Petrucci • Harwood • Herring • Madura
GENERAL
CHEMISTRY
Ninth
Edition
Principles and Modern Applications
Chapter 1: Matter—Its Properties and
Measurement
Doç. Dr. Sevnur KESKİN DOĞRUYOL
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General Chemistry: Chapter 1
Prentice-Hall © 2007
Contents
1-1
1-2
1-3
1-4
1-5
1-6
1-7
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The Scientific Method
Properties of Matter
Classification of Matter
Measurement of Matter: SI (Metric) System
Density and Percent Composition:
Their Use in Problem Solving
Uncertainties in Scientific Measurements
Significant Figures
General Chemistry: Chapter 1
Prentice-Hall © 2007
Figure 1-1 The Scientific Method
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General Chemistry: Chapter 1
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1-2 Properties of Matter
Matter:
Occupies space, has mass and inertia.
Composition: Parts or components.
ex. H2O, 11.19% H and 88.81% O
Properties:
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Physical and Chemical properties.
General Chemistry: Chapter 1
Prentice-Hall © 2007
Physical and Chemical Properties
Physical Properties and Physical Changes:
• A physical property is one that a sample of matter
displays without changing its composition.
• Color is a physical property.
• When liquid water freezes into solid water (ice), this is a
physical change.
Chemical Properties and Chemical Changes:
• In a chemical change or chemical reaction, one or more
kinds of matter are converted to new kinds of matter
with different compositions.
• Ability of paper to burn is an example of a chemical
property.
1-2 Classification of Matter
•
•
•
•
•
Matter is made of atoms.
118 elements.
About 90% available from natural sources.
Compounds are comprised of two or more elements.
Molecules are the smallest units of compounds.
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General Chemistry: Chapter 1
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Separating Mixtures
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General Chemistry: Chapter 1
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Separating Mixtures
a) Filtration
b) Distillation
c) Paper
chromatography
of ink
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General
Chemistry:Chapter
Chapter
General Chemistry:
1 1
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States of Matter
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General Chemistry: Chapter 1
Solid
H2O(s) Ice
Liquid
H2O(l)
Water
Gas
H2O(g) Vapor
Plasma, the Forth State of Matter
1-4 The Measurement of Matter
SI (Systeme Internationale d’Unites): The scientific unit system.
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Units
S.I. Units
Other Common Units
Length
meter, m
Length
Angstrom, Å, 10-8 cm
Mass
Kilogram, kg
Volume
Liter, L, 10-3 m3
Time
second, s
Energy
Calorie, cal, 4.184 J
Temperature Kelvin, K
Quantity
Mole, 6.0221023 mol-1
Pressure
1 Atm = 1.064  102 kPa
1 Atm = 760 mm Hg
Derived Quantities
Force
Newton, kg m s-2
Pressure
Pascal, kg m-1 s-2
Energy
Joule, kg m2 s-2
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General Chemistry: Chapter 1
Mass and Weight
• Mass is the quantity of
matter in an object.
• Weight is the force of
gravity on an object
Wm
W=gm
g (acceleration of gravity): The
acceleration for any object moving
under the influence of gravity.
g = 9.8 m\s2
Temperature
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General Chemistry: Chapter 1
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Conversion of Temperature Units
• T (K) = t (0C) + 273,15
• t (0F) = 9/5 t (0C) + 32
• t (0C) = 5/9 [t (0F) – 32]
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General Chemistry: Chapter 1
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Volume
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General Chemistry: Chapter 1
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1-5 Density and Percent Composition
d = m/V
g/mL
Mass and volume are extensive properties
(depends on the quantity of the observed item).
Density is an intensive property (independent of
the amount of the observed substance).
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General Chemistry: Chapter 1
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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 = 22.48 g/cm3
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General Chemistry: Chapter 1
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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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General Chemistry: Chapter 1
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Precision
Reproducibility  0.1 g
Precision
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 0.0001 g
low
high
General Chemistry: Chapter 1
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1-7 Significant Figures
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Significant Figures in Numerical Calculations
ADDITION and
SUBTRACTION
MULTIPLICATION and
DIVISION
The result must be expressed
with the same number of
digits of quantity carrying
the smallest number of such
digits.
The result may contain only
as the least precisely known
quantity in the calculation.
1.14
0.6
11.676
13.416  13,4
0.01208  0.236 = 0.0512
 5.12  10-2
Rounding Off Numerical Results
•
Increase the final digit by one unit, if the digit dropped is 5,
6, 7, 8, or 9.
•
Example: 7.5647
•
Leave the final digit unchanged, if the digit dropped is 0, 1,
2, 3, or 4.
•
Example: 3.6247
7.565
3.62
Example: To three significant figures, 15.44 rounds off to
15.4, and 15.45 rounds off to 15.5.
Examples:
•
•
54.1875
54.1275
54.2
54.1
•
•
0.016880
168.80
1.7 x 10 -2
1.7 x 10 2