Chemistry is the study of matter and the changes in matter. Together with its counterpart, physics, it is at the foundation of all our scientific understanding. The importance of chemistry extends far beyond the classroom and laboratory into every aspect of our material world.
Chemists have always sought to understand the very nature of matter. We will learn how a chemist works so that we too can focus on the nature of matter. Chemists have made large contributions such as, the development of drugs to wipe out many diseases, fertilizers to help feed the world, and new sources of energy to help conserve our dwindling fuel. These developments have brought costs as well as benefits to society. One of our goals this year will be to try to make informed choices when confronted with similar dilemmas.
The key to success in chemistry is understanding the concepts, not memorization. Science by its very nature is a logical subject, where concepts build upon each other and are interrelated. Once you understand the concepts, it will be easier to assimilate the material.EXPECTATIONS AND GRADING POLICIES
The text is Introductory Chemistry: A Foundation by Zumdahl Houghton Miflin (2000) You may leave this book at home and only bring it into school when instructed. Other reference texts are available in the classroom for loan on a short-term basis.
A basic scientific calculator (under $20) is required for this course. It must have the following functions: exponential notation, powers, roots, and logarithms. Though most of the math is simple, this will permit you to get answers quickly when working with very large and very small numbers, which need to be expressed in scientific notation. It should be brought to every class. You will be expected to do a portion of each test without a calculator. Sharing of calculators will not be allowed during quizzes or tests.
Computers will be used extensively throughout the year. You will use interactive computer simulations to develop basic concepts under ideal conditions. You will use these programs to collect experimental data. You will then export the data to spreadsheet programs for record keeping and to graphing programs for data analysis. You will be expected to use the computers outside of regularly scheduled class time. All the necessary programs can be accessed from any computer throughout the school.
Each of the chemistry teachers will be available for weekly group labs. These will be announced and posted in the science lab. If your schedule conflicts with your own chemistry teacher's group lab, feel free to attend any of the other group labs. You must keep one of these periods free. If you have a scheduling conflict see your teacher ASAP to schedule an alternate time. You are always welcome to come to these labs, but if you are having difficulty you will be required to come. The weekly labs will focus on problem solving and will mainly cover last weeks work. Individual labs are always available to cover other work. A sign up sheet is located next to each chemistry teacher's desk.
In case of absence from class you are required to obtain class notes and schedule a lab with your teacher.
In case of absence from an experiment you are required to get class notes and make-up the experiment in a timely fashion during your free time. It is the teacher’s discretion which labs need to be made up.

Your quarter grade will be based on the following criteria:
1. Tests will count 40%. All full period tests will be announced at least one week in advance. Science test days are on Wednesdays and Thursdays.
2. Lab work , lab reports and projects count 40%. Your lab grade will be based on your pre-preparation, experimental techniques, and your write-ups or formal lab reports. You will be given a handout with a set of instructions for some of the labs. The data analysis and the questions can be answered directly on the handout. You will also be responsible for writing several formal lab reports during the semester. Directions for writing a formal lab report will be handed out in class later in the year. If you use outside sources to answer any questions in your labs, you must include a bibliography with the name and author of the text.
3. Homework, quizzes, demos and class participation count 20%. The assignment contains readings and problem sets from the text. We strongly recommend that you read and work through the self check problems Solutions to self check exercises and answers to even numbered problems and cumulative exercises are in the back of your book. Be sure to refer to these if you are experiencing difficulty!!!
Additional worksheets may also be assigned. Homework will be assessed on a regular basis.
You are encouraged to do problem solving at the blackboard and to participate in class discussions. However, if you are shy, see me during lab time instead.

***Your semester grade will be based on the same format with the addition of either the mid-year or final. If your grade on your mid-year/ final is higher than your test average for that semester, that grade will replace your tests (for that semester only). If your grade on your mid-year/final is lower it will count as two test grades and will be factored into your entire grade.
Introduction to Matter and Energy
THE NATURE OF MATTER
Making careful observations, both qualitative and quantitative is one of the most critical aspects of science. We may tell someone that it is "very cold" outside, but only if we state that it is -10° C will there be no confusion as to how cold it really is.
In the first experiment you will observe that matter can undergo both chemical and physical changes. For example, by gently heating a candle, you can melt the wax into a clear liquid. If you allow it to cool, the liquid will become solid once more. Melting has not changed the fundamental characteristics of the substance. This is an example of a physical change. If the candle is burned, and the candle and the air around it are allowed to cool, candle wax does not form. The wax and the oxygen in the air have combined to form new substances —mainly carbon dioxide and water. This is an example of a chemical change.
Pure substances that cannot be further decomposed by ordinary chemical changes are called elements. There are about ninety naturally occurring elements. The smallest unit of an element that retains the properties of that element is the atom. Atoms may be linked by electrostatic forces called chemical bonds. When atoms of differing elements are chemically bonded (e.g. H2O), then the substance is called a compound. There are two basic types of compounds: ionic and covalent (molecular). If elements and/or compounds are physically mixed together but are not chemically bonded, then the substance is called a mixture. The following chart summarizes some of these terms and concepts.

Chemical Physical
Methods Methods

The great French chemist, Antoine Lavoisier (1743-1794), is generally given much of the credit for introducing the scientific method to the study of matter. Lavoisier observed matter closely and was the first to make extensive measurements. From his observations, he made guesses or hypotheses, and then he designed experiments to test them. If the experiments did not support his hypotheses, he modified his ideas. This was a very refreshing change from the medieval alchemists, who spent their lifetimes trying to make reality conform to their ideas. After Lavoisier, students of matter began to make some rapid progress. The steps of the scientific method are outlined below, but you should be aware that the order may vary greatly.

Concepts:
The Scientific Method, hypothesis, theory, scientific law, chemical reactions, product, reactant, chemical vs. physical change, chemical vs. physical change, chemical vs physical property, particles: nature of matter, definition, properties; homogeneous vs. heterogeneous mixtures, separation methods.
Skills: Qualitative vs. quantitative observations, observations vs. inferences, factor label method, making detailed observations and recording data during experiments, writing lab reports.
Experiments/ Activities:
Identifying Physical & Chemical Changes
Separation of Mixtures-takehomeReading #1: 1.3-4 The Scientific method and a Mystifying problem p.4-9
3.1-2 Matter, physical and Chemical changes p.59-64
HW #1 Questions and problems p.12 #7, 10, 11
p.78 # 2-7, p. 79 # 18
Reading #2 3.3-5 Elements, compounds, pure substances and mixtures and separation of mixtures p.64-9
HW #2 Questions and problems p 79 # 20, 22-25, 27-29
p. 80 # 33-36, P. 81 # 64
Experiment – Separation of mixture at home – write a careful plan and then a summary of results
MEASUREMENTS
Measurements are made to quantify observations. Scientists use the Metric System which is based on the SI System of Measurement. The metric system is a decimal system which makes it easy to learn and it makes the conversion between units fairly simple.
Chemistry often demands that we use extremely large or extremely small numbers. We use scientific notation to represent very large and small numbers to prevent us from making careless errors when transcribing such numbers. For example it is much easier to write 6.02 x 1023 than 602,000,000,000,000,000,000,000. Similarly it is easier to write a small number such as 9.11 x 10-28 than .000000000000000000000000000911.
Concepts: Measurements, accuracy vs. precision, significant figures and mathematical calculations, scientific notation, use of calculator, matter, volume, mass vs weight, conversion factors, density
Skills: Meaurement, use and recognition of significant figures, scientific notation, use of a calculator factor
Experiments/Activities
Use of instruments
Density of a metal
Density of liquidsReading #3 2.1-4 Scientific notation and Units, Measurements, and uncertainty in measurement p.16-25
Questions and problems p.49-51 # 8a-d, 10a-d, 18, p.55 #119
Reading #4 2.5- Significant figures p. 25-28 , Density 2.8 p.44-48
HW#4 Questions and problems p.51-2 # 26, 37, 42, 44a,c, 48, 54, 56d
p. 53-7 # 83, 87, 89, 94, 95, 98, 114, 154, 157ENERGY

Energy is the capacity to do work. It cannot be created or destroyed.
Heat is a form of energy. It flows spontaneously from a hot to a cold system until their temperatures have equalized. Heat is the sum total of the kinetic energy of the particles of the system including its surroundings. Specific heat is a property of matter. It is defined as the amount of energy required to raise the temperature of 1 gram of a substance 1 degree Celsius. Temperature is a measure of the average kinetic energy of the particles of the substance. It is a measure of how hot or cold a substance is relative to another substance. The three common temperature scales are Fahrenheit, Celsius and Kelvin. In the lab we work in degrees Celsius.Concepts: Energy: and energy changes, Chemical energy, kinetic vs. potential energy, Law of Conservation of Energy, heat vs. temperature, specific heat,
Skills: Measurement, factor label method for making conversions, writing a lab report
Experiments/ Activities:
Specific heat of a metal

Reading #5 2.6 Conversions using factor label method p.30-35 – to be read if you have difficulty with the problems. The problems should be solved using the method shown in class
HW #5 Questions and problems p.52-7 # 60cd, 64, 66ab, 147abdef, 149, 92abc
Reading # 6 3.6 Energy and Energy changes p. 69-77
HW #6 Questions and problems p. 80 # 38, 40, 41, 45a, 50cd, 52, 54