Presentation is loading. Please wait.

Presentation is loading. Please wait.

Recall: Werner Heisenberg formulated the Uncertanity Principle that states it is impossible for us to know an electrons exact position (where it is) and.

Similar presentations


Presentation on theme: "Recall: Werner Heisenberg formulated the Uncertanity Principle that states it is impossible for us to know an electrons exact position (where it is) and."— Presentation transcript:

1 Recall: Werner Heisenberg formulated the Uncertanity Principle that states it is impossible for us to know an electrons exact position (where it is) and momentum (where it is going) As a result, we cannot identify specific orbits that electrons travel in We can only identify regions of space within an atom where an electron is most likely to be found ORBITALS! Schrodingers complex math equation allows us to: Calculate the shape of the electron cloud Probability of finding the electron at distinct locations within those clouds

2 An Introduction to Electron Configurations

3 Complete the activity Welcome to Atomos Apartments! on page 208

4 We use electron configurations The way electrons are arranged in atoms There are rules to follow! Aufbau principle Electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for aufbau German for build up or construct

5 1s 3s 2s2p 3d3p 4s4p4d4f 5s5p5d5f

6 Paulis Exclusion Principle An orbital can hold only two electrons

7 Hunds Rule Electrons must fill a sub-level such that each orbital has a spin up electron before they are paired with spin down electrons A bus analogy: If you enter a bus and dont know anyone on it, you will pick a seat that is completely empty rather than one that already has a person in it

8 Electrons fill in order from lowest to highest energy The Pauli exclusion principle holds. An orbital can hold only two electrons Two electrons in the same orbital must have opposite signs (spins) You must know how many electrons can be held by each orbital 2 for s 6 for p 10 for d 14 for f Hunds rule applies. The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons for a set of orbitals By convention, all unpaired electrons are represented as having parallel spins with the spin up

9 Just a thought… How do you determine the number of electrons in an element? Examples: Oxygen Magnesium Argon Scandium

10

11 Use the Noble Gas symbol to abbreviate or shorten the electron configuration Krypton Rubidium Zirconium

12 Use Quantum Numbers!

13 Each electron has a specific address in the space around a nucleus An electrons address is given as a set of four quantum numbers Each quantum number provides specific information on the electrons location

14 state town street house number

15 state (energy level) - quantum number n town (sub-level) - quantum number l street (orbital) - quantum number m l house number (electron spin) - quantum number m s

16 Same as Bohrs n Integral values: 1, 2, 3, …. Indicates probable distance from the nucleus Higher numbers = greater distance from nucleus Greater distance = less tightly bound = higher energy

17 Integral values from 0 to n - 1 for each principal quantum number n Indicates the shape of the atomic orbitals Table 7.1 Angular momentum quantum numbers and corresponding atomic orbital numbers Value of l01234 Letter used spdfg

18 Integral values from l to -l, including zero Relates to the orientation of the orbital in space relative to the other orbitals 3-D orientation of each orbital

19

20 An orbital can hold only two electrons, and they must have opposite spins Spin can have two values, +1/2 and -1/2 Pauli Exclusion Principle (Wolfgang Pauli) "In a given atom no two electrons can have the same set of four quantum numbers"

21

22 Complete the Closer on Page 206

23 Begin homework on page 209 – FRONT AND BACK!


Download ppt "Recall: Werner Heisenberg formulated the Uncertanity Principle that states it is impossible for us to know an electrons exact position (where it is) and."

Similar presentations


Ads by Google