unit 4 Flashcards
VSEPR theory?
valence shell electron pair repulsion. based on mutual repulsion between valence electron pairs surrounding an atom. electron pairs want to be as far apart as possible, the atoms surrounding the central atom adopt an arrangement that minimises this repulsion.
repulsion?
repulsion between bonding pairs dictates geometry.
simple molecular geometry?
2 bonds - linear 3 bonds - trigonal planar 4 - tetrahedral 5 - trigonal bipyramidal 6 - octahedral
2 bonds with 1 lone pair or 2 bonds with 2 lone pairs?
bent.
4 bonds and 1 lone pair?
seesaw.
3 bonds 2 lone pairs?
t-shaped.
3 bonds 1 lone pair?
trigonal pyramidal.
5 bonds 1 lone pair?
square pyramidal.
2 bonds 3 lone pairs?
linear.
4 bonds 2 lone pairs?
square planar.
bond angles?
linear - 180 trigonal planar - 120 tetrahedral - 109.5 trigonal bipyramidal - axial 90, equatorial 120 octahedral - axial 90, equatorial 90
hybridization?
the mixing of two or more orbitals to form a new set of hybrid orbitals.
sigma bonds?
covalent bonds formed by orbitals overlapping end to end with the electron density concentration between the nuclei of the two atoms involved.
pi bonds?
covalent bonds formed by sideways overlapping orbitals with electron density concentrated above or below the plane of the nuclei of the two atoms involved.
bonds?
single bonds - 1 sigma
double - 1 sigma 1 pi
triple - 2 pi 1 sigma