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19 Cards in this Set
- Front
- Back
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1st one
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principle quantum number: (n)
energy lvl of electron i.e. orbital n=1,2,3...7 |
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orbital
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region of space where e- most likely found based on probability
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2nd one
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secondary quantum number: (l)
divides energy lvl into sublevels l = 0, 1, 2, 3 s, p, d, f |
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s
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l=0
sharp |
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p
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l=1
principle |
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d
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l=2
difuse |
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f
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l=3
fundamental |
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3rd one
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magnetic quantum number: (m(sub L))
describes orientation of orbital Ml= -L to L |
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4th one
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spin quantum number: (m(sub s))
electron spinning about an axes 2 poss: clockwise: alpha: +.5 : 1st e- in counterclockwise: beta: -.5 : 2nd e' in |
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Aufbau Principle
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e-'s go into available sublevels of lowest energy
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Pauli Exclusion Principle
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no 2 e-'s in an atom can have the same 4 quantum #s
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Hund's Rule
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electrons enter vacant orbitals until all possible orbitals contain 1e- then they pair up
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Quantum address only describes...
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last electron
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Cr electron configuration
Chromium |
[Ar]3d5 4s1
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Cu electron configuration
Copper |
[Ar]3d10 4s1
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paramagnetic
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Fe Iron
Co Cobalt Ni Nickel |
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y paramagnetic?
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due to unpaired d electrons
Unpaired d's required for magnetism |
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shape of s
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sphere
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shape of p
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dumbell
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