1. Unit 1 Properties of and Changes in Matter 1 https://www.youtube.com/watch?v=5_kt0ecu_jk Rounding song

2. Describing matter Chemical properties Physical properties 2

3. Physical Properties Observed or measured without changing the composition Describe bulk quantities, not single atoms 3

4. Observation Mini Activity 4

5. Physical Properties Intensive (also called intrinsic) – INdependent of sample size – Examples: color, state of matter, luster, texture, boiling point, melting point, solubility, density – Can identify a substance OR Extensive (also called extrinsic) – dependent on sample size – Examples: mass, volume, length – Try this: http://www.texasgateway.org/node/2357http://www.texasgateway.org/node/2357 5

6. Physical Properties Examples: – Color – State of matter (solid, liquid, gas) – Luster – Texture (granular, powdery) – boiling point and melting point – Solubility – Density – Size (mass, volume, length) 6

7. Chemical Properties Describe the type of changes that form new materials Become evident during a chemical reaction Examples: – A chemical property of metals is the ability to react with acids. – A chemical property of carbon dioxide gas is that no combustion reaction can take place in its presence. 7

8. Measurement A quantitative observation that includes a number and a unit 8

9. Good measurements Read graduated cylinder at eye level Record volume at the bottom of the meniscusbottom of the meniscus 9

10. Sig Figs and Song Sig Figs and Song Any measurement has some degree of uncertainty. When recording measurements, always include one estimated (uncertain) digit (or place value position). – Example: This graduated cylinder has markings every 1 mL. You estimate the tenths place. – 43.0 mL 10

11. Significance in Measurement For each of the rulers, give the correct length measurement for the steel pellet as a single number rather than a range

12. Significance in Measurement The graduated cylinder on the right has scale marks 0.1 mL apart, so it can be read to the nearest 0.01 mL.

13. Significance in Measurement

14. Signficance in Measurement Numbers obtained by counting (exact numbers) have no uncertainty unless the count is very large. Conversion factors are exact numbers and have no uncertainty. – Conversions (3 feet = 1 yard)

15. Sig fig rules 1.Non-zero digits and zeros between non-zero digits are always significant. Example: 145.6 grams has 4 sig figs 10405.6 has 6 sig figs 15

16. 2.Leading zeros are not significant. Example: 0.001456 has 4 sig figs 0.000000000742 has 3 sig figs 16

17. 3.Zeros to the right of all non-zero digits are only significant if a decimal point is shown. Example: 993.000 has 6 sig figs 993,000 has 3 sig figs 17

18. 4.For values written in scientific notation, the digits in the coefficient are significant. Example: 4.65 x 10 8 has 3 sig figs 4.650 x 10 8 has 4 sig figs 18

19. Measurement Activity 19

20. Scientific notation 20

21. Scientific notation Expresses numbers as a coefficient multiplied by a base raised to a power. Example: 456 = 4.56 x 10 2 Positive exponents indicate that a value is greater than 1. 0.00456 = 4.56 x 10 -3 Negative exponents indicate that a value is less than 1. 21

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23. Did you hit the target = accurate Did you hit it everytime = precise Did you do both = accurate and precise 23

24. Accuracy & Precision Three different groups of students measure the mass of a medal, with a known value of 5.000 grams. Evaluate each group’s data for its accuracy and precision (low or high): Trial 15.003 g Trial 25.002 g Trial 35.001 g Trial 15.400 g Trial 25.202 g Trial 35.905 g Trial 15.503 g Trial 25.499 g Trial 35.501 g Group 2Group 1Group 3 Accuracy ______ Precision ______ Accuracy ______ Precision ______ Accuracy ______ Precision ______ high low high low

25. Which set of data is valid Data that is both accurate and precise Trial 15.003 g Trial 25.002 g Trial 35.001 g Trial 15.400 g Trial 25.202 g Trial 35.905 g Trial 15.503 g Trial 25.499 g Trial 35.501 g Group 2Group 1Group 3 Accuracy ______ Precision ______ Accuracy ______ Precision ______ Accuracy ______ Precision ______ high low high low

26. Density Activity 26

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28. Density Which container is more dense? Which container has more mass? Which container has more volume? 28

29. Density 1.Which container is more dense? 2.Which container has more mass? 3.Which container has more volume? 4.If you cut sample B in half, what happens to the: a)Mass of B? b)Volume of B? c)Density of B? 29

30. Density TRUE OR FALSE 1.Mass of A is greater than Mass of B. 2.Mass of A is greater than Mass of C. 3.Mass of B is greater than Mass of C. 4.Volume of A is less than Volume of B. 5.Volume of A is less than Volume of C. 6.Volume of B is less than Volume of C. 7.Density of A is greater than Density of B. 8.Density of B is greater than Density of C. 30 B A c

31. Density of water Density of water is 1.00 g/ml or 1.00 g/cm 3 31 1 cm 3 = 1 mL = 1 cc

32. Density calculations. Find the density of a material that has a mass of 137.5 grams and takes up 26.5 cubic centimeters of space. Include: formula, substitution, and answer with units 32

33. Density calculations What is the density of the solution in the container? Include: formula, substitution, and answer with units More practice 33 = 187.2 g = 21.7 cm 3

34. K density calculation example The density of magnesium is 1.7 g/cm 3, and the density of iron is 7.9 g/cm 3. Consider a block of iron with a mass of 819 g. What is the mass of a block of magnesium that has the same volume as the block of iron? A) 1.8 x 10 2 g B) 61 g C) 2.8 x 10 3 g D) 3.8 x 10 3 g 34

35. Density graph activity for K 35

36. Density graph Calculate the density of the substance. Include: formula, substitution, and answer with units 36

37. Density graph Key points: – Best fit line – Outliers – Error associated with measurement 37

38. Review Brain pop movie (measuring matter and property changes) http://glencoe.mcgraw- hill.com/sites/0078600510/student_view0/brain pop_movies.html# Tutorial and online practice 38

39. Computer DA activity Joneslhs.weebly.com 39

40. Dimensional Analysis An organized method for converting between units. Uses “conversion factors” – Example: 1000 m = 1 km – Can be written as a fraction: 1000m/1km or 1 km/1000m 40

41. Dimensional Analysis 41

42. Conversion Factors Base Unit = Meters, Liters and Grams 1 Base Unit = 1000 Milli Units 1000 Base Units = 1 Kilo Units 1 Base Unit = 100 Centi Units 42

43. Conversion practice 1.1256 mg = ________ g 2.14 kg = __________ g 3.1.89 L = __________ mL 43

44. 4.109 g = __________ kg *5. 160 cL = __________ mL *6. 250 km = __________ mm 44

45. In chemistry, the term used to describe how much matter we have is the…..

46. What’s a Mole? 1 mole = 6.02 X 10 23 particles AtomsAtoms 6.02 x 10 23 particles Smallest particle of an element that maintains the identity (#protons) of that element.

47. How big is a Mole? http://www.youtube.com/watch?v=TEl4jeETVmg http://www.youtube.com/watch?v=TEl4jeETVmg (4:32)

48. Mole Practice

49. Physical Changes Usually involve small amounts of energy (compared to chemical changes) Involve the particles moving closer together or farther apart Don’t change the identity of the substance Only change physical properties of substance 49

50. Physical change examples – all phase changes – changing size or shape – warming or cooling – Dissolving 50

51. Chemical Changes involve more energy than physical changes Result in a different substance than you started with 51

52. Mini Activity chemical change 52

53. Chemical change indicators (only need one, but more than one may be seen) – Formation of a gas (will see bubbles) – Formation of a precipitate (an insoluble substance) – Formation of a new odor – Release of light (energy) – Internal temperature change(hotter or colder) – Unexpected color change 53