Mrs. Bechtum blogs.waukeeschools.org/abechtum

Welcome to AP Chemistry!!

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?”

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 If questions ….ASK!

Prerequisites

Required Materials

AP Requirements Monday, May 4th!

Grade Breakdown 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

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.

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!

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!)

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!!

The objective is to communicate with other students in the class to determine whose card you have.

To eliminate someone from the “game” you must find the person whose card you have. (BE HONEST!)

Once you eliminate someone you can claim any cards they have and continue eliminating other students.

Once eliminated take a seat. The person with the most cards after 5 minutes… WINS!!

(collect cards)

Today’s Learning Objectives

I can identify the number of significant figures in a given measurement.

I can perform calculations involving significant figures.

I can differentiate between accuracy and precision.

I can determine the density of solids and liquids and calculate volumes or masses using the given density.

I can convert between units of temperature: degrees Celsius and Kelvin.

I can identify the characteristics of the states of matter: solids, liquids, and gases.

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 low-temperature 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/VDensity 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

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 compositionA 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)

PracticeType of Matter Classification

(Hetero, Homo Mixture, Compound, or Element)

Reason for Classification

Air(O2 , CO2 , N2 …)

Silver(Ag)

Trail Mix(M&Ms, Peanuts, Cereal…)

Hydrogen(H2)

Sodium Bicarbonate(NaHCO3)

Paint(latex, pigment, etc…)

Practice

Change Classification(Physical/Chemical Change)

Reason for Classification

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

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!!