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senior year > ap bio quiz 9/30 > Flashcards

ap bio quiz 9/30 Flashcards

1
Q

Elements are??

A

substances that cannot be broken down into other substances by chemical reactions

Ex. fluorine, carbon, hydrogen

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2
Q

what makes up 96% of living matter?

A

carbon, hydrogen, oxygen, nitrogen (CHON)

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3
Q

What do the remaining 4% of living things consist of?

A

calcium, phosphorus, potassium, sulfur

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4
Q

Trace elements

A

require by an organism in small quantities

Ex. Iron, Iodine

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5
Q

what does iodine do

A

makes a hormone called thyroxine (from thyroid gland) that activates ALL body cells and controls metabolism.
- Often put into salt (fortified)

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6
Q

what does iron do

A

allows oxygen to bond
- found in hemoglobin

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7
Q

An elements properties depend on what?

A

The structure of its atoms

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8
Q

what is found in the atomic nucleus

A

protons and neutrons

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9
Q

what charge goes around the nucleus’ rings

A

negative ; electron

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10
Q

how many electrons does an atom have

A

8

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11
Q

what is an isotope

A

two atoms of an element that differ in number of neutrons
Radioactive isotopes decay spontaneously giving off particles and energy

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12
Q

hydrolysis

A

breaking down a polymer

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13
Q

An electron state of potential energy is called …

A

its energy level or electron shell

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14
Q

The chemical behavior of an atom is determined by..

A

the distribution of electrons in electron shells

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15
Q

where are valence electrons found?

A

outermost shell

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16
Q

chemical behaivior is determined by

A

valence shell

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17
Q

Elements with full valence shells are not chemically radioactive because they are…

A

STABLE

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18
Q

covalent bond

A

sharing of a pair of valence electrons by two atoms

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19
Q

molecule

A

consists of 2 or more atoms held together by covalent bonds

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20
Q

double covalent bond/ double bond

A

sharing of TWO pairs of valence electrons

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21
Q

structural formula

A

notation used to represent atoms and bonding
Ex. H-H = H2

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22
Q

compound

A

2 or more different elements

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23
Q

bonding capacity is called

A

the atoms’ valence

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24
Q

electronegativity

A
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25
Q

nonpolar covalent bonds

A

electrons are shared equally
- neither is more electronegative

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26
Q

polar covalent bonds

A

one atom is more electronegative than others ; atoms DO NOT share electrons equally

Ex. water

27
Q

unequal sharing of electrons causes…

A

partial positive/negative charge for each atom or molecule

28
Q

Ionic bonds

A

complete transfer of electrons between atoms which form cations and anions

29
Q

a charged atom is called an

A

ion

30
Q

ionic meaning

A

attraction between cation and anion

31
Q

weak chemical bonds

A

bonds in order from strongest to weakest
; london dispersion forces

32
Q

INTRAmolecular

A

within atoms

33
Q

INTERmolecular

A

between atoms

34
Q

how does a hydrogen bond form?

A

when a hydrogen atom bonds to a highly electronegative atom

35
Q

transport proteins (hemoglobin)

A
36
Q

electronegative atoms

A

sulfur, hydrogen, fluorine, oxygen

37
Q

Van der waals interaction

A

A weak force of attraction between electrically neutral molecules that collide with or pass very close to each other.

38
Q

antibodies

A

specific proteins made by white blood cells
- kills antigen (bacteria/virus) ; anything that causes an immune response

39
Q

shape of water

A

bent

40
Q

acids

A
  • Compounds that release hydrogen ions (H+)
    Substances containing acids are described as acidic
  • As the [H+] INCREASES the pH DECREASES
    Inverse relationship
    On the LEFT side of the pH scale
    0-6
    “Sour”
    Vinegar, coffee/tea, soda, alcohol, citrus fruit
41
Q

bases

A

Compounds that accept hydrogen ions (H+)
Substances containing bases are described as basic or alkaline
“Bitter”
Baking soda, egg whites, soaps, shampoos, ammonia
On the RIGHT of the pH scale
8-14

42
Q

neutral

A

Water is typically considered neutral
The H+ and OH- ions cancel each other out
7 is neutral

43
Q

Amphoteric

A

can act as either a base or acid

-

44
Q

buffers

A

Substances that prevent large fluctuations in pH but DO NOT neutralize the solution

45
Q

buffering system uses what

A

carbonic acid and biocarbonate ion

46
Q

cells are what % water?

A

70-95%

47
Q

properties of water

A
  • Keeps mucosal membranes from drying out (eyes, mouth, etc.)
  • Regulates body temperature
    Maintains optimal digestive function and elimination
  • Supports the efficient removal of toxins and waste from internal organs
    Permits the absorption of life-essential nutrients and energy
  • Allows body fluids (blood) to deliver hormones, nutrients, and oxygen
48
Q

adhesion

A
  • water bonding to OTHER THINGS
  • capillary actions due to
  • Water allows all metabolic reactions to occur by dissolving all minerals and nutrients (provides an aqueous environment)
  • Versatility as a solvent
49
Q

cohesion

A
  • WATER BONDING TO ITSELF
  • High surface tension
  • High heat capacity (amount of energy needed to move temp one degree)
  • High heat of vaporization
50
Q

waters special properties are due to what?

A

bent shape

51
Q

solution

A

homogeneous mixture that consists of 2 parts

52
Q

solvent

A

substance that dissolves another

53
Q

solute

A

substance BEING dissolved

54
Q

polar only mixes with…
nonpolar only mixes with…

A

polar ; nonpolar

55
Q

Alcohol dissolves in both water and oil. Explain how this is possible

A

Alcohol can dissolve in both water and oil because of the polar and nonpolar areas of alcohol. Polar substances dissolve other polar substances because of hydrogen bonding, so, because of alcohol’s polar region, water can dissolve it. Alcohol also has a nonpolar region, so this allows it to also dissolve in oil

56
Q

Since most substances dissolve in water (including polar covalent and ionic substances) water is referred to as the..

A

universal solvent

57
Q

water is less dense as a solid

A
  • Hydrogen bonding accounts for the difference in density between liquid water and ice
  • water freezes = hydrogen bonds stabilize which means water molecules are further apart
58
Q

Is there a biological/ecological advantage to the difference in density?

A

Floating ice helps to insulate the water below (little temperature change) this prevents further freezing and thus, allows life to exist under the frozen surface

59
Q

nucleic acid shape

A

double helix
- allows for DNA replication

60
Q

proton charge determines —–

A

element

61
Q

neutron charge determines —–

A

isotope

62
Q

electron charge determines ——

A

behaivior

63
Q

radioactive isotopes

A
  • unstable forms of elements that decay over time, releasing radiation in the process
  • giving off energy ; follow around
64
Q

Stanley Millers experiment

A

demonstrated abiotic synthesis of organic compounds

  • experiments support the idea that abiotic synthesis of organic compounds, perhaps near volcanoes, could have been a stage in the origin of life
  • used inorganic matter to make organic matter

senior year (6 decks)

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