Chemical Bonding

Subatomic particles

Protons, neutrons, and electrons that make up an atom

Proton

Positive charge (+); located in the nucleus

Neutron

Neutral charge (0); located in the nucleus

Electron

Negative charge (−); located in the electron cloud

Cation

Positively charged ion formed when an atom loses electrons

Anion

Negatively charged ion formed when an atom gains electrons

Ions formed by metals

Cations

Ions formed by nonmetals

Anions

Octet rule

Atoms gain, lose, or share electrons to have 8 valence electrons

Why atoms follow the octet rule

To achieve a stable noble gas configuration

Ionic bond

Bond formed by transfer of electrons between a metal and a nonmetal

What holds ionic compounds together

Electrostatic attraction between opposite charges

When ionic compounds conduct electricity

When molten or dissolved in water

Why solid ionic compounds don’t conduct

Ions are fixed in place and cannot move

How to name ionic compounds

Cation name + anion name ending in -ide

Metallic bonding

Bonding between metals with a sea of electrons

Why metals conduct electricity

Electrons move freely

Why metals are malleable and ductile

Ion layers slide without breaking bonds

Why metals are shiny

Electrons reflect light

Covalent bond

Bond formed by sharing electrons between nonmetals

How covalent compounds are named

Using Greek prefixes (mono, di, tri, etc.)

Why “monosulfur dioxide” is incorrect

Mono is never used on the first element

Lewis dot structure

Dots represent valence electrons

Valence electrons

Outer shell electrons involved in bonding