Question 1

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

Accepted Answer

Many biological molecules have polar characteristics.Water is extremely polar and is capable of competing with other polar molecules by weakening their electrostatic and hydrogen bonds.The oxygen atom can act as a hydrogen-bond acceptor,and the hydrogen can act as a donor.

Question 2

The simplest way to depict stereochemistry is to use

Accepted Answer

A)  ball-and-stick models. 
B)  ribbon diagrams. 
C)  space-filling models. 
D)  Fisher projections. 
E)  None of the answers is correct. 
A)  ball-and-stick models. 
B)  ribbon diagrams. 
C)  space-filling models. 
D)  Fisher projections. 
E)  None of the answers is correct. D

Question 3

Provide a simple example of a process in which the entropy of a system changes.

Accepted Answer

Several examples can be provided,including the random mixture of atoms when two different gases are mixed,or the creation of water molecules from energy gained following the mixture of oxygen and hydrogen under certain conditions.

Question 4

DNA is made from the building blocks adenine,guanine,cytosine and _____.

Accepted Answer

A)  uridine 
B)  thymine 
C)  inosine 
D)  ribose 
E)  None of the answers is correct. 
A)  uridine 
B)  thymine 
C)  inosine 
D)  ribose 
E)  None of the answers is correct.

Question 5

What is the significance of using $\Delta$G in biochemistry?

Accepted Answer

Gibbs free energy,also called the free-e

Question 6

If most proteins are found surrounded by water in the cell,what type of functional groups would you expect to find on the surface of a water-soluble protein?

Accepted Answer

Polar and charged am

Question 7

Which of the following describes the relationship between the strengths of hydrogen and covalent bonds?

Accepted Answer

A)  Hydrogen bonds are always stronger than covalent bonds. 
B)  Hydrogen bonds and covalent bonds have equivalent strength. 
C)  Hydrogen bonds are always weaker than covalent bonds. 
D)  With a few exceptions, most hydrogen bonds are stronger than covalent bonds. 
E)  With a few exceptions, most covalent bonds are stronger than hydrogen bonds. 
A)  Hydrogen bonds are always stronger than covalent bonds. 
B)  Hydrogen bonds and covalent bonds have equivalent strength. 
C)  Hydrogen bonds are always weaker than covalent bonds. 
D)  With a few exceptions, most hydrogen bonds are stronger than covalent bonds. 
E)  With a few exceptions, most covalent bonds are stronger than hydrogen bonds.

Question 8

What are the enthalpy and entropy changes that accompany the formation of DNA double helices from complementary single strands of DNA?

Accepted Answer

There is a loss of entropy from the syst

Question 9

What is significant about the fact that metabolic processes are common to many organisms?

Accepted Answer

These metabolic proc

Question 10

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

Accepted Answer

The bonds are weak enough to b

Question 11

How can a cell exist if the Second Law of Thermodynamics is true?

Accepted Answer

Entropy in a local area can be

Question 12

Entropy is defined as

Accepted Answer

A)  a spontaneous reaction. 
B)  the enthalpy of the system. 
C)  the measure of randomness of a system. 
D)  the amount of heat exchanged. 
E)  None of the answers is correct. 
A)  a spontaneous reaction. 
B)  the enthalpy of the system. 
C)  the measure of randomness of a system. 
D)  the amount of heat exchanged. 
E)  None of the answers is correct.

Question 13

Using the Henderson-Hasselbalch equation,calculate the pH of a buffer solution made from 0.20 M CH3COOH and 0.050 M CH3COO- that has pKa= 4.7.

Accepted Answer

A)  5.3 
B)  4.1 
C)  2.5 
D)  0.4 
E)  None of the answers is correct. 
A)  5.3 
B)  4.1 
C)  2.5 
D)  0.4 
E)  None of the answers is correct.

Question 14

The First Law of Thermodynamics states

Accepted Answer

A)  diversity is the result of gradual evolution. 
B)  the total entropy of a system and its surroundings always increases for a spontaneous process. 
C)  the total energy of a system and its surroundings is constant. 
D)  light is both particle and wave. 
E)  None of the answers is correct. 
A)  diversity is the result of gradual evolution. 
B)  the total entropy of a system and its surroundings always increases for a spontaneous process. 
C)  the total energy of a system and its surroundings is constant. 
D)  light is both particle and wave. 
E)  None of the answers is correct.

Question 15

Which of the following atoms commonly found in biological molecules are often hydrogen-bond acceptors?

Accepted Answer

A)  carbon 
B)  oxygen 
C)  nitrogen 
D)  All of the answers are correct. 
E)  oxygen and nitrogen 
A)  carbon 
B)  oxygen 
C)  nitrogen 
D)  All of the answers are correct. 
E)  oxygen and nitrogen

Question 16

What gives proteins such a dominant role in biochemistry?

Accepted Answer

A)  the rigidity of the peptide backbone 
B)  the ability to act as a blueprint 
C)  the ability to self-replicate 
D)  the ability to spontaneously fold into complex three-dimensional structures 
E)  All of the answers are correct. 
A)  the rigidity of the peptide backbone 
B)  the ability to act as a blueprint 
C)  the ability to self-replicate 
D)  the ability to spontaneously fold into complex three-dimensional structures 
E)  All of the answers are correct.

Question 17

Which of the following is a hydrogen bond donor?

Accepted Answer

A)  the N in N-H D 
B)  the H in S-H 
C)  the O in P-O 
D)  the H in O-H 
E)  None of the answers is correct. 
A)  the N in N-H D 
B)  the H in S-H 
C)  the O in P-O 
D)  the H in O-H 
E)  None of the answers is correct.

Question 18

Describe the shape of methane.

Accepted Answer

Methane is tetrahedr

Question 19

The Second Law of Thermodynamics states

Accepted Answer

A)  the total entropy of a system and its surroundings always increases for a spontaneous process. 
B)  temperatures will always decrease in a spontaneous process. 
C)  the total energy of a system and its surroundings is constant. 
D)  diversity is the result of gradual evolution. 
E)  None of the answers is correct. 
A)  the total entropy of a system and its surroundings always increases for a spontaneous process. 
B)  temperatures will always decrease in a spontaneous process. 
C)  the total energy of a system and its surroundings is constant. 
D)  diversity is the result of gradual evolution. 
E)  None of the answers is correct.

Question 20

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

Accepted Answer

At the interface of two large

Exam 1: Biochemistry: An Evolving Science

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

The simplest way to depict stereochemistry is to use

Provide a simple example of a process in which the entropy of a system changes.

DNA is made from the building blocks adenine,guanine,cytosine and _____.

What is the significance of using Δ\DeltaΔ G in biochemistry?

If most proteins are found surrounded by water in the cell,what type of functional groups would you expect to find on the surface of a water-soluble protein?

Which of the following describes the relationship between the strengths of hydrogen and covalent bonds?

What are the enthalpy and entropy changes that accompany the formation of DNA double helices from complementary single strands of DNA?

What is significant about the fact that metabolic processes are common to many organisms?

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

How can a cell exist if the Second Law of Thermodynamics is true?

Entropy is defined as

Using the Henderson-Hasselbalch equation,calculate the pH of a buffer solution made from 0.20 M CH3COOH and 0.050 M CH3COO- that has pKa= 4.7.

The First Law of Thermodynamics states

Which of the following atoms commonly found in biological molecules are often hydrogen-bond acceptors?

What gives proteins such a dominant role in biochemistry?

Which of the following is a hydrogen bond donor?

Describe the shape of methane.

The Second Law of Thermodynamics states

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

Protein Composition and Structure

Exploring Proteins and Proteomes

DNA, RNA, and the Flow of Genetic Information

Exploring Genes and Genomes

Exploring Evolution and Bioinformatics

Hemoglobin: a Portrait of a Protein in Action

Enzymes: Basic Concepts and Kinetics

Catalytic Strategies

Regulatory Strategies

Carbohydrates

Lipids and Cell Membranes

Membrane Channels and Pumps

Signal-Transduction Pathways

Metabolism: Basic Concepts and Design

Glycolysis and Gluconeogenesis

The Citric Acid Cycle

Oxidative Phosphorylation

The Light Reactions of Photosynthesis

The Calvin Cycle and the Pentose Phosphate Pathway

Glycogen Metabolism

Fatty Acid Metabolism

Protein Turnover and Amino Acid Catabolism

The Biosynthesis of Amino Acids

Nucleotide Biosynthesis

Biosynthesis of Membrane Lipids and Steroids

The Integration of Metabolism

DNA Replication, repair, and Recombination

RNA Synthesis and Processing

Protein Synthesis

The Control of Gene Expression in Prokaryotes

The Control of Gene Expression in Eukaryotes

Sensory Systems

The Immune System

Molecular Motors

Drug Development

Filters

What is the significance of using $\Delta$ G in biochemistry?

Using the Henderson-Hasselbalch equation,calculate the pH of a buffer solution made from 0.20 M CH₃COOH and 0.050 M CH₃COO^- that has pK_a= 4.7.