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AP Bio > Life's Chemical Basis > Flashcards

Life's Chemical Basis Flashcards

(62 cards)

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1
Q

matter

A

takes up space and has mass

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2
Q

basic ingredient of matter

A

element

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3
Q

element

A

substance that cannot be

broken down into other substances by chemical reactions (cannot be chemically broken down.) Found on periodic table.

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4
Q

compound

A

Two or more elements

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5
Q

4 most important elements (96% of living matter):

A

C, O, H, N (in order of amount)

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6
Q

Atom

A

smallest unit of an element

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7
Q

parts of atom

A

neutron, proton, electron

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8
Q

neutron

A

neutral charge, found in nucleus,

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9
Q

proton

A

positive charge, found in nucleus,

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10
Q

electron

A

negative charge, moves rapidly around the nucleus

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11
Q

valence shell

A

outermost shell of atom

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12
Q

What determines the reactivity of the atom with other atoms?

A

Number of electrons in valence shell

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13
Q

When will an atom be unreactive or reactive?

A

Unreactive if shell is full and vv

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14
Q

full valence shell

A

full=8 electrons

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15
Q

Chemical bonds

A

form when atoms with

incomplete valence shells interact to produce complete valence shells

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16
Q

Chemical reactions

A

break or form chemical bonds to

change reactants into products

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17
Q

law of conservation of matter

A

cannot be created or destroyed

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18
Q

What happens to matter during a reaction bc of the law of CoM?

A

conserved

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19
Q

Are chemical reactions reversible?

A

Most

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20
Q

When is chemical equilibrium reached?

A

when the forward and backward

reaction rates are equal

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21
Q

types of bonds

A

ionic, covalent (nonpolar and polar)

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22
Q

Ionic bonds-

A

form when electrons are

transferred from one atom to the other

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23
Q

ions

A

Resulting atoms of ionic bonds are called ions, and positive and
negative charges of ions?
(ion–charged atom/s)

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24
Q

covalent bonds

A

electrons are shared, occurs between two
atoms of
similar pulls on electrons

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25
electronegativity--
pull on electron
26
electronegativity trend
right and up on pd table-stronger electronegativity
27
Nonpolar covalent
electrons are shared | equally--identical bond
28
Polar covalent
electrons are shared unequally
29
pole
charge
30
significance of polar covalent bonds in charge
Bond is closer to atom with higher pull and | produces a negative charge, or pole, near that atom
31
Where are slightly positive poles found?
area around atom w weaker pull
32
H2O poles
O2 a slight negative charge--stronger pull on electron than hydrogen
33
Hydrogen Bonds
weak bonds between molecules
34
When do H bonds form?
Form when positively charged hydrogen atom in one | covalently bonded molecule is attracted to a negatively charged area of another covalently bonded molecule
35
Example of H bonds
Example- in water molecules- helps in cohesion between | molecules
36
Properties of Water due to H bonds
cohesion, adhesion, Capillary action, Surface tension, Versatile solvent, high heat of vaporization, high heat capacity
37
cohesion
water is self attracted
38
adhesion
water is attracted to other molecules
39
Capillary action-
water can be pulled up thin tubes | against pull of gravity (combo of cohesion and adhesion)
40
Ex of Capillary action-
meniscus--moves up sides of tube of graduated cylinder, forming a curve/meniscus--measure the bottom of meniscus; happens with water in trees-small tubes in plants used for transferring water. called xylem tubes, and since they have no pumping organ it can just move through physical means, including CA.
41
Surface tension
the surface of water exposed to the air is | difficult to puncture--you can, but there's an added resistance
42
high heat capacity
compared to other substances, it takes | water a large amount of heat in order to raise its temp by 1d C
43
Why does water have a high heat capacity
heat first needed to break H bonds, then the water molecules start moving faster.
44
how does water's high heat capacity help the environment?
helps minimize variations in atmospheric | temperature throughout the planet.
45
high heat of vaporization
a lot of heat is required to | change water from a liquid to a gas
46
Why does evaporation have a cooling effect on the environment?
high heat of vaporization--bc it takes heat to do, so it's subtracting heat--same with sweat. we use heat to sweat, using it up from our bodies.
47
Why does ice float on its surface?
ice is less dense than water (d=m/v ice has more air spaces H bonds always breaking and forming in water)
48
Why is water a versatile solvent?
because of the fact that it is polar- it is attracted to other polar/charged substances and breaks them apart the charges can help draw the molecules of opposite charge apart to dissolve
49
solvent
dissolves other substances easily
50
Why is ice less dense than water
This is due to the fact that when the water molecules slow down, each water molecule forms four permanent H bonds to other water molecules, spreading out molecules + creating air spaces
51
What does ice's less dense status allow for during the winter?
This allows bodies of water to have a protective insulating layer on top during the winter time.
52
solute
gets dissolved
53
Hydrophilic substances-
attracted to water--polar or charged
54
hydrophobic substances
repels water-non-polar substances
55
H+ ion interchangeable with...
H+ ion interchangeable with a proton
56
Why is water neutral?
neutral bc H+ and OH- amounts are equal
57
alkaline
alkaline=base
58
What two ions can water dissociate into?
OH-, base, hydroxide ion, and H+, hydrogen ion, acid (same as hydronium ion when sometimes it attaches off)
59
pH
The concentration of H+ ions is measured in pH units. Each pH unit increase is tenfold difference in H+ ion concentration 10*, not 10+!!!!
60
pH range
pH ranges from 0 (most acidic) to 14 (most basic)
61
Neutral solution
has equal H+ and OH- pH of 7. The internal pH of | most living cells must be kept close to 7.
62
pH of 4
pH of 4 = 1* 10^-4, or .0001 H+ ions | exponent is pH

AP Bio (35 decks)

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