This document is a slide presentation on chapter 1 of a general chemistry textbook. It covers the following key topics: 1) The scientific method and its application to chemistry. 2) The basic properties of matter including composition, physical and chemical properties, and the classification of elements, compounds, and molecules. 3) The measurement of various chemical properties including mass, temperature, volume, and density. It also discusses units of measurement and uncertainties in scientific measurements. 4) Significant figures and how they impact calculations and measurements.

1. General Chemistry: Chapter 1Slide 1 of 25
PHILIP DUTTON
UNIVERSITY OF WINDSOR
DEPARTMENT OF CHEMISTRY AND
BIOCHEMISTRY
TENTH EDITION
GENERAL CHEMISTRY
Principles and Modern Applications
PETRUCCI HERRING MADURA BISSONNETTE
Copyright © 2011 Pearson Canada Inc.
Matter: Its Properties
and Measurement 1

2. Copyright © 2011 Pearson Canada Inc.General Chemistry: Chapter 1Slide 2 of 25
Matter: Its Properties
and Measurement

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1-1 The Scientific Method
Louis Pasteur (1822-1895)
developer of germ theory
pasteurization
rabies vaccination
Called the greatest physician of
all time by some.
He was a chemist by training
and profession.

4. FIGURE 1-1
The Scientific Method Illustrated
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1-2 Properties of Matter
tter: Occupies space, has mass and inertia
mposition: Parts or components
ex. H2O, 11.19% H and 88.81% O
perties: Distinguishing features
physical and chemical properties

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1-3 Classification of Matter
Matter is made of atoms.
114 elements.
About 90% available from natural sources
Compounds are comprised of two or more elements.
Molecules are the smallest units of compounds.

7. FIGURE 1-4
A classification scheme for matter
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8. Separating Mixtures: a physical process
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FIGURE 1-5

9. A chemical change: decomposition of ammonium dichromate
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FIGURE 1-6

10. Macroscopic and microscopic views of matter
Figure 1-7
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1-4 The Measurement of Matter

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General Chemistry: Chapter 1

13. Mass
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Mass is the quantity of
matter in an object.
Weight is the force of
gravity on an object
W ∝m W = g × m

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Temperature

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Volume

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SI and non-SI Units Compared
1 kg 1 lb
1 in 1 cm
1 US qt
0.936 L
1 L
1 Imperial qt
1.136 L

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SI Units
Length meter, m
Mass Kilogram, kg
Time second, s
Temperature Kelvin, K
Quantity Mole, 6.022×1023
mol-1
Derived Units
Force Newton, kg m s-2
Pressure Pascal, kg m-1
s-2
Energy Joule, kg m2
s-2
Non-SI Units
Length Angstrom, Å, 10-8
cm
Volume Liter, L, 10-3
m3
Energy Calorie, cal, 4.184 J
Pressure
1 Atm = 1.064 × 102
kPa
1 Atm = 760 mm Hg

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1-5 Density and Percent Composition
δ= m/V
m=Vδ V=m/δ
g/mL
Mass and volume are extensive properties
Density is an intensive property

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Density in Conversion Pathways
What is the mass of a cube of osmium that is 1.25
inches on each side?
Have volume, need density = 22.59g/cm3

20. Measuring Volume of an Irregular Object
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FIGURE 1-10

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1-6 Uncertainties in Scientific Measurements
Systematic errors.
Thermometer constantly 2°C too low.
Random errors
Limitation in reading a scale.
Precision
Reproducibility of a measurement.
Accuracy
How close to the real value.

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Precision
Reproducibility ∼ 0.1 g ∼ 0.0001 g
Precision low high

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1-7 Significant Figures
Determining the number of significant figures in a quantity
Figure 1-11

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Significant Figures
The calculators show the effect of the change in a low precision
number (N) in a calculation 14.79 × 12.11 × N
N = 5.04 5.05 5.06

25. Copyright © 2011 Pearson Canada Inc.General Chemistry: Chapter 1Slide 25 of 25
End of Chapter Questions
Instructors may provide lists of questions that
reinforce topics they feel are particularly pertinent in
the chapter. If no list is given students should attempt
questions from each section of the chapter.
Build from the easier questions where the topic is
identified, to the more difficult integrative examples
where the approach to the question must be identified.