Ch. 2 “Matter” 2.1: “What Is Matter?” 2.2: “Matter and Energy” 2.3: “Properties of Matter”
Matter
description
Transcript of Matter
Chem 106, Prof. J.T. Spencer 11
What is ChemistryWhat is Chemistry– Study of the “Physical” Properties Matter (Form and Function)
– Study of How Matter Changes (Reactivity)
Benefits of ChemistryBenefits of Chemistry– Pharmaceuticals
– Enhanced food production (fertilizers, herbicides, etc...)
– Plastics and Polymers
Why Study ChemistryWhy Study Chemistry– Core requirement (?)
– Central Science
EmploymentEmployment– Many fields
MatterMatter
Chapt. 1.1
BIO
Physics Medicine
GEO Engr
CHEM
Law
also: environmental economics electronics agriculture politics etc...
S.U. B.S.
Chem 106, Prof. J.T. Spencer 22
Matter; A ReviewMatter; A Review
Chapt. 1.1
Definition of MatterDefinition of Matter– anything that occupies space and has mass
StatesStates– gas (vapor); no fixed volume or shape, compressable
– liquid; fixed volume no fixed shape, mostly incompressable
– solid; fixed volume and shape, incompressable
FormsForms– Substances (pure or single); has a fixed composition and distinct
properties. Most things encountered are mixtures of substances.
PropertiesProperties– Physical Properties; can be measured without changing the substance,
i.e., color, density, melting point, etc...
– Chemical Properties; the way a substance changes (reacts), i.e., combustion
Chem 106, Prof. J.T. Spencer 33
Matter; A ReviewMatter; A Review
Chapt. 1.1
ChangesChanges
– Physical - Changes in appearance but not identity, i.e., evaporation, melting (all changes of state)
– Chemical - transformation into a different substance
Chemical ChangesChemical Changes Physical ChangesPhysical Changes
burning burning meltingmelting CC66HH1212OO66 + 6O + 6O22 6CO 6CO22 + 6H + 6H22OO H H22O(s)O(s) HH22O(l)O(l)
chemical reactionschemical reactions sublimationsublimation NaOH + HCl HNaOH + HCl H22O + NaCl O + NaCl H H22O(s)O(s) HH22O(g)O(g)
corrosioncorrosion dissolutiondissolution 4Fe + 3O4Fe + 3O22 2 Fe 2 Fe22OO3 3 H H22O(l ) + NaCl(s)O(l ) + NaCl(s) NaCl(aq)NaCl(aq)
Chem 106, Prof. J.T. Spencer 44
Matter; A ReviewMatter; A Review
Chapt. 1.1
Mixtures; combinations of substancesMixtures; combinations of substances
–MixtureMixture-
–Homogeneous Homogeneous –
–Heterogeneous Heterogeneous -
Chem 106, Prof. J.T. Spencer 55
Matter; A ReviewMatter; A Review
Chapt. 1.1
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Filtration Sand from SaltSand from Salt
Filter
Everyday ExamplesEveryday Examples;Auto Oil FilterAuto Air FilterAquarium Water FilterSpaghetti StrainerWindow ScreensRegistrar
Flow
Chem 106, Prof. J.T. Spencer 66
Matter; A ReviewMatter; A Review
Chapt. 1.1
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Distillation Water from Salt WaterWater from Salt Water
NaCl(aq)
NaCl(s) + H2O(l)
Chem 106, Prof. J.T. Spencer 77
Matter; A ReviewMatter; A Review
Chapt. 1.1
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Chromatograpgy Dyes from M&M’sDyes from M&M’s
Before After
Dyes
Chem 106, Prof. J.T. Spencer 88
Salt and Sand Mixture Ink from Cabbage Juicesolubility and filtrationsolubility and filtration chromatography chromatography
Water from Salt Water Iron and Gold Mixturedistillationdistillation magnetic propertiesmagnetic properties
melting point melting point differencesdifferences
chem. reactivity chem. reactivity (acids)(acids)
Iodine from Copper Chloridesolubility and filtrationsolubility and filtration
Matter; A ReviewMatter; A Review
Chapt. 1.1
Separating Mixtures using Physical PropertiesSeparating Mixtures using Physical Properties– How would you separate;
Chem 106, Prof. J.T. Spencer 99
Matter; Elements and CompoundsMatter; Elements and Compounds
Chapt. 1.2
SubstancesSubstances– Elements - substances which cannot be decomposed into simpler
substances (see periodic table)
– Compounds- substances which can be separated into two or more elements
ElementsElements– 110 Known (periodic table to be revisited)
– make up all matter and composed of “subatomic particles”
– symbols used for abbreviations (from older or common names)
CompoundsCompounds– Elements combined in a definite proportion by mass (law of definite
proportion)
– properties different than consititutent elements
Water; example of mixtures, compound and elements?Water; example of mixtures, compound and elements?
Chem 106, Prof. J.T. Spencer 1010
MatterMatter
MatterMatter
Uniform ?Uniform ?HeterogeneousHeterogeneousMixtureMixture
HomogeneousHomogeneous
Can be separatedCan be separatedby physical methodsby physical methodsPure SubstancePure Substance
HomogeneousHomogeneousMixture (solution)Mixture (solution)
Decomposed ?Decomposed ?
CompoundCompoundElementElement
YesYesNoNo
NoNo
NoNo
YesYes
YesYes
Chem 106, Prof. J.T. Spencer 1111
Matter; MeasurementMatter; Measurement
Chapt. 1.3
SystemsSystems
–Metric - base 10
– SI- international scientific system
– mass Kilogram
– length Meter
– time Second
– electric current Ampere
– temperature Kelvin
– light Candela
– Amount Mole Factor label method for conversionsFactor label method for conversions
Chem 106, Prof. J.T. Spencer 1212
Matter; MeasurementMatter; Measurement
Chapt. 1.3
PrefixesPrefixes
Mega M 106
Kilo k 103
Deci d 10-1
Centi c 10-2
Milli m 10-3
Micro 10-6
Nano n 10-9
Chem 106, Prof. J.T. Spencer 1313
Matter; MeasurementMatter; Measurement
Chapt. 1.3
Common Units:Length and Mass
Length - unit of distance measured in meters
Mass - measures the amount of matter in an object in grams
TemperatureKelvinCelsius °C = 5/9 (°F -32)
K = °C + 273.15
Chem 106, Prof. J.T. Spencer 1414
Matter; MeasurementMatter; Measurement
Chapt. 1.3
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F
Chem 106, Prof. J.T. Spencer 1515
Matter; MeasurementMatter; Measurement
Chapt. 1.3
Derived Units:Volume
Length x length x lengthmeasured in cm3, which is equal to mL
Chem 106, Prof. J.T. Spencer 1616
Matter; MeasurementMatter; Measurement
Chapt. 1.3
Derived Units:Density
amount of mass per unit volumemeasured in g/cm3, or g/mL
Chem 106, Prof. J.T. Spencer 1717
Matter; MeasurementMatter; Measurement
Chapt. 1.3
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed?
Chem 106, Prof. J.T. Spencer 1818
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.4
Precision and AccuracyPrecision and Accuracy– Precision - how closely individual measurements
agree– Accuracy- how closely the measurements agree with
the true value
Significant FiguresSignificant Figures– All measurements are inaccurate intrinsically
– measured quantities are reported such that the last figure is uncertain
Chem 106, Prof. J.T. Spencer 1919
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Good PrecisionPoor Accuracy
Good PrecisionGood Accuracy
Poor PrecisionPoor Accuracy
Chem 106, Prof. J.T. Spencer 2020
Determining Significant FiguresDetermining Significant Figures
–all non zero digits are significantall non zero digits are significant
– zeros between nonzero digits are significantzeros between nonzero digits are significant
– zeros to the left of first nonzero digit are not zeros to the left of first nonzero digit are not significantsignificant
– zeros at the end of a number and to the right zeros at the end of a number and to the right of a decimal point are significantof a decimal point are significant
–when a number ends in a zero but with no when a number ends in a zero but with no decimal point, the zero may or may not be decimal point, the zero may or may not be signigicant (use scientific notation)signigicant (use scientific notation)
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.4
Chem 106, Prof. J.T. Spencer 2121
Determining Significant FiguresDetermining Significant Figures
3.573 has 4 significant figures3.573 has 4 significant figures
0.073 has 2 significant figures0.073 has 2 significant figures
3.070 has 4 significant figures3.070 has 4 significant figures
0.003 has 1 significant figures0.003 has 1 significant figures
- - multiplication and divisionmultiplication and division; result can have no ; result can have no more than the figure with the fewest significant more than the figure with the fewest significant figuresfigures
- - addition and subtractionaddition and subtraction; result can have the ; result can have the same number of decimal places as the term with same number of decimal places as the term with the least number of decimal placesthe least number of decimal places
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.4
Chem 106, Prof. J.T. Spencer 2222
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g
B) 2.3 x 104 cm
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 2323
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 2424
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) 0.00134 m3
Chem 106, Prof. J.T. Spencer 2525
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: How many significant figures are in each of the following measurements?
A) 3.549 g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) 0.00134 m3 3 sig figs
Chem 106, Prof. J.T. Spencer 2626
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
Chem 106, Prof. J.T. Spencer 2727
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
Chem 106, Prof. J.T. Spencer 2828
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
x = 2172.6144 m
Chem 106, Prof. J.T. Spencer 2929
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs 1 is infinitely significant
Chem 106, Prof. J.T. Spencer 3030
Matter; Uncertainty in MeasurementMatter; Uncertainty in Measurement
Chapt. 1.3
Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = 1 mi
x 1609.344 m
1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs x = 2170 m 1 is infinitely significant
Chem 106, Prof. J.T. Spencer 3131
Use Units throughout the calculation (helps “guide” calculation.
Should always yield the proper units Uses conversion factors Example; How fast is 50 mph in in/sec.?
Dimensional AnalysisDimensional Analysis
50 mi.50 mi. 1 hour1 hour 5280 ft5280 ft 12 in.12 in. = = inin1 hour1 hour 3600 sec.3600 sec. 1 mi.1 mi. 1 ft1 ft sec.sec.
Chem 106, Prof. J.T. Spencer 3232
Dimensional AnalysisDimensional Analysis
Chapt. 1.3
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
Chem 106, Prof. J.T. Spencer 3333
Dimensional AnalysisDimensional Analysis
Chapt. 1.3
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi
Chem 106, Prof. J.T. Spencer 3434
Dimensional AnalysisDimensional Analysis
Chapt. 1.3
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km
0.62137 mi
Chem 106, Prof. J.T. Spencer 3535
Dimensional AnalysisDimensional Analysis
Chapt. 1.3
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km = 804.674 km
0.62137 mi
Chem 106, Prof. J.T. Spencer 3636
Dimensional AnalysisDimensional Analysis
Chapt. 1.3
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race.
500.0 mi 1 km = 804.674 km
0.62137 mi
* answer can only have 4 sig figs; 804.7 km
Chem 106, Prof. J.T. Spencer 3737
Matter: Chemical and Physical ChangesMatter: Chemical and Physical Changes Elements and CompoundsElements and Compounds Units of MeasurementUnits of Measurement Uncertainty and Significant FiguresUncertainty and Significant Figures Precision and AccuracyPrecision and Accuracy ““Factor Label” Method (Dimensional Factor Label” Method (Dimensional
Analysis)Analysis)
Chapter One; ReviewChapter One; Review