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18 Cards in this Set

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