How do covalent bonds form between atoms?

Covalent bonds are formed through the sharing of pairs of electrons between non-metal atoms. In a covalent bond, each atom contributes at least one electron to the bond, allowing them to attain a full outer shell of electrons, which leads to increased stability. This sharing can occur in various ways, often resulting in the formation of molecules.

For example, in a water molecule (H₂O), each hydrogen atom shares one electron with the oxygen atom, allowing oxygen to achieve a stable electronic configuration. This process is characteristic of non-metal atoms, which tend to have similar electronegativities, making it energetically favorable to share electrons rather than transfer them.

The other options illustrate different bonding types. The transfer of electrons is typical of ionic bonding, where electrons are transferred from a metal to a non-metal. A lattice structure represents the arrangement of ions in ionic compounds, and the attraction of opposite charges pertains to ionic interactions as well. Thus, while these options describe valid bonding mechanisms, they do not apply to the formation of covalent bonds specifically.