Ch.2
No description yet. This curated deck is ready for daily study.
Card preview (23)
Intermolecular Forces
Interactions that exist between molecules
London Forces
Induce a temporary dipole moment in a nearby molecule so an attractive dipole-dipole interaction results for a fraction of a second
Rank intermolecular forces from weakest to strongest
London, dipole-dipole, hydrogen bonding, ion-ion
What is ion-ion bonding
Bonding between two ionic compounds (ex. NaCl, LiF)
How does strength of intermolecular forces relate to boiling point?
Stronger intermolecular forces, higher boiling point
How does surface area relate to boiling point?
Increased surface area, higher boiling point
What is the reactive part of a molecule?
The functional group
Bronsted-Lowry acid and base definitions
Acid: proton donor Base: proton acceptor; donates electrons to a proton
Acidity Constant (Ka) Formula
[H3O+][A-]/[HA]
pKa formula
pKa = log[Ka]
Strong acids are _____ bases and vice versa
weak
Youcan stabalize a negative charge easily if pKa is ______, if it is difficult pKa must be ______
low; high
How is pKa and electronegaticity related
Increased electronegativity, decreased pKa
Why are s orbitals more stable?
In s-orbitals, electrons are closer to the nucleus than p-orbitals
Does delocalizing a charge lower or raise pKa
Lowers; Charge is put on more than one atom
Closer the electronegative atoms ____ the pKa. The more electronegative the atom the _____ the pKa. The higher amount of electronegative atoms, the _____ the pKa
lower, lower, lower
Keq formula
10^ (± IpH-pKaI)
If pH < pKa, the proton…
stays on
If pH > pKa, the proton…
comes off
Lewis base
An electron pair donator; donates to anything that is electron deficient
Lewis acids
An electron pair acceptor
Nucleophile
“proton-loving”, has a negative or partial negative charge
Electrophile
“electron-loving”, positive or partial positive charge