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18 Cards in this Set
- Front
- Back
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Valence electron
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the electrons present in the valence shell of an atom
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Peripheral atom
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atoms surrounding the central atom
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bond dipole
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the charge separation that happens when the electroneg. difference of two bonded atoms shifts the shared electrons, making one end of the bond negative and one end positive
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polar covalent bond
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a bond in which the bonding electrons are NOT shared equally because the bonded atoms have different electronegativities.
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VSEPR theory
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theory that helps determine shapes of molecules
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orbital
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region of space around the nucleus of an atom where an electron is likely to be found
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lone pair
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two valence electrons occupying the same orbital
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octet rule
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idea that a maximum of eight electrons can occupy orbitals in the valence level of an atom
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lewis formula
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chemical formula that shows all valence electrons in shared or lone pairs around each atom in a molecule
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ionic bond
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simultaneous attraction among POS and NEG ions
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covalent bond
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simultaneous attraction of two nuclei for a shared pair of bonding electrons
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crystal lattice
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continious 3d pattern of atoms, ions or molecules in a crystalline solid
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central atom
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atom in a molecule that has the most bonding electrons and is likely to make most bonds
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dipole dipole forces
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the simultaneous attraction between oppositely charged ends of polar molecules
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electronegativity
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# that describes the relative ability of an atom to attract a pair of bonding electrons in its valence shell
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intramolecular forces
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strong bonds or forces of attraction and repulsion within a molecule; typically covalent bonds
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hydrogen bonds
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simultaneous attraction of a hydrogen nucleus, that is covalently bonded to a very electronegative atom
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non polar molecule
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molecule in which the negative charge is distributed symmetrically among atoms making up the molecule
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