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Bio 5A Lecture > Chapter 3: Water And Life > Flashcards

Chapter 3: Water And Life Flashcards

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Biology 101 flashcards
1
Q

How much of the earth is covered by water?

A

75%

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2
Q

_____ is the only common substance on Earth to exist in the natural environment in all three physical states of matter.

A

Water

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3
Q

What are warmer climates in the Arctic and smaller ice packs resulting in?

A

Blooms of phytoplankton

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4
Q

Define Polar Covalent Bonds

A

A covalent bond between atoms that differ in Electronegativity. The shared electrons are pulled closer too the more electronegative atom, making it slightly negative and the other slightly positive.

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5
Q

Define Polar Molecule

A

A molecule (such as water) with an uneven distribution of charges in different regions of the molecule.

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6
Q

Are hydrogen bonds fragile when water is in its liquid form?

A

Yes

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7
Q

What is a typical behavior exhibited by hydrogen bonds?

A

They break and re-form with great frequency.

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8
Q

Define Cohesion

A

The linking together of like molecules, often by hydrogen bonds.

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9
Q

How does water move against gravity inside of plants?

A

Cohesion due to hydrogen bonding contributes to the transport of water and dissolved nutrients against gravity of plants. Water from the roots reaches the leaves through a network of water-conducting cells. As water evaporates from a leaf, hydrogen bonds cause water molecules leaving the veins to tug on molecules farther down, and the upward pull is transmitted through the water-conducting cells all the way to the roots.

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10
Q

Define Adhesion

A

The clinging of one substance to another, such as water to plant cell walls by means of hydrogen bonds.

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11
Q

What is related to cohesion?

A

Surface Tension

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12
Q

Define Surface Tension

A

A measure of how difficult it is to stretch or break the surface of a liquid. Water has a high surface tension because of the hydrogen bonds of surface molecules.

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13
Q

Define Kinetic Energy

A

The energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to another matter.

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14
Q

Define Thermal Energy

A

Kinetic energy due to the random motion of atoms and molecules; energy in its most random form.

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15
Q

Is thermal energy the same thing as temperature?

A

No

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16
Q

Define Temperature

A

A measure in degrees of the average kinetic energy (thermal energy) of the atoms and molecules in a body of matter.

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17
Q

Does a pot of coffee has more thermal energy or a swimming pool? Why?

A

A swimming pool.

Although the pot of coffee has a much higher temperature than the water in a swimming pool, the swimming pool contains more thermal energy because of its much greater volume.

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18
Q

Whenever two objects of different temperatures are brought together, thermal energy passes from the _____ to the _____ object until the two are the same temperature.

A

Warmer-Cooler

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19
Q

How does an ice cube cool a drink?

A

An ice cube cools a drink not by adding coolness to the liquid, but by absorbing thermal energy from the liquid as the ice itself melts.

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20
Q

Define Heat

A

Thermal energy in transfer from one body of matter to another.

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21
Q

Define Calorie

A

The amount of heat energy required to raise the temperature of 1 gram of water by 1 degree Celsius; also the amount of heat energy that 1 gram of water releases when it cools down by one degree Celsius. The calorie, usually used to indicated the energy of food content, is a kilocalorie.

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22
Q

Define Kilocalorie

A

A thousand calories; the amount of heat energy required to raise the temperature of 1 kg water by 1 degree Celsius.

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23
Q

Define Joules (J)

A

A unit of energy. 1J= 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 1g of a substance to change its temperature by 1 degree Celsius.

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25
Q

What is another way in which specific heat can be regarded?

A

A measure of how well a substance resists changing its temperature when it absorbs or release heat.

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26
Q

Is heat absorbed or released when hydrogen bonds are formed?

A

Heat is RELEASED

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27
Q

Define Heat of Vaporization

A

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

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28
Q

What is the heat of vaporization of water?

A

580 calories.

29
Q

What effects does the high heat of vaporization of water have?

A

Helps moderate the earth’s climate. C

Accounts for the severity of severe burns. B

A considerable amount of solar heat absorbed by tropical seas is consumed during the evaporation of surface water. Then, as moist tropical air circulates poleward, it releases heat as it condenses and forms rain.

30
Q

Define Evaporative Cooling

A

The process in which the surface of an object becomes cooler during evaporation, a result of the molecules with the greatest kinetic energy changing from the liquid to the gaseous state.

31
Q

What does the evaporative cooling property of water do for the environment?

A

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

32
Q

How does sweating help cool down the body?

A

Evaporation of sweat from human skin dissipates body heat and helps prevent overheating on a hot day when excess heat is generated by a strenuous activity.

33
Q

How does water behave upon freezing?

A

It expands

34
Q

At what temperature does water reach its greatest density?

A

4 degrees Celsius

35
Q

What would happen if the density of solid water was higher than liquid water?

A

Eventually, all ponds, lakes, and even oceans would freeze solid, making life as we know it impossible on earth.

36
Q

What causes global warming?

A

Carbon dioxide and other greenhouse gases.

37
Q

Define Solution

A

A liquid that is a homogenous mixture of two or more substances.

38
Q

Define Solvent

A

The dissolving agent of a solution. Water is the most versatile solvent known.

39
Q

Define Solute

A

A substance that is dissolved in the solution.

40
Q

Define Aqueous Solution

A

A solution in which water in the solvent.

41
Q

Define Hydration Shell

A

The sphere of water molecules around a dissolved ion.

42
Q

Does a compound need to be ionic to dissolve in water?

A

NO

43
Q

Define Hydrophilic

A

Having an affinity (attraction) for water.

44
Q

Define Hydrophobic

A

Having no affinity for water; tending to coalesce and form droplets in water.

45
Q

Define Molecular Mass

A

The sum of the masses of all the atoms in a molecule; sometimes called molecular weight.

46
Q

Define Mole (mol)

A

The number of grams of a substance that equals its molecular or atomic mass in daltons; a mole contains Avogadro’s number of the molecules or atoms in question.

47
Q

How many daltons are there in 1g?

A

6.022x10^23

48
Q

Define Molarity

A

A common measure of solute concentration, referring to the number of moles of solute per liters of solution.

49
Q

Define Hydrogen Ion

A

A single proton with a charge of +1. The dissociation of a water molecule leads to the generation of a hydroxide ion and a hydrogen ion; in water, H+ is not found alone but associates with a water molecule to form a hydronium ion.

50
Q

Define Hydroxide Ion

A

A water molecule that has lost a proton; OH-.

51
Q

Define Hydronium ion

A

A water molecule that has an extra proton bound to it; H3O+, commonly expressed as H+.

52
Q

Does H+ exist on its own in an aqueous solution?

A

No

53
Q

What do double arrows mean in a chemical reaction?

A

It means that it’s reversible.

54
Q

What is the concentration of hydrogen and hydroxide ions in pure water?

A

10^-7 M

55
Q

Define Acid

A

A substance that increases the hydrogen ion concentration of a solution.

56
Q

Define Base

A

A substance that reduces the hydrogen ion concentration of a solution.

57
Q

Which arrows are present in weak/strong acid/base reactions?

A

In the case that the substance at hand is a strong acid/base, the reaction is not reversible and the arrow is one-sided.

In the case that the substance at hand is a weak acid/base, the reaction is reversible and the arrow is double-sided.

58
Q

What is the equation for the product of hydrogen and hydroxide concentrations?

A

[H+][OH-]=10^-14

59
Q

Define pH

A

A measure of hydrogen ion concentration equal to -log [H+] and ranging in value from 0 to 14.

60
Q

What happens to pH as the concentration of the hydrogen ion increases?

A

It decreases.

61
Q

What do the pH ranges indicate?

A

Lower than 7 means it’s an acid.

7 means it’s neutral.

Above 7 means it’s basic.

62
Q

The internal pH of most living cells is close to _____.

A

7

63
Q

Define Buffer

A

A solution that contains a weak acid and its corresponding base. A buffer minimizes changes in pH when acids or bases are added to the solution.

64
Q

Most buffer solutions contain a _____ and its corresponding _____.

A

Weak Acid-Base

65
Q

Define Ocean Acidification

A

The process by which the pH of the ocean is lowered (made more acidic) when excess CO2 dissolves in seawater and forms carbonic acid.

66
Q

Describe the process of ocean acidification.

A

As seawater acidifies, the extra hydrogen ions combine with carbonate ions to form bicarbonate ions, thereby reducing the carbonate ion concentration. The decrease in carbonate ion concentration is significant because the ions are required for calcification, the production of calcium carbonate by many marine organisms, including reef-building corals and animals that build shells.

67
Q

What are the 4 emergent properties of water that contribute to Earth’s suitability for life?

A

Cohesive/Adhesive Properties-Ability to Moderate Temperature-Expansion Upon Freezing-Versatility as a Solvent

CTES. (Cohesive-Temperature-Expansion-Solvent)

68
Q

What is the acronym for Cohesion and Adhesion?

A

CI-AO. Cohesion-Itself; Adhesion-Other

Bio 5A Lecture (16 decks)

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