Chem Ch. 8

Coordinate covalent bond

a covalent bond in which one atom contributes both bonding electrons.

Dispersion force

interaction caused by the motion of electrons.

Double covalent bond

a covalent bond involving two pairs of electrons ; each atom donates one pair of electrons to the bond.

Hybridization

the mixing of several atomic orbitals to form the same number of equivalent hybrid orbitals.

Hydrogen bond

force that occurs when a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared pair of electrons in the same or a nearby molecule.

Molecular compound

an electrically neutral group of atoms joined together by covalent bonds.

Molecular formula

shows the kinds and numbers present in a molecule of a compound.

Network solid

a substance in which all of the atoms are covalently bonded to each other.

Nonpolar covalent bond

a covalent bond formed by the equal sharing of bonding electrons by two atoms.

Polar covalent bond

a covalent bond formed between two different atoms in which the bonding electrons are shared unequally.

Polar molecule

a molecule in which one end is slightly negative and the other end is slightly positive.

Resonance structures

two or more valid electron dot formulas that can be written for the same molecule.

Single covalent bond

a covalent bond in which one pair of electrons is shared between two atoms.

Structural formula

a chemical formula that shows the arrangement of atoms in molecules and polyatomic ions.

Triple covalent bond

a covalent bond in which three pairs of electrons are shared by two bonded atoms.

Van der Waals forces

the weakest attractions that exist between molecules.

VSEPR theory

because electron pairs repel