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Biology 102 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q 
About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living matter? 
A) carbon, sodium, hydrogen, nitrogen 
B) carbon, oxygen, phosphorus, hydrogen 
C) oxygen, hydrogen, calcium, nitrogen 
D) carbon, hydrogen, nitrogen, oxygen 
E) carbon, oxygen, nitrogen, calcium
A

D

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2
Q 
Trace elements are those required by an organism in only minute quantities. Which of the following is a trace element that is required by humans and other vertebrates, but not by other organisms such as bacteria or plants? 
A) nitrogen 
B) calcium 
C) iodine 
D) sodium 
E) phosphorus
A

C

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3
Q

Which of the following statements is false?
A) Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements of living matter.
B) Some trace elements are very abundant on Earth.
C) Virtually all organisms require the same elements in the same quantities.
D) Iron is an example of an element needed by all organisms.
E) Other than some trace elements, animals are mostly made up of the same elements as plants, in similar proportions.

A

C

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4
Q

Which of the following statements is false?
A) Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements of living matter.
B) Some trace elements are very abundant on Earth.
C) Virtually all organisms require the same elements in the same quantities.
D) Iron is an example of an element needed by all organisms.
E) Other than some trace elements, animals are mostly made up of the same elements as plants, in similar proportions.

A

E

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5
Q

Why is each element unique and different from other elements in chemical properties?
A) Each element has a unique atomic mass.
B) Each element has a unique atomic weight.
C) Each element has a unique number of protons in its nucleus.
D) Each element has a unique number of neutrons in its nucleus.
E) Each element has different radioactive properties.

A

C

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6
Q

Knowing just the atomic mass of an element allows inferences about which of the following?
A) the chemical properties of the element
B) the number of protons in the element
C) the number of neutrons in the element
D) the number of protons plus neutrons in the element
E) both the number of protons and the chemical properties of the element

A

D

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7
Q

In what way are elements in the same column of the periodic table the same?
A) They have the same number of protons.
B) They have the same number of neutrons.
C) They have the same number of electrons.
D) They have the same number of electrons in their valence shell.
E) They have the same number of electron shells.

A

D

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8
Q 
Oxygen has an atomic number of 8 and a mass number of 16. Thus, what is the atomic mass of an oxygen atom? 
A) exactly 8 grams 
B) exactly 8 daltons 
C) approximately 16 grams 
D) approximately 16 daltons 
E) 24 amu (atomic mass units)
A

D

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9
Q

The nucleus of a nitrogen atom contains 7 neutrons and 7 protons. Which of the following is a correct statement concerning nitrogen?
A) The nitrogen atom has a mass number of approximately 7 daltons and an atomic mass of 14.
B) The nitrogen atom has a mass number of approximately 14 daltons and an atomic mass of 7.
C) The nitrogen atom has a mass number of 14 and an atomic mass of 7 grams.
D) The nitrogen atom has a mass number of 7 and an atomic number of 14.
E) The nitrogen atom has a mass number of 14 and an atomic mass of approximately 14 daltons.

A

E

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10
Q

Molybdenum has an atomic number of 42. Several common isotopes exist, with mass numbers of 92, 94, 95, 96, 97, 98, and 100. Therefore, which of the following can be true?
A) Molybdenum atoms can have between 50 and 58 neutrons.
B) The isotopes of molybdenum have different electron configurations.
C) The isotopes of molybdenum can have between 50 and 58 protons.
D) The isotopes of molybdenum have between 50 and 58 neutrons and have different electron configurations.
E) The isotopes of molybdenum have between 50 and 58 protons and have different electron configurations.

A

A

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11
Q

Carbon-12 is the most common isotope of carbon, and has an atomic mass of 12 daltons. A mole of carbon in naturally occurring coal, however, weighs slightly more than 12 grams. Why?
A) The atomic mass does not include the mass of electrons.
B) Some carbon atoms in nature have an extra proton.
C) Some carbon atoms in nature have more neutrons.
D) Some carbon atoms in nature have a different valence electron distribution.
E) Some carbon atoms in nature have undergone radioactive decay.

A

C

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12
Q

The precise weight of a mole of some pure elements like silicon (Si) can vary slightly from the standard atomic mass, or even from sample to sample. Why?
A) The element may undergo radioactive decay.
B) The element may react with itself and gain or lose subatomic particles.
C) The atoms of the element form chemical bonds with each other, and that changes the weight of the element.
D) The element may have multiple stable isotopes, and the isotopic composition may vary from sample to sample.
E) The amount of energy absorbed by the element affects the mass of its electrons, and thus the atomic mass can vary slightly.

A

D

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13
Q

One difference between carbon-12 (12/6 C) is that carbon-14 (14/6 C) has
A) two more protons than carbon-12.
B) two more electrons than carbon-12.
C) two more neutrons than carbon-12.
D) two more protons and two more neutrons than carbon-12.
E) two more electrons and two more neutrons than carbon-12.

A

C

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14
Q 
An atom has 6 electrons in its outer shell. How many unpaired electrons does it have? 
A) 0 
B) 2 
C) 4 
D) 6 
E) 2 or 4
A

B

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15
Q 
The atomic number of nitrogen is 7. Nitrogen-15 is heavier than nitrogen-14 because the atomic nucleus of nitrogen-15 contains how many neutrons? 
A) 6 
B) 7 
C) 8 
D) 12 
E) 14
A

C

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16
Q

Electrons exist only at fixed levels of potential energy. However, if an atom absorbs sufficient energy, a possible result is that
A) an electron may move to an electron shell farther away from the nucleus.
B) an electron may move to an electron shell closer to the nucleus.
C) the atom may become a radioactive isotope.
D) the atom would become a positively charged ion, or cation, and become a radioactive isotope.
E) the atom would become a negatively charged ion, or anion.

A

A

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17
Q

The atomic number of neon is 10. Therefore, which of the following is most correct about an atom of neon?
A) It has 8 electrons in its outer electron shell.
B) It is inert.
C) It has an atomic mass of 10 daltons.
D) It has 8 electrons in its outer electron shell and it is inert.
E) It has 8 electrons in its outer electron shell, it is inert, and it has an atomic mass of 10 daltons.

A

D

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18
Q

From its atomic number of 15, it is possible to predict that the phosphorus atom has
A) 15 neutrons.
B) 15 protons.
C) 15 electrons.
D) 8 electrons in its outermost electron shell.
E) 15 protons and 15 electrons.

A

E

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19
Q

Atoms whose outer electron shells contain 8 electrons tend to
A) form ions in aqueous solutions.
B) form hydrogen bonds in aqueous solutions.
C) be stable and chemically nonreactive, or inert.
D) be gaseous at room temperature.
E) be both chemically inert and gaseous at room temperature.

A

E

20
Q 
The atomic number of each atom is given to the left of each of the elements below. Which of the atoms has the same valence as carbon (12/6 C)? 
A) ₇N nitrogen 
B) ₉F flourine 
C) ₁₀Ne neon 
D) ₁₂Mg magnesium 
E) ₁₄Si silicon
A

E

21
Q

Two atoms appear to have the same mass number. These atoms
A) must have the same atomic number.
B) must have the same number of electrons.
C) must have the same chemical properties.
D) must have the same number of protons + neutrons.
E) must have the same atomic number, the same number of protons + neutrons, the same number of electrons, and the same chemical properties.

A

D

22
Q 
Fluorine has an atomic number of 9 and a mass number of 19. How many electrons are needed to complete the valence shell of a fluorine atom? 
A) 1 
B) 3 
C) 0 
D) 7 
E) 9
A

A

23
Q 
24) What is the maximum number of electrons in a single 2 p orbital of an atom? 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5
A

B

24
Q

An atom with atomic number 12 would have what type of chemical behavior in bonding with other elements?
A) It would form ions with a +1 charge.
B) It would form ions with a +2 charge.
C) It would form ions with a -1 charge.
D) It would form ions with a -2 charge.
E) It would form two covalent bonds with other atoms.

A

B

25
Q 
What is the maximum number of covalent bonds an element with atomic number 8 can make with hydrogen? 
A) 1 
B) 2 
C) 3 
D) 4 
E) 6
A

B

26
Q

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; the nitrogen atom has a partial negative charge.
B) The nitrogen atom has a strong positive charge; each hydrogen atom has a strong positive charge.
C) Each hydrogen atom has a slight negative charge; the nitrogen atom has a strong positive charge.
D) The nitrogen atom has a slight positive charge; each hydrogen atom has a slight negative charge.
E) There are covalent bonds between the hydrogen atoms and polar bonds between each hydrogen atom and the nitrogen atom.

A

A

27
Q 
When two atoms are equally electronegative, they will interact to form 
A) hydrogen bonds. 
B) van der Waals interactions. 
C) polar covalent bonds. 
D) nonpolar covalent bonds. 
E) ionic bonds.
A

D

28
Q 
Which of the following molecules contains the most polar covalent bond? 
A) H₂ 
B) O₂ 
C) CO₂ 
D) H₂O 
E) CH₄
A

D

29
Q

In comparing covalent bonds and ionic bonds, which of the following would you expect?
A) An atom can form covalent bonds with multiple partner atoms, but only a single ionic bond with a single partner atom.
B) Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons.
C) Both involve electrical attraction between the electrons of one atom and the nucleus of the other atom.
D) Ionic interactions remain when covalent bonds are broken in water. Ionic bonds are much stronger than covalent bonds.

A

B

30
Q

What is the difference between covalent bonds and ionic bonds?
A) Covalent bonds are formed between atoms to form molecules; ionic bonds are formed between atoms to form compounds.
B) Covalent bonds involve the sharing of pairs of electrons between atoms; ionic bonds involve the sharing of single electrons between atoms.
C) Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the electrical attraction between atoms.
D) Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the sharing of protons between atoms.
E) Covalent bonds involve the transfer of electrons between atoms; ionic bonds involve the sharing of electrons between atoms.

A

C

31
Q 
In ammonium chloride salt (NH₄Cl) the anion is a single chloride ion, Cl. What is the cation of NH₄Cl? 
A) N, with a charge of +1 
B) NH, with a charge of +1 
C) H₃, with a charge of +1 
D) NH₄, with a charge of +1 
E) NH₄, with a charge of +4
A

D

32
Q 
The atomic number of chlorine is 17. The atomic number of magnesium is 12. What is the formula for magnesium chloride? 
A) MgCl 
B) MgCl₂ 
C) Mg₂Cl 
D) Mg₂Cl₂ 
E) MgCl₃
A

B

33
Q 
Which of the following explains most specifically the attraction of water molecules to one another? 
A) nonpolar covalent bond 
B) polar covalent bond 
C) ionic bond 
D) hydrogen bond 
E) hydrophobic interaction
A

D

34
Q

Van der Waals interactions result when
A) hybrid orbitals overlap.
B) electrons are not symmetrically distributed in a molecule.
C) molecules held by ionic bonds react with water.
D) two polar covalent bonds react.
E) a hydrogen atom loses an electron.

A

B

35
Q 
What bonding or interaction is most likely to occur among a broad array of molecules of various types (polar, nonpolar, hydrophilic, hydrophobic)? 
A) covalent bonding 
B) polar covalent bonding 
C) ionic bonding 
D) hydrogen bonding 
E) van der Waals interactions
A

E

36
Q

Which of the following is not considered to be a weak molecular interaction?
A) a covalent bond
B) a van der Waals interaction
C) an ionic bond in the presence of water
D) a hydrogen bond
E) both a hydrogen bond and a covalent bond

A

A

37
Q 
What is the maximum number of hydrogen atoms that can be covalently bonded in a molecule containing two carbon atoms? 
A) 2 
B) 3 
C) 4 
D) 6 
E) 8
A

D

38
Q

of the following is true for this reaction?
3 H₂ + N₂ ↔ 2 NH₃
A) The reaction is nonreversible.
B) Hydrogen and nitrogen are the reactants of the reverse reaction.
C) Hydrogen and nitrogen are the products of the forward reaction.
D) Ammonia is being formed and decomposed.
E) Hydrogen and nitrogen are being decomposed.

A

D

39
Q

Which of the following correctly describes any reaction that has reached chemical equilibrium?
A) The concentration of the reactants equals the concentration of the products.
B) The rate of the forward reaction is equal to the rate of the reverse reaction.
C) All of the reactants have been converted to the products of the reaction.
D) All of the products have been converted to the reactants of the reaction.
E) Both the forward and the reverse reactions have stopped with no net effect on the concentration of the reactants and the products.

A

B

40
Q

Which of these systems is least likely to be at chemical equilibrium?
A) a test tube of living cells
B) a test tube of organic molecules, kept in the freezer
C) a test tube of dry organic molecules, kept at room temperature
D) a test tube of organic molecules dissolved in water, kept at room temperature
E) a test tube of dead cells in water, kept at room temperature

A

A

41
Q

group of molecular biologists is trying to synthesize a new artificial compound to mimic the effects of a known hormone that influences sexual behavior. They have turned to you for advice. Which of the following compounds is most likely to mimic the effects of the hormone?
A) a compound with the same number of carbon atoms as the hormone
B) a compound with the same molecular mass (measured in daltons) as the hormone
C) a compound with the same three-dimensional shape as part of the hormone
D) a compound with the same number of orbital electrons as the hormone
E) a compound with the same number of hydrogen and nitrogen atoms as the hormone

A

C

42
Q

In the term trace element, the modifier trace means that
A) the element is required in very small amounts.
B) the element can be used as a label to trace atoms through an organism’s metabolism.
C) the element is very rare on Earth.
D) the element enhances health but is not essential for the organism’s long-term survival.
E) the element passes rapidly through the organism.

A

A

43
Q 
Compared with ³¹P, the radioactive isotope ³²P has 
A) a different atomic number. 
B) a different charge. 
C) one more proton. 
D) one more electron. 
E) one more neutron.
A

E

44
Q

The reactivity of an atom arises from
A) the average distance of the outermost electron shell from the nucleus.
B) the existence of unpaired electrons in the valence shell.
C) the sum of the potential energies of all the electron shells.
D) the potential energy of the valence shell.
E) the energy difference between the s and p orbitals.

A

B

45
Q

Which statement is true of all atoms that are anions?
A) The atom has more electrons than protons.
B) The atom has more protons than electrons.
C) The atom has fewer protons than does a neutral atom of the same element.
D) The atom has more neutrons than protons.
E) The net charge is 1-.

A

A

46
Q 
The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound: 
A) HS 
B) HS₂ 
C) H₂S 
D) H₃S₂ 
E) H₄S
A

C

47
Q 
What coefficients must be placed in the following blanks so that all atoms are accounted for in the products? 
C₆H₁₂O₆ → \_\_\_\_ C₂H₆O + \_\_\_\_ CO₂ 
A) 1; 2 
B) 3; 1 
C) 1; 3 
D) 1; 1 
E) 2; 2
A

E

Biology 102 (21 decks)

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