Typically, ionic bonds are formed between atoms with a large difference in electronegativity, which is the ability of an atom to attract electrons. This difference in electronegativity causes one atom to strongly attract electrons from the other atom, resulting in the formation of positive and negative ions.

Atoms that typically form ionic bonds include:

1. Alkali metals (Group 1): These elements have a low electronegativity and readily lose their outermost electron to form positive ions (cations). Examples include lithium (Li), sodium (Na), and potassium (K).

2. Alkaline earth metals (Group 2): Similar to alkali metals, alkaline earth metals have a low electronegativity and easily lose their two outermost electrons to form positive ions. Examples include calcium (Ca), magnesium (Mg), and strontium (Sr).

3. Halogens (Group 17): Halogens have a high electronegativity and strongly attract electrons from other atoms. They readily gain one electron to achieve a stable electron configuration and form negative ions (anions). Examples include fluorine (F), chlorine (Cl), and bromine (Br).

4. Oxygen and Sulfur (Group 16): Oxygen and sulfur have a high electronegativity and can form negative ions by gaining electrons from more electropositive elements. They often form ionic bonds with metals.

In general, ionic bonds occur when there is a large electronegativity difference between a metal and a non-metal. The metal loses electrons to the non-metal, resulting in the formation of positively charged metal ions and negatively charged non-metal ions. These oppositely charged ions are then held together by electrostatic forces to form an ionic compound.