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:_____________________________________

 

Arorbital

 

 

 

2. 60Co27   Chemist Shorthand:_____________________________________

 

 

e-1Kr

 

 


Module Three: Part B: Electron Configuration continued:

 

3.  40Ca20         Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

4.  52Cr24         Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

 

 

 

 

 

 

 

Module Three: Part B: Electron Configuration continued:

 

5.  65Zn30         Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

 

6.  85Nb41         Chemist Shorthand:____________________________

 

 

e-1Xe

 

 

 

 

 

 

 

 

Module Three: Part B: Electron Configuration continued:

 

7.  96Mo42         Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

8.  180Au79         Chemist Shorthand:____________________________

e-1Rn

 

 

 

 

 

9.  Pd46         Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

10.  Pt78         Chemist Shorthand:____________________________

e-1Rn

 

 

 

 

 

 

 

 

11.  Ag47         Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

12.  W74         Chemist Shorthand:____________________________

e-1Rn

 

 

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

e-1rules1

 

e-1rules2

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

 

e-1rules3

 

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

Group

1

2

 

3

4

5

6

7

8

9

10

11

12

13

14

15

16

17

18

Period

 

1

1
 

 

2
 

2

3
 

4
 

 

5
 

6
 

7
 

8
 

9
 

10
 

3

11
 

12
 

 

13
 

14
 

15
 

16
 

17
 

18
 

4

19
 

20
 

 

21
 

22
 

23
 

24
 

25
 

26
 

27
 

28
 

29
 

30
 

31
 

32
 

33
 

34
 

35
 

36
 

5

37
 

38
 

 

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
Fr

88
Ra

**

103
Lr

104
Rf

105
Db

106
Sg

107
Bh

108
Hs

109
Mt

110
Ds

111
Rg

112
Uub

113
Uut

114
Uuq

115
Uup

116
Uuh

117
Uus

118
Uuo

 

 

*Lanthanoids

*

57
 

58
 

59
 

60
 

61
 

62
 

63
 

64
 

65
 

66
 

67
 

68
 

69
 

70
 

 

 

**Actinoids

**

89
Ac

90
Th

91
Pa

92
U

93
Np

94
Pu

95
Am

96
Cm

97
Bk

98
Cf

99
Es

100
Fm

101
Md

102
No

 

 

 

 

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

 

 

 

 

H

 

 

 

 

 

IIIA

IVA

VA

VIA

VIIA

He

2

 

 

 

 

 

  *

 

 

 

 

*

 

 

 

 

 

 

Ne

3

 

 

IIIB

IVB

VB

VIB

VIIB

VIIIB

 

 

IB

IIB

 

 

 

 

 

Ar

4

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Kr

5

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Xe

6

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Rn

7

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

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)

 

  1. 1H         __________________________________________

 

 

  1. 30Zn      __________________________________________

 

 

  1. 35Br       __________________________________________

 

 

  1. 74W        ___________________________________________

 

  1. 8O         ___________________________________________

 

  1. 15P        ___________________________________________

 

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: ___________________________

 

Arorbital

 

2.  K1+ ion  Chemist Shorthand: _____________________________

 

 

e-1Kr

 

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:

PeriodicPostReport

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