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AP Economics > Chapter 2: The Chemical Context of Life > Flashcards

Chapter 2: The Chemical Context of Life Flashcards

1
Q

What does matter consist of?

A

chemical elements in pure form and in combinations called compounds

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2
Q

What does an element’s properties depend on

A

the structure of its atoms

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3
Q

What does the formation and function of molecules depend on?

A

chemical bonding between atoms

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4
Q

What do chemical reactions do?

A

make and break chemical bonds

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5
Q

What gives water properties that help make life possible on Earth

A

Hydrogen bonding

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6
Q

What are organisms composed of?

A

matter

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7
Q

What is matter?

A

anything that takes up space and has mass

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8
Q

What is an element?

A

a substance that cannot be broken down to other substances by chemical reactions

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9
Q

How many elements occur in nature?

A

92

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10
Q

What is a compound?

A

a substance consisting of two or more elements combined in a fixed ratio

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11
Q

What elements are needed to live a healthy life and reproduce?

A

Essential elements

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12
Q

How many essential elements do humans need?

A

25

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13
Q

How many elements do plants need?

A

17

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14
Q

What elements are required by an organism in only mine quantities?

A

Trace elements

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15
Q

T/F: Fe is only required in humans

A

False - it is required in all forms of life

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16
Q

What is iron used to make in humans?

A

hemoglobin in blood

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17
Q

What is I used by

A

the thyroid gland

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18
Q

What is Iodine deficiency called?

A

goiter

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19
Q

What compound accounts for the high percentage of oxygen in the human body?

A

water

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20
Q

What is an atom?

A

The smallest unit of matter that still retains the properties of that element

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21
Q

What are the 3 parts an atom is composed of?

A

neutrons, protons, and electrons

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22
Q

What is the charge of a neutron

A

neutral

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23
Q

What is a charge of a proton?

A

positive

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24
Q

What is the charge of an electron?

A

negative

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25
Q

What is the mass of a neutron in daltons?

A

1

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26
Q

What is the mass of a proton in daltons?

A

1

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27
Q

What is the mass of an electron in daltons?

A

1/2000 (but we consider it to be 0)

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28
Q

Where is the neutron?

A

the atomic nucleus

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29
Q

Where is the proton?

A

atomic nucleus

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30
Q

Where is the electron?

A

orbitals around the nucleus

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31
Q

What is the atomic number?

A

the number of protons which is unique to each element?

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32
Q

What is the mass number?

A

the number of protons and neutrons found in the nucleus

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33
Q

What is equal since an atom is electrically neutral?

A

The number of protons and the number of electrons

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34
Q

What are isotopes?

A

atoms of the same element that have the same number of protons but different numbers of neutrons (different weights)

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35
Q

What is a radioactive isotope?

A

an isotope that decays spontaneously releasing particles and energy

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36
Q

What is half-life?

A

the time required for 50% of the atom of any radioactive material to decay

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37
Q

What is energy?

A

the capacity to cause change–for instance, by doing work

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38
Q

What is potential energy?

A

the energy that matter possesses because of its location or structure

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39
Q

What does matter have a tendency to do?

A

move to the lowest possible state of potential energy

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40
Q

What are valence electrons?

A

the number of electrons in the outermost shell

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41
Q

What does the chemical behavior of an atom depend on?

A

the number of valence electrons

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42
Q

What happens when an electron is moved away from the nucleus?

A

NRG is absorbed

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43
Q

What happens when an electron is moved toward the nucleus?

A

NRG is released

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44
Q

Why is neon unreactive?

A

Because its valence shell is already filled, therefore it is inert

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45
Q

How many electrons can be placed in the first orbital?

A

2

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46
Q

How many electrons can be placed in the second orbital?

A

8

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47
Q

How many electrons can be placed in the third orbital?

A

8

48
Q

Why do Fluorine and Chlorine exhibit similar chemical behavior?

A

Because they have the same number of valence electrons

49
Q

What are chemical bonds

A

attractions caused by interactions that either share or transfer valence electrons

50
Q

What type of bond shares one pair of electrons?

A

A single bond

51
Q

What type of bond shares two pairs of electrons?

A

Double

52
Q

What us electronegativity?

A

the attractions of a particular atom for the electrons of the covalent bond

53
Q

What bond if formed when two atoms have the same electronegativity?

A

non-polar covalent bond

54
Q

What bond is formed when two atoms do not share the electrons equally?

A

polar covalent bond

55
Q

When does ionic bonding occur?

A

when there is a transfer or stealing of electrons from one atom to another

56
Q

What happens any time an atom loses or gains electrons?

A

it becomes charged and is considered an ion

57
Q

What is a cation?

A

a positively charged atom

58
Q

What is an anion?

A

a negatively charged atom

59
Q

What are ionic compounds?

A

compounds formed by ionic bonds

60
Q

What is another word for ionic compounds?

A

salts

61
Q

What are covalent and ionic bonds found within the molecule considered?

A

intramolecular bonds

62
Q

What are bonds that exist between different molecules called?

A

intermolecular bonds

63
Q

hat is a hydrogen bond?

A

a non-covalent attraction between a hydrogen and an electronegative atom such as oxygen or nitrogen

64
Q

What are van Der Waals interactions

A

weak temporary regions of positive and negative charges that occur when atoms and molecules are very close together

65
Q

What do van Der Waals interactions allow molecules to do?

A

come together and respond to each other in some way and then separate

66
Q

Why is molecular shape crucial in biology?

A

it determines how biological molecules recognize and respond to one another with specificity

67
Q

Why do opiates and endorphins have similar effects in the brain?

A

opiates have similar shapes to Endorphins and mimic them by binding to endorphin receptors in the brain

68
Q

What are chemical reactions?

A

the making and breaking of chemical bonds, leading to changes in the composition of matter

69
Q

What are reactants?

A

starting materials

70
Q

What are resulting materials?

A

products

71
Q

All chemical reactions are ________

A

reversible

72
Q

What happens when a chemical reaction is reversed?

A

the products of the forward reaction become reactants of the reverse reaction

73
Q

What is chemical equilibrium

A

the point at which the rate of the forward reaction equals the rate of the reverse reaction

74
Q

What is water the only common substance to do?

A

exist in the natural environment in all three physical states of matter solids, liquids, and gasses

75
Q

What makes a polar molecule?

A

unequal sharing of electrons, meaning that its overall charge in unevenly distributed

76
Q

What makes water a polar molecule?

A

its V-like shape and unequal sharing of electrons

77
Q

What charge does the oxygen region of the water molecule have?

A

negative

78
Q

What charge does the hydrogen region of the water molecule have?

A

positive

79
Q

What are water’s four properties that contribute to the fitness of the Earth?

A

cohesive behavior, ability to moderate temperature, expansion upon freezing, versatility as a solvent

80
Q

What is adhesion?

A

the clinging of one substance to another

81
Q

What is cohesion in water?

A

all of the hydrogen bonds that collectively hold together the water molecules

82
Q

What is transpiration?

A

when cohesion of the water molecules and the adhesion to the cell walls of the xylem work together to transport water to the leaves in tall plants against the pull of gravity

83
Q

What is surface tension?

A

a measure of how difficult it is to stretch or break the surface of a liquid

84
Q

Why is surface tension unusually high in water?

A

the high number of hydrogen bonds

85
Q

How does water moderate air temperatures?

A

by absorbing heat from air that is warmer and releasing the stored heat to the air that is cooler

86
Q

What is the water moderating air temperatures called?

A

the lake effect

87
Q

What is kinetic energy

A

the energy of moment

88
Q

What is thermal energy?

A

the kinetic energy associated with the random movement of atoms or molecules

89
Q

What does temperature represent?

A

the average kinetic energy of the molecules in a body of matter

90
Q

What is heat?

A

thermal energy in transfer from one body of matter to another

91
Q

What is a calorie?

A

the amount of heat it takes to raise the temperature of 1 g of water by 1 degree C

92
Q

Where does the ability of water to stabilize temperature stem from?

A

its relatively high specific heat

93
Q

What is specific heat?

A

the amount of heat that must be absorbed or lost by that substance to change its temperature by 1 degree C

94
Q

What can specific heat be thought of as?

A

a measure of how well a substance resists changing its temperature when it absorbs or releases heat

95
Q

What is vaporization or evaporation

A

the transformation from a liquid to a gas

96
Q

What does evaporative cooling do?

A

helps stabilize temps, and provides a mechanism for organisms to keep from overheating

97
Q

Water is less dense as a ______ than it is a ______

A

solid; liquid

98
Q

When is water at its greatest density?

A

at 4 degrees C

99
Q

What happens below 4 degrees Celsius?

A

the hydrogen bonds keep the water molecules far enough apart to make it 10% less dense than liquid water

100
Q

How can freezing of water crack boulders?

A

water seeps between cracks and then its structure expands when forming ice which fractures the rock

101
Q

What is a solution?

A

a liquid that is a completely homogeneous mixture of two or more substances

102
Q

What is a solvent?

A

the dissolving agent

103
Q

What is a solute?

A

the substance being dissolved

104
Q

What is an aqueous solution?

A

a solution in which the solvent is dissolved in water

105
Q

What is water a very good solvent for?

A

ionic and polar compounds

106
Q

Whaat is a hydrophilic molecule?

A

a molecule that has an affinity for water (water-loving)

107
Q

What is a hydrophobic molecule?

A

a molecule that repels water (water fearing)

108
Q

What is an acid

A

a substance that increases the H+ concentration in a solution

109
Q

What is a base

A

a substance that reduces the concentration in a solution

110
Q

How can a base reduce the H+ concentration in a solution?

A

directly by accepting hydrogen ions from the solution, and indirectly by donating hydroxide ions to the solution (OH-)

111
Q

What is the difference between a strong acid and a weak acid (strong base and weak base)?

A

A weak acid’s reaction is reversible, a strong acid’s is not (fully dissociate)

112
Q

What is the internal pH of living organisms?

A

7

113
Q

Why is any change in pH dangerous?

A

because chemical processes are very sensitive to the concentration of hydrogen and hydroxide ions

114
Q

What are buffers?

A

substances that protect biological fluids from changes in pH

115
Q

Are buffers commonly weak acids/bases or strong acids/bases

A

Weak acids or bases

116
Q

Why does pH decrease as the H+ concentration increase?

A

because the pH of a solution is defined as the negative logarithm of the hydrogen concentration

AP Economics (7 decks)

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