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Review Exam 1 for Biochemistry | CH 409, Exams of Biochemistry

Athens State UniversityBiochemistry
Prof. Nancy Mcdonald

Material Type: Exam; Professor: McDonald; Class: Biochemistry; Subject: Chemistry; University: Athens State University; Term: Spring 2011;

Typology: Exams

2010/2011

Uploaded on 03/27/2011

jcomeens1067
jcomeens1067 🇺🇸

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Biochemistry CH409 Exam I
Ch1 Review Questions:
4. Identify the functional groups in the following molecules:
A. aldehyde group
B. Carboxylic acid and amino group
C. Sulfhydryl group
D. Ester Group
E. Alkene
F. Amide Group
H. Ketone Group
i.Alcohol Group
5. Name 4 classes of small biomolecules. In what larger biomolecules are they found?
Amino acids, sugars, fatty acids and nucleotides.
Amino acids occur in peptides/proteins. Sugars occur in oligosaccharides/polysaccharides. Nucleotides
are in nucleic acids. Fatty acids are found in lipid molecules (triacylglycerols/phospholipids).
12. What is the difference between an unsaturated and a saturated hydrocarbon?
Saturated hydrocarbons contain only C-C single bonds, and unsaturated carbons contain C=C double or
C≡C triple bonds.
15. Assign each of the following compounds to one of the major classes of biomolecules:
A. Amino acid B. Sugar C. Fatty acid D. Nucleotide
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Biochemistry CH409 Exam I Ch1 Review Questions:

  1. Identify the functional groups in the following molecules: A. aldehyde group B. Carboxylic acid and amino group C. Sulfhydryl group D. Ester Group E. Alkene F. Amide Group H. Ketone Group i.Alcohol Group
  2. Name 4 classes of small biomolecules. In what larger biomolecules are they found? Amino acids, sugars, fatty acids and nucleotides. Amino acids occur in peptides/proteins. Sugars occur in oligosaccharides/polysaccharides. Nucleotides are in nucleic acids. Fatty acids are found in lipid molecules (triacylglycerols/phospholipids).
  3. What is the difference between an unsaturated and a saturated hydrocarbon? Saturated hydrocarbons contain only C-C single bonds, and unsaturated carbons contain C=C double or C≡C triple bonds.
  4. Assign each of the following compounds to one of the major classes of biomolecules: A. Amino acid B. Sugar C. Fatty acid D. Nucleotide
  1. Define the following terms: Metabolism: the sum of the chemical reactions carried out in a living cell. Nucleophile: an atom or group with an unshared pair of electrons that is involved in a nucleophilic substitution reaction. Reductionism: the belief that complex processes can be understood by examining their simpler parts. Electrophile: an electron deficient species. Energy: The ability to do work.
  2. What are the primary functions of metabolism? Primary functions of metabolism are acquisition and utilization of energy, synthesis of biomolecules and removal of waste.
  3. Give an example of each of the following reaction processes: Nucloephilic substitution: A reaction in which a nucleophile bonds to a carbon atom in a molecule, displacing a leaving group. AKA: nucleophilic displacement. Elimination: A chemical reaction involving elimination of some portion of a reactant compound, with the production of a second compound. Oxidation-reduction: A chemical reaction in which an atom or ion loses electrons to another atom or ion. Addition: A type of reaction of unsaturated hydrocarbons with hydrogen, halogens, halogen acids, and other reagents, so that no change in valency is observed and the organic compound forms a more complex one. Thought Section: 36.Biochemical reactions have been viewed as exotic versions of organic reactions. How do biochemical reactions differ from those used in organic synthesis? The assumption that the biochemical processes in prokaryotes and eukaryotes are similar is safe only when we consider basic living processes (ie glycolysis, and the general principles of genetic inheritance ). Living organisms are so diverse in their adaptations that information acquired from research with prokaryotes must be judiciously interpreted in reference to eukaryotes.
  4. The bases of two complementary DNA chains pair with each other because of hydrogen bonding; that is: Thymine-adenine base pair
  1. Describe how you would prepare a 0.1 M phosphate buffer with a pH of 7.2. What ratio of conjugate base of acid would you use?
  2. Which of the followings compounds can form hydrogen bonds with like molecules or with water? a. b. c. d.
  3. What is the osmolarity of a 1.3M solution of sodium phosphate (NaPO4)? Assume 85% ionization for this solution.
  4. A dialysis bag containing a 3M solution of the sugar fructose is placed in the following solutions. In each case, give the direction in which the water flows. A. 1M sodium lactate B. 3Msodium lactate C. 4.5 M sodium lactate
  5. What interactions occur between the following molecules and ions? a. water and ammonia b. lactate and ammonium c. benzene and octane d. carbon tetrachloride and chloroform e. chloroform and diethylether
  6. A solution containing 56mg of a protein in 30mL of distilled water exerts as osmotic pressure of 0. atm at T = 25*C. Determine the molecular weight of the unknown protein.
  1. Tyrosine is an amino acid. Which atoms in this molecule can form hydrogen bonds?
  2. Which of the following molecules would you expect to have a dipole moment? a. hydrogen bond b. pH c. buffer d. osmotic pressure e. osmolytes
  3. Which of the following molecules would you expect to form micelles? a. NaCl b.CH 3 COOH C.CH 3 COO -^ NH 4 + D. CH 3 (CH 2 ) 10 COO -^ NA+ E. CH 3 (CH 2 ) 10 CH 3
  4. Briefly define: Isotonic Amphipathic Hydrophobic interactions Dipole Induced dipole
  5. Bicarbonate is one of the main buffers of the blood and phosphate is the main buffer of the cells. Why might this be?
  6. Describe how you can increase the buffering capacity of a 0.1M acetate buffer.
  7. Which of the following molecules or ions are weak acids? Explain. A. HCl B.H 2 PO 4 - C.CH 3 COOH D.HNO 3 E. HSO 4 –
  8. Briefly define: Electrostatic interaction
  1. Determine the pH of a solution composed of 1M acetic acid and 1M sodium acetate.
  2. What would be the pH of the solution in Q30 is 1mL of 1M HCl is added?
  3. What would be the pH of 1L of water is 1mL HCl is added? Thought: 46. In many cells that can survive severe dehydration, certain sugars replace water. These sugars interact with and protect membrane surfaces and prevent protein aggregation. What structural feature of the sugar molecules is responsible for this phenomenon? Ch4 Review:
  4. Which of the following reactions could be driven by coupling to the hydrolysis of ATP? (The ∆ G*’ value for each reaction is indicated in parenthesis in units of kilojoules per mole.) ATP + H 2 O ---- ADP + P (^) i (30.5) A. Pyruvate + P (^) i  phosphoenolpyruvate (+31.7) B. Glucose + P (^) i  glucose-6-phosphate (+13.8) C. Acetic acid -- acetic anhydride (+99.6) D. Glycylglycine + water - 2 glycine (-9.2)
  5. Define: dissipative structure Respiration Electron donor High-quality energy Resonance hybrid
  1. The following reaction is catalyzed by the enzyme glutamine synthase: ATP + glutamate + NH3 ---- ADP + Pi + glutamine Use the following equations (with ∆ G’ values given in kJ/mol) to calculate ∆ G’ for the overall reaction. ATP + H2O -- ADP + P (^) i (-30.5) Glutamine + H 2 O -- glutamate + NH 3 (-14.2)
  2. Under standard conditions, which statements are true? a. ∆ G = ∆ G* b. ∆ H = ∆ G c. ∆ G’ = ∆ G + RTlnKEQ d. ∆ G* = ∆ H – T ∆ S e. P = 1atm f. T = 273 K g. [reactants} = [products] = 1M
  3. Which of the following compounds would you expect to liberate the least free energy when hydrolyzed? Explain. a. ATP b. ADP c. AMP d. phosphoenolpyruvate e. phosphocreatine 2
  4. Describe why ATP, the molecule that serves as the energy currency for the body, has an intermediate phosphoryl group transfer potential.
  5. Methanococcus janaschii obtains energy by converting carbon dioxide to methane: CO 2 + 4H 2 --- CH 4 + 2H 2 O Considering that CO 2 has a lower energy content than CH 4 , how does the organism accomplish this conversion?
  6. Magnesium ion (Mg 2 +) forms complexes with the negative charges of the phosphate in ATP. In the absence of Mg 2 +, would ATP have more, less or the same stability as when the ion is present?