Chap 1: The Chemical Foundations of BioChem

Question 1

Thermodynamics

Answer 1

Study of Energy

Question 2

Reactions

Answer 2

Reactants —> Products

Question 3

First Law of Thermodynamics

Answer 3

Energy is converted
Cannot be created nor destroyed only converted

Question 4

Forms of energy

Answer 4

Kinetic
Potential
Heat
Chemical

Question 5

Second Law of Thermodynamics

Answer 5

The entropy (chaos) of the universe (S) is always increasing

Question 6

Third Law of Thermodynamics

Answer 6

The entropy of a perfect crystalline at 0 K is 0

Question 7

Gibbes Free Law

Answer 7

Δ G = Δ H − T Δ S
H = Enthalpy
T = Temperature (K)
S = Entropy

Question 8

Spontaneous means

Answer 8

It is likely to happen in nature

Question 9

Free energy standard state conditions

Answer 9

T = 298K
P = 1 atm
Solutes = 1 M
pH = 7

Question 10

When products have less energy vs when products have more energy

Answer 10

Favorable (spontaneous) vs unfavorable

Question 11

Coupling Reactions

Answer 11

A process in which unfavorable reactions can be made energetically possible by linking them to favorable ones

Question 12

Equilibrium

Answer 12

Chemical state when the rate of the forward and reverse state of a reaction are equal

Question 13

Kinetics

Answer 13

the field of study that analyzes the rates of chemical reactions

Question 14

Rate Law

Answer 14

the rate of any chemical reaction that can be described using mathematical expressions

Question 15

Catalyst

Answer 15

Biological enzymes that speeds up a reaction by lowering the activation energy

Question 16

Functional Group

Answer 16

Fragments of a molecule (ex. hydroxyl or carbonyl)

Question 17

Reactions mechanism

Answer 17

Explains the making and breaking of bonds at the molecular level

Question 18

Hydrogen Bond

Answer 18

Weak bond (easily formed and broken)

*Bonds with electro negative elements (ex. Oxygen & Nitrogen)

Question 19

Provide electron vs Accepts proton

Answer 19

Acceptor vs Donor

Question 20

Arrhenius
Acids vs Bases

Answer 20

Acids: H+ donors
Bases: generates OH-

Question 21

Bronsted-Lowry
Acids vs Bases

Answer 21

Acids: H+ donors
Bases: H+ acceptors

Question 22

pKa =

Answer 22

• log Ka

Question 23

Ka =

Answer 23

[H+] [A-]/[HA]

Question 24

pH =

Answer 24

-log[H+]

Question 25

^pKa =

Answer 25

low pH

Question 26

Henderson-Hasselbalch Equation

Answer 26

pH = pKa + log[A-]/[HA]

Question 27

Buffering Capacity

Answer 27

the pH at which a weak acid or conjugate base system will buffer

Question 28

The capacity of a buffer to resist changes in pH upon addition of protons or hydroxide ions depends on

Answer 28

+ The pH of the buffer

+ the pKa of the weak acid in the buffer

+ the concentration of the weak acid and its conjugate base in the buffer

Question 29

pka represents

Answer 29

the acidity of a particular molecule

Question 30

ka represents

Answer 30

the equilibrium constant of an acid’s dissociation reaction