Untitled Flashcards Set

Isoelectric

Having the same number of electrons per atom, ion, or molecule.

Ionic bond

The electrostatic attraction between oppositely charged ions.

Covalent bond

A chemical bond in which atoms share the bonding electrons.

Bonding electron pair

An electron pair that is involved in bonding, found in the space between two atoms.

Lewis structure

A diagram that represents the arrangement of covalent electrons and bonds in a molecule or polyatomic ion.

Duet rule

The observation that the complete outer shell of valence electrons is stable when hydrogen and period 2 metals are involved in bonding.

Octet rule

The observation that many atoms form the most stable substances when surrounded by 8 electrons in their valence shells.

Lone electron pair

A pair of valence electrons that is localized to a given atom but not involved in bonding.

Non-polar covalent bond

A covalent bond in which the electrons are shared equally between atoms.

Polar covalent bond

A covalent bond in which the electrons are not shared equally due to one atom attracting them more strongly.

Electronegativity

The ability of an atom in a molecule to attract shared electrons to itself.

Dipole

A separation of positive and negative charges in a region in space.

Polar molecule

A molecule that has a net dipole.

Non-polar molecule

A molecule that has only nonpolar bonds or a bond dipole sum of zero.

Valence electron theory

A theory stating that atomic orbitals overlap to form a new orbital with a pair of opposite spin electrons.

Hybrid orbital

An orbital that forms from the combination of at least two different orbitals.

Hybridization

The process of forming hybrid orbitals from the combination of at least two different orbitals.

Sigma bond

A bond formed when the lobes of two orbitals directly overlap end to end.

Pi bond

A bond formed when the sides of the lobes of two orbitals overlap.

Intramolecular bond

The chemical bond within a molecule.

Intermolecular force

A force that causes one molecule to interact with another molecule, occurring between molecules.

Van der Waals forces

Types of intermolecular forces including dipole-dipole forces, London dispersion forces, and hydrogen bonding.

Dipole-dipole force

The intermolecular force that occurs when the dipoles of polar molecules position their positive and negative ends nearby.

Hydrogen bond

The strong dipole-dipole force that occurs when a hydrogen atom bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine) is attracted to a partially negative atom on a nearby molecule.

London dispersion forces

Intermolecular forces that exist in non-polar molecules and increase as molecular mass increases.

Polarizability

The ability of a substance to form a dipolar charge distribution.

Surface tension

The resistance of a liquid to increase its surface area.

Capillary action

The spontaneous rising of a liquid in a narrow tube.

Viscosity

The measure of a liquid’s resistance to flow.

Composite material

A material composed of two or more distinct materials that remain separate in the solid phase.

Metallic crystal

A solid with closely packed atoms held together by electrostatic interactions and free-moving electrons.

Metallic bonding

The bonding that holds the nuclei and electrons of metals together.

Molecular crystal

A solid composed of individual molecules held together by intermolecular forces of attraction.

Covalent network crystal

A solid in which the atoms form covalent bonds in an interwoven network.

Semiconductor

A substance that conducts a slight electric current at room temperature but has increasing conductivity at higher temperatures.