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Biology 111 > Chapter 3: Water > Flashcards

Chapter 3: Water Flashcards

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1
Q

The polarity of water molecules results in:

A

hydrogen bonding (polar covalent bonding)

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2
Q

The _____ of water molecules results in hydrogen bonding

A

polarity

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3
Q

T/F Hydrogen bonds are 1/10th as strong as covalent bonds

A

False. Hydrogen bonds are 1/20th as strong as covalent bonds

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4
Q

Are covalent bonds stronger than hydrogen bonds?

A

yes

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5
Q

What is the cohesion attraction at the water surface?

A

a. Surface tension

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6
Q

T/F Covalent bonds are stronger than hydrogen bonds

A

True

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7
Q

Cohesion:
______ tension
Water from roots can reach leaves

A

surface

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8
Q

Clinging of one substance to another

A

adhesion

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9
Q

Water molecules stay close to each other as a result of hydrogen bonding to hold the substance together

A

Cohesion

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10
Q

This is how water from roots can reach leaves

A

cohesion

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11
Q

A measure of how well molecules stick to each other or group together. Caused by the attractive forces between like molecules.

A

Cohesion

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12
Q

1 calorie is the amount of ___ ____ needed to raise the temp. of 1 g of water by 1 degree celsius

A

heat energy

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13
Q

The specific heat of fusion is the heat energy needed to take ____ from 0 degrees C to 0 degrees _____

A

ice, water

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14
Q

A water spider can raise along the surface of the water. What force is at work that allows him to do it?

A

Surface tension (caused by cohesion - hydrogen bonding)

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15
Q

The amount of heat that must be ABSORBED or LOST for 1 g of that substance to change its temperature by 1 degree celsius

A

specific heat of a substance

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16
Q

Surface tension is caused by:

A

cohesian

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17
Q

Water from the roots of a tree can reach the leaves. What is this caused by?

A

Cohesion

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18
Q

The specific heat of water

A

1 cal / 1 g / 0 c

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19
Q

Specific heat of alcohol

A

0.6 cal / 1 g / 0 c

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20
Q

Coastal regions have more mild climates than inland regions do.

A

True

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21
Q

Coastal areas have milder climates than inland regions. What factor majorly causes this phenomena?

A

High specific heat of water

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22
Q

If organisms are made of a liquid with a higher specific heat….

A

they are more able to resist changes in their own temperatures than if they were made of a liquid with a lower specific heat

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23
Q

The transformation from a liquid to a gas

A

Evaporation

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24
Q

The quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gas phase:

A

Heat of vaporization

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25
Q

Regarding heat of vaporization, the quantity of heat that a liquid must absorb causes how much of the liquid to be converted from the liquid to the gas

A

1 g

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26
Q

T/F as a liquid evaporates, the surface of the liquid that remains behind cools down

A

true

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27
Q

1 g of water at 25°C needs 580 cal of heat, much higher than _______

A

alcohol (so water has a higher heat of vaporization - more resistant to changes in temperature and less evaporative)

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28
Q

What, as mentioned in the lecture, contributed to the stability of lake temperatures?

A

evaporative cooling

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29
Q

You are a scientist who is studying a freshwater lake in Oregon. You notice that the lake consistently has a temperature of approx. 55 degrees C. What is this most likely due to?

A

Evaporative cooling

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30
Q

________ of water from the leaves of a plant helps the tissues in the leaves from becoming too warm in the sunlight

A

evaporation

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31
Q

Evaporation of sweat from the human skin has what effect?

A

Dissipates body heat

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32
Q

T/F Evaporation does not prevent terrestrial organisms from overheating

A

False

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33
Q

Why is ice less dense than liquid water?

A

Stable hydrogen bonding occurs between hydrogen atoms in ice (where as in water, the bonds are breaking and reforming)

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34
Q

Ice is less dense than water due to _______ _______

A

hydrogen bonding

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35
Q

T/F Ice is more dense than liquid water due to hydrogen bonding

A

False

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36
Q

Ice floats on top of water because of….

A

hydrogen bonding (stable hydrogen bonding between hydrogen elements in ice)

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37
Q

At 0 C, water molecules become locked into a ____ ____. Each water molecule is hydrogen-bonded to ____ partners

A

crystalline lattice, four partners

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38
Q

T/F Each water molecule in ice is hydrogen-bonded to four partners

A

True

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39
Q

Liquid water is always at a state of dynamic adjustment, so it doesn’t have a chance to be locked into a ____ ____

A

crystalline lattice

40
Q

With ice, below 4 degrees celsius, the amount of heat energy is minimal and the weaker partial charges even out and create a ____ lattice: less dense

A

crystalline

41
Q

At _______ Water behaves like other liquids, expanding as

it warms and contracting as it cools

A

4 degrees celsius

42
Q

At _______ Water molecules become locked into a crystalline lattice, each water molecule hydrogen-bonded to four partners

A

0 degrees celsius

43
Q

When ice is warmed to 4 degrees celsius, what do you expect to happen?

A

Water behaves like other liquids. It will expand when warmed and constrict when cooled.

44
Q

At 0 celsius, hydrogen bonds keep molecules at “arm’s length,” far enough apart to make ice about ______ less dense than liquid water at 4 degrees celsius.

A

10% less dense

45
Q

T/F Floating ice insulates the liquid water below, preventing it from freezing and allowing life to exist under the frozen surface

A

True

46
Q

A dissolving agent

A

solvent

47
Q

Substance that is dissolved

A

solute

48
Q

Liquid that is a completely homogenous mixture of two or more substances

A

Solution

49
Q

Sphere of water around each dissolved ion

A

hydration shell

50
Q

T/F A solution MUST be homogenous for it to be a true solution

A

True

51
Q

2 types of molecules that are water-soluble

A

ionic or non-ionic polar molecules

52
Q

Solvent

A

a dissolving agent

53
Q

Solute

A

substance that is dissolved

54
Q

Solution

A

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

55
Q

Hydration shell

A

sphere of water molecules around each dissolved ion

56
Q

These molecules are water-soluble:

A

ionic or non-ionic polar molecules

57
Q

Has an affinity for water

A

hydrophilic substances

58
Q

hydrophilic substances have a….

A

affinity for water

59
Q

What substances have an affinity for water?

A

hydrophilic substances

60
Q

A mixture of suspended molecules

A

colloid

61
Q

A colloid is ____ but has very big molecules such as cellulose (cotton)

A

hydrophilic

62
Q

Is a colloid a stable or unstable suspension of fine particles in a liquid?

A

A colloid is a stable suspension of fine particles in a liquid

63
Q

T/F a colloid is made up of molecules or compounds

A

molecules

64
Q

Nonionic and non-polar substances

A

hydrophobic

65
Q

What two types of substances are likely to by hydrophobic

A

nonionic and non-polar substances

66
Q

Cell membrane components are what type of substances (mentioned in lecture)

A

hydrophobic (outside) and hydrophilic (inside)

67
Q

Oil is a _____ or _____ substance. This explains why you see two layers in salad dressing.

A

Hydrophobic

68
Q

Cell membrane components are hydrophobic. For example. The inside of the cell membrane contains the ______ tails but the lipid ____ are facing out towards the exterior water

A

hydrophilic, hydrophobic heads (water does not free flow in and out of cells)

69
Q

Define molecular weight.

A

____ g/mol

70
Q

the number of atoms or molecules in one mole of a substance

A

6.023x 10^23 atoms/molecules

71
Q

the concentration of a solution expressed as the number of moles of solute (m) per liter of solution (L)

A

molarity (m/L)

72
Q

You have 1 mole of of hydrogen atoms. How many atoms do you have?

A

6.023x10^23

73
Q

molarity is the number of moles of solute dissolved per liter of solution (m/L) . Molality is then the number of moles of solute per kilogram of the SOLVENT, NOT solution! (mol solute / kg solvent)

A
74
Q

Molality units:

A

mol solute / kg solvent

75
Q

T/F Molality deals with mass and molarity deals with volume

A

True

76
Q

Molality:

A

moles of solute / kg solvent

77
Q

A substance that increases the hydrogen ion in a solution

A

acid

78
Q

Name on strong acid (disassociation reaction) mentioned in lecture

A

HCL - H+ and Cl-

79
Q

The higher the _____, the lower the PH number

A

acidity

80
Q

Ph of 8 means the solution has _____ hydrogen ions in solution than in a solution with a PH of 12

A

less

81
Q

The specific disassociation reaction of a weak acid (mentioned in lab)

A

H2C03 -> HCO3- + H+

82
Q

What is the basic difference between strong and weak acids:

A

partial vs. complete disassociation

83
Q

Know the logarithmic laws:

A

PH = - log [H+]

pOH = - log [OH-}

84
Q

A pH unit represents a ____ difference in H+ and OH- concentrations

A

tenfold

85
Q

A _____ is a substance that minimizes the changes int he concentrations of hydrogen ions

A

buffer

86
Q

Strong alkali vs. Weak alkali

A

NaOH —-> Na+ and OH-

NH3 + H+ —–> NH4+

87
Q

Draw out the reaction which the PP mentioned as part of the buffer concept

A

H2CO3 ⇔ HCO3- + H+

88
Q

Addition of a buffer (acid): if pH rises, the reaction will proceed to the….

A

right

89
Q

Addition of a buffer (base): if pH drops, the reaction will proceed to the…

A

left

90
Q

A substance that reduces the hydrogen ion in solution

A

base

91
Q

H2C03 —> HCO3- + H+ is an example of a…

A

weak acid

92
Q

Know the PH scale

A

….

93
Q

List two threats to water quality on earth

A

a. acid precipitation (rain, snow pH < 5.2)

b. CO2 in the air (greenhouse effect)

94
Q

In acid precipitation, rain, snows or fog have a pH ____ than what?

A

less than 5.2

95
Q

The green house effect is due to what non-polar compound in the atmosphere

A

CO2 (linear)

Biology 111 (4 decks)

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