(v) The number of single covalent bonds in C₂H₂ molecule are _____.

(vi) Melting points and boiling points of ionic compounds are generally _____ than those of covalent compounds.

Solution:

(v) Two: The carbon atom requires extra electrons to establish four bonds with hydrogen and other carbon atoms in the creation of C₂H₂. Each carbon’s 2s orbital combines with one of the 2p orbitals to generate two sp hybrid orbitals. Between the two carbon atoms in ethyne, there is a triple bond.

(vi) Higher: Electrostatic interactions between oppositely charged ions hold ionic compounds together. Ionic bonding is the term used to describe these forces. Due to the enormous number of ions in the ionic lattice, it takes a lot of energy to break the ionic bonds, hence ionic compounds have high melting and boiling temperatures.

The charge on the ions determines the strength of the ionic bonds. Higher-charged ions will have stronger forces between them, necessitating more energy to overcome these forces.