographic paper, film, and plates.
bitter smell. This gas is also used as Iodine is also used as a stronger
an antichlor. It exhibits the property germicide (insecticide).
of bleaching action, but it is
temporary. The structure of SO2 is INERT GASES
angular. Helium (He): This is a light non-volatile
2. Sulphuric Acid (H2SO4): It is called gas, and it is the second largest element
chemical king of all the acids, and it is found in the universe. Helium is used in
also known as oil of vitriol. On the filling the tyres of the aircraft, and, due
industrial level, H2SO4 is to its lightness with comparison to air, it
manufactured by two processes- helps in uplifting the aircrafts to upward.
Contact process and Lead Chamber To obtain the weather related
process. information's or observations, helium
3. Hydrogen Sulphide (H2S): During gas-filled balloons are left in open sky,
volcanic eruption, hydrogen sulphide and relevant predictions and calculations
gas is also released in small amount. are made. The mixture of helium and
This is basically a colourless gas, oxygen is used by deep sea diver (sailor)
which is poisonous (toxic), and its on the behalf of air, because, at larger
smell is like rotten eggs. pressure, helium is less soluble than
nitrogen. The mixture of helium and
CHLORINE oxygen is also used in artificial breathing,
Symbol: Cl, Atomic Number—17, Mass specially to the patients suffering from
Number—35 asthma in hospitals. Liquid helium is used
Uses: The chemical substances like as a low temperature reagent in the
bleaching powder, chloroform, etc. are experiments occurring at a low temperature.
manufactured by chlorine. It is also used
as a drinking water purifier, as a Neon (Ne): This gas is frequently
germicide, in removing colours from the used in fluorescent bulbs and in glazing
garments and cloths, in whitening sugar, advertisement. This is also used in Neon
etc. It is also used in the production of lamp through which symbolic indication is
toxic gases like phosgene, mustard gas, given to the aircrafts pilot at the
etc. aerodrome or airport. Infact, this light of
the lamp extremely shines in the fog.
BROMINE Thus, neon is today used frequently in
Symbol: Br, Atomic Number—35, Mass discharge lamps and fluorescent bulbs,
Number—80 which are used frequently in the
Uses: In the production of salts of advertisement.
bromide, hypobromide, bromates etc. in
making toxic and weeping gases, in the Argon (Ar): This is the most
production of AgBr used in photography. abundantly occurring gas in the
It is also used as a reactant in organic atmosphere, and it is used in filling the
chemistry, in the production of KBr, which ordinary electric bulbs, because, in the
is used in the form of sleeping drugs and presence of this gas, filaments of the bulb
pain reliever. have a longer live and remain intact even
after the regular and longer use. This gas
IODINE is also used in high temperature
Symbol: I, Atomic Number—35 metallurgical operations and the
Uses: It is used as a tincture of iodine processes involve behind it or in creating
and iodoform in the form of antiseptic and vacuum (being evacuated) in the arch
analgesic. lodex (compound of iodine) is welding of the alloys.

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Xenon (Xe): This gas forms the Carbon atoms can form compounds by
maximum number of chemical combining with other carbon atoms as
compounds. well as atoms of other elements. Carbon
Redon (Rn): This is a radioactive has the unique property of forming long
element. This element is used in chains of carbon atoms. These long
Radiotherapy in the treatment of cancer. chains serve as a backbone on which
various groups can attach to give a large
variety of compounds.
CARBON
Carbon is the sixth most abundant Carbon can form bonds with atoms of
element in the universe. It can exist in other elements such as hydrogen (H),
the free state or in the form of its nitrogen (N), oxygen (O), sulphur (S),
compounds. It is the major chemical and halogens. It also has the property of
constituent of most organic matter. self-combination, i.e., bond formation
Carbon is the second most common with the other carbon atoms. Thus,
element in the human body after oxygen. carbon can form long chains of carbon
Carbon is present in coal, oil, and natural atoms. This unique property of forming
gas. long chains is known as catenation.

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