Chapter 2: Chemistry and Measurements Flashcards
(119 cards)
1
Q
It is the standard system of
measurement used in
chemistry
A
Metric System
2
Q
Scientist use the _ of measurement and have
adopted a modification of the metric system called the ___ as a worldwide standard
A
Metric system; International System of Units
3
Q
is an official system of
measurement used throughout the world for units of length,
volume, mass, temperature, and time.
A
The International System of Units (SI)
4
Q
Length in metric
A
Meter (m)
5
Q
Volume in metric
A
Liter (L)
6
Q
mass in metric
A
gram (g)
7
Q
Temperature in metric
A
degrees celsius (C)
8
Q
Time in metric
A
second (s)
9
Q
SI unit in length
A
Meter (m)
10
Q
SI unit in volume
A
cubic meter (m^3)
11
Q
SI unit in mass
A
kilogram (kg)
12
Q
SI unit in temperature
A
Kelvin (K)
13
Q
SI unit in time
A
second (s)
14
Q
__ in the metric and SI systems is based on the meter,
which is slightly longer than a yard.
A
Lenght
15
Q
1 m = ___cm
A
100cm
16
Q
1 m = _in.
A
39.4 in.
17
Q
1m = _yd
A
1.09 yd
18
Q
2.54 cm = _in.
A
1 in
19
Q
It is the space
occupied by a substance
A
Volume
20
Q
The SI unit of volume _
A
m3
21
Q
In the metric
system, volume is based on
the _which is slightly
larger than a quart.
A
Liter
22
Q
1 L = _ml
A
1000 mL
23
Q
1 L = _qt
A
1.06 qt
24
Q
946 mL = _ qt
A
1 qt
25
_ of an object is a
measure of the quantity of
material it contains.
Mass
26
1 kg = _g
1000 g
27
1 kg = _lbs
2.20 lbs
28
454 g = _lb
1 lb
29
_ tells us how hot or cold
something is
Temperature
30
Water freezes at
32 °F, or 0 °C,273 K
31
Conversion of Kelvinto Celsius
C = K - 273.15
32
Conversion of Celsius to Kelvin
Kelvin = Celsius + 273.15
33
Time is measured in units such as
the following:
* years (yr)
* days
* hours (h)
* minutes (min)
* seconds (s)
34
The SI and metric unit of time is _
second (s)
35
The last digit in your measurement is an
estimate, obtained by visually __ between the marked lines.
dividing the space
36
___ are the numbers obtained when you
measure a quantity such as your height, weight, temperature
Measured numbers
37
Significant figures are the following:
1. not a zero
2. a zero between nonzero digits
3. a zero at the end of a decimal (23.00 -4 sig fig)
4. in the coefficient of a number written in scientific notation
38
A zero is not significant if it is :
1. at the beginning of a decimal (0.0004 - 1 sig fig)
2. used as a placeholder in a large number without a decimal point ( 850 000 000- 2 sig fig)
39
Zeros at the end of large standard numbers without a
decimal point are ___
not significant.
40
Zeros at the beginning of a decimal number are used as placeholders and are ___
not significant
41
0.000 4 in scientific notation is
4 × 10^−4
42
0.000 0046 in scientific notation is
4.6 × 10^−6
43
0.002 650 has how many sig fig?
4 sig fig
44
The zero in the last decimal place is ___
significant
45
The zeros between nonzero digits or at the end of decimal numbers are ___
significant
46
43.026 has how many sig fig?
5 sig fig
47
1 044 000 has how many sig fig?
4 sig fig
48
The zeros between nonzero digits are
significant
49
The zeros at end of a number with no decimal point
are ___
not significant (1 044 000 - 4 sig fig)
50
___ are not measured and do not have a limited number of
significant figures
Exact numbers
51
___ are numbers obtained by counting
Exact numbers
52
_ definitions in the same measuring system (1 qt = 4 cups)
Exact numbers
53
Example of some exact number in Metric System
1L= 1000mL
1m =100cm
1kg = 1000g
54
Example of some exact number in U.S. System
1ft = 12 in
1 qt = 4 cups
1lb = 16 oz
55
The diameter of a circle is 7.902 cm is it exacted or measured number?
measured number
56
60 min = 1 h , an exact or measured number?
exact number
57
In following the decimal point for the final answer, follow the given that has the ___
lowest decimal point
58
In multiplication or division, the final answer is written so that it
has the same number of significant figures (SFs) as the measurement with the ____
fewest significant figures
59
3 sig fig x 2 sig fig = __
2 sig fig
60
When the calculator display contains fewer SFs than needed, ____ significant zeros to obtain the correct number of significant figures
add one or more (eg, 6.0 + 2.00 = 3 --- 3.0 = 2 sig fig)
61
In addition or subtraction, the final answer is written so that it has the same number of decimal places as the measurement with the __
fewest decimal places.
62
A special feature of the SI as well as the metric system is
that a ____ can be placed in front of any unit to increase or decrease its size by some factor of ten
prefix
63
milli and micro are used to make ____
the smaller units
64
peta = __ in scientific notation
10^15
65
tera = __ in scientific notation
10^12
66
giga = __ in scientific notation
10^9
67
mega = __ in scientific notation
10^6
68
kilo = __ in scientific notation
10^3
69
doci = __ in scientific notation
10^-1
70
centi = __ in scientific notation
10^-2
71
milli = __ in scientific notation
10^-3
72
micro = __ in scientific notation
10^-6
73
nano = __ in scientific notation
10^-9
74
pico = __ in scientific notation
10^-12
75
fento = __ in scientific notation
10^-15
76
1000 m = 1 ___ m
1km
77
1 × 10−3 g = 1 ___ g
1mg
78
0.01 m = 1 ___ m
1 cm
79
1 m = 100 cm = ___ in scientific notation
1 × 10^2 cm
80
1 m = 1000 mm = ___ in scientific notation
1 × 10^3 mm
81
1 cm = 10 mm = ___ mm in scientific notation
1 × 10^1 mm
82
1 L = 10 dL = ___ dLin scientific notation
1 × 10^1 dL
83
1 L = 1000 mL = ___ in scientific notation
1 × 10^3 mL
84
1 L = 1000mL = ___ mL in scientific notation
1 × 10^3 mL
85
___ is the
volume of a cube whose dimensions are 1 cm on each side
cubic centimeter (abbreviated as cm3 or cc)
86
1 cm3 is also equal to ____
1 cc and 1 mL
87
1000 cm3 is also equal to ____
= 1000 ml and 1 L
88
It uses two different units to describe the same measured
amount.
Equalities
89
___ are written for relationships between units of the metric system, U.S. units, or between metric and U.S. units.
Equalities
90
____ a definition are exact and are not used to determine significant figures
Equalities
91
The equality 1 in. = 2.54 cm has been defined as an exact relationship
Therefore, 2.54 is an exact number.
92
2.2.lb/ 1kg can also be written into
1kg/2.20kg
93
A dosage is typically
measured in ____
1. milligrams per kilogram
(mg/kg) of body mass.
2. micrograms per kilogram
(mcg/kg) of body mass.
94
What is the formula for solving the density?
Density= mass of a substance / volume of a substance
95
Density of solids, liquids is equal to ____
g/cm^3 or g/ml
96
Density of gas is equal to ____
g/L
97
1 mL is also equal to ___
1 cm^3
98
____ is a relationship between the density of a substance and the density of water.
- is a unitless quantity
Specific gravity
99
_____ is calculated by dividing the density of a sample by the density of water, which is 1.00 g/mL at 4 °C
Specific gravity
100
What is the formula for the specific gravity?
Specific gravity = density of sample/ density of water
101
102
103
Use in smaller unit
milligram (mg)
microgram (ug or mcg)
104
Kilo =
10^3
105
____ exact and do not determine sig. fig.
Equalities
106
Freezing point temperature of water in F is ___
32 F
107
Freezing point temperature of water in K is ___
273 K or 273.25 K
108
Freezing point temperature of water in Celsius is ___
0 degrees Celsius
109
Normal temperature of water in Celsius is ___
37 degrees Celsius
110
Normal temperature of water in Fahrenheit is ___
98.6 F
111
Normal temperature of water in Kelvin is ___
310 K or 310.15 K
112
Boiling point temperature of water in F is ___
212 F
113
Boiling point temperature of water in Celsius is ___
100 degrees Celsius
114
Boiling point temperature of water in K is ___
373K or 373.15K
115
_cm^3 = _ ml = _ cc
1, 1, 1 (all have the same value)
116
the conversion factor of water in heat of fusion (J/g or cal/g)
334J/ 1g of H2O or 80 cal/1 g of H2O
117
the conversion factor of water in heat vaporation (J/g or cal/g)
2260J/ 1g of H2O or
540 cal/1 g of H2O
118
heat of fusion is changing of state between?
solid to liquid and vice versa
119
heat vaporization is changing of state between?
gas to liquid and vice versa
