1. Chapter 1 Introduction: Matter and Measurement

2. Chemistry:
The study of matter and the changes it undergoes.

3. Scientific Method:
A systematic approach to solving problems.

4. Matter:
Anything that has mass and takes up space.

5. Matter
Atoms are the building blocks of matter.

6. Matter Atoms are the building blocks of matter.
Each element is made of the same kind of atom.

7. Matter Atoms are the building blocks of matter.
Each element is made of the same kind of atom.
A compound is made of two or more different kinds of elements.

8. States of Matter

9. Classification of Matter

10. Classification of Matter

11. Classification of Matter

12. Classification of Matter

13. Classification of Matter

14. Classification of Matter

15. Classification of Matter

16. Classification of Matter

17. Classification of Matter

18. Classification of Matter

19. Mixtures and Compounds

20. Properties and Changes of Matter

21. Properties of Matter Physical Properties: Chemical Properties:
Can be observed without changing a substance into another substance.
Boiling point, density, mass, volume, etc.
Chemical Properties:
Can only be observed when a substance is changed into another substance.
Flammability, corrosiveness, reactivity with acid, etc.

22. Properties of Matter Intensive Properties: Extensive Properties:
Independent of the amount of the substance that is present.
Density, boiling point, color, etc.
Extensive Properties:
Dependent upon the amount of the substance present.
Mass, volume, energy, etc.

23. Changes of Matter Physical Changes: Chemical Changes:
Changes in matter that do not change the composition of a substance.
Changes of state, temperature, volume, etc.
Chemical Changes:
Changes that result in new substances.
Combustion, oxidation, decomposition, etc.

24. Chemical Reactions
In the course of a chemical reaction, the reacting substances are converted to new substances.

25. Chemical Reactions

26. Compounds
Compounds can be broken down into more elemental particles.

27. Electrolysis of Water

28. Separation of Mixtures

29. Distillation:
Separates homogeneous mixture on the basis of differences in boiling point.

30. Distillation

31. Filtration:
Separates solid substances from liquids and solutions.

32. Chromatography:
Separates substances on the basis of differences in solubility in a solvent.

33. Units of Measurement

34. SI Units Système International d’Unités
Uses a different base unit for each quantity

35. Metric System
Prefixes convert the base units into units that are appropriate for the item being measured.

36. Volume
The most commonly used metric units for volume are the liter (L) and the milliliter (mL).
A liter is a cube 1 dm long on each side.
A milliliter is a cube 1 cm long on each side.

37. Uncertainty in Measurements
Different measuring devices have different uses and different degrees of accuracy.

38. Temperature:
A measure of the average kinetic energy of the particles in a sample.

39. Temperature
In scientific measurements, the Celsius and Kelvin scales are most often used.
The Celsius scale is based on the properties of water.
0C is the freezing point of water.
100C is the boiling point of water.

40. Temperature The Kelvin is the SI unit of temperature.
It is based on the properties of gases.
There are no negative Kelvin temperatures.
K = C

41. Temperature
The Fahrenheit scale is not used in scientific measurements.
F = 9/5(C) + 32
C = 5/9(F − 32)

42. Physical property of a substance
Density:
Physical property of a substance d= m V

43. Uncertainty in Measurement

44. Significant Figures
The term significant figures refers to digits that were measured.
When rounding calculated numbers, we pay attention to significant figures so we do not overstate the accuracy of our answers.

45. Significant Figures All nonzero digits are significant.
Zeroes between two significant figures are themselves significant.
Zeroes at the beginning of a number are never significant.
Zeroes at the end of a number are significant if a decimal point is written in the number.

46. Significant Figures
When addition or subtraction is performed, answers are rounded to the least significant decimal place.
When multiplication or division is performed, answers are rounded to the number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation.

47. Accuracy versus Precision
Accuracy refers to the proximity of a measurement to the true value of a quantity.
Precision refers to the proximity of several measurements to each other.

48. Review Learned Skills Define accuracy Define precision
Operations with Scientific Notation
Significant digits

49. Review Learned Skills
Accuracy – how close to the actual true value you are.
Precision – how close your measurements are to each other.

50. Review Learned Skills Operations with Scientific Notation
Addition (exponents must be the same)
Subtraction (exponents must be the same)
Multiplication (add exponents)
Division (subtract exponents)

51. Review Learned Skills Significant digits
123.5 ( four significant digits)
12, (six significant digits)
(2 significant digits)
14,000 (2 significant digits)
6.022 x (four significant digits)

52. Review Learned Skills Significant digits in calculations
In multiplication and division the answer must contain the fewest significant figures.
Example
4.38 meters x 3.1 meters = or 14 m2
2.85 cm x 7.2 cm = or 21 cm2

53. Review Learned Skills Significant digits in calculations
In addition and subtraction the result must have the same number of decimal places as the one with the fewest decimal places.
Example
4.38 meters meters = or 7.5 m
2.85 cm cm = or cm

54. Dimensional Analysis Method of managing multiple levels of conversion
Used to organize solutions to chemistry problems

55. Compound Calculations
Utilize derived formulas to determine the resulting calculations.
Utilize dimensional analysis to determine the appropriate units

56. Compound Calculations
Example
What is the area of a rectangular that is 10.3m long and 3.7m wide. Provide the answer in cm2.
Area = length x width

57. Dimensional Analysis
What is the area of a rectangular that is 10.3m long and 3.7m wide. Provide the answer in cm2.
10.3m m cm2 m2

58. Dimensional Analysis
10.3m m cm x 103 cm2 m2

59. Dimensional Analysis Practice
Example
What is the average speed of an object that travels 1856 meters in 900 seconds. Provide the answer in Kilometers.
Average speed = distance / time

60. Dimensional Analysis
What is the average speed of an object that travels 1856 meters in 900 seconds. Provide the answer in Kilometers.
1856 m Km
900 s m

61. Dimensional Analysis 1856 m 1 Km 1856 Km 900 s 1000 m 900,000 s
2.06 x Km/s

62. Dimensional Analysis Practice
Example
What is the average acceleration of an object that travels 956 meters in 200 seconds. Provide the answer in Kilometers.
Average speed = distance / time
Acceleration = Average speed / time

63. Dimensional Analysis Practice
What is the average acceleration of an object that travels 956 meters in 200 seconds. Provide the answer in Kilometers.
956 m Km
200 s s m

64. Dimensional Analysis Practice
956 m Km x Km/s2
200 s s m

65. Complex Compound Calculations
Example
Using the ideal gas law what is the pressure in
Torr of 2 moles of gas at 298 K that fills a
container totaling 1.5 L.
PV = NRT
P (atm) V (liters) = N R (L atm/mol K) T (Kelvin)

66. Dimensional Analysis
Using the ideal gas law what is the pressure in Torr of 2 moles of gas at 298 K that fills a container totaling 1.5 L.
2.0 mol L atm K torr
1.5 L mol K
P = NRT V

67. Dimensional Analysis 2.47 x 104 Torr
2.0 mol L atm K torr , torr
1.5 L mol K atm
2.47 x 104 Torr

68. Complex Compound Calculations Practice
Example
Using the ideal gas law what is the volume in milliliters of 3 moles of gas at 200 K at a pressure of 3 atmospheres.
PV = NRT
P (atm) V (liters) = N R (L atm/mol K) T (Kelvin)

69. Dimensional Analysis Practice
Using the ideal gas law what is the volume in milliliters of 3 moles of gas at 200 K at a pressure of 3 atmospheres
3.0 mol L atm K ml
3 atm mol K L

70. Dimensional Analysis Practice
3.0 mol L atm K ml
3 atm mol K L
1.64 x 104 ml

71. Complex Compound Calculations Group work
Example
A specific type of ore contains 10 grams of gold per 1000 kg. of ore. If gold is worth $400 an ounce, what mass of ore must be mined to obtain $ 1,000,000?
(28.35 grams = 1 ounce)

72. Dimensional Analysis Practice
A specific type of ore contains 10 grams of gold per 1000 kg. of ore. If gold is worth $400 an ounce, what mass of ore must be mined to obtain $ 1,000,000?
(28.35 grams = 1 ounce)
$1 x oz AU g kg ore $ oz g AU

73. Dimensional Analysis Practice
A specific type of ore contains 10 grams of gold per 1000 kg. of ore. If gold is worth $400 an ounce, what mass of ore must be mined to obtain $ 1,000,000?
(28.35 grams = 1 ounce)
$1 x oz AU g kg ore $ oz g AU
7.09 x 106 kg ore