OrbitalOrbital ConfigurationConfiguration

By: Allison SticklerBy: Allison Stickler

OverviewOverview

1.1. Review of quantum numbersReview of quantum numbers2.2. What is an orbital?What is an orbital?3.3. What is orbital configuration?What is orbital configuration?4.4. Pauli Exclusion PrinciplePauli Exclusion Principle5.5. Hund’s RuleHund’s Rule6.6. Review of rulesReview of rules7.7. QuizQuiz8.8. sourcessources

quantum numbers in quantum numbers in reviewreview

11stst-n- outer -n- outer shellshell

22ndnd -l- subshell -l- subshell33rdrd -m- -m-

direction in direction in spacespace

44thth -s- the spin -s- the spin

11stst quantum number quantum number

The numbers refer to the 1The numbers refer to the 1stst quantum number, the outer quantum number, the outer shell.shell.

22ndnd quantum number quantum numberThe letters refer to the 2The letters refer to the 2ndnd quantum number, the subshell.quantum number, the subshell.

The third and fourth quantum The third and fourth quantum numbers deal directly with numbers deal directly with

orbital configuration!orbital configuration!

33rdrd quantum number quantum number

m= direction in spacem= direction in space x, y, and z x, y, and z Only allowed 2 electrons per Only allowed 2 electrons per

orbitalorbital

44thth quantum number quantum number

Shows direction of the spinShows direction of the spin values of spin include:values of spin include:

+1/2 called up or clockwise +1/2 called up or clockwise

-1/2 called down or counter -1/2 called down or counter clockwiseclockwise

What is an Orbital?What is an Orbital?

An orbital is a An orbital is a three-dimensional three-dimensional region around the region around the nucleus in which an nucleus in which an electron moves.electron moves.

What is Orbital Configuration?What is Orbital Configuration?

It shows the spin of an electronIt shows the spin of an electron

*the actual *the actual ↑↓↑↓ (up and down)* (up and down)* Example of Oxygen Example of Oxygen

↑↓↑↓ ↑↓↑↓ ↑↓ ↑ ↑↑↓ ↑ ↑

Examples of orbital Examples of orbital configurationconfiguration

*It is important to *It is important to remember…*remember…*

Orbital configuration is Orbital configuration is not 1s2 2s2 2p6… etc. not 1s2 2s2 2p6… etc.

That is electron That is electron configuration, a different configuration, a different

concept!concept!

The following are two The following are two

rules that you rules that you mustmust apply when writing an apply when writing an orbital configuration!orbital configuration!

Pauli Exclusion PrinciplePauli Exclusion Principle

No orbital can have more No orbital can have more than two electrons in it.than two electrons in it.

↑↓↑↓ ↑↓↑↓ ↑ ↑ ↑ ↑ ↑ ↑ 1s2 2s2 2p3

*NOT*↑↓↑↑↓↑ ↑↓↑↑↓↑ ↑ ↑ ↑ ↑ ↑ ↑

1s2 2s2 2p3

Pauli Exclusion con’tPauli Exclusion con’t

Two electrons in the same Two electrons in the same orbital must have opposite orbital must have opposite

spins.spins.

ex. ex. ↓↑↓↑

*NOT**NOT* ↓↓↓↓ or or ↑↑↑↑

Hund’s RuleHund’s Rule

Within a subshell, the electrons Within a subshell, the electrons will occupy the orbitals singly will occupy the orbitals singly

first.first. ↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑ ↑ ↑ ↑

1s2 2s2 2p3

*NOT**NOT*

↑↓↑↓ ↑↓ ↑↓ ↑↓ ↑↑↓ ↑__ __ 1s2 2s2 2p3

Hund’s RuleHund’s Rule

All electrons in singly occupied All electrons in singly occupied orbitals, have the same spin.orbitals, have the same spin.

↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑ ↑ ↑ ↑ 1s2 2s2 2p3 all spins are up

*NOT*↑↓↑↓ ↑↓ ↑↓ ↑ ↓ ↑↑ ↓ ↑1s2 2s2 2p3

all must go up before

adding the second electron in the pair

*Remember**Remember*

1. Must put clockwise or up first1. Must put clockwise or up first ex. ex. ↑↓↑↓ *NOT* *NOT* ↓↑↓↑

2. No orbital can have more than 2. No orbital can have more than two electrons in it.two electrons in it.

3. Two electrons in the same orbital 3. Two electrons in the same orbital must have opposite spins.must have opposite spins.

4.Fill each shell first, then fill the 4.Fill each shell first, then fill the subshells.subshells.

5. Only two directions are allowed 5. Only two directions are allowed for an electron in an atom.for an electron in an atom.

6. Within a subshell, the electrons 6. Within a subshell, the electrons will occupy the orbitals singly will occupy the orbitals singly first.first.

7. 7. All electrons in singly occupied All electrons in singly occupied orbitals, have the same spin.orbitals, have the same spin.

Now you can take a quiz on Now you can take a quiz on Orbital Configuration to Orbital Configuration to

see if you are an expert.see if you are an expert.

Quiz Quiz

(1)According to the Pauli Exclusion Principle, (1)According to the Pauli Exclusion Principle, choose the correct answer.choose the correct answer.

A. A. ↑↓↑↓ ↑↓↑↓ ↑ ↑ ↑ ↑ ↑ ↑

B. B. ↑↓↑↑↓↑ ↑↓↑↑↓↑ ↑ ↑ ↑ ↑ ↑ ↑

C. C. ↑↑↑↑ ↓↓↓↓ ↓ ↓ ↓↓ ↓ ↓

Great answer Great answer

Click Click here here for question #2 for question #2

Woops!Woops!

The right answer is…The right answer is…A)A)↑↓↑↓ ↑↓↑↓ ↑ ↑ ↑↑ ↑ ↑

click here for an explanation

ExplanationExplanation

No orbital can have more No orbital can have more than two electrons in it.than two electrons in it.

↑↓↑↓ ↑↓↑↓ ↑ ↑ ↑ ↑ ↑ ↑ 1s2 2s2 2p3

*NOT*↑↓↑↑↓↑ ↑↓↑↑↓↑ ↑ ↑ ↑ ↑

1s2 2s2 2p3 click here for question #2

(2)According to the Pauli Exclusion Principle, choose the

correct answer.

A)A)↑↑↑↑ ↑↑↑↑

B)B)↑↓↑↓ ↑↓↑↓

C)C)↓↓↓↓ ↓↓↓↓

Stellar Job!Stellar Job!

Keep it up!Keep it up!

Click here for question #3Click here for question #3

Sorry Sorry

The correct answer is…The correct answer is…

B) B) ↑↓↑↓ ↑↓↑↓ ↑ ↑ ↑↑ ↑ ↑

Click here for an explanation

ExplanationExplanation

Two electrons in the same orbital Two electrons in the same orbital must have opposite spins.must have opposite spins.

ex. ex. ↓↑↓↑

*NOT**NOT* ↓↓↓↓ or or ↑↑↑↑

click here for question #3

(3) According to Hund’s Rule (3) According to Hund’s Rule choose the correct orbital choose the correct orbital configuration.configuration.

A) ↑↓ ↑↓ ↑ ↑ ↑B) ↑↓ ↑↓ ↑↓ ↑__C) ↑↓ ↑↓ ↑ ↑↓__

Wow!Your doing

awesome…pat yourself on the

back!

Click here for question #4

You thought wrong…the right answer isA)A)↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑ ↑ ↑ ↑ . T. Try looking at this explanation to see where you went wrong.

Hund’s RuleHund’s Rule

Within a subshell, the electrons will Within a subshell, the electrons will occupy the orbitals singly first.occupy the orbitals singly first.

↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑ ↑ ↑ ↑ 1s2 2s2 2p3

*NOT**NOT*

↑↓↑↓ ↑↓ ↑↓ ↑↓ ↑↑↓ ↑____ 1s2 2s2 2p3 click here for question #4

(4) According to Hund’s Rule choose the correct orbital

configuration.

A)A) ↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑↑ ↑ ↑

B)B) ↑↓↑↓ ↑↓ ↑↓ ↑ ↓ ↑↑ ↓ ↑

C)C) ↑↓↑↓ ↑↓ ↑↓ ↑ ↓ ↑↑ ↓ ↑

Wooopeee!

You’re amazing

click here for your last question!

Caution!Caution!

Wrong AnswerWrong Answer

The right answer is:The right answer is:A) A) ↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑↑ ↑ ↑

click click herehere for an explanation. for an explanation.

ExplanationExplanation

All electrons in singly occupied orbitals, All electrons in singly occupied orbitals, have the same spin.have the same spin.

↑↓↑↓ ↑↓ ↑↓ ↑ ↑ ↑ ↑ ↑ ↑ 1s2 2s2 2p3 all spins are up

*NOT*

↑↓↑↓ ↑↓ ↑↓ ↑ ↓ ↑↑ ↓ ↑1s2 2s2 2p3

all must go up before

Click here for adding the second Your last question electron in the pair

(5) Knowing that the electron (5) Knowing that the electron configuration of fluorine is 1s2 configuration of fluorine is 1s2 2s2 2p5, choose which is the 2s2 2p5, choose which is the correct orbital configuration.correct orbital configuration.

A)A) ↑↓↑↓ ↑↓ ↑↓ ↑ ↓↑ ↑↓ ↑ ↓↑ ↑↓

B) B) ↑↓↑↓ ↑↓↑↓ ↓↑ ↑↑ ↓ ↓↑ ↑↑ ↓

C)C) ↑↓↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↑↓ ↑↓ ↑

You have just completed the You have just completed the orbital configuration quiz! orbital configuration quiz!

If you feel you need more help click If you feel you need more help click herehere to view this again. to view this again.

If you feel that you are an expert, If you feel that you are an expert, click click herehere to view the sources used. to view the sources used.

Whoops!Whoops!

The correct answer is:The correct answer is:

C) C) ↑↓↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↑↓ ↑↓ ↑

If you feel you need more help click If you feel you need more help click herehere to view this again. to view this again.

If you feel that you are an expert, If you feel that you are an expert, click click herehere to view the sources used. to view the sources used.

SourcesSources

http://www.chemistry.mcmaster.ca/http://www.chemistry.mcmaster.ca/esam/Chapter_8/section_1.htmlesam/Chapter_8/section_1.htmlhttp://www.chem.purdue.edu/gchelp/http://www.chem.purdue.edu/gchelp/gloss/hundsrule.html gloss/hundsrule.html hyperphysics.phy-astr.gsu.edu/.../hyperphysics.phy-astr.gsu.edu/.../eleorb.htmleleorb.htmlMr. Wolfe’s chemistry 1 notesMr. Wolfe’s chemistry 1 notesSevenair, John P. and Burkett, Allan R. Sevenair, John P. and Burkett, Allan R. Introductory Chemistry: Investigating the Introductory Chemistry: Investigating the Molecular Nature of Matter.Molecular Nature of Matter. Pages 203- Pages 203-209. 209.