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AP Biology > Chapter 2 & 3 - The Chemical Context of Life & Water and Life > Flashcards

Chapter 2 & 3 - The Chemical Context of Life & Water and Life Flashcards

1
Q

anything that takes up space and has mass

A

Matter

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2
Q

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

A

element

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3
Q

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

A

compound

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4
Q

elements that an organism needs to live a healthy life and reproduce

A

essential elements

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5
Q

required by an organism in only minute quantities

A

trace elements

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6
Q

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

A

atom

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7
Q

number of protons, which is unique to each element

A

atomic number

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8
Q

total number of protons and neutrons in the nucleus of an atom

A

mass number

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9
Q

the total mass of an atom

A

atomic mass

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10
Q

different atomic forms of the same element

A

isotopes

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11
Q

the nucleus decays spontaneously, giving off particles and energy

A

radioactive isotope

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12
Q

fixed rate at which a parent isotope decays into its daughter isotope (the time it takes for 50% of the parent isotope to decay)

A

half-life

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13
Q

process where scientists measure the ratio of different isotopes and calculate how many half-lives have passed since an organism was fossilized or a rock was formed

A

radiometric dating

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14
Q

the capacity to cause change, by doing work

A

energy

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15
Q

the energy that matter possesses because of its location or structure

A

potential energy

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16
Q

outer electrons in an atom

A

valence electrons

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17
Q

the outermost electron shell

A

valence shells

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18
Q

the 3D space where an electron is found 90% of the time

A

orbital

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19
Q

interactions usually result in atoms staying close together, held by attractions

A

chemical bonds

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20
Q

sharing of a pair of valence electrons by two atoms

A

covalent bonds

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21
Q

two or more atoms held together by covalent bonds

A

molecule

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22
Q

a pair of shared electrons

A

single bond

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23
Q

bonding capacity of an atom (equals number of electrons required to complete the atoms’s outermost shell

A

valence

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24
Q

the attraction of a particular atom for the electrons of a covalent bond

A

electronegativity

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25
Q

bond where electrons are shared equally in a covalent bond because they have the same electronegativity

A

nonpolar covalent bond

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26
Q

bond where an atom is bonded to a more electronegative atom, the electrons are not shared equally

A

polar covalent bond

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27
Q

oppositely charged atoms (or molecules)

A

ions

28
Q

positively charged ion

A

cation

29
Q

negatively charged ion

A

anion

30
Q

bond where cations and anions attract each other

A

ionic bond

31
Q

compounds formed by ionic bonds

A

ionic compounds or salts

32
Q

noncovalent attraction between a hydrogen and an electronegative atom

A

hydrogen bond

33
Q

individually weak and occur only when atoms and molecules are very close together

A

van der Waals interactions

34
Q

the making and breaking of chemical bonds, leading to changes in the composition of matter

A

chemical reactions

35
Q

starting materials in a chemical reaction

A

reactants

36
Q

resulting materials in a chemical reaction

A

products

37
Q

the point at which the reactions offset one another exactly

A

chemical equilibrium

38
Q

molecule where its overall charge is unevenly distributed

A

polar molecule

39
Q

hydrogen bonds hold the substance together

A

cohesion

40
Q

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

A

surface tension

41
Q

clinging of one substance to another

A

adhesion

42
Q

energy of motion

A

kinetic energy

43
Q

kinetic energy associated with the random movement of atoms or molecules (TOTAL kinetic energy)

A

thermal energy

44
Q

represents the AVERAGE kinetic energy of the molecules in a body of matter, regardless of volume

A

temperature

45
Q

thermal energy in transfer from one body of matter to another

A

heat

46
Q

amount of heat it takes to raise the temp of 1g of water by 1 degree Celsisus

A

calorie (cal)

47
Q

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

A

specific heat

48
Q

quantity of heat a liquid must absorb for 1g of it to be converted form liquid to gaseous state

A

heat of vaporization

49
Q

as a liquid evaporates, the surface of the liquid that remains behind cools down

A

evaporative cooling

50
Q

a liquid that is completely homogenous mixture of tow or more substances

A

solution

51
Q

dissolving agent of a solution

A

solvent

52
Q

substance that is dissolved

A

solute

53
Q

solution in which the solute is dissolved in water

A

aqueous solution

54
Q

sphere of water molecules around each dissolved ion

A

hydration shell

55
Q

any substance that has an affinity for water (WATER LOVING)

A

hydrophilic

56
Q

substances that are nonionic and nonpolar that seem to repel water

A

hydrophobic

57
Q

sum of the masses of all the atoms in a molecule

A

molecular mass

58
Q

represents an exact number of objects (6.02 x 10 ^23)

A

mole (mol)

59
Q

the number of moles of solute per liter of solution

A

molarity

60
Q

a single proton with a charge of 1+

A

hydrogen ion (H+)

61
Q

when a water molecule loses a proton and now has a charge of 1 -

A

hydroxide ion (OH–)

62
Q

the proton binds to the other water molecule, which now has 3 hydrogens

A

hydronium ion (H3O-)

63
Q

substance that increases the hydrogen ion concentration of a solution

A

acid

64
Q

a substance that reduces the hydrogen ion concentration of a solution

A

base

65
Q

The _____ of a solution is defined as the negative logarithm (base 10) of the H+ ion concentration

A

pH

66
Q

substance that minimizes changes in the concentrations of H+ and OH– in a solution

A

buffer

67
Q

when CO2 dissolves in seawater, it reacts with water to form carbonic acid which lowers the ocean pH

A

ocean acidification

AP Biology (2 decks)

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