WEBSITE

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WEBSITE

• http//teacherweb.com/MI/BattleCreek/Gonzales/

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The Big Ideas of Physical Science

• Space and TimeEarth Science
• Matter and ChangeChemistryMatter has volume
  and mass, and usually takes the form of a solid,
  liquid, or gas.
• Forces and MotionPhysicsIf you push on
  something that is sitting still, it starts to
  move. If you push on something that is already
  moving, you will change its motion. Force work.
• EnergyAll SciencesEnergy exists in many forms.

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• Chemistry
• 1. the study of
• a. composition
• b. structure
• c. properties of matter
• d. changes or reactions

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• Three good reasons why you should study chemistry
  in high school.
• Learning chemistry will increase your
  understanding of science, and labs will give you
  an opportunity to follow methods to make
  conclusions for yourself. (and blow things up!)
• In today's world, it's useful to know chemistry.
  Chemicals (legal illegal) are all around you.
• Most important I LOVE CHEMISTRY and so will you!
  

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• The goal of all science is to expand knowledge.
• The use of knowledge to solve practical problems
  is technology.
• The goal of technology is to apply that
  knowledge.
• Think back to the 1700s, when there were no
  televisions, cars, antibiotics, or electricity.

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The telephone, was invented in 1876. Within two
years, the first telephone operators were
connecting calls by hand.
The first coin-operated phones appeared in 1889.
By 1927, it was possible to make a phone call
from New York to London.

• World War II saw the development of the first
  mobile phones, which paved the way for modern
  cellular phones. Today, you can communicate by
  telephone between almost any two places in the
  world.

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• Science is a system of knowledge and the methods
  you use to find that knowledge.
• What will you find when you flip over a rock?
• Science begins with curiosity and often ends with
  discovery.
• Curiosity provides questions but is seldom enough
  to achieve scientific results.
• Methods such as observing and measuring provide
  ways to find the answers.

You won't know until you look.  
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• Design a paper airplane. We will test them
  tomorrow to see which fly the best

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Observations information gathered by using the
5 senses
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A) 2 types
1. qualitative it describes physical
characteristics
no measurements
shapes
color
odor
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2. quantitative numerical measurements
how big,
tall,
little,
fast
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Extensive v Intensive

• Physical properties of matter are categorized as
  either Intensive or Extensive
• Intensive - Properties that do not depend on the
  amount of the matter present.
• Extensive - Properties that do depend on the
  amount of matter present.

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• Color
• Odor
• Luster - How shiny a substance is.
• Malleability - The ability of a substance to be
  beaten into thin sheets.

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• Ductility - The ability of a substance to be
  drawn into thin wires.
• Conductivity - The ability of a substance to
  allow the flow of energy or electricity.
• Hardness - How easily a substance can be
  scratched.
• Melting/Freezing Point - The temperature at which
  the solid and liquid phases of a substance are in
  equilibrium at atmospheric pressure.

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• Boiling Point - The temperature at which the
  vapor pressure of a liquid is equal to the
  pressure on the liquid (generally atmospheric
  pressure).
• Density - The mass of a substance divided by its
  volume

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• Mass - A measurement of the amount of matter in a
  object (grams).
• Weight - A measurement of the gravitational force
  of attraction of the earth acting on an object.
• Volume - A measurement of the amount of space a
  substance occupies. (liter)
• Length (meter)

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• Some experiments are impossible to observe (like
  the creation of the universe.) However,
  scientists can use the evidence of the universe
  around them to envision how this event occurred.

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• What happens to a candle when it is lit?
• What do you predict will happen when it is
  covered?
• Explain how you decided using chemical terms.

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• Scientists working in the field, or in a
  laboratory, like those in the picture below, are
  trained to use safe procedures when carrying out
  investigations. Laboratory work may involve
  flames or hot plates, electricity, chemicals, hot
  liquids, sharp instruments, and breakable
  glassware.

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• Use your senseswhich ones?to observe
  (qualitative quantitative) and the equipment
  provided at your lab bench (beakers, scales,
  stirring rods) to carryout your first lab.

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• An organized plan for gathering, organizing,
  and communicating information is called the
  scientific method. The steps to follow are
• Make observations
• Ask questions
• Develop a hypothesis
• Experiment to test your hypothesis
• Collect and organize data
• Draw conclusions
• Revise hypothesis if necessary
• Develop a theory

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• Make observation 5 senses
• Ask questionsIdentify the problem. (What are
  you being asked to do?)
• Develop a hypothesis a proposed answer to the ?
  based on observations
• Experiment to test your hypothesis
• controlled experiment-only change 1 variable
• Collect and organize data charts, tables,
  equations and graphs

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• Draw conclusions based on your data. Was your
  hypothesis supported?if it was, then do more
  trials to validate the results.
• Revise hypothesis if your data did not support
  your hypothesis make a new one and do the
  experiment over.
• Develop a theory a well-tested explanationwe
  will not develop real theories in this class.

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• A scientific law describes an observed pattern in
  nature without attempting to explain it. The
  explanation of such a pattern is provided by a
  scientific theory. For example, Newton's law of
  gravity describes how two objects attract each
  other by means of a gravitational force. This law
  has been verified over and over. However,
  scientists have yet to agree on a theory that
  explains how gravity works.

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• Scientific notation is a way of expressing a
  value as the product of a number between 1 and 10
  and a power of 10. Scientific notation makes very
  large or very small numbers easier to work with.
• Ex 300,000,000 is 3.0  108. (right of )
• Ex 0.00086 8.6  10-4. (left of )

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• When multiplying numbers in scientific notation,
  you multiply the numbers and add the exponents.
• (3.0 x 108 m/s) x (5.0 x 102 s) 15 x 1010 m
  1.5 x 1011m
• When dividing numbers in scientific notation, you
  divide the numbers and subtract the exponents.
• 1.5 x 1011m 1.5 x 1011-8 s 0.5 x 103 s
  5.0 x 102 s
• 3.0 x 108 m/s 3.0

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• 1. (7.6  10-4 m)  (1.5  107 m)
• 2. 0.00053  29 5.3 x 10-4 2.9 x 101
• 3. Calculate how far light travels in
  8.64  104 seconds. (Hint The speed of light is
  about 3.0  108 m/s.)
• 3.0  108 m x 8.64  104 seconds
• 1 sec
• 4. A rectangular parking lot has a length of
  1.1  103 meters and a width of 2.4  103 meters.
  What is the area of the parking lot?
• 1.1  103 m x 2.4  103 m

1.14 x 104 m2
5.3/2.9 x 10 (-4-1) 1.8 x 10-5
2.6 x 1013m
2.6 x 106 m2
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PREFIX SYMBOL MEANING MULT BY
giga G 109 (BILLION) 1,000,000,000
mega M 106 (MILLION) 1,000,000
kilo k 103 (THOUSAND) 1,000
deci d 10-1(TENTH) 0.1
centi c 10-2 (HUNDRETH) 0.01
milli m 10-3 (THOUSANDTH) 0.001
micro µ 10-6 (MILLIONTH) 0.000001
nano n 10-9 (BILLIONTH) 0.000000001
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• Kittens kilo
• Hate hecto
• Dogs deka
• Because base
• Dogs deci
• Cant centi
• Meow milli

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• kilo hecto deca deci
  centi milli
• 103 102 10 1 10-1 10-2
  10-3

base
1. Put a decimal point behind the number of your
measurement. 2. Find the column of your
measurement. 3. Then, find the column of the
metric measurement you want to convert to. 4.
Count how many spaces you moved and the direction
you went (left or right). 5. Move the decimal
point that many spaces (adding zeros if
necessary) in the same direction.
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• The easiest way to convert from one unit of
  measurement to another is to use conversion
  factors. A conversion factor is a ratio of
  equivalent measurements.
• Convert the height of Mount Everest, 8848 meters,
  into kilometers.
• The prefix kilo-, means 1 kilometer 1000 meters.
  This ratio gives you two possible conversion
  factors.

1km 1000m 1000m 1km
and
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• When you convert, you always start with your
  GIVEN. Since you are given 8848 meters you put
  that down first
• given conversion
  factor
• 8848 meters 1km 8848 km
• 1000 m 1000
• 8.848 km
• converting from meters to kilometers, the
  number should get smaller.

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• In Chemistry Physics you will use the
  conversion factors a lot.
• This is called the factor label method.
• Conversion factor 1 in 2.54 cm
• What is the length of a 12 in. object in cm? m?
  km?
• What is the length of a 3 in. object in cm? m?
  km?
• Convert your final answer (km) into scientific
  notation.

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• Convert
• 1.) 2.75 km to cm
• 2.) 455 mg to g
• 3.) 45 dm to m   
• 4.) 3.5 µg to g   
• 5.) 67 mm to m   
• 6.) 0.005 kg to µg

2.75 x 105 cm
275,000 cm
0.455 g
4.55 x 101 g
4.5 x 100 m
4.5 m
.0000035 g
3.5 x 10-6 g
6.7 x 10-2 m
0.067 m
5.0 x 106 µg
5,000,000 µg
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• Write the following in scientific notation
• 7.) 635.000
• 8.) 22,000
• 9.)  5201
• 10.)   81 
• 11.) 0.00073
• 12.) 0.0000023

6.35 x 102
2.2 x 104
5.201 x 103
8.1 x 101
7.3 x 10-4
2.3 x 10-6
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• Scientists use a set of measuring units called
  SI, or the International System of Units.

Seven metric base units make up the foundation of
SI.
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• Additional SI units, called derived units, are
  made from combinations of the 7 base units

QUANTITY UNIT SYMBOL
Area square meter m2
Volume cubic centimeter cm3
Density kg per cubic meter kg/ m3
Pressure pascal (kg/m?s2) Pa
Energy joule (kg ?m2/s2) J
Frequency hertz (1/s) Hz
Electric charge Coulomb (A?s) C
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• Specific combinations of SI base units yield
  derived units. Density is a derived unit. It is
  the ratio of an object's mass to its volume.

m dv
D m v
m
most times m mass (g) v volume (ml) units
of DENSITY g/ml or g/cm3
V m D
v
D
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DEMONSTRATION DIET COKE / COKE Balls
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• 1. A shiny, gold colored bar weighs 57.3 g and
  has a volume of 4.7 cm3. Is the bar made of pure
  gold? (D of Au 19.32g/cm3)
• D m/v
• 57.3 g
• 4.7 cm3
• No it is not made of gold. D ?
• 2. Oxygen will sink
• Nitrogen will float

12.19 g/cm3
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Color Mass d x v Volume m/v Density m/v Math
Orange
Purple
Green
White
black
0.5g/cm3
80 g
80/0.5
160cm3
29 cm3
0.759g/cm3
.759x29
22 g
gt1.0
12 cm3
1.083x12
13 g
1.083 g/cm3
gtG
40 51 are left
29 cm3
40 g
40/29
1.38 g/cm3
gt2.7
51/18
18 cm3
51 g
2.83 g/cm3
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• Orange
• D 0.5g/cm3 m 80g v 160cm3
• Purple
• D 0.75g/cm3 m 22g v 29cm3
• Green
• D 1.083g/cm3 m 13g v 12cm3
• White
• D 1.38g/cm3 m 40g v 29cm3
• Black
• D 2.83g/cm3 m 51g v 18cm3

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Limits of measurement

• Which would you want? Accuracy or precision?

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Accuracy vs. Precision

• Accuracy how close a measured value is to an
  accepted value
• 
  
• 2. Precision the reproducibility or reliability
  a gauge of how exact a measurement is. Can you
  do it again?

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• There are limits of measurementaccuracy v
  precision.

                                                                                                                                                                                            
Which is more accurate? Precise? Why?
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• The digital clock offers more precision.
  According to an analog clock, it might take you
  5 minutes to eat your breakfast. Using a digital
  clock, however, you might measure 5 minutes and
  15 seconds, or 5.25 minutes. The second
  measurement has more significant figures.

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• Accuracy
• Percent error compares your result to the known
  or standard value.
• EQUATION
• error MEASURED ? ACCEPTED
• ACCEPTED

X 100
Also in Table T of your reference table
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EXAMPLE

• In a laboratory experiment you find the melting
  point of cesium to be 30.1C. Calculate the
  error.
• melting point of cesium 28.4C
• 30.1C ? 28.4C
• 28.4C

5.98
X 100
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Percentage error problems

• Determine the percentage error if the
  experimental value is 1.24g and the
• accepted value is 1.3g.
• 1.24g ? 1.3g
• 1.3g

4.6
X 100
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• Significant figures are all the digits that are
  known in a measurement, plus the last digit that
  is estimated. The fewer the significant figures,
  the less precise the measurement is.

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• Uncertainty when reading any measurement, the
  last digit is really an estimate. Therefore that
  digit is uncertain.

between 5.2 5.3
5.2 are 2 known digits
last digit is an estimate it is uncertain
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Measuring with Significant Figures
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Which ruler would give you the most precise
length?
top
What is the length of this pencil?
How many sig figs?
27.64 cm
3 certain 1 uncertain
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Significant Figures are used when measuring is
done with scientific equipment they indicate
exactnessThey include certain and a final
uncertain or estimated digit. All are obtained
through measuringExamples11.12cm, 2.63 ml,
5.14 grams
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• A calculation result cannot be more precise than
  the numbers used to generate it!

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C. Rules for Determining Significant Figures in a
Measurement

• 1. All non zero digits are significant.
• Ex. 25 g 5.471
• 2. Zeros between non zero digits are
  significant.
• Ex. 309 40.06
• 3. Zeros to the right of a decimal point at the
  end of a number are significant.
• Ex. 2.20 2.00000

4 sf
2 sf
3 sf
4 sf
3sf
6sf
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If there is not a decimal point, the final 0s
are not significant Ex. 300
15600000 4. Zeros preceding the first non
zero digit in a number are not significant. (they
keep place) Ex. 0.005 0.000006

1 sf
3 sf
1 sf
1sf
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Zeros seem to be the problemTry these

• Example significance ? sf
• 570.
• 570
• 5.70
• 0.75
• 50.75
• 5.075

3
Y
N
2
3
Y
N
2
Y
4
4
Y
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Examples

• Value of significant figures
• a. 15.02 g
• b. 0.00035 cm3
• c. 0.032100 g
• d. 460.00L
• e. 500 m

4
2
5
5
1
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1. Addition and Subtraction

• The result can have no more digits to
• the right of the decimal point than the
  measurement with the least number of digits to
  the right of the decimal point
• Example 1
• Add 12.52 m, 349.0m and 8.24 m

Calc 369.76 sf 369.8
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• Example 2
• Four students were measuring out hydrochloric
  acid needed for an experiment. The first student
  measured 14.5 mL the second, 16.62mL the third
  17mL and the fourth 10.5 mL. How much
  hydrochloric acid did they have all together to
  the correct number of sig figs?

Calc 58.62 sf 59
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2. Multiplication and division

• When measurements are multiplied or divided,
  the number of significant figures in the result
  is equal to that of the measurement with the
  least number of significant figures.

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Example

• Calculation Calculator shows Answer
• 8.3 m x 1.22 m
• 5.3 x 10-2 m/0.255
• 4.29 x 3.24
• 1.36 x 5.2
• 8.47/4.2

2
3
10.126
10.
2
3
.21
2.0784 x 10-1
3
3
13.8996
13.9
3
2
7.1
7.072
3
2
2.0166
2.0
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Determine the number of significant figures in
the following numbers.

• 1. 0.02 6. 5,000.
• 2. 0.020 7. 6,051.00
• 3. 501 8. 0.0005
• 4. 501.0 9. 0.1020
• 5. 5,000 10. 10,001

1
4
2
6
3
1
4
4
1
5
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Perform the following operations expressing the
answer in the correct number of significant
figures.
3
4

• 1. 1.35 m x 2.467 m
• 2. 1,035 m2 42 m
• 3. 12.01 mL 35.2 mL 6 mL
• 4. 55.46 g 28.9 g
• 5. 0.021 cm x 3.2 cm x 100.1 cm

3.33 m2
4
2
25 m
2
1
0
53mL
2
1
26.6g
2
2
4
6.7cm3
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3
2
2

• 6. 0.15 cm 1.15 cm 2.051 cm
• 7. 150 L3 4 L
• 8. 505 kg 450.25 kg
• 9. 1.252 mm x 0.115 mm x 0.012 mm
• 10. 1.278 x 103 m2 1.4267 x 102 m

3.35 cm
1
2
40 L2
0
2
55 kg
4
3
2
.0017mm3
4
5
8.958 m
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Temperature

• scale freezing pt. boiling pt.
  main uses
• of water of water
  impt. info.
• Celsius 0 100 used in chem
• (C) and the world
• Fahrenheit 32 212 used in USA
• (F)
• Kelvin (K) 273 373 SI unit
• absolute zero

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• The Celsius scale used to be called the
  "centigrade" scale. Centigrade means "divided
  into 100 degrees." Starting with the freezing
  point of water 0 degrees Celsius and the boiling
  point at 100 degrees C. This scale is used for
  the metric system.
• Kelvins scale starts at 0 degrees Kelvin, which
  is called absolute temperature. The Kelvin Scale
  measures the coldest temperature there can be. He
  said there was no upper limit of how hot things
  can get, but he said there was a limit as to how
  cold things can get. Kelvin developed the idea of
  Absolute Zero. This is at minus 273.15 degrees
  Celsius (or -523.67 F)! At this temperature,
  everything, including the movement of electrons
  in an atom, stops completely.
• As far as scientists know, nothing in the
  universe can get that cold!

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You can make a thermometer with 2 fixed points.
They are 0C (freezing) and
100C (boiling)

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conversions

• F 9/5 C 32
• 98.6 F 37C 72 F 22.2 C
• C 5/9 ( F - 32)
• 25 C 77 F 30 C 89.6 F
• K C 273

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Examples
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• 10 C _____ K
• 15 C _____ K
• 25 C _____ K

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298
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Organizing Data

•   Scientists can organize their data by using
  data tables and graphs, to make it easier to spot
  patterns or trends in the data.
• Data Tables The simplest way to organize data is
  to present them in a table. The table relates two
  variablesan independent or manipulated variable
  is what changes and a dependent or responding
  variable is what is measured.

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• Name the dependent independent variable.
• D average annual precipitation (measure)
• I city (change)

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• Line Graphs are used for showing changes that
  occur in related variables.
• The independent (manipulated) variable is plotted
  on the horizontal axis, or x-axis.
• The dependent (responding) variable is plotted on
  the vertical axis, or y-axis (Y B dependent?)

                                    
Name the dependent independent variable from
the graph
D
I
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• The slope of this line is the ratio of a vertical
  change (risechange in Y) to the corresponding
  horizontal change (runchange in X). The formula
  
• rise change in Y
• run change in X

The slope of this line 5gm/5cm3 1gm/cm3
It also mass/volume or the Density
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• As this graph shows it is possible to draw
  a line even when the data is obviously not
  linear. Notice how far some of the points are
  from the line. Best fit lines are used to average
  out the errors of your experiment.

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• This graph (2 variables) demonstrates a direct
  proportion
• Directly proportional
• one increases the other increases or one
  decreases the other decreases
• This graph demonstrates an indirect or inverse
  proportionone increases the other decreases

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another.
                                        

• Bar Graphs are used to compare a set of
  measurements, amounts, or changes.

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substance.
                                     

• Circle Graphs are a divided circle that shows
  how a part substance relates to the whole.

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Type of graph Description Used for
Line represents variable Y vs. X (dep vs. ind) Showing how 1 responds to changes in the other
Bar represent scaled measurements Comparing 2 sets of similar data
Circle represents a fraction of the whole Shows how parts relate to the whole