A bond formed between a metal and a non-metal is called an ionic bond.
An ionic bond occurs when one atom donates an electron to another atom, leading to the formation of positively charged and negatively charged ions. Metals, which are typically found on the left side of the periodic table, tend to lose electrons easily and become positively charged cations. Non-metals, located on the right side of the periodic table, tend to gain electrons to achieve a full outer shell, becoming negatively charged anions.
This transfer of electrons creates an electrostatic attraction between the oppositely charged ions, resulting in the formation of an ionic compound. A common example of this is sodium chloride (NaCl), where sodium (a metal) donates an electron to chlorine (a non-metal), leading to the formation of a stable ionic compound.