Updated Aug 2006Created by C. Ippolito August 2006 Measurement Objectives: list three requirements...
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Transcript of Updated Aug 2006Created by C. Ippolito August 2006 Measurement Objectives: list three requirements...
Created by C. IppolitoAugust 2006
Updated Aug 2006
MeasurementObjectives:
list three requirements for making a measurementexpress measurements in the International System of Units (SI)list the seven basic SI unitsbe able to combine SI units to form SI derived unitsdetermine the amount of uncertainty in a measured quantitycorrectly apply the terms accuracy and precisiondetermine the number of significant digits for a given calculation or measurementcalculate the percent error of an experimental result
Updated Aug 2006 Created by C. IppolitoAugust 2006
Chemical Quantities
• Chemistry– science that studies the structure and
nature of matter– describes characteristics or properties
of matter– QualitativeQualitative
• characteristics that can be described using words
– QuantitativeQuantitative• characteristics that can be measured and
described using a standard numerical unit
Updated Aug 2006 Created by C. IppolitoAugust 2006
Measurements
• Requirements for Measuring1. know what is being measured
2. have a standard to compare measurement to
3. have a method of making comparison
• Measurements– comparison between quantity
measured and a standard unit
Updated Aug 2006 Created by C. IppolitoAugust 2006
International System of Units
• International agreement– determined a set of standard units to be
used in scientific measurements– based on older French system used in
Europe– a.k.a. metric system
• advantages– calculations easier with use of decimals– units change from larger to smaller and
from smaller to larger in multiples of ten
Updated Aug 2006 Created by C. IppolitoAugust 2006
SI Base Units
QuantityQuantity UnitUnit SymbolSymbol
length meter m
mass kilogram kg
time second s
amount of substance mole mol
temperature kelvin K
electric current ampere A
luminous intensity candela cd
Updated Aug 2006 Created by C. IppolitoAugust 2006
SI Prefixes
• used with base units to form new units that are greater than or less than the base unit
• units increase or decrease by some multiple of 10
Updated Aug 2006 Created by C. IppolitoAugust 2006
Prefixes for Greater Units
PrefixPrefix SymbolSymbol Multiply byMultiply by
exa- E 1 000 000 000 000 000 000
peta- P 1 000 000 000 000 000
tera- T 1 000 000 000 000
giga- G 1 000 000 000
mega- M 1 000 000
kilo- k 1 000
hecto- h 100
deca- da 10
Updated Aug 2006 Created by C. IppolitoAugust 2006
Prefixes for Lesser Units
PrefixPrefix SymbolSymbol Multiply byMultiply by
deci- d 0.1
centi- c 0.01
milli- m 0.001
micro- μ 0.000 001
nano- n 0.000 000 001
pico- p 0.000 000 000 001
femto- f 0.000 000 000 000 001
atto- a 0.000 000 000 000 000 001
Updated Aug 2006 Created by C. IppolitoAugust 2006
Simple Conversion
• conversion from one unit to another is as simple as moving the decimal point– move decimal point to leftleft to convert to larger units– move decimal point to rightright to convert to smaller units
1018 1015 1012 109 106 103 102 101 10-1 10-2 10-3 10-6 10-9 10-12 10-15 10-18
E P T G M k h da 1 d c m μ n p f a
Updated Aug 2006 Created by C. IppolitoAugust 2006
Derived vs Fundamental Units
• Fundamental UnitsFundamental Units– measure or describe basic qualities of any physical
object or phenomena• mass• length• time
• Derived Units– ones formed from new mathematical expressions
needed to quantify qualities of a physical object• area• density• volume• speed• concentration
Updated Aug 2006 Created by C. IppolitoAugust 2006
SI Derived Unit Quantities
Quantity Name Symbol Base Unit
area square meter m2 m2
volume cubic meter m3 m3
speed meter per second m/s m/s
density kilogram per cubic meter kg/m3 kg/m3
concentration mole per cubic meter mol/m3 mol/m3
force newton N m●kg/s2
pressure pascal Pa kg/m●s2
energy joule J m2●kg/s2
Updated Aug 2006 Created by C. IppolitoAugust 2006
Common Non SI unitsQuantity Name Symbol
time minute
hour
day
min
h
d
volume liter
milliliter
L
mL
density gram per milliliter g/mL
temperature degree Celsius oC
distance angstrom pressure millimeter of mercury
atmosphere
mm Hg
atm
energy calorie cal
Updated Aug 2006 Created by C. IppolitoAugust 2006
Uncertainty in Measurement• limited by the accuracy of the tools
being used to make them• some digits are certain and the final
digit is an estimate– 6.25 --- 6.2 is certain the .05 is estimate
Updated Aug 2006 Created by C. IppolitoAugust 2006
Accuracy Versus Precision
• AccuracyAccuracy– quality of the measuring instrument as compared with
the standard for that measurement– how close is the measurement to the actual standard
• PrecisionPrecision– the degree of exactness with which a measurement is
taken– reproducibility of measurements– uncertainty of measurement
Updated Aug 2006 Created by C. IppolitoAugust 2006
Significant Figures• all the digits that
are well known plus one estimated figure represent the significant figures in a measurement
• using a millimeter ruler (6.25) gives more significant digits (3) and greater precision that a centimeter (6.1) ruler with less significant digits (2)
Updated Aug 2006 Created by C. IppolitoAugust 2006
Use of Plus or Minus Notation
• Scientist’s use a ± notation to describe the degree of uncertainty– cm ruler
• 6.1 cm ± .5 cm or 61 mm ± .5 mm
– mm ruler• 6.25 cm ± .05 cm or 62.5 mm ± .05 mm
Updated Aug 2006 Created by C. IppolitoAugust 2006
Calculating and Significant Figures• Multiplication/ Division RuleMultiplication/ Division Rule
– express product or quotient to same number of significant figures as the measurement with the fewest significant figures
• i.e.
cmcm
cm
cm
3.10362.10
30.3
14.3
Updated Aug 2006 Created by C. IppolitoAugust 2006
Calculating and Significant Figures• Addition/ Subtraction RuleAddition/ Subtraction Rule
– round the sum or difference so that it has same number of significant figures as the measurement with the fewest significant figures
• i.e.
cmcm
cm
cm
cm
8.2076.20
12.6
3.9
34.5
Updated Aug 2006 Created by C. IppolitoAugust 2006
Percent Error
• Observed ValueObserved Value– value based on laboratory measurement
• True ValueTrue Value– most probable value based on generally
accepted references
• Absolute ErrorAbsolute Error– difference between observed and true value
• Percent ErrorPercent Error– (absolute error/true value) x 100
Updated Aug 2006 Created by C. IppolitoAugust 2006
Calculating Percent Error
• Boiling point of water– observed value 105.25oC– true value 100.0oC
%25.5
%1000.100
25.5
%1000.100
0.10025.105
errorpercent
xerrorpercent
xerrorpercent
Updated Aug 2006 Created by C. IppolitoAugust 2006
Scientific Notation
• makes working with large or small numbers is easier– all numbers expressed as the product
of a number between 1 and 10 and a whole number power of 10
• (M x 10n)
– i.e.• 2000 cm becomes 2 x 103 cm
Updated Aug 2006 Created by C. IppolitoAugust 2006
Calculations in Scientific Notation
• Multiplication– (1 x 10-2) (3 x 105) (2 x 1012) = ?
• multiply M values– (1 x 3 x 2 = 6)
• add exponents– (-2+5+12 = 15)
• (1 x 10-2) (3 x 105) (2 x 1012) = 6 x 1015
• Division– (6 x 105)(2 x 1012) = ?
• divide M values– (6 2 = 3)
• subtract denominator exponent from numerator exponents– (5-12 = -7)
• (6 x 105) (2 x 1012) = 3 x 10-7