Chemistry
(a) State whether the following statements are True or False.
Electrovalent compounds have low melting point.
Carbon tetrachloride will conduct electricity only in aqueous solution state.
(b) Give reason - Hydrogen chloride can be termed as a polar covalent compound.
Chemical Bonding
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Answer
(a)
False
Reason — Electrovalent compounds have a high melting point and boiling point because there exists a strong force of attraction between the oppositely charged ions, so a large amount of energy is required to break the strong bonding force between ions.False
Reason — Carbon tetrachloride (CCl4) is a liquid that does not conduct electricity because it is a non-polar covalent compound. In the case of CCl4, carbon atom shares electrons with four chlorine atoms. The electrons are shared equally between the atoms, and the molecule has no permanent dipole moment, meaning there is no separation of charge. Therefore, there are no ions present in the compound, and no free electrons to carry an electrical current.
(b) Chlorine exhibits a higher electronegativity than hydrogen, causing it to attract the shared pair of electrons towards itself in the bond. As a result, chlorine develops a slight negative charge and hydrogen develops a slight positive charge. Hence, the bond formed between hydrogen and chlorine is termed a polar covalent bond, and the compound is classified as a polar covalent compound.
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