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Related Flashcards
Cards In This Set
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Name the types of spectrums that can be seen when viewing light.
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EmissionContinuousAbsorption
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Define Ground-State and Excited State energy levels.
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Ground-State: An electron in it's normal position.Excited-State: An electron in a position that has higher energy than the normal.
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What are the 4 Quantum Numbers?
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N, l, ml, and ms.
Principal Quantum Number (n)Orbital Shape Quantum Number (l)Magnetic Quantum Number (ml)Spin Quantum Number (ms) |
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What does the Principal Quantum Number represent?
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The energy level on which an electron can be found.
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What does the Orbital Shape Quantum Number represent?
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The Orbital in which an electron can be found.
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What does the Magnetic Quantum Number represent?
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The sub-orbital in which an electron can be found.
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What does the Spin Quantum Number represent?
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The spin of an electron in it's position; Positive or Negative one-half.
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Describe the Pauli Exclusion Principle.
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No two electrons can have the same 4 quantum numbers, because then they would be occupying the same space. Two electrons in the same orbital must have opposite spin values.
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Describe the Aufbau Principle.
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 Electrons fill orbitals based on energy levels; the less, the better. The Aufbau principle shows the most effective way to do so based on the energy levels and orbital shapes. |
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What are the limits to the Orbital Shape Quantum Number?
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It can only go as high as n - 1... or ...The Principal Quantum Number - 1.
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What are the limits to the Magnetic Quantum Number?
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It ranges from -l to +l, including 0.... or ...- to + Orbital Shape Quantum Number, including 0.
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List the Quantum Numbers for Carbon's 17th Electron.
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N = 3l = 1ml = 1ms = -1/2
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What is Hund's rule?
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Electrons will singly occupy each sub-orbital before starting to pair up.
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What is the trend for Ionization Energy as you move across the periodic table?
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Ionization Energy Increases.
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What is the trend for Ionization Energy as you move down the periodic table?
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Ionization Energy Decreases.
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