CHM 1025C Name: __________________

Module Three Homework Packet-Hein

Module 3i: Atomic Theory & The Periodic Chart (Chapter 5 ,10)

A. _____ (02) Atomic Notation-Section 5.5 Answers

B. _____ (08) Electron Configuration-Sections 10.4 Answers

C. _____ (03) Orbitals / Subshells of the Periodic Table-Section 10.5 Answer

C1. ____ (06) Spectroscopic Notation from Periodic Chart Section 10.5 Answer

_______(19) Module 3i Total (Fifth Exam)

Module 3ii: Atomic Theory & The Periodic Chart (Chapter 5, 6, & 11)

D. _____ (02) Electron Dot Structures-Section 11.2 Answers

E. _____ (03) e^-1 Configuration of Ions-lecture Answers

F. _____ (02) Periodic Ionic Character-Section 6.2 Answers

P. _____ (04) Periodic Chart Identifications – Chapter 5 Answer

_______(11) Module 3ii Total (Sixth Exam)

Module Three: 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 = ______

Additional Homework (not required) for your practice:

Corwin 7^th edition Section 4.4: Page 127 Questions #17-24

Hein 14^th edition Section 5.5: Page 05 Questions #9-26 especially #17-18

Module Three: Part B: Electron Configuration 5 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

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

Additional reference for your information

Corwin 7^th Sections 4.10-4.11 Pages 119-129

Hein 14^th Sections 10.3-10.4 Pages 195-201

Additional Homework (Not required) for your practice and study for MC exam:

Corwin 7^th: Energy levels and Subshells: Questions #65-72

Corwin 7^th: Electron Configuration: Questions #73-78

Corwin 7^th:Quantum Mechanical Model of the Atom: #79-86

Hein 14^th: Orbitals/e^1- Configuration Questions #7-30 especially #11-22

Module Three: 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

Corwin’s 7^th edition: Sections 5.6 See Figure 5.6 on Pages 143-144

Hein’s 14^th edition: Section 10.5 See Figure 10.16 page 204

A similar Figure:

Hein 7^th Page 204

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 2 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 __________________________________________

2. ³⁰Zn __________________________________________

3. ³⁵Br __________________________________________

4. ⁷⁴W ___________________________________________

5. ⁸O ___________________________________________

6. ¹⁵P ___________________________________________

7. ⁴⁷Ag __________________________________________

8. ²⁴Cr ___________________________________________

9. ⁷N ___________________________________________

10. 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

Corwin 7^th: Section 5.6 Page 144 See example 5.7 p144

Hein 14^th: Section 10.5 Pages 201-206 see example10.5 p205/try 10.6

Additional Homework (Not required) for your practice and study for MC exam:

Corwin 7^th : Blocks of Elements: p157 #47-56
Hein 14^th : Page 209 Questions 45-46

Module Three: 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 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

Corwin 7^th: Section 5.8 Pages 146-147 See example 5.9 p147

Hein’s 14^th: Section 11.2 Pages 216-217 see figure 11.4 try example 11.2

Hein’s 14^th: Try Questions 14-15 page 241

Module Three: 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 chemist’s shorthand:

1. Cl^{1- ion} Chemist Shorthand: ___________________________

2. K¹⁺ ion Chemist Shorthand: _____________________________

Additional reference for your information

Corwin’s 7^th : Section 5.10 Pages 151 See Example 5.13 p151-152

Hein’s 14^th : Section 11.3 Pages217-218 See images page 218

Additional Homework Problems (not Required) Corwin Ionic Charges P157-8 #75-80

Hein’s 14^th :Questions #23-24 page 242

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 1 point

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

Corwin’s 7^th: Section 5.7 Pages 145-146 See example 5.8 p145

Corwin’s 7^th: Section 5.10 Pages 149-151 See Examples 5.11-5.12 p150

Hein’s 14^th: Section 6.2 pages 100-103 See Figure 6.2 page103

Hein’s 14^th: Section 11.3 Pages 217-222 See Example 11.7 & 11.8 p222

Additional Homework Problems (not Required)
Corwin’s 7^th Ionic Charges P157 #71-74
Hein’s 14^th p242 Questions #13-16

Module Three Part P: Periodic Chart Identification 2 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

Review Corwin’s 7^th Sections 5.1-5.3 pages 134-138 Additional Questions: p155-6 #8-36

Main Group Elements are also called Representative Elements