Download Name: Period : ______ Chemistry – Chapter 13 – Electrons in

Name: _____________________________________ Period : ________
Chemistry – Chapter 13 – Electrons in Atoms
State/District Chemistry Standards Addressed:
SC 2.2 Describe the arrangements of electrons in atoms using various theories and models.
SC 2.4 Explain Chemical Periodicity and the classification of elements.
SC 6.0 Demonstrate that the scientific process applies to all areas of science
Objectives: Students will be able to:
 Describe the various atomic models that led to the development of the atomic theory
 Describe what is meant by quantized energy levels
 Describe what s, p, d and f sublevels are and how many sublevels occupy each main energy level
 Know how many orbitals occupy each of the s, p, d and f sublevels
 Determine how many electrons occupy each orbital, sublevel and main level
Textbook Pages 361- 366
1. Using figure 13.2 page 362 draw each of the 4 models of the atom, name and describe each model.
2. If electrons have negative charge and the nucleus has a positive charge, why aren’t electrons in an atom pulled
into the nucleus?
3. Define energy level
4. How do electrons move from one energy level to another?
5. Electrons cannot do what when they move from one energy level to another?
6. Define quantum7. How is the quantum model of the atom like the Bohr model of the atom?
8. How is the quantum model of the atom different from the Bohr model of the atom?
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9. Using Table 13.1 and/or the Energy level Diagram fill in the following table. Main level 3 is completed so you
can see the pattern.
Main
Sublevels
Orbitals Maximum
Maximum number
Maximum number
Level
(each orbital Number of
of orbitals in each
of electrons in each
can hold a
electrons in
main level
main level
maximum of
each
2 electrons
sublevel
1
2
3
3s
3p
3d
1
3
5
2
6
10
A maximum of 9
orbitals can occupy
main level 3
18 total electrons
are in main level 3
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5 (*)
5s
5p
5d
5f
5g
(*)In main level 5, g orbitals have not been discussed in the textbook. See if you can see the pattern and fill out
the remainder of the information in the table for main level 5
10. Looking at the patterns in the table above answer the following: What is the maximum number of
sublevels that could be in main level 6? ____ What is the maximum number of orbitals that could be in
main level 6? _____What is the maximum number of electrons that could be in main level 6? _____
11. If n represents the main level give a mathematical formula in terms of n for the maximum number
of sublevels in any main level n. ______Give a mathematical formula for the maximum number of
orbitals in any main level n ______ Give a mathematical formula for the maximum number of electrons
in any main level n ______
12. Describe the shape of a
s orbital –
p orbital d orbital –
13. Give the maximum number of electrons in the following sublevels:
4f ____ 3d ______ 2p______ 4p _______ 5s _______ 4d_______ 1s _______ 5f ______
14. Look at the table in question 9 above. Electrons that have the lowest energy are in sublevel 1s and
the energy of the electrons increases for each sublevel as you go down column 2 with the highest
energy electrons occupying sublevel 5g. Using this information, arrange the sublevels in question 13
starting with the lowest energy sublevel and list them in order to the highest energy sublevel.
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Objectives: Students will be able to:
 Explain what is meant by the Aufbau Principle
 Explain what is meant by Hund’s rule
 Explain what is meant by the Pauli Exclusion Principle
 Write electron configurations
 Explain why Cr and Cu are exceptions to the expected electron configuration
Pages 367 – 371 in Textbook
1. Define Aufbau Principle –
2. Define Pauli Exclusion Principle –
3. Define Hund’s Rule –
4. Write the incorrect electron configuration for Chromium. Also write the orbital notation for this
configuration.
5. Write the correct electron configuration for Chromium. Also write the orbital notation for this
configuration.
6. Write the incorrect electron configuration for Copper. Also write the orbital notation for this
configuration.
7. Write the correct electron configuration for Copper. Also write the orbital notation for this
configuration.
Objectives: Students will be able to:
 Describe what is meant by wavelength and frequency of waves.
 Rank the different types of electromagnetic radiation from least to most energy
 Calculate wavelength and frequency given the speed of light.
 Calculate the energy of electromagnetic radiation given Planck’s constant
 Distinguish between ground state and excited states as they refer to the energy of
electrons
 Describe the Heisenberg Uncertainty Principle
Pages 372 – 377 and Page 382 in Textbook
1.
Define wavelength -
2.
Define frequency –
3.
Using the figure on the bottom of page 373 answer the following questions:
4.
What are the units that frequency is measured in? ______ What is the symbol for frequency?
____
What are the units that wavelength is measured in? ______ What is the symbol for wavelength?
____
5.
3
6.
7.
8.
9.
What happens to the frequency of waves as the wavelength gets larger?
Which type of electromagnetic radiation has the highest frequency? ___________________
Which type of electromagnetic radiation has the longest wavelength? __________________
List all the types of electromagnetic radiation from lowest frequency to highest frequency.
10. Ground state is when electrons are at the lowest possible energy level. Excited state is when
energy is added to atoms of an element the electrons are excited and move to a higher energy
level. These electrons then fall back to lower energy levels giving off light known as the
emission spectrum. What can be said about the emission spectrum of each element?
11. How is this useful?
12. Calculate the wavelength of light that has a frequency of 5.10 x 1014 1/sec given c = 3 x1010
cm/sec and c = λν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate:
13. Calculate the frequency of electromagnetic radiation that has a wavelength of 5.00 x 10-6 cm
given c = 3 x1010 cm/sec and c = λν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate:
14. Calculate the wavelength of electromagnetic radiation that has a frequency of 1.50 x 1013 1/sec
given c = 3 x1010 cm/sec and c = λν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate:
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:
15. Calculate the Energy of electromagnetic radiation that has a frequency of 1.50 x 1013 1/sec given
h = 6.62 x10 -34 J sec and E = hν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate
16. A type of electromagnetic radiation has energy of 2.12 x 10-22 Joules. What is the frequency of
this radiation given and E = hν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate
17. Calculate the Energy of electromagnetic radiation that has a frequency of 8.13 x 1018 1/sec given
h = 6.62 x10 -34 J sec and E = hν
o Given:
o Find:
o Formula:
o Substitute: all numbers must have units
o Calculate
18. A type of electromagnetic radiation has wavelength of 3.12 x 10 -5 cm. What is the energy of this
radiation given c = 3 x1010 cm/sec c = λν
h = 6.62 x10 -34 J sec and E = hν
Hint: This is a two step problem. Use the same order of steps Given, Find, Formula, Substitute
and Calculate.
o
o
o
o
o
Given:
Find:
Formula:
Substitute: all numbers must have units
Calculate
o
o
o
o
o
Given:
Find:
Formula:
Substitute: all numbers must have units
Calculate
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19. A type of electromagnetic radiation has energy of 6.8 x 10 -19 Joules. What is the wavelength of
this radiation given c = 3 x1010 cm/sec c = λν
h = 6.62 x10 -34 J sec and E = hν
.
Hint: This is a two-step problem. Use the same order of steps Given, Find, Formula, Substitute
and Calculate
o
o
o
o
o
Given:
Find:
Formula:
Substitute: all numbers must have units
Calculate
o
o
o
o
o
Given:
Find:
Formula:
Substitute: all numbers must have units
Calculate
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Name: _________________________________ Period: ________
Chapter 13 Practice Exam
1. What causes electrons move from one energy level to another?
2. Electrons cannot do what when they move from one energy level to another?
3. What sublevels occupy the 3rd main level?
4. How many electrons are in each of the following sublevels? 3d _____ 6s _____ 4f _____ 3p
____
5. Rank the above sublevels from Highest to Lowest.
6. What is the maximum number of electrons that can occupy the following main levels: 1___
2_____ 3 _______ 4 ______ 5_______
7. What is the maximum number of electrons that can occupy a single orbital? ______
8. Compare and contrast the Bohr model of the atom with the Quantum mechanical model of the
atom.
9. Define Aufbau Principle –
10. Define Pauli Exclusion Principle –
11. Define Hund’s Rule –
12. Write the correct orbital notation for Chromium. Also write the electron configuration for this
element.
13. Write the correct orbital notation for Copper. Also write the electron configuration for this
element.
14. Define wavelength 15. Define frequency –
16. What happens to the wavelength of waves, as the frequency gets larger?
17. Define Ground state 18. Define Excited state –
Write the Orbital notation, Electron configuration and Electron dot structure for the following elements:
19. Nitrogen
Orbital Notation:
Electron Configuration:
Electron dot notation:
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20. Calcium
Orbital Notation:
Electron Configuration:
Electron dot notation:
21. Krypton
Orbital Notation:
Electron Configuration:
Electron dot notation:
22. Cerium
Orbital Notation: outer shell only
Electron Configuration:
Electron dot notation:
23. Calculate the frequency of electromagnetic radiation that has a wavelength of 7.25 x 10-5 cm
given c = 3 x1010 cm/sec and c = λν
24. Calculate the Energy of electromagnetic radiation that has a frequency of 6.50 x 1015 1/sec
given h = 6.62 x10 -34 J sec and E = hν
25. Calculate the wavelength of electromagnetic radiation that has a frequency of 8.50 x 1012 1/sec
given c = 3 x1010 cm/sec and c = λν
26. A type of electromagnetic radiation has energy of 5.12 x 10-19 Joules. What is the frequency of
this radiation given h = 6.62 x10 -34 J sec and E = hν
27. A type of electromagnetic radiation has wavelength of 8.02 x 10 -8 cm. What is the energy of this
radiation given c = 3 x1010 cm/sec c = λν
h = 6.62 x10 -34 J sec and E = hν
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