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Models of the
Atom
Bohr’s model…
• Electrons are found in specific
circular paths (orbits) around the
nucleus.
• The electrons have fixed energies
called energy levels. (like rungs on a
ladder)
• The amount of energy required to
move an electron to another energy
level is called a quantum.
The Quantum Mechanical model
• It is based on the energy and possible
location of an electron.
• how likely it is to find an electron is
described in terms of probability. (ie.
Propeller blades)
• Based on work done by Shrodinger…
Atomic Orbitals
• The energy levels of electrons are labeled
by principal quantum numbers (n)
• Each energy sublevel corresponds to an
orbital of a different shape, which describes
where the electron is likely to be found.
Atomic Orbitals
Shapes and
Orientations of
Orbitals
1s Orbital
• Sphere around the nucleus
The one tells you that the electron
is in the orbital closest to the
nucleus
• S tells you about the shape
2s Orbital
• Similar to 1s except the electron is most
likely in the region farther from the nucleus
p Orbitals
• At the first energy level there is only the 1s
orbital, after the second energy level there
are 2p orbitals
• Look like dumbbells
• In the three directions
Remember….
MAX NUMBER OF ELECTRONS
IN AN ENERGY LEVEL
ENERGY LEVEL MAX # OF ELECTRONS
1 2
2 8
3 18
4 32
5 50
Electron
Configuration
A detailed way of showing the
order in which electrons fill in
around the nucleus
Electron Configuration
Symbols
1s2
Energy Level
Sub Level
(s, p, d, f )
# of e- in
sub level
We must follow 3 rules…
• Aufbau priciple
• Electrons occupy energy levels with lowest
energy first.
Pauli exclusion principle
• If 2 electrons occupy the same energy level
they must have opposite spins.
Hund’s rule…
• Electrons that occupy orbitals of the same
energy will have the maximum number of
electrons with the same spin.
• 2p
To start we will use orbital filling
diagrams to help us with electron
configurations….
• Example
Boron- has 5 electrons
Periodic table arrangement
• the quantum theory helps to explain the
structure of the periodic table.
• n - 1 indicates that the d subshell in period 4
actually starts at 3 (4 - 1 = 3).
s (n) d (n - 1) p (n)
1
2
3
4
5
6
7
f (n -2)
Summary: p orbitals and d orbitals
p orbitals look like
a dumbell with 3
orientations: px,
py, pz (“p sub z”).
Four of the d orbitals resemble two dumbells in a
clover shape. The last d orbital resembles a p
orbital with a donut wrapped around the middle.
1st Quantum #
Principle Quantum #
(n)
Specifies the energy level
that the electron is on.
2nd Quantum #
Specifies the shape of the
sub level .
(l)
The 3rd (m) and 4th quantum
numbers (s) …
• Deals with the orbital within the sublevel
and the spin of the electron.
Four Energy Sub-Levels
Energy Level Sub-level Type of sub # of
Orbitals
s Sphere 2 1
p Dumbbell 6 3
d 4-Lobed 10 5
f 6-8 Lobed 14 7

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orbital-shape-orientationt.ppt

  • 2. Bohr’s model… • Electrons are found in specific circular paths (orbits) around the nucleus. • The electrons have fixed energies called energy levels. (like rungs on a ladder) • The amount of energy required to move an electron to another energy level is called a quantum.
  • 3. The Quantum Mechanical model • It is based on the energy and possible location of an electron. • how likely it is to find an electron is described in terms of probability. (ie. Propeller blades) • Based on work done by Shrodinger…
  • 4.
  • 5. Atomic Orbitals • The energy levels of electrons are labeled by principal quantum numbers (n) • Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found.
  • 8. 1s Orbital • Sphere around the nucleus The one tells you that the electron is in the orbital closest to the nucleus • S tells you about the shape
  • 9. 2s Orbital • Similar to 1s except the electron is most likely in the region farther from the nucleus
  • 10. p Orbitals • At the first energy level there is only the 1s orbital, after the second energy level there are 2p orbitals • Look like dumbbells • In the three directions
  • 11.
  • 12.
  • 13.
  • 14. Remember…. MAX NUMBER OF ELECTRONS IN AN ENERGY LEVEL ENERGY LEVEL MAX # OF ELECTRONS 1 2 2 8 3 18 4 32 5 50
  • 15. Electron Configuration A detailed way of showing the order in which electrons fill in around the nucleus
  • 16. Electron Configuration Symbols 1s2 Energy Level Sub Level (s, p, d, f ) # of e- in sub level
  • 17. We must follow 3 rules… • Aufbau priciple • Electrons occupy energy levels with lowest energy first.
  • 18. Pauli exclusion principle • If 2 electrons occupy the same energy level they must have opposite spins.
  • 19. Hund’s rule… • Electrons that occupy orbitals of the same energy will have the maximum number of electrons with the same spin. • 2p
  • 20. To start we will use orbital filling diagrams to help us with electron configurations…. • Example Boron- has 5 electrons
  • 21. Periodic table arrangement • the quantum theory helps to explain the structure of the periodic table. • n - 1 indicates that the d subshell in period 4 actually starts at 3 (4 - 1 = 3). s (n) d (n - 1) p (n) 1 2 3 4 5 6 7 f (n -2)
  • 22. Summary: p orbitals and d orbitals p orbitals look like a dumbell with 3 orientations: px, py, pz (“p sub z”). Four of the d orbitals resemble two dumbells in a clover shape. The last d orbital resembles a p orbital with a donut wrapped around the middle.
  • 23. 1st Quantum # Principle Quantum # (n) Specifies the energy level that the electron is on.
  • 24. 2nd Quantum # Specifies the shape of the sub level . (l)
  • 25. The 3rd (m) and 4th quantum numbers (s) … • Deals with the orbital within the sublevel and the spin of the electron.
  • 26. Four Energy Sub-Levels Energy Level Sub-level Type of sub # of Orbitals s Sphere 2 1 p Dumbbell 6 3 d 4-Lobed 10 5 f 6-8 Lobed 14 7

Editor's Notes

  1. 7
  2. 21
  3. 22