Chemistry Unit 5

Chemical bond

mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

Ionic bond

A chemical bond that forms between cations and anions; atoms completely give up electrons to other atoms; usually nonmetals and metals

Ionic compound

positive and negative ions combined so charges are equal and ions form into a crystal lattice (like salt)

Lattice energy

energy required to form an ionic bond

Covalent bond

chemical bond that forms when atoms share one or more pairs of electrons

Nonpolar covalent bond

A covalent bond where electrons are shared equally and the electrical charge is balanced

Polar covalent bond

A covalent bond where the atoms have an unequal attraction for shared electrons because one atom attracts the electron more than the other

Electron sea

these valence electrons are free from any [particular atom and are only held collectively by the entire assemblage of atoms: electrons are free to move about

Ionic

forms between metals and nonmetals; melting and boiling points are very high; nonconductors in the solid phase; good conductors in the liquid phase; great conductors when dissolved in water; generally dissolve in water

Covalent

forms between nonmetals; melting and boiling points are very low; nonconductors in the solid phase; poor conductors in the liquid phase and when dissolved in water; nonpolar does not dissolve; polar does dissolve

Resonance structures

Lewis structures that represent different ways of combining atoms in molecules and ions

Resonance

refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure

Bond Energy

the energy required to break a covalent bond

Double Bond

Higher in energy and shorter in length than single bonds

Triple Bond

higher in energy and shorter in length than double bonds

Molecule

smallest unit of a covalently bonded substance