1. Chapter to 1.9
Chemical Foundations

2. 1.9 Classification of Matter
Chapter 1
Table of Contents
1.6 Dimensional Analysis
1.7 Temperature
1.8 Density
1.9 Classification of Matter
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3. Section 1.6
Dimensional Analysis
Use when converting a given result from one system of units to another.
To convert from one unit to another, use the equivalence statement that relates the two units.
Derive the appropriate unit factor by looking at the direction of the required change (to cancel the unwanted units).
Multiply the quantity to be converted by the unit factor to give the quantity with the desired units.
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4. The two unit factors are:
Section 1.6
Dimensional Analysis
Example #1
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
To convert from one unit to another, use the equivalence statement that relates the two units.
1 ft = 12 in
The two unit factors are:
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5. Dimensional Analysis Example #1
Section 1.6
Example #1
Dimensional Analysis
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
Derive the appropriate unit factor by looking at the direction of the required change (to cancel the unwanted units).
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6. Dimensional Analysis Example #1
Section 1.6
Example #1
Dimensional Analysis
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
Multiply the quantity to be converted by the unit factor to give the quantity with the desired units.
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7. Dimensional Analysis Example #2
Section 1.6
Dimensional Analysis
Example #2
An iron sample has a mass of 4.50 lb. What is the mass of this sample in grams?
(1 kg = lbs; 1 kg = 1000 g)
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8. React 3
What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Chicago? Provide estimates of values and a sample calculation.
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9. Dimensional Analysis Concept Check
Section 1.6
Dimensional Analysis
Concept Check
What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.
This problem requires that the students think about how they will solve the problem before they can plug numbers into an equation. A sample answer is:
Distance between New York and Los Angeles: miles
Average gas mileage: 25 miles per gallon
Average cost of gasoline: $2.75 per gallon
(3200 mi) × (1 gal/25 mi) × ($2.75/1 gal) = $352
Total cost = $350
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10. Examples
Because you never learned dimensional analysis, you have been working at a fast food restaurant for the past 35 years wrapping hamburgers. Each hour you wrap 184 hamburgers. You work 8 hours per day. You work 5 days a week. you get paid every 2 weeks with a salary of $ How many hamburgers will you have to wrap to make your first one million dollars?

11. A senior was applying to college and wondered how many applications she needed to send. Her counselor explained that with the excellent grade she received in chemistry she would probably be accepted to one school out of every three to which she applied. She immediately realized that for each application she would have to write 3 essays, and each essay would require 2 hours work. Of course writing essays is no simple matter. For each hour of serious essay writing, she would need to expend 500 calories which she could derive from her mother's apple pies. Every three times she cleaned her bedroom, her mother would make her an apple pie. How many times would she have to clean her room in order to gain acceptance to 10 colleges?

12. Units to a Power 3 How many m3 is 1500 cm3? 1 m 100 cm 1 m 100 cm 1 m

13. Units to a Power
How many cm2 is 15 m2?
36 cm3 is how many mm3?

14. Three Systems for Measuring Temperature
Section 1.7
Temperature
Three Systems for Measuring Temperature
Fahrenheit
Celsius
Kelvin
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15. The Three Major Temperature Scales
Section 1.7
Temperature
The Three Major Temperature Scales
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16. Converting Between Scales
Section 1.7
Temperature
Converting Between Scales
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17. React 4 At what temperature does °C = °F? Prove your answer.
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18. 0ºC is not 0ºF ºF 9 5 ºC

19. (0,32)= (C1,F1) ºF ºC

20. (0,32) = (C1,F1)
(100,212) = (C2,F2) ºF ºC

21. At what temperature does °C = °F?
Section 1.7
Temperature
Exercise
At what temperature does °C = °F?
The answer is -40. Since °C equals °F, they both should be the same value (designated as variable x). Use one of the conversion equations such as °C = (°F- 32)(5/9), and substitute in the value of x for both °C and °F. Solve for x.
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22. Use one of the conversion equations such as:
Section 1.7
Temperature
Solution
Since °C equals °F, they both should be the same value (designated as variable x).
Use one of the conversion equations such as:
Substitute in the value of x for both TC and TF. Solve for x.
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23. Temperature Solution Section 1.7 Return to TOC
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24. Mass of substance per unit volume of the substance.
Section 1.8
Density
Mass of substance per unit volume of the substance.
Common units are g/cm3 or g/mL.
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25. Section 1.8
Density
Example #1
A certain mineral has a mass of 17.8 g and a volume of cm3. What is the density of this mineral?
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26. Section 1.8
Density
Example #2
What is the mass of a 49.6-mL sample of a liquid, which has a density of 0.85 g/mL?
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27. Anything occupying space and having mass.
Section 1.9
Classification of Matter
Matter
Anything occupying space and having mass.
Matter exists in three states.
Solid
Liquid
Gas
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28. The Three States of Water
Section 1.9
Classification of Matter
The Three States of Water
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29. Has fixed volume and shape.
Section 1.9
Classification of Matter
Solid
Rigid
Has fixed volume and shape.
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30. Classification of Matter
Section 1.9
Classification of Matter
Structure of a Solid
Click below for visual concept while in play mode
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31. Has definite volume but no specific shape. Assumes shape of container.
Section 1.9
Classification of Matter
Liquid
Has definite volume but no specific shape.
Assumes shape of container.
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32. Classification of Matter
Section 1.9
Classification of Matter
Structure of a Liquid
Text
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33. Has no fixed volume or shape.
Section 1.9
Classification of Matter
Gas
Has no fixed volume or shape.
Takes on the shape and volume of its container.
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34. Classification of Matter
Section 1.9
Classification of Matter
Structure of a Gas
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35. Have variable composition.
Section 1.9
Classification of Matter
Mixtures
Have variable composition.
Homogeneous Mixture
Having visibly indistinguishable parts; solution.
Heterogeneous Mixture
Having visibly distinguishable parts.
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36. Classification of Matter
Section 1.9
Classification of Matter
Homogeneous Mixtures
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37. Homogeneous vs. Heterogeneous Mixtures
Section 1.9
Classification of Matter
Homogeneous vs. Heterogeneous Mixtures
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38. Classification of Matter
Section 1.9
Classification of Matter
Compound vs. Mixture
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39. Pure water Gasoline Jar of jelly beans Soil Copper metal
Section 1.9
Classification of Matter
Concept Check
Which of the following is a homogeneous mixture?
Pure water
Gasoline
Jar of jelly beans
Soil
Copper metal
gasoline
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40. Key Terms: Properties
A physical property is displayed by a sample of matter without undergoing any change in the composition of the matter.
Physical properties include mass, color, volume, temperature, density, melting point, etc.
Chemical property – displayed by a sample of matter as it undergoes a change in composition.
Flammability, toxicity, reactivity, acidity are all chemical properties.
Copper is red-brown, opaque, solid: physical properties.
Ethanol is flammable: a chemical property.
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Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry

41. Change in the form of a substance, not in its chemical composition.
Section 1.9
Classification of Matter
Physical Change
Change in the form of a substance, not in its chemical composition.
Example: boiling or freezing water
Can be used to separate a mixture into pure compounds, but it will not break compounds into elements.
Distillation
Filtration
Chromatography
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42. Section 1.9
Classification of Matter
Chemical Change
A given substance becomes a new substance or substances with different properties and different composition.
Example: Bunsen burner (methane reacts with oxygen to form carbon dioxide and water)
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43. Key Terms: Properties
In a physical change, there is no change in composition.
No new substances are formed.
Examples include: evaporation; melting; cutting a piece of wood; dissolving sugar in water.
In a chemical change or chemical reaction, the matter undergoes a change in composition.
New substances are formed.
Examples include: burning gasoline; dissolving metal in acid; spoilage of food.
The vapor burns, combining with oxygen: a chemical change.
The liquid fuel evaporates: a physical change.
Prentice Hall © 2005
Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry

44. Pulverizing (crushing) rock salt Burning of wood
Section 1.9
Classification of Matter
Concept Check
How many of the following are examples of a chemical change?
Pulverizing (crushing) rock salt
Burning of wood
Dissolving of sugar in water
Melting a popsicle on a warm summer day
1 (burning of wood)
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45. The Organization of Matter
Section 1.9
Classification of Matter
The Organization of Matter
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46. Classifying Matter Figure 1.9
Atoms
Molecules
make up
ALL MATTER
which exists as
Substances
Mixtures
Pure
which may be
Elements
Compounds
Heterogeneous
which may be
Homogeneous
Prentice Hall © 2005
Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry

47. The Organization of Matter
Mixtures:
a) Homogeneous (Solutions)
b) Heterogeneous
Pure Substances
Elements
Compounds
Atoms
Nucleus
Electrons
Protons
Neutrons
Quarks
Quarks

48. General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry
Classifying Matter
A (pure) substance has a definite or fixed composition that does not vary from one sample to another.
All substances are either elements or compounds.
An element cannot be broken down into other simpler substances by chemical reactions.
About 100 elements known at this time
Each element has a chemical symbol: O, H, Ag, Fe, Cl, S, Hg, Au, U, etc.
A compound is made up of two or more elements in fixed proportions, and can be broken down into simpler substances.
Carbon dioxide, sodium chloride, sucrose (sugar), etc.
Prentice Hall © 2005
Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry

49. General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry
Classifying Matter
A mixture does not have a fixed composition.
A homogeneous mixture has the same composition throughout, though the composition of different homogeneous mixtures may vary.
Soda pop, salt water, 14K gold, and many plastics are homogeneous mixtures.
10K gold and 14K gold have different compositions but both are homogeneous.
A heterogeneous mixture varies in composition and/or properties from one part of the mixture to another.
Adhesive tape, CD, pen, battery, chair, and people are examples of heterogeneous mixtures.
Most everyday “stuff” consists of mixtures.
Prentice Hall © 2005
Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry

50. The Organization of Matter
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51. Phase Differences
Solid – definite volume and shape; particles packed in fixed positions.
Liquid – definite volume but indefinite shape; particles close together but not in fixed positions
Gas – neither definite volume nor definite shape; particles are at great distances from one another
Plasma – high temperature, ionized phase of matter as found on the sun.

52. Properties of Matter
Extensive properties depend on the amount of matter that is present.
Volume
Mass
Energy Content (think Calories!)
Intensive properties do not depend on the amount of matter present.
Melting point
Boiling point
Density

53. Separation of a Mixture
The constituents of the mixture retain their identity and may be separated by physical means.

54. Separation of a Mixture
The components of dyes such as ink may be separated by paper chromatography.

55. Figure 1.15a A Line of the Mixture to be Separated is Placed at One End of a Sheet
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56. Figure 1.15b The Paper Acts as a Wick to Draw up the Liquid
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57. Figure 1.15c Component with the Weakest Attraction for the Paper Travels Faster
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58. Separation of a Mixture by Distillation

59. Separation of a Compound The Electrolysis of water
Compounds must be separated by chemical means.
With the application of electricity, water can be separated into its elements
Reactant Products
Water  Hydrogen + Oxygen
2 H2O 2 H O2

60. React 5
Sketch a magnified view (showing atoms/molecules) of each of the following:
a heterogeneous mixture of two different compounds.
a homogeneous mixture of an element and a compound.
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