| A | B |
|---|
| Bond Energy | Energy required to break a chemical bond and form neutral atoms. |
| Bond Length | The average distance between two bonded atoms. |
| Chemical Bond | A link between atoms that results form mutual attractions. |
| Chemical Formula | Represents the relative numbers of atoms in each chemical compounds using symbols and subscripts. |
| Covalent Bond | Results through the sharing of two electrons between atoms. |
| Diatomic Molecule | A molecule that contains two atoms. |
| Dipole | Equal but opposite charges separated by a short distance. |
| Dipole-Dipole Forces | Attraction forces between polar molecules. |
| Double Bond | Is a covalent bond produced by the sharing of two pairs of electrons. |
| Ductility | The strength of a metals resistance to be pulled apart. |
| Formula Unit | The smallest amount of atoms which can be combined to make a chemical formula. |
| Hybrid Orbital | Are orbitals of equal energy produced by the combination of two or more orbitals of the same atom. |
| Hybridization | The mixing of two or more atomic orbitals to one orbital to give all orbitals equal energy. |
| Hydrogen Bond | The intermolecular forces between a hydrogen atom and an unshared pair of electrons of a highly electronegative atom. |
| Intermolecular Forces | The forces of attraction between molecules. |
| Ionic Bond | A bond between two atoms with positive and negative charges. |
| Ionic Compound | When positive and negative ions are combined so they have an equal charge. |
| Lattice Energy | The energy that is released when one mole of an ionic crystal is formed with a gaseous ion. |
| Lewis Structure | Shows the dots and shared electrons between atoms as dashes in an easy to read format. |
| London Dispersion Forces | Intermolecular forces resulting in the constant motion of electrons and the creation of instantaneous diploes and induced dipoles. |
| Malleability | The ability of a metal to be changed into a different shape. |
| Metallic Bond | Is a chemical bond resulting from the attraction between positive ions and surrounding mobile electrons. |
| Molecular Compound | A chemical compound whose simplest formula units are molecules. |
| Molecular Formula | Shows the types and numbers of atoms combined in a single molecule. |
| Molecule | Is the smallest unit of matter that can exist by itself and retain all the properties of the original substance. |
| Multiple Bond | Used when explaining double or triple bonds. |
| Nonpolar-Covalent Bond | A covalent bond where bonding energies are shared between the two bonded atoms equally. |
| Octet Rule | Chemical compounds tend to form so that each atom has eight electrons in the highest occupied energy level. |
| Polar | Molecules with an uneven charge at either end. |
| Polar-Covalent Bond | Is a covalent bond where bonding energies are unequally shared between the two bonded atoms. |
| Polyatomic Ion | A charged group of covalently bonded atoms as a result of excess or storage of electrons. |
| Single Bond | Is a covalent bond produced by the sharing of one pair of electrons. |
| Structural Formula | Indicates the kinds, number, arrangement, and bonds of the atoms in a molecule. |
| Triple Bond | Is a covalent bond produced by the sharing of three pairs of electrons. |
| Unshared Pair | Lone electrons that are the atoms own electrons. |
| VSEPR Theory | States that the repulsion between unshared electrons will attempt to be spaced as far apart as possible. |
