AP Biology: Chapter 2-4 Take Home Quiz
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AP Biology: Chapter 2-4 Take Home Quiz
Directions: Please choose the best answer and mark all answers directly on your quiz. Each question is worth 1 point.
Chapter 2 Questions
1. A covalent bond is likely to be polar when
A) one of the atoms sharing electrons is much more electronegative than the other atom.
B) the two atoms sharing electrons are equally electronegative.
C) the two atoms sharing electrons are of the same element.
D) it is between two atoms that are both very strong electron acceptors.
E) the two atoms sharing electrons are different elements
Questions 3-6 refer to Figure 2.1.
2. Which diagram depicts the electron configuration of neon (2010Ne)?
3. The reactive properties or chemical behavior of an atom depend on the number of
A) valence shells in the atom.
B) orbitals found in the atom.
C) electrons in each orbital in the atom.
D) electrons in the outer valence shell in the atom.
E) hybridized orbitals in the atom.
4. What are the chemical properties of atoms whose valence shells are filled with electrons?
A) They form ionic bond in aqueous solutions.
B) They form covalent bond in aqueous solutions.
C) They are stable and unreactive.
D) They exhibit similar chemical behaviors.
E) Both C and D are correct.
Use the information extracted from the periodic table in Figure 2.2 to answer question 9.
5. Based on electron configuration, which of these elements would exhibit chemical behavior most like that of oxygen?
A) C B) H C) N D) S E) P
6. What results from the chemical reaction illustrated in Figure 2.3?
A) a cation with a net charge of +1
B) a cation with a net charge of -1
C) an anion with a net charge of +1
D) an anion with a net charge of -1
E) Both A and D are correct.
7. The ionic bond of sodium chloride is formed when
A) chlorine gains an electron from sodium.
B) sodium and chlorine share an electron pair.
C) sodium and chlorine both lose electrons from their outer valence shells.
D) sodium gains and electron from chlorine.
E) chlorine gains a proton from sodium.
8. Nitrogen (N) is much more electronegative than hydrogen (H). Which of the following statements is correct about the atoms in ammonia (NH3)?
A) Each hydrogen atom has a partial positive charge.
B) The nitrogen atom has a strong positive charge.
C) Each hydrogen atom has a slight negative charge.
D) The nitrogen atom has a partial positive charge.
E) There are covalent bonds between the hydrogen atoms.
9. Van der Waals interactions result when
A) atoms and molecules are very close together.
B) covalent bonds are present.
C) molecules held by ionic bonds react with water.
D) two polar covalent bonds react.
E) a hydrogen atom loses an electron.
10. Which of the following is not considered to be a weak molecular interaction?
A) covalent bond
B) van der Waals interactions
C) ionic bond in the presence of water
D) hydrogen bond
E) Both A and B are correct.
11. The mass number of an element can be easily approximated by adding together the number of
A) protons and neutrons.
B) electron orbitals in each energy level.
C) protons and electrons.
D) neutrons and electrons.
E) isotopes of the atom.
12. The atomic number of neon is 10. Therefore, it
A) has 8 electrons in the outer electron shell.
B) is inert.
C) has an atomic mass of 10.
D) Only A and B are correct.
E) A, B, and C are correct.
13. Which of the following best describes the relationship between the atoms described below?
Atom 1 Atom 2
3115P 3215P
A) They are both radioactive.
B) They are both phosphorous cations.
C) They are both phosphorous anions.
D) They are both isotopes of phosphorous.
E) They contain 31 and 32 protons respectively.
14. Which four elements make up approximately 96% of living matter?
A) carbon, hydrogen, nitrogen, oxygen
B) carbon, sulfur, phosphorous, hydrogen
C) oxygen, hydrogen, calcium, sodium
D) carbon, sodium, chlorine, magnesium
E) carbon, oxygen, sulfur, calcium
Chapter 3 Questions
15. The four emergent properties of water that are important for life are:
A) Cohesion, expansion upon freezing, high heat of evaporation, and capillarity
B) Cohesion, moderation of temperature, expansion upon freezing, and solvent properties
C) Moderation of temperature, solvent properties, high surface tension, and capillarity
D) Heat of vaporization, high specific heat, high surface tension, and capillarity
E) Polarity, hydrogen bonding, high specific heat, and high surface tension
16. Which one of the following hypothetical changes in a water molecule would tend to make it more polar?
A) It is a linear molecule, as in H-O-H.
B) Adjacent water molecules form covalent bonds with each other.
C) The electronegativity values for H is increased.
D) The electronegativity value for O is increased.
E) All of the above would make water more polar.
17. Water has an unusually high specific heat. This is directly related to which one of the following?
A) At its boiling point, water changes from liquid to vapor.
B) More heat is required to raise the temperature of water.
C) Ice floats in liquid water.
D) Salt water freezes at a lower temperature than pure water.
E) Floating ice can insulate bodies of water.
18. Which of the following explains what is happening when sodium chloride dissolves in water?
A) More hydrogen bonds are forming between water molecules.
B) Sodium and chloride atoms are separating from one another.
C) Hydration shells are forming around the sodium and chloride ions.
D) Covalent bonds are breaking and re-forming.
E) Nonpolar substances are mixing with polar substances.
19. Surfactants reduce surface tension of a liquid. Which of the following would result if water was treated
with surfactants?
A) Surfactant-treated water droplets will form a thin film instead of beading on a waxed surface.
B) Surfactant-treated water will form smaller droplets when dripping from a sink.
C) Water striders will sink.
D) All of the above will occur
E) Only a and c will occur.
20. Predict how life on earth would be different if water were less polar. Which one of the following would
result if organisms lived in and consisted of a less polar medium than water?
A) Heavier insects than water striders would be able to walk on the surface of a pond.
B) Increased cohesion would contribute to increased upward water transport in plants.
C) The water temperature of ponds and pools would increase more slowly when in sunlight.
D) Sweating would be a less effective means of keeping cool.
E) More salts would go into the solution in blood and body fluids.
21. In a lake, mineral nutrients accumulate at the bottom while dissolved oxygen is greater near the surface.
These nutrients can be mixed during water turnover that occurs with annual temperature changes.
Which one of the following properties of water explains this turnover?
A) Individual water molecules move less vigorously as water cools.
B) Hydrogen bonds among water molecules form a crystal lattice at 0°C.
C) The density of water is greatest at 4°C.
D) Water changes from liquid to solid at 0°C.
E) The distance between water molecules is greater in ice than in liquid form.
22. A calorie is defined as:
A) The amount of energy required to raise the temperature of 1 gram of water by 1 degree F.
B) The amount of energy required to raise the temperature of 1 gram of water by 1 degree C.
C) The amount of energy released by metabolism of one gram of glucose.
D) The amount of energy contained in one gram of fat.
E) The amount of energy required to raise the temperature of 1 liter of water by 1 degree C.
23. To make a 1 M solution of calcium chloride (CaCl2), you would place how many gm of CaCl2 into a
container and then add how much pure water?
[mass of a Ca atom = 40; mass of a Cl atom = 35;
mass of an O atom = 16; mass of an H atom = 1]
A) 75 gm of CaCl2 then add 1 liter of water
B) 110 gm of CaCl2 then add 1 liter of water
C) 128 gm of CaCl2 then add 1 liter of water
D) 75 gm of CaCl2 then add water to make a total volume of 1 liter
E) 110 gm of CaCl2 then add water to make a total volume of 1 liter
24. In humans, blood pH is around 7.4, and a decrease in blood pH to 6.4 would be fatal. A drop by 1 pH unit
represents which of these?
A) 1/10 as many H+ ions in the solution
B) 1/7 as many H+ ions in the solution
C) 1/2 as many H+ ions in the solution
D) twice as many H+ ions in the solution
E) ten times as many H+ ions in the solution
25. The chemical equilibrium between carbonic acid and bicarbonate acts as a pH regulator in our blood. If
the blood pH begins to rise, what will happen?
H2CO3 ↔ HCO3- + H+
Carbonic acid Bicarbonate ion Hydrogen ion
A) reaction proceeds to the right; more carbonic acid dissociates
B) reaction proceeds to the right; more carbonic acid forms
C) reaction proceeds to the left; more carbonic acid dissociates
D) reaction proceeds to the left; more carbonic acid forms
26. Scientists are concerned about increased concentrations of atmospheric carbon dioxide due to increased
fossil fuel combustion and deforestation. In addition to major effects on global temperatures, increased
levels of CO2 can threaten aquatic organisms in which way?
A) forming more carbonic acid in a solution that raises the pH of seawater
B) forming more carbonic acid that decreases the concentration of carbonate ions in seawater
C) increasing photosynthesis rates in aquatic plants and algae
D) decreasing the oxygen available for cellular respiration in aquatic organisms
E) increasing the levels of harmful sulfur oxides and nitrous oxides
Chapter 4 Questions
27. What functional group is commonly used in cells to transfer energy from one organic molecule to
another?
A) carboxyl
B) sulfhydryl
C) hydroxyl
D) phosphate
E) amino
28. The Miller-Urey experiment, shown below,
A) showed that the conditions of early Earth were inhospitable to life
B) demonstrated that amino acids and other organic molecules form under conditions that may have existed on Earth before life began
C) proved that life could originate from inorganic chemicals
D) both B and C
29. Based on carbon’s valence (4), how many different molecular shapes can be made from 6 carbons?
A) 1
B) 2
C) 4
D) 6
E) More than 6
30. Silicon (atomic number 14, atomic weight 28) is in the same column as carbon in the periodic table of the
elements (Group IV). Why isn’t life on Earth based on silicon, instead of carbon?
A) Silicon is far more rare than carbon in the Earth’s crust
B) Silicon cannot form polar covalent bonds with oxygen
C) Silicon has a different valence than carbon
D) Silicon compounds often have very different physico-chemical properties than the analogous carbon compounds
E) Silicon is not present in the environment in a form that can be used by living organisms
31. How many isomers can you make from the molecular formula C6H12O6?
A) 1
B) 2
C) 4
D) 6
E) more than 6
32. Given a chemical formula for an organic molecule, (e.g., C6H12O6), one can usually deduce its
A) Structure
B) Molecular weight
C) Solubility in water
D) All of the above
E) Molecular weight and solubility in water
33. Is this molecule soluble in water?
A) yes
B) no
34. Compared to a carbon atom with only single covalent bonds, a carbon with a double bond
A) Shares fewer electron pairs with other atoms
B) Is more flexible in the spatial arrangement of its bonds
C) Has a planar configuration of its electron orbitals rather than a tetrahedral configuration
D) Is more polar