Chem exam 4 Flashcards
N atoms
Will always have a lone pari if it has 3 bonds
Sigma bonds
Head on
Single: 1
Double: 1
Triple: 1
Pi bonds
Overlapping of P orbitals
Single: 0
Double: 1
Triple: 2
Hybridization orbitals
Sp: 2 electron domain
Sp2: 3 electron domains
Sp3: 4 electron domains
Sp3d: 5 electron domains
Sp3d2: 6 electron domains
Valence bond theory
-Valence electrons reside in quantum mechanical atomic orbitals. They can be S P D F or hybridized combinations of these
-A chemical bond results from the overlap of these 2 half filled orbitals and spin pairing
-The geometry of the overlapping orbitals determines the shape of the molecule
Melting points
Stronger= higher
Boiling points
Stronger= higher
Vapor pressure
Stronger=lower
Viscosity
Stronger= higher
Surface tension
Stronger = higher
Boiling point physical phase
If boiled before 295 = gas
Boiling point definition
Temperature at which the liquids vapor pressure equals the external pressure
Bond polarity
Caused by differences in electronegativity of elements
Molecule polarity
requires bond dipoles, but also has geometric considerations
Dipole moment
-Bigger electrongativety difference =bigger dipole moment
-Farther apart = bigger dipole moment
-Tells how big the difference is
Net dipole moment
-Overall dipole moment of a molecule
-Sum of individual bond dipoles
-Vector
Dipole-Dipole interactions
-Polar
-Permanent dipole moment
-Asymmetric
-Stronger when molecules are closer and bigger difference in electronegativity
Dispersion interactions
-Instant non permanent
-in everything
-constant motion
-can be temporarily asymmetric
-creates instantaneous dipole moment
-Bigger molecules = stronger dispersion forces ( more e = larger charges)
Ion dipole forces
-ions and a polar molecule interacting
-Full charge atoms
-Ion dipole must compete with ion-ion to get salts to dissolve
Hydrogen Bonding
-Lone pairs
-On O, N, F sometimes Cl
-H atom
-Bonded to another electronegative atom
H bond acceptor
Lone pairs are connected
H bond donor
The one with H
Covalent naming
1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- octa
9- nona
10- deca
How many moles of (element) are in ___ moles of (compound)
Atoms of element * moles they want