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AP Chemistry > chapter 1: introduction to chemistry > Flashcards

chapter 1: introduction to chemistry Flashcards

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1
Q

chemistry: study of matter and its interactions with

A

other matter and with energy

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2
Q

foundation of chemistry is

A

experimentation

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3
Q

chemistry is an experimental science in which we derive knowledge from

A

carefully planned and performed experiments

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4
Q

to formulate ideas for experiments, scientists draw on

A

experience, using experimental data and theory

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5
Q

hypothesis is a possible

A

explanation for an event

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6
Q

law: a statement that can summarize

A

a large number of observations

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7
Q

theory: an explanation of

A

the laws of nature

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8
Q

theories are subject to change when

A

new data becomes available

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9
Q

matter: anything with

A

mass and volume

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10
Q

mass: amount of

A

matter in an object

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11
Q

weight: force of …. between a particular object and ….

A

attraction; another object

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12
Q

weight is also the measure of the

A

gravitational pull on an object

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13
Q

balance to measure

A

mass

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14
Q

scale to measure

A

weight

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15
Q

property: observations or

A

measurements regarding matter

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16
Q

physical properties: properties that can be measured without

A

changing the composition of the sample

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17
Q

examples of physical properties:

A

mass, volume, color, phase

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18
Q

chemical properties: describe

A

reactivity of a material

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19
Q

examples of chemical properties:

A

explosiveness, flammability, lack of reactivity

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20
Q

physical change: does not change the

A

composition/ identity of a substance

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21
Q

examples of physical change

A

freezing, melting, boiling

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22
Q

chemical change: involves the transformation of matter into

A

different substances

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23
Q

examples of chemical change

A

rusting, burning

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24
Q

extensive properties: depend on the

A

size of the sample

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25
Q

extensive properties measure how much … is in a particular sample

A

matter

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26
Q

examples of extensive properties:

A

mass, volume

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27
Q

intensive properties: not dependent on the

A

size of the sample

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28
Q

intensive properties depend on

A

what the sample is

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29
Q

examples of intensive properties:

A

colors, melting points, densities

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30
Q

intensive properties can be used to

A

identify a substance

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31
Q

substance: chemically the

A

same throughout

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32
Q

element: cannot be broken down into

A

simpler, stable substances

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33
Q

compound: can be

A

broken down into simpler, stable substance

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34
Q

matter can be classified by:

A

chemical composition, physical state, color, etc.

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35
Q

compounds are uniform in

A

composition and properties throughout

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36
Q

mixture: matter that can be separated into two or more substances by differences in the

A

physical properties of the components

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37
Q

homogenous mixture:

A

uniform in composition

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38
Q

examples of homogenous mixtures:

A

sugar-water solution, air

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39
Q

heterogenous mixtures:

A

not uniform in composition

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40
Q

examples of heterogenous mixtures:

A

mixture of iron and sand, vegetable soup, salt and pepper

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41
Q

samples of the same mixture can have different …, unlike …

A

compositions; substances

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42
Q

alloy: a solid solution that consists of a

A

metal and another substance, usually another metal

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43
Q

substance: matter that cannot be separated into

A

component parts by a physical process

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44
Q

compounds: substances that can be decomposed into simpler substances or into their elements by

A

chemical processes

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45
Q

compounds always contain the same elements in the

A

same proportions

46
Q

all samples of a compound have the same

A

intensive properties

47
Q

symbols for the elements are abbreviations for their

A

names

48
Q

numerical measurements have 4 aspects:

A

object, value; units; reliability

49
Q

reliability:

A

accuracy and precision

50
Q

accuracy: expresses how close a measurement is to the

A

correct or accepted value

51
Q

precision: refers to the closeness of a set of measurements to

A

each other, but not necessarily the accepted value

52
Q

accurate: number has a small

A

error

53
Q

precise: number has small

A

uncertainty

54
Q

significant figures: used to display the

A

uncertainty of results

55
Q

significant figures: all digits known with certainty, plus one more digit that is

A

not certain

56
Q

uncertainty of final digit is

A

± 1

57
Q

nonzero digits are

A

significant

58
Q

zeros between nonzero digits are

A

significant

59
Q

with no decimal point to the right of a zero, the trailing zero may or may not be

A

significant (clarified by scientific notation)

60
Q

if there is a decimal point, leading zeros are …, but zeros at the end of the number are …

A

insignificant; significant

61
Q

number of sig figs in a calculated value results from the… of the …and the …that were used to attain the final value

A

uncertainties; measurements; operations

62
Q

addition/subtraction sig figs: answer has the same number of decimal places as the component with the

A

least number of decimal places

63
Q

multiplication/division sig figs: answer has the same number of sig figs as the component with the

A

least number of significant digits

64
Q

(rounding rules) if digit after the last sig fig is

A

round down

65
Q

(rounding rules) if digit after the last sig fig = 5,

A

round to even

66
Q

(rounding rules) if digit after the last sig fig is > 5

A

round up

67
Q

density: ratio of

A

mass to volume

68
Q

three kinds of numbers never limit sig fits:

A

counted numbers/tallies, defined numbers, power of ten

69
Q

quantities: describe… and illustrate …

A

properties; precise information

70
Q

units: standards by which

A

measurements are compared

71
Q

SI units: 7 base units which define

A

length, mass, time, temperature, amount of substance, electrical current, luminous intensity

72
Q

length:

A

meter

73
Q

mass:

A

kilogram

74
Q

time:

A

second

75
Q

temperature

A

kelvin

76
Q

amount of substance:

A

mole

77
Q

electrical current:

A

ampere

78
Q

luminous intensity:

A

candela

79
Q

base units can be

A

reproduced in labs (exception: kilogram)

80
Q

derived units: physical quantities that can be expressed as a

A

combination of base units

81
Q

when multiplying by conversion factors, the … are what change, along with the ….

A

units; numeric value

82
Q

(prefixes) yotta- Y

A

10^24

83
Q

(prefixes) zeta- Z

A

10^21

84
Q

(prefixes) exa- E

A

10^18

85
Q

(prefixes) peta- P

A

10^15

86
Q

(prefixes) tera-T

A

10^12

87
Q

(prefixes) giga-G

A

10^9

88
Q

(prefixes) mega- M

A

10^6

89
Q

(prefixes) kilo- k

A

10^3

90
Q

(prefixes) hecto- h

A

10^2

91
Q

(prefixes) deka- da

A

10^1

92
Q

(prefixes) deci- d

A

10^-1

93
Q

(prefixes) centi- c

A

10^-2

94
Q

(prefixes) milli- m

A

10^-33

95
Q

(prefixes) micro- µ

A

10^-6

96
Q

(prefixes) nano- n

A

10^-9

97
Q

(prefixes) pico- p

A

10^-12

98
Q

(prefixes) femto- f

A

10^-15

99
Q

(prefixes) atto- a

A

10^-18

100
Q

(prefixes) zepto- z

A

10^-21

101
Q

(prefixes) yocto- y

A

10^-24

102
Q

unit conversion factor: fraction in which the numerator is a quantity that is equal or equivalent to the quantity in

A

the denominator but expressed in different units

103
Q

to know what conversion factor should be used, determine which units should be … and which units you are attempting to …

A

canceled; attain

104
Q

standard unit for volume is

A

m^3

105
Q

density is a … property that can help

A

physical; identify substances

106
Q

density can’t be used to convert between

A

different substances

107
Q

standard unit for density:

A

kg/ m^3

108
Q

none of the relationships between the English and SI units is …; effects …

A

exact; sig figs

109
Q

conversion factors between Celsius and Fahrenheit

A 
TF = TC  x (1.8℉/1.0℃) + 32 ℉
TC  = (TF - 32 ℉) x (1.0℃/1.8℉)
110
Q

absolute zero:

A

-273.15 degrees C

111
Q

conversion between Celsius and kelvin:

A

Tk = Tc + 273.15

AP Chemistry (24 decks)

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