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BIOL121 > Biology Chp 3 > Flashcards

Biology Chp 3 Flashcards

1
Q

Four Emergent Properties of Water

chp 3

A

Cohesion, moderation of temp, expansion upon freezing, versatility as a solvent

Water is the only substance to exist in natural environment in all three physical states of matter

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2
Q

Polar covalent bonds

chp 3

A

e- spend more time closer to the higher electronegative atoms

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3
Q

Polar molecule

chp 3

A

unequal sharing of e-, overall charge unequally distributed

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4
Q

Cohesion

chp 3

A

hydrogen bonds hold a substance together.
- Contributes to the transport of water and dissolved nutrients in plants

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5
Q

Surface tension

chp 3

A

result of cohesion. a measure of how difficult it is to stretch or break the surface of a liquid

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6
Q

Adhesion

chp 3

A

the clinging of one substance to another.
- Contributes to transport of water and dissolved nutrients in plants

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7
Q

Kinetic Energy

chp 3

A

the energy of motion

atoms and molecules have kinetic energy

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8
Q

Thermal energy

chp 3

A

the kinetic energy accociated with the random movement of atoms or molecules.
- reflects total kinetic energy -> depends on matter’s volume

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9
Q

Temperature

chp 3

A

represents the average kinetic energy of the molecules in a body of matter, regardless of volume

passes from warmer to cooler object

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10
Q

Heat

chp 3

A

Thermal energy in transfer from one body of matter to another

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11
Q

Calorie (cal)

chp 3

A

the amount of heat it takes to raise the temperature of 1g of water by 1° C

Also the amount of heat water releases when lowering in temp

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12
Q

Kilocalorie (1,000cal)

chp 3

A

quantity of heat required to raise the temp of 1kg of water by 1° C

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13
Q

Joule (J)

chp 3

A

1 J = 0.239cal ; 1cal = 4.184 J

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14
Q

Specific Heat

chp 3

A

the amount of heat that must be absorbed or lost for 1g of that substance to change its temp by 1° C.
- HIgher specific heat means less temperature change

The specific heat of H20 = 1cal/(g°C)

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15
Q

Vaporization/Evaporation

chp 3

A

when molecules move fast enough to overcome attractions keeping them together

higher heat = greater evaporation

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16
Q

Heat of vaporization

chp 3

A

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

17
Q

Evaporative cooling

chp 3

A

as a liquid evaporates, the surface of the liwuid that remains behind cools down

18
Q

Floating Ice on Liquid Water

chp 3

A

H20 is less dense as a solid
- due to h-bonding
- floating ice allows for marine life

19
Q

Solution

chp 3

A

completely homogenous mixture of 2 or more substances

20
Q

Solvent

chp 3

A

dissolving agent in a solution

21
Q

Aqueous solution

chp 3

A

solution in which solute is dissolved in water

22
Q

Solute

chp 3

A

substance that is dissolved

23
Q

Hydration shell

chp 3

A

sphere of h20 molecules around each dissolved ion

24
Q

Hydrophilic

chp 3

A

any substance that has an affinity for water

25
Q

Hydrophobic

chp 3

A

substances that repel H2O

major ingredients in cell membranes

26
Q

Molecular mass

chp 3

A

sum of the masses of all the atoms in a molecule

27
Q

mole (mol)

chp 3

A

unit used to measure substances.
- sometimes called molar mass

28
Q

Molarity

chp 3

A

the number of moles of solute per liter of solution

29
Q

Hydroxide Ion (OH-)

chp 3

A

The result of a water molecule losing a proton (H+). has a negative charge

30
Q

Hydronium Ion

chp 3

A

The result of the proton from another water molecule binding to another H20 molecule, making it H3O+

H+ often represents H3O+

31
Q

Dissociation of Water

chp 3

A
  • Statistically rare
  • reversible reaction
32
Q

Acid

chp 3

A

a substance that increases the hydrogen ion concentration [H+] of a solution

33
Q

Base

chp 3

A

a substance that reduces the hydrogen ion concentration of a solution

34
Q

Neutral Solutions

chp 3

A

[H+] = [OH-]

35
Q

Weak Acids

chp 3

A

acids that reversibly release and accept back hydrogen ions

Carbonic Acid

36
Q

pH of any aqueous solution

chp 3

A

In any aqueous solution at 25° C, the product of the H+ and OH- concentrations is constant at 10^-14

Can be written as [H+][OH-] = 10^-14
[H+] = 10^-7
[OH-] = 10^-7

brackets indicate molar concentration

37
Q

pH

chp 3

A

the negative logarithim(base 10) of the H+ concentration.
- Higher pH is more basic while lower pH is more acidic

pH = -log[H+]
internal pH of most living cells must stay close to pH=7

38
Q

Buffers

chp 3

A

A substance that minimizes changes in the concentrations of H+ and OH- in a solution
- accepts hydrogen ions from the solution when they are in excess and donates hydrogen ions when they have been depleted

Most contain a weak acid and it’s corresponding base
One of the buffers that contributes to pH stability in blood is carbonic acid (H2CO3) which is formed when CO2 reacts with H2O in blood plasma

39
Q

Ocean acidification

chp 3

A

when CO3 dissolves in dea water, reacting with H2O to form carbonic acid, which lowers ocean pH

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