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Bio I Exam 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Proton

A

positively-charged subatomic particle

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2
Q

center of an atom that contains protons and neutrons

A

nucleus

(chemistry)

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3
Q

substance made up of atoms of more than one element

A

compound

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4
Q

bond between charged ions

A

Ionic Bond

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5
Q

positively-charged subatomic particle

A

Proton

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6
Q

Base

A

substance that can accept hydrogen ion in solution

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7
Q

heat of vaporization

A

energy required to convert liquid to a gas

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8
Q

solution

A

solvent and dissolved solute mixture

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9
Q

hydrophobic

A

uncharged, nonpolar groups of atoms/molecules that have no affinity for water

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10
Q
  • measure of a solution’s acidity/hydrogen ion concentration
  • -log( [H+] )
A

pH

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11
Q

hydrophillic

A

having an affinity for water; polar

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12
Q

anion

A

negatively charged ion

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13
Q

energy

A

capacity to do work or to accomplish change in physical or chemical systems

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14
Q

orbital

A

region in space surrounding nucleus in which an electron is most likely to be found

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15
Q

acid

A

substance that can release a proton in solution

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16
Q

polar

A

having opposite electric charges at two ends

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17
Q

molecule

A

chemical substance consisting of two or more atoms joined by bonds or attractions

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18
Q

reactant

A

substance that enters into a chemical reaction

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19
Q

solvent

A

liquid in which solutes are dissolved to form a solution

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20
Q

Molecular Weight

A

sum of atomic weights in a molecule

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21
Q

electron

(def)

A

negatively charged subatomic particle

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22
Q

hydrogen bond

A

weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom

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23
Q

ion

A

electrically charged particle that forms when atom gains or loses electron(s)

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24
Q

van der Waals forces

A

weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another

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25
Q

van der Waals forces

(strength)

A

bonds that are about 1/4 as strong as hydrogen bonds

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26
Q

neuton

A
  • neutrally-charged subatomic particle located in the nuclei of atoms
  • molecular weight of approx. 1 amu
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27
Q

reversible reaction

A

chemical change that can occur in both forward and reverse direction

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28
Q

electron shell

A

region in which electrons orbit; surrounding atomic nucleus at fixed energy level

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29
Q

sum of an atom’s protons and neutrons

A

mass number

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30
Q

radioisotope

A

radioactive isotope

(e.g. carbon-14, hydrogen-3, tritium)

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31
Q

substance that can accept or release hydrogen ions to resist changes in pH

A

buffer

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32
Q

amount of energy required to raise 1 gram of a substance by 1 deg C

A

specific heat

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33
Q

isotope

A

atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus

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34
Q

specific heat

A

amount of energy required to raise 1 gram of a substance by 1 deg C

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35
Q

compound

A

substance made up of atoms of more than one element

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36
Q

cohesion

A

tendency of molecules to stick together

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37
Q

element

A

substance that cannot be converted to a simpler substance

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38
Q

atomic number

A
  • equivalent to the number of protons in an atom’s nucleus (equal to electrons around atom)
  • determines chemical properties of atom
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39
Q

electronegativity

A

affinity of an atom to attract electrons when it occurs as part of a compound

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40
Q

mole

A

avogadro’s number of something

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41
Q

covalent bond

A

bond based on the (equal or unequal) sharing of electrons between two atoms

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42
Q

avogadro’s number

A

6.022 x 10^23

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43
Q

chemical bond

A

attractive force linking two atoms

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44
Q

pH

A
  • measure of a solution’s acidity/hydrogen ion concentration
  • -log( [H+] )
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45
Q

buffer

A

substance that can accept or release hydrogen ions to resist changes in pH

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46
Q

nucleus

(chemistry)

A

center of an atom that contains protons and neutrons

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47
Q

substance that can accept hydrogen ion in solution

A

Base

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48
Q

energy required to convert liquid to a gas

A

heat of vaporization

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49
Q

solvent and dissolved solute mixture

A

solution

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50
Q

uncharged, nonpolar groups of atoms/molecules that have no affinity for water

A

hydrophobic

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51
Q

radioactive isotope

(e.g. carbon-14, hydrogen-3, tritium)

A

radioisotope

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52
Q

solute

A

substance dissolved in a liquid to form a solution

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53
Q

mass number

A

sum of an atom’s protons and neutrons

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54
Q

having an affinity for water; polar

A

hydrophillic

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55
Q

negatively charged ion

A

anion

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56
Q

Ionic Bond

A

bond between charged ions

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57
Q

capacity to do work or to accomplish change in physical or chemical systems

A

energy

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58
Q

region in space surrounding nucleus in which an electron is most likely to be found

A

orbital

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59
Q

tendency of molecules to stick together

A

cohesion

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60
Q

substance that can release a proton in solution

A

acid

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61
Q

having opposite electric charges at two ends

A

polar

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62
Q

substance that cannot be converted to a simpler substance

A

element

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63
Q

chemical substance consisting of two or more atoms joined by bonds or attractions

A

molecule

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64
Q

substance that enters into a chemical reaction

A

reactant

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65
Q
  • equivalent to the number of protons in an atom’s nucleus (equal to electrons around atom)
  • determines chemical properties of atom
A

atomic number

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66
Q

liquid in which solutes are dissolved to form a solution

A

solvent

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67
Q

substance dissolved in a liquid to form a solution

A

solute

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68
Q

affinity of an atom to attract electrons when it occurs as part of a compound

A

electronegativity

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69
Q

sum of atomic weights in a molecule

A

Molecular Weight

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70
Q

avogadro’s number of something

A

mole

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71
Q

negatively charged subatomic particle

A

electron

(def)

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72
Q

bond based on the (equal or unequal) sharing of electrons between two atoms

A

covalent bond

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73
Q

weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom

A

hydrogen bond

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74
Q

positively charged ion

A

cation

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75
Q

electrically charged particle that forms when atom gains or loses electron(s)

A

ion

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76
Q

6.022 x 10^23

A

avogadro’s number

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77
Q

weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another

A

van der Waals forces

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78
Q

attractive force linking two atoms

A

chemical bond

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79
Q

bonds that are about 1/4 as strong as hydrogen bonds

A

van der Waals forces

(strength)

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80
Q
  • neutrally-charged subatomic particle located in the nuclei of atoms
  • molecular weight of approx. 1 amu
A

neuton

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81
Q

cation

A

positively charged ion

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82
Q

chemical change that can occur in both forward and reverse direction

A

reversible reaction

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83
Q

region in which electrons orbit; surrounding atomic nucleus at fixed energy level

A

electron shell

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84
Q

the (weighted) average mass numbers of a sample of atoms

A

atomic weight

85
Q

atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus

A

isotope

86
Q

atomic weight

A

the (weighted) average mass numbers of a sample of atoms

87
Q

Phosphorus has an atomic number of 15 and an atomic mass of 31. How many neutrons does phosphorus have?

A. 5
B. 16
C. 30
D. 31
E. 47

A

B

88
Q

Particles having a net negative charge are called

A. electronegative
B. cations
C. anions
D. acids
E. bases

A

C

89
Q

Which of the following correctly states an unusual property of water?

A. Water will not react with other atoms
B. Water’s solid state is denser than its liquid state.
C. Energy is not required to change water from a wolid to a liquid.
D. Little heat energy is needed to raise the temperature of water.
E. The hydrogen bonds between water molecules continually form and break.

A

E

90
Q

Polar molecules

A. have bonds with an overall positive charge.
B. have bonds with an unequal distribution of electric charge.
C. must form ions in water solution.
D. have bonds with an equal distribution of electrical charge.
E. have bonds with an overall negative charge.

A

B

91
Q

Covalent bond formation depends ont eh ability of atoms to

A. share electrons with other atoms.
B. donate electrons to other atoms.
C. receive electrons from other atoms.
D. both a and b
E. all of the above

A

A

92
Q

The element with which of the following atomic numbers would be most stable?

A. 1
B. 3
C. 12
D. 15
E. 18

A

E

93
Q

The role of a buffer is to

A. allow the pH of a solution to vary widely.
B. make a solution basic.
C. maintain pH homeostasis.
D. disrupt pH homeostasis.
E. make a solution more acidic.

A

C

94
Q

Based on the symbol for iron (Fe) shown here, select the correct list of characteristics for iron.

A. Number of protons = 26; number of electrons = 29; number of neutrons = 29
B. Number of protons = 29; number of electrons = 26; number of neutrons = 26
C. Number of protons = 26; number of electrons = 26; number of neutrons = 55
D. Number of protons = 26; number of electrons = 26; number of neutrons = 29
E. Number of protons = 55; number of electrons = 55; number of neutrons = 26

A

D

95
Q

The graph shown depicts a pH scale with the pH values of several substances indicated. Which of the following statements is false?

A. Distilled water (pH 7.0) has an equal concentration of H+ and OH– ions.
B. Baking soda (pH 9.0) has a higher concentration of H+ ions than black coffee (pH 5.0).
C. Milk of magnesia (pH 10.0) has a higher concentration of OH– ions than seawater (pH 8.0)
D. A solution with a lower pH has a higher concentration of H+ ions than a solution with a higher pH.
E. A solution with a higher pH has a higher concentration of OH– ions than a solution with a lower pH.

A

B

96
Q

Which example shown (A–E) depicts the correct distribution of charge and hydrogen bonding between two water molecules?

A
B
C
D
E

A

A

97
Q

The accompanying figure demonstrates the process of salt dissolving in water. Which of the following is not depicted?

A. Cations and anions
B. Ionic bonding
C. Hydrogen bonding
D. Solute dissolving in water
E. Hydrophobic interactions

A

E

98
Q

In comparing solid water (ice) and liquid water, select the false statement from the following choices.

A. Liquid water is less dense than solid water.
B. Solid water has a crystalline structure.
C. Hydrogen bonds hold water molecules in a rigid state in solid water.
D. In solid water, each water molecule can be hydrogen-bonded to four other water molecules.
E. Hydrogen bonds continue to break and re-form in liquid water.

A

A

99
Q

Consider the accompanying figure showing a hydrogen bond between two water molecules. Which of the following properties of water is not caused by this interaction?

A. High surface tension
B. Great cohesive strength
C. Low specific heat
D. Excellence as a solvent
E. High heat of evaporation

A

C

99
Q

Consider the carbonic acid (H2CO3) buffer system depicted in the graph shown. In this system, the following reaction (H2CO3 → HCO3– + H+) is utilized to reduce the effect of adding acid. From the following choices, select the one that makes the following statement true: In this buffer system, HCO3– is _______, H2CO3 is _______, and _______ would predominate in the system, receiving zero units of base.

A. a base; an acid; HCO3–
B. a base; an acid; H2CO3
C. an acid; a base; HCO3–
D. an acid; a base; H2CO3
E. basic; acidic; H2CO3

A
100
Q

This figure shows the radioisotope tritium. Which of the following statements regarding radioisotopes is false?

A. Radioisotopes differ from other isotopes in that they give off energy.
B. Radioisotopes can be used as a molecular “tag” for medical diagnostic purposes.
C. Radioisotopes are unstable because they contain more protons than nonradioactive forms of the same element.
D. Radioisotopes can be damaging to cells.
E. During the process of radioactive decay, radioisotopes can release energy in the form of alpha radiation.

A

C

101
Q

The part of the atom that determines how the atom behaves chemically is the

A. proton.
B. election.
C. neutron.
D. innermost shell.
E. nucleus.

A

B

103
Q

Which of the following statements about chemcial reactions is false?

A. They occur when atoms combine or change their bonding partners.
B. Reactions may go to completion.
C. The products of a chemica reaction are formed from the reactants.
D. Energy may be created or destroyed in a chemical reaction.
E. Changes in forms of energy may accompany chemical reactions.

A

D

104
Q

Refer to the periodic table. Which of the following has the same number of outer-shell (valence) electrons as oxygen?

A. S
B. N
C. F
D. Na
E. Ca

A

A

105
Q

Covalent Bonds: Given the shell configurations of hydrogen, carbon, and sulfur (shown), select a molecule from the list below that could not be formed

A. CH4
B. H–C=C–H
C. H3C–CH3
D. H–S–H
E. S=S

A

B

106
Q

Oxygen forms ___ covalent bond(s), carbon forms ___, and hydrogen forms ___.

A. 1, 4, 1
B. 4, 4, 4
C. 2, 4, 0
D. 2, 4, 1
E. 2, 2, 2

A

D

107
Q

The four most common elements in organisms are

A. Ca, Fe, H, O
B. H2O, C, H, O
C. C, O, H, N
D. N, C, Fe, H
E. P, H2O, C, O

A

C

108
Q

Atomic and Mass Numbers I: This figure shows an atom of helium. Which of the following characteristics is true for helium?

A. Mass number = 4; atomic number = 2; net charge = 0
B. Mass number = 4; atomic number = 4; net charge = 0
C. Mass number = 4; atomic number = 2; net charge = +2
D. Mass number = 6; atomic number = 2; net charge = 0
E. Mass number = 6; atomic number = 2; net charge = +1

A

A

109
Q

Chemical Reactions: Which of the following statements about the chemical reaction in the figure shown is false?

A. The reactants are to the left of the arrow.
B. The arrow represents the direction of the chemical reaction.
C. There is more potential chemical energy in the products than in the reactants.
D. The energy associated with this reaction could be measured in calories.
E. The difference in potential chemical energy in this reaction is released as heat and light.

A

C

110
Q

A basic solution contains

A. more OH- ions than H+ ions.
B. more H+ ions than OH- ions.
C. the same number of OH- ions and H+ ions.
D. no OH- ions.
E. none of the above

A

A

111
Q

Ions: Given the electron shell configuration and mass and atomic numbers for the sodium ion (Na+) shown here, select the correct choice below to complete the following sentence: The sodium ion has _______ protons in its nucleus, _______ electrons in its outermost shell, and it is a(n) _______.

A. 10; 0; anion
B. 11; 8; anion
C. 11; 0; anion
D. 10; 0; cation
E. 11; 8; cation

A

E

112
Q

Given the electron shell configuration for sulfur (S) shown, select the correct choice below to complete the following sentence: Sulfur has _______ protons in its nucleus and requires _______ more electrons to complete its outer shell.

A. 8; 2
B. 8; 6
C. 16; 2
D. 16; 6
E. 16; 8

A

C

113
Q

What determines if a molecule is polar, nonpolar, or ionic?

A. the number of protons
B. the bond distances
C. the differences in the electronegativities of the atoms
D. the ionic charges
E. the distance of the electrons from the nucleus

A

C

114
Q

The three most abundant elements in a human skin cell are

A. calcium, carbon, and oxygen.
B. carbon, hydrogen, and oxygen.
C. carbon, hydrogen, and sodium.
D. carbon, nitrogen, and potassium.
E. nitrogen, hydrogen, and argon.

A

B

115
Q

Which of the following statements about the isotopes of an element is not true?

A. They all have the same atomic number.
B. They all have the same number of protons.
C. They all have the same number of neutrons.
D. They all have the same number of electrons.
E. They all have identical chemical properties.

A

C

116
Q

The atomic weight (atomic mass) of an element

A. equals the number of neutrons in an atom.
B. equals the number of protons in an atom.
C. equals the number of electrons in an atom.
D. equals the number of neutrons plus the number of protons.
E. depends on the relative abundances of its electrons and neutrons.

A

D

117
Q

The atomic number of an element

A. equals the number of neutrons in an atom.
B. equals the number of protons in an atom.
C. equals the number of protons minus the number of neutrons.
D. equals the number of neutrons plus the number of protons.
E. depends on the isotope.

A

B

118
Q

When table salt (NaCl) is added to water,

A. a covalent bond is broken.
B. an acidic solution is formed.
C. the Na+ and Cl− ions are separated.
D. the Na+ ions are attracted to the hydrogen atoms of water.
E. water molecules surround the Na+ (but not Cl−) ions.

A

C

119
Q

Hydrophobic interactions

A. are stronger than hydrogen bonds.
B. are stronger than covalent bonds.
C. can hold two ions together.
D. can hold two nonpolar molecules together.
E. are responsible for the surface tension of water.

A

D

121
Q

The reaction HCl → H+ + Cl− in the human stomach is an example of the

A. cleavage of a hydrophobic bond.
B. formation of a hydrogen bond.
C. elevation of the pH of the stomach.
D. formation of ions by dissolving an acid.
E. formation of polar covalent bonds.

A

D

122
Q

Which of the following statements about water is not true?

A. It releases a large amount of heat when changing from liquid into vapor.
B. Its solid form is less dense than its liquid form.
C. It is the most effective solvent for polar molecules.
D. It is typically the most abundant substance in a living organism.
E. It takes part in some important chemical reactions.

A

A

123
Q

The hydrogen bond between two water molecules arises because water is

A. polar.
B. nonpolar.
C. a liquid.
D. small.
E. hydrophobic

A

A

124
Q

Which of the following statements about covalent bonds is not true?

A. A covalent bond is stronger than a hydrogen bond.
B. A covalent bond can form between atoms of the same element.
Cc. Only a single covalent bond can form between two atoms.
D. A covalent bond results from the sharing of electrons by two atoms.
E. A covalent bond can form between atoms of different elements.

A

C

125
Q

positively-charged subatomic particle

A

Proton

126
Q

nucleus

(chemistry)

A

center of an atom that contains protons and neutrons

127
Q

compound

A

substance made up of atoms of more than one element

128
Q

Ionic Bond

A

bond between charged ions

129
Q

Proton

A

positively-charged subatomic particle

130
Q

substance that can accept hydrogen ion in solution

A

Base

131
Q

energy required to convert liquid to a gas

A

heat of vaporization

132
Q

solvent and dissolved solute mixture

A

solution

133
Q

uncharged, nonpolar groups of atoms/molecules that have no affinity for water

A

hydrophobic

134
Q

pH

A
  • measure of a solution’s acidity/hydrogen ion concentration
  • -log( [H+] )
135
Q

having an affinity for water; polar

A

hydrophillic

136
Q

negatively charged ion

A

anion

137
Q

capacity to do work or to accomplish change in physical or chemical systems

A

energy

138
Q

region in space surrounding nucleus in which an electron is most likely to be found

A

orbital

139
Q

substance that can release a proton in solution

A

acid

140
Q

having opposite electric charges at two ends

A

polar

141
Q

chemical substance consisting of two or more atoms joined by bonds or attractions

A

molecule

142
Q

substance that enters into a chemical reaction

A

reactant

143
Q

liquid in which solutes are dissolved to form a solution

A

solvent

144
Q

sum of atomic weights in a molecule

A

Molecular Weight

145
Q

negatively charged subatomic particle

A

electron

(def)

146
Q

weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom

A

hydrogen bond

147
Q

electrically charged particle that forms when atom gains or loses electron(s)

A

ion

148
Q

weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another

A

van der Waals forces

149
Q

bonds that are about 1/4 as strong as hydrogen bonds

A

van der Waals forces

(strength)

150
Q
  • neutrally-charged subatomic particle located in the nuclei of atoms
  • molecular weight of approx. 1 amu
A

neuton

151
Q

chemical change that can occur in both forward and reverse direction

A

reversible reaction

152
Q

region in which electrons orbit; surrounding atomic nucleus at fixed energy level

A

electron shell

153
Q

mass number

A

sum of an atom’s protons and neutrons

154
Q

radioactive isotope

(e.g. carbon-14, hydrogen-3, tritium)

A

radioisotope

155
Q

buffer

A

substance that can accept or release hydrogen ions to resist changes in pH

156
Q

specific heat

A

amount of energy required to raise 1 gram of a substance by 1 deg C

157
Q

atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus

A

isotope

158
Q

amount of energy required to raise 1 gram of a substance by 1 deg C

A

specific heat

159
Q

substance made up of atoms of more than one element

A

compound

160
Q

tendency of molecules to stick together

A

cohesion

161
Q

substance that cannot be converted to a simpler substance

A

element

162
Q
  • equivalent to the number of protons in an atom’s nucleus (equal to electrons around atom)
  • determines chemical properties of atom
A

atomic number

163
Q

affinity of an atom to attract electrons when it occurs as part of a compound

A

electronegativity

164
Q

avogadro’s number of something

A

mole

165
Q

bond based on the (equal or unequal) sharing of electrons between two atoms

A

covalent bond

166
Q

6.022 x 10^23

A

avogadro’s number

167
Q

attractive force linking two atoms

A

chemical bond

168
Q
  • measure of a solution’s acidity/hydrogen ion concentration
  • -log( [H+] )
A

pH

169
Q

substance that can accept or release hydrogen ions to resist changes in pH

A

buffer

170
Q

center of an atom that contains protons and neutrons

A

nucleus

(chemistry)

171
Q

Base

A

substance that can accept hydrogen ion in solution

172
Q

heat of vaporization

A

energy required to convert liquid to a gas

173
Q

solution

A

solvent and dissolved solute mixture

174
Q

hydrophobic

A

uncharged, nonpolar groups of atoms/molecules that have no affinity for water

175
Q

radioisotope

A

radioactive isotope

(e.g. carbon-14, hydrogen-3, tritium)

176
Q

substance dissolved in a liquid to form a solution

A

solute

177
Q

sum of an atom’s protons and neutrons

A

mass number

178
Q

hydrophillic

A

having an affinity for water; polar

179
Q

anion

A

negatively charged ion

180
Q

bond between charged ions

A

Ionic Bond

181
Q

energy

A

capacity to do work or to accomplish change in physical or chemical systems

182
Q

orbital

A

region in space surrounding nucleus in which an electron is most likely to be found

183
Q

cohesion

A

tendency of molecules to stick together

184
Q

acid

A

substance that can release a proton in solution

185
Q

polar

A

having opposite electric charges at two ends

186
Q

element

A

substance that cannot be converted to a simpler substance

187
Q

molecule

A

chemical substance consisting of two or more atoms joined by bonds or attractions

188
Q

reactant

A

substance that enters into a chemical reaction

189
Q

atomic number

A
  • equivalent to the number of protons in an atom’s nucleus (equal to electrons around atom)
  • determines chemical properties of atom
190
Q

solvent

A

liquid in which solutes are dissolved to form a solution

191
Q

solute

A

substance dissolved in a liquid to form a solution

192
Q

electronegativity

A

affinity of an atom to attract electrons when it occurs as part of a compound

193
Q

Molecular Weight

A

sum of atomic weights in a molecule

194
Q

mole

A

avogadro’s number of something

195
Q

electron

(def)

A

negatively charged subatomic particle

196
Q

covalent bond

A

bond based on the (equal or unequal) sharing of electrons between two atoms

197
Q

hydrogen bond

A

weak electrostatic bond between slightly-positive hydrogen atom and slightly-negative charge on a nearby atom

198
Q

cation

A

positively charged ion

199
Q

ion

A

electrically charged particle that forms when atom gains or loses electron(s)

200
Q

avogadro’s number

A

6.022 x 10^23

201
Q

van der Waals forces

A

weak attractions between atoms resulting from interactions between electons of one atom and the nucleus of another

202
Q

chemical bond

A

attractive force linking two atoms

203
Q

van der Waals forces

(strength)

A

bonds that are about 1/4 as strong as hydrogen bonds

204
Q

neuton

A
  • neutrally-charged subatomic particle located in the nuclei of atoms
  • molecular weight of approx. 1 amu
205
Q

positively charged ion

A

cation

206
Q

reversible reaction

A

chemical change that can occur in both forward and reverse direction

207
Q

electron shell

A

region in which electrons orbit; surrounding atomic nucleus at fixed energy level

208
Q

atomic weight

A

the (weighted) average mass numbers of a sample of atoms

209
Q

isotope

A

atom containing same number of protons as shown in the periodic table, but differing in the number of neutrons within the nucleus

210
Q

the (weighted) average mass numbers of a sample of atoms

A

atomic weight

Bio I Exam 1 (11 decks)

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