Question

Which of the following statements is true? I. Carbon forms covalent rather than ionic bonds. II. Carbon has an electronegativity value that is midway between that of the most metallic element and the most nonmetallic element. III. Carbon forms four bonds in virtually all its compounds. IV. A Si-Si bond is much stronger than a C-C bond. V. Relatively little heat is released when a C chain reacts and one bond replaces the other. Group of answer choices I, II, II, V I only II only III only IV only V only I and II I and III I and IV I and V II and III II and IV II and V III and IV III and V

Answer 1

Explanation:

Atomic number of carbon is 6 and its electronic distribution is 2, 4. As there are 4 valence electrons present in a carbon atom. Hence, it belongs to group 14 of the periodic table.

So, being a non-metal carbon atom tends to form covalent bonds. Also, the electronegativity value of carbon atom is mid-way between those of metals and non-metals.

In order to complete its octet, carbon atom tends to gain or share its 4 valence electrons. Therefore, it forms four bonds in all its compounds.

The Si-Si bond will be less stronger than C-C bond due to the larger size of silicon atom. As a result, there will be less overlapping between the silicon atoms due to which the bond formed will be weak in nature.

Whereas C-C bond is more stronger as a carbon atom is smaller in size as compared to silicon atom. As a result, more will be the overlapping between the carbon atoms. Hence, more stronger will be C-C bond than Si-Si bond.

As there will be covalent bonds present in a carbon chain and these bonds are weak as compared to ionic bonds. Hence, relatively little heat is released when a C chain reacts and one bond replaces the other.

Thus, we can conclude that out of the given options statements of I, II, III and V are true.