Table of Contents

General Classroom Rules & Procedures.......................................page 2Standard Practices in the Laboratory

Safety Practices........................................................................page 3Housekeeping Practices ...........................................................page 4

Flinn Safety Contract Page 1……………………………………...page 5Flinn Safety Contract Page 2……………………………………...page 6Guidelines for Writing Lab Reports.............................................page 7Common Lab Equipment ............................................................pages 8-9Guidelines for Measuring.............................................................page 10Measuring Worksheet..................................................................page 11Guidelines for Graphing...............................................................page 121st Semester Text References and Key Terms...............................pages 13-162nd Semester Text references and Key Terms...............................pages 16-19Conversion Factors, Gas Laws, Abbreviations.............................page 20Vapor Pressure Table, Rules of Solubility, Activity Series...........page 21Periodic Table of the Elements.....................................................page 221st Semester Calendar...................................................................pages 23-262nd Semester Calendar..................................................................pages 27-30Course Outline ………………………………………………….. page 31

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GENERAL CLASSROOM RULES & PROCEDURES

Classroom Rules1. All school policies will be strictly enforced (including the makeup policies for absences).2. All safety policies in the safety contract, workbooks, and this booklet will be strictly enforced;

Failure to follow safety procedures will result in disciplinary action; Severe violations will result in the permanent removal from class.

3. Unnecessary pulling of the safety shower or eyewash fountain will result in a suspension.4. Students not wearing appropriate clothing for lab (goggles, long pants/skirt, closed-toed shoes)

will lose points on the lab; The teacher reserves the right to prohibit a student from participating in the lab if they do not wear appropriate clothing.

Makeup and Late Work5. If an absence is excused, a student is allowed two extra days for each day missed; No credit is

allowed for work for an unexcused absence.6. You must see your teacher prior to a school related absence or field trip to make arrangements

for makeup; Failure to do so will result in a zero for the assignment.7. Late vocabulary words, practice problems, and/or practice tests for a quiz or test will be accepted

one day late for half credit; Late labs will be accepted with a penalty of 20% per day.Cheating

8. Any student caught communicating with others or using unauthorized materials on a quiz or test will get a zero for that quiz or test with no retake allowed; A major referral will be issued for gross insubordination/defiance and a phone call will be made home.

9. Although working together with a lab partner(s) on labs is encouraged, blatantly copying labs is also not allowed; Doing so will result in a zero for the lab.

Calculators10. Students are strongly encouraged to buy a SCIENTIFIC CALCULATOR for this course.

Scientific calculators are usually very inexpensive but can do exponents (Look for a key that says “EXP” or “EE”.). Because of issues related to cheating, NO GRAPHING CALCULATORS WILL BE PERMITTED ON TESTS (Sorry!)! Because of budgetary constraints, no calculators will be provided (Again, sorry!).

Grading Scale11. The grading scale is as follows: A = 90-100%

B = 80-89%C = 70-79%D = 60-69%F = 59% and lower

Final Exam12. The final exam will count as 15% of the overall grade; To study for the final exam, students

should review their workbook AND the textbook pages and key concept words listed in this booklet.

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STANDARD PRACTICES IN THE LABORATORYThe science laboratory is normally a safe environment, but it is not free of physical and chemical hazards.

Injury can result from broken glassware, fire, electric shock, and exposure to chemicals that can stain, cause skin irritation, spatter, and/or produce noxious odors. Standard safety practices have been developed to minimize risks in the science laboratory environment. By learning and following these practices, you will protect yourself and your classmates from potential injury.

SAFETY PRACTICES

1. PROTECT YOUR EYES. The State of Illinois School Code requires that goggles be worn when heating chemicals that are caustic or explosive. Safety goggles are provided in each chemistry laboratory. Only goggles provide maximum protection from spattering, splashes, and projectiles.

2. WEAR APPROPRIATE PROTECTIVE CLOTHING. When working in the laboratory, the following clothing items are not appropriate: sandals, cloth shoes, shorts, short skirts, and loose clothing. Closed, leather shoes and long pants or a long skirt provide maximum protection from broken glass, burns, and chemical spills. It is also recommended that watches, bracelets, rings, and contacts be removed and safely stored since they can trap chemicals against the skin and/or eyes and aggravate an injury. Tie back loose hair to avoid burning it, dipping it in chemicals, or getting it caught in laboratory equipment. Aprons are available in all chemistry rooms for further protection.

3. NEVER EAT, CHEW GUM, DRINK, OR APPLY COSMETICS IN THE LABORATORY. You may accidentally ingest and/or contaminate skin or eyes with harmful chemicals.

4. WHEN WORKING WITH CHEMICALS,NEVER: taste them, smell them directly, pipette them by mouth, or remove them from the laboratory.DO: flush the area with water if you spill any chemical on your skin or eyes; wash your hands

with soap and water before touching your eyes, nose, or mouth AND when leaving the laboratory.

5. KNOW THE LOCATION AND OPERATION OF ALL SAFETY EQUIPMENT. Every laboratory has an eyewash fountain, fire blanket, fire extinguisher, first aid kit, fume hood, safety shower, telephone, and two exits. Report any accidents, spills, or unsafe equipment to your teacher immediately.

6. KNOW THE HAZARDS OF MATERIALS BEING USED. Metal and glass look the same whether hot or cold. Allow for adequate time for cooling. If in doubt, use the correct tongs or mitts. Many chemicals differ in only one letter but have quite different chemical properties and reactions (ex. copper (II) sulfate and copper (II) sulfite). A Material Safety Data Sheet (MSDS) Index is maintained for all chemicals used.

7. PEFORM AUTHORIZED EXPERIMENTS ONLY. Read all labels carefully to make sure you are using the correct chemical. Note all safety alerts provided with each experiment. Follow all experimental procedures exactly. If you want additional time or experience in the laboratory, you must consult your teacher. For safety purposes, there must be a teacher in the laboratory if an experiment is being conducted.

8. MINIMIZE ACCIDENTS. The chemistry laboratory is a place for serious work. Inappropriate and careless behavior will result in removal from the laboratory and disciplinary action. Return all chemicals and equipment to the proper storage area. Breakage and chemical spills must be cleaned up immediately. Notify your teacher immediately in the event of any accident, injury, breakage, fire and/or large spills.

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HOUSEKEEPING PRACTICES

1. AVOID WASTE. Regardless of grade (technical, reagent, assay), chemicals used in the chemistry laboratory are pure. The cost of individual chemicals depends on production, quality, and quantity desired. Whenever you measure a chemical out of the stock container, carefully tap out the required amount; try not to waste. Likewise, distilled water is produced at the expense of time and electrical energy. Please be conservative when using distilled water to clean glassware.

2. AVOID UNKNOWN CONTAMINANTS. Lab jars should be taken to the weighing tables when measuring out a specified mass. Use care with the lids or stoppers of lab jars. Laying them down on the counter or switching them is a source of contamination. Make sure all glassware is clean. If you have any doubts, wash it with soap, rinse with tap water, and do a final rinse with a small amount of distilled water. Tap out solids directly from the lab jar into the desired container (if possible). Never insert a spatula, dropper, or pipette into a lab jar (unless given permission by your teacher). Pour a small amount of a liquid chemical into a small beaker and dispense it from there. Never return an unused chemical to a lab jar. You must assume that the chemical is contaminated. It is to be disposed of in the appropriate manner - solid chemical wastes are to be put in the solid chemical waste crocks or dropped into the trash can (if given by your teacher); Liquid chemical waste is to be poured into a designated container or flushed down the drain with an ample amount of water (if given permission by your teacher); Extinguished matches, paper towels, and other garbage should be placed in trash cans, not in the sinks or solid waste crocks. Use only distilled water when adding water to a chemical. Tap water contains contaminants that will alter the results of many experiments.

3. CORRECT WEIGHING PROCEDURE. The digital balances used are accurate to + 0.01 g. When using the balances, always make sure the window reads “0.00 g” before you start the weighing process. Pressing the TARE (ZERO) pad will return the balance to zero. Never put a chemical directly on the balance pan. If a chemical is to be added to some glass container, you may place the glassware on the balance pan and then press the TARE (ZERO) button. Now you can add your chemical to the glassware until the window shows the desired mass. Note that there is a delay before the measured amount is indicated, so add the chemical slowly to get the exact amount. The maximum load for the digital balance is 200.00 g. Make sure to clean up any spills on the balances.

4. CORRECT WASTE DISPOSAL. The custodial staff removes all non-chemical waste from two designated containers: the broken glass container, which contains all broken, chipped, or cracked glassware; AND the trash can, which contains waste paper, paper towels, and extinguished matches. Your teacher removes solid chemical waste from the solid chemical waste crocks and liquids from the designated containers.

5. EQUIPMENT SET UP. Most labs will already be set up for you; Please make sure you leave the lab equipment and chemicals as you found them (organized, clean, and dry) and that you close all lids and stoppers on chemicals. If a piece of equipment is not already set out for you, you will most likely find it either in the tall end cabinets of each lab bench or in the common property area along the wall; Set up your equipment away from the front edge of the bench so it does not get knocked onto the floor; Chemicals and other supplies for particular labs can be found in the labeled drawers on the back lab islands.

6. LABELS. Read the entire label on all chemical containers to make sure you have the correct substance and concentration. Inform your teacher immediately if a label falls off of a chemical container or is missing a label (and do not use it until it is fixed). When leaving an experiment overnight in the “Experiments in Progress” cabinet, be sure you label with your name, period number, and the date and place it on the correct shelf for your period.

7. CLEAN WORK AREA. Every chemistry student is entitled to a clean work area. When you are finished working, make sure your work area is breakage and spill-free. Return all equipment to its proper storage place. Make sure the gas and water outlets are shut off.

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Flinn Safety Contract Page #1

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Flinn Safety Contract Page #2

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GUIDELINES FOR WRITING LAB REPORTS

It is required that you buy a graph-paper science notebook for recording and reporting laboratory findings. Every lab write-up must be checked off and/or initialed by your teacher prior to beginning a lab. The following format should be used.

Date Your nameLab partner’s name(s)

Title of the Experiment

Purpose: Copy the purpose from the workbook pages.

Pre-lab Some labs will require you to look up definitions to key terms using your textbook. Exercises: Others will ask you to answer questions to stimulate background information.

Procedure: Use a series of pictures, summarize in words, or do both to describe what you will do in the lab (DO NOT just copy the entire procedure word for word out of your workbook!).

Data: Write down all observations you make during the course of the experiment. Collected data should be organized into charts or tables whenever possible. Make sure that all measurements include the correct number of significant figures and units.

Analysis: Complete the list, calculations, analysis, graphs, and/or questions as directed. Make sure that all analysis calculations include the correct number of significant figures and units. Consult the Guidelines for Graphing for all graphs. Answer the analysis questions in complete sentences. Include/restate the analysis question as part of the answer. Do not use pronouns.

Questions: Answer the questions in complete sentences. Include/restate the question as part of the answer. Do not use pronouns.

Conclusion: Answer each part of the purpose. Do not use pronouns (Using them implies that your results cannot be repeated. If ten people are following the same directions, all ten should have similar results.). This section answers each part of the purpose, giving support from lab data, and includes at least two possible sources of error (Note: Sources of error should be experimental or technological design flaws or limitations with solutions whenever possible. “My lab partner didn’t read or calculate right are NOT acceptable sources of error.”).

Mind Prober:Answer the question(s) as they relate to the investigation you just completed. Use complete sentences. Do not use pronouns.

All lab reports are to be neatly hand-written in blue or black non-erasable ink (or neatly typed and spell checked if permitted by your instructor). Make all lab reports your best work. If you would be comfortable to have it on display and seen by others, then it’s good enough to be submitted for grading.

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Lab Equipment#1

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Lab Equipment #2

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GUIDELINES FOR MEASURING

When using any non-electronic instrument designed for measuring, the reported measurement must include one number (digit) beyond what you can read directly when reading the printed measurement scale on the instrument. Another way of saying this is, when measuring, read any instrument to one half of the smallest scale division.

Meter Stick/Centimeter RulerA meter stick or centimeter ruler has a printed scale showing whole numbers of centimeters (cm) and small lines showing tenths of centimeters (or millimeters (mm)). Therefore, when reading a meter stick or centimeter ruler using significant figures, one would write the number of whole centimeters and tenths of centimeters using the printed scale and then estimate the number of hundredths of centimeters to the nearest 5 (i.e. If the measured object ended on a scale line, the measurement would end in a “0”; if the measured object ended between two scale lines, the measurement would end in a “5”.). As a result, all measurements with a meter stick or centimeter ruler should always be given to two places past the decimal (ex. 7.80 cm or 60.95 cm are possible measurements with a meter stick. 4 cm, 5.0 cm, or 84.200 cm are not!).

Graduated CylinderSince the ten milliliter (mL) graduated cylinder has identical markings (except that that they are vertical instead of horizontal) to a meter stick or centimeter ruler, a ten milliliter graduated cylinder should also be read to two places past the decimal. A 50 or 100 milliliter graduated cylinder has scale markings to the nearest one milliliter, so, unlike the meter stick or 10 mL graduated cylinder, it should be read to one place past the decimal.

Special Note: Make sure to always read the center of the meniscus (i.e. curved line) at eye level when reading any graduated cylinder.

Electronic BalancesOur electronic balances will automatically give two places past the decimal.

Special Note: Make sure balance is clean and tared (zeroed) before and after use. Also, make sure objects placed on the balance are cool and in an appropriate container for weighing (i.e. beaker, graduated cylinder, weighing boat etc.). Finally, if the balance readout does not “settle” fairly quickly, check for drafts from fans or open windows and doors.

Other Measuring Instruments (i.e. thermometers, burettes, pipettes etc.)Use the general rule above and see your teacher for more specific instructions.

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Measuring and Calculations Worksheet

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GUIDELINES FOR GRAPHING

Line graphs are often used in experiments to provide a visual representation of the relationship between two variables. Following are guidelines, which are to be used when making graphs in this course. If the line has a positive slope, the relationship is described as direct. If the line has a negative slope, the relationship is described as indirect or inverse.

1. Use black or blue non-erasable ink (some labs may be typed … see your teacher for more details).

2. Be neat.

3. The data on the graphs must “fill the page”.

4. The origin of the axes must begin at zero.

5. The independent variable (data controlled by the experimenter) is plotted on the horizontal axis; the dependent variable (the resulting data) is plotted on the vertical axis.

6. Divide the number the divisions of each axis in such a way that the data is spread over the majority of the axis and the intervals on the same axis are equal in size.

7. Label each axis by printing the name of each variable, followed by the unit of each variable in parentheses; make sure to spell out the name and unit completely. Do not abbreviate (ex., Time (minutes)).

8. Plot the points and circle them. The circles, sometimes called error circles, both highlight the location of the data point and account for uncertainty.

9. Draw a smooth, solid line or curve between the data points. Do not “connect the dots”. This line should reflect the average trend of the data. It is possible that not all points will fall on the line.

10. Extrapolate beyond the data points with a broken (dashed) line. The extrapolated line should continue the trend of the line established by the data.

11. Place the graph title box in the largest empty area on the graph. The title should describe the information on the graph and is often the dependent variable versus the independent variable.

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1st Semester Chemistry:QUANTITATIVE AND QUALITATIVE SKILLS

E-1 Metric System & Conversions (Test)Illinois State Learning Standards: 13B-13.11.09.Textbook pages: 17-21, 30-33, 38-44Key Concept Words: metric system, SI base unit, derived unit, length, volume, mass, weight, meter, liter, gram, kilo-, hecto-, deka-, deci-, centi-, milli-, scientific notation, and conversion factor.

E-2 Significant Figures & Measurement (Test)Illinois State Learning Standards: 13A-13.11.05.Textbook pages: 22-29Key Concept Words: significant figures, precision, accuracy, measurement, meter stick, graduated cylinder, electronic balance, significant digit, Atlantic/Pacific Rule, addition/subtraction rule, multiplication/division rule, rounding, hundreds place, tens place, ones place, tenths place, and hundredths place.

E-3 Types of Observations (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 13C-13.11.01,04-05,08-09.Textbook pages: 8-9, 74-79, 65-71, 501, 505, 562-563 246, 472-473, 280Key Concept Words: beaker, element, compound, pure substance, mixture, matter, solid, liquid, gas, physical property, chemical property, physical change, chemical change, solution, aqueous solution, dissolution, precipitation, precipitate, hydrate, reactant, product, qualitative observation, quantitative observation, and indicator of a chemical change.

E-4A Using the Bunsen Burner (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 13C-13.11.01,04-05, 08-09.Textbook pages: NAKey Concept Words: Bunsen Burner, air adjustment, barrel, base, flame, gas adjustment, hose, beaker tongs, and methyl mercaptain.

E-4B Using the Bunsen Burner (Lab Practical)

E-5 Solids on Warming (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47; 13C-13.11.01,04-05, 08-09.Textbook pages: 458-460, 479-480, 485, 488, 66-71, 246, 472-473Key Concept Words: Kinetic Theory, state (or phase) change, melting point, freezing point, solid, liquid, physical property, chemical property, physical change, chemical change, hydrate, hygroscopic, and Handbook of Chemistry and Physics.

E-6A Cooling/Heating Curves (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47-48; 13C-13.11.01,04-05, 08-09.Textbook pages: 76, 479-489, 66-71, 44-47 Key Concept Words: ring stand, ring, test tube, test tube clamp, thermometer, wire gauze, pure substance, state (or phase) change, melting point, freezing point, boiling point, condensation point, sublimation, deposition, heating and cooling curve, plateau, phase diagram, gas, physical property, physical change, independent variable, dependent variable, horizontal axis, and vertical axis.

E-6B Heating and Cooling (Quiz) SEE E-4 thru E-6A.

E-7 Physical & Chemical Changes (Test)Illinois State Learning Standards: 11A-11.11.02; 12C-12.11.37,42,47,53.Textbook pages: 66-71, 74-79, 92, 106, 501, 503, 505, 480-488Key Concept Words: quantitative, qualitative, solid, liquid, gas, physical property, extensive physical property, intensive physical property, chemical property, physical change, chemical change, atom,

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ion, element, compound, mixture, solution, alloy, amalgam, aqueous solution, melting, boiling, evaporation, condensation, sublimation, deposition, and four indicators of a chemical change.

E-8 Heat of Solidification/Heat of Combustion (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47,64; 13C-13.11.01,04-05, 08-09.Textbook pages: 68, 485, 487, 296, 382, 384-386, 393-403, 57-58Key Concept Words: physical change, chemical change, solidification (freezing), liquification (melting), combustion, calorimetry, heat, q, specific heat, calorie, and Joule.

E-9A Discovering Density (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47; 13C-13.11.01,04-05, 08-09.Textbook pages: 34-37, 33Key Concept Words: regular solid, irregular solid, liquid, gas, mass, volume, density, meter stick, graduated cylinder, electronic balance, significant figure, and percent error.

E-9B Density Quiz SEE E-9A.

E-10 Beverage Density (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47; 13C-13.11.01,04-05, 08-09.Textbook pages: 34-37, 33, 44-47, 57-58Key Concept Words: pipette, bulb, density, percent, independent variable, dependent variable, horizontal axis, vertical axis, calibration curve, and calorie.

E-11 Boyle’s Law (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47,49-51; 13C-13.11.01,04-05, 08-09.Textbook pages: 67, 424-430, 431-434, 441, 44-47 Key Concept Words: gas, volume, temperature, pressure, atmospheric pressure, barometer, enclosed gas, STP, standard temperature, standard pressure, Boyle’s Law, independent variable, dependent variable, horizontal axis, vertical axis, direct relationship, indirect (or inverse) relationship, and K.

E-12 Charles’ Law (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.47,49-52; 13C-13.11.01,04-05, 08-09.Textbook pages: 67, 424-430, 61-64, 435-438, 441, 44-47Key Concept Words: gas, volume, temperature, enclosed gas, standard temperature, thermometer, Celsius temperature, Kelvin temperature, absolute zero, Charles’ law, independent variable, dependent variable, horizontal axis, vertical axis, direct relationship, indirect (or inverse) relationship, and extrapolation.

E-13 Gas Laws (Test)Illinois State Learning Standards: 12C-12.11.47,49-52.Textbook pages: 66-67, 418-425, 429-430, 61-64, 431-443, 38-47Key Concept Words: solid, liquid, gas, Kinetic Theory, vibrational motion, rotational motion, translational motion, volume, temperature, pressure, STP, standard temperature, standard pressure, Celsius temperature, Kelvin temperature, Boyle’s Law, Charles’ law, Gay-Lussac’s Law, Combined Law, Dalton’s Law, vapor pressure, ideal gas, conversion factor, direct relationship, and indirect (or inverse) relationship.

E-14 Molar Mass (Test)Illinois State Learning Standards: 12C-12.11.37-38,53.Textbook pages: 74-76, 236-237, 92, 110-111, 312, 320-321, 164-167, 246, 472-473Key Concept Words: element, symbol, compound, molecule, chemical (molecular) formula, subscript, mole ratio, atom, atomic mass, molecular mass, molar mass, amu, group, family, period, hydrate, and seven diatomic elements.

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E-15 Equal Volumes (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,47,49-53; 12D-12.11.77; 13C-13.11.01,04-05, 08-09.Textbook pages: 15, 359, 67, 418-427, 429-430, 439-441, 34-37, 446-449, 502-504, 516, 319-322Key Concept Words: flammable, flame accelerant, gas, Kinetic Theory, volume, temperature, pressure, atmospheric pressure, barometer, STP, standard temperature, standard pressure, fluid, apparent mass, actual mass, buoyant force, ratio, density, solubility, and molar mass.

E-16 Moles (Test)Illinois State Learning Standards: 12C-12.11.37-38,53,58.Textbook pages: 310-331, 429-430, 38-44Key Concept Words: mole, atomic mass, Avogadro’s number, molar mass, molar volume, STP, conversion factor, one step problem, and two step problem.

E-17 Molar Volume of a Gas (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,47,49-53; 13C-13.11.01,04-05, 08-09.Textbook pages: 329-331, 439, 424-427, 429-430, 439-441, 33Key Concept Words: eudiometer, gas, volume, temperature, pressure, atmospheric pressure, barometer, molar volume, barometer, atmospheric pressure, STP, standard temperature, standard pressure, Dalton’s Law, vapor pressure, and percent error.

E-18 Molarity (Test)Illinois State Learning Standards: 12C-12.11.37-38,53,58,63.Textbook pages: 320, 506-507, 501, 505,Key Concept Words: molar mass, molarity (M), concentration, solute, solvent, solution, aqueous solution, basic molarity equation, dilution equation, and total molarity equation.

E-19 Single Replacement Reaction (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,53,56-58,63; 13C-13.11.01,04-05,08-09.Textbook pages: 293-295, 284-289, 280Key Concept Words: funnel, funnel rack, filter paper, single replacement (displacement) reaction, balanced chemical equation, coefficient, mole ratio, reactant, and product.

E-20 Balancing Equations (Test)Illinois State Learning Standards: 12C-12.11.37,53,56-57.Textbook pages: 279-295Key Concept Words: chemical reaction, reactant, product, yield, balanced chemical equation, coefficient, direct combination (synthesis) reaction, decomposition reaction, single replacement (displacement) reaction, and double replacement (displacement) reaction.

E-21 Mass & Mole Relationships (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,53,56-58,63; 13C-13.11.01,04-05,08-09.Textbook pages: 193, 249, 213, 598, 347-353Key Concept Words: evaporating dish, watch glass, sodium chloride, sodium bicarbonate, carbon dioxide, hydrochloric acid, water, neutralization reaction, stoichiometry, and conservation of matter.

E-22 Stoichiometry (Test)Illinois State Learning Standards: 12C-12.11.37-38,53,56-58.Textbook pages: 284-290, 280, 346-373Key Concept Words: mole ratio, atom ratio, balanced chemical equation, coefficient, reactant, product, stoichiometry, theoretical yield, actual yield, and percent yield.

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E-23 Double Replacement Reaction (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,53,56-58; 13C-13.11.01,04-05, 08-09.Textbook pages: 310-326, 295, 284-290, 280, 347-357, 365-373Key Concept Words: mole, double replacement (displacement) reaction, balanced chemical equation, coefficient, reactant, product, stoichiometry, conservation of matter, limiting reactant, theoretical yield, actual yield, and percent yield.

E-24 Empirical Formula (Test)Illinois State Learning Standards: 12C-12.11.37-38,53,56-58.Textbook pages: 320. 332-339, 246, 472-473Key Concept Words: molar mass, percent composition, empirical (simplest) formula, molecular formula, hydrate, and anhydrous salt.

2nd Semester ChemistryATOMIC STRUCTURE AND MECHANICS

E-25 Electrostatic Forces (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.45,65-66; 12D-12.11.80-81; 13C-13.11.01,04-05, 08-09.Textbook pages: 95-96, 474-475, 112-113Key Concept Words: nylon monofilament thread, pith ball, electrostatic force (static electricity), attraction, repulsion, ground, conductor, insulator, distance, and strong nuclear force.

E-26 History of the Atom (Crossword)Illinois State Learning Standards: 12C-12.11.37-38,45,54,59,64-66,70,73,80-81; 13A-13.11.03,06.Textbook pages: Chapters 3-4 allKey Concept Words: alpha radiation, Aristotle, atom, atomic mass, atomic mass unit, atomic number, Aufbau, beta radiation, Bohr, cathode ray, Curie, Dalton, Democritus, Einstein, electromagnetic spectrum, electron, excited state, frequency, gamma radiation, ground state, Heisenberg, Hund, infrared radiation, ion, isotope, Millikan, neutron, nucleus, orbital, orbital diagram, Pauli, photon, Planck, principal energy level, proton, quantum, quantum mechanical model, quantum number, radio wave, radioactivity, red light, Rutherford, spectrum, Thomson, uncertainty principle, UV light, violet light, visible spectrum, and wavelength.

E-27 Atomic Structure I (Test)Illinois State Learning Standards: 12C-12.11.37-41,44-45,54,66.Textbook pages: 74-75, 92, 103-111, 168-169, 226, 231-232Key Concept Words: element, atom, proton, neutron, electron, amu, atomic number, ion, isotope, mass number, atomic mass, Z, A, metal, nonmetal, cation, and anion.

E-28 Oxidation Numbers (Test)Illinois State Learning Standards: 12C-12.11.37-41,44,54.Textbook pages: 106, 226, 231-232Key Concept Words: ion, cation, anion, monatomic ion, polyatomic ion, and oxidation number.

E-29 Formula Writing (Test)Illinois State Learning Standards: 12C-12.11.37-42,44-45,53-55,66; 12D-12.11.80.Textbook pages: 106, 226, 231-237, 244-249, 618-619Key Concept Words: inorganic nomenclature, binary compound, chemical formula, ion, oxidation number, monatomic ion, polyatomic ion, anion, cation, metal, nonmetal, and acid.

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Periodic Table: Beginning with this evaluation and continuing through the E-33 evaluation, you are to construct a replica of the Periodic Table that you can use to complete the E-30 thru E-33 evaluations. Your teacher will provide you with the blank form. Certain information on this periodic table may be restricted see your teacher for details. Suggested information to write on your periodic table includes the following:

CONFIGURATIONS (in box) TRENDS1. Symbols (including solid, liquid, gas “colors”)1. Group numbers (“A” and “B” and/or 1-18)2. Atomic number (Z) 2. Main group oxidation numbers3. Orbital notations 3. Metals, nonmetals, metalloids, & “stair step”4. Electronegativity values 4. Main energy levels, sublevels, orbitals & electrons

5. Main group reactivity (metals, & nonmetals)6. 7 Diatomic elements7. Group (family) and period (series) names8. Melting and boiling points9. Atomic mass (A), atomic radii, and ion size10. Ionization energies11. Electron affinity12. Electron dot, number of covalent bonds, & molecular geometry

E-30 Atomic Structure II (Test)Illinois State Learning Standards: 12C-12.11.37-41,43-45,54,59,64,66.Textbook pages: 136-137, 141-153, 211-212, 170-173Key Concept Words: Bohr model, quantum number, ground state, excited state, stability, wave or quantum mechanical model, electron cloud, probability, orbital, principal energy level, sublevel, electron spin, electron configuration, Aufbau order (principle), Pauli Exclusion Principle, Hund’s rule, orbital diagram, noble gas, valence electron, noble gas configuration, orbital notation, valence level orbital diagram, s- block, p-block, d-block, and f-block.

E-31 Bonding and Structure (Test)Illinois State Learning Standards: 12C-12.11.37-42,44,53-55,66; 12D-12.11.80.Textbook pages: 184, 224-231, 236-243, 254-264, 266-267Key Concept Words: electronegativity, ionic bond, covalent bond, Octet Rule, Lewis (electron) dot diagram, molecule, structural formula, single bond, double bond, polar bond, nonpolar bond, polar molecule, nonpolar molecule, VSEPR Theory, linear, trigonal planar, tetrahedral, (trigonal) pyramidal, bent, hybrid orbital, and coordinate covalent bond.

E-32A Group Properties (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,47,53-57,66; 12D-12.11.80; 13C-13.11.01,04-05,08-09.Textbook pages: 447, 632-633, 636-640, 599, 164-169, 190-194, 209-211, 293-295, 667-669Key Concept Words: Hindenburg explosion, phenolphthalein, Arrhenhius base, seven diatomic elements, group or family, alkali metal, halogen, halide, metal, nonmetal, single replacement reaction, and reactivity series.

E-32B Group Properties (Quiz) See E-32A

E-33 The Periodic Table (Test)Illinois State Learning Standards: 12C-12.11.37-41,43-44,46-47.Textbook pages: 158-169, 226, 191-212, 174-185Key Concept Words: Mendeleyev, periodic table, periodic trend (law), group, family, period, main group element, alkali metal, alkaline earth metal, transition metal (inner and outer), lanthanide series, actinide series, carbon group, nitrogen group, chalcogen (oxygen) group, halogen, noble gas, metal,

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nonmetal, metalloid (semimetal), cation, anion, atomic radius, ionic size, ionization energy, electron affinity, and electronegativity.

E-34 Rates of Reaction (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,49,53-55,57,63-64,66; 12D-12.11.80; 13C-13.11.01-02,04-05, 08-09.Textbook pages: 458-460, 420-423, 720-724, 738, 506-507Key Concept Words: Kinetic Molecular Theory (collision theory), elastic (collision), chemical kinetics, reaction rate, five general factors that effect reaction rate, and molarity.

E-35 Endothermic/Exothermic Reactions (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,47,53-55,57,59,64,66-67; 12D-12.11.80; 13C-13.11.01,04-05, 08-09.Textbook pages: 380-383Key Concept Words: endothermic reaction, exothermic reaction, four indicators of a chemical change, and four driving forces of a chemical reaction.

E-36 Energy Graphs (Test)Illinois State Learning Standards: 12C-12.11.37,42,53,57,59,64,67.Textbook pages: 280, 734-737, 384-387Key Concept Words: reactant (Er), product (Ep), energy diagram, activation energy (Ea), activated complex (Eac), endothermic reaction, exothermic reaction, enthalpy, and ΔH.

E-37A Precipitation Reactions (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,47,49,53-55,57,63,66; 12D-12.11.80; 13C-13.11.01,04-05,08-09.Textbook pages: 295, 571-579, 502, 505, 172 Key Concept Words: double replacement reaction, precipitation reaction, precipitate, solubility rule, (complete) ionic equation, net ionic equation, reacting species, spectator ion, soluble, insoluble, and aqueous solution.

E-37B Precipitation Reactions (Quiz) See E-37AE-38 Equilibrium (Test)

Illinois State Learning Standards: 12C-12.11.37-38,42,49,53-55,57,63.Textbook pages: 534-579, 595, 599, 609-613Key Concept Words: reversible reaction, chemical equilibrium, equilibrium constant, Keq, equilibrium expression, Le Chatelier’s Principle, dissolution, precipitation, solubility product, Ksp, acid, base, acid dissociation constant, Ka, base dissociation constant, and Kb.

E-39 Acids & Bases (Test)Illinois State Learning Standards: 12C-12.11.37-42,44,53-55,57,60-63,66; 12D-12.11.80.Textbook pages: 594-601, 605-607, 614, 629-630, 632-633, 636-640, 505Key Concept Words: indicator, neutralization reaction, salt, Arrhenhius acid/base, Bronstead-Lowry acid/base, Lewis acid/base, strong acid/base, weak acid/base, salt, pH, pOH, titration, equivalence point, phenolphthalein, electrolyte, strong electrolyte, and weak electrolyte.

E-40 Vinegar Titration Mini-Lab (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,53-55,57,60-63,66; 12D-12.11.80; 13C-13.11.01-02,04-05, 08-09.Textbook pages: 597-598, 632-633, 636-640, 605-606, 617, 636, 853, 506-507, 332-334Key Concept Words: indicator, neutralization reaction, phenolphthalein, titration, equivalence point, end point, acetic acid, vinegar, molarity, and percent composition.

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E-41A Acid /Base Titration (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-38,53-55,57,60-63; 13C-13.11.01-02,04-05, 08-09.Textbook pages: 597-598, 632-633, 636-640, 506-507Key Concept Words: buret, indicator, neutralization reaction, phenolphthalein, titration, standard solution, standardize, equivalence point, end point, and molarity.

E-41B Acid /Base Titration (Lab Practical)

E-42 Environmental Chemistry (Test)Illinois State Learning Standards: 12B-12.11.31,34; 12C-12.11.37-42,44,53-55,57,60-63,66,71,73; 12D-12.11.80; 12E-85,90-91,95-98; 13A-13.11.03,06-08.Textbook pages: 201, 702, 828-831, 33, 791, 504, 536-537, 542, 549, 631, 403, 764, 751, 150, 448, 839Key Concept Words: lead poisoning, toxic metals, Reduce/Reuse/Recycle, biodegradable, nonbiodegradable, recycling plastics, radon, air pollution, smog, smog reaction, nitrous oxide, acid rain, sulfur dioxide, infrared radiation, Greenhouse Effect, global warming, carbon dioxide, alternative energy sources, UV rays, ozone, ozone hole, and CFC.

E-43A Reactivity Series (Lab)Illinois State Learning Standards: 11A-11.11.01-08; 12C-12.11.37-42,44,47,53-55,57,63,66; 12D-12.11.80.13C-13.11.01,04-05, 08-09.Textbook pages: 293-295, 667-669, 656-659, 663 Key Concept Words: four indicators of a chemical change, single replacement reaction, reactivity series, seven diatomic elements, oxidation, reduction, reducing agent, and oxidizing agent.

E-43B Reactivity Series (Quiz) SEE E43A

E-44 Oxidation/Reduction (Test)Illinois State Learning Standards: 12C-12.11.37-42,44,47,53-55,57,63,66; 12D-12.11.80.Textbook pages: 656-665, 674-677, 232-233Key Concept Words: oxidation, reduction, redox reaction, oxidation number, reducing agent, oxidizing agent, half reaction method, monatomic ion, and polyatomic ion.

E-45 Organic Nomenclature (Test)Illinois State Learning Standards: 12C-12.11.37-42,44,53.Textbook pages: 804-819, 823-826, 836-861Key Concept Words: carbon, organic chemistry, hydrocarbon, fossil fuel, structural formula, saturated hydrocarbon, alkane, backbone carbon chain (parent chain), alkyl group (branch carbon), cycloalkane, unsaturated hydrocarbon, alkene, alkyne, benzene, and aromatic compound.

E-46 Organic Nomenclature (Test)Illinois State Learning Standards: 12C-12.11.37-42,44,53.Textbook pages: 804-819, 823-826, 836-861Key Concept Words: carbon, organic chemistry, hydrocarbon, fossil fuel, structural formula, saturated hydrocarbon, alkane, backbone carbon chain (parent chain), alkyl group (branch carbon), cycloalkane, unsaturated hydrocarbon, alkene, alkyne, benzene, aromatic compound, alkyl halide (halocarbon), alcohol, ether, aldehyde, ketone, carboxylic acid, and ester.

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CONVERSION FACTORSMetric English Metric – English

Length1 km = 1000 m 1 ft = 12 in 2.54 cm = 1 in1 m = 100 cm 1 yd = 3 ft 1 m = 39.97 in1 m = 1000 mm 1 mi = 5280 ft 1.609 km = 1 mi

Mass1 kg = 1000 g 1 lb = 16 oz 1 kg = 2.2 lb1 g = 1000 mg 1 ton = 2000 lb 454 g = 1 lb

Volume1 L = 1000 mL 1 gal = 4 qt 29.32 L = 1 ft3

1 mL = 1 cm3 = 1 g 1 qt = 2 pt 1 L = 1.057 qt1 pt = 16 oz = 2 cups 946 mL = 1 qt

29.6 mL = 1 oz1 mL = 1 cm3

Energy Pressure Electrical Units1 cal = 4.184 J 1 atm = 760 torr = 29.92 in Hg 1 C = 1 A x s1 J = 1 kg m2s-2 = 1 x 10-7 erg 1 atm = 101,325 Pa = 101.3 kPa 1 V = 1J/C1eV/molecule = 23.06 kcal/mol 1 Pa = 1 N m-2 1 W = 1 J/s

= 96.49 kJ/mol 1 torr = 1 mm Hg 1 mol e¯ = 9.648 x 104 C1 L atm = 24.217 cal 1 atm = 760

= 101325 J = 0.1013 kJ = 14.7 lb/in2(psi)= 1.013 bar

Useful Relationshipsln x = 2.303 log x oC = 5/9 (oF – 32) oF = 9/5 oC + 32 K = oC + 273.15

GAS LAWS ABBREVIATIONS AND SYMBOLSBoyle’s Law P2V2 = P1V1 amount of substancen gas constant R

ampere A gram gCharles’ Law V2 = V1 Atmosphere atm joule J

T2 T1 Atomic mass amu Kelvin KAvogadro’s constantN kilo- (prefix) k

Combined Gas V2 = n2 Celsius temperatureoC liter L Law V1 n1 centi- (prefix) c Measure of pressurekPa

concentration c milli- (prefix) mDalton’s Law Ptotal = PA + PB Coulomb C molal m

density d molarity MIdeal Gas Law PV = nRT electromotive forceE mole mol

energy of activationEa Planck’s constant hVan der Waals P = nRT - a enthalpy H pressure P Equation V – b V2 entropy S rate constant k

equilibrium constantK second sFaraday constant F speed of light cformula molar massM temperature, K Tfree energy G time tfrequency v volt V

volume V

**Note: Notation such as g·mol-1 is read as “grams per mole.”

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Vapor Pressure of Water at Various TemperaturesTEMPERATURE,

OC

PRESSURE,

mmHg

TEMPERATURE,

OC

PRESSURE,

mmHg

TEMPERATURE,

OC

PRESSURE,

mmHg0 4.6 21 18.7 50 92.55 6.5 22 19.8 55 118.0

10 9.2 23 21.1 60 149.411 10.5 24 22.4 65 187.512 10.5 25 23.8 70 233.713 11.2 26 25.2 75 289.114 12.0 27 26.7 80 355.115 12.8 28 28.3 85 433.616 13.6 29 30.0 90 525.817 14.5 30 31.8 95 633.918 15.5 35 42.2 100 760.019 16.5 40 55.3 105 906.120 17.5 45 71.9

Rules of Solubility:1. All common nitrates (NO3

-1), chlorates (ClO3-1) and acetates (C2H3O2

-1) are soluble.2. All chlorides (Cl-1), bromides (Br -1) and iodides (I-1) are soluble except those of Hg2

+2, Ag+1 and Pb+2.3. Most sulfates (SO4

-2) are soluble except Ba+2, Ca+2, Pb+2, Hg2+2, Ag+1 and Sr+2.

4. All carbonates (CO3-2), sulfides (S-2), oxides (O-2), chromates (CrO4

-2) and phosphates (PO4-3) are insoluble,

except those of Group 1 elements and ammonium (NH4+).

5. All hydroxides (OH-1) are insoluble except those of Group 1 elements, Sr(OH)2 and Ba(OH)2.

Activity Series of the Elements

React vigorously with acidic solutions to give H2.

LiReact vigorously with liquid water to give H2.

KBaCaNa

React with acids to give H2.

Mg

React slowly with liquid waterbut readily with steam to give H2.

AlZnCrFeCdCoNiSnPbH2

Do not react with acids to give H2*.CuHgAgAu

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*Cu, Hg and Ag react with HNO3 but do not produce H2.

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Periodic Table

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Chemistry Calendar Page #1

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Chemistry Calendar Page #2

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Chemistry Calendar Page #3

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Chemistry Calendar Page #4

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Chemistry Calendar Page #5

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Chemistry Calendar Page #6

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Chemistry Calendar Page #7

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Chemistry Calendar Page #8

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MHS Chemistry OutlineThe following is a list of the Chemistry topics that we will study this year. All topics are covered in the MHS Chemistry workbook. In addition, this booklet contains all relevant textbook reference pages, key terms, reference tables, and important rules. NOTE: “L”=lab; “LP”=lab practical; “Q”=quiz; “T”=test; and “X”=crossword puzzle.

FIRST SEMESTER

E-1 Metric System & Conversions TE-2 Significant Figures & Measurement TE-3 Types of Observations LE-4A Using the Bunsen Burner LE-4B Using the Bunsen Burner LPE-5 Solids on Warming LE-6A Cooling/Heating Curves LE-6B Heating and Cooling QE-7 Physical & Chemical Changes TE-8 Heats of Solidification & Combustion LE-9A Discovering Density LE-9B Density QE-10 Beverage Density LE-11 Boyle’s Law LE-12 Charles’ Law LE-13 Gas Laws TE-14 Molar Mass TE-15 Equal Volumes LE-16 Moles TE-17 Molar Volume of a Gas LE-18 Molarity TE-19 Single Replacement LE-20 Balancing Equations TE-21 Mass & Mole Relationships L E-22 Stoichiometry TE-23 Double Replacement LE-24 Empirical Formula T

SECOND SEMESTER

E-25 Electrostatic Forces LE-26 History of the Atom XE-27 Atomic Structure I TE-28 Oxidation Numbers TE-29 Formula Writing TE-30 Atomic Structure II TE-31 Bonding & Structure TE-32A Group Properties LE-32B Group Properties QE-33 The Periodic Table TE-34 Rates of Reaction LE-35 Endothermic/Exothermic

Reactions LE-36 Energy Graphs TE-37A Precipitation Reactions LE-37B Precipitation Reactions QE-38 Equilibrium TE-39 Acids & Bases TE-40 Vinegar Titration Mini-Lab LE-41A Acid/Base Titration LE-41B Acid/Base Titration LPE-42 Environmental Chemistry TE-43A Reactivity Series LE-43B Reactivity Series QE-44 Oxidation/Reduction TE-45 Organic Nomenclature TE-46 Advanced Organic T

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