Chem Ch6

Bond energy

the energy required to break the bonds in 1 mol of a chemical compound

Chemical bond

the attractive force that holds atoms or ions together

Chemical Formula

A combination of chemical symbols and numbers to represent a substance

Covalent Bonding

a bond formed when atoms share one or more pairs of electrons

Dipole

a molecule or a part of a molecule that contains both positively and negatively charged regions

Ductility

the ability of a substance to be hammered thin or drawn out into a wire

Electron-dot notation

an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol

Formula unit

the collection of atoms corresponding to an ionic compound's formula such that the molar mass of the compound is the same as the mass of 1 mol of formula units

Hybrid orbitals

orbitals that have the properties to explain the geometry of chemical bonds between atoms

Hybridization

the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals; hybridization represents the mixing of higher and lower energy orbitals

Hydrogen bonding

The intermolecular force occurring when a hydrogen atoms that is bonded to a highly electronegative atom that is bonded to a highly electronegative atom of one molecule is attracted to two unshared electrons of another molecule

Ionic bonding

a force that attracts electrons from one atom to another, which transforms a neutral atom into an ion

Ionic compound

a compound composed of ions bound together by electrostatic attraction

Lattice energy

The energy associated with constructing a crystal lattice relative to the energy of all constituent atoms separated by infinite distances

Lewis structure

A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.

London dispersion forces

the intermolecular attraction resulting from the uneven distribution of electrons and the creation of temporary dipoles

Malleability

the ability of a substance to be hammered or beaten into thin sheets

Metallic Bonding

a bond formed by the attraction between positively charged metal ions and the electrons around them

Molecular Compound

a chemical compound whose simplest units are molecules

Molecular Formula

A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms.

Molecule

a group of atoms that are held together by chemical forces; a molecule is the smallest unit of matter that can exist by itself and retain all of a substance's chemical properties

Multiple Bonds

a bond in which the atoms share more than one pair of electrons, such as a double bond or a triple bond

Non polar covalent bonds

a covalent bond in which the bonding electrons are shared equally by the bonded atoms

Polar

describes a molecule in which the positive and negative charges are separated

Polar covalent bond

a covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom

Polyatomic ion

an ion made of two or more atoms

Resonance

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

Single bond

a covalent bond in which two atoms share one pair of electrons

Structural formula

a formula that indicates the location of the atoms, groups, or ions relative to one another in a molecule and that indicates the number and location of chemical bonds

VSEPR theory

a theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other