CHM
2045C Name:
__________________
Module Three Part I: Atomic
Theory & The Periodic Chart -Jespersen
A. _____ (02) Atomic Notation-Section
0.5 p13-14 Answers
B. _____ (12) Electron Configuration-Sections
7.7-7.8 pages 324-332 Answers
C. _____ (03) Orbitals/Subshells
Section 7.8 Fig7.21 p327 Answer
C1.
____ (06) Spectroscopic
Notation from Periodic Chart Section 7.8 Answer
D. _____ (03) Electron Dot
Structures-Section 8.4 Answers
E. _____ (04) e-1
Configuration of Ions-Section 8.3 Answers
F. _____ (03) Periodic Ionic
Character-Section 2.5 p82-83 Answers
P. ____ (04) Periodic table
Properties Section 2.1-2.2 Chapters 2, 7, 8 Answers
_______(37) Total = ______%
Module
Three: Part A Atomic Notation 2 points
Given
the following elements, atomic numbers, and mass numbers, State the number of
electrons, protons, and neutrons in the following elements:
1. 23Na11 Protons = ______
Electrons = ______
Neutrons
= ______
2. 93Nb41 Protons = ______
Electrons = ______
Neutrons
= ______
3. 20Ne10 Protons = ______
Electrons = ______
Neutrons
= ______
4. 59Ni28 Protons = ______
Electrons = ______
Neutrons
= ______
5. 19F9 Protons = ______
Electrons = ______
Neutrons
= ______
Additional Homework (not required) for your practice:
Read McMurry Section 2.5, 2.6 pages 43-45
Look
at: McMuury Q2.54-2.73 page 70-71 especially 2.64-2.69
jESPERSEN 7th : Read
Section 0.5 of Chapter 0; See Example 0.1p15;
Look at Review questions 0.18-0.42 pages 21-22
Module
Three: Part B: Electron
Configuration 08 points
Given the following
elements and atomic numbers, use arrows to fill-in the electron configuration,
then rewrite the configuration into the chemist’s shorthand (spectroscopic
Notation):
*remember 4/9 rule
exceptions: Never 4/9 total d orbital electrons except for elements 41, 74, 78.
1. 12C6
Chemist Shorthand:_____________________________________
2. 60Co27
Chemist Shorthand:_____________________________________
Module
Three: Part B: Electron Configuration continued:
3. 40Ca20 Chemist Shorthand:____________________________
4. 52Cr24 Chemist Shorthand:____________________________
Module
Three: Part B: Electron Configuration continued:
5. 65Zn30 Chemist Shorthand:____________________________
6. 85Nb41 Chemist Shorthand:____________________________
Module
Three: Part B: Electron Configuration continued:
7. 96Mo42 Chemist Shorthand:____________________________
8. 180Au79 Chemist Shorthand:____________________________
9. Pd46 Chemist Shorthand:____________________________
10. Pt78 Chemist Shorthand:____________________________
11. Ag47 Chemist Shorthand:____________________________
12. W74 Chemist Shorthand:____________________________
Interactive Electron Configuration
Web Site:
http://www.lsua.info/e_config/e-1instruct.html
Electron Configuration Rules Menu:
http://www.fccj.info/e_configMenu/e-1Menu.html
Reference
Taylor’s d4-9 rule:
Read McMurry Section 5.12 Some Anomalous Electron Configurations
Read Jespersen Sections 7.7-7.8 pages 324-332 Try
Exercises 7.12-7.16 Page 328; See Example 7.4, p328; 7.6 p331;Review Questions 7.111-7.128 pages 349-350
Check
Your Answers. Click on the element on the periodic table:
http://fscj.me/e-1Spectroscopic/pc.html
Notice
d4-9 application:
Animation
of Elements 1-112 filling electrons:
http://www.northcampus.net/ElectronConfiguration/SpectroscopicNotation/spectroscopicNotation.html
Additional reference
for your information
Read McMurry Sections
5.10, 5.11, 5.12, 5.13
Additional Homework
(Not required) for your practice and study for MC exam:
Orbitals and Quantum
Mechanics (sections 5.6-5.9) Q5.54-5.69 p182-183
Electron Configurations (Sections 5.10-5.13) Q5.70-5.85) page 183
Module
Three: Part C Orbital Subshells & Periodic Chart 3 points
On
the periodic chart below show all the s, p, d and f block elements on the the
first six rows of the periodic table (Label each area beginning with 1s, 2s,
2p, etc):
periodic
table |
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Group |
1 |
2 |
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3 |
4 |
5 |
6 |
7 |
8 |
9 |
10 |
11 |
12 |
13 |
14 |
15 |
16 |
17 |
18 |
Period |
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1 |
1 |
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2 |
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2 |
3 |
4 |
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5 |
6 |
7 |
8 |
9 |
10 |
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3 |
11 |
12 |
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13 |
14 |
15 |
16 |
17 |
18 |
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4 |
19 |
20 |
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21 |
22 |
23 |
24 |
25 |
26 |
27 |
28 |
29 |
30 |
31 |
32 |
33 |
34 |
35 |
36 |
5 |
37 |
38 |
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39 |
40 |
41 |
42 |
43 |
44 |
45 |
46 |
47 |
48 |
49 |
50 |
51 |
52 |
53 |
54 |
6 |
55 |
56 |
* |
71 |
72 |
73 |
74 |
75 |
76 |
77 |
78 |
79 |
80 |
81 |
82 |
83 |
84 |
85 |
86 |
7 |
87 |
88 |
** |
103 |
104 |
105 |
106 |
107 |
108 |
109 |
110 |
111 |
112 |
113 |
114 |
115 |
116 |
117 |
118 |
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*Lanthanoids |
* |
57 |
58 |
59 |
60 |
61 |
62 |
63 |
64 |
65 |
66 |
67 |
68 |
69 |
70 |
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**Actinoids |
** |
89 |
90 |
91 |
92 |
93 |
94 |
95 |
96 |
97 |
98 |
99 |
100 |
101 |
102 |
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Additional reference
for your information:
Read McMurry Section
5.13 pages 175-177
McMurry Section 5.13 See Figure 5.17 6th
edition p175
Jespersen 7th Section
7.8 Fig7.21 p327
Practice Exercises
7.17-7.18 p 328;
Review Questions
7.129-7.142 p348-9
A similar
Figure:
Spectroscopic Notation
from Periodic Chart
1 |
IA |
IIA |
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H |
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IIIA |
IVA |
VA |
VIA |
VIIA |
He |
2 |
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* |
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* |
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Ne |
3 |
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IIIB |
IVB |
VB |
VIB |
VIIB |
VIIIB |
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IB |
IIB |
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Ar |
4 |
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Kr |
5 |
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Xe |
6 |
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Rn |
7 |
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M-3 C1: Spectroscopic Notation
using the Periodic Chart
6 Points
Given
the Element’s Atomic Number, use the Periodic Chart above to write the
Spectroscopic Notation for the following elements..
You may do it the long way showing all blocks of orbitals,
or you may use the shorter method applying the square brackets around the Nobel
Gas which indicates the complete inner filled electrons in the core (or
Kernal).
i.e: [Ar] represents 1s2 2s2 2p6 3s2
3p6 or
the 18 electrons in the Argon core.
*
In columns VIB and IB, you may have to apply the d4/9 Rule (Never 4/9 total d orbital electrons in any spectroscopic notation
except Nb 41; W 74; and Pt 78)
Additional reference
for your information
Read McMurry Sections
5.12-5.13
Additional Homework
(Not required) for your practice and study for MC exam:
Electron Configurations(Sections 5.10-5.13) Especially problems
5.80-5.85
See worked examples
5.8 and 5.9 on the following pages.
Jespersen 7th Exanple
7.5 page 329; Exampl 7.6 page 331;
McMurry’s Text
has two good application problems for M-3B and M-3C1:
Tro’s Text
demonstrates how to read spectroscopic notations from the periodic Chart. After
understanding the blocks of elements in M-3C, you can do the notation by the
position of the element in the block:
Neon is 10. Chlorine
17 so count seven element blocks on Period 3
Scandium
is element 34 – 18 for argon cound 16 element blocks over period 4
Module
Three: Part D Electron Dot
Formulas 3 points
Using the periodic
chart, draw the electron dot formulas of the following elements (the numbers
shown are the element’s atomic number and mass number):
1. 6C12 6. 1H1
2. 14Si28 7. 7N14
3. 9F19 8. 8O16
4. 11Na23 9. 10Ne20
5. 15P31 10. 16S32
Additional reference
for your information
McMurry Section 6.6 Pages 196-198 See
example
McMurry Section 7.5 Electron
Dot-Structures
Jespersen 7th
Section 8.4; Example
8.3 page 362;
Module
Three: Part E: Electron Configuration
of Ions 4 points
Given the following
ions, use arrows to fill-in the electron configuration of the ion, then rewrite
the configuration into the chemist’s shorthand:
1. Cl1- ion Chemist Shorthand:
___________________________
2. K1+ ion Chemist Shorthand: _____________________________
Additional reference
for your information
McMurry Section 6.1
Pages 187-188
Jespersen 7th
Section 8.3; SeeExamples 8.1
& 8.2 pages 360-361
Problems 8.67-8.76 p
398;
Remember
positive ions have lost electrons from the neutral atom, while negative ions
have gained electrons into the neutral atom.
Module
Three: Part F Periodic Ionic
Properties 3 points
Using
a periodic chart, write the ionic character (monoatomic ionic charge) of the
following elements: (The number before the element is its atomic number)
1. 19 K ________ 6. 9F _____
2. 20Ca _______ 7. 1H _____
_____
3. 7N _______ 8. 16S _____
4. 17Cl _______ 9. 10Ne _____
5. 53I ______ 10.
15P _____
Additional reference
for your information: McMurry Sections 2.11; 6.1; and 6.6
Jespersen 7th
Section 2.5 p82-83; Review
Module
Three Part P: Periodic Chart Identification 4 points
Selected symbols
have been placed into the following blank periodic table of elements:
Which symbol in the
above periodic table fits the following description?
_____1. an alkali metal
_____2. A halogen
_____3. an alkaline earth
element
_____4. a noble gas
_____5. A representative element in the fifth
period
_____6. a semimetal
_____7. An element in the lanthanide series
_____8. an element with the atomic number 13
_____9. an element
filling a 5d sublevel
_____10. an element with
six valence electrons
_____11. an element
corresponding to: 1s2 2s2 2p6 3s2
3p6 4s2 3d7
_____12. an element with
four valence electrons
_____13. an element in the
actinide series
_____14. the main isotope
of this element has zero neutrons in the nucleus
_____15. a representative
element in the first period of the periodic table
McMurry:
Review Sections 5.1-5.3 pages
134-138 Additional Questions: p155-6 #8-36
Jespersen 7th Section 2.1-2.2 Chapters 2, 7, 8; Review Question
2.1-2.8 p100-101