Complete the exercises below. Identify the following hydrides as ionic, metallic, or molecular: a. B₂H₆, b. RbH, c. Th₄H₁.₅.

Chemical bonds can be classified into three main types: ionic, metallic, and covalent (molecular). Ionic bonds form between metals and nonmetals through the transfer of electrons, resulting in charged ions. Metallic bonds occur between metal atoms, characterized by a 'sea of electrons' that allows for conductivity and malleability. Covalent bonds, or molecular bonds, involve the sharing of electrons between nonmetals.

Hydrides are compounds formed between hydrogen and other elements. They can be classified based on the type of bonding present. Ionic hydrides, like RbH, consist of hydrogen anions and metal cations, while molecular hydrides, such as B₂H₆, involve covalent bonding between hydrogen and nonmetals. Understanding the nature of the elements involved helps in determining the type of hydride.

The properties of elements, including their tendency to form ionic, metallic, or molecular compounds, are influenced by their position in the periodic table. Metals, typically found on the left side, tend to lose electrons and form ionic bonds, while nonmetals, located on the right, often gain electrons or share them, leading to covalent bonds. Transition metals can exhibit metallic bonding due to their unique electron configurations.