Chemistry

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CHAPTER 11 – MODERN ATOMIC THEORY Day Plans for the day 1  Begin Chapter 11  11.1 – Atoms & Energy o Rutherford’s Atom o Energy & Light o Emission of Energy by Atoms o Flame Tests (demo)  11.2 – The Hydrogen Atom o Energy Levels of Hydrogen o The Bohr Model o The Wave Mechanical Model 2  Section 11.3 – Atomic Orbitals o The four quantum numbers 3

4

5

6 7 8

 11.4 – Electron Configurations & Atomic Properties o Electron Configurations (full)  11.4 – Electron Configurations & Atomic Properties  Electron Configurations (Noble Gas shortcut)  11.4 – Electron Configurations & Atomic Properties o Atomic Size o Ionization Energy  Work on Assignment 11.5  Grade & discuss Assignment 11.5  Review for Chapter 11 Test  Chapter 11 Test

Assignment(s) for the day  Assignment 11.0  Assignment 11.1  Read section(s) 11.3

   

Assignment 11.2 Assignment 11.3 Read section(s) 11.4 Assignment 11.4a

 Assignment 11.4b

 Assignment 11.4c

 Assignment 11.5   Read section(s) 12.1

Chemistry

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Study Guides Chapter 11 Quizzes

Quiz 11.1

Atoms & Energy

1. Be able to describe Rutherford’s model of the atom. 2. Know the definition of electromagnetic radiation. 3. What is the relationship between the wavelength of light and the energy carried by the light wave? 4. Think of a rainbow and answer the following. a. Which color of light has the longest wavelength? b. Which color of light has the highest energy? c. Which color of light has the shortest wavelength? d. Which color of light has the lowest energy?

Quiz 11.2

The Hydrogen Atom

5. Combine knowledge from sections 11.1 and 11.2 to match the color of light with the amount of energy carried by specific colors. 6. Define the term “quantized”.

Quiz 11.3

Atomic Orbitals

7. Know the number of sublevels in each of the first four energy levels. 8. Define the term “orbital”. 9. Know the number of orbitals within each sublevel. 10. Know the maximum number of electrons that a single orbital can contain. 11. State the “Pauli Exclusion Prinicple”.

Quiz 11.4

Electron Configurations & Atomic Properties

12. Define the term “electron configuration”. 13. Understand each “part” of an electron configuration. a. What does the coefficient represent? b. What does the letter represent? c. What does the exponent represent? 14. Define the term “valence electron”. 15. Define the term “core electron”. 16. Positive ions are formed when an atom ___ electrons. 17. Negative ions are formed when an atom ___ electrons. 18. Know the periodic trends regarding atomic size and the periodic trend regarding ionization energy.

Study Guide Chapter 11 Test At the completion of chapter 11 you should… 1.

2. 3. 4. 5. 6.

7.

8.

Know the definitions of the following terms. a. Electromagnetic Radiation b. Photons c. Quantized d. Wave Mechanical Model e. Orbital f. Principle Energy Level g. Sublevel h. Electron Configuration i. Valance Electrons j. Core Electrons k. Ionization Energy Be able to describe Rutherford’s model of the atom. Understand how the light emitted by atoms can be used to identify atoms. Be able to describe Bohr’s model of the atom Understand how the electron’s position is represented in the wave mechanical model Know the four quantum numbers a. the symbol (the letter) b. what it represents c. the theoretical range of values d. the actual range of values Be able to write electron configuration a. The full electron configuration b. Use the noble gas shortcut Be able to describe and explain periodic trends in properties a. Atomic size b. Ionization energy

Chemistry

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Assignment 11.0 – Vocabulary Define each of the following terms. 1. Electromagnetic Radiation

2.

Photons

3.

Quantized

4.

Wave Mechanical Model

5.

Orbital

6.

Principle Energy Levels

7.

Sublevels

8.

Electron Configuration

9.

Valance Electrons

10.

Core Electrons

11.

Ionization Energy

Chemistry

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Assignment 11.1 – Atoms & Energy 1)

What is wrong with Rutherford’s model of the atom? Why did it need to be modified?

2)

What is electromagnetic radiation? Provide three examples.

3)

How is the frequency of a wave different from its speed?

4)

What is a photon?

5)

What is the relationship between wavelength of light and the energy of its photons?

Chemistry

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Assignment 11.2 – The Hydrogen Atom 1)

In the hydrogen spectrum (Figure 11.8, page 367) there are four different colored lines. You already know that hydrogen has only one electron. How can we get four lines from one electron?

2)

Explain the terms ground state and excited state. When a photon of energy is absorbed by an atom, does the electron go from the ground state to an excited state or from an excited state to the ground state?

3)

What is wrong with the Bohr model of the atom?

4)

How does the wave mechanical model of the atom differ from Bohr’s model?

Chemistry

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Assignment 11.3 – Atomic Orbitals 1)

What is the difference between an orbit and an orbital in atomic theory?

2)

Draw figure 11.14 (page 371) and fill in the different types of sublevels (s, p, d, and f) for each principle energy level.

3)

Tell how many orbitals are found in each type of sublevel: s, p, d, f.

4)

What is the Pauli Exclusion Principle and how does it help us determine where an electron is within the atom?

Chemistry

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Assignment 11.4a – Electron Configurations (1) Write the full electron configurations for the following elements. 1)

nitrogen

2)

silicon

3)

potassium

4)

iron

5)

silver

6)

barium

7)

europium

8)

platinum

9)

plutonium

10)

einsteinium

Give the name of the element that has the following electron configuration. 2

2

6

2

4

2

2

6

2

6

2

10

6

2

10

2

2

6

2

6

2

10

6

2

2

2

2

6

2

6

2

10

6

2

10

11)

1s 2s 2p 3s 3p

12)

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d

13)

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d

14)

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s

6

2

14

10

6

2

14

10

6

1

Chemistry

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Assignment 11.4b – Electron Configurations (2) Write the electron configuration for each of the following elements. You MUST use the noble gas shortcut. 1)

Magnesium

2)

Titanium

3)

Germanium

4)

Rubidium

5)

Rhenium

6)

Indium

7)

Osmium

8)

Dysprosium

9)

Uranium

10)

Nobelium

[

Give the name of the element that has the following electron configuration. 11)

[Ne] 3s23p5

12)

[Ar] 4s23d8

13)

[Kr] 5s24d105p6

14)

[Xe] 6s24f5

15)

[Xe] 6s24f145d2

16)

[Rn] 7s25f7

Chemistry

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Assignment 11.4c – Electron Configurations & Atomic Properties 1.

(2 pages) A) What is the difference between a valence electron and a core electron? B) Write the electron configuration for Fe. Label both the valance electrons and the core electron electrons.

2.

Elements in groups (vertical columns) show similar chemical behavior. Why?

3.

What chemical properties distinguish metals from nonmetals?

4.

Explain the general trend in atomic size across rows and down columns of the periodic table.

5.

Circle the larger atom in each pair. a.

Na

K

b.

Na

Mg

c.

Fe

Zn

d.

O

Se

6.

Explain the general trend in ionization energy across rows and down columns of the periodic table.

7.

Circle the atom with the larger ionization energy in each pair. a.

Na

K

b.

Na

Mg

c.

Fe

Zn

d.

O

Se

Chemistry

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Assignment 11.5 – Chapter Review 1)

(4 pages) A) How are the different types of electromagnetic radiation similar? B) How do they differ?

2)

What is a “packet” of electromagnetic energy called?

3)

Do the colors of flame tests result from taking in energy or releasing energy?

4)

What does it mean to say that an atom is in an “excited state”?

5)

When an atom in an excited state returns to the ground state, what happens to the excess energy of the atom?

6)

What is meant by the ground state of an atom?

7)

According to Bohr, what types of motions do electrons have in an atom, and what happens when energy is applied to the atom?

8)

Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of an atom.)

9)

A) Which orbital is the first to be filled in any atom? B) Why?

10)

A) Which electrons of an atom are the valence electrons? B) Why are these electrons especially important?

11)

A) How are electron arrangements in a given group (vertical column) of the periodic table related? B) How is this relationship shown in the properties of the elements in a given group?

12)

Write the full electron configuration (1s2 2s2 etc.) for each of the following elements. How many valence electrons does each atom possess? A) strontium B)

zinc

C)

helium

D)

bromine

E)

calcium

F)

potassium

G)

fluorine

H)

krypton

Chemistry

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13)

Why do we believe that the valence electrons of calcium and potassium reside in the 4s sublevel rather than the 3d sublevel?

14)

Using the noble gas shortcut, write the electron configuration for each of the following elements. How many valence electrons does each atom possess? A) calcium B)

francium

C)

yttrium

D)

cerium

E)

phosphorus

F)

chlorine

G)

magnesium

H)

zinc

15)

A) What types of ions do the metals and nonmetals form? B) Do the metals lose or gain electrons in doing this? C) Do the nonmetals gain or lose electrons in doing this?

16)

Why do the metallic elements of a given period (horizontal row) typically have much lower ionization energies that do the nonmetallic elements of the same period?

17)

Explain why the atoms of the elements at the bottom of a give group (vertical column) of the periodic table are larger than atoms at the top of the same group.

18)

19)

In each of the following sets of elements, which element has the lowest ionization energy? Which element has the highest ionization energy? Lowest Highest A) Cs, Rb, Na ____________ ____________ B)

Ba, Ca, Be

____________

____________

C)

F, Cl, Br

____________

____________

D)

O, S, Te

____________

____________

Arrange the following sets of elements in order of increasing atomic size. A) Sn, Xe, Rb, Sr B)

Rn, He, Xe, Kr

C)

Pb, Ba, Cs, At