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Flashcards in Review 5 Deck (37):
1

Carboxylation

COOH group is added to substrate

2

Enthalpy formula

- ∆H formula

H = E + PV

- E = internal energy of system

- PV = work

- ∆H = q

3

Positive delta H

Endothermic

4

Kinetically controlled = ______ (reversible/irreversible) Thermodynamically controlled = _______

Kinetic = irreversible Thermodynamic = reversible

5

Which energy level do transition metals lose e- from first?

Outermost shell

6

Catalytic efficiency

kcat/Km

7

Michaelis-Menten Equation

V = kcat*[E]*[S] / (Km + [S])

8

How many H bond acceptors/donors does C have?

- A/T?

- G?

- C: 2 acceptors (N and O)

- A/T: 1 donor, 1 acceptor

- G: 2 donors, 1 acceptor

9

Thymine (purine/pyrimidine?) substituents? Uracil?

Pyrimidines (1 ring)

- T = 2 carbonyls, one methyl

- U = 2 carbonyls

10

Cytosine substituents?

- C = 1 carbonyl, 1 NH2

11

Adenine (purine/pyrimidine?) substituents? Guanine?

Purines (2 rings)

- A = 1 NH2

- G = 1 NH2, 1 carbonyl

12

What are the byproducts of AK DH forming OAA from AK?

2 NADH

1 FADH2

13

What catalyzes the final step of both glycogenolysis and gluconeogenesis?

Glucose 6 Phophatase

14

Starting materials of gluconeogenesis

TCA intermediates

Lactate

Glycerol

Pyruvate

15

What catalyzes rate-limiting step in glycogenolysis?

Glycogen phosphorylase

16

Succinyl CoA Synthetase catalyzes what reaction

Succinyl CoA => Succinate + GTP

17

What part of mitochondria has high H+ concentration?

Intermembrane space

- Travels down gradient into matrix

18

Paramagnetic

Unpaired electrons => attract to magnets

- Align w/ magnetic fields

19

Diamagnetic

Paired electrons => repel magnets

- Oppose magnetic fields

20

If n = 4, what can l equal?

0 (s)

1 (p)

2 (d)

3 (f)

21

In the p subshell, what is l and what can m1 be?

l = 1

m1 = -1, 0, or 1

22

Divalent cation

Cation w/ +2 charge

23

The ionization energy to remove a second electron is _____ than the first

Greater due to larger effective charge of cationic nucleus on electrons

24

Ionization energy increases from ______ to ______ in a group

Left to right - Left = low ionization energy

25

Ammonium

NH4+

26

What do ionic compounds form?

Large arrays of ions in crystalline solids

- Measured w/ formula weights

27

What are covalent compounds measured with? - Ionic compounds?

- Covalent = molecular weights - Ionic = formula weights

28

Acetone

C3H6O

A image thumb
29

Stronger electrolyte has _____ and _____

More ions and greater total charge

30

What does the rate constant depend on?

Temperature and activation energy

31

Increase pressure on a gaseous system will do what?

Shift equilibrium towards side w/ fewer moles of gas

32

Increasing temperature of endothermic reaction or decreasing temperature of exothermic reaction does what?

Shifts reaction to right

33

Does water in the liquid or gas phase appear in equilibrium expressions?

Only gas phase

34

Closed system

Exchanges energy but not matter with surroundings

35

Adiabatic

No heat change

36

Fusion

Melting

37

Longer hydrocarbons release more or less heat during combustion?

More due to having more reactants