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Biology 111 > Chapter 3: Water > Flashcards

Chapter 3: Water Flashcards

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
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
1 g
26
T/F as a liquid evaporates, the surface of the liquid that remains behind cools down
true
27
1 g of water at 25°C needs 580 cal of heat, much higher than _______
alcohol (so water has a higher heat of vaporization - more resistant to changes in temperature and less evaporative)
28
What, as mentioned in the lecture, contributed to the stability of lake temperatures?
evaporative cooling
29
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?
Evaporative cooling
30
________ of water from the leaves of a plant helps the tissues in the leaves from becoming too warm in the sunlight
evaporation
31
Evaporation of sweat from the human skin has what effect?
Dissipates body heat
32
T/F Evaporation does not prevent terrestrial organisms from overheating
False
33
Why is ice less dense than liquid water?
Stable hydrogen bonding occurs between hydrogen atoms in ice (where as in water, the bonds are breaking and reforming)
34
Ice is less dense than water due to _______ _______
hydrogen bonding
35
T/F Ice is more dense than liquid water due to hydrogen bonding
False
36
Ice floats on top of water because of....
hydrogen bonding (stable hydrogen bonding between hydrogen elements in ice)
37
At 0 C, water molecules become locked into a ____ ____. Each water molecule is hydrogen-bonded to ____ partners
crystalline lattice, four partners
38
T/F Each water molecule in ice is hydrogen-bonded to four partners
True
39
Liquid water is always at a state of dynamic adjustment, so it doesn't have a chance to be locked into a ____ ____
crystalline lattice
40
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
crystalline
41
At _______ Water behaves like other liquids, expanding as | it warms and contracting as it cools
4 degrees celsius
42
At _______ Water molecules become locked into a crystalline lattice, each water molecule hydrogen-bonded to four partners
0 degrees celsius
43
When ice is warmed to 4 degrees celsius, what do you expect to happen?
Water behaves like other liquids. It will expand when warmed and constrict when cooled.
44
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.
10% less dense
45
T/F Floating ice insulates the liquid water below, preventing it from freezing and allowing life to exist under the frozen surface
True
46
A dissolving agent
solvent
47
Substance that is dissolved
solute
48
Liquid that is a completely homogenous mixture of two or more substances
Solution
49
Sphere of water around each dissolved ion
hydration shell
50
T/F A solution MUST be homogenous for it to be a true solution
True
51
2 types of molecules that are water-soluble
ionic or non-ionic polar molecules
52
Solvent
a dissolving agent
53
Solute
substance that is dissolved
54
Solution
a liquid that is completely homogenous mixture of two or more substances
55
Hydration shell
sphere of water molecules around each dissolved ion
56
These molecules are water-soluble:
ionic or non-ionic polar molecules
57
Has an affinity for water
hydrophilic substances
58
hydrophilic substances have a....
affinity for water
59
What substances have an affinity for water?
hydrophilic substances
60
A mixture of suspended molecules
colloid
61
A colloid is ____ but has very big molecules such as cellulose (cotton)
hydrophilic
62
Is a colloid a stable or unstable suspension of fine particles in a liquid?
A colloid is a stable suspension of fine particles in a liquid
63
T/F a colloid is made up of molecules or compounds
molecules
64
Nonionic and non-polar substances
hydrophobic
65
What two types of substances are likely to by hydrophobic
nonionic and non-polar substances
66
Cell membrane components are what type of substances (mentioned in lecture)
hydrophobic (outside) and hydrophilic (inside)
67
Oil is a _____ or _____ substance. This explains why you see two layers in salad dressing.
Hydrophobic
68
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
hydrophilic, hydrophobic heads (water does not free flow in and out of cells)
69
Define molecular weight.
____ g/mol
70
the number of atoms or molecules in one mole of a substance
6.023x 10^23 atoms/molecules
71
the concentration of a solution expressed as the number of moles of solute (m) per liter of solution (L)
molarity (m/L)
72
You have 1 mole of of hydrogen atoms. How many atoms do you have?
6.023x10^23
73
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)
---
74
Molality units:
mol solute / kg solvent
75
T/F Molality deals with mass and molarity deals with volume
True
76
Molality:
moles of solute / kg solvent
77
A substance that increases the hydrogen ion in a solution
acid
78
Name on strong acid (disassociation reaction) mentioned in lecture
HCL - H+ and Cl-
79
The higher the _____, the lower the PH number
acidity
80
Ph of 8 means the solution has _____ hydrogen ions in solution than in a solution with a PH of 12
less
81
The specific disassociation reaction of a weak acid (mentioned in lab)
H2C03 -> HCO3- + H+
82
What is the basic difference between strong and weak acids:
partial vs. complete disassociation
83
Know the logarithmic laws:
PH = - log [H+] pOH = - log [OH-}
84
A pH unit represents a ____ difference in H+ and OH- concentrations
tenfold
85
A _____ is a substance that minimizes the changes int he concentrations of hydrogen ions
buffer
86
Strong alkali vs. Weak alkali
NaOH ----> Na+ and OH- NH3 + H+ -----> NH4+
87
Draw out the reaction which the PP mentioned as part of the buffer concept
H2CO3 ⇔ HCO3- + H+
88
Addition of a buffer (acid): if pH rises, the reaction will proceed to the....
right
89
Addition of a buffer (base): if pH drops, the reaction will proceed to the...
left
90
A substance that reduces the hydrogen ion in solution
base
91
H2C03 ---> HCO3- + H+ is an example of a...
weak acid
92
Know the PH scale
....
93
List two threats to water quality on earth
a. acid precipitation (rain, snow pH < 5.2) | b. CO2 in the air (greenhouse effect)
94
In acid precipitation, rain, snows or fog have a pH ____ than what?
less than 5.2
95
The green house effect is due to what non-polar compound in the atmosphere
CO2 (linear)

Biology 111 (4 decks)

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