| A | B |
|---|
| bond energy | The energy required to break a given chemical bond. |
| square planar structure | Structure with six electron pairs and the lone pairs at 180 degrees. |
| ionic compound | A compound that results when a metal reacts with a nonmetal to form a cation and an anion. |
| Coulomb's law | E = 2.31 x 10^-19 (Q1Q2/r) |
| bond length | The distance between the nuclei of the two atoms connected by a bond; the distance where the total energy of a diatomic molecule is minimal. |
| covalent bonding | A type of bonding in which electrons are shared by atoms. |
| polar covalent bond | A covalent bond in which the electrons are not shared equally because one atom attracts them more strongly than the other. |
| electronegativity | The tendency of an atom in a molecule to attract shared electrons to itself. |
| dipolar | A molecule that has a center of positive charge and a center of negative charge is said to be this. |
| dipole moment | A property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge. |
| isoelectronic ions | Ions containing the same number of electrons. |
| lattice energy | The energy change occurring when separated gaseous ions are packed together to form an ionic solid. |
| single bond | A bond in which one pair of electrons is shared by two atoms. |
| double bond | A bond in which two pairs of electrons are shared by two atoms. |
| triple bond | A bond in which three pairs of electrons are shared by two atoms. |
| localized electron (LE) model | A model which assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms. |
| lone pair | An electron pair that is localized on a given atom; an electron pair not involved in bonding. |
| bonding pair | An electron pair found in the space between two atoms. |
| Lewis structure | A diagram of a molecule showing show the valence electrons are arranged among the atoms in the molecule. |
| duet rule | Rule when two shared electrons are needed to form a stable molecule. |
| octet rule | The observation that atoms of nonmetals tend to form the most stable molecules when they are surrounded by eight electrons (to fill their valence orbitals). |
| resonance | A condition occurring when more than one valid Lewis structure can be written for a particular molecule. |
| resonance structure | Electron structures of a molecule that have more than one valid Lewis strucutre. Represented by a double arrow. |
| formal charge | The charge assigned to an atom in a molecule or polyatomic ion derived from a specific set of rules. |
| molecular structure | The three-dimensional arrangement of atoms in a molecule. |
| valence shell electron-pair repulsion (VSEPR) model | A model whose main postulate is that the structure around a given atom in a molecule is determined principally by monimizing electron-pair repulsions. |
| linear structure | Two pairs of electrons with 180 degree bond angles of a molecule. |
| trigonal planar structure | Thee pairs of electrons with 120 degree bond angles and a flat structure. |
| tetrahedral structure | Four pairs of electrons with 109.5 degree bond angles. |
| trigonal pyramid | Structure with a lone pair and three identical electron pairs and atoms. |
| trigonal bipyramid | Shape of the structure with 5 electron pairs that produces minimum repulsion. |
| octahedral structure | Structure formed by six electron pairs with 90 degree angle. |
| ionic bonding | The electrostatic attraction between oppositely charged ions. |
