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AP CHEMISTRY > TEST ONE > Flashcards

TEST ONE Flashcards

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1
Q

EFU=

A

MM of Molecular formula/ MM of Empirical Formula

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2
Q

Covalent

A

2 non-metals

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3
Q

Ionic

A

non-metal & metal

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4
Q

mon

A

one

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5
Q

di

A

two

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6
Q

tri

A

three

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7
Q

tetra

A

four

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8
Q

penta

A

five

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9
Q

hexa

A

six

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10
Q

hepta

A

seven

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11
Q

octa

A

eight

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12
Q

nona

A

nine

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13
Q

deca

A

ten

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14
Q

Coulombic Attraction

A

the attraction between oppositely charged particles

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15
Q

theory

A

hypotheses are assembled in an attempt at explaining “why” the “what” happened

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16
Q

Model

A

explain natural phenomenon- when new evidence is found, the model changes

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17
Q

Robert Boyl

A

defined elements as anything that cannot be broken down into simpler substances

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18
Q

Scientific Laws

A

a summary of observed (measurable behavior)

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19
Q

Law of Conservation of Mass

A

Mass reactants=mass products

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20
Q

law of conservation of energy

A

energy CANNOT be created NOR destroyed; can only change forms

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21
Q

Scientists are subjected to

A 
data misinterpretations
emotional attatchments to theories
loss of objectivity
politics
ego
profit motives
fads
wars
religious beliefs
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22
Q

Galileo

A

forced to recant his astronomical observations in the face of strong religious resistance

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23
Q

Lavoisier

A

“father of modern chemistry”

beheaded due to political affiliations

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24
Q

SI system

A

1960 international agreement of measurement

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25
Q

mass

A

Kg

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26
Q

tera

A

ten to the power of twelve

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27
Q

giga

A

ten to the power of nine

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28
Q

mega

A

ten to the power of six

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29
Q

kilo

A

ten to the power of three

30
Q

hecto

A

ten to the power of two

31
Q

deka

A

ten to the power of one

32
Q

deci

A

ten to the power of negative one

33
Q

centi

A

ten to the power of negative two

34
Q

milli

A

ten to the power of negative three

35
Q

micro

A

ten to the power of negative six

36
Q

nano

A

ten to the power of negative nine

37
Q

pico

A

ten to the power of negative twelve

38
Q

one mole

A
  1. 4 L

6. 02x10^23

39
Q

decimeter cubed

A

1 liter

40
Q

gravity

A

varies with altitude

originates from the center of the earth

41
Q

random or indeterminate error

A

equal probability of a measurement being high or low

42
Q

systematic or determinate error

A

occurs in the same direction each time

error built into device

43
Q

Circa

A

400-5 B.C. Greek philosopher Democritus proposes the idea of matter being made up of small indivisible particles (atomos)

44
Q

Late 18th century

A

Lavoisier proposes the law of conservation of mass and Proust proposes the Law of Constant Composition

45
Q

Early 19th Century

A

John Dalton uses the previously unconnected ideas above to formulate his Atomic Theory

46
Q

1803

A

Daltons theory:

  1. all matter is made of atoms. These indivisible and indestructible objects are the ultimate chemical properties
  2. All the atoms of a given element are identical, but atoms of different elements are different
  3. A chemical reaction involves only the combination, separation, or rearrangement of atoms; atoms are neither created nor destroyed in the course of ordinary chemical reactions
  4. Compounds are formed by the combination of different atoms in the ratio of small whole numbers
47
Q

Two modifications to Daltons theory

A

subatomic particles were discovered

isotopes were discovered

48
Q

Crookes

A

Cathode Ray Tube experiment

electron

49
Q

JJ Thompson

A

Cathode Ray
Deflection
Mass/Charge Ratio
electron

50
Q

Millikan

A

Oil drop experiment

charge on the electron

51
Q

Rutherford, Marsden And Geiger

A

Gold Foil Experiment

Nucleus Present in atom

52
Q

Chadwick

A

discovered neutron

53
Q

Bohr’s model (20th century)

A

nucleus of protons and neutrons is orbited by electrons

54
Q

Law of Conservation of Matter

A

matter can neither be created nor destroyed in a chemical reaction

55
Q

Law of Definite proportion

A

a given compound always contains exactly the same proportion of elements by mass

56
Q

all matter composed of only one type of atom

A

is an element
92 naturally
all other manmade

57
Q

proton

A

positive charge
responsible for the identity of the element
defines atomic number
1 amu

58
Q

neutron

A

no charge
same size and mass as a proton
responsible for isotopes
alters atomic mass number

59
Q

electron

A

negative charge
1/1836 the mass of a proton or neutron
responsible for bonding
easily added or removed

60
Q

atomic number

A

Z

61
Q

mass number

A

A

62
Q

isotopes

A

atoms having the same atomic number but a dfferent number of neutrons

63
Q

average atomic mass

A

% of each isotope(atomic mass of each isotope)/100

64
Q

isoelectric

A

have the same number of electrons

65
Q

anhydrous

A

without water

66
Q

molecules

A

a definite number of atoms are joined together by chemical bonds

67
Q

ions

A

formed when atoms loose or gain electrons, causing charges

68
Q

anions

A

negative

69
Q

cations

A

positive

70
Q

monatomic

A

ion made up of only one type of atom

71
Q

polyatomic

A

ion made up of more than one type of atom

AP CHEMISTRY (2 decks)

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