fourth lowest energy level, 16 shells, 1/3/5/7 sub shell
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degenerate
orbitals in the same sub shell are _______
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different
For a given shell, the subshells are NOT degenerate, the subshells have ____ energies
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n
Principle Quantum Number
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l
Angular Momentum Quantum Number
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ml
Magnetic Quantum Number
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smaller
As n increases, the energy differences between shells becomes _______
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overlap
There is an ________ or penetration of the n=4 and higher shells
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4s, 3d
The __ sub shell is lower in energy than the __ sub shell
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5s, 4d
The __ sub shell is lower in energy than the __ sub shell
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6s, 4f, 5d
The __ sub shell is lower in energy than the __ which is lower than the __ sub shell
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Stern-Gerlach Experiment 1922
A fundamental property of electrons is spin. All electrons have the same amount. There are only two possible spin orientations, aligning with an external magnetic field or against. "Spin up or Spin down." The different spins are deflected differently by the magnetic field.
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Ms
the fourth quantum number (spin), independent of ml, l, and n. Either equal to -1/2 or +1/2.
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Pauli Exclusion Principle
no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers (ml, n or l). Electrons that occupy the same orbital have thee identical quantum numbers (ex. 2, 1, 3)
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2
No orbital can contain more than _ electrons. (one up one down)
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electron configuration
Arrangement of electrons in the orbitals of an atom is called an atoms _____ ______
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ground state
the lowest energy state of an atom or other particle
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excited state
the higher energy state of an atom or other particle
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Aufbau Principle
Lowest energy orbitals fill up first, then higher energy orbitals. (Do not pair first!)
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Hund's Rule
For degenerate orbitals (with the same energy), the lowest energy arrangement is attained when the number of electrons with the same spin is maximized.
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condensed notation
Show closest Noble Gas configuration in brackets, with valence electrons
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valence electrons
Determines properties and chemical behaviors of element. Outermost shell, largest n. Most loosely held, involved in bonding.
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core electrons
inner shells, filled orbitals, used to provide shielding for valence electrons from the positive charges from nucleus.
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s-block
1-2 column, 1s for 1st period, 2s for second period, etc. holds two electrons.
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d-block
3-12 column, mostly metals, 3d follows 4s, 4d follows 5s, 5d follows 4f and 6s, 6d follows 5f and 7s. Holds 10 electrons.
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p-block
13-18 column, includes noble gases, holds 6 electrons.
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f-block
transition metals, between s block and d block, holds 14 electrons.
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4
How many unpaired electrons are found in the ground state of iron?
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Anomalous electron configurations
Result from the unusual stability of half-filled and full-filled sub shells. These occur where the sub shell energy differences are small. (ex. 4s v. 3d)
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