Chapter 4: Atomic Structure Section 4.1: Studying...

Chapter 4: Atomic Structure Section 4.1: Studying Atoms I. Ancient Greek Models of Atoms Group #_____

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II. Dalton’s Atomic Theory Group #_____

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A. Evidence for Atoms Group #_____

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B. Dalton’s Theory Group #_____

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III. Thomson’s Model of Atoms Group #______

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A. Thomson’s Experiments Group #_____

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B. Evidence for Subatomic Particles Group #_____

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C. Thomson’s Model Group #_____

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IV. Rutherford’s Atomic Theory Group #______

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A. Rutherford’s Hypothesis Group #_____

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B. The Gold Foil Experiment Group #_____

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C. Discovery of the Nucleus Group #_____

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Section 4.2: The Structure of an Atom I. Properties of Subatomic Particles Group #_____

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A. Protons Group #_____

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B. Electrons Group #_____

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C. Neutrons Group #_____

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II. Comparing Subatomic Particles Group #_____

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III. Atomic Number and Mass Number Group #_____

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A. Atomic Number Group #_____

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B. Mass Number Group #_____

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IV. Isotopes Group #______

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Section 4.3: Modern Atomic Theory I. Bohr’s Model of the Atom Group #_____

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A. Energy Levels Group #_____

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B. Evidence for Energy Levels Group #_____

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II. Electron Cloud Model Group #_____

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III. Atomic Orbitals Group #_____

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IV. Electron Configurations Group #______

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Chapter 5: States of Matter Section 5.1: Organizing the Elements I. The Search for Order Group #_____

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II. Mendeleev’s Periodic Table Group #_____

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A. Mendeleev’s Proposal Group #_____

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B. Mendeleev’s Prediction Group #_____

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C. Evidences Supporting Mendeleev’s Table Group #_____

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Section 5.2: The Modern Periodic Table

I. The Periodic Law Group #______

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A. Periods Group #_____

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B. Groups Group #_____

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II. Atomic Mass Group #______

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A. Atomic Mass Units Group #_____

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B. Isotopes of Chlorine Group #_____

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C. Weighted Average Group #_____

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III. Classes of Elements Group #______

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A. Metals Group #_____

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B. Non Metals Group #_____

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C. Metalloids Group #_____

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IV. Variation Across a Period Group #_____

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Section 5.3: Representative Groups

I. Valence Electrons Group #_____

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II. The Alkali Metal Group #_____

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III. The Alkaline Earth Metals Group #_____

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A. Magnesium Group #_____

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B. Calcium Group #_____

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IV. The Boron Family Group #_____

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V. The Carbon Family Group #_____

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VI. The Nitrogen Family Group #_____

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VII. The Oxygen Family Group #_____

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VIII. The Halogens Group #_____

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IV. The Noble Gases Group #_____

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Chapter 4 Atomic Structure

Section 4.1 Studying Atoms (pages 100-105)This section discusses the development of atomic models.

Reading Strategy (page 100)

Summarizing As you read, complete the table about atomic models.For more information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end ofyour textbook.

Atomic Models

Scientist Evidence Model

Ratio of masses in compounds

Deflected beam

Rutherford Positive, dense nucleus

Ancient Greek Models of Atoms (page 100)

1. Democritus named the smallest particles of matter because they could not be divided.

2. List the four elements that Aristotle included in his model of matter. a. b.c. d.

Dalton’s Atomic Theory (page 101)

3. Is the following sentence true or false? John Dalton gatheredevidence for the existence of atoms by measuring the masses ofelements that reacted to form compounds.

4. What theory did Dalton propose to explain why the elements in a compound always join in the same way?

5. Circle the letters of the sentences that represent the main points ofDalton’s theory of atoms.a. All elements are composed of atoms.b. In a particular compound, atoms of different elements always

combine the same way. c. All atoms have the same mass.d. Compounds contain atoms of more than one element.

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Physical Science Reading and Study Workbook ■ Chapter 4 35

Thomson’s Model of the Atom (pages 102–103)

6. Objects with like electric charges , and objects withopposite electric charges .

7. What happened to the beam when Thomson placed a pair of charged metal plateson either side of the glass tube?

8. Thomson concluded that the particles in the glowing beam had a(n)charge because they were attracted to a positive plate.

9. Is the following sentence true or false? Thomson’s experimentsprovided the first evidence for the existence of subatomic particles.

10. Describe Thomson’s model.

Rutherford’s Atomic Theory (pages 104–105)

11. What is an alpha particle?

12. Fill in the table to show what Rutherford hypothesized wouldhappen to the paths of alpha particles as they passed through athin sheet of gold.

Rutherford’s Hypothesis

Most particles would travel Particles that did not pass straight

from their source to a screen that lit up through would be

when struck.

13. Circle the letters of the sentences that describe what happenedwhen Marsden directed a beam of particles at a piece of gold foil.a. Fewer alpha particles were deflected than expected. b. More alpha particles were deflected than expected.c. None of the alpha particles were deflected.d. Some alpha particles bounced back toward the source.

14. Circle the letter of the sentence that states what Rutherford concluded from the gold foil experiment.a. An atom’s negative charge is concentrated in its nucleus.b. Thomson’s model of the atom was correct.c. An atom’s positive charge is concentrated in its nucleus. d. An atom’s positive charge is spread evenly throughout

the atom.

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Chapter 4 Atomic Structure©

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36 Physical Science Reading and Study Workbook ■ Chapter 4

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Section 4.2 The Structure of an Atom(pages 108–112)This section compares the properties of three subatomic particles. It alsodiscusses atomic numbers, mass numbers, and isotopes.


Monitoring Your Understanding Before you read, list in the tableshown what you know about atoms and what you would like to learn.After you read, list what you have learned. For more information onthis Reading Strategy, see the Reading and Study Skills in the Skillsand Reference Handbook at the end of your textbook.

What I Know What I Would What I HaveAbout Atoms Like to Learn Learned

Properties of Subatomic Particles (pages 108–109)

1. What are three subatomic particles? a. b. c.

2. Circle the letter that identifies a subatomic particle with a positive charge.a. nucleus b. protonc. neutron d. electron

3. Why did Chadwick conclude that the particles produced by his experiment wereneutral in charge?

Comparing Subatomic Particles (pages 109–110)

4. Circle the letters of properties that vary among subatomic particles.a. color b. massc. charge d. location in the atom

5. Circle the letter of the expression that accurately compares themasses of neutrons and protons. a. mass of 1 neutron = mass of 1 protonb. mass of 2000 neutrons = mass of 1 protonc. mass of 1 electron = mass of 1 protond. mass of 1 neutron = mass of 1 electron

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Atomic Number and Mass Number (page 110)

6. Is the following sentence true or false? Two atoms of the sameelement can have different numbers of protons.

7. What is an atomic number?

8. Circle the letters that identify quantities that are always equalto an element’s atomic number.a. number of nucleib. number of protonsc. number of neutrons d. number of electrons

9. Is the following sentence true or false? Two different elements canhave the same atomic number.

10. What is the mass number of an atom?

11. Complete the equation in the table below.

Number of neutrons � �

Isotopes (page 112)

12. Every atom of a given element has the same number ofand .

13. Every atom of a given element does not have the same number of.

14. What are isotopes?

15. All oxygen atoms have 8 protons. Circle the letter of the number ofneutrons in an atom of oxygen-18.a. 8 b. 9c. 10 d. 18

16. Is the following sentence true or false? Isotopes of oxygen havedifferent chemical properties.

17. Water that contains hydrogen-2 atoms instead of hydrogen-1 atoms is called .

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Section 4.3 Modern Atomic Theory(pages 113–118)This section focuses on the arrangement and behavior of electrons in atoms.

Reading Strategy (page 113)Sequencing After you read, complete the description in the flow chartbelow of how the gain or loss of energy affects electrons in atoms. Formore information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end ofyour textbook.

Bohr’s Model of the Atom (pages 113–116)

1. Circle the letter of the sentence that tells how Bohr’s model of theatom differed from Rutherford’s model.a. Bohr’s model focused on the nucleus.b. Bohr’s model focused on the protons.c. Bohr’s model focused on the neutrons.d. Bohr’s model focused on the electrons.

2. Is the following sentence true or false? In Bohr’s model of the atom,electrons have a constant speed and move in fixed orbits aroundthe nucleus.

3. What can happen to an electron in an atom when the atom gains or loses energy?

4. What evidence do scientists have that electrons can move from one energy level to another?

5. Is the following sentence true or false? When electrons releaseenergy, some of the energy may be released as visible light.

Electron Cloud Model (page 116)

6. Is the following sentence true or false? Bohr’s model was correct inassigning energy levels to electrons.

7. When trying to predict the locations and motions of electrons inatoms, scientists must work with .

8. What is an electron cloud?

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Excited State Emits energy

9. Is the following sentence true or false? Scientists use the electroncloud model to describe the exact location of electrons around thenucleus.

Atomic Orbitals (page 117)

10. Is the following sentence true or false? An orbital is a region ofspace around the nucleus where an electron is likely to be found.

11. An electron model is a good approximation of .

Use this table to answer questions 12 and 13.

Energy Number of Maximum NumberLevel Orbitals of Electrons

1 1 2

2 4 8

3 9 18

4 16 32

12. Higher energy levels have orbitals thanlower energy levels do.

13. What is the relationship between the number of orbitals and the maximum number of electrons in an energy level?

Electron Configurations (page 118)

14. What is an electron configuration?

15. Circle the letter of the number of energy levels needed for alithium atom’s three electrons when the atom is in its ground state.a. zero b. one c. two d. three

16. Is the following sentence true or false? An excited state is lessstable than a ground state.

17. Circle the letters of each sentence that is true when all of the electronsin an atom are in orbitals with the lowest possible energies.a. The electrons are in the most stable configuration.b. The electrons are in an unstable configuration.c. The atom is in an excited state.d. The atom is in its ground state.

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Chapter 5 The Periodic Table


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Section 5.1 Organizing the Elements (pages 126–129)This section explains how Mendeleev organized elements into a periodic table.It also discusses the predictions he made about undiscovered elements and howthe discovery of those elements supported his version of the table of the table.


Identifying Main Ideas As you read, complete the table byidentifying the main idea for each topic. For more information on thisreading strategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Topic Main Idea

Mendeleev’s proposal

Mendeleev’s prediction

Evidence supportingMendeleev’s table

The Search for Order (page 126)

1. Is the following sentence true or false? The first elements to beidentified were mainly gases.

2. As the number of known elements grew, so did the need to organizethem into groups based on their .

3. Circle the letter of each category that the French chemist AntoineLavoisier used to classify elements.a. gases b. metalsc. liquids d. nonmetals

Mendeleev’s Periodic Table (pages 127–129)

4. Is the following sentence true or false? Mendeleev needed toorganize information about 63 elements.

5. Mendeleev’s strategy for classifying elements was modeled on a(n).

6. Circle the letter of each type of information Mendeleev knew abouteach element.a. nameb. number of protonsc. relative massd. properties

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7. Mendeleev arranged the elements into rows in order ofso that elements with similar properties

were in the same column.8. Is the following sentence true or false? A periodic table is an

arrangement of elements in columns, based on a set of propertiesthat repeat from row to row.

9. Mendeleev published the table above in 1872. Why did Mendeleev leave somelocations in his periodic table blank?

10. Circle the letters of two elements that have similar properties.a. zinc (Zn) b. chlorine (Cl)c. nitrogen (N) d. bromine (Br)

11. How did Mendeleev decide where to place arsenic (As) and selenium (Se)?

12. Is the following sentence true or false? Mendeleev was the firstscientist to arrange elements in a periodic table.

13. Describe a test for the correctness of a scientific model.

14. Mendeleev used the located near the spacesin his table to predict properties for undiscovered elements.

15. The close match between Mendeleev’s predictions and the actual properties of new elements showed .

16. Circle the letter of each element that was discovered after Mendeleevpublished his periodic table that supported Mendeleev’s predictionsand provided evidence validating the table.a. gallium b. scandiumc. germanium d. aluminum

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Section 5.2 The Modern Periodic Table(pages 130–138)This section explains the organization of the modern periodic table anddiscusses the general properties of metals, nonmetals, and metalloids.


Previewing Before you read, complete the table by writing twoquestions about the periodic table on pages 132–133. As you read,write answers to your questions. For more information on this readingstrategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Questions About the Periodic Table

Question Answer

The Periodic Law (pages 131–133)

1. Is the following sentence true or false? In the modern periodic table,elements are arranged by increasing number of protons.

2. Explain why the number of elements per period varies.

3. Properties of elements repeat in a predictable way when atomicnumbers are used to arrange elements into groups. This pattern ofrepeating properties is called the .

Atomic Mass (page 134)

4. Label the four types of information supplied for chlorine in the diagram.

a. b.c. d.

17

ClChlorine35.453

a.

b.

d.c.

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5. Define atomic mass.

6. Circle the letter of each sentence that is true about a carbon-12atom.a. It has 6 protons and 6 neutrons.b. Scientists assigned a mass of 6 atomic mass units to the

carbon-12 atom.c. It is used as a standard for comparing the masses of atoms.d. An atomic mass unit is defined as one twelfth the mass of a

carbon-12 atom.7. Is the following sentence true or false? Most elements exist as a

mixture of two or more isotopes. 8. The mass of an atom of chlorine-37 is than

the mass of an atom of chlorine-35.9. Is the following sentence true or false? All values are equally

important in a weighted average.

Classes of Elements (pages 135–136)

10. Name the three categories into which elements are classified basedon their general properties.a.b.c.

11. Is the following sentence true or false? All metals react withoxygen in the same way.

12. An important property of transition elements is their ability toform compounds .

13. Circle the letter of each sentence that is true about nonmetals.a. Nonmetals are poor conductors of heat and electric current. b. Many nonmetals are gases at room temperature. c. Some nonmetals are extremely reactive and others hardly

react at all. d. Nonmetals that are solids tend to be malleable.

Variation Across a Period (page 138)

14. Across a period from left to right, the elements becomemetallic and

nonmetallic in their properties.15. Circle the letter of each Period 3 element that is highly reactive.

a. sodium b. siliconc. chlorine d. argon

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Section 5.3 Representative Groups (pages 139–145)This section discusses how the number of valence electrons affectsthe properties of elements. It also describes properties of elementsin Groups 1A through 8A.


Monitoring Your Understanding As you read, record an importantfact about each element listed in the table. For more information onthis reading strategy, see the Reading and Study Skills in the Skillsand Reference Handbook at the end of your textbook.

Element Important Fact

Magnesium

Aluminum

Chlorine

Valence Electrons (page 139)

1. An electron that is in the highest occupied energy level of an atom isa(n) electron.

2. Elements within a group have the number ofvalence electrons.

The Alkali Metals (page 140)

3. The reactivity of alkali metals from the top ofGroup 1A to the bottom.

4. Sodium is stored under oil because it .

The Alkaline Earth Metals (page 141)

5. Differences in reactivity among alkaline earth metals are shown bythe way they react with .

Find and match two properties to each element listed.Alkaline Earth Metal Property

6. magnesium7. calcium

a. Helps build strong teeth and bonesb. Helps plants produce sugarc. Is used to make lightweight bicycle framesd. Is the main ingredient in limestone

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The Boron Family (page 142)

8. List the four metals in Group 3A. a. b.c. d.

9. Circle the letter of each sentence that is true about aluminum.a. It is the most abundant metal in Earth’s crust. b. It is often found combined with oxygen in bauxite. c. It is more reactive than sodium and magnesium. d. It is a good conductor of electric current.

The Carbon Family (page 142)

10. List the two metalloids in Group 4A. a. b.

11. Except for water, most of the compounds in your body contain.

The Nitrogen Family (page 143)

12. List the nonmetals in Group 5A. a. b.

13. Name two elements in the nitrogen family that are contained in fertilizer. a. b.

The Oxygen Family (page 143)

14. List the nonmetals in Group 6A. a. b. c.

15. Name the most abundant element in Earth’s crust.

The Halogens (page 144)

16. List the four nonmetals in Group 7A. a. b.c. d.

17. Halogens have similar properties butdifferent properties.

The Noble Gases (page 145)

18. Name three characteristics of noble gases.a. b. c.

19. How can an element that does not react easily with other elementsbe useful?

Chapter 4: Atomic Structure Section 4.1: Studying...

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