Deck 2: Water, Weak Bonds, and the Generation of Order Out of Chaos

Question 1

A solvent with a low dielectric constant would be a ____________ solvent for salts.

Answer 1

poor

Question 2

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
Electrostatic interactions between atoms with opposite electrical charges are also called ____________.

Answer 2

a

Question 3

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
____________: The type of bond found between an oxygen on one water molecule and hydrogen on a different water molecule.

Answer 3

d

Question 4

Lipids that interact with both the water and the hydrophobic regions of the membrane are considered ____________.

Question 5

The source of the key buffering component of blood is ____________.

Question 6

The transient force which, while weak, still has a large impact on how macromolecules interact is the ____________.

Question 7

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
____________: The charge of the side group of aspartate when the pH is more than one pH unit above the pKa.

Question 8

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
The distance when two atoms no longer repulse each other yet have the strongest attraction is known as the____________ radii or contact distance.

Question 9

Buffers are critical in maintaining proper ____________ levels in biological systems.

Question 10

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
____________: Thermodynamic force that drives hydrophobic interactions.

Question 11

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
Water weakens the electrostatic interaction of ions due to its high ____________.

Question 12

When the pH is more than two pH units above the pKa of a carboxyl group, the acid is ____________.

Question 13

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
Movement of particles due to the random fluctuations of energy content of the environment is known as ____________.

Question 14

Hydrophobic molecules are driven together by ____________, not because they have an affinity for each other.

Question 15

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
____________: A molecule with two distinctive chemical properties or characteristics.

Question 16

Molecules that are readily soluble in water are considered ____________.

Question 17

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
____________: The charge of an amino group when the pH is one pH unit below the pKa.

Question 18

Use the following to answer questions 1-10:
Choose the correct answer from the list below. Not all of the answers will be used.
a) ionic bonds or salt bridges
b) Brownian motion
c) hydrophobic
d) hydrogen
e) polar
f) nonpolar
g) van der Waals
h) entropy
i) zwitterion
j) amphipathic
k) positive
l) dielectric constant
m) negative
Which type of amino acids are responsible for increasing entropy as a protein folds?

Question 19

The force that is quantified by Coulomb's law is called the ____________.

Question 20

An acid ionizes to form a proton and its ________________.

Question 21

Water can form hydrogen bonds with the ___________ of another molecule.

A) carbonyl groups
B) amine groups
C) aromatic rings
D) alcohol groups
E) A, B, and D

Question 22

Using Coulomb's law, describe how water is an ideal solvent for the ions found in cells?

Question 23

What two properties of water are important for biological interactions?

A) the polarity of water
B) the density of water
C) the cohesive properties of water
D) A and C
E) B and C

Question 24

What is the concentration of acetic acid in 250 ml of a 100 mM acetate buffer at pH 4.76?

A) 250 mM
B) 100 mM
C) 50 mM
D) 75 mM
E) There is not enough information to tell.

Question 25

What happens to nonpolar molecules in water?

A) They dissolve independently.
B) They aggregate together.
C) They precipitate.
D) All of the above.
E) None of the above.

Question 26

What thermodynamic and free-energy changes participate in protein folding?

Question 27

How is protein folding driven?

Question 28

What charged group(s) are present in glycine at a pH of 7?

A) -NH3+
B) -COO-
C) -NH2+
D) A and B
E) A, B, and C

Question 29

List atoms commonly found in biological molecules that are often hydrogen-bond acceptors.

A) carbon
B) oxygen
C) nitrogen
D) B and C
E) All of the above.

Question 30

What is the net effect of many van der Waals interactions?

Question 31

What is the [A−]/[HA] ratio when the weak acid is in a solution one pH unit above its pKa?

A) 1:1
B) 1:10
C) 10:1
D) 2:1
E) None of the above.

Question 32

What are the primary chemical components present in a phosphate buffer at pH 7.4?

A) H3PO4 and PO4−3
B) H2PO4− and PO4−3
C) HPO4-2 and PO4-3
D) H2PO4− and HPO4−2
E) H3PO4 and HPO4−2

Question 33

What is the H+ concentration in a urine sample that has a pH of 6?

A) 10−6 M
B) 10−8 M
C) 106 M
D) 10−14 M
E) 8 M

Question 34

If noncovalent bonds are so much weaker than covalent bonds, how do they stabilize large biochemical structures?

Question 35

What is an electrostatic interaction? Give an example.

Question 36

What pairs of atoms in bases are involved in hydrogen bonds?

A) N-H and O-H
B) N-H and S-H
C) O-H and P-O
D) All of the above.
E) None of the above.

Question 37

How is water able to be a solvent for so many biological molecules?

Question 38

Which of the following is considered a noncovalent bond?

A) electrostatic interactions
B) hydrogen bonds
C) van der Waals interactions
D) All of the above.
E) None of the above.

Question 39

What is the significance of hydrogen bonding in biochemical structures such as DNA?

Question 40

Typical van der Waals energies are about:

A) 4-20 kJ/mol.
B) 2-4 kJ/mol.
C) 200 kJ/mol .
D) All of the above.
E) None of the above.

Question 41

Give examples of key functional groups found in biochemistry.

Question 42

Why are conjugate acid-base pairs so important in biological systems?

Question 43

How do hydrophobic interactions aid in membrane formation?