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AP Biology > Chapter Two > Flashcards

Chapter Two Flashcards

1
Q

matter

A

anything that takes up space and has mass

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2
Q

element

A

a substance that cannot be broken down to other substances by chemical reactions

92 occur in nature

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3
Q

compound

A

a substance consisting of two or more different elements combined in a fixed ratio

has chemical and physical characteristics different than those of its elements (due to emergent properties)

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4
Q

essential element

A

a chemical element required for an organism to survive, grow, and reproduce

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5
Q

4 elements that make up 96% of living matter

A

oxygen, carbon, hydrogen, nitrogen

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6
Q

trace elements

A

an element indispensable for life but required in minute amounts

iron, iodine

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7
Q

atom

A

the smallest unit of matter that still retains the properties of an element

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8
Q

proton

A

positive charge

found in the nucleus of an atom

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9
Q

neutron

A

no charge

found in the nucleus of an atom

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10
Q

electron

A

negative charge

stays in the vicinity of the nucleus due to an attraction to the proton

only subatomic particle directly involved in chemical reactions

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11
Q

atomic nucleus

A

an atom’s dense, central core that contains protons and neutrons

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12
Q

dalton (atomic mass unit)

A

a measurement of mass of atoms and subatomic particles

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13
Q

atomic number

A

the number of protons in the nucleus (same as the number of electrons)

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14
Q

mass number

A

the sum of the number of protons and neutrons in an atom’s nucleus

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15
Q

atomic mass

A

the total mass of an atom, which is the mass in grams of 1 mole of an atom

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16
Q

identify mass number and atomic number

23Na
11

A

(top) mass number

(bottom) atomic number

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17
Q

isotopes

A

form of an atom with a differing number of neutrons

DIFFERS IN ATOMIC MASS

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18
Q

radioactive isotope

A

a form of a chemical element that is unstable

the nucleus decays spontaneously, giving off detectable particles

WHEN DECAY LEADS TO A CHANGE IN THE NUMBER OF PROTONS, AN ATOM BECOMES ANOTHER ATOM

14C
6 becomes nitrogen

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19
Q

uses for radioactive isotopes

A

following substances through the body

detecting cancer

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20
Q

energy

A

the capacity to cause change, especially to do work

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21
Q

to do work

A

to move matter against an opposing force

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22
Q

potential energy

A

energy that matter possesses as a result of its location or structure

the farther away from the nucleus, the greater potential energy an atom has

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23
Q

electron shells

A

average distance from the nucleus of an atom

chemical behavior of an atom is determined by the distribution of electrons in the atom’s shells

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24
Q

valence electrons

A

an electron in the outermost shell

determines the behavior of the atom

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25
Q

valence sh

A

outermost shell

atoms with the same # of electrons in their outer shells behave similarly

an atom with a full valence shell will not react readily and is said to be INERT

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26
Q

chemical bonds

A

an attraction between two atoms, resulting from a sharing of outermost electrons

the bonded atoms gain complete outer electron shells

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27
Q

covalent bond

A

a type of strong chemical bond in which two atoms share one of more pairs of valence electrons

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28
Q

molecule

A

two or more atoms held together by covalent bonds

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29
Q

single bond

A

a single covalent bond

the sharing of a pair of valence electrons by two atoms

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30
Q

double bond

A

a double covalent bond

the sharing of two pairs of valence electrons by two atoms

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31
Q

valence

A

the number of covelent bonds an atom can form

32
Q

electronegativity

A

the more electronegative an atom is, the more strongly it pulls the atoms in a covalent bond towards itself

33
Q

nonpolar covalent bond

A

electrons are shared EQUALLY between two atoms of similar elecrtonegativity

34
Q

polar covalent bond

A

electrons are shared UNEQUALLY between two atoms of differing electronegativity

35
Q

ion

A

an atom, or group of atoms that has gained or lost one or more electrons, thus acquiring a charge

36
Q

cation

A

a positive ion

37
Q

anion

A

a negative ion

38
Q

ionic bond

A

attraction between a cation and an anion

atoms take electrons from their bonding partners, resulting in both being charged

39
Q

ionic compound

A

a compound resulting from the formation of an ionic bond; also called a SALT

40
Q

hydrogen bond

A

slightly positive hydrogen atom from one molecule is attracted to a slightly negative atom

can be within the same molecule or another molecule entirely

41
Q

van der Waals interactions

A

resulting from unequal distribution of electrons

due to local partial charges

42
Q

reactants

A

a starting material in a chemical reaction

to the left in a chemical equation

43
Q

products

A

a material resulting from a chemical reaction

to the right in a chemical equation

44
Q

chemical equilibrium

A

the forward reaction is the same as the reverse reaction

45
Q

polar molecule

A

a molecule with an uneven distribution of charges in different regions of the molecule

46
Q

cohesion

A

the linking together of like molecules, often by hydrogen bonds

47
Q

adhesion

A

the clinging of one substance to another, such as water to plant cell walls by the means of hydrogen bonds

48
Q

surface tension

A

a measure of how difficult it is to break the surface of a liquid

49
Q

kinetic energy

A

the energy of motion

50
Q

thermal energy

A

energy due to the random motion of atoms or molecules

51
Q

temperature

A

a measure, in degrees of the average kinetic (thermal) energy of the atoms and molecules within a body of matter

52
Q

heat

A

thermal energy transfer from one body of matter to another

53
Q

calorie (cal)

A

amount of heat it takes to raise the temperature of 1g of water by 1 C

54
Q

kilocalorie (kcal)

A

1 kg of water by 1 C (1,000 cal)

55
Q

specific heat

A

the amount of heat that must be absorbed or lost for 1 g of a substance to change its temperature by 1 C

how well a substance resists change in temperature

56
Q

heat of vaporization

A

the quantity of heat a liquid must absorb for 1g of it to transform into a gas

57
Q

evaporative cooling

A

surface of an object becomes cooler during evaporation

a result of the atoms with the greatest amount of kinetic energy changing into a gas

58
Q

solution

A

a liquid that is a homogeneous mixture of two or more substances

59
Q

solvent

A

the dissolving agent of a solution

water is the most versatile solvent known

60
Q

solute

A

a substance that is dissolved in a solution

61
Q

aqueous solution

A

a solution in which water is the solvent

62
Q

hydration shell

A

the sphere of water molecules around a dissolved ion

63
Q

hydrophilic

A

having an affinity for water

64
Q

hyrdophobic

A

having no affinity for water

tending to coalesce to exclude water

65
Q

molecular mass

A

sum of all atoms in a molecule

66
Q

mole (mol)

A

the number of grams of a substance that equals its molecular weight

6.02 x 10^23

67
Q

molarity

A

number of moles of solute per liter of solution

68
Q

hydrogen ion

A

a single proton with a charge of 1+

69
Q

acid

A

a substance that increases the hydrogen ion concentration of a solution

70
Q

hydroxide ion

A

a water molecule that has lost a proton

OH-

71
Q

hyrdronium ion

A

a water molecule that has an extra proton bound to it

H3O+, commonly represented as H+

72
Q

base

A

a substance that reduces the hydrogen ion concentration of a solution

73
Q

pH

A

a measure of hydrogen ion concentration

ranging in value from 0 to 14

74
Q

internal pH

A

human blood 7.4

cells cannot function if not at 7

75
Q

buffer

A

a substance that minimalizes changes in the concentrations of H+ and OH- in a solution

it accepts extra hydrogen ions while donating hydrogen ions if they have been depleted

AP Biology (3 decks)

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