Welcome to AP Chemistry

1. Welcome to AP Chemistry

2. What is AP Chemistry? • It is several things: • Equivalent of 1 year college inorganic chemistry class • A class that will prepare you for a test • May 4, 2015 • Hard work • A wonderful way to spend your day • Now on to the details

3. Rules and Procedures I like the term “expectations” • I expect a commitment to excellence and total immersion in the details of chemistry! • I will endeavor to treat everyone with DIGNITY, DECENCY, & RESPECT and expect no less from you! • I expect HONESTY! • I expect everyone will take care of equipment, furnishing, and the room!

4. Rules and Procedures • MAKE-UP WORK: • It is your responsibility to make up all the work you missed. You have the same number of days that you were absent to turn in the missing work. • Pick up any missing work, and notes during Chemistry Clinic. • If you miss a test or quiz, it must be made up during a single visit to Chemistry Clinic.

5. Rules and Procedures • TARDIES – read the school policy – don’t be late and you don’t have a problem. • No Food, Drink Or Gum In Class • LATE WORK – I don’t accept late homework. • I do accept other assignment late (10% off each day)

6. Rules and Procedures • PASSES: Since every minute of class time is valuable, hall passes will be given only on an emergency basis. • No Mole Bucks issued or used in AP

7. Rules and Procedures • LAB- Because of the importance of safety in the lab, violation of laboratory safety rules and procedures may result in loss of lab privileges. • You Break it – you pay for the replacement include shipping and handling.

8. Grading • Grade breakdown • Homework / Classwork / Quizzes & Shakhashiri 10% • Labs & Lab Reports 25% • POGILS & Virtual Chem. Labs 25% • Tests 40%

9. What you need for class DAILY • Paper • Pencil & pen • Calculator- Scientific • Zumdahl Text • Lab Notebook

10. Any questions? • Lets get started

11. Significant figures • Meaningful digits in a MEASUREMENT • If it is measured, it has sig figs. • If not it is exact. • All numbers except zero are significant. • Some zeros are, some aren’t • See the H Chem handout for examples and more specific rules. • USE SIG FIG ON EVERYTHING, ALL SEMESTER

12. Which zeroes count? • In between other sig figs does • Before the first number doesn’t • After the last number counts if there is a decimal point • Examples • 3200 2 sig figs • 3200.4 sig figs

13. Doing the math • Multiplication and division, same number of sig figs in answer as the least in the problem • Addition and subtraction, same number of decimal places in answer as least in problem.

14. Scientific Method Steps. • A way of solving problems • Observation (2 general types): • Qualitative (color, precipitate, warm) • Quantitative (involves number w/ units) • Hypothesis - possible explanation • Experiment - test hypothesis • Reiterations – repeat the process

15. Scientific method. • After many cycles, a broad, generalizable explanation is developed for why things behave the way they do with considerable evidence = Theory (Model) • A concise verbal or mathematical statement summarizes a variety of observation = Law • Laws are summaries of observations

16. Scientific method. • Theories have predictive value. • The true test of a theory is if it can predict new behaviors. • If the prediction is wrong, the theory must be changed. • Theory- why • Law - how

17. Theory (Model) Law Observations Hypothesis Modify Experiment Prediction Experiment

18. Metric System • Every measurement has two parts • Number • Scale (unit) • SI system (le Systeme International) based on the metric system • Prefix + base unit • Prefix tells you the power of 10 to multiply by - decimal system -easy conversions

19. Metric System • Base Units • Mass - kilogram (kg) • Length- meter (m) • Time - second (s) • Temperature- Kelvin (K) • Electric current- ampere (amp, A) • Amount of substance- mole (mol) Chemistry generally uses gram & millimeter

20. Mass and Weight • Mass is measure of resistance to change in motion • Weight is force of gravity. • Sometimes used interchangeably • Mass can’t change, weight can

21. Uncertainty • Basis for significant figures • All measurements are uncertain to some degree • Precision- how repeatable • Accuracy- how correct - closeness to true value. • Random error - equal chance of being high or low- addressed by averaging measurements - expected

22. Uncertainty • Systematic error- same direction each time - Want to avoid • Better precision implies better accuracy • You can have precision without accuracy • You can’t have accuracy without precision

23. Dimensional Analysis Using the units to solve problems

24. Dimensional Analysis • Use Conversion Factors to change the units • Conversion factors = 1 • 1 foot = 12 inches (equality) • 12 in =1= 1 ft. 1 ft. 12 in • 1 equality = 2 conversion factors • multiply by the one that will give you the correct units in your answer.

25. Examples • 11 yards = 2 rod • 40 rods = 1 furlong • 8 furlongs = 1 mile • The Kentucky Derby race is 1.25 miles. How long is the race in rods, furlongs, meters, and kilometers? • A marathon race is 26 miles, 385 yards. What is this distance in rods, furlongs, meters, and kilometers?

26. Examples • Science fiction often uses nautical analogies to describe space travel. If the starship U.S.S. Enterprise is traveling at warp factor 1.71, what is its speed in knots? • Warp 1.71 = 5.00 times the speed of light • speed of light = 3.00 x 108 m/s • 1 knot = 2000 yd/h exactly

27. Examples • Apothecaries (druggists) use the following set of measures in the English system: • 20 grains ap = 1 scruple (exact) • 3 scruples = 1 dram ap (exact) • 8 dram ap = 1 oz. ap (exact) • 1 dram ap = 3.888 g • 1 oz. ap = 1 oz. troy = 28.349 grams • What is the mass of 1 scruple in grams?

28. Examples • The speed of light is 3.00 x 108 m/s. How far will a beam of light travel in 1.00 ns?

29. Temperature and Density

30. Temperature • A measure of the average kinetic energy • WE WILL USE ONLY CELSIUS IN AP • Different temperature scales, all are talking about the same height of mercury. • Derive a equation for converting ºF toºC

31. 0ºC = 32ºF 32ºF 0ºC

32. 100ºC = 212ºF 0ºC = 32ºF 0ºC 100ºC 212ºF 32ºF

33. 100ºC = 212ºF 0ºC = 32ºF 100ºC = 180ºF 0ºC 100ºC 212ºF 32ºF

34. 100ºC = 212ºF 0ºC = 32ºF 100ºC = 180ºF 1ºC = (180/100)ºF 1ºC = 9/5ºF 0ºC 100ºC 212ºF 32ºF

35. ºF ºC

36. (0,32)= (C1,F1) ºF ºC

37. (0,32) = (C1,F1) (120,212) = (C2,F2) ºF ºC

38. Density • Ratio of mass to volume • D = m/V • Useful for identifying a compound • Useful for predicting weight • An intrinsic property- does not depend on what the material is

39. Density Problem • An empty container weighs 121.3 g. Filled with carbon tetrachloride (density 1.53 g/cm3 ) the container weighs 283.2 g. What is the volume of the container?

40. Density Problem • A 55.0 gal drum weighs 75.0 lbs. when empty. What will the total mass be when filled with ethanol? density 0.789 g/cm3 1 gal = 3.78 L 1 lb = 454 g

41. Classification of Matter • Def. Matter is anything that occupies space and has mass • 3 States: Solid, Liquid, and Gas • 2 Types of Mixtures: • Homogeneous – parts are not easily distinguishable, not easily separated, example: solution • Heterogeneous – visibly distinguishable parts

42. Classification of Matter • Pure Substance – constant composition • 3 Methods of Separating Mixtures • Distillation – based on temperature each part changes from liquid to gas • Filtration – based on size of parts • Chromatography – based on parts in 2 different phases