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Electron Orbitals
Notes (on your template)
Implication of Heisenberg Uncertainty Principle
Link to Heisenberg and Probability

The implication of the Heisenberg Uncertainty
Principle is that it is impossible to trace the exact
trajectory (path) that an electron will follow.
The more accurately the position of the electron is known, less
accurately the momentum is known.
De Broglie/ Schrodinger: Treating
electron as a standing wave
Only certain specific electron wavelengths will fit in the space
occupied by the standing wave without destructive interference
Since wavelength determines energy, restricted
wavelengths means restricted energies
Schrodinger converted the wave equations in
orbital descriptions (probability maps)

It is only possible to describe the probability of
an electron being in a particular region of space
at a particular time.
Modern Quantum Theory CANNOT describe the exact path
(orbit) of an electron. The Modern Wave Mechanical model describes a
general area of SPACE where there is a HIGH PROBABILITY
of finding an electron.

Orbital: a region of space (3D) in which
there is a high (90%) probability of
locating an electron.
Orbital ≠ Orbit
Firefly Analogy for Electron Orbital
Firefly’s position at different
times in a dark room revealed
by instantaneous flash
HW 8-5, p. 334: #26,27,28
Capacity of an Orbital:
Each orbital can hold a total (maximum)
2 electrons (1 pair).
of ____
Types (or Shapes) of Orbitals:
s Orbital
Shape: spherical
Number: 1
(per energy level)
Types (or Shapes) of Orbitals:
p Orbital
Shape: peanut
Number: 3
p
(per energy level); levels 2-7
P-orbitals come as a set of 3
P –orbitals link
s orbitals are found in every energy level;
p orbitals are found in level 2 or higher orbitals
Remember that the shape of an orbital does
NOT represent a path of the electron!
The shape is a 3D region of space in which
the electron is free to move.
Types (or Shapes) of Orbitals:
d Orbital
Shape: Daisy
Number: 5
(per energy level); levels 3-7
D orbitals appear in level 3 or higher
For test be able to draw s, p and d orbitals
Types (or Shapes) of Orbitals:
f Orbital (Do NOT have draw for test)
Number: 7
(per energy level); levels 4-7
Electron orbitals and Energy Levels
Connection between orbitals and Periodic Table
Relationship between energy and size of orbital
In general: The higher the energy level, the
larger the average distance of the electron
is from the nucleus.
Higher Energy Level = Bigger Orbital
(on average e- are farther from nucleus)
High Energy Level = Bigger
orbital
Higher Energy Level =
Bigger Orbital (on
average e- are farther
from nucleus)
2p orbital
3p orbital
The 1s orbital is a
sphere, centered
around the nucleus
(l = 0)
once the
1s orbital
is filled,
once the
1s orbital
is filled,
the 2s orbital
begins to fill
around the
1s orbital
once the 2s
orbital is
filled,
the 2p orbitals
begin to fill
each 2p orbital
intersects the
2s orbital and
the 1s orbital
each 2p orbital
gets one electron
before pairing begins
once each 2p orbital
is filled with a pair
of electrons, then
the 3s orbital
gets the next
two electrons
the 3s electrons
have a higher energy
than 1s, 2s, or 2p
electrons,
so 3s electrons are
generally found
further from the
nucleus than 1s,
2s, or 2p electrons