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2.06 Electron Configuration Parts I and II. Part I: Bohr Model of the Atom How are electrons arranged in an atom? Bohr: Electrons in definite energy levels.

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Presentation on theme: "2.06 Electron Configuration Parts I and II. Part I: Bohr Model of the Atom How are electrons arranged in an atom? Bohr: Electrons in definite energy levels."— Presentation transcript:

1 2.06 Electron Configuration Parts I and II

2 Part I: Bohr Model of the Atom How are electrons arranged in an atom? Bohr: Electrons in definite energy levels around the nucleus Explained Hydrogen but not comprehensive enough for other elements

3 Modern Theory for Electrons Modern Theory (also called the Quantum Mechanical Model or Electron Cloud Model): Electrons move in a “beehive” around the nucleus in a “cloud” of energy An _________ is a region of space where an electron is likely to be found

4 Shapes Different types of orbitals have sublevel shapes depending on how much energy there is: –s ___________ –p ___________ –d ___________ –f ____________

5 Definitions Aufbau Principle--- electrons arrange to have the lowest energy so they fill from _______ energy to ________ energy Pauli Exclusion Principle---maximum of _______ electrons are in each orbital and they have ________ spins (shown by an up and down arrow in the orbital) Hund’s Rule---Fill ______ electron in each orbital all the way across then then go back to fill the second electrons if the electrons are available (think of filling a bus with one person in a seat first)

6 Orbitals Each orbital is shown as a box can hold a maximum of 2 electrons (one electron is represented with an “up” arrow and the other electron is represented with a “down” arrow) s has 1 orbital = _____ electrons p has 3 orbitals = _____ electrons d has 5 orbitals = _____ electrons f has 7 orbitals = ___electrons

7 Periodic Table

8 Using the Periodic Table

9 Order of electrons filling the orbitals

10 Electron Diagram Example

11 Definitions Electron configuration is the written summary of the arrangement of _______ in an atom 1s 2 2s 2 2p 6 3s 2 3p 3 Noble gas configuration is the short cut that saves you time (yeah!) but you have to know all three. Go to the noble gas in the row ________ your element. [Ne] 3s 2 3p 3

12 Carbon Example

13 Valence Electrons

14 Part II: Titanium Example (review)

15 F orbitals

16 Exceptions Chromium (Cr) and Copper (Cu) Rule: Filled and ½ filled sublevels are stable For these exceptions, one electron is “promoted” to make the other sublevel more stable

17 Chromium Example (Exception)


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