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Bio 111 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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Biology 101 flashcards
1
Q

all matter is composed of ___?

A

ATOMS!

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2
Q

why does chemistry matter in biology?

A

the reactions in cells involve atoms and chemical bonds joining together or breaking apart

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3
Q

what charge do electrons have?

A

negative

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4
Q

what charge do protons have?

A

positive

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5
Q

what charge do neutrons have?

A

no charge, they are neutral

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6
Q

what subatomic particles are located in the nucleus of the atom?

A

protons and neutrons

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7
Q

what subatomic particles orbit the nucleus?

A

electrons

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8
Q

what makes different atoms different?

A

the number of electrons and neutrons

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9
Q

what is an element?

A

a substance whose atoms all have the same number of protons

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10
Q

what are isotopes?

A

atoms of the same element that have different atomic mass numbers due to different number of neutrons

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11
Q

what is a way that the characteristics of atoms can change?

A

radioactive decay

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12
Q

what are neutral atoms?

A

atoms that have an overall neutral charge

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13
Q

what is the overall goal of nature?

A

equilibrium

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14
Q

why does equilibrium matter?

A

atoms want to be neutral, meaning their electrons want to be paired

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15
Q

what are ions?

A

atoms that have gained or lost an electron and have a changed overall net charge

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16
Q

what are cations?

A

positively charged ions that have lost an electron

Plussy Cat’s are a good, positive thing :0

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17
Q

what are anions?

A

negatively charged ions that have gained an electron

An(T)ions are bad and negative because they bite you!

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18
Q

where in the atom does chemical bonding take place?

A

in the outermost electron orbital

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19
Q

what type of energy do electrons possess?

A

potential energy

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20
Q

where is the potential energy of an electron the strongest?

A

in the outermost orbital

like a ball at the top of a hill

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21
Q

where is the potential energy of an electron the weakest?

A

closest to the nucleus

like the ball at the bottom of a hill

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22
Q

what two things can happen to an electron during bonding?

A

oxidation or reduction

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23
Q

what is oxidation? (OiL)

A

Oxidation is the Loss of an electron by an atom during bonding, resulting in a cation

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24
Q

what is reduction? (RiG)

A

Reduction is the Gain of an electron by an atom during bonding, resulting in an anion

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25
Q

what is it called when atoms engage in and OiLRiG reaction?

A

a Redox reaction!

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26
Q

what are valence electrons?

A

electrons in the outermost energy shell of an atom

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27
Q

what’s so special about hydrogen?

A

it only has a single electron, and only one energy shell, so it’s very reactive, because that electron is lonely :(

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28
Q

what’s special about the Group 18 elements?

A

all their valence electrons are paired, so they are inert and never form bonds

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29
Q

what’s special about CARBON and silicon?

A

they have 4 unpaired valence electrons, so they can form bonds with up to four other atoms

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30
Q

do atoms like their energy levels empty or full?

A

FULL

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31
Q

how do atoms fill their empty outer energy levels?

A

by bonding with another atom

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32
Q

are atoms with full energy levels more or less reactive than atoms with unfilled energy levels

A

MORE REACTIVE, every electron wants a friend!

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33
Q

how many naturally occurring elements are there?

A

90

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34
Q

how many elements are found in living organisms in substantial amounts?

A

12

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35
Q

how many elements make up 96.3% of living things, and what are they?

A 
4: CHON
Carbon
Hydrogen
Oxygen
Nitrogen
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36
Q

what elements MUST organic compounds contain?

A

carbon, hydrogen, and oxygen

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37
Q

what compound makes up most of our cells?

A

water

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38
Q

is water (H20) an organic compound?

A

NO

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39
Q

why isn’t water an organic compound?

A

it does not contain Carbon

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40
Q

what are molecules?

A

groups of atoms held together in a stable association

ex. hydrogen gas, H2

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41
Q

what are compounds?

A

molecules that contain more than one type of elements

all compounds are molecules, but not all molecules are compounds

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42
Q

what holds atoms together?

A

chemical bonds

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43
Q

name the three kinds of chemical bonds

A

ionic, covalent, and hydrogen bonds

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44
Q

how are ionic bonds formed?

A

by the attraction of oppositely charged ions (cations and anions)

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45
Q

list an example of an ionic bond

A

the bond between Sodium (Na) and Chlorine (Cl) to form NaCl

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46
Q

which is the electronegative element in NaCl?

A

Chlorine, both have one unpaired electron, but Chlorine is electron greedy and tries to steal Sodium’s unpaired electron for itself

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47
Q

what happens to the unpaired electron when Chlorine tries to steal it from Sodium?

A

Sodium is not pleased, and clings to Chlorine to try to get its electron back, thus the ionic bond is formed

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48
Q

what is the cation in NaCl?

A

Sodium, its electron is stolen :(, which makes it positive :)

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49
Q

what is the anion in NaCl?

A

Chlorine, our mean electron thief >:(

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50
Q

are ionic bonds strong?

A

no, they’re pretty weak

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51
Q

how are covalent bonds formed?

A

electron sharing

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52
Q

how many levels of bond strength are covalent bonds capable of?

A

3, and strength increases as the number of bonds increases

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53
Q

give an example of a single covalent bond

A

hydrogen gas, has one electron available for bonding

54
Q

give an example of a double covalent bond

A

oxygen gas, has two electrons available for bonding

55
Q

give an example of a triple covalent bond

A

nitrogen gas, has three electrons available for bonding

56
Q

what is electronegativity?

A

electron greediness

57
Q

why is electronegativity important in biology?

A

oxygen is VERY electronegative and forms MANY bonds

58
Q

what are nonpolar covalent bonds?

A

covalent bonds where electrons are shared equally between interacting atoms

59
Q

what are polar covalent bonds?

A

covalent bonds where electrons are NOT equally distributed around the nuclei of interacting atoms
@oxygen

60
Q

what gives water its polarity?

A

the polar covalent bonds between oxygen and hydrogen

61
Q

what happens when polar and nonpolar substances interact?

A

they repel each other, and form droplets, called micelles

62
Q

chemical reactions involve ____?

A

chemical bonds between atoms

63
Q

whether a chemical reaction occurs is influenced by _____?

A

how many unpaired electrons are present

64
Q

how are chemical equations written?

A

reactants first, followed by the products

65
Q

can chemical reactions be reversed?

A

yes, and they often are, especially in biology!

66
Q

what kinds of chemical reactions do cells use?

A

reversible chemical reactions!

67
Q

all living organisms are dependent on ____?

A

WATER!

68
Q

what is the structure of water?

A

polar covalent bonds between oxygen and hydrogen

69
Q

what is the most important property of water?

A

its ability to form hydrogen bonds

70
Q

what are hydrogen bonds?

A

when two molecules of water interact and join together due to oxygen’s electronegativity

71
Q

how does oxygen’s electronegativity form hydrogen bonds?

A

oxygen tries to steal the hydrogens of other oxygens

it really be ya own bitches

72
Q

what forms water droplets?

A

hydrogen bonds!

73
Q

what is the weakest chemical bond?

A

hydrogen bonds!

74
Q

are the bonds between hydrogen and oxygen in H2O polar or nonpolar?

A

VERY polar

75
Q

what kind of partial charges develop when hydrogen and oxygen join together?

A

oxygen is partially negative, and hydrogen is partially positive
OXYGEN IS ELECTRONEGATIVE

76
Q

name three ways to illustrate H2O

A

bohr model, ball and stick model, space-filling (mickey mouse) model

77
Q

hydrogen bonds are WEAK attractions between ______?

A

individual water molecules

78
Q

what specifically do hydrogen bonds form between?

A

the HYDROGEN of one H2O molecule, and the OXYGEN of another H2O molecule because
OXYGEN IS ELECTRON GREEDY

79
Q

what is cohesion?

A

cooperation, H2O sticks to other H2O molecules

80
Q

give an example of H2O cohesion

A

water puddles and surface tension

81
Q

what is adhesion?

A

H2O sticks to other polar molecules

82
Q

give an example of H2O adhesion

A

capillary action, water sticks to polar plant stems and travels from the root to the tip, with evaporation acting as suction

83
Q

list the 6 properties of water

A
  1. water has a high specific heat
  2. water has a high heat of vaporization
  3. solid water is less dense than liquid water
  4. water is a GREAT solvent
  5. water organizes nonpolar molecules
  6. water can form ions
84
Q

what is specific heat?

A

the amount of energy required to raise 1 gram of water by 1 degree celcius

85
Q

why is water’s high heat of vaporization important?

A

water can absorb a lot of heat before evaporating

think: oceans, sweat

86
Q

why is solid water less dense than liquid water?

A

as water cools, the hydrogen bonds are stretched further apart due to air pockets in between those hydrogen bonds

87
Q

why does it matter that ice is less dense than liquid water?

A

water is a great insulator and can float

think: lake in the winter, animals living happily under a layer of ice

88
Q

what’s another name for water?

A

the universal solvent

89
Q

why does water’s great dissolving ability matter?

A

it will dissolve the bonds between almost anything

ex. the ionic bonds between NaCl

90
Q

what is one thing water can’t dissolve?

A

nonpolar molecules

91
Q

why can water dissolve almost anything?

A

it’s SUPER polar, the oxygen tries to take everyone’s electrons

92
Q

what happens when water organizes nonpolar/hydrophobic molecules?

A

droplets/spheres/MICELLES form

93
Q

what is a micelle?

A

a spherical structure that forms when a nonpolar molecule contacts H2O

94
Q

give a SUPER important example of micelles

A

the phospholipid bilayer of cell membranes!!

95
Q

define hydrophobic

A

water fearing, nonpolar

96
Q

give a real world example of a hydrophobic substance

A

the oil ducks secrete to help them float on water and stay warm

97
Q

define hydrophilic

A

water loving, polar

98
Q

what two ions does H2O dissociate to form?

A

one hydroxide ion (OH-) and one hydrogen ion (H+)

99
Q

what is the basis of the pH scale?

A

the hydrogen ion (H+)

100
Q

pH refers to the concentration of ____ in a solution

A

hydrogen ions (H+)

101
Q

a greater pH concentration equals a ____?

A

lower pH number

102
Q

a lower pH concentration equals a ____?

A

higher pH number

103
Q

what is the formula for pH?

A

pH = -log[H+]

104
Q

what kind of relationship exists between H+ concentration and pH number?

A

an inverse relationship

105
Q

what is the range of the pH scale?

A

0-14

106
Q

what pH does distilled water have?

A

7, it is neutral

107
Q

what does a pH above 7 indicate?

A

a basic/alkaline solution

108
Q

what does a pH below 7 indicate?

A

an acidic solution

109
Q

what does a neutral pH mean?

A

there is an equal concentration of H+ and OH- ions

110
Q

what is the average pH for human blood?

A

6.5

111
Q

is human blood usually basic or acidic?

A

it is slightly acidic

112
Q

what does the pH of the soil of a hydrangea effect?

A

the color of the hydrangea

113
Q

what pH levels cause hydrangeas to be blue?

A

5.5 and lower

114
Q

what pH levels cause hydrangeas to be pink?

A

6.02 and higher

115
Q

pine needles ____ soil?

A

acidify

116
Q

are acids hydrogen acceptors or hydrogen donors to a solution?

A

they are hydrogen donors

117
Q

what does a hydrogen donor do?

A

releases H+ ions into a solution, which drops pH levels, ACIDS DO THIS

118
Q

are bases hydrogen acceptors or hydrogen donors to a solution

A

hydrogen acceptors

119
Q

what does a hydrogen acceptor do?

A

absorbs H+ ions and binds them up into OH- ions, raising pH levels
BASES DO THIS

120
Q

what lowers pH levels?

A

an acidic solution

121
Q

what do buffers do?

A

maintain homeostasis of blood pH

122
Q

what makes up most biological buffers?

A

one acidic molecule and one basic molecule

123
Q

give an example of a biological buffer

A

carbon dioxide-bicarbonate buffer

DO NOT TURN THIS OVER UNTIL YOU CAN DESCRIBE THIS WHOLE BUFFER SYSTEM

124
Q

if xenon has an atomic number of 54 and a mass number of 108, how many neutrons does it have?

A

54

125
Q

atoms that vary in the number of neutrons found in their nuclei are called ____?

A

isotopes

126
Q

what is the weakest chemical bond?

A

hydrogen bonds

127
Q

when acids are added to a solution, the pH should ___?

A

decrease

128
Q

a molecule that binds up excess hydrogen ions in a solution is called a ____?

A

base

129
Q

each carbon molecule can bond with as many as ____ other atoms or molecules?

A

4

130
Q

why can some insects walk on water?

A

surface tension from hydrogen bonds

Bio 111 (17 decks)

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