Pathway 4: Chapter 4 Homework Pack

Chapter 4: Subatomic Particles

Part A: Atomic Notation Answers

Part B: Electron Configuration Answers

Part B1: Electron Configuration of Ions Answers

Part C: Orbitals and Subshells of the Periodic Table Answer

Part D: Spectroscopic Notation from Periodic Table Answer

Part P: Periodic Properties Answer
Part P1: Electron Dot Structures using the Periodic Table Answers
Part P2: Periodic Ionic Character using the Periodic Table Answers

Part S: Shapes of Orbitals
Part V: Chapter 4 Vocabulary Chapter 4 pages 123-124 Answers

Module Three: Part A Atomic Notation

Chapter 4 Part A: Atomic Notation

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 4 Part B: Electron Configuration

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 4: Part B: Electron Configuration

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 4: Part B: Electron Configuration continued:

3. ⁴⁰Ca₂₀ Chemist Shorthand:____________________________

4. ⁵²Cr₂₄ Chemist Shorthand:____________________________

Chapter 4: Part B: Electron Configuration continued:

5. ⁶⁵Zn₃₀ Chemist Shorthand:____________________________

6. ⁸⁵Nb₄₁ Chemist Shorthand:____________________________

Chapter 4: 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:____________________________

Chapter 4 Part B1: Electron Configuration of Ions

Chapter 4 Part B1: Electron Configuration of Ions

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: _____________________________

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

Negative Ions are always isoelectronic with the Nobel Gas at the end of the period:

Nitride N^3- Ion is isoelectronic with the Neon atom
Oxide O^2- Ion is isoelectronic with the Neon Atom
fluoride F^1- Ion is isoelectronic with the Neon Atom

Positive Ions are always isoelectronic with the Nobel Gas which ends the
previous period:

Aluminum Al³⁺ Ion is isoelectronic with the Neon atom
Magnesium Mg²⁺ Ion is isoelectronic with the Neon Atom
Sodium Na¹⁺ Ion is isoelectronic with the Neon Atom

How about the Hydrogen atom which some classify as an element in a class by itself CAN become an ion (two different ways).

1. H^1- ion Chemist Shorthand: ___________________________

2. H¹⁺ ion Chemist Shorthand: _____________________________

Chapter 4: Part C Orbital Subshells & Periodic Chart:

A lot of students label the helium box 1p.

A lot of students label the 3d block of elements as 4d!

Chapter 4: Part C Orbital Subshells & Periodic Chart Sample Exam
On the periodic chart below show all the s, p, d and f block elements on 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

Chapter 4 Part C1: Spectroscopic Notation from Periodic Chart
Sample #1: Write the spectroscopic notation of the Chlorine atom:
a. Chlorine is on the third row of the periodic table.
b. Neon is the Nobel Gas which ends the second period. Write [Ne] to begin the answer.
c. Look at the Periodic Table and Count the squares Left to Right on the third row to the chlorine atom.
d. write 3s² after count 1,2
e. then 3,4,5,6,7 to Chlorine and write 3p⁵
Answer: [Ne] 3s²3p⁵

Sample #2: Write the spectroscopic notation for Selenium atom:

On the fourth row of the periodic table you have to include the 3d orbitals when counting from left to right: #1,2=4s^#; #3-12=3d¹⁰; #13,14,15,16=4p⁴

Answer: [Ar] 4s²3d¹⁰4p⁴

Chapter 4 Part C1: 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

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 Kernel).

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 ___________________________________________

Chapter 4 Part F1: Electron Dot Structures using the Periodic Table

Please Note how Helium is different. Why?

Chapter 4: Part F1 Electron Dot Formulas of Atoms

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

Chapter 4: Part F2 Periodic Ionic Character

Chapter 4: Part F2 Periodic Ionic Properties

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 _____

Chapter 4 Part F: Periodic Properties
Same as Chapter 3 Part P

Pathway 4: Chapter 4 Vocabulary
Fill the blanks with word or the words that best fit the description
Reference Chapter 4 Page 123-124.

1._____________________ The total mass of an atom. The atomic mass of each element presented in the periodic table is the average atomic mass of the various isotopes of that element occurring in nature.

2. _____________________The dense, positively charged center of every atom.

3. _____________________The number of protons in the atomic nucleus of each atom of a given element.

4. _____________________The pattern of frequencies of electromagnetic radiation emitted by the atoms of an element, considered to be an element’s “fingerprint.”

5. _____________________A representation of a system that helps us predict how the system behaves.

6. _____________________The nuclear charge experienced by outer-shell electrons, diminished by the shielding effect of inner-shell electrons and also by the distance from the nucleus.

7. _____________________The complete range of waves, from radio waves to gamma rays.

8. _____________________ An extremely small, negatively charged subatomic particle found outside the atomic nucleus.

9. _____________________The arrangement of an atom’s electrons within orbitals.

10. _____________________A schematic drawing used to arrange atomic orbitals in order of increasing energy levels.

11. _____________________The tendency of inner-shell electrons to partially shield outer-shell electrons from the attractive pull exerted by the positively charged nucleus.

12. _____________________The amount of energy needed to pull an electron away from an atom.

13. _____________________ Any member of a set of atoms of the same element whose nuclei contain the same number of protons but different numbers of neutrons.

14. _____________________The number of nucleons (protons plus neutrons) in the atomic nucleus. Used primarily to identify isotopes.

15. _____________________ An electrically neutral subatomic particle found in atomic nuclei.

16. _____________________ Any subatomic particle found in an atomic nucleus. Another name for either proton or neutron.

17. _____________________A representation of an object on some convenient scale.

18. _____________________ A positively charged subatomic particle in atomic nuclei.

19. _____________________ A small, discrete packet of energy.

20. _____________________An integer that specifies the quantized energy level within an atom.

21. _____________________ A graphic representation of a collection of orbitals of comparable energy in a multielectron atom. A shell can also be viewed as a region of space about the atomic nucleus within which electrons may reside.

22. _____________________ A device that uses a prism or diffraction grating to separate light into its color components and measure their frequencies.