Valence electrons as dots

Ionic bonds

Result from electrostatic forces between ions of opposite charge, typically involving a metal and a nonmetal.

Covalent bonds

Formed by the sharing of electrons between two nonmetallic atoms.

Metallic bonds

Found in solid metals, where bonding electrons are free to move throughout the 3-dimensional structure.

Lewis electron dot symbols

A system of symbols that represent valence electrons surrounding the chemical symbol for an element.

Octet Rule

The tendency of atoms to prefer having eight electrons in their valence shell for stability.

Valence electrons

Electrons available for bonding that reside in the outermost shell of an atom.

Electron configuration

The distribution of electrons in an atom's electron shells.

Noble gases

Elements that have filled valence shells and do not readily form compounds.

Stable arrangement

When an atom is surrounded by eight electrons, achieving a full valence shell.

Chlorine (Cl) Lewis dot symbol

Constructed with seven dots surrounding the symbol, indicating its seven valence electrons.

Sodium (Na) Lewis dot symbol

Constructed with one dot surrounding the symbol, indicating its one valence electron.

CsF (cesium fluoride)

An ionic compound formed from the transfer of an electron from cesium to fluorine.

NaCl (table salt)

An ionic compound formed from Na+ and Cl- ions, resulting in a stable arrangement.

Bond formation

The process by which atoms share or transfer electrons to achieve stability.

Abegg's rule

States that the difference between maximum positive and negative valences of an element is frequently eight.

Hydrogen bond

A bond formed between atoms when their valence electrons pair up.

Exceptions to the octet rule

Molecules where one or more atoms contain fewer or more than eight electrons.