Question

Read the questions and answer any 4 out of 5

1. Two allotropic forms of carbon which are crystalline in nature, are

diamond and graphite. They differ physically but chemically they are

similar. Diamond is the hardest crystalline form of carbon. In

diamond, each carbon atom is linked to four other carbon atoms by

covalent bonds. In graphite, each carbon atom is linked to three other

carbon atoms by covalent bond. Graphite is relatively soft and greasy.

It is also a good conductor of electricity. The C — C bond length in

graphite is 141.5 pm while in diamond it is 154 pm.

I. Which of the following is a good conductor of heat and electricity?

II. Graphite is a good conductor of electricity because ?

III. Which binding forces is present in the structure of diamond?

Or

IV. Diamond is not a good conductor of electricity .Give reason​

Answer 1

Answer:

1.graphite is a good conductor of heat and electricity.

2. Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised 'sea' of electrons loosely bonding the layers together. These delocalised electrons can all move along together – making graphite a good electrical conductor.

3.covalant bond

4. each carbon atom is covalently bonded with other carbon atoms. So the four outermost electrons, four carbon atoms, are engaged or trapped in the covalent bonds which means that there are no free electrons. ... So diamond is a bad conductor of electricity.