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TEST ONE Flashcards

(71 cards)

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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
mass
Kg
26
tera
ten to the power of twelve
27
giga
ten to the power of nine
28
mega
ten to the power of six
29
kilo
ten to the power of three
30
hecto
ten to the power of two
31
deka
ten to the power of one
32
deci
ten to the power of negative one
33
centi
ten to the power of negative two
34
milli
ten to the power of negative three
35
micro
ten to the power of negative six
36
nano
ten to the power of negative nine
37
pico
ten to the power of negative twelve
38
one mole
22. 4 L | 6. 02x10^23
39
decimeter cubed
1 liter
40
gravity
varies with altitude | originates from the center of the earth
41
random or indeterminate error
equal probability of a measurement being high or low
42
systematic or determinate error
occurs in the same direction each time | error built into device
43
Circa
400-5 B.C. Greek philosopher Democritus proposes the idea of matter being made up of small indivisible particles (atomos)
44
Late 18th century
Lavoisier proposes the law of conservation of mass and Proust proposes the Law of Constant Composition
45
Early 19th Century
John Dalton uses the previously unconnected ideas above to formulate his Atomic Theory
46
1803
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
Two modifications to Daltons theory
subatomic particles were discovered | isotopes were discovered
48
Crookes
Cathode Ray Tube experiment | electron
49
JJ Thompson
Cathode Ray Deflection Mass/Charge Ratio electron
50
Millikan
Oil drop experiment | charge on the electron
51
Rutherford, Marsden And Geiger
Gold Foil Experiment | Nucleus Present in atom
52
Chadwick
discovered neutron
53
Bohr's model (20th century)
nucleus of protons and neutrons is orbited by electrons
54
Law of Conservation of Matter
matter can neither be created nor destroyed in a chemical reaction
55
Law of Definite proportion
a given compound always contains exactly the same proportion of elements by mass
56
all matter composed of only one type of atom
is an element 92 naturally all other manmade
57
proton
positive charge responsible for the identity of the element defines atomic number 1 amu
58
neutron
no charge same size and mass as a proton responsible for isotopes alters atomic mass number
59
electron
negative charge 1/1836 the mass of a proton or neutron responsible for bonding easily added or removed
60
atomic number
Z
61
mass number
A
62
isotopes
atoms having the same atomic number but a dfferent number of neutrons
63
average atomic mass
% of each isotope(atomic mass of each isotope)/100
64
isoelectric
have the same number of electrons
65
anhydrous
without water
66
molecules
a definite number of atoms are joined together by chemical bonds
67
ions
formed when atoms loose or gain electrons, causing charges
68
anions
negative
69
cations
positive
70
monatomic
ion made up of only one type of atom
71
polyatomic
ion made up of more than one type of atom

AP CHEMISTRY (2 decks)

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