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Chemistry- JIB Topic 1 Matter and Measurement
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Transcript of Chemistry- JIB Topic 1 Matter and Measurement
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Chemistry – science that deals with matter and the changes that matter undergoes
Macroscopic – all around us
Microscopic – air, molecules, etc
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Scientific Problem Solving3 Step Process
1. state problem and make observations (qualitative vs. quantitative)
2. formulate a possible solution3. perform experiments to test hypothesis
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Theory vs. LawTheory – gives a universally accepted
explanation of the problem
Law – state what general behavior is observed that occurs normally
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States of MatterAll matter has 2 characteristics
Has mass and occupies space
3 types: solid, liquid, gas
Solids – definite shape and volume; packed tightly together; vibrate gently around fixed positions
Liquids – no shape of own; fill container; definite volume; particles are free to move
Gases – no shape or definite volume; particles spread apart; filling all space in container
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Physical and Chemical Properties and Changes
Physical Property: color, odor, density, hardness, solubility, melting point, boiling point
Physical Change: chemical composition always remains the same. Ex. Phase changes (2 less known ones are sublimation (solid to gas) and deposition (gas to solid)
Chemical Property: reacts with acid, reacts with base, oxidation and reduction
Chemical Change: won’t go back to original substance. Ex. combustion
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E, C, MElement – pure substance that cannot be broken
down any further…..single substance from periodic table
Compound – pure substance that cannot be broken down by physical means; formed when elements bond together….have fixed composition
Mixture – varying composition and is made up of a number of pure substances.Homogeneous – uniform compositionHeterogeneous – varying composition
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MeasurementScientific Notation
The number of places the decimal point has moved determines the power of 10
Decimal moves left = positive powerDecimal moves right = negative power
42000 = 4.2 x 104
0.00012 = 1.2 x 10-4
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SI Units and prefixes
Base Quantity Unit Symbol
Mass Kilogram kg
Length Meter m
Time Second s
Amt. of Substance
Mole mol
Temperature Kelvin K
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Prefix Symbol Meaning
Giga G 109
Mega M 106
kilo k 103
deci d 10-1
centi c 10-2
milli m 10-3
micro μ 10-6
nano n 10-9
pico p 10-12
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3 scales for temperatureCelsiusKelvinFahrenheit
Celsius to Kelvin (°C + 273)Kelvin to celsius (K – 273)Celsius to fahrenheit (°C * 9/5) + 32Fahrenheit to celsius (°F – 32) * 5/9
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Derived UnitsAll other units can be derived from base
quantitiesExamples:
1. Volume: unit is length3
Common units are L or mL (how much is a cm3?)
1.00 L = 1000 mL = 1000 cm3 = 1.00 dm3
2. Density = mass/volume
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UncertaintyWhen reading the scale on a piece of lab
equipment, there is always a degree of uncertainty
Estimate must be made to record the final digitThis “uncertain” digit is recorded by using the
+/- scale
Rounding – don’t round until the end of a calculation
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Significant FiguresRemember the Atlantic and Pacific rule
In Calculations Multiplying and dividing: limit answer to least
number of sig figs used Adding and subtracting: limit answer to same
number of decimal places that appear in the original data with fewest number of decimal places
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Accuracy vs. Precision
Accuracy – relates to how close the measured value is to the actual value of the quantity
Precision – how close 2 or more measurements of the same quantity are to one another
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Percent ErrorData that is derived from experiments will
often differ from the accepted, published, actual value
Common way of expressing accuracy is: | Actual – Calculated | x 100
Actual