Chapter 12 key terms

Bond (p. 351)

A force that holds groups of two or more atoms together and makes them function as a unit.

Bond Energy (p. 351)

The energy required to break a given chemical bond.

Ionic Bonding (p. 351)

A type of bonding that results from the attraction between oppositely charged ions.

Ionic Compound (p. 351)

A compound formed between a metal and a nonmetal involving ionic bonds.

Covalent Bonding (p. 351)

A type of bonding in which electrons are shared between atoms.

Polar Covalent Bond (p. 355)

A covalent bond in which electrons are not shared equally due to differences in electronegativity.

Electronegativity (p. 353)

The ability of an atom to attract shared electrons.

Dipole Moment (p. 355)

A measure of the separation of positive and negative charges in a molecule.

Lewis Structure (p. 361)

A diagram that represents the valence electrons of atoms in a molecule.

Duet Rule (p. 361)

The tendency of hydrogen and helium to form stable molecules when they have two electrons in their valence shell.

Octet Rule (p. 361)

The principle that atoms tend to form stable compounds in which they have eight valence electrons.

Bonding Pair (p. 361)

A pair of electrons shared between two atoms.

Lone Pairs / Unshared Pairs (p. 361)

A pair of valence electrons that are not involved in bonding.

Single Bond (p. 366)

A covalent bond involving one shared pair of electrons.

Double Bond (p. 366)

A covalent bond involving two shared pairs of electrons.

Triple Bond (p. 366)

A covalent bond involving three shared pairs of electrons.

Resonance (p. 366)

A phenomenon where more than one valid Lewis structure can be drawn for a molecule.

Resonance Structures (p. 366)

The different possible Lewis structures for a molecule that exhibit resonance.

Molecular Structure (p. 372)

The three-dimensional arrangement of atoms in a molecule.

Geometric Structure (p. 372)

The shape of a molecule determined by the arrangement of atoms.

Bond Angle (p. 372)

The angle between two bonds in a molecule.

Linear Structure (p. 372)

A molecular shape where atoms are arranged in a straight line.

Trigonal Planar Structure (p. 372)

A molecular shape where three atoms form a triangle around a central atom.

Tetrahedral Structure (p. 372)

A molecular shape where four atoms are positioned around a central atom in a tetrahedral arrangement.

Valence Shell Electron Pair Repulsion (VSEPR) Model (p. 373)

A model that predicts the shape of a molecule based on the repulsion between electron pairs.

Tetrahedral Arrangement (p. 373)

The spatial arrangement of four pairs of valence electrons around a central atom.

Trigonal Pyramid (p. 373)

A molecular shape where three atoms and one lone pair surround a central atom in a pyramid-like arrangement.