![Noble Gas Configuration
Noble Gas Configuration
The Noble Gases are:
The Noble Gases are:
He, Ne, Ar, Kr, Xe, Rn
He, Ne, Ar, Kr, Xe, Rn
Notice that each noble gas finishes a row,
Notice that each noble gas finishes a row,
or energy level.
or energy level.
Noble gas configurations take advantage
Noble gas configurations take advantage
of this by condensing what you have to
of this by condensing what you have to
write:
write:
Ex.
Ex. He :
He : 1s
1s2
2
Ex.
Ex. C :
C : 1s
1s2
2
2s
2s2
2
2p2
2p2
Noble Gas Configuration for C:
Noble Gas Configuration for C: [He]
[He] 2s
2s2
2
2p2
2p2](https://image.slidesharecdn.com/electronconfigurationsreview-250123002250-2fea4f80/85/Electron-Configurations-review-practice-ppt-10-320.jpg)
![Noble Gas Config. – an example
Noble Gas Config. – an example
The normal configuration for As-(Arsenic)
The normal configuration for As-(Arsenic)
1s
1s2
2
2s
2s2
2
2p
2p6
6
3s
3s2
2
3p
3p6
6
4s
4s2
2
3d
3d10
10
4p
4p3
3
Notice, the part in yellow is the same as
Notice, the part in yellow is the same as
Argon’s configuration:
Argon’s configuration: 1s
1s2
2
2s
2s2
2
2p
2p6
6
3s
3s2
2
3p
3p6
6
The noble gas configuration will start with
The noble gas configuration will start with
the gas in the row before it.
the gas in the row before it.
[Ar]
[Ar] 4s
4s2
2
3d
3d10
10
4p
4p3
3
It cuts down on a lot of writing, and that’s a
It cuts down on a lot of writing, and that’s a
good thing.
good thing.](https://image.slidesharecdn.com/electronconfigurationsreview-250123002250-2fea4f80/85/Electron-Configurations-review-practice-ppt-11-320.jpg)
Electron Configurations review practice.ppt
- 2. s, p, d, and f s, p, d, and f The different sections of the Periodic The different sections of the Periodic Table are very important in understanding Table are very important in understanding Electron Configuration. Electron Configuration. There are 4 “Blocks” in the Periodic Table: There are 4 “Blocks” in the Periodic Table: the s-block, p-block, d-block, & f-block. the s-block, p-block, d-block, & f-block. Remember the special rules for the d- and Remember the special rules for the d- and f- blocks: f- blocks: d – n-1 d – n-1 f – n - 2 f – n - 2
- 3. What do s, p, d, and f mean? What do s, p, d, and f mean? These refer to the These refer to the sublevels sublevels within the within the principal quantum level (n). principal quantum level (n). So, for n = 1, there is only one sublevel, s. So, for n = 1, there is only one sublevel, s. n = 2, there are 2 sublevels: s & p n = 2, there are 2 sublevels: s & p n = 3, there are 3 sublevels: s, p, & d n = 3, there are 3 sublevels: s, p, & d So, within each level, there are n So, within each level, there are n sublevels. sublevels.
- 4. This shows the different blocks in the Periodic Table. This shows the different blocks in the Periodic Table. It also shows in what order to write electron configurations It also shows in what order to write electron configurations (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d,7p) 5f, 6d,7p) Block Table Block Table
- 5. An Example An Example As - Arsenic As - Arsenic 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s2 2 3d 3d10 10 4p 4p3 3 The first number is which row it’s in, or the The first number is which row it’s in, or the principal quantum number (energy level) principal quantum number (energy level) The character is the block its in, which The character is the block its in, which refers to the refers to the sublevel sublevel The superscript is the total number of The superscript is the total number of electrons in the electrons in the sublevel sublevel
- 6. A shortcut! A shortcut! 1s 1s 2s 2p 2s 2p 3s 3p 3d 3s 3p 3d 4s 4p 4d 4f 4s 4p 4d 4f 5s 5p 5d 5f 5s 5p 5d 5f 5g 5g 6s 6p 6d 6s 6p 6d 6f 6f 6g 6g 6h 6h 7s 7p 7s 7p 7d 7d 7f 7f 7g 7g 7h 7h 7i 7i Do not exist in normal ground state atoms
- 7. d d4 4 and d and d9 9 rules rules Sometimes an electron configuration will end Sometimes an electron configuration will end with 4 or 9 electrons in the d-sublevel; these with 4 or 9 electrons in the d-sublevel; these are unstable are unstable Will steal electrons from the s-sublevel before Will steal electrons from the s-sublevel before it to stabilize. Ex. Chromium: it to stabilize. Ex. Chromium: 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s2 2 3d 3d4 4 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s1 1 3d 3d5 5
- 8. d d4 4 and d and d9 9 rules rules Ex. 2; Silver Ex. 2; Silver 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s2 2 3d 3d4 4 4p 4p6 6 5s 5s2 2 4d 4d9 9 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s2 2 3d 3d4 4 4p 4p6 6 5s 5s1 1 4d 4d10 10
- 9. The Noble Gas The Noble Gas Configuration Configuration An obvious solution and An obvious solution and convenient short cut! convenient short cut!
- 10. Noble Gas Configuration Noble Gas Configuration The Noble Gases are: The Noble Gases are: He, Ne, Ar, Kr, Xe, Rn He, Ne, Ar, Kr, Xe, Rn Notice that each noble gas finishes a row, Notice that each noble gas finishes a row, or energy level. or energy level. Noble gas configurations take advantage Noble gas configurations take advantage of this by condensing what you have to of this by condensing what you have to write: write: Ex. Ex. He : He : 1s 1s2 2 Ex. Ex. C : C : 1s 1s2 2 2s 2s2 2 2p2 2p2 Noble Gas Configuration for C: Noble Gas Configuration for C: [He] [He] 2s 2s2 2 2p2 2p2
- 11. Noble Gas Config. – an example Noble Gas Config. – an example The normal configuration for As-(Arsenic) The normal configuration for As-(Arsenic) 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 4s 4s2 2 3d 3d10 10 4p 4p3 3 Notice, the part in yellow is the same as Notice, the part in yellow is the same as Argon’s configuration: Argon’s configuration: 1s 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 The noble gas configuration will start with The noble gas configuration will start with the gas in the row before it. the gas in the row before it. [Ar] [Ar] 4s 4s2 2 3d 3d10 10 4p 4p3 3 It cuts down on a lot of writing, and that’s a It cuts down on a lot of writing, and that’s a good thing. good thing.
- 12. Orbital Diagrams Orbital Diagrams They’re Useful! They’re Useful!
- 13. Orbitals Orbitals Orbitals Orbitals Each sublevel (s, p, d, f) contains orbitals. Each sublevel (s, p, d, f) contains orbitals. Remember, orbitals are electron-clouds that Remember, orbitals are electron-clouds that hold the electrons 90% of the time. hold the electrons 90% of the time. Each orbital can hold TWO electrons, so Each orbital can hold TWO electrons, so s - 2 electrons, 1 orbital s - 2 electrons, 1 orbital p – 6 electrons, 3 orbitals p – 6 electrons, 3 orbitals d – 10 electrons, 5 orbitals d – 10 electrons, 5 orbitals f – 14 electrons, 7 orbitals f – 14 electrons, 7 orbitals
- 14. The Aufbau Principle The Aufbau Principle Each electron occupies Each electron occupies the lowest energy the lowest energy orbital orbital Electrons are Lazy!!! Electrons are Lazy!!! All orbitals related to an All orbitals related to an energy level are of energy level are of equal energy. equal energy. Ex. The three 2p orbitals Ex. The three 2p orbitals are the same energy are the same energy level. level. All equivalent energy
- 15. Pauli Exclusion Principle Pauli Exclusion Principle A maximum of two A maximum of two electrons may occupy a electrons may occupy a single orbital, but single orbital, but only if the only if the electrons have opposite electrons have opposite spins. spins. Spin -- Electrons has an Spin -- Electrons has an associated “spin,” either one associated “spin,” either one way or the other, like a top. way or the other, like a top. These spins are called “spin These spins are called “spin up” and “spin down.” up” and “spin down.” See example on board. See example on board. Box = orbital Arrow = electron
- 16. Hund’s Rule Hund’s Rule Single electrons with Single electrons with the the same same spin must spin must occupy each equal- occupy each equal- energy orbital energy orbital before before additional electrons with additional electrons with opposite spins can opposite spins can occupy the occupy the same same orbitals. orbitals. Electrons are Electrons are UNFRIENDLY UNFRIENDLY Why? Why? 1s2 2s2 2p3 1s2 2s2 2p3 NOT Ex. Nitrogen: •1s2 2s2 2p3
- 17. The order of Things… The order of Things… Electrons, being Electrons, being unfriendly, fill up the unfriendly, fill up the empty orbitals before empty orbitals before sharing orbitals. sharing orbitals. Similar to seats on a Similar to seats on a bus – on a bus, you sit bus – on a bus, you sit alone, rather than with a alone, rather than with a stranger, if there is an stranger, if there is an option. option.
- 18. The Shapes of the s, p, and d Orbitals The Shapes of the s, p, and d Orbitals Sketch these at bottom of outline Sketch these at bottom of outline
- 19. F-Orbitals! F-Orbitals! Do not bother sketching these—just notice Do not bother sketching these—just notice how STRANGE they are! how STRANGE they are! If you want to see more, go to: http://www.orbitals.com/orb/orbtable.htm
- 20. Please write this at the bottom of your outline Please write this at the bottom of your outline Orbital Shape No. per sublevel s Spherical 1 p Figure-8, dumbbells 3 d Double figure-8s & drops with coffee 5 f Don’t worry! 7
- 21. e e- - Config. and Orb. Diag. for Ions Config. and Orb. Diag. for Ions What is an ion? What is an ion? Examples of ions: Examples of ions: Na Na+ + Mg Mg2+ 2+ Fe Fe3+ 3+ Cl Cl- - S S2- 2- When writing electron When writing electron configurations or orbital configurations or orbital diagrams for ions it’s a diagrams for ions it’s a little harder because it little harder because it can look like a can look like a different different atom. atom. Just subtract the missing Just subtract the missing electrons or add the extra electrons or add the extra electrons (highest energy electrons (highest energy level) level) Li+ (1s2 2s0 ) He (1s2 )
- 22. Example Configs Example Configs Na Na+ + : 1s : 1s2 2 2s 2s2 2 2p 2p6 6 Mg Mg2+ 2+ : 1s : 1s2 2 2s 2s2 2 2p 2p6 6 Fe Fe3+ 3+ : 1s : 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 3d 3d5 5 Cl Cl- - : 1s : 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6 S S2- 2- : 1s : 1s2 2 2s 2s2 2 2p 2p6 6 3s 3s2 2 3p 3p6 6