Question

identify the type of bonding within each substance.

co(s)
covalent
metallic
ionic

cocl₂(s)
ionic
metallic
covalent

ccl₄(l)
metallic
covalent
ionic

Explanation:

• For \(Co(s)\): Metals like cobalt (\(Co\)) have metallic bonding. In metallic bonding, metal atoms lose their valence electrons, which form a "sea of electrons" that hold the positively - charged metal ions together.
• For \(CoCl_{2}(s)\): \(CoCl_{2}\) is an ionic compound. Cobalt (\(Co\)) is a metal and chlorine (\(Cl\)) is a non - metal. Ionic bonding occurs when there is a transfer of electrons from the metal (which forms a cation) to the non - metal (which forms an anion). The electrostatic attraction between the cations and anions holds the compound together.
• For \(CCl_{4}(l)\): Carbon (\(C\)) and chlorine (\(Cl\)) are both non - metals. In \(CCl_{4}\), atoms share electrons to achieve a stable electron configuration. This sharing of electrons is characteristic of covalent bonding.

Answer:

• \(Co(s)\): metallic
• \(CoCl_{2}(s)\): ionic
• \(CCl_{4}(l)\): covalent