Electron arrangement in atoms
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Transcript of Electron arrangement in atoms
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Chapter 5
Electron Arrangement in Atoms
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What are the three rules for writing the electron configurations of elements?
Electron Configurations
Electron ConfigurationsElectron Configurations
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The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations.
Electron ConfigurationsElectron Configurations
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Three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.
Electron ConfigurationsElectron Configurations
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Aufbau Principle
Electron ConfigurationsElectron Configurations
According to the aufbau principle, electrons occupy the orbitals of lowest energy first. In the aufbau diagram, each box represents an atomic orbital.
Incr
easi
ng e
nerg
y
6s
5s
4s
3s
2s
1s
6p
5p5d
4p
4d
4f
3p
3d
2p
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Aufbau Principle
Electron ConfigurationsElectron Configurations
Incr
easi
ng e
nerg
y
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.
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Aufbau Principle
Electron ConfigurationsElectron Configurations
Incr
easi
ng e
nerg
y
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.
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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.
Electron ConfigurationsElectron Configurations
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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 .
Electron ConfigurationsElectron Configurations
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Hund’s RuleAccording 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.
Electron ConfigurationsElectron Configurations
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Hund’s RuleThree electrons would occupy three orbitals of equal energy as follows.
Electron ConfigurationsElectron Configurations
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Hund’s RuleThree 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.
Electron ConfigurationsElectron Configurations
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Electron ConfigurationsElectron Configurations
Look at the orbital filling diagram of the oxygen atom. Electron Configurations of Selected Elements
Element 1s 2s 2px 2py 2pz 3s Electron configuration
H 1s1
He 1s2
Li 1s22s1
C 1s22s22p2
N 1s22s22p3
O 1s22s22p4
F 1s22s22p5
Ne 1s22s22p6
Na 1s22s22p63s1
• An oxygen atom contains eight electrons.
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Electron ConfigurationsElectron Configurations
Look at the orbital filling diagram of the oxygen atom. Electron Configurations of Selected Elements
Element 1s 2s 2px 2py 2pz 3s Electron 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.
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Electron ConfigurationsElectron Configurations
Look at the orbital filling diagram of the oxygen atom. Electron Configurations of Selected Elements
Element 1s 2s 2px 2py 2pz 3s Electron 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.
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Electron ConfigurationsElectron Configurations
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.
Electron Configurations of Selected Elements
Element 1s 2s 2px 2py 2pz 3s Electron configuration
H 1s1
He 1s2
Li 1s22s1
C 1s22s22p2
N 1s22s22p3
O 1s22s22p4
F 1s22s22p5
Ne 1s22s22p6
Na 1s22s22p63s1
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• 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.
Electron ConfigurationsElectron Configurations
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• 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.
Electron ConfigurationsElectron Configurations
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• For hydrogen, with one electron in a 1s orbital, the electron configuration is written 1s1.
Electron ConfigurationsElectron Configurations
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• For hydrogen, with one electron in a 1s orbital, the electron configuration is written 1s1.
• 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 1s22s22p4.
Electron ConfigurationsElectron Configurations
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• For hydrogen, with one electron in a 1s orbital, the electron configuration is written 1s1.
• 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 1s22s22p4.
Electron ConfigurationsElectron Configurations
Note that the sum of the superscripts equals the number of electrons in the atom.
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Sample Problem 5.1
Analyze Identify the relevant concepts.
Phosphorus has 15 electrons. There is a maximum of two electrons per orbital. Electrons do not pair up within an energy sublevel (orbitals of equal energy) until each orbital already has one electron.
1
When writing electron configurations, the sublevels
within the same principal energy level are written
together.
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Sample Problem 5.1
Solve Apply the concepts to this problem.
• Use the aufbau diagram to place electrons in the orbital with the lowest energy (1s) first.
2
1s
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Sample Problem 5.1
Solve Apply the concepts to this problem.
• Use the aufbau diagram to place electrons in the orbital with the lowest energy (1s) first.
• Continue placing electrons in each orbital with the next higher energy level.
2
1s 2s 2p 3p3s 4s
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Sample Problem 5.1
• The electron configuration of phosphorus is 1s22s22p63s23p3.
• The superscripts add up to the number of electrons.
2 Solve Apply the concepts to this problem.
Write the electron configuration.
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Exceptional Electron Configurations
Electron ConfigurationsElectron Configurations
• You can obtain correct electron configurations for the elements up to vanadium (atomic number 23) by following the aufbau diagram for orbital filling.
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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
Electron ConfigurationsElectron Configurations
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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.
Electron ConfigurationsElectron Configurations
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Exceptional Electron ConfigurationsSome 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.
Electron ConfigurationsElectron Configurations
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What is the correct electron configuration of a sulfur atom?
A. 1s22s22p43s23p6
B. 1s22s22p63s23p3
C. 1s22s22p63s23p4
D. 1s22s22p63s63p2
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What is the correct electron configuration of a sulfur atom?
A. 1s22s22p43s23p6
B. 1s22s22p63s23p3
C. 1s22s22p63s23p4
D. 1s22s22p63s63p2
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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.