Topic 1

Question 1

cation

Answer 1

loses electrons, becomes positive

Question 2

anion

Answer 2

gains electrons, becomes negative

Question 3

electrovalent bonding

Answer 3

aka ionic bonding
valence electrons are transferred forming ions
weaker than covalent
dissociates in water

Question 4

covalent bonding

Answer 4

atoms share electrons

Question 5

non polar covalent

Answer 5

equally shared e.g. H2 or O2

Question 6

polar covalent

Answer 6

unequally shared with +/- polarity e.g. H2O

Question 7

coordinate covalent

Answer 7

one atom provides Both electrons e.g. NH4

Question 8

hydrogen bonding

Answer 8

when H+ forms polar bond with another atom

has a slight + charge and attracts to nearby - atom e.g. between 2 H2Os

Question 9

hydrophilic

Answer 9

soluble in water

Question 10

hydrophobic

Answer 10

insoluble in water

Question 11

osmosis

Answer 11

movement of water across a semipermeable membrane to higher solute concentration

Question 12

osmotic pressure

Answer 12

pressure required to maintain equilibrium

Question 13

osmolarity

Answer 13

solute concentration required to create osmotic pressure on cellular membrane

Question 14

isotonic

Answer 14

solution that has equal osmolarity

Question 15

hypotonic

Answer 15

solution that has lower osmolarity; swelling of cell

Question 16

hypertonic

Answer 16

solution that has higher osmolarity; shrinkage of cell

Question 17

acid

Answer 17

proton donator pH<7

Question 18

strong acids

Answer 18

completely ionize; e.g. hydrochloric acid and sulfuric acid

Question 19

weak acids

Answer 19

partial ionize; e.g. phosphoric acid, carbonic acid

Question 20

base

Answer 20

proton acceptor, hydroxyl releaser, ph>7

Question 21

strong base

Answer 21

completely dissociate; e.g. sodium hydroxide, calcium hydroxide

Question 22

weak base

Answer 22

partially dissociates; e.g. ammonium hydroxide

Question 23

ionization of water

Answer 23

quantified by ion products of water and basis of pH scale

Question 24

pH

Answer 24

H+ concentration in a solution
scale 0-14
pH = -log [H+]
blood pH = 7.4 (7.35-7.45)

Question 25

buffers

Answer 25

composed of weak acid (base) and its conjugate base (acid)

Question 26

Henderson-Hasselbach equation

Answer 26

``` pH = pKa + log [A+]/[HA] pKa = -log Ka Ka = [H+][A-]/[HA] ```

Question 27

When does pH = pKa?

Answer 27

with equal concentrations of [A-] and [HA]

Question 28

human buffer systems

Answer 28

hemoglobin bicarbonate phosphate plasma protein

Question 29

redox reaction

Answer 29

involves transfer of electrons between 2 species oxidation = lose electrons reduction = gain electrons

Question 30

oxidation of primary alcohols

Answer 30

aldehyde

Question 31

oxidation of aldehyde

Answer 31

carboxylic acid

Question 32

reduction of carboxylic acid

Answer 32

aldehyde

Question 33

reduction of aldehyde

Answer 33

primary alcohol

Question 34

oxidation of secondary alcohol

Answer 34

ketone

Question 35

reduction of ketone

Answer 35

secondary alcohol

Question 36

acid + alcohol =

Answer 36

ester

Question 37

acid + sulfhydryl =

Answer 37

thioester

Question 38

acid + amine

Answer 38

amide

Question 39

phosphoric acid + alcohol =

Answer 39

phosphoester