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Published byDerick Barker Modified over 9 years ago
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Aufbau Principle An electron occupies the lowest energy orbital that can receive it.
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Pauli Exclusion Principle No two electrons in the same atom can have the same set of four quantum numbers.
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Hund’s Rule Orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.
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Heisenberg Uncertainty Principle It is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.
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Bohr Model of Hydrogen http://science.sbcc.edu/physics/solar/sciencesegment/boh ratom.swf
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Symbolized by n Indicates the energy level Values are all positive integers # of orbitals in energy level = n 2
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Symbolized by l Indicates the shape of the orbital Values of l: 0 and all integers ≤ n-1
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Symbolized by m Indicates the orientation of an orbital around the nucleus
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Has only two possible values +1/2, -1/2 Indicates the two fundamental spin states of an electron in an orbital
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Chapter 4 Things to Review Vocabulary Electron Configuration Orbital Notation Noble Gas Configuration Bohr’s Model of Hydrogen Wave: crest, trough, amplitude, wavelength Calculations: Energy, Wavelength, Frequency
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Chapter 4 Review page 118 1, 3, 4, 6, 8, 9,11,12, 13, 14a&b, 16, 17,18a, 19a, 20, 21, 22, 23, 24,25, 36, 27, 28. 29, 30, 32, 36, 37, 39, 40, 41, 42, 43, 44, 44, 45 1, 3, 4, 6, 8, 9, 11-13, 14a&b, 16, 17,18a, 19a, 20-30, 32, 36, 37, 39- 45
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