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Biology 1010 > Properties of water > Flashcards

Properties of water Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

substance that makes all life possible

A

water

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2
Q

All familiar organisms are made mostly of

A

water

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3
Q

water is the Only substance to exist in

A

all three states

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4
Q

Water’s unique behavior is related to its

A

structure and interaction of it’s molecules

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5
Q

water molecule shape

A

a wide V with two hydrogen atoms joined to the oxygen atom by single covalent bonds

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6
Q

properties of water come from the

A

attractions between oppositely charged atoms of different molecules

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7
Q

hydrogen bond

A

The hydrogen of one water is attracted to the oxygen of another

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8
Q

In the liquid form, hydrogen bonds are

A

fragile

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9
Q

why are hydrogen bonds fragile

A

They form, break and reform very frequently

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10
Q

which atom is is more electronegative in water

A

oxygen

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11
Q

what does it mean that oxygen has a higher electronegativity

A

electrons in the covalent bond spend time closer to it

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12
Q

The oxygen region has a partial

A

negative charge

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13
Q

the hydrogen region has a

A

partially positive charge

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14
Q

The overall charge of water is unevenly distributed because

A

unequal sharing of electrons

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15
Q

Four emergent properties of water

A
  1. Cohesive behavior
    1. Ability to moderate temps
    2. Expansion upon freezing
      Versatility as a solvent
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16
Q

Cohesion of water molecules

A

the molecules stay close together because of the hydrogen bonding

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17
Q

cohesion contributes to what in plants

A

transport of water and dissolved nutrients against gravity

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18
Q

hydrogen bonds cause water molecules to do what in plants

A

water molecules in veins to tug on those farther down

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19
Q

Adhesion

A

the clinging of one substance to another

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20
Q

adhesion in plants

A

Adhesion of water by hydrogen bonds to molecules of the cell walls counters the downward pull of gravity

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21
Q

surface tension is related to

A

cohesion

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22
Q

surface tension

A

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

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23
Q

water has a ______ surface tension

A

high

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24
Q

why does hydrogen have a high surface tension

A

hydrogen bonding between the molecules of the air and water below

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25
Q

how does water moderate air temps

A

by absorbing heat from warmer air and releasing stored heat to colder air

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26
Q

why is water an effective heat bank

A

can absorb or release a large amount of heat with only slight changes in own temp

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27
Q

why does a desert have huge temp changes

A

there is no water to moderate the temp

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28
Q

places closer to the ocean will have ____ temp fluctuations

A

less

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29
Q

When two objects of different temps are brought together, the

A

Thermal energy passes from the warmer object to the cooler one

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30
Q

when does the thermal energy stop passing from the warmer object to the cooler one

A

when they are the same temp

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31
Q

Molecules in cooler objects

A

Speed up at the expanse of the thermal energy of the warmer object

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32
Q

Kinetic energy:

A

The energy of motion

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33
Q

. Anything that moves has this energy

A

kinetic energy

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34
Q

The faster the movement the greater the

A

kinetic energy

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35
Q

Thermal energy

A

Kinetic energy associated with the random movement of atoms or molecules

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36
Q

thermal energy reflects

A

total kinetic energy

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37
Q

Temperature

A

The average kinetic energy of molecules in a body of matter

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38
Q

does volume matter for temp

A

nope

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39
Q

Heat

A

Thermal energy transferred from one body of matter to another

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40
Q

heat is measured in

A

Joules

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41
Q

1 cal

A

4.184 J

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42
Q

heat is also measured in

A

calories

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43
Q

calories

A

. Heat needed to raise the temp of 1 g of water by 1 degree Celsius

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44
Q

Water’s high specific heat has the ability to

A

stabilize temps

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45
Q

why can water stabilize temps

A

because of it’s relatively high specific heat capacity

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46
Q

Specific heat

A
  1. The amount of heat that must be absorbed or lost for 1 g of that substance to change temps by 1 degree Celsiu
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47
Q

Water has a specific heat of

A

4.18

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48
Q

Water changes it’s temp less than other liquids when it

A

absorbs or loses heat

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49
Q

water loses a _____ amount of water with each degree of change

A

large

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50
Q

The high specific heat of water can be traced to the

A

hydrogen bonds

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51
Q

To beak hydrogen bonds,

A

heat must be absorbed

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52
Q

when hydrogen bonds form they

A

release heat

53
Q

before a water molecule can move faster

A

the heat goes towards disrupting the hydrogen bonds

54
Q

When water temp drops slightly

A

releases large amount of energy in HEAT

55
Q

what is the relevance of water’s specific heat capacity

A

Large body of water
a. Can absorb and store huge amounts of heat from the sun
b. Only warms up a few degrees

56
Q

high specific heat capacity of water creates

A

a favorable environment for marine life

57
Q

Evaporative cooling

A

Liquid evaporates and the surface left behind cools down (temp decreases)

58
Q

the hottest molecules are the most likely

A

to become gas

59
Q

evaporating cooling contributes

A

to the stability of temps in lakes and ponds
a mechanisms that prevents the organism from overheating

60
Q

Molecules stay close together because

A

they are attracted to one another

61
Q

Molecules must moving fast enough

A

overcome these attractions

62
Q

VAPORIZATION or EVAPORATION

A

Depart the liquid phase and enter the air as gas

63
Q

even at the low temps, the speediest molecules can

A

escape into the air

64
Q

Heat of vaporization

A
  1. Quantity of heat a liquid must absorb for 1 g to be converted from liquid to gas
65
Q

water has a ____ heat of vaporization compared to other liquids

A

high

66
Q

heat of vaporization is an emergent property from

A

strength of hydrogen bonds

67
Q

what must be broken before the molecule can exit liquid stage into the water vapor

A

the hydrogen bonds

68
Q

Water is one of the few substances that is ____ dense as a solid than a liquid

A

less

69
Q

what does water do when it solidifies

A

expands

70
Q

what causes this expansion as water turns solid

A

the hydrogen bonds

71
Q

when water is at a temp above 4 degree Celsius

A

Water is like any other liquid

72
Q

Temps from 4 degree Celsius to 0 degree Celsius

A

Water begins to freeze as more and more of it’s molecules are moving too slowly to break hydrogen bonds

73
Q

At 0 degree Celsius

A

Molecules become locked together in a crystalline lattice

74
Q

Hydrogen bonds keep the molecules _____ apart than at 4 degree Celsius

A

farther

75
Q

When ice absorbs enough heat for the temp to rise above 0 degree Celsius

A

Hydrogen bonds between molecules are shattered

76
Q

At 4 degree Celsius water has reached

A

its greatest density

77
Q

floating ice on water allows the liquid below to be

A

insulated and stops it from freezing

78
Q

how is Global warming affecting ice

A

a. Ice has formed later in the year and melts earlier
b. It covers a smaller area

79
Q

why is Water a very versatile solvent

A

polarity of water molecules

80
Q

A compound does not need to be _____ to dissolve in water

A

ionic

81
Q

how do non-ionic molecules dissolve in water

A

water molecules surround each of the solute molecules and form hydrogen bonds with them

82
Q

Large molecules like proteins can dissolve in water if

A

they have polar regions on their surface

83
Q

Solution

A
  1. A liquid that is a completely homogeneous mixture of two or more substances
84
Q

Solvent

A

Dissolving agent of a solution

85
Q

Solute

A
  1. Substance that is dissolved
86
Q

Aqueous solution

A

The solute is dissolved in water

87
Q

Hydration shell

A

The sphere of water molecules that surround a dissolved ion and prevent those ions from rejoining together

88
Q

Working inward, water will eventually do what to the ions

A

dissolve them all

89
Q

Hydrophilic

A
  1. Any substance that has an affinity (liking) for water
90
Q

can something be hydrophilic without dissolving in water

A

yes, think of a cotton towel

91
Q

Hydrophobic

A
  1. Substances that are non-ionic and non-polar (can’t form hydrogen bonds)
92
Q

Molecular mass

A

Sum of the mass of all atoms in a molecule

93
Q

Mole (mol)

A

6.02 x 10^23

94
Q

6.02 x 10^23 daltons in

A

1 gram

95
Q

Moles of one substance equals the same number

A

MOLECULES as a mole of another substance

96
Q

Molarity

A

Number of moles of solute per liter of solution

97
Q

a hydrogen atom can shift between

A

two water molecules during a hydrogen bond

98
Q

Hydrogen ion (H+)

A

A single proton with a charge of 1+

99
Q

H+ does NOT exist on

A

its own in an aqueous solution

100
Q

h+ Always associated with a water molecule in the form

A

H3O

101
Q

Hydroxide ion (OH-)

A

The water molecule that lost a proton

102
Q

Dissociation of water importance

A

H+ and OH- are very reactive and concentration changes can affect a cell’s proteins

103
Q

in pure water, H+ and OH- are

A

equal in concentration

104
Q

Acids

A

donate H+ ions when dissolved in water

105
Q

Substance that increases the hydrogen ion concentration of a solution

A

acid

106
Q

An acidic solution has more

A

H+ to OH-

107
Q

Base

A
  1. Reduces the hydrogen ion concentration of a solution
108
Q

Some bases reduce H+ concentrations directly by accepting Hydrogen ions

A

Ammonia

109
Q

Other bases reduce H+ concentration indirectly by dissociating to form hydroxide ions

A

Sodium hydroxide

110
Q

Basic solutions

A

Have a higher concentration of OH- than H+

111
Q

Neutral solutions

A

Solutions that have equal H+ and OH-

112
Q

Strong Base and acids

A

Compounds that dissolve completely when mixed with water

113
Q

what is not a reversable reaction when used

A

Strong Base and acids

114
Q

The reaction is reversible when using

A

Weak acid or base

115
Q

The PH scale

A

Compresses the range of H+ and OH- concentrations by logarithms

116
Q

each jump in the PH scale is a jump in

A

ten

117
Q

EXAMPLE
Ph of 3 to PH of 6

A

It is a thousand times more acidic (10 x 10 x 10)

118
Q

PH formula

A

PH = -log [H+]

119
Q

Ph _____ as H+ concentrations increase

A

declines

120
Q

Neutral solutions formula

A

-log 10-7 = -(-7) = 7

121
Q

PH above 7

A

Basic solutions

122
Q

PH of less than 7

A

Acidic solution

123
Q

An acid not only adds hydrogen ions to a solution but it also

A

removes hydroxide ions

124
Q

A base increases OH- concentrations but also

A

reduced H+ concentrations by the formation of water

125
Q

Buffers

A

substance that minimizes changes in concentrations of H+ and OH- in a solution

126
Q

buffers must be

A

weak acids and its corresponding base

127
Q

how do buffers work

A
  1. Buffers accept hydrogen ions from the solution when they are in excess
  2. Donate hydrogen ions to the solution when there aren’t enough
128
Q
A

Biology 1010 (14 decks)

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