Definition: Ionic bonding involves the transfer of electrons from metals to non-metals, resulting in the formation of charged ions.

Highlight: Metals tend to lose electrons (becoming cations) while non-metals gain electrons (becoming anions).

Example: Sodium (Na) and Fluorine (F) form an ionic bond where Na loses an electron to F, creating Na+ and F- ions.

Vocabulary: Electronegativity is the measure of an atom's ability to attract electrons in a chemical bond.

Definition: An ionic compound is a neutral substance formed by the combination of positively and negatively charged ions.

Example: The formation of sodium oxide (Na₂O) involves two sodium atoms each donating one electron to one oxygen atom.

Highlight: The total charge in an ionic compound must equal zero, requiring the correct ratio of cations to anions.

Vocabulary: Chemical formula represents the ratio of elements in an ionic compound using subscript numbers.

Definition: A chemical bond is a force of attraction that brings atoms together to form compounds or molecules.

Highlight: The driving force behind chemical bonding is atoms' tendency to achieve a stable octet configuration, similar to noble gases.

Example: Noble gases like Helium (He), Neon (Ne), and Argon (Ar) naturally have stable electron configurations.

Vocabulary: Valence electrons are the outermost electrons of an atom that participate in chemical bonding.