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AP Biology Quiz 1 Ch. 2,3

18 Questions
AP Biology Quizzes & Trivia

Quiz 1 in AP Biology for Ch. 2,3 in Reece and Campbell book.

Questions and Answers
  • 1. 
    Which of the following best explains the distinction between biology and chemistry?
    • A. 

      Biologists study living things, whereas chemists study nonliving things

    • B. 

      Biology has a hierarchy of structural levels, whereas chemistry does not

    • C. 

      Chemists study molecules, whereas biologists do not

    • D. 

      Chemical systems have emergent properties; biological systems do not

    • E. 

      There is no clear distinction because the two sciences are parts of the same whole

  • 2. 
    • A. 

      O=C-H

    • B. 

      H H I I H-O-C-C=O I H

    • C. 

      H H I I H-C-H-C=O I H

    • D. 

      O I H-N-H

  • 3. 
    What bond does NH4 form wilt Cl to make ammonium chloride salt?
    • A. 

      Nonpolar covalent bond

    • B. 

      Polar covalent bond

    • C. 

      Ionic bond

    • D. 

      Hydrogen bond

    • E. 

      Covalent bond

  • 4. 
    Which of the following best describes the relationship between the atoms described below?     Atom 1          Atom 2      1H                  3H      1                    1
    • A. 

      They are isomers.

    • B. 

      They are polymers.

    • C. 

      They are isotopes

    • D. 

      They are ions.

    • E. 

      They are both radioactive.

  • 5. 
    What do the four elements most abundant in life-carbon, oxygen, hydrogen, and nitrogen-have in common?
    • A. 

      They all have the same number of valence electrons.

    • B. 

      Each element exists only in one isotopic form.

    • C. 

      They are equal in electronegativity.

    • D. 

      They are elements produced only by living cells.

    • E. 

      They all have unpaired electrons in their valence shells,

  • 6. 
    What are the chemical properties of atoms whose valence shells are filled with electrons?
    • A. 

      They form ionic bonds in aqueous solutions.

    • B. 

      They form covalent bonds in aqueous solutions.

    • C. 

      They are stable and unreactive

    • D. 

      They exhibit similar chemical behaviors

    • E. 

      Both C and D are correct.

  • 7. 
    What are the maximum number of covalent bonds an element with atomic number 16 can make with hydrogen?
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      4

    • E. 

      5

  • 8. 
    Oxygen has an atomic number of 8. Therefore, it must have
    • A. 

      8 protons

    • B. 

      8 electrons

    • C. 

      16 neutrons

    • D. 

      Only A and B are correct.

    • E. 

      A, B, and C are correct.

  • 9. 
    Which of the following best describes chemical equilibrium?
    • A. 

      Reactions continue with no effect on the concentrations of reactants and products.

    • B. 

      Concentrations of products are high.

    • C. 

      Reactions have stopped.

    • D. 

      Reactions stop only when all reactants have been converted to products.

    • E. 

      There are equal concentrations of reactants and products.

  • 10. 
    If the pH of a solution is increased from pH 8 to pH 9, it means that
    • A. 

      Concentration of H+ is 10 times greater than what it was at pH 8.

    • B. 

      Concentration of H+ is 100 times less than what it was at pH 8.

    • C. 

      Concentration of OH- is 10 times greater than what it was at pH 8.

    • D. 

      Concentration of OH- is 100 times greater than what it was at pH 8.

    • E. 

      Concentration of H+ is greater and the concentration of OH- is less than at pH 8.

  • 11. 
    What is the maximum number of hydrogen bonds a water molecule acan form with neighboring water molecules?
    • A. 

      One

    • B. 

      Two

    • C. 

      Three

    • D. 

      Four

    • E. 

      Five

  • 12. 
    Which bonds must be broken for water to vaporize?
    • A. 

      Ionic bonds

    • B. 

      Nonpolar covalent bonds

    • C. 

      Polar covalent bonds

    • D. 

      Hydrogen bonds

    • E. 

      Both C and D are correct.

  • 13. 
    One of the buffers that contribute to pH stability in human blood is carbonic acid (H2CO3). Carbonic acid is a weak acid that dissociates into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). Thus,H2CO3 <--> HCO3- + H+ If the pH of the blood drops, one would expect
    • A. 

      A decrease in the concentration of H2CO3 and an increase in the concentration of HCO3-.

    • B. 

      The concentration of hydroxide ion (OH-) to increase.

    • C. 

      The concentration of bicarbonate ion (HCO3-) to increase.

    • D. 

      The HCO3- to act as a base and remove excess H+ with the formation of H2CO3.

    • E. 

      The HCO3- to act as an acid and remove excess H= with the formation of H2CO3.

  • 14. 
    When an ice cube cools a drink 1 degree C, which of the following is true?
    • A. 

      Molecule collisions in the drink increase.

    • B. 

      Kinetic energy in the drink decreases.

    • C. 

      A kilocalorie of heat is transferred to the water.

    • D. 

      A kilocalorie of heat is transferred to the ice.

    • E. 

      Exaporation of the water increases.

  • 15. 
    Which of the following statements is completely correct?
    • A. 

      H2CO3 is a weak acid, and NaOH is a weak base

    • B. 

      H2CO3 is a strong acid, and NaOH is a strong base.

    • C. 

      NH3 is a weak base and, and H2CO3 is a strong acid.

    • D. 

      NH3 is a strong base, and HCl is a weak acid.

    • E. 

      NH3 is a weak base, and HCl is a strong acid.

  • 16. 
    Which of the following ionizes completely in solution and is therefore a strong base?
    • A. 

      NaOH

    • B. 

      HCl

    • C. 

      NH3

    • D. 

      H2CO3

    • E. 

      NaCl

  • 17. 
    Buffers are substances that help resist shifts in pH by
    • A. 

      Releasing H+ in acidic solutions.

    • B. 

      Releasing H+ in basic solutions.

    • C. 

      Releasing OH- in basic solutions.

    • D. 

      Combining with OH- in acidicsolutions.

    • E. 

      Combining with H+ in basic solutions.

  • 18. 
    Whater's high specific heat is mainly a consequence of the
    • A. 

      Small size of the water molecules.

    • B. 

      High specific heat of oxygen and hydrogen atoms.

    • C. 

      Absorption and release of heat when hydrogen bonds break and form.

    • D. 

      Fact that water is a poor heat conductor.

    • E. 

      Inability of water to dissapate heat into dry air.