To identify the compound containing ionic, covalent, and coordinate bonds, we need to analyze the bonding in each option.

• Ionic bond: Formed by the complete transfer of electrons between a metal and a non-metal, resulting in electrostatic attraction between oppositely charged ions.
• Covalent bond: Formed by the sharing of electrons between two non-metal atoms.
• Coordinate bond (dative bond): A type of covalent bond where both shared electrons are contributed by only one of the participating atoms.

Let's analyze the bonding in NH₄Cl (Ammonium Chloride):

1. Ionic bond: NH₄Cl exists as an ionic compound, consisting of the ammonium cation (NH₄⁺) and the chloride anion (Cl⁻). The electrostatic attraction between NH₄⁺ and Cl⁻ constitutes the ionic bond.
2. Covalent bond: Within the ammonium ion (NH₄⁺), there are three N-H covalent bonds formed by the sharing of electrons between nitrogen and hydrogen atoms.
3. Coordinate bond: Also within the ammonium ion (NH₄⁺), the fourth N-H bond is a coordinate bond. The nitrogen atom (with a lone pair of electrons) donates both electrons to form a bond with a proton (H⁺), which has an empty orbital.

Thus, NH₄Cl contains all three types of bonds.

• A) Li₂CO₃ (Lithium Carbonate): Contains ionic bonds between Li⁺ and CO₃²⁻. Within the carbonate ion (CO₃²⁻), there are covalent bonds (C-O) and resonance structures involving double bonds, but no distinct coordinate bond in the typical sense.
• B) KCl (Potassium Chloride): Primarily an ionic compound, formed by the transfer of electrons from K to Cl, resulting in K⁺ and Cl⁻ ions. It does not contain covalent or coordinate bonds.
• D) HCN (Hydrogen Cyanide): Contains covalent bonds (H-C and C≡N). The triple bond in C≡N consists of one sigma and two pi bonds, all covalent. It does not contain ionic or coordinate bonds.

Correct Answer: (C)