mod 2 ch 2

Question 1

polar covalent bond

Answer 1

electrons are attached to one atom more than the other and there is pull (between covalent and ionic in electronegativity)

Question 2

most electronegative element

Answer 2

Fluorine

Question 3

as the difference in electronegativity between two bonded atoms increases, the bond polarity and ionic character ______ __________

Answer 3

also increases

Question 4

C - O, C - N, C - X, C - M bonds are

Answer 4

polar

Question 5

electrons are more concentrated near the

Answer 5

electronegative atom

Question 6

red on a electrostatic potential map indicates

Answer 6

electron rich

Question 7

blue on a electrostatic potential map indicates

Answer 7

electron poor

Question 8

what is the only IMFA present in non polar compounds

Answer 8

London dispersion forces

Question 9

why are London dispersion forces the weakest IMFA

Answer 9

due to temporary dipoles

Question 10

what creates dipole - dipole forces

Answer 10

differences in electronegativity

Question 11

what creates hydrogen bonds

Answer 11

interaction of H and the lone pair of N, O, or F

Question 12

the strength of H-bonding increases with…

Answer 12

increasing electronegativity

Question 13

what does the formal charge reflect and what is it used for

Answer 13

• it reflects the electron count of a particular atom in a molecule compared to an isolated neutral atom
• it is used for bookkeeping purposes

Question 14

what are resonance structures

Answer 14

structures that differ in the position of the pi bond or lone pair

Question 15

define Arrhenius acids and bases

Answer 15

arrhenius acid - H in front, releases H+
arrhenius base - OH in back, releases OH

Question 16

define Bronsted Lowry acids and bases

Answer 16

bronsted lowry acid - Acids Donate H+ (proton) (ADD)
bronsted lowry base - Bases Accept H+ (proton) (BAD)

Question 17

define Lewis acids and bases

Answer 17

Lewis Acid:
1. positive charge
2. B, Al, Ti, Fe
3. -COOH (carboxylic acid)
Lewis Base:
1. negative charge
2. group I or II metal (Li, Mg…)
3. Nitrogen w/o a charge

Question 18

the _______ the pka the weaker the acid

Answer 18

higher

Question 19

the equilibrium of a reaction will always move towards the ___________ acid

Answer 19

weaker

Question 20

the butt of a curvy arrow always goes from a Lewis ____ to a Lewis _____ .

Answer 20

LEWIS BASE TO A LEWIS ACID

Question 21

acids donate ____ and bases accept ___

Answer 21

H+

Question 22

label

Answer 22

green: conjugate base
purple: conjugate acid

Question 23

label

Answer 23

pink : conjugate base
orange : conjugate acid

Question 24

the stronger the acid the weaker its __________ ______

Answer 24

conjugate base

Question 25

define electrophile and nuclceophile

Answer 25

electrophile accepts electrons
nucleophile gives electrons

Question 26

what are the factors that affect acid strength

Answer 26

C - charge
A - atom effects
R - resonance effects
I - inductive effects
O - orbital effects

Question 27

how does CHARGE affect acid strength

Answer 27

protonated and positively charged acids are stronger than their neutral counterparts

Question 28

how do ATOM EFFECTS affect acid strength

Answer 28

• the proton (H+) that is attached to a more electronegative atom is more acidic
• the proton (H+) that is attached to a bigger atom is more acidic

Question 29

how do RESONANCE EFFECTS affect acid strength

Answer 29

the acid with a conjugate base that is stabilized by resonance will be more acidic

Question 30

how do INDUCTIVE EFFECTS affect acid strength

Answer 30

the closer and the more electron withdrawing groups present the more acidic

Question 31

how do ORBITAL EFFECTS affect acid strength

Answer 31

if the proton (H+) is attached to a hybridized carbon sp is most acidic and sp3 is least