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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
nonpolar covalent bonds
electrons are shared equally - neither is more electronegative
26
polar covalent bonds
one atom is more electronegative than others ; atoms DO NOT share electrons equally Ex. water
27
unequal sharing of electrons causes...
partial positive/negative charge for each atom or molecule
28
Ionic bonds
complete transfer of electrons between atoms which form cations and anions
29
a charged atom is called an
ion
30
ionic meaning
attraction between cation and anion
31
weak chemical bonds
bonds in order from strongest to weakest ; london dispersion forces
32
INTRAmolecular
within atoms
33
INTERmolecular
between atoms
34
how does a hydrogen bond form?
when a hydrogen atom bonds to a highly electronegative atom
35
transport proteins (hemoglobin)
must have globular shape to carry 02 in red blood cells -
36
electronegative atoms
sulfur, hydrogen, fluorine, oxygen
37
Van der waals interaction
A weak force of attraction between electrically neutral molecules that collide with or pass very close to each other.
38
antibodies
specific proteins made by white blood cells - kills antigen (bacteria/virus) ; anything that causes an immune response
39
shape of water
bent
40
acids
- 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
bases
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
neutral
Water is typically considered neutral The H+ and OH- ions cancel each other out 7 is neutral
43
Amphoteric
can act as either a base or acid -
44
buffers
Substances that prevent large fluctuations in pH but DO NOT neutralize the solution
45
buffering system uses what
carbonic acid and biocarbonate ion
46
cells are what % water?
70-95%
47
properties of water
- 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
adhesion
- 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
cohesion
- WATER BONDING TO ITSELF - High surface tension - High heat capacity (amount of energy needed to move temp one degree) - High heat of vaporization
50
waters special properties are due to what?
bent shape
51
solution
homogeneous mixture that consists of 2 parts
52
solvent
substance that dissolves another
53
solute
substance BEING dissolved
54
polar only mixes with... nonpolar only mixes with...
polar ; nonpolar
55
Alcohol dissolves in both water and oil. Explain how this is possible
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
Since most substances dissolve in water (including polar covalent and ionic substances) water is referred to as the..
universal solvent
57
water is less dense as a solid
- 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
Is there a biological/ecological advantage to the difference in density?
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
nucleic acid shape
double helix - allows for DNA replication
60
proton charge determines -----
element
61
neutron charge determines -----
isotope
62
electron charge determines ------
behaivior
63
radioactive isotopes
- unstable forms of elements that decay over time, releasing radiation in the process - giving off energy ; follow around
64
Stanley Millers experiment
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 (7 decks)

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