Chapter 2 lecture Flashcards
Bronsted lowry acid
contains proton net
Bronsted lowry base
lone pair or pi bond with net charge 0 or -
CH3OH +NH2-=
name the acid, base, and conjugates
CH3O- +NH3
Acid is CH3OH, Base is NH2-, Conjugate base CH3O, Conjugate acid NH3
CH3OH +HCl=
name the acid, base, and conjugates
CH3OH2+ +Cl-
Acid strength
tendency of acid to donate proton therefore more readily a compound donates proton high acidity
Ka equillibrium
If Ka is 1 products and reactants are =
If Ka greater for products products favored
If Ka greater for reactants reactants favored
What factors determine acid strength
Charge, element, inductive, resonance, hybridization
What happens if a molecules + charge increases
acidity increases
Rank acidity
1. OH- -H+= O2-
2.OH- +H+=OH2
3. OH3+
1,2,3
What happens when you increase electronegativity?
increase acidity
ranking increasing acidity
CH4, HF, OH2, NH3
CH4
NH3
OH2
HF
What happens when size decreases
decreases acidity
Rank acidity
HI,HCl,HF,HBr
HF,HCl,HBr,HI
What is inductive effect
pull of electron density through sigma bonds caused by electronegative differences
What are some ways when inductive effect is occurring the acidity increases
Electronegative greater= more acidity
electronegative atoms are closer together
resonance effect and how does it effect acidity
delocalization of charge through resonance influence acidity therefore more resonance structure is more acidity
How does hybridization affect acidity
S character increases= increase in acidity
Rank which is more acidic
CH3CH3, CHCH, CH2CH2
CH3CH3,CH2CH2,CHCH
Lewis bases
electron pair donors
lewis acids
electron pair acceptors
pi bases
use pi bonds as electron donors
Electrophile
Lewis acid and attracts electrons
Nucleophile
lewis base and attracts nucleus
(CH3)3C+ +Br-+
(CH3)3CBr
