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Published byGrady Marris Modified over 3 years ago

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Electron Orbitals Cartoon courtesy of lab-initio.com

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**Quantum Mechanical Model of the Atom**

Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found. These laws are beyond the scope of this class…

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**Heisenberg Uncertainty Principle**

“One cannot simultaneously determine both the position and momentum of an electron.” The more certain you are about where the electron is, the less certain you can be about where it is going. The more certain you are about where the electron is going, the less certain you can be about where it is. Werner Heisenberg

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Quantum Numbers Each electron in an atom has a unique set of 4 quantum numbers which describe it. Principal quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number

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**Electron Energy Level (Shell)**

Generally symbolized by n, it denotes the probable distance of the electron from the nucleus. “n” is also known as the Principle Quantum number Number of electrons that can fit in a shell: 2n2

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Electron Orbitals An orbital is a region within an energy level where there is a probability of finding an electron. Orbital shapes are defined as the surface that contains 90% of the total electron probability. The angular momentum quantum number, generally symbolized by l, denotes the orbital (subshell) in which the electron is located.

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**s Orbital shape The s orbital**

(l = 0) has a spherical shape centered around the origin of the three axes in space.

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p orbital shape There are three dumbbell-shaped p orbitals (l = 1) in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.

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d orbital shapes Things get a bit more complicated with the five d orbitals (l = 2) that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells” …and a “dumbell with a donut”!

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**Shape of f (l = 3) orbitals**

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**Energy Levels, Sublevels, Electrons**

Sublevels in main energy level (n sublevels) Number of orbitals per sublevel Electrons per sublevel electrons per level (2n2) 1 s 2 p 3 6 8 d 5 10 18 4 f 7 14 32

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**Magnetic Quantum Number**

The magnetic quantum number, generally symbolized by m, denotes the orientation of the electron’s orbital with respect to the three axes in space.

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Orbital filling table

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Electron Spin The Spin Quantum Number describes the behavior (direction of spin) of an electron within a magnetic field. Possibilities for electron spin:

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**Pauli Exclusion Principle**

Two electrons occupying the same orbital must have opposite spins Wolfgang Pauli

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**Element Configuration notation Orbital notation Noble gas**

Lithium 1s22s1 ____ ____ ____ ____ ____ 1s s p [He]2s1 Beryllium 1s22s2 [He]2s2 Boron 1s22s2p1 [He]2s2p1 Carbon 1s22s2p2 [He]2s2p2 Nitrogen 1s22s2p3 1s s p [He]2s2p3 Oxygen 1s22s2p4 [He]2s2p4 Fluorine 1s22s2p5 [He]2s2p5 Neon 1s22s2p6 [He]2s2p6

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Exclusion Warning! Assigning quantum numbers to electrons has been exluded and will not be tested! The following slides are purely for your entertainment

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Assigning the Numbers The three quantum numbers (n, l, and m) are integers. The principal quantum number (n) cannot be zero. n must be 1, 2, 3, etc. The angular momentum quantum number (l ) can be any integer between 0 and n - 1. For n = 3, l can be either 0, 1, or 2. The magnetic quantum number (ml) can be any integer between -l and +l. For l = 2, m can be either -2, -1, 0, +1, +2.

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**Quantum numbers for the first four levels of orbitals in the hydrogen atom**

Orbital designation ml # of orbitals 1 1s 2 2s 2p -1, 0, 1 3 3s 3p 3d -2, -1, 0, 1, 2 5 4 4s 4p 4d 4f -3, -2, -1, 0, 1, 2, 3 7

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