Which of the following compounds contain ionic bonds? Which contain covalent bonds? Which contain coordinate covalent bonds? (A compound may contain more than one type of bond.) a. BaCl₂

Verified step by step guidance

1. Identify the types of elements involved in the compound BaCl₂. Barium (Ba) is a metal, and chlorine (Cl) is a non-metal.
2. Recall that ionic bonds typically form between metals and non-metals due to the transfer of electrons from the metal to the non-metal.
3. Determine if there are any polyatomic ions or complex structures in BaCl₂ that might suggest the presence of coordinate covalent bonds. In this case, BaCl₂ is a simple binary compound without such structures.
4. Conclude that the primary type of bond in BaCl₂ is ionic, as it involves a metal and a non-metal.
5. Note that BaCl₂ does not contain covalent or coordinate covalent bonds, as these typically involve non-metals sharing electrons or a lone pair donation, respectively.

Key Concepts

Ionic Bonds

Ionic bonds are formed when electrons are transferred from one atom to another, resulting in the creation of charged ions. Typically, this occurs between metals and nonmetals, where the metal loses electrons to become a positively charged cation, and the nonmetal gains electrons to become a negatively charged anion. The electrostatic attraction between these oppositely charged ions holds the compound together.

Covalent Bonds

Covalent bonds occur when two atoms share one or more pairs of electrons, allowing each atom to attain a stable electron configuration. This type of bond usually forms between nonmetals and can involve single, double, or triple bonds depending on the number of shared electron pairs. The shared electrons create a strong bond that holds the atoms together in a molecule.

Coordinate Covalent Bonds

Coordinate covalent bonds, also known as dative bonds, occur when one atom donates both electrons to form a bond with another atom that has an empty orbital. This type of bond is common in complex ions and coordination compounds, where a central metal atom is surrounded by ligands. The key distinction is that in a coordinate bond, one atom provides both electrons for the bond, unlike in standard covalent bonds where each atom contributes one electron.