Welcome to AP Chemistry!!
Mrs. Bechtum
blogs.waukeeschools.org/abechtum
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Science is collaboration.
“Alone we can do so little; together we can do so much. “
– Helen Keller
Science is the study of cosmic order… or how things fit together.
Problem-Solving Framework
“What am I trying to accomplish?”
“What strategies am I using?”
“How well am I using the strategies?”
“What else could I do?”
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Puzzle:
 Trying to put together the puzzle/ produce an image.
 Edges first… faces… shapes…
 Have I separated out the edge pieces correctly
 Would putting together the shapes or colors work better? Could I look at
the box as a model?
Course Syllabus
 Please Read Thoroughly
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If questions ….ASK!
Prerequisites
 Required Materials
 AP Requirements
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Monday, May 4th!
Grade Breakdown
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70% Exams and 30% Labs
**Please note that homework is not graded, but completion and
understanding of the homework will significantly impact your grade!**
Course Syllabus Cont…
 Safety and Lab
 Addressed in-depth later.
 No open-toed shoes or sandal permitted during labs. You will be
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required to make it up at a later date!
You have ONE WEEK to make up a missed lab.
Your lowest lab score will be dropped.
You will work in partners but will submit your own lab report
(data should be the same but questions, conclusions may vary)
Keep your lab notebook organized!! (College Lab Credit)
Lab Reports
 Format on blog
 Prelab
 Title-Names-Block-Date (lab completed)
 Purpose
 Procedure
 Data/Measurements
 Calculations
 Graphs (if applicable)
 Conclusion and Error Analysis
Course Syllabus Cont…
 Assessments
 Exams and quizzes are geared toward AP style
 50% Multiple Choice (no calculators)
 50% Free Response
 Exams will cover current AND previous material
 Term finals will be 75 questions (multiple choice)
 You have 2 weeks to make up a missed exam.
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I will facilitate review sessions on Saturdays in April! Keep
posted for more information!
 Academic Dishonesty – not tolerated (see syllabus for additional
information).
Classroom Expectations
 Follow standards set forth by WHS in Student Handbook.
 Respect ….Responsibility ……Trustworthiness
 …and Safety!
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Do not bring food or drink into class. This is a working lab.
 Wear appropriate clothing.
 Study the text before we discuss in class (course outline).
 Work through assigned problems and ASK QUESTIONS when they
arise!
 Come in for help when needed (I am here to SUPPORT you!)
 Collaborate with peers while learning! Setup study groups.
Classroom Expectations Cont…
 Communicate with instructor when extenuating circumstances
arise!
 You ARE capable of doing well in this class if you are willing to
put in the effort and open to new learning strategies!!
Course Outline
 **Subject to change**
 Readings done prior to class.
 Pre-labs done prior to lab.
 Keep up with assignments to be prepared for exams!
Guess Who?
 Objective: To communicate with the other students in the
class to determine whose card you have.
Take 3 minutes to…
 Answer the following questions on your note card. (DO NOT PUT
YOUR NAME ON THE CARD OR TALK WITH CLASSMATES!)
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A single concern of yours. Concerns can range from big concerns
(What to do about global warming) to small concerns (what to eat for
lunch).
Your favorite something, can be anything from color to food to movie.
TWO words describing your personality.
 Flip your card over and sit quietly when done.
Example
 When my son learns to open doors!
 Vancouver Island, BC
 Supportive
 Adventurous
MOVE IT!!
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The objective is to communicate with other students in the class to
determine whose card you have.
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To eliminate someone from the “game” you must find the person whose
card you have. (BE HONEST!)
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Once you eliminate someone you can claim any cards they have and
continue eliminating other students.
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Once eliminated take a seat.
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The person with the most cards after 5 minutes… WINS!!
(collect cards)
Today’s Learning Objectives
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I can identify the number of significant figures in a given measurement.
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I can perform calculations involving significant figures.
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I can differentiate between accuracy and precision.
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I can determine the density of solids and liquids and calculate volumes or
masses using the given density.
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I can convert between units of temperature: degrees Celsius and Kelvin.
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I can identify the characteristics of the states of matter: solids, liquids, and
gases.
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I can identify changes as being physical or chemical.
Chapter 1 – Chemical Foundations
 Measurement
 SI UNITS
 Precision and Accuracy
 Significant Figures
 Dimensional Analysis
 Temperature
 Density
 Classification of Matter
 Changes in Matter
SI Units
Practice
 The diameter of a helium atom is about 30 pm. Write this
length using exponential notation with units of m.
 (A: 3 x 10-11 m)
Precision and Accuracy
 Accuracy – the agreement of a particular value with a
true value.
 Precision – the degree of agreement among several
measurements of the same quantity.
 The degree of precision refers to the number of digits
that a measuring device permits one to measure. For
example, a balance which measures to the nearest
0.001g is more precise than one that measures to the
nearest 0.01g.
Error… Systematic or Random
 Random error means that a measurement has an
equal probability of being high or low.
 Systematic error occurs in the same direction
each time, it is either always high or always low.
Uncertainty
 Accurate, Precise,
Neither, or Both?
 Random Error,
Systematic Error, or
both?
Uncertainty
 Accurate, Precise,
Neither, or Both?
 Random Error,
Systematic Error, or
both?
Uncertainty
 Accurate, Precise,
Neither, or Both?
 Random Error,
Systematic Error, or
both?
Uncertainty
 Accurate, Precise,
Neither, or Both?
 Random Error,
Systematic Error, or
both?
Significant Figures
 The significant figures of a measurement are all of
the certain digits in a measurement, those that
represent actual marks on the measuring
instrument, and the first uncertain digit (estimated
number).
 The final reported result cannot have more certainty
than the least precise measurement.
What is the volume?
What is the length?
Significant Figures Cont…
 Rules for COUNTING Significant Figures (sig figs)
 1. Nonzero integers always count as sig figs.
 2. Zeros:
 Leading zeros precede all the nonzero digits and do not count as
significant figures. (0.0065 has 2 sig figs)
 Sandwiched zeros are zeros between nonzero numbers. These always
count as sig figs. (4.0185 has 5 sig figs)
 Trailing zeros are zeros at the right end of the number.
 If the number contains a decimal point the zeros ARE significant.
(2.50 * 102 has 3 sig figs)
 If the number does not contain a decimal point the zeros are NOT
significant. (250 has 2 sig figs)
 Exact numbers, which arise from counting or definitions never limit
the number of sig figs. (a dozen or Avogadro’s number)
Practice
Give the number of significant figures for each of the following results.
a.
A student’s extraction procedure on tea yield’s 0.0105 g
of caffeine.
(A: three)
b.
A chemist records a mass of 0.050080 g in an
analysis.
(A: five)
c.
In an experiment a span of time is determined to be
8.050 x 10-3 s.
(A: four)
Significant Figures Cont…
 Rules for Significant Figures in CALCULATIONS.
 For multiplication and division, the number of
significant figures in the result is the same as
the measurement with the fewest number of
significant figures in the calculation.
 For addition and subtraction, the result has the
same number of decimal places as the
measurement with the fewest number of
decimal places in the calculation.
Practice
Carry out the following mathematical operations, and give each result
with the proper units and the correct number of significant figures.
a.1.05 x 10-3 g ÷ 6.135 L (A: 1.71 x 10-4 g/L)
b.21 cg – 13.8 cg (A: 7 cg)
c.As part of a lab assignment to determine the value of the gas constant
(R), a student measures the number of moles (n), pressure (P),
volume (V), and temperature (T) for a sample of gas, where
PV = nRT
The following values were obtained: n = 1.00 mol; P = 2.560 atm;
T = 275.15 K; and V = 8.8 L. Calculate R to the correct number of
significant figures and use proper labels. (A: 0.082 atm·L/mol·K)
Dimensional Analysis
 Dimensional analysis is used to convert
from one unit to another.
 The method involves conversion factors to
cancel units until you have the proper (or
desired) unit.
Practice
Michael Oher (offensive tackle for the Baltimore Ravens and subject of
the movie The Blind Side) has a mass of 141,000 grams. What is his mass
in lbs? (1.00 kg = 2.20 lbs)
(A: 310. lbs)
You are the purchasing agent at a start-up biotechnology firm. If sucrose
costs $1.20 per pound, and a bottle contains 2.00 kg, how much would
you pay for a case of sucrose containing 12 bottles? (1 kg = 2.2 lbs)
(A: $63.36)
Temperature
 Conversion between Celsius and Kelvin
 TK = TC + 273.15
 Conversion between Celsius and Fahrenheit
 TC = (TF – 32°F) (5/9)
 TF = TC * (9/5) + 32°F
 Water freezes at 0 C or 273.15K or 32F
 Water boils at 100C or 373.15K or 212F
Practice
Liquid nitrogen, which is often used as a coolant for lowtemperature experiments, has a boiling point of 77 K. What is this
temperature on the Celsius scale?
 (A: -196°C)
Density
 Density is the mass of a substance per unit
volume.
 D=m/V
 Density of regular shaped objects can be
determined by calculating the volume such as
length * width* height for a cube.
 Density of an object can be determined via water
displacement method.
Practice
 The density of pure silver is 10.5 g/cm3 at 20ºC. If 5.25 g of pure
silver pellets is added to a graduated cylinder containing 11.2
mL of water, to what volume level will the water in the cylinder
rise?
Classification of Matter
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Matter exists in 3 states: solid, liquid, and gas. Properties of these 3 states
of matter are in table below.
State of Matter
Shape
Volume
Solid
Fixed
Fixed
Liquid
Not Definite
Fixed
Gas
Takes shape of
container (Not Fixed)
Takes volume of
container (Not Fixed)
Classification of Matter
 Heterogeneous (having visibly distinguishable parts)
 Homogeneous (having invisibly distinguishable parts)
 Solution
 Separation of mixtures is done by a physical change.
 Distillation
 Filtration
 Chromatography
 Paper Chromatography
Changes in Matter
 Physical Change
 Do NOT change the original composition of the
substance.
 Boiling, melting, tearing
 Intramolecular bonds are NOT broken
Changes in Matter
 Chemical Change
 DOES change the original composition of the
substance by breaking and making bonds between
atoms.
 A NEW substance is produced
 Evidence:
 Change in color or odor
 Production of gas or solid (precipitate)
 Absorption or release of energy (light or
temperature change)
Compounds and Elements
 A compound has constant composition
 A chemical change is required for a
compound to be broken up into elements.
 Elements are substances that cannot be
decomposed into simpler substances by
chemical OR physical means.
 (Figure 1.16 page 28)
Practice
Type of Matter
Air
(O2 , CO2 , N2 …)
Silver
(Ag)
Trail Mix
(M&Ms, Peanuts, Cereal…)
Hydrogen
(H2)
Sodium Bicarbonate
(NaHCO3)
Paint
(latex, pigment, etc…)
Classification
(Hetero, Homo Mixture,
Compound, or Element)
Reason for Classification
Practice
Change
Burning a Piece of Paper
Dissolving Sugar in Water
Autumn Leaves Changing
Color
An Ice/Cold Pack
Adding Food Coloring to
Water
Melting Cooper Metal
Classification
(Physical/Chemical Change)
Reason for Classification
For tomorrow…
 Complete the first 3 pages of the Review Packet
 Complete the following problems in the textbook:
 #39, 45, 49, 51, 53, 57, 59, 67, 69, 70, and 79
Textbooks and Lab Materials
 Grab a textbook (Zumdahl)
 Grab a Green Lab Book (DO NOT WRITE IN/ON!)
 Grab a Black Lab Binder (DO NOT WRITE IN/ON!)
 Please record the number to all three on class roster!
 Grab an AP Equation Sheet/Periodic Table
 The rest of today is for you to begin working on Chapter 1!
 ASK QUESTIONS…Work together!
Lab Safety
 Lab Safety Video
 Lab Safety Contract
 Lab Expectations
Have a WONDERFUL afternoon!!