CHM 1032C†††††††††††††††† †††††††††††††††††††††††† Name: __________________

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Chapter 2 Homework Packet-McMurry 7th

 

Chapter 2: Atomic Theory & The Periodic Chart (Formerly Module 3)

A. _____ (01) Atomic Notation-Section 2.6 Answers

B. _____ (04) Electron Configuration-Sections 2.7 Answers

C. _____ (01) Orbitals / Subshells of the Periodic Table-Section 2.8 Answer

C1. ____ (02) Spectroscopic Notation from Periodic Chart Section 2.8Answer

D. _____ (01) Electron Dot Structures-Section2.9 Answers

E. _____ (01) e-1 Configuration of Ions-lecture (Section 3.5) Answers††††††††††††††††††††††††††††††

F. _____ (01) Periodic Ionic Character-Section 3.2/3.5Answers

P. _____ (01) Periodic Chart Identifications Ė Section 2.4/2.5 Answer

_______(12) Chapter 2 Total

 

 

Chapter 2: Part A†† Atomic Notation††††††††††††††††††††††† 1 point

 

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= ______

 

 

 

 

Chapter 2: Part B:†† Electron Configuration††† 4 points

Given the following elements and atomic numbers, use arrows to fill-in the electron configuration, then rewrite the configuration into the chemistís 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

 

 


Chapter 2: Part B: Electron Configuration continued:

 

3.40Ca20†††††††† Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

4.52Cr24†††††††† Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

 

 

 

 

 

 

 

Chapter 2: Part B: Electron Configuration continued:

 

5.65Zn30†††††††† Chemist Shorthand:____________________________

 

e-1Kr

 

 

 

 

6.85Nb41†††††††† Chemist Shorthand:____________________________

 

 

e-1Xe

 

 

 

 

 

 

 

 

Chapter 2: Part B: Electron Configuration continued:

 

7.96Mo42†††††††† Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

8.180Au79†††††††† Chemist Shorthand:____________________________

e-1Rn

 

 

 

 

 

B#1.Pd46†††††††† Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

B#2.Pt78†††††††† Chemist Shorthand:____________________________

e-1Rn

 

 

 

 

 

 

 

 

B#3.Ag47†††††††† Chemist Shorthand:____________________________

 

e-1Xe

 

 

 

 

B#4.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

 

e-1rules3

 

 

 

 

 

 

 

 

Check Your Answers. Click on the element on the periodic table:

http://fscj.me/e-1Spectroscopic/pc.html

 

Animation of Elements 1-112 filling electrons:

http://www.northcampus.net/ElectronConfiguration/SpectroscopicNotation/spectroscopicNotation.html

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Chapter 2: Part C Orbital Subshells & Periodic Chart†† 1 point

 

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

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

A similar Figure:

 

Hein 7thPage 204

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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

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Chapter2 C1: Spectroscopic Notation using the Periodic Chart 2 Points

Given the Elementís 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] represents1s2 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††††††† ___________________________________________

 

  1. 47Ag†††††† __________________________________________

 

  1. 24Cr††††††† ___________________________________________

 

  1. 7N†††††††† ___________________________________________

 

  1. 17Cl††††††† ___________________________________________

 

 

Look at the Periodic Table and Count the squares Left to Right:

 

 

 

On the fourth row of the periodic table you have to included the 3d orbitals:

 

 

 

Additional reference for your information

 

 

 

 

 

 

 

 

 

Chapter Two: Part D††††††† Electron Dot Formulas†††††††† 1 point

 

Using the periodic chart, draw the electron dot formulas of the following elements (the numbers shown are the elementís 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

 

 

 

 

 

Chapter Two: Part E:†† Electron Configuration of Ions††† 1 point

Given the following ions, use arrows to fill-in the electron configuration of the ion, then rewrite the configuration into the chemistís shorthand:

 

1.†††† Cl1-ion††††† Chemist Shorthand: ___________________________

 

Arorbital

 

2.K1+ ionChemist Shorthand: _____________________________

 

 

e-1Kr

 

Additional reference for your information

 

 

 

 

 

 

 

Remember positive ions have lost electrons from the neutral atom, while negative ions have gained electrons into the neutral atom.

 

 

 

 

Chapter Two: Part F†††††† Periodic Ionic Properties††††††† 1 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

 

 

Dr. Lukacs Pod Casts:

 

Atoms and Ions

http://weinstruct.org/weinstruct/main/lecture/20

 

 

 

 

 

 

 

Chapter Two Part P: Periodic Chart Identification††††† †††††††††1 point

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 fillinga 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

 

Review Corwinís 7th Sections 5.1-5.3 pages 134-138 Additional Questions: p155-6 #8-36

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Main Group Elements are also called Representative Elements

 

 

 

 

 

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