chapter 1 matter and measurement. what is chemistry? the study of all substances and the changes...
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Chapter 1Chapter 1Matter and Matter and
MeasurementMeasurement
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What is Chemistry?What is Chemistry?
The study of all substances and the The study of all substances and the changes that they can undergochanges that they can undergo
The CENTRAL SCIENCEThe CENTRAL SCIENCE
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Why Study Chemistry?Why Study Chemistry?
Useful for other sciencesUseful for other sciences
Required course Required course Fun and ChallengingFun and Challenging
Remember:Remember:– Process of DiscoveryProcess of Discovery– Understand Concepts, NOT Single FactsUnderstand Concepts, NOT Single Facts
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Scientific MethodScientific MethodObservatio
n
Question
Hypothesis
Experiment
Conclusion
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Scientific MethodScientific Method
Natural Law
•Explains how nature behaves
Theory•Explains why nature behaves in a certain
way
Conclusion
Prediction Experiment
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LiquidsLiquids
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LiquidsLiquids
Definite Definite
Molecules Molecules
Not affected by Not affected by
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SolidsSolids
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SolidsSolids
Don’t Don’t
Definite Definite
Molecules Molecules
Not affected by Not affected by
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GasesGases
Low Low
Density Density
Expands to Expands to
Indefinite Indefinite
Molecules move Molecules move
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The Metric SystemThe Metric SystemThe International System of UnitsThe International System of Units
Standards of measurementStandards of measurementBase units (7) – Fig 1-14 p. 18Base units (7) – Fig 1-14 p. 18
1.1. MASS: MASS: 2.2. LENGTH: LENGTH: 3.3. TIME: TIME: 4.4. COUNT, QUANTITY: COUNT, QUANTITY: 5.5. TEMPERATURE: TEMPERATURE: 6.6. ELECTRIC CURRENT: ELECTRIC CURRENT: 7.7. LUMINOUS INTENSITY: LUMINOUS INTENSITY:
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The Metric SystemThe Metric SystemDerived Units:Derived Units: AREA: AREA: VOLUME: VOLUME: ENERGY: ENERGY: FORCE: FORCE: PRESSURE:PRESSURE: POWER: POWER: VOLTAGE: VOLTAGE: FREQUENCY: FREQUENCY: ELECTRIC CHARGE: ELECTRIC CHARGE:
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The Metric SystemThe Metric System
Metric Prefixes – make base unit larger Metric Prefixes – make base unit larger or smalleror smaller
Based on 10Based on 10
Math method vs. “Stairs”Math method vs. “Stairs”
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Convert a volume of 12 microliters into Convert a volume of 12 microliters into centiliterscentiliters
Express a distance of 15 meters in Express a distance of 15 meters in kilometerskilometers
Convert 83 cm into metersConvert 83 cm into meters
Which is the longer amount of time, 1351 Which is the longer amount of time, 1351 ps or 1.2 ns?ps or 1.2 ns?
Convert 16 dL into LConvert 16 dL into L
Conversion PracticeConversion Practice
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Types of MeasurementsTypes of Measurements
Mass – amount of Mass – amount of – Expressed in Expressed in – Does not Does not
Weight – Weight – – Expressed in Expressed in – Changes with Changes with
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Types of MeasurementsTypes of Measurements
Volume – the amount of Volume – the amount of – – Many instruments to measureMany instruments to measure
Temperature – Temperature – – – Degrees Degrees – Degress Degress
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DensityDensityCommon ratio used in Common ratio used in chemistrychemistry
Physical property of a Physical property of a substancesubstance
SI units: SI units:
SolidSolid–
LiquidLiquid–
GasGas–
Can change due to temperature and/or pressure changes
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DensityDensity
1.Find the density of a piece of metal with a volume of 2.7 cm3 and a mass of 10.8 g.
2. Determine the mass of an object with a density of 0.24 g/cm3 and a volume of 2 cm3.
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Uncertainty in MeasurementUncertainty in Measurement
Why are digits in measurements uncertain?Why are digits in measurements uncertain?
1.1. Instruments never completely free of flawsInstruments never completely free of flaws
2.2. Always involves estimationAlways involves estimation Choose the right instrument for the jobChoose the right instrument for the job May be estimated for you (electronic May be estimated for you (electronic
scales)scales) Scale is marked but you estimate the in-Scale is marked but you estimate the in-
betweenbetween
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Uncertainty in MeasurementUncertainty in Measurement
Precision: Precision:
Accuracy: Accuracy:
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Significant DigitsSignificant DigitsAll digits known with certainty plus one All digits known with certainty plus one final digit which is uncertain (or estimated)final digit which is uncertain (or estimated)
All non-zeros are All non-zeros are
A zero is significant when :A zero is significant when :– It is It is – It is It is
A zero is not significant when:A zero is not significant when:– It is It is – It is It is
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Significant Digits - PRACTICESignificant Digits - PRACTICE
How many significant digits?How many significant digits?1.1. 54.2354.232.2. 23.0000523.000053.3. 0.00040.00044.4. 35000350005.5. 0.0005040.0005046.6. 45.62320045.6232007.7. 5,000,0005,000,0008.8. 4,000,000.14,000,000.1
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Significant Digits - CalculationsSignificant Digits - Calculations
Addition and SubtractionAddition and Subtraction–
1.21 + 5.002 + 10. = 1.21 + 5.002 + 10. = 16.212 becomes 1616.212 becomes 16
34.5 + 12.45 + 23.0505 = 34.5 + 12.45 + 23.0505 =
186.31 + 11.1 = 186.31 + 11.1 =
12.0231 + 3.86 = 12.0231 + 3.86 =
0.100012 + 120. =0.100012 + 120. =
1200 + 12 + 15 + 0.5 =1200 + 12 + 15 + 0.5 =
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Significant Digits - CalculationsSignificant Digits - Calculations
Multiplication and DivisionMultiplication and Division– The answer has as many sig figs as the The answer has as many sig figs as the
number with the fewest sig figsnumber with the fewest sig figs14.8 x 3.1 = 14.8 x 3.1 = 45.88 becomes 4645.88 becomes 46
18.2 x 3.0 =18.2 x 3.0 =
52/1.5 =52/1.5 =
321.868783 x 1 =321.868783 x 1 =
2400 x 2.123 =2400 x 2.123 =
15000/12.354 =15000/12.354 =
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Scientific NotationScientific Notation
Convenient way of writing very large or Convenient way of writing very large or very small numbers and showing only very small numbers and showing only significant figuressignificant figuresNumber between 1 & 10 with a power of Number between 1 & 10 with a power of tenten5120 becomes 5.12 x 105120 becomes 5.12 x 1033
Move decimal point in original number to Move decimal point in original number to make number 1-10make number 1-10Move left = +; move right = -Move left = +; move right = -
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Scientific Notation PracticeScientific Notation Practice
123,000 =123,000 =
0.000045 =0.000045 =
23.45 =23.45 =
0.0000000003 =0.0000000003 =
1,000,000 =1,000,000 =
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Scientific NotationScientific Notation
Adding and subtractingAdding and subtracting
Multiply and divideMultiply and divide
3.38 x 103
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Conversion FactorsConversion Factors
Enable movement between metric system and Enable movement between metric system and “English” system“English” system
See back cover of book and Appendix IIISee back cover of book and Appendix III
Common conversions you should memorizeCommon conversions you should memorize– 1 inch = 2.54 cm1 inch = 2.54 cm– 1 mile = 1.609 km1 mile = 1.609 km– 1 kg = 2.20 pounds1 kg = 2.20 pounds– 1 mL = 1 cm1 mL = 1 cm33
– 0 K = -273.15 0 K = -273.15 00CC– 00F = 1.8(F = 1.8(00C) + 32C) + 32
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Dimensional AnalysisDimensional Analysis(Problem Solving)(Problem Solving)
Remember: ALWAYS use UNITS OF Remember: ALWAYS use UNITS OF MEASUREMENT in your work!!!MEASUREMENT in your work!!!
A technique of converting between unitsA technique of converting between units– Same system (metrics)Same system (metrics)– Different systems (inches to meters)Different systems (inches to meters)– Chemical equations….later chapters…Chemical equations….later chapters…
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Dimensional AnalysisDimensional Analysis(Problem Solving)(Problem Solving)
Conversion Factors: ratio derived from the Conversion Factors: ratio derived from the equality between 2 different unitsequality between 2 different units
CF can be written either wayCF can be written either way
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Dimensional AnalysisDimensional Analysis(Problem Solving)(Problem Solving)
The “t” methodThe “t” method
Example: How many liters are in 125.6 gallons?
Conversion Factor
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How many seconds are in 4.15 hours?
Dimensional AnalysisDimensional Analysis(Problem Solving)(Problem Solving)
Dimensional AnalysisDimensional Analysis(Problem Solving)(Problem Solving)
If a student needs 1.5 mL of water, how many cups does he need?