My powerpoint from Chapter 3 of my Chemistry I class.

1. Chapter 3 Scientific Measurement

2. A. Qualitative Measurements B. Quantitative Measurements - give results in descriptive , non-numeric form - give results in definite form, numbers and units Examples: Mr. Smith is tall. The room is hot. Examples: Mr. Smith is 6 feet tall. The room is 70 degrees Fahrenheit.

3. II. Scientific Notation Def – Scientific notation is simply writing a number as a product of two numbers . Examples: 12,300,000 = _____________ 1.23 x 10 7 0.0000546 = _____________ 5.46 x 10 -5 .

5. Calculations with Scientific Notation 1. Multiplication and Division a. Multiplying – MULTIPLY the coefficients and ADD the exponents. b. Dividing – DIVIDE the coefficients and SUBTRACT the exponents. Example 1: (9 x 10 4 ) x (2 x 10 3 ) 18 x 10 7 1.8 x 10 7 x 10 8 Example 2: (8 x 10 4 ) ÷ (2 x 10 7 ) 4 x 10 -3

6. Calculations with Scientific Notation 2. Addition and Subtraction Rule: First the powers of 10 must be the same! Then just add or subtract the coefficients and keep the power of 10 the same Example 1: (9 x 10 4 ) + (2 x 10 3 ) (9 x 10 4 ) ( 0.2 x 10 4 ) (0.2 x 10 4 ) 9.2 x 10 4 90 000 2 000 92 000

7. Calculations with Scientific Notation 2. Addition and Subtraction Rule: First the powers of 10 must be the same! Then just add or subtract the coefficients and keep the power of 10 the same Example 2: (4 x 10 8 ) - (9 x 10 6 ) (4 x 10 8 ) ( 0.09 x 10 8 ) (0.09 x 10 8 ) 3.91 x 10 8

9. II. Accuracy, Precision, and Error A. Accuracy – The measure of how close a measurement is to the accepted value . B. Precision – How close a series of measurements are to each other . Note: Precision also describes how “ exact ” a measuring tool allows you to be. Example: Which is more precise? 19 grams or 18.895 grams

10. The Dartboard Model Accuracy = Precision = Accuracy = Precision = Accuracy = Precision = Low Low Low High High High

11. C. Error Def – The difference between the experimental value and the accepted value. Experimental Value – The value measured in the lab Accepted Value – The correc t value, based on reliable references or calculations Equation: [Experimental] – [Accepted] = Error

12. Sample Problem: James weighs a metal cylinder and finds it has a mass of 48.34 grams. If the actual mass of the cylinder is exactly 50.00 grams, what is his error? 48.34 – 50.00 = -1.66 grams

13. D. Percent Error Def – The absolute value of the error divided by the accepted value, multiplied by 100 - Compares the error to the accepted value , showing how bad the error really is. Equation: % Error = | error | x 100 accepted value

14. Steve and Martin each order bricks from a lumber yard. Steve orders 500 bricks to build a wall, but the lumber yard only delivers 499. Martin orders 5 bricks, but only recieves 4. Calculate the error and percent error in each order. 499 – 500 = -1 4 – 5 = -1 499 – 500 = -1 4 – 5 = -1 Steve Martin The error in both orders is the same! In which order is it more significant? | -1 | 500 x 100 = | -1 | 5 x 100 = 0.2% 20%

15. II. Significant Figures in Measurements Significant Figures – All the digits that are known in a measurement, plus one estimated digit How tall is the rectangle on the left according to the ruler shown? cm 1.64 1 2 Between 1.6 & 1.7 Known Digits Estimated Digit

16. 4.13 *Note: With all measuring tools, you are expected to estimate one digit beyond what you can actually see marked = significant! 4 5 What is the volume of water in the graduated cylinder to the left? mL Between 4.1 & 4.2 Known Digits Estimated Digit

17. Reporting Measurements in proper Sig Figs - Measurements must be reported with the correct number of significant figures ! - Significant figures describe the precision with which your measuring tool is calibrated . 0.6 cm 0.62 cm 0.628 cm 0 1 0 1 0 1

18. Rules for Sig Figs (Rules for Zero’s) 1. All nonzero digits ARE significant. 2. Zero’s appearing between nonzero digits ARE significant. 3. Zeros to the left in front of nonzero digits ARE NOT significant. (They are just placeholders !) 546 = ________ sig figs 13.456 = _________ sig figs 104.3 = ________ sig figs 20.05 = _________ sig figs 0.00224 = ________ sig figs 0.34 = _________ sig figs 3 5 4 4 3 2

19. Rules for Sig Figs (Rules for Zero’s) 4. Zeros at the end of a number and to the right of a decimal ARE ALWAYS significant. 5. Zeros at the end of a number and LEFT of a decimal are SOMETIMES significant. Unless it is stated that they are specifically measured, we WILL NOT count them as significant. 55.00 = ________ sig figs 320.0 = _________ sig figs 120 = ________ sig figs 33,000 = _________ sig figs 2 2 4 4

20. V. Significant Figures in Calculations General Rule : Your answer cannot be more precise than the measurements used to calculate that answer. * You must round your answers to the proper number of significant figures. Example: Tennis Ball Drop Times – Averaged Trial 1 - 0.89 seconds Trial 2 - 0.91 seconds Trial 3 - 1.04 seconds Trial 4 - 0.84 seconds Trial 5 - 0.73 seconds Average Time - 0.882 seconds 0.88 seconds

21. 1. Rounding – Calculations must be rounded to make them consistent with the measurements from which they were calculated. How to Round Numbers: a. First, decide how many significant figures your answer should have. * Follow the rules for addition/subtraction or multiplication/division below! b. Once significant figures have been decided, count that many places , starting from the left .

23. 2. Addition and Subtraction Rule: The answer should be rounded to have the same number of places after the decimal as the measurement with the LEAST number of decimal places. 24.312 0.2332 19.5 0.4 + 4.66 + 0.66257 19.5 2.6 - 4.66 - 1.55 48.472 1.29577 14.84 1.05 48.5 14.8 1.3 1.1

24. 3. Multiplication and Division Rule: Round your answer to have the same number of significant figures as the measurement with the least number of significant figures. 24.312 0.2332 19.5 0.40 x 0.66 x 0.66257 19.5 2.6 ÷ 4.6 ÷ 1.55 312.89544 0.06180453 4.2456… 1.6774… 4.2 310 0.062 1.7

25. VI. International System of Units - Abbreviated SI , after the French name, Le Syst é me International d’Unit é s - A revised version of the Metric System . 1. The Metric System - All metric units are based on the number 10 or multiples of 10 . - Measurements consist of a base unit to which a prefix may be added to make it larger or smaller by a power of 10 .

26. 3 main base units: a. Length = meter (m) b. Volume = liter (L) c. Mass = gram (g)

27. Metric Prefixes: ( Memorize!) giga- G 1,000,000,000x larger 10 9 mega- M 1,000,000x larger 10 6 kilo- k 1,000x larger 10 3 hecto- h 100x larger 10 2 deka- da 10x larger 10 1 deci- d 10x smaller (1/10 th or 0.1) 10 -1 centi- c 100x smaller (1/100 th or 0.01) 10 -2 milli- m 1000x smaller (1/1000 th or 0.001) 10 -3 micro-  1,000,000x smaller (1/1,000,000 th or 0.000 001) 10 -6 nano- n 1,000,000,000x smaller (1/1,000,000,000 th or 0.000 000 001) 10 -9 pico- p 1,000,000,000,000x smaller (1/1,000,000,000,000 th or 0.000 000 000 001) 10 -12 Power of 10 Value Symbol Prefix

28. Examples: 1 kilogram = 10 3 grams (1000x larger) 1 millimeter = 10 -3 meter (1000x smaller) 1 hectoliter = 10 2 liters (100x larger) 10 1 m = 1 dekameter = 1 dam 1 m 10 meters

29. 10 birds = 1 meter Each bird = 1/10 th of a meter (10 -1 m) 1 bird = 1 decimeter (1 dm) Example: 1 meter stick

30. 2. Measurements A. Length – measure of linear distance - Unit = meters (m) Associations: 1 meter  1 yard (39.5 inches) 1 inch = 2.54 centimeters 1 mile = 1.6 kilometers 1 kilometer = 0.6 miles ( 10 km = 6 mi )

32. Ways to Measure Volume 1. Geometric Solid – (cube, rectangular solid, pyramid, cylinder, sphere, etc…) - use an equation to derive the volume from length measurements Example 1: Rectangular Solid volume = length x width x height volume = meters x meters x meters = m 3 volume = cm x cm x cm = cm 3 Kleenex Box = 22 cm x 11 cm x 5 cm = 1210 cm 3

33. Example 2: Cylindrical Solid (area of base x height) area of circle =  r 2 volume =  r 2 h * r = radius (1/2 the diameter) Petri Dish diameter = 9.5 cm radius = 4.75cm height = 2.0 cm volume = 141.8 cm 3

34. 2. Liquids – pour the liquid into a measured container (graduated cylinder) - read the level of the meniscus in liters or mL Note: Liquids are usually measured in liters or mL , while solids are usually measured in m 3 or cm 3 . Associations: 1 liter  1 quart (4 cups) 1 gallon  4 liters 1 mL  20 drops 1 mL = 1 cm 3 = 1 cm x 1cm x 1 cm 1 L = 1 dm 3 = 10cm x 10cm x 10cm 1 L = 1000 mL

35. 3. Irregular shaped solids – Water displacement ! - Dunk an object in water and the water level goes up ! 4.13 mL 4.78 mL - Simply subtract the final and initial volumes to get difference – Indirect method! 4 5 4 5 Volume _______ Volume _______

37. 1 kg = mass of 1 L of water at 4 degrees Celsius 1 kg = 2.2 lbs 1 ounce  28 grams 1 kg = 1000 grams 1 penny  3 grams

38. VII. Temperature Definition – a measure of the average kinetic energy of particles in matter. - Kinetic energy is energy of motion , therefore, temperature actually measures the speed of particles . Wikipedia.org – Temperature (click here)

39. - Temperature also describes the direction of heat flow – from hotter to colder a. When you hold an ice cube it feels cold = heat flowing from hand to ice b. When you hold an cup of coffee it feels hot = heat flowing from coffee to hand

40. Temperature Scales: a. Celsius scale – based on the boiling and freezing points of water b. Kelvin scale – based on absolute zero , the lowest temperature theoretically possible. * At absolute zero, all particle motion stops !

41. Fahrenheit =  F Celsius =  C Kelvin = K -273 0 100 -460 32 212 373 273 0 Freezing point of water Boiling point of water Absolute Zero

42. The End