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| A mixture composed of two or more elements, at least one of which is a metal. |
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| An expression that indicates the number and type of atoms present in the smallest representative unit of a substance. |
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| The number of ions of opposite charge that surround each ion in a crystal. |
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| Electron Dot Structure (or Lewis Dot Diagram) |
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Definition
| A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the nucleus and the inner shell electrons. |
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| The lowest whole number ratio of ions in an ionic compound; in calcium fluoride, the ratio of calcium cations to fluoride anions is 1:2 and the formula unit is CaF2 |
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| A negative ion formed when a halogen atom gains an electron |
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| The electrostatic attraction that binds oppositely charge ions together. Typically ionic bonds from between a metal and a nonmetal or a metal and an anionic polyatomic ion. |
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| A compound composed of positive and negative charges. |
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| The force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions. |
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| Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons. |
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| An electron in the highest occupied energy level of an atom. |
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| The energy required to break the bond between two covalently bonded atoms. |
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| A molecular orbital that can be occupied by two electrons of a covalent bond. |
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| A bond formed by the sharing of electrons between atoms. These bonds are typically between nonmetal atoms. |
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| A covalent bond in which one atom contributes both bonding electrons. |
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| A molecule consisting of two and only two atoms. |
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Definition
| A molecule that has two poles, or regions with opposite charges. |
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| Dipole-Dipole Forces (or Dipole Interactions) |
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Definition
| Intermolecular forces that result from the attraction of oppositely charged regions of polar molecules. |
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Term
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Definition
| Weakest intermolecular forces that occur between two nonpolar molecules. |
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Definition
| A bond in which two atoms share two pairs of electrons. |
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Definition
| Attractive forces between covalently bonded molecules. This type of intermolecular force occurs when hydrogen is covalently bonded to a highly electronegative atom (like Fluorine or Oxygen). The hydrogen is then attracted to an unshared electron pair on an atom of a different molecule. |
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Definition
| A compound that is composed of covalently bonded molecules. |
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Definition
| A chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound. |
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| An orbital that applies to the entire molecule. |
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Definition
| A neutral group of atoms that is joined together by covalent bonds. |
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| A solid in which all of the atoms are covalently bonded to each other. |
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| A covalent bond in which the electrons are shared equally by the two atoms. |
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| A molecule that does not contain two oppositely charged regions. |
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Definition
| A covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms. |
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Definition
| A covalent bond between atoms in which the electrons are shared unequally. |
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Definition
| A molecule in which one side of the molecule is slightly positive and the opposite side is slightly negative. |
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Definition
| A tightly bound, covalently-bonded group of atoms that behaves as a unit and has a positive or negative charge. |
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Definition
| A convention for drawing molecules in which the atomic symbol stands for the nucleus and inner-shell electrons of an atom, dots represent unshared electrons, and dashes represent shared electron pairs. |
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Definition
| A bond formed when two atoms share one pair of electrons. |
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Definition
| A covalent bond in which two atoms share three pairs of electrons. |
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Definition
| A pair of valence electrons that is not shared between atoms of a molecule. |
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Definition
| Collectively, the two weakest intermolecular forces of attraction: London Dispersion Forces and Dipole-Dipole Forces. |
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| The Valence Shell Electron Pair Repulsion Theory, which states that because electrons repel each other, molecules will adjust their shapes so that valence electron pairs are as far apart as possible. |
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Definition
| A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei. |
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Definition
| A mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals. |
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Definition
| One of the two or more equally valid Lewis structures of a molecule or a polyatomic ion. |
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Definition
| An abbreviated form of a Lewis structure in which the shared pairs of electrons are shown as dashes, but no unshared pairs of electrons are shown. |
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