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Quantum Mechanical Model Notes

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1 Quantum Mechanical Model Notes
Electrons DO NOT travel around the nucleus of an atom in orbits like planets around a sun. Orbitals are 3-D areas around the nucleus with a high probability of finding electrons.

2 The higher the density of dots indicates the higher (most) probable location(s) of electron(s).
Boundary line = 90% probability of finding electrons within the circular region.

3 Principle Quantum #1 (n):
Each electron in an electron cloud has a four-part quantum number. This is like a street address. Principle Quantum #1 (n): Indicates the relative size and energy of orbitals. It is designated with numbers, 1-7). Electrons are found at different distances away from the nucleus in different energy levels.

4 Electrons cannot exist between energy levels (they are like the rungs of a ladder).
Only a certain number of electrons may exist in a given energy level, but the number varies. It can be determined by a formula: Total number of electrons in level = 2 x (# of energy level )2

5 Energy levels are broken up into sublevels:
For Example: Energy level 1 = 2 (1)2 = 2 Energy level 2 = 2 (2)2 = 8 Solve for the energy levels below using the equation (2 x (# of energy level)2 Energy level 3 = Energy level 4 = Energy levels are broken up into sublevels:

6 Principle Quantum #2 (s; p; d; f; etc
Principle Quantum #2 (s; p; d; f; etc.): Are called energy sublevels and have specific orbital shapes. Table Team — what is the relationship between n and sublevels?

7 Principle Quantum Number 4:
Prinicple Quantum Number 3: Designates the orientation of orbitals in the electron cloud. Principle Quantum Number 4: Designates the ‘spin’ of an electron (either clock-wise or counter clock wise), allowing two electrons to occupy the same orbital. Each electron has a unique set of four quantum numbers.

8 Principle Energy Level 1:
Only has one s sublevel (a spherical shape; see model). A sphere has only one orientation in the space of the electron cloud. Two electrons may fit in this sublevel—each one has an opposite spin. Pauli exclusion principle —no more than two electrons may be found in the same orbital.

9 An ‘s’ Orbital

10 Has two energy sublevels: s and p. There are 2 electrons in a ‘s’
Principle Energy Level 2: Has two energy sublevels: s and p. There are 2 electrons in a ‘s’ There are 3 different p orbitals, each can hold 2 electrons for 6 total. (‘dumb-bell’ shape; three orientations in electron cloud space). There can be a total of 8 electrons overall in energy level 2.

11 ‘p’ Orbitals

12 Principle Energy Level 3:
has 3 sublevels: s, p, and d. Two electrons in the s orbital Six total electrons in the three p orbitals. There are 5 different d orbitals, and 2 electrons can fit in each—for a total of 10. Total of 18 electrons for energy level 3.

13 The five ‘d’ Orbital Images
d-orbital notes

14 Principle Energy Level 4:
Has 4 sublevels: s, p, d , and f. 2 electrons in s 6 electrons in p 10 electrons in d 14 electrons in f (7 different orbitals for f) A total of 32 electrons in this energy level.

15 Seven ‘f’ orbitals

16 The order that electrons fill up orbitals does not follow the logical order of all 1’s, then all 2’s, then all 3’s, etc.

17 The first rule states that each electron occupies the lowest energy level possible. This is called the Aufbau principle. The second rule for filling orbitals is that only one electron will be put in each orbital of a sublevel until all of them are filled, and after that, they may be paired up until the sublevel is full. This is called Hund’s rule.

18 An easy way to remember this is to use the periodic table--it is arranged to show how these orbitals are filled. Stay tuned!

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