Term
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Definition
-Dissociates in water to give H30+
-Proton donor
-Electron-pair acceptor (nucleophile) |
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Term
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Definition
-Dissociates in water to give OH-
-Proton donor
-Electron-pair donor (nucleophile) |
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Term
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Definition
| The acid that results from protonation of a base. |
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Term
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Definition
| The base that results from loss of a proton from an acid. |
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Term
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Definition
| Bonding that occurs by the sharing of electrons in the region between two nuclei. |
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Term
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Definition
| A covalent bond that involves the sharing of one pair of electrons. |
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Term
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Definition
| A covalent bond that involves the sharing of two pairs of electrons. |
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Term
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Definition
| A covalent bond that involves the sharing of three pairs of electrons. |
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Term
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Definition
| A method of drawing curved arrows to keep track of electron movement from nucleophile to electrophile (or within a molecule) during the course of a reaction. |
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Term
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Definition
| Orbitals with identical energies. |
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Term
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Definition
| A measure of the polarity of a bond (or a molecule), proportional to the product of the charge separation times the bond length. |
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Term
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Definition
| The relative probability of finding an electron in a certain region of space. |
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Term
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Definition
| A measure of an element's ability to attract electrons. Elements with higher electronegativities attract electrons more strongly. |
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Term
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Definition
| An electron-pair acceptor (Lewis acid). |
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Term
| Electrostatic Potential Map (EPM) |
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Definition
| A computer-calculated molecular representation that uses colors to show the charge distribution in a molecule. In most cases, the EPM uses red to show electron-rich regions (most negative electrostatic potential) and blue or purple regions to show electron-poor regions (most positive electrostatic potential). The intermediate colors orange, yellow, and green show regions with intermediate electrostatic potentials. |
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Term
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Definition
| The ratios of atoms in a compound. |
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Term
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Definition
| A method for keeping track of charges, showing what charge would be on an atom in a particular Lewis structure. |
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Term
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Definition
| When there are two or more unfilled orbitals of the same energy (degenerate orbitals), the lowest-energy configuration places the electrons in different orbitals (with parallel spins) rather than paired in the same orbital. |
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Term
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Definition
| Bonding that occurs by the attraction of oppositely charged ions. Ionic bonding usually results in the formation of a large, three-dimensional crystal lattice. |
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Term
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Definition
| Atoms with the same number of protons but different numbers of neutrons; atoms of the same element but with different atomic masses. |
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Term
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Definition
| A structural formula that shows all valence electrons, with the bonds symbolized by dashes (-) or by pairs of dots, and nonbonding electrons symbolized by dots. |
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Term
| Line-Angle Formula (Skeletal structure, Stick figure) |
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Definition
| A shorthand structural formula with bonds represented by lines. Carbon atoms are implied wherever two lines meet or a line begins or bends. Atoms other than C and H are drawn in, but hydrogen atoms are now shown unless they are on an atom that is drawn. Each carbon atom is assumed to have enough hydrogens to give it four bonds. |
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Term
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Definition
| A pair of nonbonding electrons |
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Term
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Definition
| The number of atoms of each element in one molecule of a compound. The empirical formula simply gives the ratios of atoms of the different elements. For example. the molecular formula of glucose is C6H12O6. It's empirical formula is CH2O. Neither the molecular formula nor the empirical formula gives structural information. |
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Term
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Definition
| A region in an orbital with zero electron density. |
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Term
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Definition
| A flat (planar) region of space with zero electron density. |
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Term
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Definition
| Valence electrons that are not used for bonding. A pair of nonbonding electrons is often called a lone pair. |
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Term
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Definition
| An electron-pair donor (Lewis base). |
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Term
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Definition
| Atoms generally form bonding arrangements that give them filled shells of electrons (noble-gas configurations). For the second-row elements, this configuration has eight valence electrons. |
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Term
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Definition
| An allowed energy state for an electron bound to a nucleus; the probability function that defines the distribution of electron density in space. The Pauli exclusion principle states that up to two electrons can occupy each orbital if their spins are paired. |
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Term
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Definition
| The chemistry of carbon compounds; the study of compounds derived from living organisms and their natural products. |
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Term
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Definition
| a measure of the acidity of a solution, defined as the negative logarithm (base 10) of the H3O+ concentration: pH = -log[H3O+] |
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Term
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Definition
| A covalent bond in which electrons are shared unequally. A bond with equal sharing of electrons is called a nonpolar covalent bond. |
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Term
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Definition
| A molecule or ion for which two or more valid Lewis structures can be drawn, differing only in the placement of the valence electrons. These Lewis structures are called resonance forms or resonance structures. Individual resonance forms do no exist, but we can estimate their relative energies. The more important (lower-energy) structures are called major contributors, and the less important (higher-energy) structures are called minor contributors. When a charge is spread over two or more atoms by resonance, it is said to be delocalized and the molecule is said to be resonance stabilized. |
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Term
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Definition
| A complete structural formula (such as a Lewis structure) shows all the atoms and bonds in the molecule. A condensed structural formula shows each central atom along with the atoms bonded to it. A line-angle formula (sometimes called a skeletal structure or stick figure) assumes that there is a carbon atom wherever two lines meet or a line begins or ends. |
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Term
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Definition
| The number of bonds an atom usually forms. |
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Term
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Definition
| Those electrons that are in the outermost shell. |
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Term
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Definition
| The belief that synthesis of organic compounds require the presence of a "vital force." |
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