1. Chapter 1 Introduction: Matter and Measurement
Chem101
Lecture Presentation
Chapter 1 Introduction: Matter and Measurement
John D. Bookstaver
St. Charles Community College
Cottleville, MO
Dr. Ali Jabalameli

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Chem101
Chemistry
In this science we study matter, its properties, and its behavior.
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Dr. Ali Jabalameli

4. © 2012 Pearson Education, Inc.
Chem101
Matter
We define matter as anything that has mass and takes up space.
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Dr. Ali Jabalameli

5. © 2012 Pearson Education, Inc.
Chem101
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.
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Dr. Ali Jabalameli

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Chem101
States of Matter
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Dr. Ali Jabalameli

7. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

8. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

9. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

10. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

11. Classification of Matter
Chem101
Classification of Matter
© 2012 Pearson Education, Inc.
Dr. Ali Jabalameli

12. Classification of Matter
Chem101
Classification of Matter
© 2012 Pearson Education, Inc.
Dr. Ali Jabalameli

13. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

14. Classification of Matter
Chem101
Classification of Matter
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Dr. Ali Jabalameli

15. Classification of Matter
Chem101
Classification of Matter
Matter
And
Measurement
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Dr. Ali Jabalameli

16. Classification of Matter
Chem101
Classification of Matter
Matter
And
Measurement
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Dr. Ali Jabalameli

17. Classifying Matter

18. Properties and Changes of Matter
Chem101
Properties and Changes of Matter
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Dr. Ali Jabalameli

19. © 2012 Pearson Education, Inc.
Chem101
Types of Properties
Physical 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.
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Dr. Ali Jabalameli

20. © 2012 Pearson Education, Inc.
Chem101
Types of Properties
Intensive Properties…
Are independent of the amount of the substance that is present.
Density, boiling point, color, etc.
Extensive Properties…
Depend upon the amount of the substance present.
Mass, volume, energy, etc.
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Dr. Ali Jabalameli

21. © 2012 Pearson Education, Inc.
Chem101
Types of Changes
Physical Changes
These are changes in matter that do not change the composition of a substance.
Changes of state, temperature, volume, etc.
Chemical Changes
Chemical changes result in new substances.
Combustion, oxidation, decomposition, etc.
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Dr. Ali Jabalameli

22. Some Physical Properties
Chem101
Some Physical Properties
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23. Some Chemical Properties
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24. Phase Changes are Physical Changes
Chem101
Phase Changes are Physical Changes
gas
Boiling = liquid to ___
Melting = solid to ______
Subliming = solid to ___
Condensing = gas to _____
Freezing = liquid to ____
Deposition = gas to ____
state changes require heating or cooling the substance
liquid
gas
liquid
solid
solid
Dr. Ali Jabalameli

25. © 2012 Pearson Education, Inc.
Chem101
Chemical Reactions
In the course of a chemical reaction, the reacting substances are converted to new substances.
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Dr. Ali Jabalameli

26. Separation of Mixtures
Chem101
Separation of Mixtures
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Dr. Ali Jabalameli

27. © 2012 Pearson Education, Inc.
Chem101
Filtration
In filtration, solid substances are separated from liquids and solutions.
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Dr. Ali Jabalameli

28. © 2012 Pearson Education, Inc.
Chem101
Distillation
Distillation uses differences in the boiling points of substances to separate a homogeneous mixture into its components.
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Dr. Ali Jabalameli

29. © 2012 Pearson Education, Inc.
Chem101
Chromatography
This technique separates substances on the basis of differences in solubility in a solvent.
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Dr. Ali Jabalameli

30. © 2012 Pearson Education, Inc.
Chem101
Units of Measurement
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31. © 2012 Pearson Education, Inc.
SI Units
Chem101
Système International d’Unités
A different base unit is used for each quantity.
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Dr. Ali Jabalameli

32. © 2012 Pearson Education, Inc.
Metric System
Chem101
Prefixes convert the base units into units that are appropriate for the item being measured.
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Dr. Ali Jabalameli

33. Conversions Convert 17.6 inches to centimeters:
17.6 in x 2.54 cm/1 in = cm
~ 44.7 cm

34. Conversion with Units Raised to a Power
Convert 1255 cubic centimeters to cubic inches:
1255 cm3 x 1 in3/ cm3 = in3
~ in3

35. © 2012 Pearson Education, Inc.
Chem101
Volume
The most commonly used metric units for volume are the liter (L) and the milliliter (mL).
A liter is a cube 1 decimeter (dm) long on each side.
A milliliter is a cube 1 centimeter (cm) long on each side.
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Dr. Ali Jabalameli

36. Derived Units
Derived unit – a unit formed from the combination of other units
Ex: volume – measure of the amount of three-dimensional space occupied
For solids: usually measured in cm3
V = s V = l x w x h V = π/4(d)2h V = π/6(d)3
(s = side, l = length, w = width, h = height, d = diameter, π = 3.14)

37. For liquid volume: (usually measured in Liter (L) or milliliter (mL)
meniscus – the lowest point of the concave

38. The Meaning of Temperature
Temperature is a measure of the average kinetic energy of the molecules in a sample
Not all molecules have in a sample the same amount of kinetic energy
a higher temperature means a larger average kinetic energy

39. Temperature Scales

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Chem101
Temperature
By definition temperature is a measure of the average kinetic energy of the particles in a sample.
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Dr. Ali Jabalameli

41. © 2012 Pearson Education, Inc.
Chem101
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.
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Dr. Ali Jabalameli

42. © 2012 Pearson Education, Inc.
Chem101
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
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Dr. Ali Jabalameli

43. © 2012 Pearson Education, Inc.
Chem101
Temperature
The Fahrenheit scale is not used in scientific measurements.
F = 9/5(C) + 32
C = 5/9(F − 32)
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Dr. Ali Jabalameli

44. Temperature Conversion Formulas:

45. Scientific Notation decimal exponential
Chem101
Scientific Notation
Scientific Notation – a system used to write very big or very small numbers in a more compact and precise way
– consists of a _______ part (a number usually between 1 and 10) and an __________ part (10 raised to a particular exponent)
decimal
exponential
1.23
10-8
decimal part
exponent part
exponent x
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46. Scientific Notation 3.4567 x 106 1.2 x 10-7
Chem101
Scientific Notation
Ex: Write the following numbers in scientific notation:
3, 456, 700 becomes ___________
becomes _________
x 106
1.2 x 10-7
Dr. Ali Jabalameli

47. © 2012 Pearson Education, Inc.
Chem101
Derived Units
Density is a physical property of a substance.
It has units (g/mL, for example) that are derived from the units for mass and volume.
d = m V
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Dr. Ali Jabalameli

48. Derived Units
Density – units of mass divided by volume (most commonly expressed in g/cm3, g/mL, or g/L
Density = mass / volume

49. Uncertainty in Measurement
Chem101
Uncertainty in Measurement
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Dr. Ali Jabalameli

50. Uncertainty in Measurements
Chem101
Uncertainty in Measurements
Different measuring devices have different uses and different degrees of accuracy.
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Dr. Ali Jabalameli

51. © 2012 Pearson Education, Inc.
Chem101
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.
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Dr. Ali Jabalameli

52. © 2012 Pearson Education, Inc.
Chem101
Significant Figures
All nonzero digits are significant. 3.04
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 &
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Dr. Ali Jabalameli

53. © 2012 Pearson Education, Inc.
Chem101
Significant Figures
When addition or subtraction is performed, answers are rounded to the least significant decimal place.
5.02 x x 0.10 = ~ 45
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.
5.892 / 6.10 = ~ 0.966
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Dr. Ali Jabalameli

54. Rules of Significant Figures with Addition and Subtraction
Addition and subtraction using significant figures: The sum or difference has the same number of decimal places as the quantity carrying the _____________________ Ex: ~ ____
fewest decimal places
9.20

55. Rules of Significant Figures with Multiplication/Division & Addition/ Subtraction
Calculations involving both multiplication/division AND addition/subtraction:
Follow order of operations.
Keep track of significant figures through each step and only round at the end.
Ex: x x (5.489 – 5.01)
= 6.78 x x =
~ ___ 19

56. Accuracy versus Precision
Chem101
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.
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Dr. Ali Jabalameli

57. Chem101
Precision & Accuracy
Precision – the reproducibility of multiple measurements, it is how close the experimental values for different trials are to each other
Accuracy – has to do with how close the experimental results are to the true value
Dr. Ali Jabalameli

58. © 2012 Pearson Education, Inc.
Chem101
Dimensional Analysis
We use dimensional analysis to convert one quantity to another.
Most commonly, dimensional analysis utilizes conversion factors (e.g., 1 in. = 2.54 cm)
1 in.
2.54 cm or
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Dr. Ali Jabalameli

59. © 2012 Pearson Education, Inc.
Chem101
Dimensional Analysis
Use the form of the conversion factor that puts the sought-for unit in the numerator:
Given unit 
 desired unit
desired unit
given unit
Conversion factor
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Dr. Ali Jabalameli

60. © 2012 Pearson Education, Inc.
Chem101
Dimensional Analysis
For example, to convert 8.00 m to inches,
convert m to cm
convert cm to in.
8.00 m 
100 cm
1 m
1 in.
2.54 cm 
315 in. 
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Dr. Ali Jabalameli