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Matter and Measurements
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Matter and Energy - Vocabulary
• Chemistry• Matter• Energy• Natural Law-(scientific law)
– Observation, Hypothesis, Theory, Law
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States of Matter
• Solids
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States of Matter
• Solids• Liquids
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States of Matter
• Solids• Liquids• Gases
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States of Matter
• Change States– heating– cooling
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States of Matter• Illustration of changes in state
– requires energy
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Substances, Compounds, Elements and Mixtures
• Substance– matter that all samples have identical composition
and properties• Elements
– Pure substances that cannot be decomposed into simpler substances via chemical reactions
– Special elemental forms of atoms (diatomic)Elemental symbols
– found on periodic chart
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Substances, Compounds, Elements and Mixtures
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Substances, Compounds, Elements and Mixtures
• Compounds– Pure substances composed of two or more
elements in a definite ratio by mass– can be decomposed into the constituent elements
REVIEW– Element cannot be broken down– Compound can be broken down into its elements!
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Substances, Compounds, Elements and Mixtures
• Mixtures– composed of two or more substances– homogeneous mixtures
• Uniform throughout• Example: solutions
– heterogeneous mixtures• Not uniform • Example: rocks
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Classify the following substances as an element, compound or a mixture
(homogeneous or heterogeneous). Which are pure substances?
• Lightly scrambled egg• Water• Lava lamp• Seawater• Chicken noodle soup• Root beer• Sucrose (C12H22O11)
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Separating Mixtures• Distillation
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Separating Mixtures• Chromatography
paper
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Chemical and Physical Properties• Extensive Properties - depend on quantity
of material Ex. mass
• Intensive Properties - do not depend on quantity of material
Ex. boiling point
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Chemical and Physical Properties• Chemical Properties - chemical changes
– Observed during change of material to new material• Iron rusting
• Physical Properties - physical changes– No change to the identity of the substance
• changes of state• density • color • solubility
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Physical Properties• Density
– mass / volume intensive property– Mass and volume extensive
properties• Solubility
– Amount of substance dissolved in the solvent at a given temperature• Saturated solution• Unsaturated solution• Supersaturated solution
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Identify the following as either a chemical or physical change.
• Combination of sodium and chlorine to give sodium chloride.
• Liquefaction of gaseous nitrogen.• Separation of carbon monoxide into
carbon and oxygen.• Freezing of water.
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Measurements in Chemistry
• length meter m• volume liter l• mass gram g• time second s• current ampere A• temperature Kelvin K• amt. substance mole mol
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Measurements in Chemistry• mega M 106
• kilo k 103
• deka da 10• deci d 10-1
• centi c 10-2
• milli m 10-3
• micro m 10-6
• nano n 10-9
• pico p 10-12
• femto f 10-15
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Units of Measurement• Mass
– measure of the quantity of matter in a body• Weight
– measure of the gravitational attraction for a body
• Length 1 m = 39.37 inches2.54 cm = 1 inch
• Volume1 liter = 1.06 qt 1 qt = 0.946 liter
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The Use of Numbers
• Exact numbers 1 dozen = 12 things• Accuracy
– how closely measured values agree with the correct value
• Precision– how closely individual measurements
agree with each other
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The Use of Numbers
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The Use of Numbers
• Exact numbers 1 dozen = 12 things– Counted numbers ex. 3 beakers
• Significant figures– digits believed to be correct by the person
making the measurement• Scientific notation
– Way of signifying the significant digits in a number
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Significant Figures - rules
• leading zeroes - never significant0.000357 has three sig fig
• trailing zeroes - may be significantmust specify (after decimal – significant
before decimal - ambiguous)
1300 nails - counted or weighed?
Express 26800 in scientific notation with4 sig figs 3 sig figs 2 sig figs
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Significant Figures - rules• imbedded zeroes are always significant
3.0604 has five sig fig
How many significant figures are in the following numbers?
0.01240.1241.2401240
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Significant Figures - rules
multiply & divide rule - easyproduct has the smallest number of sig. fig.
of multipliers
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Significant Figures - rules
• multiply & divide rule - easyproduct has the smallest number of sig. fig.
of multipliers
310 x 5.22 tooff round
66.5217
31.2x 2424
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Significant Figures - rules
• multiply & divide rule - easyproduct has the smallest number of sig. fig.
of multipliers
310 x 5.22 tooff round
66.5217
31.2x 2424
3.9 tooff round89648.3
41.x 2783.2
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Practice
• 142 x 2 = • 4.180 x 2.0 = • 0.00482 / 0.080 = • 3.15x10-2 / 2.00x105 = • 24.8x106 / 6.200x10-2 =
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Practice
• 142 x 2 = 300• 4.180 x 2.0 = • 0.00482 / 0.080 = • 3.15x10-2 / 2.00x105 = • 24.8x106 / 6.200x10-2 =
32
Practice
• 142 x 2 = 300• 4.180 x 2.0 = 8.4• 0.00482 / 0.080 = • 3.15x10-2 / 2.00x105 = • 24.8x106 / 6.200x10-2 =
33
Practice
• 142 x 2 = 300• 4.180 x 2.0 = 8.4• 0.00482 / 0.080 = 0.060• 3.15x10-2 / 2.00x105 = • 24.8x106 / 6.200x10-2 =
34
Practice
• 142 x 2 = 300• 4.180 x 2.0 = 8.4• 0.00482 / 0.080 = 0.060• 3.15x10-2 / 2.00x105 = 1.58x10-7
• 24.8x106 / 6.200x10-2 =
35
Practice
• 142 x 2 = 300• 4.180 x 2.0 = 8.4• 0.00482 / 0.080 = 0.060• 3.15x10-2 / 2.00x105 = 1.58x10-7
• 24.8x106 / 6.200x10-2 = 4.00x108
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Significant Figures - rules
• add & subtract rule - subtleanswer contains smallest decimal place of
the addends
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Significant Figures - rules
• add & subtract rule - subtleanswer contains smallest decimal place of
the addends
6.95 tooff round9463.6
20.2423.13692.3
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Significant Figures - rules
• add & subtract rule - subtleanswer contains smallest decimal place of
the addends
6.95 tooff round9463.6
20.2423.13692.3
6.671 tooff round6707.6
312.27793.8
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Practice
• 416.2 – 10.18 =• 16.78 + 10. = • 422.501 – 420.4 = • 25.5 + 21.1 + 3.201 = • 42.00x10-4 + 1.8x10-6 =
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Practice
• 416.2 – 10.18 = 406.0• 16.78 + 10. = • 422.501 – 420.4 = • 25.5 + 21.1 + 3.201 = • 42.00x10-4 + 1.8x10-6 =
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Practice
• 416.2 – 10.18 = 406.0• 16.78 + 10. = 27• 422.501 – 420.4 = • 25.5 + 21.1 + 3.201 = • 42.00x10-4 + 1.8x10-6 =
42
Practice
• 416.2 – 10.18 = 406.0• 16.78 + 10. = 27• 422.501 – 420.4 = 2.1• 25.5 + 21.1 + 3.201 = • 42.00x10-4 + 1.8x10-6 =
43
Practice
• 416.2 – 10.18 = 406.0• 16.78 + 10. = 27• 422.501 – 420.4 = 2.1• 25.5 + 21.1 + 3.201 = 49.8• 42.00x10-4 + 1.8x10-6 =
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Practice
• 416.2 – 10.18 = 406.0• 16.78 + 10. = 27• 422.501 – 420.4 = 2.1• 25.5 + 21.1 + 3.201 = 49.8• 42.00x10-4 + 1.8x10-6 = 4.2 x 10-3
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More Practice
4.18 – 58.16 x (3.38 – 3.01) =
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More Practice
4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (0.37) =
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More Practice
4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (0.37) =4.18 – 21.5192 =
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More Practice
4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (0.37) =4.18 – 21.5192 = -17.3392Round off correctly
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More Practice
4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (0.37) =4.18 – 21.5192 = -17.3392Round off correctly to 2 sig. figs-17
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Unit Factor MethodDimensional Analysis
• simple but important way to always get right answer
• way to change from one unit to another• make unit factors from statements
1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft3 ft = 1 yd becomes 3ft/1yd or 1yd/3ft
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Unit Factor MethodDimensional Analysis
• simple but important way to always get right answer
• way to change from one unit to another• make unit factors from statements
1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft• Example: Express 12.32 yards in
millimeters.
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Unit Factor Method
.).........yd1ft3( yd 12.32
mm ?yd 12.32
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Unit Factor Method
mm 1011.27)cm1mm10( )
in1cm2.54( )
ft1in12( )
yd1ft3( yd 12.32
mm ?yd 12.32
3
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Unit Factor Method• Example: Express 323. milliliters in
gallons
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Unit Factor Method• Express 323. milliliters in gallons.
gal 0.0856gal 0.085595gal ?
)qt4
gal1( )L1
qt1.06( )mL1000
L1( mL 323gal ?
mL 323gal ?
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Unit Factor Method• Example: Express 5.50 metric tons in
pounds. 1 metric ton = 1 Megagram
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Unit Factor Method• Example: Express 5.50 metric tons in
pounds.
lbsxlbsglbgrams 4
6
1021.1537.121144541
tonmetric 11x10 tons5.50 lbs ?
tonsmetric 5.50 lbs ?
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Unit Factor Method• area is two dimensional• Example: Express 4.21 x 106 square
centimeters in square feet
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Unit Factor Method• area is two dimensional
express 4.21 x 106 square centimeters in square feet
2262 )cm 2.54
in 1(cm104.21ft ?
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Unit Factor Method• area is two dimensional
express 4.21 x 106 square centimeters in square feet
22262 )in12ft 1()
cm2.54in 1(cm104.21ft ?
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Unit Factor Method• area is two dimensional
express 4.21 x 106 square centimeters in square feet
232
22262
ft 4.53x10ft 4531.6063
)in12ft1()
cm2.54in1(cm104.21ft ?
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Unit Factor Method• volume is three dimensional• Example: Express 3.61 cubic feet in
cubic centimeters.
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Unit Factor Method• volume is three dimensional• Example: Express 3.61 cubic feet in
cubic centimeters.
353
3333
cm 101.02cm 102223.42
)in 1
cm 2.54()ft 1in 12(ft 3.61cm ?
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Percentage
• Percentage is the parts per hundred of a sample.
• Example: A 500. g sample of ore yields 27.9 g of sulfur. What is the percent of sulfur in the ore?
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Percentage• Percentage is the parts per hundred of
a sample.• Example: A 500. g sample of ore yields
27.9 g of sulfur. What is the percent of sulfur in the ore?
5.58%
100%x ore g 500S g 27.9
100% x ore of grams
sulfur of grams iron % ?
66
Derived Units - Density • density = mass/volume• What is density?• Example: Calculate the density of a
substance if 123. grams of it occupies 57.6 cubic centimeters.
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Derived Units - Density • density = mass/volume• What is density?• Example: Calculate the density of a
substance if 123. grams of it occupies 57.6 cubic centimeters.
Vm D
mL 6.57cm 57.6 mL 1 cm 1 33
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Derived Units - Density • density = mass/volume• What is density?• Example: Calculate the density of a
substance if 123. grams of it occupies 57.6 cubic centimeters.
g/mL 2.13 DmL 57.6
g 123. D
Vm D
mL 6.57cm 57.6 mL 1 cm 1 33
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Derived Units - Density • Example: Suppose you need 175. g of a
corrosive liquid for a reaction. What volume do you need? – liquid’s density = 1.02 g/mL
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Derived Units - Density • Example: Suppose you need 175. g of a
corrosive liquid for a reaction. What volume do you need? – liquid’s density = 1.02 g/mL
DmV
VmD
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Derived Units - Density • Example: Suppose you need 175. g of a
corrosive liquid for a reaction. What volume do you need? – liquid’s density = 1.02 g/mL
mL 172mL 171.57 1.02g 175V
DmV
VmD
mLg
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Heat & Temperature• heat and T are not the same thing
T is a measure of the intensity of heat in a body• 3 common T scales - all use water as a
reference
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Heat & TemperatureMP BP
• Fahrenheit 32oF 212oF• Celsius 0oC 100cC• Kelvin 273 K 373 K
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Relationships of the 3 T Scales
273KC
or 273 C K
o
o
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Relationships of the 3 T Scales
1.859
1018
100180
273K C
or273 C K
o
o
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Relationships of the 3 T Scales
1.832FC
or32C 1.8F
1.859
1018
100180
273KC
or273 C K
oo
oo
o
o
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Heat and Temperature• Example: Convert 111.oF to degrees
Celsius.
1.832111C
1.832FC
o
oo
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Heat and Temperature• Example: Convert 111.oF to degrees
Celsius.
9.438.1
791.8
32111C
1.832FC
o
oo
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Heat and Temperature• Example: Express 757. K in Celsius
degrees.
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Heat and Temperature• Example: Express 757. K in Celsius
degrees.
.484C
273..757C
273.KC
o
o
o
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The Measurement of Heat
• SI unit J (Joule)• calorie
1 calorie = 4.184 J• English unit = BTU
82
Synthesis Question• It has been estimated that 1.0 g of
seawater contains 4.0 pg of Au. The total mass of seawater in the oceans is 1.6x1012 Tg, If all of the gold in the oceans were extracted and spread evenly across the state of Georgia, which has a land area of 58,910 mile2, how tall, in feet, would the pile of Au be?Density of Au is 19.3 g/cm3. 1.0 Tg = 1012g.
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Au g106.4)OH of g
Au g104.0O)(H of g10(1.6
OH of g 101.6)Tg
g 10( Tg) 10(1.6
12
2
12
224
224
1212
84
331533
3113
12
12
2
12
224
224
1212
mile 1cm 104.16 mile 1cm 160,934
cm 160,934in 1
cm 2.54ft 1in 12
mile 1ft 5280mile 1
Aucm103.3Au g 19.3
1cmAu g106.4
Au g106.4)OH of g
Au g104.0O)(H of g10(1.6
OH of g 101.6)Tg
g 10( Tg) 10(1.6
85
ft 107.13mile 1
ft 5280mile)10(1.35mile 58,910
mile107.96
mile107.96cm104.16
mile 1Au) cm 10(3.3
692
35
35315
3311
86
Group Activity• On a typical day, a hurricane expends
the energy equivalent to the explosion of two thermonuclear weapons. A thermonuclear weapon has the explosive power of 1.0 Mton of nitroglycerin. Nitroglycerin generates 7.3 kJ of explosive power per gram of nitroglycerin. The hurricane’s energy comes from the evaporation of water that requires 2.3 kJ per gram of water evaporated. How many gallons of water does a hurricane evaporate per day?