Bonding 1

Helps keep track of the electro distribution between variius reactants and products in a chemical reaction

The oxidation number of the element becomes more positive during s chemical reaction

The oxidation number becomes more negative during s chemical reaction

When all electrons are in the lowest energy orbitals available

A condition referred to as an octet when considering s and p valence electrons

Predicts shape of simple molecules; one rule = electron pairs, whether bonding or non bonding, attempt to move as far apart as possible

A molecule with a 180 bond angle

Determine the atom’s geometric identity

Linear sp hybridization

Trigonal planar sp2 hybridization

Tetrahedral sp3 hybridization

Triagonal bipyramidal dsp3 hybridization

Octahedral d2sp3 hybridization

• ) count number of electron groups = geometric family 2. ) determine shape based on non binding pairs

Orbitals always get used up s -> d; start left and work right until all orbitals are filled; Hybridization of carbon on Methane = s+p+p+p = sp3

Atoms attempt at closed shell stability; it is two atoms with similar electronegativities compromise to achieve octet

Covalent bonds in which the electron pair spends the same amount of time around each atom

Covalent bonds that are fatter at one end than at the other

Model in which the metal is thought of as a giant molecule in which delocalized molecular orbitals cover the entire structure

Formed when N molecular orbitals are very closely spaced in energy and form a band covering a range of energies

Band that is the highest energy and contains freely moving valence electrons

The empty band that overlaps the valence band; if electrons jump into it the material will be able to conduct electricity

When a valence band is not fully occupied, valence electrons can move in many energy states

Valence electrons can jump into the conduction band