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Whisker-Biology > Test 9/26/16 > Flashcards

Test 9/26/16 Flashcards

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1
Q

Explain what it means when we say water has a high specific heat

A
  • The amount of heat that must be absorbed or lost to change 1g of the substance by 1°C
  • Water has a higher specific heat than many water substances
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2
Q

State 4 ways in which waters high specific heat impacts life on Earth

A
  • oceans store heat, making coastal environment milder
  • stabilize ocean temps
  • keeps earths temp within reasonable range
  • helps organisms resist temp changes
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3
Q

Explain how evaporative cooling is important to life.

A
  • helps moderate earths climate
  • stability of temp in lakes and ponds
  • prevents land organisms from overheating (sweat on skin) (water evaporating from plants)
  • high humidity= decreased evaporative rate
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4
Q

Describe what happens to water when it freezes. How is this important to life in earth?

A
  • H-Bonds B/w water molecules stabilize causing a crystalline structure
  • ice is less dense than liquid water and floats
  • insulates lakes and ponds(prevents them from freezing through)
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5
Q

Solute

A

Substance being dissolved

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6
Q

Solvent

A

Dissolving agent

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7
Q

Solution

A

Homogenous mixture of solute and solvent

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8
Q

Know how water dissolves an ionic compound such as NaCl

A

Ok

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9
Q

Describe how even large proteins become dissolved by water

A

Large proteins can have areas of positive and negative charge which affects water

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10
Q

Hydrophilic

A

Attraction for water

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11
Q

What is an example of hydrophilic

A

Cotton/cellulose

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12
Q

Hydrophobic

A

Repels water

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13
Q

Examples of hydrophobic

A

Non ionic and non poor molecules oils

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14
Q

Water is dissociated into what 2 components? Give the equation.

A

H2O—> H(+) + OH(-)

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15
Q

Describe a basic solution

A

More hydroxide (OH-)

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16
Q

Describe an acidic solution

A

More hydrogen (H+)

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17
Q

What percentage of water are cells?

A

70%-95%

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18
Q

What amount of earths surface is submerged in water?

A

3/4

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19
Q

___% of earths water is saltwater

A

97

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20
Q

____% of freshwater is locked in ice caps

A

70

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21
Q

____% of earths freshwater is accessible

A

Less than 1

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22
Q

What are the three physical states of matter

A

Solid and liquid and gas

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23
Q

Polarity

A

The uneven distribution of charge in a molecule

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24
Q

What are the four emergent properties of water?

A
  • waters cohesive behavior
  • its ability to moderate behavior
  • its expansion upon freezing
  • its versatility as a solvent
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25
Q

Cohesion

A

The binding together of like molecules often by hydrogen bonds

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26
Q

Adhesion

A

The attraction between different kinds of molecules

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27
Q

Capillary action

A

As water evaporates from a leaf, the H-Bonds between water molecules allow for the water lower in the plant to be pulled upward

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28
Q

Surface tension

A

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

29
Q

Water has a ______surface tension than most other liquids

A

Greater

30
Q

Element

A

A substance that cannot be broken down to other substances by chemical reaction

31
Q

Compounds

A

A substance consisting of two or more different elements

32
Q

How many natural elements?

A

92

33
Q

How many elements are easential for life?

A

25

34
Q

How many elements make up 96% of all living matter? What are they?

A

4//C, H, O, N

35
Q

Trace elements

A

Elements required by an organism in small quantities

36
Q

What are examples of trace elements?

A

Iron, Iodine, Fluorine

37
Q

Where are protons and neutrons found?

A

In the nucleus of an atom

38
Q

Proton

A

Positive

39
Q

Neutron

A

Neutral

40
Q

Where do electrons travel

A

Around the nucleus in orbit

41
Q

Electron

A

Negative

42
Q

Atomic #

A

Number of protons

43
Q

Mass #

A

Sum or protons plus neutrons

44
Q

Atomic weight/mass

A

An approx of the total mass of an atom

45
Q

Valence

A

The outer electron shell that they travel in

46
Q

Isotopes

A

Atoms that have more neutrons than other atoms of the same element

47
Q

Isotopes can be ______________

A

Stable or radioactive

48
Q

How are radioactive isotopes useful?

A

Traces thru metabolic pathways and diagnostic tools for cancer
-they are picked up by cells just like other isotopes but they can be detected by equipment

49
Q

An atom with a full valence shell is _________________

A

Unreactive and will not readily interact with other atoms

50
Q

Incomplete valence shells=??

A

Chemically reactive

51
Q

What is a nonpolar covalent bond?

A

A bond formed what two atoms are equally electronegative and thus equally share electrons

52
Q

Examples of non polar covalent bonds

A

H2 and 02

53
Q

What is a polar covalent bond?

A

A bond formed when one atom is more electronegative than the other thus pulling the shared electron more to itself. Results in partial charges thru the molecule.

54
Q

Give 2 examples and describe the relative strength of their polarity

A

Methane//Water
-methane is slightly polar because C and H differ slightly in electronegativity. Water has strong polarity because oxygen is much more electronegative than Hydrogen

55
Q

What is an ionic bond?

A

A bond formed when two 2 atoms have an unequal attraction for valence electrons. The more electronegative atom strips the E- from the other atom. The bond is formed because of the attraction B/w the now oppositely charged ions.

56
Q

What 2 ways are weak binding important?

A
  1. Important late biological molecules are held in their functional form by weak bonds
  2. Weak bonds are very reversible which allows two molecules to come together, respond, and then separate
57
Q

Explain how hydrogen bonds form

A

Hydrogen bonds form when a H is covalently bonded to an atom and is also attracted to another electronegative atom. The H of a water molecule will be attracted to the O of an adjacent water molecule.

58
Q

Explain Van der Walls interaction

A

Occur B/w atoms and molecule that are very close together and “hot spots” of electronegativity occur randomly based on the spontaneous travel of the electrons through their orbitals.

59
Q

How does shape influence function?

A

Molecular shape determines how molecules recognize and respond to one another with specificity. Only molecules with conplementary shapes are able to bind to each other by weak bonds

60
Q

Describe the specific example of pain relief

A

Natural endorphins born with receptors in the brain producing pain relief. Morphine, heroine are similar in shape and will bind the same receptors thus having the same effect

61
Q

What is the chemical equation for photosynthesis?

A

6CO2 + 6H2O —-> C6H12O6 + 6O2

62
Q

Explain how the concentration of the reactant affects the rate of the reaction

A

The higher the concentration of reactants l, the more collisions accuse which speeds up chemical reactions.

63
Q

How is chemical equilibrium reached?

A

When the rate at which products are being formed is equal to the rate at which the reactants are being formed.

64
Q

Cation

A

Positive ion

65
Q

Anion

A

Negative ion

66
Q

Chemical bonds

A

Attraction that holds molecules together. Involves valence electrons

67
Q

Which has the strongest bond?

A

Ionic

68
Q

Which has the weakest bond?

A

Hydrogen

Whisker-Biology (31 decks)

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