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Definition
| a negatively charged ion; an ion that contains more electrons than protons |
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Term
| antibonding molecular orbital |
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Definition
| results when two orbitals of the opposite phase overlap |
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Term
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Definition
| the region of space where one or two electrons of an isolated atom are likely to be found |
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Term
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Definition
| rule for electron configurations that states orbitals should be filled starting with the lowest energy orbital first |
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Term
| bonding molecular orbital |
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Definition
| results when two orbitals of the same phase overlap; a molecular orbital that usually contains the bonding electrons |
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Term
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Definition
| a forumla that shows the carbon skeleton of a molecule with lines; the number of hydrogens used to complete each carbon's valence shell are assumed, but not depicted; other atoms (O, Cl, N, etc.) and hydrogens bonded to those atoms are written |
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Term
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Definition
| a positively charged ion; an ion that contains more protons than electrons |
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Term
| condensed structural formulas |
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Definition
| a depiction of a molecule where the hydrogens attached to a carbon are written immediately after that carbon, all covalent bonds are usually omitted but atoms are written in the order of bonding to depict connectivity |
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Term
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Definition
| different compound that have the same molecular formula, but differ in the sequence in which their atoms are bonded |
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Term
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Definition
| bond formed by the sharing of electrons by two atoms with similar electronegativities |
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Term
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Definition
| arrows used to show the movement of electrons pairs |
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Term
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Definition
| structual depiction in which atoms symbols are drawn and a line or "dash" represents pairs of bonding electrons; show connectivity but do not show geometry |
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Term
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Definition
| orbitals of equal energy; such as the three 2p orbitals |
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Term
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Definition
| negatively charged atomic particle; resides outside of the nucleus |
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Term
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Definition
| a measure of the ability of an atom to attract electrons |
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Term
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Definition
| the difference between the number of electrons assigned to an atom in a molecule and the number of electrons it has in its non-bonded state. |
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Term
| Heisenberg uncertainty principle |
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Definition
| a principle that states we cannot simultaneously know both the position and momentum of an electron |
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Term
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Definition
| when filling orbitals of equal energy, add one electron to each orbital with their spins unpaired until each orbital contains one electron. Then add additional electrons to fill the orbitals so that spins are paired. |
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Term
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Definition
| an attractive force between oppositely charged ions |
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Term
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Definition
| different compound that have the same molecular formula |
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Term
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Definition
| atoms that have the same atomic number, but differ in the number of neutrons in the nucleus |
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Term
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Definition
| a structural formula that displays bonded electrons between two atoms as a line, and nonbonding electrons as dots |
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Term
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Definition
| represents the region of space where one or two electrons of a molecule are likely to be found; the number of molecular orbitals always equals the number of atomic orbitals that were combined |
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Term
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Definition
| compounds whose atoms are joined primarily or exclusively by covalent bonds |
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Term
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Definition
| neutral atomic particle; resides in the nucleus of an atom |
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Term
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Definition
| the tendancy of an atom to achieve a configuration where its valence shell contains eight electrons |
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Term
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Definition
| region of space where the probability of finding an electron is high |
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Term
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Definition
| approach that involves combining individual atomic orbitals (s and p) to obtain new orbitals to use for bonding; new orbitals have, in varying proportions, the properties of the original orbitals taken separately |
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Term
| Pauli exclusion Principle |
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Definition
| a maximum of two electrons may be placed in each orbital, but only when the spins of the electrons are paired |
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Term
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Definition
| a bond formed when the electrons occupy a bonding pi molecular orbital; electron density of the pi bond is centered above and below the sigma bond axis; only occur when there are two or more bonds between the same two atoms |
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Term
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Definition
| a molecular orbital formed when parallel p orbitals on adjacent atoms overlap |
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Term
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Definition
| positively charged atomic particle; resides in the nucleus of an atom |
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Term
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Definition
| (resonance structure) lewis structures that differ from each other only in the position of electrons |
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Term
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Definition
| whenever a molecule can be depicted by two or more valid lewis structures that differ only in the placement of electrons |
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Term
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Definition
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Term
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Definition
| a single bond between two atoms; bond formed when eletrons occupy the bonding sigma orbital formed by the end-to-end overlap of atomic (or hybrid) orbitals on adjacent atoms; has circular symmetry when viewed along the bond axis |
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Term
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Definition
| molecular orbital formed by the end-on overlap of orbitals (or lobes of orbitals) on adjacent atoms |
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Term
| three-dimensional forumla |
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Definition
| depicts the correct geometry of an sp3 hybridized atom using dash and wedge bonds to show perspective |
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Term
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Definition
| the number of times an atom commonly bonds in a molecule to give a formal charge of 0 for that element |
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Term
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Definition
| electrons that reside in the valence shell; involved in bonding |
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Term
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Definition
| the outermost electron shell |
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