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My Packs: AP Biology > (Unit 1) Chapter 3: Water and the Fitness of the Environment > Flashcards

(Unit 1) Chapter 3: Water and the Fitness of the Environment Flashcards

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1
Q

What is the biological medium here on Earth?

A

Water

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2
Q

_____-________ of Earth’s surface is submerged in _____

A

Three-quarters

Water

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3
Q

The _______ distribution of electrons makes water a _____ molecule

A

Unequal

Polar

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4
Q

Who highlights the importance of water to life? Where?

A

Lawrence Henderson

In a book: The Fitness of the Environment

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5
Q

In water, the slightly ________ hydrogen is attracted to the slightly ________ oxygen of a nearby molecule

A

Positive

Negative

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6
Q

What are molecules of water held together by?

A

Hydrogen bonds

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7
Q

True or False:

When water is in liquid form, the hydrogen bonds are very strong

A

False, the hydrogen bonds are very fragile each about 1/20 as strong as a covalent bond

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8
Q

What is the phenomenon called when hydrogen bonds hold water together?

A

Cohesion

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9
Q

Define:

Adhesion

A

Clinging of one substance to another

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10
Q

Define:

Surface tension

A

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

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11
Q

True or False:

Water has greater surface tension than most other liquids

A

True

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12
Q

Define:

Kinetic energy

A

The energy of motion, anything that moves has kinetic energy

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13
Q

True or False:

Heat is a form of energy

A

True

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14
Q

Define:

Temperature

A

A measure of heat intensity that represents the average kinetic energy of the molecules, regardless of volume

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15
Q

For a given body of matter, the amount of ____ is a measure of the matter’s total _______ energy due to motion of its _________

A

Heat
Kinetic
Molecules

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16
Q

If the amount of heat is a measure of the matter’s total kinetic energy, what does the heat depend on?

A

Depends in part on the matter’s volume

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17
Q

In what temperature scale does water freeze at 0 degrees and boil at 100 degrees at sea level?

A

Celsius Scale

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18
Q

What is a calorie?

A

A unit of heat

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19
Q

Define:

1 cal

A

The amount of heat it takes to raise the temperature of 1 g of water by 1 degrees Celsius (or the the amount of heat 1 g of water releases when cooled by 1 degrees Celsius)

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20
Q

What does kcal represent?

A

Kilocalories

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21
Q

Define:

1 kcal

A

The amount of heat needed to raise 1 kg of water by 1 degrees Celsius

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22
Q

What is a joule?

A

An energy unit

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23
Q

Convert joule to calories and calorie to joules

A

1 J = 0.239 cal

1 cal = 4.184 J

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24
Q

Define:

Specific heat

A

The amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degrees Celsius

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25
Q

State the specific heat of water

A

1 cal/g/degrees Celsius

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26
Q

The transformation from a liquid to a gas is called:

A

Vaporization or evaporation

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27
Q

Define:

Heat of vaporization

A

The quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state

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28
Q

True or False:

Water has a high specific heat but a low heat of vaporization

A

False, for the same reason that water has a high specific heat, it also has a high heat of vaporization relative to most other liquids

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29
Q

The cooling of the surface of the liquid that remains behind after evaporation is known as:

A

Evaporative cooling

30
Q

What effect does the high amount of energy required to vaporize water have?

A

Helps moderate Earth’s climate

31
Q

What effect does the evaporative cooling of water have?

A

Contributes to the stability of temperature in lakes and ponds and provides a mechanism that prevents terrestrial organisms from overheating

32
Q

Define:

Solution

A

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

33
Q

Define:

Solvent

A

The dissolving agent of a solution

34
Q

Define:

Solute

A

The substance that is dissolved in a solution

35
Q

Define:

Aqueous solution

A

A solution which water is the solvent

36
Q

Define:

Hydration shell

A

The sphere of water molecules around each dissolved ion

37
Q

True or False:

Compounds have to be ionic to dissolve in water

A

False, compounds do not have to be ionic to dissolve in water (e.x. sugar)

38
Q

Explain what water molecules do to a table salt molecule (2)

A

The oxygen region of water attracts to the positively charged ion (sodium), forming a hydration shell
The hydrogen region of water attract to the negatively charged ion (chlorine), forming another hydration shell

39
Q

Any substance that has an affinity for water is said to be:

A

Hydrophilic

40
Q

Define:

Colloid

A

A stable suspension of fine particles in a liquid

41
Q

When a substance is hydrophobic, what properties does it have? (2)

A

Non-ionic, non-polar (or some other reason cannot form hydrogen bonds)
Seem to repel water

42
Q

Define:

Molecular Mass

A

The sum of the masses of all the atoms in a molecule

43
Q

Biological chemistry is “___” chemistry

A

Wet

44
Q

What does a mole represent?

A

An exact number of objects (6.02 * 10^23)

45
Q

What is the number of objects in a mole known as?

A

Avogradro’s number

46
Q

How many daltons are in 1 gram?

A

6.02 * 10^23 (Avogadro’s Constant)

47
Q

Define:

Molarity

A

The number of moles of solute per liter of solution

48
Q

If sucrose has a molecular mass of 342 daltons, how grams does 1 mol of sucrose weigh?

A

342 grams

49
Q

What is a hydrogen ion?

A

A single proton with a charge of +1

50
Q

What is a hydroxide ion?

A

An oxygen and hydrogen ion with a charge of -1

51
Q

Occasionally, the hydrogen atom participating in a hydrogen bond between two water molecules shifts from on molecule to the other. Explain this reaction

A

Originally, 2 water molecules are attracted via a hydrogen bond
Now, the hydrogen ion (proton) of one water molecule binds to the other water molecule to form a hydronium ion (H3O+), leaving a hydroxide ion (OH-)

52
Q

Define:

Acid

A

A substance that increases the hydrogen ion concentration of a solution

53
Q

Define:

Base

A

A substance that reduces the hydrogen ion concentration of a solution

54
Q

True or False:

The conversion of water to hydronium and hydroxide ions is a reversible reaction

A

True

55
Q

What do biologists use to describe how acidic or basic something is?

A

pH scale

56
Q

True or False:

The dissociation of water is common and can change the acidity of the water

A

False, the dissociation of water is statistically rare and only adding certain kinds of solutes can change how acidic/basic the water is

57
Q

How do acids increase the hydrogen ion concentration of a solution?

A

When acids dissolve in water, they donate additional H+ to the solution

58
Q

How do bases reduce the hydrogen ion concentration of a solution? (2)

A

Some accept hydrogen ions (e.x. Ammonia)

Some dissociate, forming hydroxide ions that combine with hydrogen ions to form water (e.x. Sodium hydroxide)

59
Q

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

A

Strong base/acid dissociates completely when mixed with water
Weak base/acid reactions with water is reversible (e.x. Ammonia can accept H+ and then release H+)

60
Q

In any aqueous solution at __ degrees Celsius, the product of the __ and ___ concentrations is constant at __^___. This can be written as:

A 
25
H+
OH-
10^-14
[H+][OH-] = 10^-14
61
Q

What is the pH of a solution defined as?

A

The negative logarithm (base 10) of the hydrogen ion concentration

62
Q

As pH increases, H+ concentration ________

A

Declines

63
Q

If the solution of a pH is 10, what is the concentration of the hydroxide ions?

A

10^-4 M

64
Q

In molarity, what is how is a 1 mol/L solution indicated?

A

1 M solution

65
Q

Define:

Buffers

A

Substances that minimize changes in the concentrations of H+ and OH- in a solution

66
Q

What is an example of a buffer? State the reaction that this buffer undergoes

A

Carbonic acid (H2CO3), formed when CO2 reacts with water in blood plasma)
When H+ concentration in blood falls, the carbonic acid dissociates to replenish hydrogen ions
When H+ concentration in blood rises, the bicarbonate combines with the H+ to form carbonic acid again

67
Q

Define:

Acid precipitation

A

Rain, snow, or fog with a pH lower (more acidic) than pH 5.2

68
Q

What is the pH of uncontaminated rain around?

A

5.6

69
Q

Define:

Calcification

A

The production of calcium carbonate (CaCO3) by corals and other organisms

70
Q

What is the calcification in corals and such related to?

A

The levels of CO3(2-) in the water

71
Q

When CO2 dissolves in seawater, it reacts with water to form what?

A

Carbonic acid

72
Q

Almost all carbonic acid in seawater dissociates into what two ions?

A

Bicarbonate (HCO3-) and Carbonate (CO3(2-))

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