1. Unit Test ch. 3-4 projected Chemistry - Holt Modern Chemistry
ch. 3 pages 66-95
ch. 4 pg
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2. ARK STANDARDS pg. 72-76 pg. 67-69, 72-76, ch. 4: 97-103, 104-106
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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3. ARK STANDARDS & pg. 70 NS.36.C4 and NS.37.C.1 Chapter menu Resources
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4. Chapter 3 Table of Contents
Atoms: The Building Blocks of Matter
Chapter 3
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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5. Chapter 3 Lesson Starter Young people should not smoke.
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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6. Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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7. Conservation of Mass
How are the mass of the reactants and the mass of the products of a chemical reaction related?
3.1
Chemical Reactions
>
Conservation of Mass
During any chemical reaction, the mass of the products is always equal to the mass of the reactants.
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8. Foundations of Atomic Theory
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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9. 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.
When the liquids in photograph A are mixed, they react. None of the products are gases. Analyzing Data How do you know that a reaction took place and that mass was conserved during the reaction?
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10. Law of Conservation of Mass
Visual Concepts
Chapter 3
Law of Conservation of Mass
Click below to watch the Visual Concept.
Visual Concept
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11. Law of Conservation of Mass
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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12. Foundations of Atomic Theory, continued
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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13. Law of Definite Proportions
Visual Concepts
Chapter 3
Law of Definite Proportions
Click below to watch the Visual Concept.
Visual Concept
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14. Foundations of Atomic Theory, continued
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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15. Law of Multiple Proportions
Visual Concepts
Chapter 3
Law of Multiple Proportions
Click below to watch the Visual Concept.
Visual Concept
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16. Law of Multiple Proportions
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
Law of Multiple Proportions
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17. Defining the Atom
3.1
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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18. 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 they are extremely small. Even with a microscope, scientists cannot see the structure of an atom.

19. Early Models of the Atom
3.1
Defining 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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20. Ancient Greek Models of Atoms
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 activity...
Democritus believed that atoms were indivisible and indestructible.
Democritus’s ideas were limited because they didn’t explain chemical behavior and they lacked experimental support

21. Early Models of the Atom
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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22. Dalton’s Atomic Theory
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.

23. Early Models of the Atom
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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24. Early Models of the Atom
3.1
Defining the Atom
>
Early Models of the Atom
1) All elements are composed of tiny indivisible particles called atoms.
According to Dalton’s atomic theory, an element is composed of only one kind of atom, and a compound is composed of particles that are chemical combinations of different kinds of atoms. a) Atoms of element A are identical. b) Atoms of element B are identical, but differ from those of element A. c) Atoms of elements A and B can physically mix together. d) Atoms of elements A and B can chemically combine to form a compound. Interpreting Diagrams How does a mixture of atoms of different elements differ from a compound?
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25. Early Models of the Atom
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.
According to Dalton’s atomic theory, an element is composed of only one kind of atom, and a compound is composed of particles that are chemical combinations of different kinds of atoms. a) Atoms of element A are identical. b) Atoms of element B are identical, but differ from those of element A. c) Atoms of elements A and B can physically mix together. d) Atoms of elements A and B can chemically combine to form a compound. Interpreting Diagrams How does a mixture of atoms of different elements differ from a compound?
3) Atoms cannot be subdivided, created, or destroyed.
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26. Early Models of the Atom
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.
According to Dalton’s atomic theory, an element is composed of only one kind of atom, and a compound is composed of particles that are chemical combinations of different kinds of atoms. a) Atoms of element A are identical. b) Atoms of element B are identical, but differ from those of element A. c) Atoms of elements A and B can physically mix together. d) Atoms of elements A and B can chemically combine to form a compound. Interpreting Diagrams How does a mixture of atoms of different elements differ from a compound?
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27. Early Models of the Atom
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.
According to Dalton’s atomic theory, an element is composed of only one kind of atom, and a compound is composed of particles that are chemical combinations of different kinds of atoms. a) Atoms of element A are identical. b) Atoms of element B are identical, but differ from those of element A. c) Atoms of elements A and B can physically mix together. d) Atoms of elements A and B can chemically combine to form a compound. Interpreting Diagrams How does a mixture of atoms of different elements differ from a compound?
Scientists used a scanning tunneling microscope to generate this image of iron atoms, shown in blue. The radius of this circle of atoms is just 7.13 × m.
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28. Chapter 3 Modern Atomic Theory
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Chapter 3
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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29. 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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30. 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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31. Chapter 3: Atoms: The Building Blocks of Matter Topic: Atomic Theory
SCI LINKS FOR CHAPTER
Additional Student SCI LINKS for CHAPTER 3
The NSTA-sponsored SciLinks Web site contains links to accurate and up-to-date science
information on the Internet. Just click on the button below to go to the SciLinks site at
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
Topic: Carbon
SciLinks code: HC60214
Topic: Subatomic Particles
SciLinks code: HC61473
Topic: Isotopes
SciLinks code: HC60820
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