1 chapter one matter and measurement. 2 matter and energy - vocabulary chemistrychemistry...

11

CHAPTER ONECHAPTER ONEMatter and MeasurementMatter and Measurement

22

Matter and Energy - VocabularyMatter and Energy - Vocabulary

• ChemistryChemistry

• MatterMatter

• EnergyEnergy

• Natural Law-(scientific law)Natural Law-(scientific law)

• Scientific MethodScientific Method– Observation, Hypothesis, Experiment, and Observation, Hypothesis, Experiment, and

TheoryTheory

33

States of MatterStates of Matter

• SolidsSolids

44


• SolidsSolids

• LiquidsLiquids

55


• SolidsSolids

• LiquidsLiquids

• GasesGases

66


• Change StatesChange States– heatingheating– coolingcooling

77

States of MatterStates of Matter• Illustration of changes in stateIllustration of changes in state

– requires energyrequires energy

88

Substances, Compounds, Substances, Compounds, Elements and MixturesElements and Mixtures

• SubstanceSubstance– matter that all samples have identical composition matter that all samples have identical composition

and propertiesand properties

• ElementsElements– Pure substances that cannot be decomposed into Pure substances that cannot be decomposed into

simpler substances via chemical reactionssimpler substances via chemical reactions– Special elemental forms of atoms (diatomic)Special elemental forms of atoms (diatomic)

Elemental symbolsElemental symbols– found on periodic chartfound on periodic chart

99


1010


• CompoundsCompounds– Pure substances composed of two or more Pure substances composed of two or more

elements in a definite ratio by masselements in a definite ratio by mass– can be decomposed into the constituent elementscan be decomposed into the constituent elements

REVIEWREVIEW– Element cannot be broken downElement cannot be broken down– Compound can be broken down into its elements!Compound can be broken down into its elements!

1111


• MixturesMixtures– composed of two or more substancescomposed of two or more substances– homogeneous mixtureshomogeneous mixtures

• Uniform throughoutUniform throughout• Example: solutionsExample: solutions

– heterogeneous mixturesheterogeneous mixtures• Nonuniform Nonuniform • Example: rocksExample: rocks

1212

Classify the following substances as an Classify the following substances as an element, compound or a mixture element, compound or a mixture

(homogeneous or heterogeneous). Which are (homogeneous or heterogeneous). Which are pure substances?pure substances?

• Lightly scrambled eggLightly scrambled egg

• WaterWater

• Lava lampLava lamp

• SeawaterSeawater

• Freshly opened root beerFreshly opened root beer

• Flat root beerFlat root beer

• Sucrose (CSucrose (C1212HH2222OO1111))

1313

Separating MixturesSeparating Mixtures• DistillationDistillation

1414

Separating MixturesSeparating Mixtures• ChromatographyChromatography

paperpaper

1515

Chemical and Physical PropertiesChemical and Physical Properties

• Extensive Properties - depend on quantity Extensive Properties - depend on quantity of materialof material

Ex. mass Ex. mass

• Intensive Properties - do not depend on Intensive Properties - do not depend on quantity of materialquantity of material

Ex. boiling point Ex. boiling point

1616

Chemical and Physical PropertiesChemical and Physical Properties

• Chemical Properties - chemical changesChemical Properties - chemical changes– Observed during change of material to new Observed during change of material to new

materialmaterial• Iron rustingIron rusting

• Physical Properties - physical changesPhysical Properties - physical changes– No change to the identity of the substanceNo change to the identity of the substance

• changes of statechanges of state• density density • color color • solubilitysolubility

1717

Physical PropertiesPhysical Properties

• DensityDensity– mass / volumemass / volume intensive propertyintensive property– Mass and volume Mass and volume extensive propertiesextensive properties

• SolubilitySolubility– Amount of substance dissolved in the solvent at Amount of substance dissolved in the solvent at

a given temperaturea given temperature• Saturated solutionSaturated solution• Unsaturated solutionUnsaturated solution• Supersaturated solutionSupersaturated solution

1818

Identify the following as either a Identify the following as either a chemical or physical change.chemical or physical change.

• Combination of sodium and chlorine to Combination of sodium and chlorine to give sodium chloride.give sodium chloride.

• Liquefaction of gaseous nitrogen.Liquefaction of gaseous nitrogen.

• Separation of carbon monoxide into Separation of carbon monoxide into carbon and oxygen.carbon and oxygen.

• Freezing of water.Freezing of water.

1919

Measurements in ChemistryMeasurements in Chemistry

• lengthlength meter meter m m

• volumevolume liter liter l l

• massmass gram gram g g

• timetime second second s s

• currentcurrent ampere ampere A A

• temperaturetemperature Kelvin Kelvin KK

• amt. substanceamt. substance mole mole molmol

2020

Measurements in ChemistryMeasurements in Chemistry• mega mega MM 10 1066

• kilo kilo k k 10 1033

• deka deka dada 10 10

• deci deci dd 10 10-1-1

• centi centi cc 10 10-2-2

• milli milli mm 10 10-3-3

• micro micro 10 10-6-6

• nano nano nn 10 10-9-9

• pico pico p p 10 10-12-12

• femto femto f f 10 10-15-15

2121

Units of MeasurementUnits of Measurement• Mass Mass

– measure of the quantity of matter in a bodymeasure of the quantity of matter in a body

• WeightWeight– measure of the gravitational attraction for a body measure of the gravitational attraction for a body

• Length Length 1 m = 39.37 inches1 m = 39.37 inches

2.54 cm = 1 inch2.54 cm = 1 inch

• VolumeVolume1 liter = 1.06 qt 1 liter = 1.06 qt

1 qt = 0.946 liter1 qt = 0.946 liter

2222

The Use of NumbersThe Use of Numbers

• Exact numbers 1 dozen = 12 thingsExact numbers 1 dozen = 12 things

• Accuracy Accuracy – how closely measured values agree with how closely measured values agree with

the correct valuethe correct value

• PrecisionPrecision– how closely individual measurements how closely individual measurements

agree with each otheragree with each other

2323


2424


• Exact numbers 1 dozen = 12 thingsExact numbers 1 dozen = 12 things– Counted numbers ex. 3 beakersCounted numbers ex. 3 beakers

• Significant figuresSignificant figures– digits believed to be correct by the person making digits believed to be correct by the person making

the measurementthe measurement– measure a mile with a 6 inch ruler vs. surveying measure a mile with a 6 inch ruler vs. surveying

equipment equipment

• Scientific notationScientific notation– Way of signifying the significant digits in a numberWay of signifying the significant digits in a number

2525

Significant Figures - rulesSignificant Figures - rules

• leading zeroes - never significantleading zeroes - never significant0.000357 has three sig fig0.000357 has three sig fig

• trailing zeroes - may be significanttrailing zeroes - may be significantmust specify (after decimal – significant must specify (after decimal – significant

before decimal - ambiguous)before decimal - ambiguous)1300 nails - counted or weighed?1300 nails - counted or weighed?

Express 26800 in scientific notation withExpress 26800 in scientific notation with4 sig figs4 sig figs 3 sig figs3 sig figs 2 sig figs2 sig figs

2626


• imbedded zeroes are always significantimbedded zeroes are always significant3.0604 has five sig fig3.0604 has five sig fig

How many significant figures are in the following How many significant figures are in the following numbers?numbers?

0.01240.01240.1240.1241.2401.24012401240

2727


multiply & divide rule - easymultiply & divide rule - easyproduct has the smallest number of sig. fig. product has the smallest number of sig. fig.

of multipliersof multipliers

2828


• multiply & divide rule - easymultiply & divide rule - easyproduct has the smallest number of sig. fig. product has the smallest number of sig. fig.


310 x 5.22 tooff round

66.5217

31.2x

224.4

2929


• multiply & divide rule - easymultiply & divide rule - easyproduct has the smallest number of sig. fig. product has the smallest number of sig. fig.


310 x 5.22 tooff round

66.5217

31.2x

224.4

3.9 tooff round

89648.3

41.x

2783.2

3030

PracticePractice

• 142 x 2 = 142 x 2 =

• 4.180 x 2.0 = 4.180 x 2.0 =

• 0.00482 / 0.080 = 0.00482 / 0.080 =

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = =

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = =

3131

PracticePractice

• 142 x 2 = 300142 x 2 = 300

• 4.180 x 2.0 = 4.180 x 2.0 =

• 0.00482 / 0.080 = 0.00482 / 0.080 =

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = =

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = =

3232

PracticePractice

• 142 x 2 = 300142 x 2 = 300

• 4.180 x 2.0 = 8.44.180 x 2.0 = 8.4

• 0.00482 / 0.080 = 0.00482 / 0.080 =

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = =

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = =

3333

PracticePractice

• 142 x 2 = 300142 x 2 = 300

• 4.180 x 2.0 = 8.44.180 x 2.0 = 8.4

• 0.00482 / 0.080 = 0.0600.00482 / 0.080 = 0.060

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = =

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = =

3434

PracticePractice

• 142 x 2 = 300142 x 2 = 300

• 4.180 x 2.0 = 8.44.180 x 2.0 = 8.4

• 0.00482 / 0.080 = 0.0600.00482 / 0.080 = 0.060

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = 1.58x10 = 1.58x10-7-7

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = =

3535

PracticePractice

• 142 x 2 = 300142 x 2 = 300

• 4.180 x 2.0 = 8.44.180 x 2.0 = 8.4

• 0.00482 / 0.080 = 0.0600.00482 / 0.080 = 0.060

• 3.15x103.15x10-2-2 / 2.00x10 / 2.00x1055 = 1.58x10 = 1.58x10-7-7

• 24.8x1024.8x1066 / 6.200x10 / 6.200x10-2-2 = 4.00x10 = 4.00x1088

3636


• add & subtract rule - subtleadd & subtract rule - subtleanswer contains smallest decimal place of answer contains smallest decimal place of

the addendsthe addends

3737




6.95 tooff round

9463.6

20.2

423.1

3692.3

3838




6.95 tooff round

9463.6

20.2

423.1

3692.3

6.671 tooff round

6707.6

312.2

7793.8

3939

PracticePractice

• 416.2 – 10.18 =416.2 – 10.18 =

• 16.78 + 10. = 16.78 + 10. =

• 422.501 – 420.4 = 422.501 – 420.4 =

• 25.5 + 21.1 + 3.201 = 25.5 + 21.1 + 3.201 =

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = =

4040

PracticePractice

• 416.2 – 10.18 = 406.0416.2 – 10.18 = 406.0

• 16.78 + 10. = 16.78 + 10. =

• 422.501 – 420.4 = 422.501 – 420.4 =

• 25.5 + 21.1 + 3.201 = 25.5 + 21.1 + 3.201 =

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = =

4141

PracticePractice

• 416.2 – 10.18 = 406.0416.2 – 10.18 = 406.0

• 16.78 + 10. = 2716.78 + 10. = 27

• 422.501 – 420.4 = 422.501 – 420.4 =

• 25.5 + 21.1 + 3.201 = 25.5 + 21.1 + 3.201 =

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = =

4242

PracticePractice

• 416.2 – 10.18 = 406.0416.2 – 10.18 = 406.0

• 16.78 + 10. = 2716.78 + 10. = 27

• 422.501 – 420.4 = 2.1422.501 – 420.4 = 2.1

• 25.5 + 21.1 + 3.201 = 25.5 + 21.1 + 3.201 =

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = =

4343

PracticePractice

• 416.2 – 10.18 = 406.0416.2 – 10.18 = 406.0

• 16.78 + 10. = 2716.78 + 10. = 27

• 422.501 – 420.4 = 2.1422.501 – 420.4 = 2.1

• 25.5 + 21.1 + 3.201 = 49.825.5 + 21.1 + 3.201 = 49.8

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = =

4444

PracticePractice

• 416.2 – 10.18 = 406.0416.2 – 10.18 = 406.0

• 16.78 + 10. = 2716.78 + 10. = 27

• 422.501 – 420.4 = 2.1422.501 – 420.4 = 2.1

• 25.5 + 21.1 + 3.201 = 49.825.5 + 21.1 + 3.201 = 49.8

• 42.00x1042.00x10-4-4 + 1.8x10 + 1.8x10-6-6 = 4.2 x 10 = 4.2 x 10-3-3

4545

More PracticeMore Practice

4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (3.38 – 3.01) =

4646


4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =4.18 – 58.16 x (0.37) =

4747


4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =4.18 – 58.16 x (0.37) =

4.18 – 21.5192 = 4.18 – 21.5192 =

4848


4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =4.18 – 58.16 x (0.37) =

4.18 – 21.5192 = 4.18 – 21.5192 =

-17.3392-17.3392

Round off correctlyRound off correctly

4949


4.18 – 58.16 x (3.38 – 3.01) = 4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =4.18 – 58.16 x (0.37) =

4.18 – 21.5192 = 4.18 – 21.5192 =

-17.3392-17.3392

Round off correctly to 2 sig. figsRound off correctly to 2 sig. figs

-17-17

5050

Unit Factor MethodUnit Factor MethodDimensional Analysis Dimensional Analysis

• simple but simple but importantimportant way to way to alwaysalways get get right answerright answer

• way to change from one unit to anotherway to change from one unit to another

• make unit factors from statementsmake unit factors from statements 1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft

3 ft = 1 yd becomes 3ft/1yd or 1yd/3ft3 ft = 1 yd becomes 3ft/1yd or 1yd/3ft

5151

Unit Factor MethodUnit Factor MethodDimensional Analysis Dimensional Analysis

• simple but simple but importantimportant way to way to alwaysalways get get right answerright answer

• way to change from one unit to anotherway to change from one unit to another

• make unit factors from statementsmake unit factors from statements 1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft

• Example: Express 12.32 yards in Example: Express 12.32 yards in millimeters.millimeters.

5252

Unit Factor MethodUnit Factor Method

.).........yd1

ft3( yd 12.32

mm ?yd 12.32

5353

Unit Factor MethodUnit Factor Method

mm 10)11.27cm1

mm10( )

in1

cm2.54( )

ft1

in12( )

yd1

ft3( yd 12.32

mm ?yd 12.32

3

5454

Unit Factor MethodUnit Factor Method• Example: Express 323. milliliters in Example: Express 323. milliliters in

gallonsgallons

5555

Unit Factor MethodUnit Factor Method• Express 323. milliliters in gallons.Express 323. milliliters in gallons.

gal 0.0856gal 0.085595gal ?

)qt4

gal1( )

L1

qt1.06( )

mL1000

L1( mL 323gal ?

mL 323gal ?

5656

Unit Factor MethodUnit Factor Method• Example: Express 5.50 metric tons in Example: Express 5.50 metric tons in

pounds. 1 metric ton = 1 Megagrampounds. 1 metric ton = 1 Megagram

5757

Unit Factor MethodUnit Factor Method• Example: Express 5.50 metric tons in Example: Express 5.50 metric tons in

pounds.pounds.

lbsxlbsg

lbgrams 46

1021.1537.12114454

1

tonmetric 1

1x10 tons5.50 lbs ?

tonsmetric 5.50 lbs ?

5858

Unit Factor MethodUnit Factor Method• area is two dimensionalarea is two dimensional

• Example: Express 4.21 x 10Example: Express 4.21 x 1066 square square centimeters in square feet centimeters in square feet

5959


express 4.21 x 10express 4.21 x 1066 square centimeters in square centimeters in square feet square feet

2262 )cm 2.54

in 1(cm104.21ft ?

6060



22262 )in12

ft 1()

cm2.54

in 1(cm104.21ft ?

6161



232

22262

ft 4.53x10ft 4531.6063

)in12

ft1()

cm2.54

in1(cm104.21ft ?

6262

Unit Factor MethodUnit Factor Method• volume is three dimensionalvolume is three dimensional

• Example: Express 3.61 cubic feet in Example: Express 3.61 cubic feet in cubic centimeters. cubic centimeters.

6363

Unit Factor MethodUnit Factor Method• volume is three dimensionalvolume is three dimensional

• Example: Express 3.61 cubic feet in Example: Express 3.61 cubic feet in cubic centimeters.cubic centimeters.

353

3333

cm 101.02cm 102223.42

)in 1

cm 2.54()

ft 1

in 12(ft 3.61cm ?

6464

PercentagePercentage

• Percentage is the parts per hundred of Percentage is the parts per hundred of a sample.a sample.

• Example: A 500. g sample of ore yields Example: A 500. g sample of ore yields 27.9 g of sulfur. What is the percent of 27.9 g of sulfur. What is the percent of sulfur in the ore?sulfur in the ore?

6565

PercentagePercentage• Percentage is the parts per hundred of Percentage is the parts per hundred of

a sample.a sample.

• Example: A 500. g sample of ore yields Example: A 500. g sample of ore yields 27.9 g of sulfur. What is the percent of 27.9 g of sulfur. What is the percent of sulfur in the ore?sulfur in the ore?

5.58%

100%x ore g 500

S g 27.9

100% x ore of grams

sulfur of grams iron % ?

6666

Derived Units - Density Derived Units - Density • density = mass/volumedensity = mass/volume

• What is density?What is density?

• Example: Calculate the density of a Example: Calculate the density of a substance if 123. grams of it occupies substance if 123. grams of it occupies 57.6 cubic centimeters.57.6 cubic centimeters.

6767




Vm D

mL 6.57cm 57.6 mL 1 cm 1 33

6868




g/mL 2.13 DmL 57.6

g 123. D

Vm D

mL 6.57cm 57.6 mL 1 cm 1 33

6969

Derived Units - Density Derived Units - Density • Example: Suppose you need 175. g of a Example: Suppose you need 175. g of a

corrosive liquid for a reaction. What corrosive liquid for a reaction. What volume do you need? volume do you need? – liquid’s density = 1.02 g/mLliquid’s density = 1.02 g/mL

7070



D

mV

V

mD

7171



mL 172mL 171.57 1.02

g 175V

D

mV

V

mD

mLg

7272

Heat & TemperatureHeat & Temperature• heat and T are not the same thingheat and T are not the same thing

T is a measure of the intensity of heat in a bodyT is a measure of the intensity of heat in a body

• 3 common T scales - all use water as a 3 common T scales - all use water as a referencereference

7373

Heat & TemperatureHeat & TemperatureMPMP BPBP

• Fahrenheit Fahrenheit 3232ooF F 212212ooFF

• Celsius Celsius 00ooC C 100100ccCC

• Kelvin Kelvin 273 K 273 K 373 K373 K

7474

Relationships of the 3 T ScalesRelationships of the 3 T Scales

273KC

or

273 C K

o

o

7575


1.85

9

10

18

100

180

273K C

or

273 C K

o

o

7676


1.8

32FC

or

32C 1.8F

1.85

9

10

18

100

180

273KC

or

273 C K

oo

oo

o

o

7777

Heat and TemperatureHeat and Temperature• Example: Convert 111.Example: Convert 111.ooF to degrees F to degrees

Celsius.Celsius.

1.8

32111C

1.8

32FC

o

oo

7878

Heat and TemperatureHeat and Temperature• Example: Convert 111.Example: Convert 111.ooF to degrees F to degrees

Celsius.Celsius.

9.438.1

791.8

32111C

1.8

32FC

o

oo

7979

Heat and TemperatureHeat and Temperature• Example: Express 757. K in Celsius Example: Express 757. K in Celsius

degrees.degrees.

8080

Heat and TemperatureHeat and Temperature• Example: Express 757. K in Celsius Example: Express 757. K in Celsius

degrees.degrees.

.484C

273..757C

273.KC

o

o

o

8181

The Measurement of HeatThe Measurement of Heat

• SI unit J (Joule)SI unit J (Joule)

• calorie calorie 1 calorie = 4.184 J1 calorie = 4.184 J

• English unit = BTUEnglish unit = BTU

8282

Synthesis QuestionSynthesis Question• It has been estimated that 1.0 g of It has been estimated that 1.0 g of

seawater contains 4.0 pg of Au. The seawater contains 4.0 pg of Au. The total mass of seawater in the oceans is total mass of seawater in the oceans is 1.6x101.6x101212 Tg, If all of the gold in the Tg, If all of the gold in the oceans were extracted and spread oceans were extracted and spread evenly across the state of Georgia, evenly across the state of Georgia, which has a land area of 58,910 milewhich has a land area of 58,910 mile22, , how tall, in feet, would the pile of Au how tall, in feet, would the pile of Au be?be?Density of Au is 19.3 g/cmDensity of Au is 19.3 g/cm33. 1.0 Tg = 10. 1.0 Tg = 101212g. g.

8383

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

8484

331533

3113

12

12

2

12

224

224

1212

mile 1cm 104.16 mile 1cm 160,934

cm 160,934in 1

cm 2.54

ft 1

in 12

mile 1

ft 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

8585

ft 107.13mile 1

ft 5280mile)10(1.35

mile 58,910

mile107.96

mile107.96cm104.16

mile 1Au) cm 10(3.3

692

35

35315

3311

8686

Group ActivityGroup Activity• On a typical day, a hurricane expends On a typical day, a hurricane expends

the energy equivalent to the explosion of the energy equivalent to the explosion of two thermonuclear weapons. A two thermonuclear weapons. A thermonuclear weapon has the explosive thermonuclear weapon has the explosive power of 1.0 Mton of nitroglycerin. power of 1.0 Mton of nitroglycerin. Nitroglycerin generates 7.3 kJ of Nitroglycerin generates 7.3 kJ of explosive power per gram of explosive power per gram of nitroglycerin. The hurricane’s energy nitroglycerin. The hurricane’s energy comes from the evaporation of water that comes from the evaporation of water that requires 2.3 kJ per gram of water requires 2.3 kJ per gram of water evaporated. How many gallons of water evaporated. How many gallons of water does a hurricane evaporate per day?does a hurricane evaporate per day?

1 chapter one matter and measurement. 2 matter and energy - vocabulary chemistrychemistry...

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