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Lecture 2310/28/05
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Quiz 1. What does the quantum number “l” represent? 2. Calculate the wavelength of light emitted when an electron changes from n = 3 to n = 1 in the H atom?
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m l orbital -l... 0... +l orientation Summary: Quantum numbers n shell1, 2, 3, 4,... size and energy l subshell0, 1, 2,... n – 1 shape m s electron spin+1/2 and -1/2 spin
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Pauli Exclusion Principle No two electrons can have the same set of the four quantum numbers (n, l, m l, m s )
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Writing Atomic Electron Configurations 1 1 s value of n value of l no. of electrons spdf notation for H, atomic number = 1 Two ways of writing configurations spdf notation Two ways of writing configurations spdf notation
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Writing Atomic Electron Configurations Two ways of writing configurations orbital box notation. Two ways of writing configurations orbital box notation. One electron has n = 1, l = 0, m l = 0, m s = + 1/2 Other electron has n = 1, l = 0, m l = 0, m s = - 1/2
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Aufbau principle Electrons are added from lowest to highest energy Single electron atom (Bohr) Energy related to n Multi-electron atom Energy related to n + l
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See “Toolbox” for Electron Configuration tool.
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LithiumLithium Group 1A Atomic number = 3 1s 2 2s 1 ---> 3 total electrons
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BoronBoron Group 3A Atomic number = 5 1s 2 2s 2 2p 1 ---> 5 total electrons 5 total electrons
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CarbonCarbon Group 4A Atomic number = 6 1s 2 2s 2 2p 2 ---> 6 total electrons 6 total electrons HUND’S RULE When placing electrons in a set of orbitals having the same energy, fill each with a single electron first
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OxygenOxygen Group 6A Atomic number = 8 1s 2 2s 2 2p 4 ---> 8 total electrons
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