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Sections 7.1 – 7.3 Electron Spin, Orbital Energies
and Electron Configurations
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Atomic Electronic Structure
In these sections…
a. Electron Spin and Magnetism
b.Energies of Orbitals
c. Electron Configurations of Atoms
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Electron Spin: Electrons exhibit a magnetic field
We think of them as spinning.
They can spin only two ways: think of it as left or right
Spin quantum number: ms can be +1/2 or -1/2
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Magnetic Properties come from additive effects ofelectron spins.
Diamagnetic: all electrons are pairedParamagnetic: 1 or more unpaired electronsFerromagnetic (real magnets): unpaired electrons all lined up in the same direction
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Pauli Exclusion Principle
• No two electrons in an atom can have the same 4 quantum numbers
• n, ℓ, mℓ define an orbital
• Therefore: an orbital can hold only two electrons, with opposite spins because ms can only be +1/2 or -1/2
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Pauli Exclusion Principle
What’s allowed?
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Orbital Energies
Why? With a single electron, energy depends only on how far from the nucleus.With multiple electrons, e-e- repulsions also play a role and differ depending on orbital shape.
Single Electron Atoms Multi-electron Atoms
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For most atoms: Energy increases as n increases: 1 < 2 < 3 < 4 … Energy increases as subshells progress: s < p < d < f
Single Electron Atoms Multi-electron Atoms
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Atomic Electron ConfigurationsAn atom has lots of electrons and lots of orbitals.
Which orbitals do the electrons occupy?
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Atomic Electron Configurations
An atom has lots of electrons and lots of orbitals.
Which orbitals do the electrons occupy?
Electrons fill the lowest energy orbitals first.
Electron Configuration: a listing of how many electrons occupy each orbital.
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Electron Configurations
General Rule: electrons fill lowest energy orbitals first
Sodium, Na as an example
Na has 11 electrons.Fill 2 electrons per orbital till you run out
A box represents an orbital.An arrow represents an electron.
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Electron Configurations:Three Notation Types
2. spdf (or spectroscopic) notation:
List subshells and how many electrons they contain:
1s22s22p63s1
3. Noble gas notation: short
[Ne]3s1
Where [Ne] = 1s22s22p6
1.
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Electron Configurations and thePeriodic Table
Examples using Electron Configuration Simulation
• Periodic Blocks
• Hund’s Rule (using the p block)
• n value increases as you move down table
• Anomalies: Cr and Cu
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Electron Configurations and thePeriodic Table: Periodic Blocks
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Electron Configurations and the Periodic Table II
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Periodic Table and the Order of Filling
In what order are subshells filled?
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Hund’s Rule: Subshells are filled to give the maximum number of unpaired electrons
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Using Periodic Blocks: C
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Using Periodic Blocks: Cl
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Noble Gas Notation: Mg
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Noble Gas Notation: Mg
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Diamagnetic vs. Paramagnetic Elements
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d-Block Elements: Fe
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Two Anomalies: Cr and Cu
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