Non metals and their compounds 2

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NON METALS AND THEIR COMPOUNDS-2
CARBON
Carbon is the non- metal with electronic configuration C= 2: 4, found in the group four and
second level. Carbon is insoluble. Carbon can be found on the rocks e.g. chalk – CaCO3 and
common in the organic food substance e.g. Glucose – C6H12O6.
Properties of carbon
1. Carbon monoxide
2. Carbon monoxide (CO)
When charcoal burns in the place where the air supply is very little (limited supply of air).
Carbon in the charcoal burn to form poisonous carbon monoxide gas which is very dangerous to
the body cells since it combines with haemoglobin(Hb) to form a stable compound called
carboxyhaemoglobin (HbCO), which prevent haemoglobin from combining with oxygen to
release it to the body cell or tissue. Lack of oxygen (suffocation) occurs then death may occur.
2C + O2 →2CO
1. (Carbon monoxide) which is poisonous
Preparation of carbon monoxide
The gas can be prepared from oxalic acid as shown below in the diagram.
Test for gas CO.
The gas burn with blue flame to form carbon dioxide gas
The physical properties
1. It is colorless.
2. It is insoluble.

3. It is odorless.
4. Neutral to litmus.
5. Less dense than air.
Commercial uses of carbon monoxide
6. Used in preparation of carbon dioxide gas.
7. Used as a reducing agent in the extraction of metals.
Chemical properties of carbon monoxide
8. Reaction with air.
9. React with metal oxides
CARBON DIOXIDE GAS (CO2)
Carbon dioxide (chemical formulaCO2) is a naturally occurring chemical compound
composed of 2 oxygen atoms each covalentlydouble bonded to a single carbon atom. It is
a gas at standard temperature and pressure and exists in Earth's atmosphere in this state,
as a trace gas at a concentration of 0.04 per cent (400 ppm) by volume, as of 2014. It is
the gas which extinguishes fire.
Preparation of carbon dioxide gas
10. From powdered chips of marble CaCo3 and dilute HCl
Consider the diagram below.

11. From Oxalic acid.
Test for carbon dioxide gas
The gas turns calcium hydroxide (lime water) to milky and also extinguishes fire.
Milky suspension
PHYSICAL PROPERTIES OF CARBON DIOXIDE GAS (CO2)
12. It is colorless
13. It is fairly soluble
14. It is slightly denser than air.
15. It is an acidic gas so turn blue litmus red.
16. It is odorless.
Chemical properties of carbon dioxide
17. Reacts with bases or alkali
18. Reacts with water.
19. Reacts with burning metals.
Burning metal continues to burn in the bottle containing CO2 gas because intense heat of
burning metal split/ decompose the carbon dioxide gas to form oxygen and carbon.
Oxygen gas formed supports combustion.

Support combustion.
Commercial uses of carbon dioxide gas
20. Use to make or synthesize cold drinks. Mainly because it brings a pleasant taste.
E.g. in Coca cola and Pepsi.
21. Used to extinguish fire because it doesn’t support combustion, carbon dioxide
keeps oxygen away from the fire source.
22. Used in the refrigerator for storage of food as it aids the formation of dry ice.
23. Used by plant for photosynthesis.
24. Used in the production of artificial rainfall but the rain is acidic.
2.
1. Carbon dioxide
1. Take any equal mass of diamond or graphite, and then burn it in air. The
products formed when masses are measured will give the same/ mass for
both allotropes.
2. Both allotropes when burnt in air produce carbon dioxide gas (CO2)
It burn in the air to form two oxides – one acidic oxide and other neutral
oxide.
Example
Allotropy and allotropes of carbon
Allotropy, this is the existence of an element with different or more or
various forms with different physical properties but same chemical
properties.

E.g. Carbon, sulphur, phosphorous etc can exist in allotropy form.
Allotropes – are different forms of the same element with different
physical properties but the same chemical properties.
Allotropes of carbon are;-
1. Diamond
2. Graphite
3. Amorphous carbon e.g. charcoal.
4. Graphite
Good conductor allotrope of carbon. This is the impure allotrope of carbon
which also good conductor of heat and electricity
Graphite can be seen within dry cell. Used as electrode since good
conductor of electricity.
Properties of graphite
5. It is a good conductor since it has mobile or free electrons.
6. Carbon atoms are arranged in the layers then held by weak
intermolecular forces.
7. Carbon atoms are equidistant to each other.
8. It is a very soft substance due to weak forces holds the atoms
across the layer.
9. It is opaque, black and greasy.
Diagram arrangement of graphite atom

Commercial uses of graphite
10. Used as the electrode. Because it is a good conductor of heat and
electricity as the metal does due to its free electrons
11. Used to make pencil. Because it’s soft so can write well on paper
12. Used as lubricant. Because it is greasy so reduce the frictional
force.
13. Used in re-enforcement of metal broken bones. Because it is hard.
14. Used for making crucible for storage of molten meal extracted.
Because it has high melting point so can’t melt easily.
15. Used to make dry cell. Because it is a good conductor of
electricity.
Graphite was considered to be a metal/ graphite is a good
conductor of electricity although is non-metal.
Graphite was considered to be a metal because electrons in graphite are
mobile or free, as those electrons present in the metal. At the same time
graphite can conduct electric current as a metal does.
Diamond is pure allotrope of carbon.
Diamond is the purest, hardest allotrope of the carbon. Diamond is a
valuable material found within the Earth`s surface.
Properties of diamonds
16. It has melting point.
17. It is the hardest substance known.
18. Its carbon atoms are not arranged in the layer
19. Its carbon atoms are held by the strong force of the attraction so
this makes electron to be more fixed.
Structure of diamond

Commercial uses of diamond
They include;
20. Used in the jeweler activities to make germ stones. Because it is
brilliant.
21. It is used in boring or drilling of the rock. Since it is the hardest
substance known.
22. It is used in glass cutting.
How to confirm the allotropes of the same element
How can we prove that diamond and graphite are allotropes of the same
element?
Properties of allotropes of the same elements
3. They have the same chemical properties/ composition.
E.g. diamond contains C and graphite contains C.
4. When burnt in air produce same product.
5. They have different physical properties.
Differences between graphite and diamond
Graphite Diamond
1.
Good conductor of heat and
electricity
Bad conductor of heat and
electricity

2.
Have lower melting point Have a higher melting point.
3.
It is black and opaque It is brilliant and transparent
4. Its carbon atoms are arranged
in the layers
Its carbon atoms are not arranged in
the layers.
5.
It has mobile or free electrons It has no mobile or free electrons
6. The carbon atoms are
equidistant
The carbon atoms are not
equidistant
Similarities between graphite and diamond
7. Both have carbon atoms
8. Both burns in air to form carbon dioxide gas
AMORPHOUS CARBON
This is an impure allotrope of carbon. This is the non crystalline allotrope of
carbon which is impure. A good example of amorphous carbon is charcoal and
soot.
Forms or amorphous carbon
They include
9. Charcoal
10. Coke
11. Soot
12. Charcoal
This is the solid material from incomplete combustion. Amorphous carbon
obtained from the destructive distillation of solid materials.
Types of charcoal

 Wood charcoal - obtained from raw material wood through process called
destructive distillation of wood.
 Animal charcoal- obtained from raw material bone through process called
destructive distillation of bone.
 Sugar charcoal- obtained from raw materials sugar through process called
destructive distillation of sugar.
Commercial uses of charcoal
16. Animal charcoal- purification of brown sugar to form white sugar since
can absorb the colored materials.
17. Sugar charcoal- used in chemical processing industry so act as mask of the
poisonous gas.
18. Wood charcoal- used in fuel for cooking, purification of water and
detoxification.
Preparation of oxides of carbon
Carbon has two oxides, namely:

Non metals and their compounds 2

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