1. CHE 106: General Chemistry
CHAPTER ONE
Copyright © James T. Spencer
All Rights Reserved

2. Matter What is Chemistry Benefits of Chemistry Why Study Chemistry
Study of the “Physical” Properties Matter (Form and Function)
Study of How Matter Changes (Reactivity)
Benefits of Chemistry
Pharmaceuticals
Enhanced food production (fertilizers, herbicides, etc...)
Plastics and Polymers
Why Study Chemistry
Core requirement (?)
Central Science
Employment
Many fields
BIO
Physics
Medicine
GEO
Engr
CHEM
Law
also: environmental
economics
electronics
agriculture
politics
etc...
S.U.
B.S.
Chapt. 1.1

3. Chemistry; Common Chemicals
acetic acid vinegar
calcium hypochloride bleaching powder
calcium sulfate plaster of paris
carbon tetrachloride cleaning fluid
ferric oxide iron rust
graphite pencil lead
magnesium sulfate Epsom salts
naphthalene mothballs
silicon dioxide sand
sodium bicarbonate baking soda
sodium borate borax
sodium hydroxide lye
sulfuric acid battery acid
sucrose cane sugar

4. Chemistry; Chemical Production
H2SO4
1995
Chemical and Engineering News N2 O2
C2H4
CaO
NH3
H3PO4
C3H6
NaOH
Cl2

5. Nanoscale Chemistry
Use simpler molecular units are molecular-architectural elements

6. Nanoscale Chemistry

7. Nanosystems

8. Nanomachines
Interstellar Space Travel - Significant concepts in this area include: launch vehicles, the space elevator, interplanetary transportation, the swarm concept, smart dust, extraterrestrial materials utilization, terraforming, suspended animation, space telescopes and virtual sample return.
Human Therapeutics - Nanotechnology has caused scientists to re-examine the problems of the human body from the perspective of atomic- engineering. By assuming a nanotechnological
red blood cell
point of view, the resolution of therapeutic ailments becomes simple.
Nano-Robots and Nano-Computers with advanced Artificial Intelligence - Nanotechnology will operate under the control of nano-sized computers which will manage the process of Molecular Manufacturing. In order to achieve this, it will be necessary to devise advanced Artificial Intelligence that will be able to automate and regulate Molecular Manufacturing systems.

9. Matter; A Review Definition of Matter States Forms Properties
anything that occupies space and has mass
States
gas (vapor); no fixed volume or shape, compressable
liquid; fixed volume no fixed shape, mostly incompressable
solid; fixed volume and shape, incompressable
Forms
Substances (pure or single); has a fixed composition and distinct properties. Most things encountered are mixtures of substances.
Properties
Physical Properties; can be measured without changing the substance, i.e., color, density, melting point, etc...
Chemical Properties; the way a substance changes (reacts), i.e., combustion
Chapt. 1.1

10. Matter; A Review Chemical Changes Physical Changes burning melting
Physical - Changes in appearance but not identity, i.e., evaporation, melting (all changes of state)
Chemical - transformation into a different substance
Chemical Changes Physical Changes
burning melting
C6H12O6 + 6O CO2 + 6H2O H2O(s) H2O(l)
chemical reactions sublimation
NaOH + HCl H2O + NaCl H2O(s) H2O(g)
corrosion dissolution
4Fe + 3O Fe2O H2O(l ) + NaCl(s) NaCl(aq)
Chapt. 1.1

11. Matter; A Review Mixtures; combinations of substances
Mixture- combination of two or more substances in which each retains its own chemical identity (and properties). Vary widely by composition (infinite possibilities of combining ratios), can be separated using the different physical properties of the component substances.
Homogeneous - appears the same throughout (solutions), liquid, gas and solid solutions are possible.
Heterogeneous - mixtures which do not have the same (uniform) appearance throughout.
Chapt. 1.1

12. Matter; A Review Salt and Sand Mixture Ink from Cabbage Juice
solubility and filtration chromatography
Water from Salt Water Iron and Gold Mixture
distillation magnetic properties
melting point differences
chem. reactivity (acids)
Iodine from Copper Chloride
solubility and filtration
Separating Mixtures using Physical Properties
How would you separate;
Chapt. 1.1

13. Matter; A Review Filtration Sand from Salt
Separating Mixtures using Physical Properties
How would you separate;
Flow
Filter
Everyday Examples;
Auto Oil Filter
Auto Air Filter
Aquarium Water Filter
Spaghetti Strainer
Window Screens
Registrar
Chapt. 1.1

14. Matter; A Review NaCl(s) + H2O(l) NaCl(aq) Distillation
Water from Salt Water
Separating Mixtures using Physical Properties
How would you separate;
NaCl(s) + H2O(l)
NaCl(aq)
Chapt. 1.1

15. Matter; A Review Chromatograpgy Dyes from M&M’s
Separating Mixtures using Physical Properties
How would you separate;
Before After
Dyes
Chapt. 1.1

16. Matter; Elements and Compounds
Substances
Elements - substances which cannot be decomposed into simpler substances (see periodic table)
Compounds- substances which can be separated into two or more elements
Elements
110 Known (periodic table to be revisited)
make up all matter and composed of “subatomic particles”
symbols used for abbreviations (from older or common names)
Compounds
Elements combined in a definite proportion by mass (law of definite proportion)
properties different than consititutent elements
Water; example of mixtures, compound and elements?
Chapt. 1.2

17. Matter; Elements and Periodic Table
See Website:

18. Matter Matter Uniform ? Heterogeneous Mixture HomogeneousNo
Yes
Uniform ?
Heterogeneous
Mixture
Homogeneous No
Can be separated
by physical methods
Pure Substance
Yes
Decomposed ?
Homogeneous
Mixture (solution) No
Yes
Element
Compound

19. Scientific Method Theory Form and test hypothesis Patterns and Trends
Observations
and Experiments

20. Observations to Theory
Observations Theory

21. Observations to Theory
Observations Theory

22. Observations to Theory
Observations Theory

23. Matter; Measurement A B
Which is True?
A = B
A > B
A < B

24. Matter; Measurement A B
Which is True?
A = B
A > B
A < B

25. Matter; Measurement A B
Which is True?
A = B
A > B
A < B

26. Matter; Measurement Systems Metric - base 10
SI- international scientific system
mass Kilogram
length Meter
time Second
electric current Ampere
temperature Kelvin
light Candela
Amount Mole
Factor label method for conversions
Chapt. 1.3

27. Matter; Measurement Kilo k 103 Deci d 10-1 Centi c 10-2 Milli m 10-3
Prefixes
Mega M 106
Kilo k 103
Deci d 10-1
Centi c 10-2
Milli m 10-3
Micro  10-6
Nano n 10-9
Chapt. 1.3

28. Matter; Measurement
Sample exercise: What fraction of a second is a picosecond, ps?
Chapt. 1.3

29. Matter; Measurement
Sample exercise: What fraction of a second is a picosecond, ps?
10-12 second
Chapt. 1.3

30. Matter; Measurement Common Units: Length and Mass
Length - unit of distance measured in meters
Mass - measures the amount of matter in an object in grams
Temperature
Kelvin
Celsius °C = 5/9 (°F -32) K = °C
Chapt. 1.3

31. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F
Chapt. 1.3

32. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F K = °C =
Chapt. 1.3

33. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F K = °C =
= K
Chapt. 1.3

34. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F K = °C =
= K
= K
Chapt. 1.3

35. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F -32)
Chapt. 1.3

36. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
Chapt. 1.3

37. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
9(-11.5) = x 5
Chapt. 1.3

38. Matter; Measurement
Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in
a) K
b) °F °C = 5/9 (°F - 32)
-11.5 = 5/9(x - 32)
9(-11.5) = x 5
11.3°F = x
Chapt. 1.3

39. Matter; Measurement Derived Units: Volume Length x length x length
measured in cm3, which is equal to mL
Chapt. 1.3

40. Matter; Measurement Derived Units: Density
amount of mass per unit volume
measured in g/cm3, or g/mL
Chapt. 1.3

41. Matter; Measurement
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is g/mL, how many milliliters of alcohol are needed?
Chapt. 1.3

42. Matter; Measurement
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
Chapt. 1.3

43. Matter; Measurement
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
= 15.0 g g/mL
Chapt. 1.3

44. Matter; Measurement
Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is g/mL, how many milliliters of alcohol are needed?
D = m/V so V = m/D
= 15.0 g g/mL
= 19.0 mL
Chapt. 1.3

45. Matter; Uncertainty in Measurement
Precision and Accuracy
Precision - how closely individual measurements agree
Accuracy- how closely the measurements agree with the true value
Significant Figures
All measurements are inaccurate intrinsically
measured quantities are reported such that the last figure is uncertain
Chapt. 1.4

46. Matter; Uncertainty in Measurement
Good Precision
Poor Accuracy
Good Precision
Good Accuracy
Poor Precision
Poor Accuracy

47. Matter; Uncertainty in Measurement
Determining Significant Figures
all non zero digits are significant
zeros between nonzero digits are significant
zeros to the left of first nonzero digit are not significant
zeros at the end of a number and to the right of a decimal point are significant
when a number ends in a zero but with no decimal point, the zero may or may not be signigicant (use scientific notation)
Chapt. 1.4

48. Matter; Uncertainty in Measurement
Determining Significant Figures
3.573 has 4 significant figures
0.073 has 2 significant figures
3.070 has 4 significant figures
0.003 has 1 significant figures
- multiplication and division; result can have no more than the figure with the fewest significant figures
- addition and subtraction; result can have the same number of decimal places as the term with the least number of decimal places
Chapt. 1.4

49. Matter; Uncertainty in Measurement
Sample exercise: A balance has a precision of g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
Chapt. 1.3

50. Matter; Uncertainty in Measurement
Sample exercise: A balance has a precision of g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
25.XXX
Chapt. 1.3

51. Matter; Uncertainty in Measurement
Sample exercise: A balance has a precision of g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement?
25.XXX
5 sig figs
Chapt. 1.3

52. Matter; Uncertainty in Measurement
Sample exercise: How many significant figures are in each of the following measurements?
A) g
B) 2.3 x 104 cm
C) m3
Chapt. 1.3

53. Matter; Uncertainty in Measurement
Sample exercise: How many significant figures are in each of the following measurements?
A) g 4 sig figs
B) 2.3 x 104 cm
C) m3
Chapt. 1.3

54. Matter; Uncertainty in Measurement
Sample exercise: How many significant figures are in each of the following measurements?
A) g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) m3
Chapt. 1.3

55. Matter; Uncertainty in Measurement
Sample exercise: How many significant figures are in each of the following measurements?
A) g 4 sig figs
B) 2.3 x 104 cm 2 sig figs
C) m3 3 sig figs
Chapt. 1.3

56. Matter; Uncertainty in Measurement
Sample exercise: There are exactly m in a mile. How many meters are in a distance of 1.35 mi?
Chapt. 1.3

57. Matter; Uncertainty in Measurement
Sample exercise: There are exactly m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = mi
x m
Chapt. 1.3

58. Matter; Uncertainty in Measurement
Sample exercise: There are exactly m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = mi
x m
x = m
Chapt. 1.3

59. Matter; Uncertainty in Measurement
Sample exercise: There are exactly m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = mi
x m
1.35 has 3 sig figs x = m has 7 sig figs is infinitely significant
Chapt. 1.3

60. Matter; Uncertainty in Measurement
Sample exercise: There are exactly m in a mile. How many meters are in a distance of 1.35 mi?
1.35 mi = mi
x m
1.35 has 3 sig figs x = m has 7 sig figs x = 2170 m is infinitely significant
Chapt. 1.3

61. Dimensional Analysis
Use Units throughout the calculation (helps “guide” calculation.
Should always yield the proper units
Uses conversion factors
Example; How fast is 50 mph in in/sec.?
50 mi. 1 hour 5280 ft 12 in = in
1 hour 3600 sec. 1 mi. 1 ft sec.

62. Dimensional Analysis
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a mi automobile race.
Chapt. 1.3

63. Dimensional Analysis
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a mi automobile race.
500.0 mi
Chapt. 1.3

64. Dimensional Analysis
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a mi automobile race.
500.0 mi 1 km mi
Chapt. 1.3

65. Dimensional Analysis
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a mi automobile race.
500.0 mi 1 km = km mi
Chapt. 1.3

66. Dimensional Analysis
Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a mi automobile race.
500.0 mi 1 km = km mi
* answer can only have 4 sig figs; km
Chapt. 1.3

67. Dimensional Analysis
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
Chapt. 1.3

68. Dimensional Analysis
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm
Chapt. 1.3

69. Dimensional Analysis
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm m mm
1012 pm m
Chapt. 1.3

70. Dimensional Analysis
Sample exercise: The distance between carbon atoms in a diamond is 154 pm. Convert this distance to millimeters.
154 pm m mm = 1.54 x 10-7 mm
1012 pm m
Chapt. 1.3

71. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
Chapt. 1.3

72. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi
gal
Chapt. 1.3

73. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi km
gal mi
Chapt. 1.3

74. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi km gal
gal mi L
Chapt. 1.3

75. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi km gal = km
gal mi L L
Chapt. 1.3

76. Dimensional Analysis
Sample exercise: A car travels 28 mi to the gallon of gasoline. How many kilometers per liter will it go?
28 mi km gal = km
gal mi L L
* 2 sig figs = 12 km L
Chapt. 1.3

77. Chapter One; Review Matter: Chemical and Physical Changes
Elements and Compounds
Units of Measurement
Uncertainty and Significant Figures
Precision and Accuracy
“Factor Label” Method (Dimensional Analysis)