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med 103- biology i > 7. ICE > Flashcards

7. ICE Flashcards

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AP® Biology flashcards
1
Q
  1. What is ice?
A
  • it is the solid form of water
  • it is less dense than liquid water
  • it floats in liquid water
  • it insulates the bodies of water underneath the surface of the ice
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2
Q
  1. How does ice insulate the bodies of water underneath it?
A
  • ice preserves the temperature of the water
  • it keeps the temperature of the liquid underneath at a constant temperature
  • this allows for life forms to survive in the water underneath the ice
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3
Q
  1. What is the difference in the hydrogen bonds between liquid water and ice?
A
  • the hydrogen bonds in ice are more ordered than in liquid water
  • these hydrogen bonds are stable
  • this means that there are less hydrogen bonds
  • this gives ice a lower density
  • in liquid water, the hydrogen bonds are not arranged in a particular order
  • they are scattered about
  • these hydrogen bonds are constantly breaking and re-forming
  • this means that there are more hydrogen bonds
  • this makes the water more dense
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4
Q
  1. What kind of solvent is water?
A
  • it is a very versatile solvent
  • this is due to its polarity
  • it can form hydrogen bonds easily
  • it can form aqueous solutions
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5
Q
  1. What happens when the different regions of the polar water molecules interact with ionic compounds?
    What is the name of these ionic compounds?
A
  • they dissolves them
  • they are called solutes
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6
Q
  1. What is a solution?
A
  • Solution= solvent + solute
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7
Q
  1. What is a solution?
A
  • it is a liquid that is a homogeneous mixture of substances
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8
Q
  1. What is a solvent?
A
  • it is the dissolving agent of a solution
  • it is the liquid in which the solute dissolves in
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9
Q
  1. What is a solute?
A
  • it is the substance that is dissolved in the solvent
  • this forms the solution
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10
Q
  1. What is an aqueous solution?
A
  • it is one in which water is the solvent
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11
Q
  1. Explain how the Sodium Chloride (NaCl) Aqueous solution is formed?
A
  • the negative oxygen atoms of the polar water molecule are attracted to the sodium cations in the sodium chloride salt
  • the positive hydrogen atoms of the polar water molecule attach to the chloride anions in the sodium chloride salt
  • this breaks apart the ionic bonds between sodium and chlorine
  • it dissolves the sodium chloride crystal into the water
  • the sodium chloride crystal is no longer differentiable
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12
Q
  1. What happens when water interacts with polar molecules (such as proteins)?
A
  • it dissolves them
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13
Q
  1. What is a hydrophilic substance?

PROVIDE EXAMPLES.

A
  • it is a substance that has an affinity for water

EG:L polar solutions, ionic molecules

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14
Q
  1. What are hydrophobic substances?

PROVIDE EXAMPLES.

A
  • they do not have an affinity for water
  • they are not attracted to water
  • they have no opposing charges
  • they cannot attract the partially charged atoms of the water molecule

EG: non-polar solutions, non ionic molecules

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15
Q
  1. What is important to calculate due to the fact that most biochemical reactions occur in water?
A
  • it is important to calculate the concentration of solutes in an aqueous solution
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16
Q
  1. What is a mole?
A
  • it represents the exact number of molecules of a substance in a given mass
  • 1 molecule of a substance has the same number of molecules as 1 mole of any other substance
    (6.02 x 10 to the 23 molecules)
    (Avogadro’s number)
    (it is a fixed number)
  • 1 mole of a substance has the same mass in grams as its molecular mass
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17
Q
  1. What is the Molecular Mass?
    (MW)
    (Molecular Weight)
A
  • it is the sum of the atomic mass of the atoms in a molecule
18
Q
  1. What is the Molarity (M)?
A
  • it is the number of moles of solute per litre of solution
    (moles/L)
19
Q
  1. What does the dissociation of water molecules lead to?
A
  • it leads to acidic and basic conditions
  • these affect living organisms
20
Q
  1. What two ions does water dissociate into?
A
  • hydronium ions (H+)
  • hydroxide ions (OH-)
21
Q
  1. What can changes in the concentrations of these ions result in?
A
  • they can have a large affect on living organisms
22
Q
  1. What is an acid?
A
  • it is a proton donor
  • it is any substance that increases the hydrogen ions concentration (H+) of a solution
  • it does this by releasing H+
23
Q
  1. What is a base?
A
  • it is any substance that reduces the hydrogen ion concentration of a solution
  • it does this by accepting H+ or by releasing OH-
24
Q
  1. What is pH?
A
  • it is the measure of the concentration of ions
  • it is the negative logarithm of 10
25
Q
  1. The concentrations of which ions are equal in pure water?
A
  • H+
  • OH-
26
Q
  1. What does the addition of acids or bases to pure water do?
A
  • it modifies the concentrations of H+ and OH-
27
Q
  1. What is the pH scale?
A
  • it describes whether a solution is acidic or basic
28
Q
  1. What is a pH of 7?
A
  • it is neutral
29
Q
  1. What is a pH of less than 7?
A
  • it is acidic
  • it has a higher amount of hydrogen ions
  • it has a lower amount of hydroxide ions
30
Q
  1. What is a pH of greater than 7?
A
  • it is alkaline/basic
  • it has a higher amount of hydroxide ions
  • it has a lower amount of hydrogen ions
31
Q
  1. What does the pH of a solution measure?
A
  • the acidity of the solution
  • this is determined by the relative concentration of hydrogen ions
32
Q
  1. What pH do most biological fluids have?
A
  • they have a pH between 6 and 8
33
Q
  1. What do acids donate in aqueous solutions?
A
  • they donate H+ ions
34
Q
  1. What do bases donate in aqueous solutions?
A
  • they donate OH- ions
  • they also accept H+ ions
35
Q
  1. What pH must the internal pH of cells remain close to and why?
A
  • it must remain close to a pH of 7
  • this is so that the cells can function and be viable (able to work successfully)
36
Q
  1. What are buffers?
A
  • they are solutions that keep the pH of another solution constant
  • they are substances that minimise the changes in the concentrations of hydrogen (H+) and hydroxide (OH-) ions in a solution
  • they consist of an acid- conjugate base pair (or vice versa)
    that reversibly combines with hydrogen ions
37
Q
  1. What do most living organisms have and why?
A
  • they have their own buffers
  • these prevent dramatic changes of pH and keep it close to 7
38
Q
  1. What are the most common buffer system in our blood?
A
  • bicarbonic acid system
  • when the pH in the blood drops
  • the blood becomes acidic
  • hydrogen ions are absorbed
  • this returns the blood to its neutral state
39
Q
  1. How do we convert mmol/l to mg/dl?
A

mmol/l x 18 = mg/dl

40
Q
  1. How do we convert mg/dl to mmol/l?
A

mg/dl / 18 = mmol/l

med 103- biology i (53 decks)

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