Water and Life Flashcards

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1
Q

Water chemical formula

A

H₂O

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2
Q

Water is a neutral molecule
(True or False)

A

True

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3
Q

Polar Molecule

A

A molecule in which the charges are unevenly distributed;
(Charges written parentheses (+) or (-) to show that the charges are weaker than ions) polar molecules attract each other because of their slight negative and positive charge

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4
Q

Why are water molecules considered polar molecules?

A

Water molecules are considered polar molecules because they consist of one oxygen atom (that has a stronger pull because it has more protons in the nucleus) and two hydrogen atoms (which have a weaker pull because it has less protons in its nucleus) This causes the oxygen molecule to get more electrons than the hydrogen atoms in the covalent bond, causing the oxygen molecule to have a slightly negative charge and the hydrogen molecules to have a slightly positive charge.

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5
Q

Hydrogen Bonding

A

Attraction of water molecules because of the slightly negative and positive charges of a water molecule; not as strong as covalent or ionic bonds (temporary)

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6
Q

What are the most common atoms involved in hydrogen bonding?

A

Oxygen, nitrogen, and fluorine

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7
Q

Cohesion

A

attraction between molecules of the same substance –> always through hydrogen bonds; creates a surface tension which allows some insects to walk on water
(Ex:water molecules)

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8
Q

Adhesion

A

attraction between molecules of different substances
(Ex: water molecules and glass molecules)

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9
Q

Capillary Action

A

One of the forces that draws water out of the roots of a plant and up into its stems and leaves. This is a combination of cohesion (which holds the water molecules together) and adhesion (which causes the water to rise)

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10
Q

Heat Capacity

A

the amount of heat energy required to increase an object’s temperature by 1 degree

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11
Q

Heat Capacity of Water

A

Water has a high temperature because it is highly cohesive.

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12
Q

Mixture

A

a material composed of two or more elements or compounds that are physically mixed together, but not chemically combined.

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13
Q

Types of mixtures

A

Solutions and Suspensions

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14
Q

Solution

A

a mixture in which all components are evenly distributed
(Ex: salt dissolving in warm water)

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15
Q

Suspension

A

mixtures of water and non dissolved material
(Ex: our blood is mostly water and suspended cells)

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16
Q

Solute

A

the substance that is dissolved

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17
Q

Solvent

A

the substance in which the solute dissolves

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18
Q

ph Scale

A

system used to indicate the concentration of H+ (hydrogen) ions in a solution. This system ranges from 0-14; below 7 the ph is acidic, at 7 the ph is neutral, above 7 the pH is basic.
the pH scale is logarithmic meaning each step represents a factor of 10 difference

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19
Q

Base

A

(aka proton acceptors) a compound that produces OH- (hydroxide) ions in a solution; pH above 7

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20
Q

Why are bases known as proton acceptors?

A

Bases are known as proton acceptors because they attract H+ ions to create water.
(look at example in notebook)

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21
Q

Buffer

A

weak acids or bases that can react with strong acids or bases to prevent sharp, sudden change in pH and maintain a specific pH –> extremely important for maintaining homeostasis because enzymes can only operate under certain conditions

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22
Q

Acid aka

A

proton donors

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23
Q

Why are acids considered proton donors?

A

Acids are considered proton donors because they give off H+ ions. These hydrogen ions are considered protons because to become an ion they need to get rid of the one electron in there valence shell.

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24
Q

One Universal Solvent

A

water

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25
Q

What can water dissolve/Why is it known as a universal solvent?

A

ionic compounds, other polar molecules

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26
Q

How does water dissolve compounds?

A

water molecules are attracted to positive/negative charge of other molecules (because of its bent shape) and pulls them apart, forming new compounds

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27
Q

What does water expand upon freezing?

A

Because when water drops in temperature, the hydrogen bonds push the H20 molecules farther apart from each other increasing the intermolecular space becuase there is air locked in by the crystal lattice structure, making it less dense than the water

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28
Q

Why is the heat capacity of water important

A

because if it was low, all the water in living organisms would evaporate on a hot day –> so it aids in regulating body temp

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29
Q

Do weak acids have a high amount of H+ or low

A

Low H+

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30
Q

Do strong acids have a high amount of H+ or low

A

High H+

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31
Q

Do weak acids have a high or low pH

A

high

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32
Q

Do weak acids have a low or high pH

A

low

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33
Q

pH equation

A

pH = -log[H+]

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34
Q

Why did the pH equation work

A

the pH equation works bc you are given molar concentration of H+ [H+] and since pH is logarithmic (to the 10th) doing -log cancels it

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35
Q

Acid definition

A

any compound that has H+

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36
Q

Acid

A

compounds that are acidic are corrosive and break down other compounds

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37
Q

pH range of acid

A

less than 7

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38
Q

Acid taste

A

sour

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39
Q

Bases make what type of solution

A

alkaline

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40
Q

Base taste + texture

A

bitter + slippery

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41
Q

Ionic bond

A

transfer of electrons; formed between anions and cations

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42
Q

Anion

A

negative ion

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43
Q

Cation

A

positive ion

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44
Q

Covalent bond

A

share electrons

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45
Q

single covalent bond

A

one pair of electron is shared

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46
Q

double covalent bond

A

two pairs of electrons are shared

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47
Q

Van der Waals forces

A

quick temporary forces where all electrons move to one side; the other side is positively charged, and a negatively charged is attracted to the positively charged side

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48
Q

Hydrogen Bond

A

weak chemical bonds that form when a H atom that is covalently bonded to an electronegtative atom is also attracted to another electronegative atom

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49
Q

When are H bonds strong

A

when there are alot of them –> like kindergarteners!

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50
Q

Surface Tension

A

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

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51
Q

What is the importance of expansion upon freezing of water

A

when liquid gets cold and loses kinetic energy, the molecules usually come closer together; however, water does the opposite so that solid is les dense than liquid which allows marine life to live under ice

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52
Q

Why is the heat capacity of water so high

A

water is super cohesive so heat energy needs to break multiple hydrogen bonds before the heat spreads. (water needs to absorb more heat before it rises in temperature)

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53
Q

Kinetic Energy

A

energy of motion

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54
Q

more kinetic energy = faster or slower

A

faster

55
Q

Thermal Energy

A

kinetic energy associated with random movement of atoms and molecules, taking volume into account

56
Q

Temperature

A

average kinetic energy of the molecules in something that has matter regardless of volume

57
Q

Relationship between thermal energy and volume

A

direct

58
Q

Relationship between thermal and kinetic energy

A

direct

59
Q

Relationship between kinetic energy and volume

A

no relationship

60
Q

describe what happens in terms of thermal energy when a cold thing touches a hot thing

A

the thermal energy from the hot thing is absorbed by the cold thing until there is equilibrium

61
Q

Heat

A

thermal energy transfer from one mass to another

62
Q

Calorie

A

the amount of heat it takes to raise 1g of water by 1 degree celsius and the amt of heat released when 1g of water cools by 1 degree celsius

63
Q

Kilocalorie

A

1000 cal is the amt of heat needed to raise 1kg of water by 1 degree celsius because of kilo

64
Q

Joule

A

unit of energy

65
Q

Specific Heat Capacity importance

A

1) regulate earth temp
2) survival of organisms

66
Q

How does water help regulate the earths temp

A

it refulates coastal temps bc it can make air warmer at night and absorb heat when its too sunny

67
Q

How does high specific heat capacity regulate body temp

A

bc humans are 75% of water so if it was low we would js evaporate and die

68
Q

Vaporization

A

water -> gas (water vapor)

69
Q

Vaporization aka

A

evaporation

70
Q

Vaporization only happens at hot temps true or false

A

false it occurs at any temperature its js that at hotter temps the molecules are faster and the process is js faster

71
Q

heat of vaporization

A

quantity of heat a liquid must absorb for 1g of it to be converted from liquid -> gas

72
Q

What is the cause of the high heat of vaporization of water

A

the strongness of the multitude of hydrogen bonds bc they all need to break before l -> g

73
Q

Does water have a high or low heat of vaporization

A

high

74
Q

Why is waters high heat of vaporization important

A

1) moderate earth climate

75
Q

How does the high heat of vaporization moderate earths climate

A

release heat at night, absorb in morning

76
Q

Why is the high heat of vaporization bad for earth

A

causes burns from steam bc the liquid is even hotter when it condenses because energy is released bc g -> l is an exothermic reaction

77
Q

Evaporative Cooling

A

when a liquid evaporates the liquid that is left behind doesn’t evaporate and instead it cools down

78
Q

what is the cause of evaporative cooling

A

the molecules with the most KE (hot and fast) will evaporate and the warmer/slower ones will stay and then slow down when the high KE leaves

79
Q

Why is evaporative cooling good

A

1) moderate water bodies temp
2) regulate bodies temp

80
Q

How does evaporative cooling moderate water bodies temp

A

the top (surface) is hot bc sun and then when it evaporates the rest of the ocean slows down so that the whole ocean doesn’t poof into thin air

81
Q

How does evaporative cooling regulate body temp

A

the hot sweat leaves the colder sweat behind so less KE so it cools u down bc it js gets colder

82
Q

Why do people feel hotter when its humid

A

bc the hotter sweat cant leave bc the air is already filled with vapor

83
Q

Hydration shell

A

the sphere of water molecules surrounding each dissolved ion of a solute

84
Q

Why do ionic and molecular compounds dissolve in water

A

bc there can be polar regions and HYDROGEN bonds can pull stuff apart by the polar water molecules

85
Q

Why does water dissolve salt and not the other way around

A

literally js bc theres more water -.-

86
Q

Hydrophilic

A

like water

87
Q

Hydrophobic

A

hate water

88
Q

Example of hydrophilic thing

A

cotton

89
Q

Examples of hydrophobic things

A

not polar or ionic and cant form H bonds
oil

90
Q

Molecular Mass

A

sum of masses of all atos in a molecule

91
Q

Avagadros number

A

6.02 x 10^23 formula units

92
Q

Molarity

A

the # of moles of soluter per liter of solution

93
Q

Molarity sumbol

A

mol

94
Q

Molarity forumla

A

M = n/V

95
Q

Aqueous solution

A

solution in which the solute is dissolved in water

96
Q

Dissociate

A

pull apart to create ions

97
Q

Acid Base Reaction

A

H2O + H2O ⇌ H3O+ OH-

98
Q

Hydroxide ion is a base or acid

A

base

99
Q

hydronium ion is acid or base

A

acid

100
Q

H30+ = what ion

A

H+

101
Q

In pure water the concentrations of hydroxide and hydronium are

A

equal

102
Q

What is important about reversible reactions

A

they are at dynamic equilibrium which means there are equal concentrations and they move back and forth at a constant rate

103
Q

Acid = proton ___

A

donor

104
Q

Base = proton ____

A

acceptor

105
Q

Acid

A

substances that add H+ to an aqueous solution by dissociating themselves

106
Q

What makes strong acid strong

A

it dissociates completely in water

107
Q

What makes a weak base weak

A

it does not completely dissociate in water

108
Q

Base

A

substances that reduced the concentration of H+ by excepting H+ or dissociating OH-

109
Q

Neutral Solution

A

solution where the concentration of H+ = OH-

110
Q

What makes a neutral solution

A

strong acid and base

111
Q

what makes a not neutral solution

A

weak acid and weak base

112
Q

Not neutral solution

A

solytion where the concentrations of H+ do not equal OH-

113
Q

In any aqueous solution at 25 degrees celsius, the product of H+ and OH- concentrations is constant at what

A

10^-14

114
Q

pH scale

A

measure of H3O+ ions that compresses the range of H+ and OH- into logarithms

115
Q

pH equation

A

ph= -log[H+]

116
Q
A
116
Q

Strong acid = ____ H+ = ____ pH

A

high low

117
Q

Every step in the ph Scale is a factor of what

A

10

118
Q

weak acid = ____ H+ = ____ pH

A

low high

119
Q

If x< 7 is it an acid or a base

A

acid

120
Q

If x> 7 is it an acid or a base

A

base

121
Q

If x= 7 is it an acid or a base

A

neither its neutral

122
Q

What are things that have a neutral pH

A

water

123
Q

as you go up things get _____ acidic

A

more

124
Q

as you go down things get more ___

A

basic

125
Q

What substances are usually buffers

A

conjugate bases

126
Q

How do buffers work

A

they accept or donate H+ when needed

127
Q

Ocean acidification

A

when the pH of the ocean lowers
when CO2 dissolves in water and forms carbonic acid

128
Q

Cause of ocean acidification

A

burning fossil fuels

129
Q

Ocean acidification makes the ocean more

A

acidic

130
Q

What particular ecosystem is ocean acidification detrimental for

A

coral reefs because they need carbonate to calcify –> this affects diversity in the ocean bc coral is super important

131
Q

Ocean Acidification (chemically)

A

CO2 is absorbed by the ocean and it reacts with hydrogen to form carbonic acid
The carbonic acid decomposes into Hydrogen and bicarbonate
the hydrogen reacts with the carbonate and forms bicarbonate ion, so the carbonate ion decreases because there’s more hydrogen

132
Q

How many bonds can a water molecule make

A

4

133
Q

What kind of bonds are in adhesion

A

can be any doesnt just have to be hydrogen