Objectives: Learn how to show Electron configuration using:
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1 4 WAYS to SHOW the Electron Configuration(Electron arrangement) Objectives: Learn how to show Electron configuration using: 1. Using Aufbau Energy Diagrams 2. Orbital Diagrams 3. Long hand Electron configuration 4. Short-hand Electron configuration
2 Filling Rules for Electron Orbitals Aufbau Principle: Electrons occupy the positions of the lowest energy until all the electrons of the atom have been accounted for. Pauli Exclusion Principle: An orbital can hold a maximum of two electrons. that must spin in opposite directions. Hund s Rule: Electrons in the same sublevel occupy empty orbitals rather than pair up *Aufbau is German for building up
3 Periodic Patterns s 2s 3s 4s 5s 6s 7s d (n-1) 3d 4d 5d 6d p 2p 3p 4p 5p 6p 7p f (n-2) 6 7 5f 4f
4 Order in which subshells are filled with electrons (AUFBAU) 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s s 2p 3s 3p 4s 3d 4p 5s 4d
5 Energy Energy Sublevels 6d 5f 7s 6p 5d 4f 6s 5p 4d 5s 4p 3d 4s 3p 3s 2p 2s 7s 6s 5s 4s 3s 2s 6p 5p 4p 3p 2p 6d 5d 4d 3d 5f 4f n = 4 n = 3 n = 2 4f 4d 4p 3d 4s 3p 3s 2p 2s n = 1
6 Energy Sublevels s p d f s p d s p s n = 4 n = 3 4f 4d 4p 3d 4s 3p 3s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 n = 2 2p 2s n = 1
7 Aufbau Energy Level Diagram of an Atom 6s 6p 5d 4f 32 5s 5p 4d 18 4s 4p 3d Arbitrary Energy Scale 3s 3p s 2p 8 2 O Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177 NUCLEUS
8 Electron capacities Copyright 2006 Pearson Benjamin Cummings. All rights reserved.
9 Copyright 2007 Pearson Benjamin Cummings. All rights reserved
10 Energy General Rules Aufbau Principle Electrons fill the lowest energy orbitals first. Lazy Tenant Rule 6d 5f 7s 6p 5d 4f 6s 5p 4d 5s 4p 3d 4s 3p 3s 2p 2s 7s 6s 5s 4s 3s 6p 5p 4p 3p 2p 6d 5d 4d 3d 5f 4f 2s Courtesy Christy Johannesson
11 Order in which subshells are filled with electrons (AUFBAU) 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s s 2p 3s 3p 4s 3d 4p 5s 4d
12 LET s WATCH this SIMPLE VIDEO on how to use the AUFBAU diagram To WRITE ELECTRON configurations VIDEO LINK LET S DO IT! If you believe you haven t understood Anything so far here is a simple video. However, the electron config is WRONG For Lithium when she shows you. It is Li 2 2s 1
13 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p Electron Configuration NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS
14 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Hydrogen 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration H = 1
15 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Helium 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration He = 2
16 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Lithium 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration Li = 2 2s 1
17 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Carbon 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration C = 2 2s 2 2p 2
18 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Nitrogen 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p Hund s Rule maximum number of unpaired orbitals. NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration N = 2 2s 2 2p 3
19 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Fluorine 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration F = 2 2s 2 2p 5
20 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Aluminum 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration Al = 2 2s 2 2p 6 3s 2 3p 1
21 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Argon 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration Ar = 2 2s 2 2p 6 3s 2 3p 6
22 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Iron 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration Fe = 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6
23 Arbitrary Energy Scale Energy Level Diagram 6s 6p 5d 4f Lanthanum 5s 5p 4d Bohr Model 4s 4p 3d 3s 3p N 2s 2p NUCLEUS H He Li C N Al Ar F Fe La CLICK ON ELEMENT TO FILL IN CHARTS Electron Configuration La = 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 5d 1
24 Electron Configurations Orbital Filling Electron Element 2s 2p x 2p y 2p z 3s Configuration H He Li C N O F Ne Na 1 2 NOT CORRECT Violates Hund s Rule 2 2s 1 2 2s 2 2p 2 2 2s 2 2p 3 2 2s 2 2p 4 2 2s 2 2p 5 2 2s 2 2p 6 2 2s 2 2p 6 3s 1
25 Electron Configurations Orbital Filling Electron Element 2s 2p x 2p y 2p z 3s Configuration H He Li C N O F Ne Na s 1 2 2s 2 2p 2 2 2s 2 2p 3 2 2s 2 2p 4 2 2s 2 2p 5 2 2s 2 2p 6 2 2s 2 2p 6 3s 1
26 Shorthand Configuration A neon's electron configuration ( 2 2s 2 2p 6 ) [Ne] 3s 1 B C third energy level one electron in the s orbital D orbital shape Na = [ 2 2s 2 2p 6 ] 3s 1 electron configuration
27 Shorthand Configuration Element symbol Ca V F Ag I Xe Electron configuration [Ar] 4s 2 [Ar] 4s 2 3d 3 [He] 2s 2 2p 5 [Kr] 5s 2 4d 9 [Kr] 5s 2 4d 10 5p 5 [Kr] 5s 2 4d 10 5p 6 Fe [He] 2s[Ar] 2 2p 6 4s 3s 3d 3p 4s 2 3d 6 Sg [Rn] 7s 2 5f 14 6d 4
28 General Rules Pauli Exclusion Principle Each orbital can hold TWO electrons with opposite spins. Wolfgang Pauli Courtesy Christy Johannesson
29 General Rules Hund s Rule Within a sublevel, place one electron per orbital before pairing them. Empty Bus Seat Rule WRONG RIGHT Courtesy Christy Johannesson
30 Notation 8 O Orbital Diagram O 8e - 2s 2p Electron Configuration 2 2s 2 2p 4 Courtesy Christy Johannesson
31 Notation 16 S Longhand Configuration S 16e - 2 2s 2 2p 6 3s 2 3p 4 Core Electrons Valence Electrons Shorthand Configuration S 16e - [Ne] 3s 2 3p 4 Courtesy Christy Johannesson
32 Periodic Patterns s 2s 3s 4s 5s 6s 7s d (n-1) 3d 4d 5d 6d p 2p 3p 4p 5p 6p 7p f (n-2) 6 7 5f 4f
33 Periodic Patterns Period # energy level (subtract for d & f) A/B Group # total # of valence e - Column within sublevel block # of e - in sublevel Courtesy Christy Johannesson
34 Periodic Patterns Example - Hydrogen st column of s-block t Period s-block Courtesy Christy Johannesson
35 Periodic Patterns Shorthand Configuration Core electrons: Go up one row and over to the Noble Gas. Valence electrons: On the next row, fill in the # of e - in each sublevel Courtesy Christy Johannesson
36 Periodic Patterns 32 Ge Example - Germanium [Ar] 4s 2 3d 10 4p 2 Courtesy Christy Johannesson
37 Stability Full energy level Full sublevel (s, p, d, f) Half-full sublevel Courtesy Christy Johannesson
38 The Octet Rule Atoms tend to gain, lose, or share electrons until they have eight valence electrons. This fills the valence shell and tends to give the atom the stability of the inert gasses. 8 ONLY s- and p-orbitals are valence electrons.
39 THIS SLIDE IS ANIMATED IN FILLING ORDER 2.PPT H = 1 He = 2 Li = 2 2s 1 2s Be = 2 2s 2 2s C = 2 2s 2 2p 2 2s 2px 2py 2pz S = 2 2s 2 2p 4 2s 2px 2py 2pz 3s 3px 3py 3pz
40 Fe = 1 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Iron has 26 electrons. 2s 2p x 2p y 2p z 3s 3p x 3p y 3p z 4s 3d 3d 3d 3d 3d 6s 6p 5d 4f 32 5s 5p 4d e- e- e - e - e - e- e - e - e - e - e - e e - e - e - e e - e - - e - e - e - e - e - e e - e- - Arbitrary Energy Scale 4s 4p 3d 3s 3p 2s 2p NUCLEUS
41 Energy Level Diagram of a Many-Electron Atom 6s 6p 5d 4f 32 5s 5p 4d 18 4s 4p 3d Arbitrary Energy Scale 3s 3p s 2p 8 2 O Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177 NUCLEUS
42 Maximum of Electrons In Each Sublevel Maximum Number of Electrons In Each Sublevel Maximum Number Sublevel Number of Orbitals of Electrons s 1 2 p 3 6 d 5 10 f 7 14 LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World, 1996, page 146
43 Stability Electron Configuration Exceptions Copper EXPECT: [Ar] 4s 2 3d 9 ACTUALLY: [Ar] 4s 1 3d 10 Copper gains stability with a full d-sublevel. Courtesy Christy Johannesson
![Stability Electron Configuration Exceptions Chromium EXPECT: [Ar] 4s 2 3d 4 ACTUALLY: [Ar] 4s 1 3d 5 Chromium](/docs-images/93/111845383/images/44-1.jpg "gains stability with a half-full d-sublevel. Courtesy Christy Johannesson www.nisd.")
44 Stability Electron Configuration Exceptions Chromium EXPECT: [Ar] 4s 2 3d 4 ACTUALLY: [Ar] 4s 1 3d 5 Chromium gains stability with a half-full d-sublevel. Courtesy Christy Johannesson
45 Energy Electron Filling in Periodic Table s s 1 p 2 3 d 4 K 4s 1 Ca 4s 2 Sc 3d 1 Ti 3d 2 V 3d 3 Cr 3d 45 Mn 3d 5 Fe 3d 6 Co 3d 7 Ni 3d 8 Cu 3d 9 3d 10 Zn 3d 10 Ga 4p 1 Ge 4p 2 As 4p 3 Se 4p 4 Br 4p 5 Kr 4p 6 n = 4 n = 3 n = 2 n = 1 4f 4d 4p 3d 4s 3p 3s 2p 2s Cr 4s 1 3d 5 4s Cu 4s 1 3d 10 3d Cr 4s 1 3d 5 Cu 4s 1 3d 10 4s 3d
46 Stability Ion Formation Atoms gain or lose electrons to become more stable. Isoelectronic with the Noble Gases Courtesy Christy Johannesson
47 Stability Ion Electron Configuration Write the e - configuration for the closest Noble Gas EX: Oxygen ion O 2- Ne O 2-10e - [He] 2s 2 2p 6 Courtesy Christy Johannesson
48 Orbital Diagrams for Nickel 28 Ni s 2p 3s 3p 4s 3d Excited State 2s 2p 3s 3p 4s 3d Pauli Exclusion 2s 2p 3s 3p 4s 3d Hund s Rule 2s 2p 3s 3p 4s 3d
49 Orbital Diagrams for Nickel 28 Ni s 2p 3s 3p 4s 3d Excited State s 2p 3s 3p 4s 3d VIOLATES Pauli Exclusion 2s 2p 3s 3p 4s 3d VIOLATES Hund s Rule 2s 2p 3s 3p 4s 3d
50 Write out the complete electron configuration for the following: 1) An atom of nitrogen 2) An atom of silver 3) An atom of uranium POP (shorthand) Fill in the orbital boxes for an atom of nickel (Ni) QUIZ 2s 2p 3s 3p 4s 3d Which rule states no two electrons can spin the same direction in a single orbital? Extra credit: Draw a Bohr model of a Ti 4+ cation. Ti 4+ is isoelectronic to Argon.
51 Answer Key Write out the complete electron configuration for the following: 1) An atom of nitrogen 2 2s 2 2p 3 2) An atom of silver 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 9 3) An atom of uranium (shorthand) [Rn]7s 2 6d 1 5f 3 Fill in the orbital boxes for an atom of nickel (Ni) 2s 2p 3s 3p 4s 3d Which rule states no two electrons can spin the same direction in a single orbital? Pauli exclusion principle Extra credit: Draw a Bohr model of a Ti 4+ cation. n = 22+ n Ti 4+ is isoelectronic to Argon.
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