Ch 2: Water and Life Flashcards

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1
Q

Define a Polar molecule?

A

A molecule that has unequal sharing of electrons due to one atom being more electronegative than the other.

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2
Q

Why is water considered polar?

A

Water is polar because the oxygen atom is more electronegative than the hydrogens, thus making it so that oxygen has electrons closer to it.

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3
Q

What is hydrogen bonding?

A

Hydrogen bonding is where the partial negative charge of oxygen attracts to the partial positive region of hydrogen from another molecule. Not from the same molecule, those are polar covalent bonds

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4
Q

How many hydrogen bonds can a single water molecule form?

A

4

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5
Q

Distinguish between cohesion and adhesion.

A

cohesion is where water molecules stick to other water molecules, adhesion is from a water molecule to a nonwater polar molecule

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6
Q

Which is demonstrated when you see beads of water on a waxed car hood?

A

adhesion because water is sticking to a nonwater molecule and maybe cohesion because beads of water

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7
Q

Water has high specific heat. What does this mean?

A

This means water can resist change in temperature/it absorbs more heat before 1g of it raises by 1C.

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8
Q

How does water’s specific heat compare to alcohol’s specific heat?

A

Water has higher specific heat than alcohol.

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9
Q

Explain how hydrogen bonding contributes to water’s high specific heat.

A

Hydrogen bonds absorb a ton of energy compared to other bonds in order to break which slightly increases the temperature

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10
Q

Summarize how water’s high specific heat contributes to the moderation of temperature. How is this property important to live?

A

Due to water’s high specific heat, water/hydrogen bonds are able to absorb large amounts of heat from hotter areas until they break, and redistribute them into colder areas reforming. This moderates the temperature. This is important to live because water-based organisms can take more heat.

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11
Q

Define evaporation

A

When atoms in a liquid move rapidly until they break apart and become a gas.

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12
Q

What is the heat of vaporization?

A

The heat needed to make 1g of that liquid into gas, water has a high heat of vaporization

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13
Q

Explain at least three effects of the evaporation property on living organisms.

A
  1. evaporation is need for the water cycle
  2. water’s high heat of vaporization makes it so organisms composed of water are not simply turned into a gas
  3. evaporation is also needed for water to be transported in plants
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14
Q

What would happen if ice did not float.

A

If ice did not float then all bodies of water would simply be filled with ice since the ice will accumulate towards the bottom and will make not only marine life impossible but also human life.

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15
Q

Now, explain why ice floats

A

Ice floats because it is less dense than the water around it

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16
Q

Why is 4°C the critical temperature?

A

at this temperature, hydrogen bonds start to slowly break and space out all the water molecules, this is when water reaches its greatest density.

17
Q

Explain why water is such a fine solvent.

A

water is a good solvent because any ionic or polar substance placed in water will dissolve

18
Q

Distinguish between hydrophobic and hydrophilic substances. Give an example of each.

A

hydrophobic means it can not dissolve in water, this consists of fats oils, or anything nonpolar. Hydrophilic is where anything ionic or polar can dissolve in water, this includes sugars.

19
Q

Oil will float on top of water. Explain this property in terms of hydrogen bonding.

A

Since oils are nonpolar they will repel away without making any hydrogen bonds with water.

20
Q

What two ions form when water dissociates?

A

OH- or hydroxide ion and H+ or hydrogen ion

21
Q

Even a slight change in pH can be harmful! How do buffers moderate pH change?

A

buffers like carbonic acid can receive H+ and redistribute it in places that lack H+

22
Q

Exercise will result in the production of CO2, which will acidify the blood. Explain the buffering system that minimizes blood pH changes.

A

judging by the name, the buffering system could use buffers like carbonic acid in order to regulate pH changes in blood

23
Q

Discuss how CO2 emissions affect marine life and ecosystems.

A

As we know CO2 can make the ocean more acidic, and slight changes in pH are very dangerous. It can hurt marine life and even destroy some ecosystems.

24
Q

define surface tension, and water’s surface tention

A

surface tension is how tough it is to stretch or break the surface of a liquid. Water uses cohesion to attach to other water molecules in order to create some kind of barrier at the surface. Water’s asymmetry gives water strong surface tension.

25
Q

solution

A

a mixture of 2 or more substances

26
Q

solvent

A

dissolves the other substance

27
Q

solute

A

the one being dissolved

28
Q

hydration shell

A

water forms around atoms of the solute and separate the molecules from each other.

29
Q

acid

A

adds more H+ by dissolving into a solution

30
Q

base

A

decreases H+ by accepting more H+

31
Q

name water’s 4 emergent properties

A

4 emergent properties of water: cohesion, moderation of temperature, expansion upon freezing, and versatility as a solvent

32
Q

What happens when hydrogen bonds are formed and broken

A

heat is absorbed when broken and heat is released when made.

33
Q

evaporative cooling

A

As a liquid evaporates, its remaining surface cools. This helps stabilize temperatures.

34
Q

how often do water molecules break and reform

A

almost every one trillionth of a second

35
Q

What is the neutral temp for pH

A

25C 10^-7 for both

36
Q

What is a more basic and acidic solution

A

a basic solution is when OH- is more than H+

37
Q

alkaline

A

a lot of hydroxide ion

38
Q

pH scale

A

1 to 14, increases 10 fold, remember the increase in pH is a decrease in acidity and H+