I. Qualit a Qualit t a ive iv vs. Quantit Quan a tit tiv a e tiv Measurements

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2 I. Qualitative vs. Quantitative Measurements

3 Qualitative Measurement 1) Qualitative measurement = a measurement that gives descriptive, NONnumeric results a)ex: Jillian ran a fast race. b)ex: The light was green.

4 Quantitative Measurement 2) Quantitative measurement = a measurement that gives results in a definite form, usually in numbers and units a) Ex: Jeff finished dhis race in 54.3 seconds. b) Ex: The light had a wavelength of 505 nanometers.

5 II. SI System

6 1) SI System = a modernized form of the metric system used by scientists

7 A. Fundamental SI Units 1) Fundamental unit = a unit that is dfi defined dby a single standard dof measurement

8 Fundamental SI Units (h (there are seven fundamental SI units) Quantity Unit Symbol Length meter m Mass kilogram kg Time second s Temperature kli kelvin K Amount of substance bt mole mol Electric current ampere A Luminous candela dl cd intensity

9 A. Fundamental SI Units 3) Length = a measure of linear distance; the fundamental lsi unit of length is the meter (m) a)the distance light travels in a vacuum during a time interval of 1/ of a second is the SI standard for one meter.

10 A. Fundamental SI Units 4) Mass = a measure of the quantity of matter in a sample; the fundamental SI unit of mass is the kilogram (g);( (kg); (the abbreviation for gram is g ) g) a) A platinum iridium cylinder kept at the International Bureau of Weights and Measures in the French town of Sevres is the SI standard for one kilogram.

11 A. Fundamental SI Units b) weight = a measure of the gravitational pull on matter

12 A. Fundamental SI Units 5) Time = a measure of the interval between occurrences; the fundamental SI unit of time is the second (s) a) The duration of 9,192,631,770 periods of particular radiation emitted by cesium 133 atoms is the SI standard for one second.

13 B. Derived Unit 1) Derived unit = a unit that can be obtained from combinations of fundamental units

14 Examples of Derived SI Units Quantity Unit Symbol Derivation Area square meter m 2 = m m length width Volume cubic meter m 3 = m m m length width height Density kilogram per cubic kg/m 3 mass meter volume Speed (velocity) meter per second m/s _length_ time Force newton N = _kg m_ s 2 Pressure pascal Pa = N/m 2 = kg m s 2 Energy joule J = N m = _kg m 2 _ s 2 mass length_ time time _force_ area force length

15 B. Derived Unit 3) Volume = a measure of the amount of space occupied by a sample of matter; the derived SI unit of volume is the cubic meter (m 3 ) a) Chemists often use a non SI unit for volume, the liter (L). b) 1 dm 3 = 1 L c) 1 cm 3 = 1 ml

16 1) Other SI units are obtained by combining prefixes with a root unit. The prefixes represent multiples or fractions of 10. The following table lists some prefixes:

17 Prefixes Used With SI Units Prefix Symbol Exponential Meaning Factor Example exa- E ,000,000,000,000,000, exameter (Em) = m peta- P ,000,000,000,000,000 1 petameter (Pm) = m tera- T ,000,000,000,000 1 terameter (Tm) = m giga- G ,000,000,000 1 gigameter (Gm) = m mega- M ,000,000 1 megameter (Mm) = m kilo- k ,000 1 kilometer (km) = 1000 m hecto- h hectometer (hm) = 100 m deka- da dekameter (dam) = 10 m meter (m) = 1 m deci- d decimeter (dm) = 0.1 m centi- c centimeter (cm) = 0.01 m milli- m millimeter (mm) = m micro- µ micrometer (µm) = m nano- n nanometer (nm) = m pico- p picometer (pm) = m femto- f femtometer (fm) = m atto- a attometer (at) = m

18 D. Prefixes Used With SI Units Prefixes Symbol Base Unit Symbol Kilo- k meter m Hecto- Deka- Deci- h da d c liter gram L g Centi- m Millisecond s

19 1) Write the correct abbreviation for each of the following units. a) kilosecond ks hg b) hectogram dal c) dekaliter d) deciliter dl e) centimeter cm mg f) milligram

20 E. Conversions (Ladder Method) Mthd) Kilo (k) 1,000 Hecto- (h) 100 Deka- (da) To convert to a smaller unit, move the decimal point to the RIGHT or MULTIPLY. 10 Base Unit Deci- m, L, g, s (d) Centi- 0.1 (c) Milli (m) 0.001

21 Try these conversions, using the ladder method. 1, Base Unit m, L, g,s Kilo Hecto- Deka- Deci- 0.1 Centi Millia) 1000 mg = g 1.0 b) 160 cm = mm 1,600 c) 109 g = kg d) 1L = ml 1,000 e) 14 km = m 14,000 f) 250 m = km

22 F. Other Useful Conversions 1) Some English System Conversions (exact conversions): 1 foot (ft) = 12 inches (in) 1 pound (lb) = 16 ounces (oz) 1 yard (yd) = 3 feet (ft) 1 ton = 2000 pounds (lb) 1 mile (mi) = 5280 feet (ft) 1 quart (qt) = 32 fluid ounces (fl oz) 1 quart (qt) = 2 pints (pt) 1 gallon (gal) = 4 quarts (qt)

23 2) Some conversions between systems: 1 inch (in) = 2.54 centimeters (cm) (exact conversion) 1 pound (lb)= grams (g) 1 gallon (gal) = liters (L)

24 III. Scientific Notation

25 1) m =

26 2) m =

27 3) For numbers expressed in scientific notation, the decimal place goes after the first nonzero digit.

28 4)Write each of the following numbers in scientific notation x 10 4 a) g = 4 g b) 289,302 km = x 10 5 km ), x 10 5 c) mm = 5 mm

29 5) Write each of the following numbers in ordinary notation. a) 8.95 x ,500 m m = b) x hm hm = c) 2.73 x ,000 cm cm =

30 IV. Taking Measurements

31 1) Review the proper way to measure using a ruler, graduated cylinder, thermometer, etc.

32 IV. Taking Measurements Meniscus = the curvature of a liquid in a container ti because of surface tension. Your eye should be level with the top of the liquid and you should read the bottom of the meniscus.

33 V. Precision, Accuracy and Percent Error: 1) Precision = a measure of how close a series of measurements are to one another a) It tk takes a series of measurements to determine precision

34 V. Precision, Accuracy and Percent Error: 2) Accuracy = a measure of how close a measurement comes to the true or accepted value of what is measured

35 3) Bull s Eye Analogy Shows BOTH Accuracy & Precision Shows ONLY Precision Shows Neither Accuracy or Precision

36 V. Precision, Accuracy and Percent Error: 4) Percent error = the difference between the measured quantity and the accepted tdvalue, expressed as a percentage of the accepted tdvalue

37 Percent Error Formula: % error = Value accepted Value experimental 100 % Vl Value accepted 5) Gary measured the density of a piece of lead to be g/cm 3. The accepted value for the density of lead is g/cm 3. Calculate the percent error.

38 VI. Problem Solving 1) Approach to solving problems: a) Analyze: 1) Read the problem carefully at least twice. 2) Identify what you know and what you are trying to find. 3) Include units.

39 b) Plan: VI. Problem Solving 1) Graphs,,p pictures,,graphic organizers, flowcharts, or other visual aids may be helpful. 2) Identify formulas and/or conversion factors that will be used. 3) Be certain that units will cancel as needed. 4) Solve formulas for an unknown variable before putting in values. 5) Set up the problem.

40 c) Compute: VI. Problem Solving 1) Plug in given information, conversion factors, and othernecessary values. Include units on all numbers! 2) Cancel units properly. 3) Calculate the answer.

41 d) Evaluate: VI. Problem Solving 1) Is the answer reasonable? 2) Is the same answer obtained after rechecking? 3) Do the units cancel correctly so the answer has the proper units? 4) Have all parts of the question been answered?

42 VII. Density: 1) What is heavier, a pound of lead or a pound of cork? Neither, they both weigh a pound!! Lead is MORE DENSE

43 VII. Density: 2) What floats in water, lead or cork? Why? Cork floats in water b/c it is LESS dense than water

44 VII. Density: Take a look at the two boxes below. Each box has the same volume. If each ball has the same mass, which box would weigh more? Why?

45 VII. Density: The box that has more balls has more mass per unit of volume. othis property of matter is called DENSITY.

46 VII. Density: 4) Density = a property of matter representing the mass per unit volume a) The derived dsi unit of density: kg/m 3 b) Other commonly used density units: g/cm 3, g/ml, g/l

47 VII. Density: c) Volumes can change with temperature, therefore, densities also change with temperature. o Ex: Increasing the temperature t of a gas would also increase the volume of the gas. Therefore the temperature of the gas, affects the density of the gas!

48 VII. Density: d) Formula: Density = Mass Volume or D = M_ V V

49 VII. Density: 5) Solve the density formula for mass.

50 VII. Density: 6) Solve the density formula for volume.

51 7) A sample of aluminum metal has a mass of 8.4 g. The volume of the sample is 3.1 cm 3. Calculate the density of aluminum.

52 8) Diamond has a density of 3.26 g/ cm 3. What is the mass of a cm 3 sample of diamond?

53 9) Suppose a scientist collects 76.2 g of mercury. Calculate the volume given that the density of mercury is 13.6 g/ml.