Chemistry Honors: Chemical Bonding, Molecular Geometry, and Intermolecular Forces

Vocabulary flashcards covering ionic, covalent, and metallic bonding, Lewis structures, VSEPR geometries, molecular polarity, and intermolecular forces based on chemistry honors lecture notes.

Ion

An atom with an unequal number of protons and electrons.

Chemical bonds

The forces that hold atoms together in compounds and molecules for greater stability.

Ionic bond

A chemical bond that forms when electrons are transferred from one atom to another, in which a metal transfers its valence electrons to nonmetal atoms.

Oxidation numbers

The variable charges of transition metals, represented by Roman numerals in parentheses.

Ionic compound naming convention

The name of the metal is listed first, followed by the nonmetal with the suffix -ide.

Covalent bond

A bond between two or more nonmetal atoms where valence electrons are shared to achieve a noble gas configuration.

Molecular compounds

Compounds whose atoms are bonded covalently.

Metallic bond

The force of attraction between positive metal ions and the valence electrons that are constantly moving around them.

Alloy

A mixture of two or more metals formed by melting a metal and dissolving other elements into it.

Central atom

The atom drawn in the center of a Lewis structure diagram.

HONK 1-2-3-4 rule

A bonding rule stating that hydrogen and halogens have $1$ bond, oxygen has $2$ bonds, nitrogen has $3$ bonds, and carbon has $4$ bonds.

Double bond

A covalent bond that consists of $4$ bonding electrons.

Triple bond

A covalent bond that consists of $6$ bonding electrons.

VSEPR theory

Stands for valence shell electrons pair repulsion.

Linear geometry

A geometry occurring when a central atom has $2$ electron groups, having a bond angle of $180^\circ$.

Trigonal planar geometry

A geometry occurring when a central atom has $3$ electron groups, with bonds at an angle of $120^\circ$.

Tetrahedral geometry

A geometry occurring when a central atom has $4$ electron groups, with a bond angle of $109.5^\circ$.

Trigonal bipyramidal geometry

A geometry occurring when a central atom has $5$ electron groups, bonding at either $120^\circ$ or $90^\circ$.

Octrahedral geometry

A geometry occurring when a central atom has $6$ electron groups bonded at $90^\circ$.

Polarity

An unequal sharing of electrons in covalent bonds.

Dipole moment

An event that occurs when a molecule is polar and has a partially positive side and a partially negative side, with the arrow pointing to the more electronegative elements.

Nonpolar molecules

Molecules with equal pulls where dipoles cancel out, having peripheral atoms of the same element.

Always-polar shapes

Molecular geometries that will always be polar due to lone pairs: trigonal pyramid, bent, V-shaped, seesaw, T-shape, and square pyramidal.

Intermolecular force (IMF)

Attractive forces that exist between neighboring molecules.

Intramolecular forces

Forces that hold atoms together in a single compound or molecule.

Relative bond and force strengths

The relative strength ranking from greatest to weakest: metallic bond, ionic bond, polar covalent bond, nonpolar covalent bond, and intermolecular forces (IMFs).

Ion-dipole force

An interaction between an ion and the charge of the end of a dipole.

Hydrogen bond

A type of IMF (not a real chemical bond) that occurs when hydrogen is covalently bonded to a highly electronegative atom, nitrogen.

Dipole-dipole force

A type of intermolecular force (IMF) that occurs between polar molecules.

London dispersion force (LDF)

The only type of intermolecular force (IMF) present in nonpolar molecules.