Gilbert Newton Lewis (surrounded by pairs of electrons) Hybrid orbitals, Lewis diagrams, the octet...
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![Page 1: Gilbert Newton Lewis (surrounded by pairs of electrons) Hybrid orbitals, Lewis diagrams, the octet rule.](https://reader034.fdocuments.in/reader034/viewer/2022052504/55147038550346b0158b4ff5/html5/thumbnails/1.jpg)
Gilbert Newton Lewis
(surrounded by pairs of
electrons)
Hybrid orbitals, Lewis diagrams, the octet rule
![Page 2: Gilbert Newton Lewis (surrounded by pairs of electrons) Hybrid orbitals, Lewis diagrams, the octet rule.](https://reader034.fdocuments.in/reader034/viewer/2022052504/55147038550346b0158b4ff5/html5/thumbnails/2.jpg)
ReviewReview• We can visualize a covalent bond as a
balance between attraction and repulsion• A second way to view the formation of a
bond is to consider orbital diagrams• Video (15 min - stop at HCl)• Now we can visualize atoms bonding
because of the lower energy achieved via the stability of filled valence shells
• The bottom line: atoms gain, lose, or share electrons to obtain noble gas electron configurations
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Video: filling subshellsVideo: filling subshells
![Page 4: Gilbert Newton Lewis (surrounded by pairs of electrons) Hybrid orbitals, Lewis diagrams, the octet rule.](https://reader034.fdocuments.in/reader034/viewer/2022052504/55147038550346b0158b4ff5/html5/thumbnails/4.jpg)
Video: filling subshellsVideo: filling subshells
•Draw orbital diagrams for F + F, H + O, Li + F
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Overlapping orbitalsOverlapping orbitals• Draw orbital diagrams for F + F, H + O, Li + F
1s 2s 2p
1s2s2p
1s 2s 2p
1s
1s
F2
H2O
1s 2s 1s2s2p
LiF is ionic (metal + non-metal)
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Hybrid orbitalsHybrid orbitals• Two overlapping orbitals form what is known
as a hybrid or molecular orbital• Just as in a s,p,d, or f orbital the electrons can
be anywhere in the orbital (even though the electron has started out in one atom, at times, it may be closer to the other nucleus)
• Each hybrid orbital has a specific shape (described in chapter 8)
• You do not need to know shapes• You need to know that hybrid orbitals exist
and that they are formed from overlapping orbitals
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Lewis diagramsLewis diagrams• Read Pg. 229. Draw Lewis dot diagrams for
Ne, Sb, Rb, F. How many variations of the Lewis diagram for P can be drawn?
Ne Sb Rb F
P P P P
• Lewis diagrams follow the octet rule: atoms when forming ions, or bonding to other atoms in compounds have 8 outer electrons
• Q - How can the octet rule be explained?• A - s (2 e–) and p (6 e–) orbitals are filled
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Cl– Na+ Cl–
Ionic bondingIonic bonding• Recall: Ionic bonding involves 3 steps:
1) loss of e-, 2) gain of e-, 3) +ve, -ve attract
Na Cl
e–1) 2)
3)
Na+
This can be represented via Lewis diagrams…• Read remainder of 7.2 (pg. 230)• Diagram the reaction between Li + Cl and Mg + O (PE 3)
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The octet rule (ionic compounds)The octet rule (ionic compounds)• Draw Li + Cl and Mg + O (PE 3, pg. 230)
Li Cl [ Cl ]–[Li]+
[ O ]2–[Mg]2+OMg
• Note also that the charge on an ion can be determined by the number of places removed from a noble gas (Ca, N, Al?)
• Ca2+, N3-, Al3+
• See pg. 230 for example of Ca + Cl
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Covalent bondingCovalent bonding• Covalent bonds can also be shown via Lewis
diagrams - E.g draw Lewis diagrams showing the combination of 1) H+Cl, 2) C+Cl, 3) H+O, 4) Mg+F, 5) N+H, 6) Do PE 4 (pg. 234)
HCl
H Cl
CCl4
C
Cl
Cl
Cl
Cl H2OH O H
MgF2 - Ionic
[ F ]2– [Mg]2+
NH3
H N H
H
• Note bonds can also be drawn with a dash to represent two electrons (read 234-5 upto 7.5)
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The octet rule (covalent compounds)The octet rule (covalent compounds)• (Read 7.4 up to PE4 (pg. 232 - 4). Do PE4.)• Read remainder of 7.4• Although the octet rule works for most
compounds, PCl5 and SF6 are examples of exceptions (see pg. 235 for structures)
• Also, it can be difficult to draw the correct bonds for atoms with multiple bonds
• Some clear rules have been established for drawing Lewis structures
• We will see that the rules dictate molecular structure, which dictates shape, which can influence chemical properties of a compoundFor more lessons, visit
www.chalkbored.com