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31 Cards in this Set
- Front
- Back
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Octet rule
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Atoms react by gaining or losing electrons so as to squire the stable electron structure of a Nobel gas, usually right valence electrons
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Valence electron
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An electron in the highest occupied energy level of an atom
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Halide ion
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A negative ion formed when a halogen atom gains an electron
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Electron dot structure
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A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot structure
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Chemical formula
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An expression that indicated the number and type of atoms present in the smallest representative unit of a substance
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Ionic compound
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A compound composed of positive and negative ions
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Formula unit
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The lowest whole-number ratio of ions in an ionic compound; in magnesium chloride, the ratio of magnesium ions to chloride is 1:2 and the formula unit is MgCl(2)
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Ionic bond
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The electrostatic attraction that binds oppositely charged ions together
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Covalent bond
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A bond formed by the sharing of electrons between atoms
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Molecule
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A neutral group of atoms joined together by covalent bonds
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Diatomic molecule
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A molecule consisting of two atoms
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Molecular compound
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A compound that is composed of molecules
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Molecular formula
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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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Single covalent bond double
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A bond formed when two atoms share a pair of electrons
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Double covalent bond
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A bond in which two atoms share two pairs of electrons
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Triple covalent bond
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A covalent bond in which three pairs of electrons are shared by two atoms
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Structural formula
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A chemical formula that shows the arrangement of atoms in a molecule or a Polyatomic ion; each dash between a pair of atoms indicated a pair of shared electrons
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Unshared pair
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A pair of valence electrons that is not shared between atoms
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Polyatomic ion
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A tightly bound groups of atoms that behaved as a unit and has a positive or negative charge
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Bond dissociation energy
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The energy required to break the none between two covalently bonded atoms; this value is usually expressed in kJ per mil of substance
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VAEPR theory
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Valence-shell electron-pair repulsion therapy; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible
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Nonpolar covalent bond
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A covalent bond in which the electrons are shared equally by the two atoms
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Polar covalent bond
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A covalent bond between atoms in which the electrons are shared unequally
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Polar bond
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A covalent bond between atoms in which the electrons are shared unequally
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Polar molecule
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A molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive
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Dipole
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A molecule that has two poles, or regions, with opposite charges
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Van der Waals forces
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The two weakest intermolecular attractions- dispersion interactions and dipole forces
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Dipole interactions
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intermolecular forces resulting from the attractions of oppositely charged regions of polar molecules
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Dispersion forces
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Attractions between molecules caused by the electron motion of one me lie affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
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Hydrogen bonds
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Attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom
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Network solids
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A solid in which all of the atoms are covalently bonded to each other
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