Ch.6 study Flashcards
VESPR theory
Describes the orientation of electron groups around the central atom
States electron groups are arranged as far apart as possible around the central atom
States the specific shape of a molecule is determined by the number of atoms attached to the central atom
Linear
2 bonded atoms
0 lone pairs
180 degree angle
Linear molecule shape
Trigonal planar (trigonal planar)
3 bonded atoms
0 lone pairs
120 degree angle
Trigonal planar (bent)
2 bonded atoms
1 lone pair
120 degree angle
Tetrahedral (tetrahedral)
4 bonded atoms
0 lone pairs
109 degrees
Tetrahedral (Trigonal pyramidal)
3 bonded atoms
1 lone pair
109 degrees
Tetrahedral (bent)
2 bonded atoms
2 lone pairs
109 degrees
Electronegativity values
H= 2.1
B= 2.0
C= 2.5
N=3.0
O= 3.5
F= 4.0
Al= 1.5
Si= 1.8
P=2.1
S=2.5
Cl= 3.0
Ga= 1.6
Ge= 1.8
As= 2.0
Se= 2.4
Br= 2.8
In= 1.7
Sn= 1.8
Sb= 1.9
Te= 2.1
I= 2.5
Li= 1.0
Be= 1.5
Na= 0.9
Mg= 1.2
K= 1.8
Ca= 1.0
Hydrogen bonds can only form with?
Flourine (F)
Oxygen (O)
Nitrogen (N)
Hydrogen bonds are all dipole dipole interactions
True
Dispersion forces
Weak attractions between nonpolar molecules
Caused by temporary dipoles that develop when molecules bump into each other
Makes it possible for nonpolar molecules to form liquids and solids
Melting points
Lower due to weak forces like dispersion forces
Higher due to stronger forces like hydrogen bonding
Highest in ionic compounds