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Quantum Numbers Activity

Quantum Numbers Activity. Quantum Numbers. Quantum numbers tell us properties of the atomic orbitals, and electrons, in an atom. Like giving each electron its own addres

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Quantum Numbers Activity

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  1. Quantum Numbers Activity

  2. Quantum Numbers • Quantum numbers tell us properties of the atomic orbitals, and electrons, in an atom. • Like giving each electron its own addres • An orbital is a 3-D region of an atom where there is a high probability of finding electrons (NOT an actual ring & NOT like the planetary orbitals)

  3. Principal Quantum Number Angular Momentum Quantum Number Magnetic Quantum Number Spin Quantum Number

  4. Textbook • You will need a textbook to look up information about the quantum numbers. Pg. 101.

  5. Know for each Quantum # • Definition • Symbol • The allowed values • An example • A visual representation of the quantum number

  6. Review Quantum Numbers as a Class Discussion of the 4 types of quantum numbers and there properties

  7. Quantum Number Review Notes

  8. Quantum Numbers • Used to describe various properties of the orbitals • Each electron is assigned a set of four quantum numbers which, in order, are n, l, ml, and ms • Like giving each electron its own address

  9. Principle quantum number • Definition: indicates the main energy level occupied by the electron • Symbol: n • Values: (written as integers) 1,2,3,4,5,6,7

  10. Angular Momentum Quantum Numbers • Definition: indicates the shape of the orbital • Symbol: l • Values: • 0 = s • 1 = p • 2 = d • 3 = f • For a specific energy level, the number of orbital shapes available is equal to n -1

  11. Magnetic Quantum Numbers • Definition: represents the orientation of an orbital around the nucleus • Symbol: ml • Values: for a p-orbital -1, 0 , 1

  12. Spin Quantum Numbers • Definition: represents the spin states of electrons in an orbital • Symbol: ms • Values: +1/2, - ½

  13. Can an e- be described by the following set of quantum numbers? n=2, l=1, ml= -1 All quantum numbers are allowed values

  14. Can an e- be described by the following set of quantum numbers? n=1, l=1, ml= +1 Not possible. The value of l must be less than the value of n.

  15. Can an e- be described by the following set of quantum numbers? n=7, l=3, ml= +3 All the quantum numbers are allowed values.

  16. Can an e- be described by the following set of quantum numbers? n=3, l=1, ml=-3 Not possible. The value of ml must be in the range -l to +l

  17. Replace the ? Mark with an appropriate quantum number. n=3, l=1, ml=? n=4, l=?, ml=-2 n=?, l=3, ml=?

  18. Can an e- be described by the following set of quantum numbers? n=2, l=1, ml=-2 n=3, l=2, ml=+2 n=4, l=3, ml=+3 n=5, l=2, ml=+3

  19. Writing Quantum Numbers • You can identify the quantum numbers for any electron in an element • Start by writing out the the electron configuration and orbital diagram for the element • Locate the electron in the orbital diagram that you are solving the quantum number for • Determine the 4 quantum numbers

  20. Hydrogen’s electron • Write electron configuration • Draw orbital diagram • n= 1 • l= 0 • ml= 0 • ms= +1/2

  21. Helium’s second electron • Write electron configuration • Draw orbital diagram • n= 1 • l= 0 • ml= 0 • ms= -1/2

  22. Lithium’s third electron • Write electron configuration • Draw orbital diagram • n= 2 • l= 0 • ml= 0 • ms= +1/2

  23. Flourine’s 6th electron • Write electron configuration • Draw orbital diagram • n= 2 • l= 1 • ml= 0 • ms= +1/2

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