Topic 1 Matter, Measurement, And Methods
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Transcript of Topic 1 Matter, Measurement, And Methods
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Topic 1
Matter and Measurement
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[1] Discuss chemistry and describe the
interrelationship of chemistry with other fields ofscience.[2] Describe the properties of the solid, liquid,and gaseous states.[3] Classify matter as element, compound or mixture.
[4] Provide specific examples of physical andchemical properties and physical and chemicalchange.[5] Distinguish between intensive and extensiveproperties.[6] Discuss the approach to science, the scientificmethod, and distinguish among the terms hypothesis,theory, and scientific law.
Learning Objectives
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[7] Learn the major units of measure in the metric
systems.[8] Know the three common temperature scales, and beable to convert from one system to another.
[9] Use density, mass and volume in problem solvingand calculate the specific gravity of a substancefrom its density.[10] Report data and results using scientificnotation and the proper number of significantfigures.
[11] Use dimensional analysis in conversion ofunits.
Learning Objectives (contd)
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------------------------------LEARNING OBJECTIVE 1
[1] Discuss chemistry anddescribe the interrelationshipof chemistry with other fields
of science.-----------------------------
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ChemistryChemistry is the study of the composition,structure, properties, and changes of matter.
Composition of matter relates to the kinds ofelements it contains.
Structure of matter relates to the ways the
atoms of these elements are arranged. Property of matter is any characteristic that
gives a sample of matter its unique identity. Changes of matter can be physical or chemical
change.
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Why study chemistry?
Chemistry is the central science , central to afundamental understanding of other sciences andtechnologies.
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------------------------------LEARNING OBJECTIVE 2
[2] Describe the properties ofthe solid, liquid, and gaseousstates.------------------------------LEARNING OBJECTIVE 3[3] Classify matter aselement, compound or mixture.
-----------------------------
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Gas (also known as vapor)
has no fixed volume or shape conforms to the volume and
shape of its container andcompressible
Liquid has a distinct volume has no specific shape assumes the shape of the
portion of the container itoccupies and incompressible
Solid has both definite volume and
shape incompressible
States of Matter
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Classification of Matter
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------------------------------LEARNING OBJECTIVE 4
[4] Provide specific examplesof physical and chemicalproperties and physical andchemical change.------------------------------LEARNING OBJECTIVE 5[5] Distinguish between
intensive and extensiveproperties.
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Physical and Chemical Change
Physical Change produces a recognizable
difference in theappearance of a substancewithout causing any change
in its composition oridentity.
Example: boiling of water,crushing a can, melting anice, mixing sand and water,breaking a glass, dissolving
sugar and water, shreddingpaper, chopping wood, mixingred and green marbles,sublimating ice
Chemical Change process of rearranging,
removing, replacing, oradding atoms to producenew substances.
Example:electrolysis of water,rusting of iron, combustionof wood, metabolism of foodin the body, mixing acid andbase, cooking an egg,digesting sugar with amylasein saliva, mixing bakingsoda and vinegar to produceCO2 gas, baking a cake,electroplating a metal,using a chemical battery
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Intensive and Extensive Properties
Intensive Properties Independent of the
amount of matterexamined
Example:
Temperature, Color, Odor,Luster, Malleability,Ductility, Conductivity,Hardness, Melting andFreezing Point, BoilingPoint, Density
Extensive Properties Relate to the amount of
substance present
Example:
Mass, Weight, Volume,Length
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------------------------------LEARNING OBJECTIVE 6
[6] Discuss the approach toscience, the scientificmethod, and distinguish amongthe terms hypothesis, theory,and scientific law.-----------------------------
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Scientific Method
Observation of
a phenomenon
A question
A hypothesis
(a potentialanswer)
Experimentation
Data analysis
Theory
Scientific law
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------------------------------LEARNING OBJECTIVE 7
[7] Learn the major units ofmeasure in the metric systems.-----------------------------
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SI Base Units
Systeme Internaional dUnites or the SI units
developed in France is widely used today!
Units of Measurement
Physical Quantity Name of Unit Abbreviation
Mass Kilogram kg Length Meter m
Time Second s or sec
Temperature Kelvin K
Amount of substance Mole mol Electric current Ampere A or amp
Luminous intensity Candela cd
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------------------------------LEARNING OBJECTIVE 8[8] Know the three common
temperature scales, and beable to convert from onesystem to another.
------------------------------LEARNING OBJECTIVE 9[9] Use density, mass andvolume in problem solving andcalculate the specific gravityof a substance from itsdensity.----------------------------- 18
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Prefixes used in the Metric System
Prefix Abbreviation Meaning
Peta P 1015
Tera T 10 12
Giga G 10 9
Mega M 10 6
Kilo k 10 3
Deci d 10 -1
Centi c 10 -2
Milli m 10 -3
Micro 10 -6
Nano n 10 -9
Pico p 10 -12
Femto f 10 -15
Atto a 10 -18
Zepto z 10-21
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Base UnitsLength 1m = 3.28ftMass 1kg = 2.2 lbTemperature K = C + 273.15
F = ( 9/5) ( C)+32C = ( 5/9) ( F-32)
Derived Units
Volume V=(L)3
, V =A.L, L=(V)1/3,
where: V=volume;L=length;1m3 = 35.29ft 3
Density D=M/V, M=D.V, V=M/Dwhere: D=density;M=mass;V=volume
Specific Gravity SG=D subs /D refwhere: D subs =density of substance
Dref =density of reference
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------------------------------LEARNING OBJECTIVE 10
[10] Report data and resultsusing scientific notation andthe proper number ofsignificant figures.------------------------------LEARNING OBJECTIVE 11[11] Use dimensional analysis
in conversion of units.
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Exact numbers and Inexact numbers Exact numbers those whose value are known exactly.
1 kilometer = 1000 meter Exact number Inexact numbers those whose values have some
uncertainty.
mass of beaker Inexact number
Precision and Accuracy Precision is a measure of how closely individual
measurements agree with one another. Accuracy refers to how closely individual
measurements agree with the correct, or truevalue.
Uncertainty in Measurement
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Significant Figures
Rules to determine the number of significant figures:
[1] All nonzero digits are significant.
1634 four significant figure
[2] Zero between nonzero digits are alwayssignificant.
1005 kg four significant figures, 7.03 cm threesignificant figures
[3] Zeros at the beginning of a number are neversignificant; they merely indicate the position of thedecimal point.
0.02 one significant figure, 0.0026 two
significant figure[4] Zeros at the end of a number are significant ifthe number contains a decimal point.
0.0200 g three significant figures, 3.0 cm twosignificant figures
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If the leftmost digit removed is less than 5, the
preceding number is left unchanged.Rounding 9.241 to two significant figures, 9.2. If the leftmost digit removed is 5 or greater, the
preceding number is increase by 1.Rounding 5.235 to three significant figures, 5.24.
Significant Figures for addition and subtraction22.3 + 3.98 + 1.221 =
Significant Figures for multiplication and division2.22 x 1.1 =
Rounding off numbers
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The key to using dimensional analysis is the
correct use conversion factors to change oneunit into another.
87.3 ft to m 124.23 m 3 to ft 3
32.19 kg to lb
Convert the following:
Dimensional analysis
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