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Chapters 1 & 2: Measurement and Calculations

Chapters 1 & 2: Measurement and Calculations. Learning Targets Identify a given substance as an element or compound Parts of scientific method/design Classify properties and changes as chemical or physical

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Chapters 1 & 2: Measurement and Calculations

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  1. Chapters 1 & 2:Measurement and Calculations Learning Targets Identify a given substance as an element or compound Parts of scientific method/design Classify properties and changes as chemical or physical Explain the structure of the periodic including properties of elements based on their location (metal, nonmetal, etc.) Express data and results of calculations with appropriate significant figures, units, and in scientific notation Calculate percent error from lab data and use this to evaluate the quality of lab data Perform density calculations and apply density conceptually (e.g. identifying substances or determining if an object will float

  2. Key Words • atom • compound • element • pure substance • mixture • homogeneous/heterogeneous • chemical change/property • physical change/property • direct/inverse proportion • family/group • period • significant figure • scientific notation • conversion factor • percent error • metal • nonmetal • metalloid • noble gas • quantitative • qualitative

  3. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 • Matter is anything that has volume and mass • Mass is a measure of the amount of matter present • Volume is the amount of space an object occupies • Atoms are the fundamental building block of matter • Elements are pure substances made of one type of atom • Compounds are substances made from the atoms of two or more elements

  4. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 Properties of Matter • Matter has physical properties and can undergo physical changes • Physical properties are observed without changing the identity of a substance (examples include: density, color, melting point) • Physical changes don’t involve a change in a substance’s identity (examples include: phase change, breaking)

  5. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 Properties of Matter • Matter has chemical properties and can undergo chemical changes • Chemical properties relate to a substance’s ability to become a new substance (example: flammability, corrosiveness) • Chemical changes involve a change in a substance’s identity • Chemical Equation (Reactants to Products)

  6. Section 1: Classifying and Changing Matter Signs of a Chemical Change • Gas Production • Formation of a Precipitate • Dramatic Temperature Change • Unexpected Color Change

  7. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 Classification of Matter • Matter can be classified as either a pure substance or a mixture • Pure Substances are fixed ratios and can be either a element or a compound. • Elements are found on the periodic table, They can not be broken down by physical means. • Compounds are substances made of two or more elements.

  8. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 Classification of Matter • Mixtures are blends of two or more types of matter, each retaining its own identity and properties • Mixtures are combined physically and can be separated using physical means • There are two types of mixtures: • Homogenous –they are unified throughout • Heterogenous – not evenly mixed

  9. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23

  10. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 Periodic Table • The periodic table organizes elements into groups based on similar properties • The vertical columns are known as groups or families; elements in the same group have similar chemical properties • The horizontal rows are called periods; elements in the same period don’t necessarily have similar chemical properties

  11. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23

  12. Section 1: Classifying and Changing MatterPages 26-27 RBQs Pgs. 59-61 #9-11,14, 15, 18-21,23 • Metals: • Nonmetals: • Metalloids: • Noble Gases:

  13. Section 2 : Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 Scientific notation is a ay of taking very large numbers and/or very small numbers and writing them more simply For example, an important number in chemistry is 602,000,000,000,000,000,000,000which suck to write…but in scientific notation it is6.02 x 1023

  14. Which of the following is a chemical change? • Sanding wood • Melting ice • Milk going sour • Vaporizing of gasoline

  15. Blood would be considered • Element • Compound • Homogenous mixture • Heterogenous mixture

  16. Section 2: Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 Exercise: Use the examples below to come up with a set of rules for converting from scientific to regular notation.Sci. NotationReg. NotationSci. NotationReg. Notation 4.521 x 105 452,100 8.2 x 10-8 .0000000823.8862 x 102 388.62 6.447 x 10-4 .0006447

  17. Section 2: Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 Exercise: Use the examples below to come up with a set of rules for converting from regular to scientific notation.Sci. NotationReg. NotationSci. NotationReg. Notation 817 8.18 x 102 0.00456 4.56 x 10-3 0.000006 6 x 10-6 48260000 4.826 x 107

  18. Convert 506100 to scientific notation: • 5 x 105 • 5.1 x 10 -5 • 5.061 x 105 • 51 x 105

  19. 4.02 x 103 in standard notation is • .00402 • .000402 • 4020 • 40020

  20. Which of the following is not in scientific notation? • 2.31 x 108 • 2.31 x 10-3 • 231 x 107 • 2.31 x 1056 • 2.31 x 103

  21. Section 2: Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 • Measurements made in the lab are never perfect • Data can only include numbers that we are sureof • Record all numbers you aresure of, then estimate anadditional number

  22. Section 2: Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 • Numbers given this way are called significant figures • Sig figs also indicate how accurate a measuring device is

  23. Section 3: Conversion FactorsPages 40-42 RBQs Pgs. 60-61 #28-32, 49 Metric conversions (mL to L, g to kg) can be performed without the use of conversion factors To convert these unit, just move the decimal the appropriate number of places This works because the metric prefixes always change the value of a number by a factor of 10, which is what you do when you move a decimal point

  24. Section 3: Conversion FactorsPages 40-42 RBQs Pgs. 60-61 #28-32, 49 Kangaroos Have Dandruff But Don’t Care Much

  25. Sample: How many meters are there in 50 cm? • 50 m • 5000 m • 500 m • .05 m • 0.5 m

  26. Sample: How many kilometers are there in 8,230 mm? • 82,300 km • .00823 km • .0823 km • .823 km • 82.3 km

  27. Sample: How many mg are in 46 g? • 46000 g • 4600 g • 460 g • 4.6 g • .046 g

  28. Section 3: Scientific Notation & Sig FigsPages 46-52 RBQs Pgs. 59-61 #21-23, 36-46 • When using conversion factors, the conversion factor has nothing to do with the number of significant figures. Sample: What is the volume in mL of a substance that has a mass of 5.00 grams and a density of 2.1 g/mL?

  29. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Data can be either quantitative or qualitativeQuantitative:Qualitative:Quantitative data is data obtained through measurements

  30. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Every measurement needs a number and a unit • In chemistry, SIunitsare used to report measurement

  31. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Derived units can be made from the base units • These units include volume and density 1. What formula is used to find the volume of a cube?2. What units are used to measure a cube’s dimensions?3. Therefore, what are possible volume units?

  32. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Density is the ratio of an object’s mass to its volume • Mass measures the amount of matter present • Volume measures the space occupied by matter • And since a ratio is just a fraction •What are some possible units for density?

  33. Sample: A sample of liquid with a volume of 23.50 mL has a mass of 35.062 g. What is the density of this liquid? • 1.492 g/mL • 1.5 g/mL • .6702 g/mL • .67024 g/mL • 1.4920 g/mL

  34. Sample: What is the volume of a sample of liquid mercury that has a mass of 76.2 g, given that the density of mercury is 13.6 g/mL? • 1.04 x 103 mL • 1.036 x 103 mL • 5.6 mL • 5.60 mL • 6 mL

  35. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Density can be usedto identify unknownsubstances • It can also be used todetermine if an objectwill float

  36. Section 4: Units, Density, and % ErrorPages 59-61 RBQs Pgs. 59-61 #14, 26-29, 30-35, 48, 50 • Percent error is a measure of the accuracy of lab results. It indicates how far data is from the true value

  37. Sample: A length is measured at 6.7 cm. The correct value is 7.1 cm. Calculate the percent error.

  38. Sample: A student measures the mass and volume of a substance and calculates its density as 1.40 g/mL. The correct value is 1.36 g/mL. What is the student’s percent error? • 42.86% • 29.41% • 28.57% • 40.00%

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