1. Chemistry is a team sport!
Come to class
prepared
to participate!
Chemistry is a team sport!
Be on time and here
for all classes!
Practice is required!

2. Building A Conceptual Understanding
Building A Conceptual Understanding
Microscopic –
the particulate nature of matter
The atomic level
(abstract)
Symbolic – mathematical equation or chemical equation
Macroscopic - observations or results of an experiment
How we represent it
The visible world or
How we SEE it

3. A Brief History of Chemistry

4. Approx. 15 Billion Years Ago
BANG !

5. What is the most important chemical reaction on Earth?

6. Photosynthesis
6 CO2 + 6 H2O  C6H12O6 + 6 O2

7. What were some of the first chemical transformations undertaken by humans?

9. Respiration (digestion)
C6H12O6 + 6 O2  6 CO2 + 6 H2O
Glucose

11. Combustion Reaction (Ideal)
CxHy + O2  CO2 + H2O

13. Making beer from barley in ancient Egypt - 4000 BC

14. Fermentation
C6H12O6  2 C2H5OH + 2 CO2
Glucose
Ethanol

16. Smelting of Copper BC

19. SMELTING
CuO + C CO2 + Cu

21. Bronze Age BC

22. Iron Age BC

24. Soap AD

26. Greek Philosophers (400 - 300 BC)
Democritus
Aristotle

27. Alchemy

28. Herbal medicines

29. Gunpowder

30. Age of steel

32. What has modern chemical knowledge and research brought to the world?

33. Phenol - First Antiseptic

34. Discovery of chloroform for anesthesia

37. Salicylic acid (first extracted from the bark of the Willow tree)

38. Acetyl salicylic acid (“Aspirin” or ASA)

40. H H
morphine

47. The Age of Plastics (Polymers)

49. Unit Conversions MEASUREMENT
Dimensional Analysis, Scientific Notation, Significant Figures, Density, Percent Error

50. A. SI Prefix Conversions
Symbol
Factor
mega- M
106
kilo- k
103
BASE UNIT
---
100
deci- d
10-1
move left
move right
centi- c
10-2
milli- m
10-3
micro- 
10-6
nano- n
10-9
pico- p
10-12

51. Mnemonic Device Kids Have Dirty Mouths, Lips, Gums Drinking Chocolate
Milk
Many
Never
Pretend

52. Chemistry Reference Table - Table C

53. A. SI Prefix Conversions
0.2
1) 20 cm = ______________ m
2) L = ______________ mL
3) 45 m = ______________ nm
4) 805 dm = ______________ km 32
45,000
0.0805

54. Packet page 1

55. B. Dimensional Analysis
The “Factor-Label” Method
Units, or “labels” are canceled, or “factored” out

56. B. Dimensional Analysis
Steps:
1. Identify starting & ending units.
2. Line up conversion factors so units cancel.
3. Multiply all top numbers & divide by each bottom number.
4. Check units & answer.

57. B. Dimensional Analysis
Lining up conversion factors:
= 1
1 in = 2.54 cm
2.54 cm cm
1 =
1 in = 2.54 cm
1 in in

58. B. Dimensional Analysis
How many milliliters are in 1.00 quart of milk? qt mL
1.00 qt
1 L
1.057 qt
1000 mL
1 L
= 946 mL 

59. B. Dimensional Analysis
You have 1.5 pounds of gold. Find its volume in cm3 if the density of gold is 19.3 g/cm3. lb
cm3
1.5 lb
1 kg
2.2 lb
1000 g
1 kg
1 cm3
19.3 g
= 35 cm3

60. Packet Page 2-3
Homework finish pages 2-3

61. Scientific Notation A short-hand way of writing large numbers without
writing all of the zeros.

62. The Distance From the Sun to the Earth
93,000,000

63. Step 1 93,000,000 = 9.3000000 Move decimal left
Leave only one number in front of decimal
93,000,000 =

64. Step 2
Write number without zeros
93,000,000 = 9.3

65. Step 3 7 93,000,000 = 9.3 x 10 Count how many places you moved decimal
Make that your power of ten
93,000,000 = 9.3 x 10 7

66. The power of ten is 7 because the decimal moved 7 places. 7
93,000,000 = 9.3 x 10 7

67. 93,000, Standard Form
9.3 x Scientific Notation

68. Practice Problem -----> -----> -----> ----->
Write in scientific notation.
Decide the power of ten.
98,500,000 = 9.85 x 10?
64,100,000,000 = 6.41 x 10?
279,000,000 = 2.79 x 10?
4,200,000 = 4.2 x 10?
9.85 x 107
----->
6.41 x 1010
----->
2.79 x 108
----->
----->
4.2 x 106

69. Scientific Notation to Standard Form
Move the decimal to the right
3.4 x 105 in scientific notation
move the decimal
--->
340,000 in standard form

70. Move the decimal to the right.
Write in Standard Form
Move the decimal to the right.
6.27 x 106
9.01 x 104
6,270,000
90,100

71. Homework Page 5

72. DETERMINING SIGNIFICANT FIGURES
Crunching numbers with accuracy and precision

73. BEFORE YOU CAN CRUNCH You must know which digits are significant
Because they are going to control the number of digits in a calculated figure
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74. WHAT IS A SIGNIFICANT FIGURE?
Significant figures are all the digits in a measurement that are known with certainty plus a last digit that must be estimated.
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75. Page 16

76. Now you try How many significant digits in each of the following:
12 apples
3000 m
69 people
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77. Answers 1.034 s - 4 significant figures
g significant figures
12 apples exact number
3000 m significant figure
69 people exact number
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78. CALCULATING WITH SIGNIFICANT FIGURES
Crunching numbers with accuracy and precision

79. SIGNIFICANT FIGURES Are important in calculations.
Significant figures tell you when and where to round.
The number of digits in a calculated number is dependent on the significant figures of the terms used in the calculation.
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80. ROUNDING
Rounding in science is different than in math. What if the digit to be dropped is:
>5  round previous digit up one
<5  do not change previous digit
= 5
If the previous digit is even, do not change it
If the previous digit is odd, round it up to make it even
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81. ROUNDING EXAMPLES – Round to 3 significant figures 12.379 cm = 12.4 cm
L = 356 L
g = g
s = 1.68 s
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82. Now you try Round to the nearest tenths place 15.265 m 1.33 s 0.9543 gcm L kg
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83. Answers
m m
1.33 s s
g g
cm cm
L L
kg kg
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84. CRUNCHING NUMBERS Multiplication and Division Addition and Subtraction
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85. MULTIPLICATION AND DIVISION
An answer has the same number of significant figures as the number in the least precise measurement used in the calculation.
36 cm x 1.03 cm = cm2
36 is the least precise measurement with 2 significant figures. Therefore the answer can have only 2 significant figures
The answer is 37 cm2
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86. ADDITION AND SUBTRACTION
The answer has the same number of decimal places as the least precise measurement used in the calculation.
12.11
 Limiting term has one decimal place
1.013
Corrected to (one decimal place)
The correct result is 31.1, since 18.0 has only one decimal place.
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87. Now you try 0.356 kg x 1.5 m 1.234 g + 0.67 g + 13.2 g 101 g / 0.33 mL
15.27 s – s
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88. Answers
0.356 kg x 1.5 m = kgm
1.234 g g g = 15.1 g
101 g / 0.33 mL = 310 g/mL
15.27 s – s = s
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89. Homework page 18 & 20

90. MEASUREMENT
I. Using Measurements

91. A. Accuracy vs. Precision
Accuracy - how close a measurement is to the accepted value
Precision - how close a series of measurements are to each other
ACCURATE = CORRECT
PRECISE = CONSISTENT

92. B. Percent Error your value accepted value
Indicates accuracy of a measurement
your value
accepted value

93. B. Percent Error % error = 2.9 %
A student determines the density of a substance to be 1.40 g/mL. Find the % error if the accepted value of the density is 1.36 g/mL.
% error = 2.9 %

94. D. Density V = 825 cm3 M = DV D = 13.6 g/cm3 M = (13.6 g/cm3)(825cm3)
An object has a volume of 825 cm3 and a density of 13.6 g/cm3. Find its mass.
GIVEN:
V = 825 cm3
D = 13.6 g/cm3
M = ?
WORK:
M = DV
M = (13.6 g/cm3)(825cm3)
M = 11,200 g

95. D. Density D = 0.87 g/mL V = M V = ? M = 25 g V = 25 g 0.87 g/mL
A liquid has a density of 0.87 g/mL. What volume is occupied by 25 g of the liquid?
GIVEN:
D = 0.87 g/mL
V = ?
M = 25 g
WORK:
V = M D
V = g
0.87 g/mL
V = 29 mL