Chemistry Unit 5 HW Packet
Name __________________________________
WKS #1 - Electromagnetic Spectrum & the Electron (2 pages)
1. Indicate whether the following pairs are inversely proportional or directly proportional.
Energy and Frequency _____________________________
Energy and Wavelength ___________________________
Frequency and Wavelength _________________________
2. Which visible color of light has the highest energy? ___________________
3. Which visible color of light has the longest wavelength? __________________
4. Which visible color of light has the highest frequency? _________________
5. Which has the longer wavelength – yellow light or green light? _________________
6. Which has the lower energy – gamma rays or X-rays? _________________
7. Which has the higher frequency – microwaves or radio waves? _________________
8. Which has the shorter wavelength – blue light or ultraviolet? _________________
9. Which has the greater energy – X-rays or microwaves? _________________
10. Which has the longer wavelength – green light or infrared? _________________
11. Which has the higher frequency – indigo light or gamma? _________________
12. Which has the longer wavelength – the light with a frequency of 7.32 x 1014 Hz or the light with a frequency of
6.0 x 1014 Hz? _________________
13. Which has higher energy, λ of 674 nm or λ of 480 nm? _________________
14. Show the calculation (metric conversion) used to convert 3.0 x 108 m/sec into nm/sec.
15. If the wavelength of light is known to be 840. nm, what is the frequency? (3.57 x 1014 Hz)
16. Find the wavelength (in nanometers) if the frequency is 4.1 x 1011 sec-1. (7.3 x 105 nm)
17. How many Joules of energy are there in one photon of yellow light whose wavelength is 630 nm? (3.2 x 10-19 J)
18. Is the light visible that has an energy of 4.75 x 10-19 Joules? Prove your answer with a calculation! (yes, 419 nm)
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #1 - Electromagnetic Spectrum (continued)
19. If the frequency of light is known to be 5.46 x 1013/sec, is the light visible? Prove your answer with a calculation!
(no, 5490 nm)
20. What is the energy of a photon of light whose frequency is 3.45 x 1014 Hz? (2.29 x 10-19 J)
21. If it is found that the energy of one photon is 4.85 x 10-19 Joules, find the frequency of this light. (7.32 x 1014 sec-1)
The six lettered arrows below represent changes in energy of an electron in energy levels 1-4 of an electron cloud.
n=4
n=3
A
B
C
D
E
F
n=2
n=1
22. Which three of the lettered energy changes involve excitation of the electrons?____________________
23. Which three of the lettered energy changes involve relaxation of the electrons?____________________
24. Which three of the lettered energy changes involve absorption of energy by the electrons?___________________
25. Which three of the lettered energy changes involve emission of EMR (light) by the electrons?________________
26. Of the three lettered energy changes that involve emission, one results in emission of blue light, one involves the
emission of yellow light, and one involves the emission of UV light. Which lettered change involves emission of
the blue light? ___________
27. Which involves emission of the yellow light? ____________
28. Which change involves emission of the UV light? ___________
29. Which number of energy level would be the “ground state” for the electron represented by A/B? __________
30. Which number of energy level would be the “excited state” for the electron represented by A/B? __________
31. Define “excited state”.
32. Define “ground state”.
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #2 – Quantum Numbers (1 page)
1. For each of the following, state if it represents the “s” sublevel or the “p” sublevel.
TRAIT
S OR P SUBLEVEL?
Fills up first within an energy level
Description of shape? __________________________
Description of shape? ___________________________
Has 3 different orbitals possible
Only sublevel present in the 1st energy level
Can contain up to 6 electrons
Has the higher amount of energy associated with it within an energy level
Has only 1 possible orbital
Fills up second within an energy level
Can contain only up to 2 electrons
2. How many total quantum “numbers” are there? What are the names of these “numbers”?
3. What is the maximum number of electrons any orbital can contain?
4. Answer the following questions about the 2nd energy level.
a. What is the maximum number of electrons that the 2nd energy level can hold? ______
b. Which sublevel(s) can be found in the 2nd energy level? _________
c. Which sublevel(s) can not be found in the 2nd energy level? _________
d. Which element on the periodic table has a full 2nd energy level for its valence electrons? ______
5. Answer the following questions about the 3rd energy level.
a. What is the maximum number of electrons that the 3rd energy level can hold? ______
b. Which sublevel(s) can be found in the 3rd energy level? _________
c. Which sublevel(s) can not be found in the 3rd energy level? _________
d. At which element on the periodic table does the 3rd energy level completely fill up? ______
6. How many orbital shapes does the “d” sublevel contain? ______
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…the “f” sublevel contain? ______
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #3 – Quantum Rules (1 page)
1. What does the Aufbau Principle tell us?
2. What does the Pauli Exclusion Principle tell us?
3. What does Hund’s Rule tell us?
4. Whose rule tells us that no two electrons can have the same 4 quantum numbers? _________________________
5. The orbital diagram below is violating which rule for electron configuration? ____________________________
6. The orbital diagram below is violating which rule for electron configuration? ____________________________
7. The orbital diagram below is violating which rule for electron configuration? ____________________________
8. On the following piece of an electron configuration, label the following components: Energy Level, Sublevel,
Number of Electrons
2
1s
9. On the following piece of an orbital diagram, label the following components: Energy Level, Sublevel, Orbital,
Spin of Each Electron
10. Does an electron configuration or an orbital diagram tell us more information? EXPLAIN.
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Chemistry Unit 5 HW Packet
WKS #4 (3 pages)
Isotope: PHOSPHORUS - 32 (NO CHARGE)
Name __________________________________
Nuclear Symbol:
Atom or Ion? _____________________________________
# of Protons: _____________
# of Neutrons: _____________
______________________
# of Electrons: _____________
Circle the Highest-Energy Electrons.
Box the Valence Electrons.
NUCLEUS
Number of Valence Electrons:
_____
Complete Electron Configuration: _____________________________________________________________
Orbital Diagram:
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Chemistry Unit 5 HW Packet
Isotope: IRON – 60 (NO CHARGE)
WKS #4 (continued) Name __________________________________
Nuclear Symbol:
Atom or Ion? _____________________________________
# of Protons: _____________
# of Neutrons: _____________
______________________
# of Electrons: _____________
Circle the Highest-Energy Electrons.
Box the Valence Electrons.
NUCLEUS
Number of Valence Electrons:
_____
Complete Electron Configuration: _____________________________________________________________
Orbital Diagram:
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Chemistry Unit 5 HW Packet
Isotope: CALCIUM – 41 (+2 CHARGE)
WKS #4 (continued) Name __________________________________
Nuclear Symbol:
Atom or Ion? _____________________________________
# of Protons: _____________
# of Neutrons: _____________
______________________
# of Electrons: _____________
Circle the Highest-Energy Electrons.
Box the Valence Electrons.
NUCLEUS
Number of Valence Electrons:
_____
Complete Electron Configuration: _____________________________________________________________
Orbital Diagram:
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #5 – Electron Configuration / Orbital Diagram Fun! (1 page)
1. Work the following regarding Selenium.
(a) Write the complete electron configuration.
(b) Write the orbital diagram across from left to right (rather than upwards).
(c) What are the highest-energy electrons?
(d) What are the outer-most (valence) electrons?
(e) How many valence electrons are there?
(f)
What is the most likely ion for Selenium? Did we lose or gain electrons to form the ion?
(g) What would be the new complete electron configuration for the Selenium ion?
(h) Would the resulting ion be larger or smaller than the original atom?
(i)
With which noble gas is the Selenium ion isoelectronic?
2. Work the following regarding Rubidium.
(a) Write the complete electron configuration.
(b) Write the orbital diagram across from left to right (rather than upwards).
(c) What are the highest-energy electrons?
(d) What are the outer-most (valence) electrons?
(e) How many valence electrons are there?
(f)
What is the most likely ion for Rubidium? Did we lose or gain electrons to form the ion?
(g) What would be the new complete electron configuration for the Rubidium ion?
(h) Would the resulting ion be larger or smaller than the original atom?
(i)
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With which noble gas is the Rubidium ion isoelectronic?
isoelectronic with each other?
Are the Rubidium ion and the Selenium ion
Page 8 of 11
Chemistry Unit 5 HW Packet
Name __________________________________
WKS #6 – MORE Electron Configuration / Orbital Diagram Fun! (1 page)
1. The following electron configurations for neutral atoms each have something wrong with them. State what is
incorrect about each of the following.
a. 1s22s22p53s23p3
b. 1s22s22p63s23p63d2
c. 1s22s22p8
d. 1s22s23s23p3
2. Does a 7s electron or a 5f electron have more energy? WHY?
3. Is a 7s electron or a 5f electron physically farther from the nucleus? WHY?
Write the Electron Configuration for each of the following using the Abbreviated Noble-Gas Format.
Electron Configuration
(abbreviated noble-gas notation)
# of
Who are
Valence the Valence
e–?
e–?
Who are
the
HighestEnergy e–?
4. beryllium
5. aluminum
6. mercury
7. manganese
8. silver
9. lead
10. tungsten
What elements are represented by each of the following electron configurations?
Element?
# of
Valence e-?
11. 1s22s22p5
12. [Ar]4s2
13. [Xe]6s24f145d8
14. [Kr]5s24d105p4
15. 1s22s22p63s23p64s23d104p5
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #7 – Periodic Trends (2 pages)
1. Explain why the radius of an atom decreases from left to right across a period, even though more electrons
are being added to the atom.
2. Explain why the radius of an atom increases down a group.
3. Consider the elements Li, Rb, F and I.
a. Which element is the smallest? ________ Explain why.
b. Which element is the largest?
_______ Explain why.
4. Choose the one you would predict would have the larger atomic radius of the two elements in each pair:
Ca or Ba?
______
B or O?
______
K or Kr?
______
S or Se?
______
Bi or Ba?
______
Xe or Ne?
______
5. What is the definition of ionization energy?
6. As atomic radius increases, what happens to ionization energy? Explain why.
7. Consider the elements Li, Rb, F and I.
a. Which one would you predict to have the lowest ionization energy? _______ Explain why.
b. Which one would you predict to have the highest ionization energy? _____ Explain why.
8. Choose the element that you would predict to have the higher ionization energy in each pair:
Ca or Ba?
______
B or O?
______
K or Kr?
______
S or Se?
______
Bi or Ba?
______
Xe or Ne?
______
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Chemistry Unit 5 HW Packet
Name __________________________________
WKS #7 – Periodic Trends (continued)
9. As atomic radius increases, what happens to electronegativity? Explain why.
10. Consider the elements Li, Rb, F and I.
a. Which one would have the lowest electronegativity? ______ Explain why.
b. Which one would have the highest electronegativity? _____ Explain why.
11. Choose the element that you would predict to have the higher electronegativity in each pair:
Ca or Ba?
______
B or O?
______
K or As?
______
S or Se?
______
Bi or Ba?
______
Sn or C?
______
12. Which element has the highest electronegativity? _____ What value does it have? ____
13. Explain why noble gases have no electronegativity values.
14. Would you expect a Ca atom or a Ca (+2) cation to have a larger radius? Explain.
15. Would you expect a Br atom or a Br (‒1) anion to have a larger radius? Explain.
Summary of the Trends: State if the following trends increase or decrease during the following
transitions.
Trend
Across a Period (Left to Right)
Down a Group/Family
Atomic Radius
Ionization Energy
Electronegativity
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