1. Welcome to ACE Chemistry…
I hope you are ready to work hard this year 

2. Chapter 1 Chemistry and Measurement

3. Chemistry is a Foreign Language

4. What is your definition of Chemistry?
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5. Chemistry
The study of the composition and structure of materials and of the changes that materials undergo.
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6. What is the scientific method?
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7. Scientific Method
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8. What is matter?
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9. Whatever occupies space and can be perceived by our senses.
Matter
Whatever occupies space and can be perceived by our senses.
Mass
The quantity of matter in a material.
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10. What is the Law of Conservation of Mass?
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11. Law of Conservation of Mass
Antoine Lavoisier (French chemist)
Mass cannot be created or destroyed in a chemical reaction
The total mass remains constant
Energy and mass are related through Einstein’s formula E = mc2 so that very small amounts of mass may be converted into energy

12. aluminum + oxygen = aluminum oxide
Aluminum powder burns in oxygen to produce a substance called aluminum oxide. A sample of 2.00 grams of aluminum is burned in oxygen and produces 3.78 grams of aluminum oxide. How many grams of oxygen were used in this reaction?
aluminum + oxygen = aluminum oxide
2.00 g + oxygen = 3.78 g
oxygen = 1.78 g
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13. What are the States of Matter?
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14. Solid: characterized by rigidity; fixed volume and fixed shape.
States of Matter
Solid: characterized by rigidity; fixed volume and fixed shape.
Liquid: relatively incompressible fluid; fixed volume, no fixed shape.
Gas: compressible fluid; no fixed volume, no fixed shape.
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16. What is a Physical Change?
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17. A change in the form of matter but not in its chemical identity.
Physical Change
A change in the form of matter but not in its chemical identity.
For example:
Melting
Dissolving
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18. What is a chemical change?
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19. Chemical Change = Chemical Reaction
A change in which one or more kinds of matter are transformed into a new kind of matter or several new kinds of matter
For example:
Rusting
Burning
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20. Physical Property
A characteristic that can be observed for a material without changing its chemical identity.
For example:
Physical state
Boiling point
Color
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21. What is the difference between a physical and chemical property?
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22. A characteristic of a material involving its chemical change.
Chemical Property
A characteristic of a material involving its chemical change.
For example:
Ability to react with oxygen
Ability to react with fluorine
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23. What is a substance?
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24. Substance
A kind of matter that cannot be separated into other kinds of matter by any physical process such as distillation or sublimation.
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25. Potassium is a soft, silvery-colored metal that melts at 64°C
Potassium is a soft, silvery-colored metal that melts at 64°C. It reacts vigorously with water, with oxygen, and with chlorine. Identify all of the physical properties and chemical properties given in this description.
Physical Property
Chemical Property
Soft
Reacts with water
Silvery-colored
Reacts with oxygen
Melting point (64°C)
Reacts with chlorine
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26. What is an element?
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27. Element
A substance that cannot be decomposed into simpler substances by any chemical reaction.
For example:
Hydrogen
Carbon
Oxygen
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28. What is a compound?
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29. A substance composed of two or more elements chemically combined.
Compound
A substance composed of two or more elements chemically combined.
For example:
Water (H2O)
Carbon dioxide (CO2)
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30. What is a mixture?
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31. Italian salad dressing Saltwater
Mixture
A material that can be separated by physical means into two or more substances
For example:
Italian salad dressing
Saltwater
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32. Heterogeneous Mixture
A mixture that consists of physically distinct parts, each with different properties.
For example:
Salt and iron filings
Oil and vinegar
Phase
One of several different homogeneous materials present in the portion of matter under study.
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33. A mixture that is uniform in its properties; also called a solution.
Homogenous Mixture
A mixture that is uniform in its properties; also called a solution.
For example:
Saltwater
Air
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35. label each figure on the next slide as an element, a compound, or a mixture.
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36. B. Compound (made of two elements) C. Mixture of two elements
A. Element
B. Compound (made of two elements)
C. Mixture of two elements
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37. Measurement
The comparison of a physical quantity with a fixed standard of measurement—a unit.
For example:
Centimeter
Kilogram
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38. Measurements
When making measurements, report all certain numbers plus one estimated number

39. Measurements SI Units (Table 1.2) Length = meter Mass = kilogram
Time = seconds
Temperature = kelvin
* Prefixes are used to identify very small or very large numbers *
Ex: diameter of Na atom = m
distance of earth to sun = 150,000,000,000 m

40. Measurements Prefixes: (memorize) M Mega 106 k kilo 103 c centi 10-2 m
milli
10-3 u
micro
10-6 n
nano
10-9 p
pico
10-12

41. Distinguish between accuracy and precision
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42. Significant Figures Precision – The “reproducibility” of measurements
Accuracy – how close a measured value is to the true value

43. Imagine that you shot five arrows at each of the targets depicted on the next slide. Each “x” represents one arrow. Choose the best description for each target.
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44. 1. Poor accuracy and good precision X
A B C
1. Poor accuracy and good precision
2. Poor accuracy and poor precision
3. Good accuracy and good precision
4. Good accuracy and poor precision
A: 1 B: 2 C: 3
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45. Significant Figures…. Atlantic –Pacific Rule Decimal point present
Decimal point absent
Examples:

46. Significant Figures
Practice Problems: How many significant figures are present in each number?
72,100
6.5 x 104
$25.03
x 10-3

47. (The tenths place is estimated)
What is the length of the nail to the correct number of significant figures?
5.7 cm
(The tenths place is estimated)
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48. Significant Figures Addition/Subtraction = least decimal places
In other words… the answer cannot have more digits to the right of the decimal place than the original number that has the least number of decimal places
Ex: = ?

49. Significant Figures Multiplication/Division = least sig figs
In other words… the answer cannot have more significant figures than the original number with the least significant figures
Ex: = 34.6 x 12.1 x 1.2 = ?

50. Ex: What is the average of 10.2, 11.4, 10.9?
Significant Figures
Exact Numbers = unlimited sig figs
* Do not round your answer based on exact numbers!
Conversions are exact numbers
1 day = 24 hr; 3 ft = 1 yd
Ex: What is the average of 10.2, 11.4, 10.9?

51. Ex: What is the average of 10.2, 11.4, 10.9?
Significant Figures
Exact Numbers = unlimited sig figs
* Do not round your answer based on exact numbers!
Conversions are exact numbers
1 day = 24 hr; 3 ft = 1 yd
Ex: What is the average of 10.2, 11.4, 10.9?

52. Significant Figures
Practice Problems: Report the answer to the correct number of sig figs =
÷ =
((3.41 – 0.237) ÷ 5.233)( ) =

53. Perform the following calculation and round your answer to the correct number of significant figures:
Calculator answer:
The answer should be rounded to three significant figures:
0.734
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54. Perform the following calculation and round your answer to the correct number of significant figures:
Calculator answer:
The answer should be rounded to two decimal places:
-1.14
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55. Perform the following calculation and round your answer to the correct number of significant figures:
Calculator answer:
The answer should be rounded to three decimal places:
0.0350
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56. Perform the following calculation and round your answer to the correct number of significant figures:
Calculator answer:
The answer should be rounded to two significant figures:
3.2
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57. How many significant figures are in each of the following measurements?
a kg
b m
c kg
d x 10-8 m
e s
f. 91,000
4 significant figures
6 significant figures
4 significant figures
2 significant figures
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58. The representation of a number in the form A × 10n 1 ≤ A < 10
Scientific Notation
The representation of a number in the form
A × 10n
1 ≤ A < 10
where n is an integer
Every digit included in A is significant.
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59. Write the following numbers in scientific notation:. 000653. 350,000
6.53 × 10-4
3.5 × 105
2.700 × 10-2
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60. Write the following measurements without scientific notation using the appropriate SI prefix: × 10-9 g × 10-2 m × s
4.851 ng
3.16 cm
8.93 ps
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61. Scientific Notation and Metric Prefixes
Because each of the metric prefixes has an equivalent power of 10, the prefix may be substituted for the power of 10.
For example:
7.9 × 10-6 s
10-6 = micro, m
7.9 × 10-6 s = 7.9 ms
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62. Using scientific notation, make the following conversions:. 6
Using scientific notation, make the following conversions: km to m cm to m ns to s mg to g
6.20 × 103 m
2.54 × 10-2 m
1.98 × 10-9 s
5.23 × 10-6 g
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63. Temperature A measure of the average kinetic energy in a system
K = °C
°C = 5/9 (°F – 32)
Ex. A person with a fever has a temperature of 102.5°F. What is this temperature in °C? In Kelvins?

64. Temperature A measure of “hotness”
Heat flows from an area of higher temperature to an area of lower temperature.
Temperature Units
Celsius, °C
Fahrenheit, °F
Kelvin, K
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66. Converting Between Temperature Units
Finding Kelvin temperature from Celsius temperature.
Finding Fahrenheit temperature from Celsius temperature.
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67. Converting Between Temperature Units
Finding Celsius temperature from Fahrenheit temperature.
Finding Celsius temperature from Kelvin temperature.
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68. In winter, the average low temperature in interior Alaska is -30
In winter, the average low temperature in interior Alaska is -30.°F (two significant figures). What is this temperature in degrees Celsius and in kelvins?
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70. Dimensional Analysis Identify: 1. Given information (w/units)
2. Quantity asked for (w/units)
3. Conversion factors necessary
Conversion factor – a ratio equal to 1 used to change units on a measurement (these are exact numbers)

71. Conversion Factors

72. Practice Problems - Conversions
How many miles are in 77 yards?
(check sig figs)

73. Practice Problems – Squared Units
How many square inches are in 1.00 square miles?
(check sig figs)

74. Practice Problems – Derived Units
How many miles per hour is a car traveling if the current speed is km/min?

75. Density as a Conversion
D = m/v (SI unit = g/mL or g/cm3)
Ex: Aspirin has a density of 1.40 g/cm3. What is the volume (in cm3) of a tablet weighing lb?

76. Percent as a Conversion
Assume a 100 g sample:
Ex: 30% of rubbing alcohol is water means…
30 g water / 100g rubbing alcohol
Ex: A solution of sucrose in water is 28.0% sucrose by mass and has a density of g/mL. What mass of sucrose, in grams, is contained in 3.50 L of this solution?

77. Combinations of fundamental units. For example:
Derived Units
Combinations of fundamental units.
For example:
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78. Definition of Quantity
SI Unit
Area
length × length m2
Volume
length × length × length m3
Density
mass per unit volume
kg/m3
Speed
distance per unit time
m/s
Acceleration
change in speed per unit time
m/s2
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79. Definition of Quantity
SI Unit
Force
mass × acceleration
kg  m/s2 =
N (newton)
Pressure
force per unit area
kg/m  s2 =
Pa (pascal)
Energy
force × distance
kg  m2/s2 =
J (joule)
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80. Density Mass per unit volume Common units solids g/cm3 liquids g/mL
gases g/L
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81. Oil of wintergreen is a colorless liquid used as a flavoring. A 28
Oil of wintergreen is a colorless liquid used as a flavoring. A 28.1-g sample of oil of wintergreen has a volume of 23.7 mL. What is the density of oil of wintergreen?
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82. A sample of gasoline has a density of 0. 718 g/mL
A sample of gasoline has a density of g/mL. What is the volume of 454 g of gasoline?
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83. Units and Dimensional Analysis (Factor-Label Method)
A method of calculations in which one carries along the units for quantities.
Conversion Factor
A factor equal to 1 that converts a quantity expressed in one unit to a quantity expressed in another unit.
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84. A sample of sodium metal is burned in chlorine gas, producing 573 mg of sodium chloride. How many grams and kilograms is this?
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85. An experiment calls for 54. 3 mL of ethanol
An experiment calls for 54.3 mL of ethanol. What is this volume in cubic meters?
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86. The Star of Asia sapphire in the Smithsonian Institute weighs 330 carats (three significant figures). What is this weight in grams? One carat equals 200 mg (exact).
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87. The dimensions of Noah’s ark were reported as 3. 0 × 102 cubits by 5
The dimensions of Noah’s ark were reported as 3.0 × 102 cubits by 5.0 × 101 cubits. Express this size in units of feet and meters. (1 cubit = 1.5 ft)
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