Chemistry, The Central Science, 11th edition
Theodore L. Brown; H. Eugene LeMay, Jr.;
and Bruce E. Bursten
Chapter 1
Introduction:
Matter and Measurement
John D. Bookstaver
St. Charles Community College
Cottleville, MO
Matter
And
Measurement
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Chemistry
In this science we
study matter and the
changes it
undergoes.
Matter
And
Measurement
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Scientific Method
The scientific method is simply a systematic
approach to solving problems.
Matter
And
Measurement
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Matter
We define matter as anything that has mass
and takes up space.
Matter
And
Measurement
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Matter
• Atoms are the building blocks of matter.
Matter
And
Measurement
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Matter
• Atoms are the building blocks of matter.
• Each element is made of the same kind of atom.
Matter
And
Measurement
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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
Matter
elements.
And
Measurement
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States of Matter
Matter
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Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Classification of Matter
Matter
And
Measurement
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Properties and
Changes of
Matter
Matter
And
Measurement
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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.
Matter
And
Measurement
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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.
Matter
And
Measurement
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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.
Matter
And
Measurement
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Chemical Reactions
In the course of a chemical reaction, the
reacting substances are converted to new
substances.
Matter
And
Measurement
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Compounds
Compounds can be
broken down into
more elemental
particles.
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And
Measurement
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Separation of
Mixtures
Matter
And
Measurement
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Distillation
Distillation uses
differences in the
boiling points of
substances to
separate a
homogeneous
mixture into its
components.
Matter
And
Measurement
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Filtration
In filtration solid
substances are
separated from liquids
and solutions.
Matter
And
Measurement
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Chromatography
This technique separates substances on the
basis of differences in solubility in a solvent.
Matter
And
Measurement
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Units of
Measurement
Matter
And
Measurement
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SI Units
• Système International d’Unités
• A different base unit is used for each quantity.
Matter
And
Measurement
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Metric System
Prefixes convert the base units into units that
are appropriate for the item being measured.
Matter
And
Measurement
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Volume
• The most commonly
used metric units for
volume are the liter (L)
and the milliliter (mL).
– A liter is a cube 1 dm
long on each side.
– A milliliter is a cube 1 cm
long on each side.
Matter
And
Measurement
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Uncertainty in Measurements
Different measuring devices have different
uses and different degrees of accuracy.
Matter
And
Measurement
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Temperature
By definition
temperature is a
measure of the
average kinetic
energy of the
particles in a
sample.
Matter
And
Measurement
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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.
Matter
And
Measurement
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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 + 273.15
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And
Measurement
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Temperature
• The Fahrenheit
scale is not used in
scientific
measurements.
• F = 9/5(C + 32)
• C = 5/9(F - 32)
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And
Measurement
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Density
Density is a physical property of a
substance.
m
d=
V
Matter
And
Measurement
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Sample Exercise 1.4 Determining Density and Using Density to Determine
Volume or Mass
(a) Calculate the density of mercury if 1.00  102 g occupies a volume of 7.36 cm3. (b) Calculate the volume
of 65.0 g of the liquid methanol (wood alcohol) if its density is 0.791 g/mL. (c) What is the mass in grams of
a cube of gold (density = 19.32 g/cm3) if the length of the cube is 2.00 cm?
Solution
(a) We are given mass and volume, so
Equation 1.3 yields
(b) Solving Equation 1.3 for volume and then
using the given mass and density gives
(c) We can calculate the mass from the
volume of the cube and its density. The
volume of a cube is given by its length cubed:
Solving Equation 1.3 for mass and
substituting the volume and density of the
cube, we have
Practice Exercise
(a) Calculate the density of a 374.5-g sample of copper if it has a volume of 41.8 cm3. (b) A student needs
15.0 g of ethanol for an experiment. If the density of ethanol is 0.789 g/mL, how many milliliters of ethanol
are needed? (c) What is the mass, in grams, of 25.0 mL of mercury (density = 13.6 g/mL)?
Answers: (a) 8.96 g/cm3, (b) 19.0 mL, (c) 340 g
Matter
And
Measurement
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Uncertainty in
Measurement
Matter
And
Measurement
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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.
Matter
And
Measurement
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Significant Figures
1. All nonzero digits are significant.
2. Zeroes between two significant figures
are themselves significant.
3. Zeroes at the beginning of a number
are never significant.
4. Zeroes at the end of a number are
significant if a decimal point is written
in the number.
Matter
And
Measurement
© 2009, Prentice-Hall, Inc.
Significant Figures
• When addition or subtraction is
performed, answers are rounded to the
least significant decimal place.
• 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.
Matter
And
Measurement
© 2009, Prentice-Hall, Inc.
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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And
Measurement
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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
2.54 cm
1 in.
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And
Measurement
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Dimensional Analysis
Use the form of the conversion factor
that puts the sought-for unit in the
numerator.
Given unit 
Conversion factor
Gift Label
John Travolta
desired unit
given unit
 desired unit
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And
Measurement
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Dimensional Analysis
• For example, to convert 8.00 m to inches,
– convert m to cm
– convert cm to in.
100 cm
1 in.
8.00 m 

 315 in.
1m
2.54 cm
Matter
And
Measurement
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Sample Exercise 1.10 Converting Units Using Two or More Conversion Factors
The average speed of a nitrogen molecule in air at 25 °C is 515 m/s. Convert this speed to miles per hour.
Solution
To go from the given units, m/s, to the desired units, mi/hr, we must convert meters to miles and seconds to
hours. From our knowledge of metric prefixes we know that 1 km = 10 3 m. From the relationships given on
the back inside cover of the book, we find that 1 mi = 1.6093 km. Thus, we can convert m to km and then
convert km to mi. From our knowledge of time we know that 60 s = 1 min and 60 min = 1 hr. Thus, we can
convert s to min and then convert min to hr. Applying first the conversions for distance and then those for
time, we can set up one long equation in which unwanted units are canceled:
Our answer has the desired units. We can check our calculation, using the estimating procedure described in
the previous “Strategies” box. The given speed is about 500 m/s. Dividing by 1000 converts m to km, giving
0.5 km/s. Because 1 mi is about 1.6 km, this speed corresponds to 0.5/1.6 = 0.3 mi/s. Multiplying by 60
gives about 0.3  60 = 20 mi/min. Multiplying again by 60 gives 20  60 = 1200 mi/hr. The approximate
solution and the detailed solution are reasonably close. The answer to the detailed solution has three
significant figures, corresponding to the number of significant figures in the given speed in m/s.
Matter
And
Measurement
© 2009, Prentice-Hall, Inc.
Sample Exercise 1.10 Converting Units Using Two or More Conversion Factors
Practice Exercise
A car travels 28 mi per gallon of gasoline. How many kilometers per liter will it go?
Answer: 12 km/L
Matter
And
Measurement
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Sample Exercise 1.11 Converting Volume Units
Earth’s oceans contain approximately 1.36  109 km3 of water. Calculate the volume in liters.
Solution
This problem involves conversion of km3 to L. From the back inside cover of the text we find 1 L = 10 –3 m3,
but there is no relationship listed involving km3. From our knowledge of metric prefixes, however, we have
1 km = 103 m and we can use this relationship between lengths to write the desired conversion factor
between volumes:
Thus, converting from km3 to m3 to L, we have
Practice Exercise
If the volume of an object is reported as 5.0 ft3, what is the volume in cubic meters?
Answer: 0.14 m3
Matter
And
Measurement
© 2009, Prentice-Hall, Inc.
Sample Exercise 1.12 Conversions Involving Density
What is the mass in grams of 1.00 gal of water? The density of water is 1.00 g/mL.
Solution
1. We are given 1.00 gal of water (the known, or given, quantity) and asked to calculate its mass in grams
(the unknown).
2. We have the following conversion factors either given, commonly known, or available on the back inside
cover of the text:
The first of these conversion factors must be used as written (with grams in the numerator) to give the
desired result, whereas the last conversion factor must be inverted in order to cancel gallons:
The units of our final answer are appropriate, and we’ve also taken care of our significant figures. We can
further check our calculation by the estimation procedure. We can round 1.057 off to 1. Focusing on the
numbers that do not equal 1 then gives merely 4  1000 = 4000 g, in agreement with the detailed
calculation.
Matter
And
Measurement
© 2009, Prentice-Hall, Inc.
Sample Exercise 1.12 Conversions Involving Density
Solution (continued)
In cases such as this you may also be able to use common sense to assess the reasonableness of your answer.
In this case we know that most people can lift a gallon of milk with one hand, although it would be tiring to
carry it around all day. Milk is mostly water and will have a density that is not too different than water.
Therefore, we might estimate that in familiar units a gallon of water would have mass that was more than 5
lbs but less than 50 lbs. The mass we have calculated is 3.78 kg × 2.2 lb/kg = 8.3 lbs—an answer that is
reasonable at least as an order of magnitude estimate.
Practice Exercise
The density of benzene is 0.879 g/mL. Calculate the mass in grams of 1.00 qt of benzene.
Answer: 832 g
Matter
And
Measurement
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