What type of bond is formed when one or more electrons are transferred from one atom to another?

The bond formed when one or more electrons are transferred from one atom to another is known as an ionic bond. This type of bond typically occurs between metals and non-metals. In an ionic bond, an atom (usually a metal) loses one or more electrons, becoming a positively charged ion (cation), while another atom (typically a non-metal) gains those electrons, becoming a negatively charged ion (anion). The electrostatic attraction between these oppositely charged ions creates the ionic bond.

Covalent bonds, on the other hand, involve the sharing of electrons between atoms rather than the transfer. Hydrogen bonds are a different type of interaction that occurs when hydrogen is covalently bonded to a highly electronegative atom, and they are relatively weaker than ionic and covalent bonds. Polar bonds refer to covalent bonds where electrons are shared unequally due to differences in electronegativity but do not involve complete transfer of electrons.

Understanding the nature of ionic bonds is crucial, as they play a significant role in the properties of various compounds, especially in relation to their solubility in water and electrical conductivity when dissolved.