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Published byLexie Devereaux Modified over 3 years ago

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Quantum Numbers Schrödinger’s equation requires 3 quantum numbers (although there are a total of 4 quantum numbers)

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**Quantum Numbers Principal Quantum Number, n.**

This number is related to the size and energy of the orbital.

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**Quantum Numbers Principal Quantum Number, n, cont.**

This is the same as Bohr’s n. As n becomes larger, the atom becomes larger and the electron is further from the nucleus. An increase in n also means higher energy.

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**Quantum Numbers Azimuthal or Angular Momentum Quantum Number, l.**

This number is related to the shape of the atomic orbitals.

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**Quantum Numbers Azimuthal or Angular Momentum Quantum Number, l, cont.**

This quantum number depends on the value of n. The values of l begin at 0 and increase to (n - 1).

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**Quantum Numbers Azimuthal Quantum Number, l, cont.**

Usually we refer to the s, p, d and f orbitals. orbital l = s p 1 d 2 f 3

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**Quantum Numbers Magnetic Quantum Number, ml.**

This quantum number is related to the orientation of the orbital in space relative to other orbitals in the atom.

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**Quantum Numbers Magnetic Quantum Number, ml.**

This quantum number depends on l. The magnetic quantum number has integral values between -l and +l.

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**Quantum Numbers Magnetic Quantum Number, ml, cont. orbital ml = s p**

p 1, 0, -1 d 2, 1, 0, -1, -2 f 3, 2, 1, 0, -1, -2, -3

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**Quantum Numbers Spin Quantum Number, ms.**

This quantum number relates to the spin of an electron and can take on two possible values: ms = +½ or ms = -½.

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Quantum Numbers Note electrons don’t actually spin, but the magnetic properties of electrons are just what we would see if the electron were a spinning charged particle, and it is useful to picture the electron as spinning.

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Quantum Numbers Orbitals and Quantum Numbers

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 4s orbital. For the s orbital, l = 0 This is the energy level number (n)

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 4s orbital. If the 2nd quantum number is 0, the 3rd quantum number must also be zero.

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 4s orbital. The spin can either be +½ or -½.

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 4s orbital. ANSWER POSSIBILITIES: (4, 0, 0, +½) or (4, 0, 0, -½)

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 3p orbital. For the p orbital, l = 1 This is the energy level number (n)

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 3p orbital. If the 2nd quantum number is 1, the 3rd quantum number may be either 1, 0 or -1.

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 3p orbital. The spin can either be +½ or -½.

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**Quantum Numbers Application of Quantum Numbers**

Write a set of quantum numbers for the electron in a 3p orbital. ANSWER POSSIBILITIES: (3, 1, 1, +½), (3, 1, 1, -½), (3, 1, 0, +½), (3, 1, 0, -½), (3, 1, -1, +½), (3, 1, -1, -½),

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4.2b Quantum Numbers and Atomic Orbitals. POINT > Describe the Principle Quantum number as an energy level POINT > Calculate number of electrons at different.

4.2b Quantum Numbers and Atomic Orbitals. POINT > Describe the Principle Quantum number as an energy level POINT > Calculate number of electrons at different.

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