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Biology Exam I - Principles of Biology 2009 - Prof. Andrew M. Smith, Exams of Biology

Ithaca CollegeBiology
Prof. Andrew M. Smith

This document consists of a biology exam from the principles of biology course held in 2009. The exam includes multiple choice questions covering various topics such as atomic structure, isotopes, hydrogen bonds, ionic bonds, electronegativity, amino acids, proteins, enzymes, and ph. The questions require identifying the number of electrons in the outer shell and bonds carbon likes to make, the atomic composition of deuterium, the behavior of d2o in hydrogen bonds, the number of bonds sulfur likes to make, the reactivity of sodium metal, the properties of ionic bonds and water, the formation of hydrogen bonds between water and ammonia, the diffusion of compounds through cell membranes, and the electronegativity of atoms.

Typology: Exams

2009/2010

Uploaded on 12/10/2010

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Principles of Biology 2009 - Exam I
Name _________________________________ September 17, 2009
For each multiple choice question, choose the BEST ANSWER (2.5 pts each)
1. How many electrons are in carbon’s OUTER SHELL and how many bonds does carbon like to make?
a. 6, 6
b. 12,6
c. 4, 4
d. 6, 4
e. 4, 6
2. Deuterium is known as a heavy stable isotope of Hydrogen. Its atomic mass is 2. How many protons,
neutrons and electrons respectively does Deuterium have?
a. 1, 2, 2
b. 1, 2, 1
c. 1, 1, 1
d. 2, 1, 1
e. 1, 2, 3
3. Deuterium can be used to label water as D
2
O and can be used to follow the behavior of water in various
reactions. Which of the following statements is TRUE?
a. D
2
O can make hydrogen bonds.
b. D
2
O will not make hydrogen bonds.
c. The D-O bonds are nonpolar.
d. The D-O bonds are ionic.
4. How many bonds does sulfur like to make given its electron shell properties and location in the periodic
table?
a. None, S is inert
b. One
c. Two
d. Three
e. Four
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Partial preview of the text

Download Biology Exam I - Principles of Biology 2009 - Prof. Andrew M. Smith and more Exams Biology in PDF only on Docsity!

Principles of Biology 2009 - Exam I

Name _________________________________ September 17, 2009

For each multiple choice question, choose the BEST ANSWER (2.5 pts each)

  1. How many electrons are in carbon’s OUTER SHELL and how many bonds does carbon like to make? a. 6, 6 b. 12, c. 4, 4 d. 6, 4 e. 4, 6
  2. Deuterium is known as a heavy stable isotope of Hydrogen. Its atomic mass is 2. How many protons, neutrons and electrons respectively does Deuterium have? a. 1, 2, 2 b. 1, 2, 1 c. 1, 1, 1 d. 2, 1, 1 e. 1, 2, 3
  3. Deuterium can be used to label water as D 2 O and can be used to follow the behavior of water in various reactions. Which of the following statements is TRUE? a. D 2 O can make hydrogen bonds. b. D 2 O will not make hydrogen bonds. c. The D-O bonds are nonpolar. d. The D-O bonds are ionic.
  4. How many bonds does sulfur like to make given its electron shell properties and location in the periodic table? a. None, S is inert b. One c. Two d. Three e. Four
  1. Why is sodium metal explosive (very reactive with other molecules like O 2 )? a. An electron in sodium is unstable and is donated to neutralize charge b. Sodium is highly electronegative c. The protons in sodium are heavy d. The neutrons make the nucleus unstable. e. An electron is readily lost to complete its outer shell
  2. An ionic bond a. can only be broken by the input of energy b. is stronger when not in a polar solvent like water c. involves the sharing of electrons between the two atoms d. all of the above e. none of the above
  3. Water a. Is a nonlinear molecule. b. Has a dipole. c. Has polar bonds. d. Has surface tension due to Hydrogen bonds. e. All of the above
  4. Water and ammonia can form hydrogen bonds in solution. Hydrogen bonds can be found between a. An H in H 2 O and an H in NH 3 b. The N in NH 3 and the O in H 2 O c. An H in H 2 O and an H in H 2 O d. An H in H 2 O and the N in NH 3 e. The O in H 2 O and the N in NH 3
  5. Which of the following compounds will most readily diffuse through the hydrophobic or non-polar region of a typical cell membrane?

a. CH 3 (CH 2 ) 3 – OH

O  b. CH 3 – C – NH 2

O  c. H 2 N – CH – C  OH

d. HO – (CH 2 ) 3 – OH

  1. Electronegativity of an atom is due primarily to a. The pull of protons in the nucleus on orbiting electrons b. The number of extra neutrons c. Electron spin d. Gravity e. None of the above f. All of the above
  1. Which of the following statements is consistent with a model for cell membranes, which states that phospholipids move freely around within a phospholipid plane that surrounds a cell? a. Saturated fatty acids decrease membrane fluidity b. Cholesterol is hydrophilic and will not insert into membranes and will therefore have no effect. c. Cellulose is known to stiffen membranes resulting in hard structures like wood. d. Glucose is hydrophobic and will decrease membrane fluidity by inserting into membranes e. none of the above
  2. Based on its R group, which of the following amino acids is polar?(see chart at end) a. Alanine b. Phenylalanine c. Proline d. Valine e. Serine
  3. In a protein, a single amino acid, phenylalanine, is substituted with asparagine. Which of the following statements regarding this substitution is FALSE?

Phenylalanine Asparagine

a. This substitution results in a change in the primary protein structure. b. The substitutes a nonpolar R group with a polar R group. c. There is likely to be no change in the protein folding because the R groups are the same size d. All of the above statements are true e. All of the above statements are false

  1. The secondary structure of a protein a. is due to the interaction between distinct polypeptide chains b. is made of coils and sheets c. is the side chain sequence d. is globular e. none of the above
  2. In a polypeptide chain, what type of bonding best describes that between the double-bonded oxygen in a carboxyl group and a hydrogen on an amine group? a. Peptide bond b. Covalent bond c. Ionic bond d. Hydrogen bond e. Hydrophobic interaction
  3. Living systems are very sensitive to changes in pH. If you have a solution of pH 7 what is the [H+] concentration? a. 10 -7^ M b. 10 -14M c. 7M d. 70M e. none of the above

O

NH 2

OH

O

O

H 2 N

NH 2

OH

  1. In human blood, the pH normally only varies from 7.39 – 7.42. Large changes in pH are prevented by a. the release of hydroxide ions from proteins b. the ability of carbonic acid (H 2 CO 3 /HCO 3 - ) to buffer changes in H+^ concentration c. the fact that H+^ is not released into the bloodstream d. all of the above e. none of the above
  2. Which answer best describes how pH affects enzyme activity? a. It changes the bond affinity between amino acids resulting in changes in the primary structure of a protein b. It changes the solubility and accessibility of R groups due to changes in charge c. It specifically disrupts hydrophobic interactions formed between amino acid R-groups d. none of the above
  3. Many things can alter enzyme activity. Which of the following underlie all types of enzyme regulation? a. Changes in the activation energy of the reaction b. Changes in the active site of the enzyme c. Changes in the free energy of the reaction d. All of the above
  4. Allosteric enzyme regulators a. Bind to the active site of the enzyme b. Bind to the substrate c. Bind to a regulatory site on the enzyme d. Bind to co-factors that stimulate the enzyme e. Do not bind to the enzyme
  5. If a reaction is to occur spontaneously a. There must be an increase in heat production b. There must be a decrease in entropy c. The free energy of the product must be less than the free energy of the initial d. None of the above
  6. The oxidation of glucose to form carbon dioxide and water demonstrates the following properties: a. The ∆G is positive b. The reaction is spontaneous c. The reaction will occur within 5 minutes at physiological temperature and pH d. A and B are true e. A, B and C are true
  7. Which of the following statements about ATP is FALSE? a. ATP provides the energy to power reactions that would not occur spontaneously. b. ATP provides energy in useable quantities for cellular reactions c. ATP is regenerated through cellular metabolism d. ATP catalyzes reactions by phosphorylating enzymes
  1. Which of the 4 types of biological macromolecules is this one? (1pt)

Draw and explain in one sentence how these molecules will behave in an aqueous solution given their shape and structure. (4pts)

  1. Remarkably, the disease Sickle Cell Anemia is due to a single amino acid change in the protein hemoglobin. This change leads to a dramatic change in red blood cell shape from being round to sickle- like, leading to painful clotting in the joints. The specific change is from a glutamic acid to a valine. Hemoglobin is a 4 subunit protein. What type of bonds are most likely to have been disrupted? Which of the 4 different levels of protein structures may have been changed? (5 points)
  2. When ATP and water interact, they form ADP and phosphate and a large amount of free energy is released; that is ∆G for this reaction is negative. Why does this reaction proceed very slowly when ATP is kept in aqueous (water) solution in the laboratory? (5 pts)
  1. For the following reaction:

Sucrose Glucose + Fructose Sucrase

Draw the expected enzyme activity response of sucrase over a temperature range from 10oC to 60oC , using the graph below. Be sure to label the axes appropriately (5 pts).