VSEPR theory

Ionic bonding description

electrostatic attraction between oppositely charged ions, metal and nonmetal

covalent bonding

sharing of electrons between atomic nuclei within a molecule

delta EN range: pure covalent

0-.04

delta EN range: polar covalent

0.4-1.7

delta EN range: ionic

1.7+

coordinate covalent bond

pair of electrons rented from the central atom to a surrounding atom

Valence bond theory

covalent bonds form orbitals of 2 atoms overlap, creating a new combined orbital of 2 electrons with opposite spin.

hybridization

theoretical process involving the mixing of orbitals to create a new set of orbitals that take part in covalent bonding, each orbital has equal energy and shape

sigma bond

end to end overlap of atomic orbitals, any combo of s and p

pi bond

created by parallel overlap of atomic orbitals, usually involving p

VSEPR Theory (Valence Shell Electron Pair Repulsion

arrangement of atoms around center atom of molecule depends on repulsion between all electron pairs. lone pairs have a stronger influence than bonded pairs

polar molecule

unequal distribution of partial charges, asymmetrical molecule

2 domains, VSEPR umbrella group and bond angle

linear, 180

3 domains, VSEPR umbrella group and bond angle

trigonal planar, 120

4 domains, VSEPR umbrella group and bond angle

tetrahedral, 109.5

5 domains, VSEPR umbrella group and angle

trigonal bipyrimidal, 120 in plane and 90 up and down (always 90)

6 domains, VSEPR umbrella group and angle

octahedral, 90

when do you have seasaw

4 bonds, 1 lp

when do you have trigonal bipyramidal t shape

3 bond, 2 lp

you always have linear when…

you only have 2 bonded pairs