Unit Test ch. 3-4 projected
Chemistry - Holt Modern Chemistry
ch. 3 pages 66-95
ch. 4 pg. 96-131
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ARK STANDARDS
pg. 72-76
pg. 67-69, 72-76,
ch. 4: 97-103, 104-106
pg. 68
64-65, 94-95
pg. 81
64-65, 94-95
64-65, 94-95
NS.34.C.2 Understand that scientific theories may be modified or expanded based on additional empirical data, verification, and peer
review pg. 81
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ARK STANDARDS
& pg. 70 NS.36.C4 and NS.37.C.1
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Chapter 3
Atoms: The Building Blocks of Matter
Table of Contents
Section 1 The Atom: From Philosophical Idea to
Scientific Theory
Section 2 The Structure of the Atom
Section 3 Counting Atoms
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Lesson Starter
• Young people should not smoke.
• Smoking at an early age may make it more difficult
to quit smoking later.
• Which of the above statements is an opinion and
which is a theory?
• Which is similar to Aristotle’s statements?
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Objectives
• Explain the law of conservation of mass, the law of
definite proportions, and the law of multiple
proportions.
• Summarize the five essential points of Dalton’s
atomic theory.
• Explain the relationship between Dalton’s atomic
theory and the law of conservation of mass, the law
of definite proportions, and the law of multiple
proportions.
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Conservation of Mass
3.1
Chemical Reactions
>
Conservation of Mass
How are the mass of the reactants and the mass
of the products of a chemical reaction related?
During any chemical
reaction, the mass of
the products is always
equal to the mass of
the reactants.
QuickTime™ and a
Sorenson Video 3 decompressor
are needed to see this picture.
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Foundations of Atomic Theory
• The transformation of a substance or substances
into one or more new substances is known as a
chemical reaction.
• Law of conservation of mass: mass is neither
created nor destroyed during ordinary chemical
reactions or physical changes
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3.1
Chemical Reactions
>
Conservation of Mass
The law of conservation of mass states that in
any physical change or chemical reaction, mass
is conserved.
The conservation of mass is easily observed
when a change occurs in a closed container.
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Chapter 3
Visual Concepts
Law of Conservation of Mass
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_
003036809x/student/ch03/
Visual Concept
sec01/vc02/hc603_01_v02
fs.htm
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Law of
Conservation of
Mass
Notice that there
are the same number
of atoms in both the
reactants and products of
each type of element.
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Foundations of Atomic Theory, continued
• Law of definite proportions: a chemical compound
contains the same elements in exactly the same
proportions by mass regardless of the size of the
sample or source of the compound
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Chapter 3
Visual Concepts
Law of Definite Proportions
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_003
Visual Concept
036809x/student/ch03/sec01/v
c03/hc603_01_v03fs.htm
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Foundations of Atomic Theory, continued
• Law of multiple proportions: if two or more different
compounds are composed of the same two
elements, then the ratio of the masses of the second
element combined with a certain mass of the first
element is always a ratio of small whole numbers
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Chapter 3
Visual Concepts
Law of Multiple Proportions
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_003
Visual Concept
036809x/student/ch03/sec01/v
c04/hc603_01_v04fs.htm
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Law of Multiple Proportions
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3.1
Defining the Atom
The lab technician shown
here is using a magnifying
lens to examine a bacterial
culture in a petri dish.
When scientists cannot see
the details of what they
study, they try to obtain
experimental data that help
fill in the picture.
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3.1 Studying Atoms
I set up to automatically play short audio clip - song about atom/matter while you read
first 3 screens.
• Studying the
structure of atoms is
a little like studying
wind. Because you
cannot see air, you
must use indirect
evidence to tell the
direction of the wind.
Atoms pose a similar
problem because
3.1
Defining the Atom
>
Early Models of the Atom
Early Models of the Atom
• An atom is the smallest particle of an element
that retains its identity in a chemical reaction.
• Philosophers and scientists have proposed
many ideas on the structure of atoms.
• How did Democritus describe atoms?
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Democritus
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3.1 Studying Atoms
Ancient Greek Models of Atoms
• If you cut a piece of aluminum foil in half, you have
two smaller pieces of the same shiny, flexible
substance. You could cut the pieces again and
again. Can you keep dividing the aluminum into
smaller pieces? Greek philosophers debated a
similar question about 2500 years ago. - Quick
Democritus
activity... believed that atoms were indivisible
and indestructible.
Democritus’s ideas were limited because they didn’t
explain chemical behavior and they lacked
experimental support
3.1
Defining the Atom
>
Early Models of the Atom
Dalton’s Atomic Theory
How did John Dalton further
Democritus’s ideas on atoms?
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3.1 Studying Atoms
Dalton’s Atomic Theory
• Evidence for Atoms
• John Dalton studied the behavior of gases
in air. Based on the way gases exert
pressure, Dalton correctly concluded that a
gas consists of individual particles.
• Dalton measured masses of elements that
combine when compounds form. The ratio
of the masses of the elements in each
compound was always the same. In other
words, compounds have a fixed
composition.
3.1
Defining the Atom
>
Early Models of the Atom
By using experimental methods, Dalton
transformed Democritus’s ideas on
atoms into a scientific theory.
The result was Dalton’s atomic theory.
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3.1
Defining the Atom
>
Early Models of the Atom
1) All elements are composed of tiny indivisible
particles called atoms.
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3.1
Defining the Atom
>
Early Models of the Atom
• 2) Atoms of a given element are identical in size, mass,
and other properties; atoms of different elements differ
in size, mass, and other properties.
• 3) Atoms cannot be subdivided, created, or destroyed.
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3.1
Defining the Atom
>
Early Models of the Atom
• 4) Atoms of different elements combine in simple
whole-number ratios to form chemical compounds.
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3.1
Defining the Atom
>
Early Models of the Atom
• 5) In chemical reactions, atoms are combined, separated,
• or rearranged.
Chemical reactions occur when atoms are
separated, joined, or rearranged. Atoms of one
element are never changed into atoms of
another element in a chemical reaction.
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Chapter 3
Section 1 The Atom: From
Philosophical Idea to Scientific Theory
Modern Atomic Theory
• Not all aspects of Dalton’s atomic theory have proven
to be correct. We now know that:
• Atoms are divisible into even smaller particles.
• A given element can have atoms with different
masses.
• Some important concepts remain unchanged.
• All matter is composed of atoms.
• Atoms of any one element differ in properties from
atoms of another element.
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Online Self-Check Quiz
Complete the online 3.1 Quiz and record
answers. Ask if you have any questions
about your answers.
click here for online Quiz 3.1
(8 questions)
You must be in the “Play mode” for the
slideshow for hyperlink to work.
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VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for Section 3.1 The Atom: From Philosophical idea to Scientific
Theory (3 videoclips)
•Atomic Structure (2:16)
•Conservation of Mass (2:29)
•Law of Definite Proportions - Law of Multiple Proportions (5:05)
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SCI LINKS FOR CHAPTER
Additional Student SCI LINKS for CHAPTER 3
The NSTA-sponsored SciLinks Web site contains links to accurate and upto-date science
information on the Internet. Just click on the button below to go to the
SciLinks site at
www.scilinks.org and log in. Then, type in the SciLinks code for the topic
you want to
research. The following is a list of the SciLinks codes for this chapter.
Chapter 3: Atoms: The Building Blocks of Matter
Topic: Atomic Theory
SciLinks code: HC60120
© Copyright Pearson Prentice Hall
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