CHM 1032C Name: __________________

Chapter 2 Homework Packet-McMurry 7^th

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 2.8 Answer

D. _____ (01) Electron Dot Structures-Section 2.9 Answers

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

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

P. _____ (01) Periodic Chart Identifications – 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 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:_____________________________________

Chapter 2: Part B: Electron Configuration continued:

3. ⁴⁰Ca₂₀ Chemist Shorthand:____________________________

4. ⁵²Cr₂₄ Chemist Shorthand:____________________________

Chapter 2: Part B: Electron Configuration continued:

5. ⁶⁵Zn₃₀ Chemist Shorthand:____________________________

6. ⁸⁵Nb₄₁ Chemist Shorthand:____________________________

Chapter 2: Part B: Electron Configuration continued:

7. ⁹⁶Mo₄₂ Chemist Shorthand:____________________________

8. ¹⁸⁰Au₇₉ Chemist Shorthand:____________________________

B#1. Pd₄₆ Chemist Shorthand:____________________________

B#2. Pt₇₈ Chemist Shorthand:____________________________

B#3. Ag₄₇ Chemist Shorthand:____________________________

B#4. 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

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 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

Chapter2 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

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 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

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 chemist’s shorthand:

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

2. K¹⁺ ion Chemist Shorthand: _____________________________

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:

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