5.2 Electron Arrangement in Atoms > 1 Copyright © Pearson Education, Inc., or its affiliates. All...

5.2 Electron Arrangement in Atoms >5.2 Electron Arrangement in Atoms >

1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Chapter 5Electrons In Atoms

5.1 Revising the Atomic Model

5.2 Electron Arrangement in Atoms

5.3 Atomic Emission Spectra and the Quantum Mechanical Model



ObjectivesObjectives

1. Define the following terms: electron configurations of elements, electron spin

2. Describe and use the aufbau principle, the Pauli exclusion principle, and the Hund’s rule

3. Write electron configurations of elements



CHEMISTRY & YOUCHEMISTRY & YOU

What makes the electron configuration of an atom stable?

Energy and stability play an important role in determining how electrons are configured in an atom.



What are the three rules for writing the electron configurations of elements?

Electron Configurations

Electron ConfigurationsElectron Configurations

Electron configuration: the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms.



Three rules—

1. the aufbau principle,

2. the Pauli exclusion principle, and

3. Hund’s rule

tell you how to find the electron configurations of atoms.




Aufbau Principle


According to the aufbau principle, electrons occupy the orbitals of lowest energy first. In the aufbau diagram, each box represents an atomic orbital.

Incr

ea

sin

g e

ne

rgy

6s

5s

4s

3s

2s

1s

6p

5p5d

4p

4d

4f

3p

3d

2p



Aufbau Principle


Incr

ea

sin

g e

ne

rgy

6s

5s

4s

3s

2s

1s

6p

5p5d

4p

4d

4f

3p

3d

2p

The aufbau diagram shows the relative energy levels of the various atomic orbitals. Orbitals of greater energy are higher on the diagram.



Aufbau Principle


Incr

ea

sin

g e

ne

rgy

6s

5s

4s

3s

2s

1s

6p

5p5d

4p

4d

4f

3p

3d

2p

The range of energy levels within a principal energy level can overlap the energy levels of another principal level.



Pauli Exclusion Principle

• According to the Pauli exclusion principle, an atomic orbital may describe at most two electrons.

• To occupy the same orbital, two electrons must have opposite spins; that is, the electron spins must be paired.




Pauli Exclusion Principle

• Spin is a quantum mechanical property of electrons and may be thought of as clockwise or counterclockwise.

• A vertical arrow indicates an electron and its direction of spin ( or ).

• An orbital containing paired electrons is written as .




Hund’s Rule

According to Hund’s rule, electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible.




Hund’s Rule

Three electrons would occupy three orbitals of equal energy as follows.

Electrons then occupy each orbital so that their spins are paired with the first electron in the orbital.





Look at the orbital filling diagram of the oxygen atom.

Electron Configurations of Selected Elements

Element 1s 2s 2px 2py 2pz 3sElectron

configuration

H 1s1

He 1s2

Li 1s22s1

C 1s22s22p2

N 1s22s22p3

O 1s22s22p4

F 1s22s22p5

Ne 1s22s22p6

Na 1s22s22p63s1

• An oxygen atom contains _______ electrons.

eight




Look at the orbital filling diagram of the oxygen atom



configuration

H 1s1

He 1s2

Li 1s22s1

C 1s22s22p2

N 1s22s22p3

O 1s22s22p4

F 1s22s22p5

Ne 1s22s22p6

Na 1s22s22p63s1

• The 1s orbital has two electrons of opposite spin.

• The 2s orbital also has two electrons of opposite spin.




Look at the orbital filling diagram of the oxygen atom

• Each of the three 2p orbitals has one electron. The remaining electron now pairs with an electron occupying one of the 2p orbitals.



configuration

H 1s1

He 1s2

Li 1s22s1

C 1s22s22p2

N 1s22s22p3

O 1s22s22p4

F 1s22s22p5

Ne 1s22s22p6

Na 1s22s22p63s1



• A convenient shorthand method for showing the electron configuration of an atom involves writing the energy level and the symbol for every sublevel occupied by an electron.

• You indicate the number of electrons occupying that sublevel with a superscript.


Nitrogen: 1s22s22p3



• For hydrogen, with one electron in a 1s orbital, the electron configuration is written ________ .

• For oxygen, with two electrons in a 1s orbital, two electrons in a 2s orbital, and four electrons in 2p orbitals, the electron configuration is _____________________ .


1s1

1s22s22p4

Note that the sum of the superscripts equals the number of __________ in the atom.electrons



CHEMISTRY & YOUCHEMISTRY & YOU

Explain why the correct electron configuration of oxygen is 1s22s22p4 and not 1s22s22p33s1.

The 2p orbitals are lower in energy than the 3s orbital, so they will be completely filled before any electrons will be found in the 3s orbital.

Hint: apply the aufbau principle



Sample Problem 5.1Sample Problem 5.1

Writing Electron Configurations

The atomic number of phosphorus is 15. Write the electron configuration of a phosphorus atom.




Analyze Identify the relevant concepts.

Phosphorus has ___ electrons. There is a maximum of _____ electrons per orbital. Electrons do not pair up within an energy sublevel (orbitals of equal energy) until

______________________________.

1

When writing electron configurations, the sublevels within the same principal energy

level are written together.

15

two

each orbital already has one electron




Solve Apply the concepts to this problem.

Step 1. Use the aufbau diagram to place electrons in the orbital with the

___________________________ first.

2

1s

lowest energy (1s)




Solve Apply the concepts to this problem.

Step 2. Continue placing electrons in each orbital with the next higher energy level.

2

1s 2s 2p 3p3s 4s




• The electron configuration of phosphorus is 1s22s22p63s23p3.

• The ____________ add up to the number of electrons.

2 Solve Apply the concepts to this problem.

Step 3. Write the electron configuration.

superscripts



Exceptional Electron Configurations• You can obtain correct electron configurations

for the elements up to vanadium (atomic number 23) by following the aufbau diagram for orbital filling.

• If you were to continue in that fashion, however, you would assign chromium and copper the following incorrect configurations.

Cr 1s22s22p63s23p63d44s2

Cu 1s22s22p63s23p63d94s2




Exceptional Electron Configurations

• The correct electron configurations are as follows:

Cr 1s22s22p63s23p63d54s1

Cu 1s22s22p63s23p63d104s1

• These arrangements give chromium a half-filled d sublevel and copper a filled d sublevel.




Exceptional Electron Configurations

Some actual electron configurations differ from those assigned using the aufbau principle because although half-filled sublevels are not as stable as filled sublevels, they are more stable than other configurations.




What is the correct electron configuration of a sulfur atom?

A. 1s22s22p43s23p6

B. 1s22s22p63s23p3

C. 1s22s22p63s23p4

D. 1s22s22p63s63p2



Key ConceptKey Concept

Three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.



Glossary TermsGlossary Terms

• electron configuration: the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms

• aufbau principle: the rule that electrons occupy the orbitals of lowest energy first

• Pauli exclusion principle: an atomic orbital may describe at most two electrons, each with opposite spin direction



Glossary TermsGlossary Terms

• spin: a quantum mechanical property of electrons; it may be thought of as clockwise or counterclockwise

• Hund’s rule: electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible



END OF 5.2END OF 5.2

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