Transcript CHAPTER 2

CHAPTER 2
Measurements and Calculations
Scientific Method
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System
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Specific portion of matter that has been
selected for study
Scientific Method
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Logical approach to solve a problem
Scientific Method
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Steps
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Observing and collecting data
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Use of senses
Quantitative data – numerical
Qualitative data - descriptive
Generalization – statements
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Organizing – Graphs, tables, statistics
Hypothesis – testable statement
Law – statement that DESCRIBES facts
Scientific Method
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Steps
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Theorizing
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Statements that EXPLAINS facts
Can never be proven!!
Testing
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Experimentation
Units of Measurement
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Unit of Measurement
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A physical quantity of a defined size
lb, in, ft, g, cm, km
SI
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International System of Units (metric
system)
Adopted in 1960, originated in France
SI
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SI base units – standard of measure
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Length – meter (m)
Mass – gram (g)
Time – second (s)
Temperature – Kelvin (K)
SI Prefixes
Prefix
Symbol
Example
Exponential
Factor
Factor
Tera
T
Terameter
1012
1000000000000
Giga
G
Gigameter
109
1000000000
Mega
M
Megameter
106
1000000
Kilo
K or k
Kilometer
103
1000
Hecto
H
Hectometer
102
100
Deca
D
Decameter
101
10
----
----
meter
100
----
Deci
d
Decimeter
10-1
0.1
Centi
c
Centimeter
10-2
0.01
Milli
m
Millimeter
10-3
0.001
Micro
µ
Micrometer
10-6
0.000001
Nano
n
Nanometer
10-9
0.000000001
Pico
p
Picometer
10-12
0.000000000001
Know the ones in BOLD above!!!
SI Prefixes
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Number Line – MEMORIZE!!
KHD
Examples:
d c m _ _ µ_ _ n
Derived SI Units
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Derived Unit – obtained from combining
base units
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Area
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Volume
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L * w * h ; m3
Speed
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L * w ; m2
Length/time ; m/s
Density
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Mass/volume ; g/mL or g/cm3
Conversion Factors and
Factor-Label Method
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Factor-Label Method – problem
solving method using algebra
Examples:
Using Scientific
Measurements
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Accuracy
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Precision
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Closeness of a measurement to the true or
accepted value
Agreement among the values
Percent Error
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Accepted value – Experimental Value x 100%
Accepted Value
http://honolulu.hawaii.edu/distance/sci122/SciLab/L5/accprec.html
Significant Figures
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Sig Figs – all certain digits plus one
uncertain digit
How many sig figs in a number?
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Table 2-5 page 47
Sig Figs
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Rules
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All non-zero numbers ARE significant
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Sandwich zeros ARE significant
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306 = 3 SF
Leading zeros ARE NOT significant
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3.456 = 4 SF
.000239 = 3 SF
Trailing zeros:
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To the left – ARE NOT significant unless a special sign
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To the right – ARE significant
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300 = 1 SF
300. = 3 SF
0.02300 = 4 SF
Scientific Notation
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All digits in the number portion ARE significant
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2.31 x 103 = 3 SF
Significant Figures
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Using Sig Figs in Math Operations
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Multiply/Divide
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Answer must have number of sig figs as least precise
number
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2.3 (2 SF) x 5.67 (3 SF) = 13 (2 SF)
16.00 (4 SF) / 8.0 (2 SF) = 2.0 (2 SF)
Add/Subtract
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Answer must have number of “columns” as least
precise number
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1.03 (hundredths)
+ 3 (ones)
4
Significant Figures
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Rounding off a number – Table 2-6 page 48
Rules –
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Decide where the number will be “cut”
Look at number to the right:
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If it is a 5 or greater, increase the number by one
If it is less than 5, leave number as is
Significant Figures
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Examples:
Scientific Notation
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Used to represent very big or very
small numbers
Generic form:
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M x 10N
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M must be greater than 1 and less than 10
If positive (+) N value = a “big” number
If negative (–) N value = a “small” number
Scientific Notation
Example:
4.21 x 102
 4.21 = number part in standard form
(one digit to left of decimal point)
 102 = tells where decimal is
 2 = exponent
Scientific Notation
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Converting TO Scientific Notation
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Count the number of spaces needed to
get into PROPER form.
This becomes the exponent.
Moving the decimal point left means N is
+. Moving the decimal point right means
N is -.
Examples:
Scientific Notation
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Converting OUT OF scientific notation:
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Move the decimal the number of spaces
indicated by the exponent (the number),
the correct direction, also indicated by the
exponent (the sign)
Examples:
Scientific Notation
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Calculator
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Type the “M”
Hit the EE or EXP button
Type the “N”
Scientific Notation
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Math and scientific notation
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Add/Subtract
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Multiply
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Exponents MUST be the same!!
Add M values and exponent stays the same
Multiply M values and add exponents
Divide
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Divide M values and subtract exponents
Heat and Temperature
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Temperature
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Measure of the AVERAGE kinetic energy
of the particles in a sample
How hot or cold something is
Heat
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SUM TOTAL of the kinetic energy of the
particles in a sample
More particles = more heat
Heat and Temperature
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Thermometer
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Device used to measure temperature
Hg or alcohol
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Liquid EXPANDS or CONTRACTS
Temp scales
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°C – Celsius, 0°C, 100°C
°F – Fahrenheit, 32°F, 212°F
Heat and Temperature
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Kelvin
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Freezing point of water = 273 K
Boiling point of water = 373 K
K = °C + 273.15
°C = K – 273.15
Examples:
Heat and Temperature
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Units of Heat
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Joule (J) – SI unit
Calorie (cal) – older, not SI
1 cal = 4.184 J
Problem Solving
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Analyze
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Plan
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Develop a plan to solve
Compute
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Read problem carefully and analyze info
Substitute data and conversion factors into plan
and solve
Evaluate
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Examine answers – is it reasonable? Does it
make sense?
Proportionality
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Variable
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Directly proportional
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Quantity that can change
One goes up, other goes up; y=kx
Graph –
Inversely proportional
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One goes up, other goes down; y=k/x
Graph –