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Addition Compounds
A molecule formed by the joining of two simpler molecules through formation of a covalent bond
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Bond Energy
The energy needed to break one mole of a particular bond to give electrically neutral fragments. Increases and bond length decreases.
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Bond Length
The distance between two nuclei that are held together by a chemical bond.
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Bond Order
# of bonding pairs of e- divided by the # of stoms bonded to central atom
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Carboxylic Acid
An organic compound whose molecules have the carboxyl group —CO 2H
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Contributing Structures
One of a set of two or more Lewis structures used in applying the theory of resonance to the structure of a compound. A resonance structure.
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Coordinate Covalent Bond
A covalent bond in which both electrons originated from one of the joined atoms, but otherwise like a covalent bond in all respects.
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Covalent Bond
A chemical bond that results when atoms share electron pairs EN < 1.7
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Dipole Moment
The product of the sizes of the partial charges in a dipole multiplied by the distance between them; a measure of the polarity of a molecule.
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Double Bond
A covalent bond formed by sharing two pairs of electrons.
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Electric Dipole
Two poles of electric charge separated by a distance
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Electronegativity
The relative ability of an atom to attract electron density toward itself when joined to another atom by a covalent bond.
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Formal Charge
The apparent charge on an atom in a molecule or polyatomic ion as calculated by a set of rules.
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Ionic Bond
The attractions between ions that hold them together in ionic compounds.
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Ionic Character
The extent to which a covalent bond has a dipole moment and is polarized.
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Lattice Energy
Energy released by the imaginary process in which isolated ions come together to form a crystal of an ionic compound.
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Lewis Formula
A structural formula drawn with Lewis symbols and that uses dots and dashes to show the valence electrons and shared pairs of electrons.
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Nonpolar Covalent Bond
A covalent bond in which the electron pair(s) are shared equally by the two atoms. EN = 0
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Octet of Electron
Eight electrons in the valence shell of an atom.
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Octet Rule
An atom tends to gain or lose electrons until its outer shell has eight electrons.
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Partial Charges
Charges at opposite ends of a dipole that are fractions of full 1+ or 1- charges
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Polar Covalent Bonds
A covalent bond in which more than half of the bond's negative charge is concentrated around one of the two atoms. EN < 1.7
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Polar Molecule
A molecule in which individual bond polarities do not cancel and in which, therefore, the centers of density of negative and positive charges do not coincide
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Reactivity
A description of the tendency for a substance to undergo reaction. For a metal, it is the tendency to undergo oxidation.
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Resonance
- A concept in which the actual structure of a molecule or polyatomic ion
- is represented as a composite or average of two or more Lewis
- structures, which are called the resonance or contributing structures
- (and none of which has real existence)
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Resonance Energy
The difference in energy between a substance and its principal resonance (contributing) structure.
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Resonance Hybrid
The actual structure of a molecule or polyatomic ion taken as a composite or average of the resonance or contributing structures.
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Resonance Structure
A Lewis structure that contributes to the hybrid structure in resonance-stabilized systems; a contributing structure
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Single Bond
A covalent bond in which a single pair of electrons is shared.
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Structural Formula
- A chemical formula that shows how the atoms of a molecule or polyatomic
- ion are arranged, to which other atoms they are bonded, and the kinds of
- bonds (single, double, or triple).
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