SS1 Chemistry Lesson Note on Carbon and its Compounds

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TOPICS: CARBON AND ITS COMPOUNDS

CONTENT:

1. CARBON, ALLOTROPES AND THEIR STRUCTURES,
2. PROPERTIES, DIFFERENCE BETWEEN DIAMOND AND GRAPHITE
3. CHEMICAL PROPERTIES OF CARBON
4. COAL AND TYPES OF COAL

PERIOD 1: CARBON, ALLOTROPES AND THEIR STRUCTURES

Carbon is a non -metal found in group 4 of the periodic table.  It occurs naturally as diamond and graphite. These physically different forms of the same chemical element are known as allotropes. Other elements that exist in different forms in their free states include tin, Sulphur and phosphorus.  Also, it occurs in an impure form as coal and in the combine state as petroleum, wood and natural gases.

Atomic structure of carbon

Carbon is the sixth element in the periodic table. the nucleus its atom it composed of six proton and six neutron and surrounded by six electrons; 2 in the first energy level (k-shell) and four in the 2^nd energy level (L-shell). its orbital configuration is 1S²2S²2P^2.Carbonatom has four valency electrons. Carbon atoms are able to catenate, i.e. join to one another by covalent bonds in a continuous fashion. The phenomenon is called catenation.

Allotropes of carbon

Allotropy is the existence of an element in the same physical state but indifferent forms. The various forms are called allotropes. Carbon exhibits allotropy. Other elements that also exhibit allotropy are sulphur, Tin, Oxygen and Phosphorus. The two crystalline allotropes of carbon are: Diamond and graphite. Charcoal is amorphous. allotrope of carbon.

DIAMOND

Structure and Bonding

In diamond, each carbon atom is at the center of a regular tetrahedron and covalently bonded to four other atoms in a strong compact fashion. The covalent linking between the atoms is continuous to produce a single infinite tightly locked 3-dimensional giant (macro) molecule, which has a network octahedral structure see the diagram below:

The rigidity of the structure is responsible for the hardness of diamond; it is the hardest known substance. Since the covalent bonds are strong and the molecule is compact, the melting point of diamond is very high.

PHYSICAL PROPERTIES OF DIAMOND

1. Pure diamond is hard, colourless and transparent.
2. Forms octahedral crystals with high refractive index.
3. It is very hard; it has a density of 3.5gcm^-3, and melting point of 3600⁰C.
4. It does not conduct electricity, because all the four valence electrons per carbon atom are used in bonding i.e.no mobile electrons.
5. It is insoluble in any solvent.

USES OF DIAMOND

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