Exam 3 vocab

Question 1

Oxidation Number Rules

Answer 1

1- an element is 0
2- simple ions = charge of ion
3- F is -1
4- H = +1; O=-2; except when H is with a metal (is -1) or O is with H2 (is -1)
5- Cl, Br, I is -1; except with O and F
6- Algebraic sum is 0

Question 2

What is the reducing agent?

Answer 2

one that lost electrons; is oxidized

Question 3

What is the oxidizing agent?

Answer 3

one that gained electrons; is reduced

Question 4

Disaccharides: ?
Oligosaccharides: ?
Polysaccharides: ?

Answer 4

Disaccharides: 2
Oligosaccharides: 3-9
Polysaccharides: 9+

Question 5

D-sugars vs. L-sugars

Answer 5

D-sugars: chiral carbon is on the right side of Fischer projections
L-sugars: left side

Question 6

What is a diastereomer?

Answer 6

Stereoisomer which are not enantiomers; mirror image at only a few chiral carbons

Question 7

What is an epimer?

Answer 7

A diastereomer in which only differs on one -OH

Question 8

alpha-anomer vs beta-anomer

Answer 8

alpha: OH is trans (down)
beta: OH is cic (up)

Question 9

What is the glycosidic bond?

Answer 9

The bond of the two carbons that connects two monosaccharides together to form a disaccharide

Question 10

Difference between lactose and sucrose?

Answer 10

lactose is a reducing sugar due to “free anomeric carbon. Sucrose has no free anomeric carbon, so it is not a reducing sugar

Question 11

What are the two types of polysaccharides?

Answer 11

Storage: used to store energy; can be broken down
Structural: physical structure of an organism; can’t be broken down

Question 12

What are the 4 classic examples of polysaccharides?

Answer 12

Storage: starch, glycogen
Structural: cellulose, chitin

Question 13

Describe attributes of a gas

Answer 13

• molecule constant motion
• high temp, high k.e, high velocity
• behave like don’t interact
• exert pressure on surroundings

Question 14

What is Charles law?

Answer 14

• temp and volume
• directly proportional
  v1 = v2
  T1 T2

Question 15

Kelvin = ?

Answer 15

C + 273.15

Question 16

What is Boyle’s law?

Answer 16

• pressure and volume
• inversely proportional
  P1 (V1) = Pf (Vf)

Question 17

What is Gay-Lussac’s law?

Answer 17

• temp and pressure
• directly proportional
  p1 = p2
  T1 T2

Question 18

What is Ideal Gas law?

Answer 18

PV = nRT

• n is moles of gas
• R= 0.082057 [given]
• units: liters, kelvin, atm

Question 19

What is a solution?

Answer 19

a homogenous mixture with small dissolved particles, usually transparent

Question 20

What is a colloid?

Answer 20

a homogenous mixture with larger particles, usually opaque

Question 21

What is a suspension?

Answer 21

a mixture that will settle

Question 22

What are the two parts of a solution?

Answer 22

solute- being dissolved; lesser
solvent- doing dissolving; greater

Question 23

What is an aqueous solution?

Answer 23

solution where solvent is water

Question 24

What is solubility?

Answer 24

the max amount of solute which can dissolve in the solvent under given conditions

Question 25

What is solution if at max or not?

Answer 25

at max: saturated
not at max: unsaturated

Question 26

Water doing dissolving is ___ and water being dissolved is ____

Answer 26

Water doing dissolving is solvation and water being dissolved is hydration

Question 27

What is Henry’s law?

Answer 27

high pressure leads to greater solubility

Question 28

What is…
Electrolyte:
Strong Electrolyte:
Weak Electrolyte:
Non Electrolyte:

Answer 28

What is…
Electrolyte: solutes that produce ions when dissolved
Strong Elec.: all solute molecules come apart to form ions
Weak Elec.: only some ions
NonElec.: does not come apart (usually polar)

Question 29

Common examples…
Strong Electrolyte:
Weak Electrolyte:
Non Electrolyte:

Answer 29

Strong Electrolyte: ionic compounds
Weak Electrolyte: carboxylic acid, amine
Non Electrolyte: everything else

Question 30

What is concentration?

Answer 30

Molarity;
the amount os solute in the solvent
moles/L of solution

Question 31

w/w %:
v/v %:
w/v %:
(with units)

Answer 31

w/w %: mass solute/mass solution x 100
v/v %: vol. solute/vol. solution x 100
w/v %: mass solute (g) / volume solution (mL) x 100

Question 32

What is equivalence?

Answer 32

ion that gives you 1 mol of charge per liter

Question 33

Dilution equation

Answer 33

C1V1 = C2V2

Question 34

What is diffusion? What is osmosis?

Answer 34

Diffusion: movement of material from higher to lower concentration
Osmosis: migration of solvent through semipermeable membrane to higher concentration

Question 35

What is osmotic pressure?

Answer 35

pressure needed to stop osmosis

Question 36

Isotonic vs hypotonic vs hypertonic

Answer 36

Isotonic: same concentration
hypotonic: solution outside has lower concentration, so itv flows into cell (hemolysis)
hypertonic: solution outside has higher concentration, water moves out (crenation)

Question 37

What is an acid? What is a base? H3O+?

Answer 37

acid: substance that donate H+
base: accepts H+
H3O+: hydronium ions

Question 38

What are polyprotic acids? Examples?

Answer 38

an acid which may donate more than one H+ to a base
examples: sulfuric acid, phosphoric acid, carbonic acid

Question 39

What are amphoteric compounds? Examples?

Answer 39

can be an acid or a base
mainly water

Question 40

Strong acid:
Weak acid:
Strong base:
Weak base:

Answer 40

Strong acid: completely disassociate in water, 1 mol
Weak acid: partially disassociate, less 1 mol
Strong base: completely disassociate in water, 1 mol (metals hydroxides)
Weak base: will react with water to pull off an H+ to create hydroxide (amines)