Warmup P-HN-H F-H a. Use your EN chart to calculate the EN differences of the bonds shown above b....
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Transcript of Warmup P-HN-H F-H a. Use your EN chart to calculate the EN differences of the bonds shown above b....
![Page 1: Warmup P-HN-H F-H a. Use your EN chart to calculate the EN differences of the bonds shown above b. Rank the bonds in order of decreasing polarity (most.](https://reader035.fdocuments.in/reader035/viewer/2022070411/56649f575503460f94c7bcbd/html5/thumbnails/1.jpg)
WarmupP-H N-H F-H
a. Use your EN chart to calculate the EN differences of the bonds shown above
b. Rank the bonds in order of decreasing polarity (most polar to least polar):
c. Draw the distribution of the electron cloud around each bond and the dipoles
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Lewis Structures*refer to handout on the back of the
Molecular Modeling Activity
https://www.youtube.com/watch?v=NgD9yHSJ29I
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Bonding (Shared) Pair
Bonding (Shared) Pair
Lone (Unshared) Pair
Lone (Unshared)
Pair
Atoms in a covalent bond share valence e- to achieve completely satisfied valence shells.Lewis structures are drawings that show HOW
atoms are covalently bonded.
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Ex. Draw the Lewis Structure for ICl
Hmmmmm how many val e- does iodine have?
What about chlorine?
I
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I Cl
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ClI
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I Cl
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I Cl
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I Cl
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I Cl
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I Cl
*They each share 1 e- with each other
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How many val e- does each atom have?
I Cl 8 Valence electrons
8 Valence electrons
Both end with “full octets”. All elements MUST end up with a full octet (few exceptions)
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C =(4 e-)(1 atom) = 4(1 e-)(2 atoms) = 2
H =
12 valence e-
Ex. Draw the Lewis Structure for H2CO1) Calculate total # of valence e-
O = (6 e-)(1 atom) = 6
What about harder structures? Let’s try like…..a method…
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2) Plan the molecular skeletonHints: C is often central, H and halogens are never central, O is rarely central
Draw the Lewis Structure for H2CO
3) Place 1 pair e- between each of the atoms
4&5) Add in e- to create double/triple bond or
lone pairs so that:
6) Check that each atom is surrounded by 8 valence e- and that total valance e- are all used
C OH
H
6 val e-
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7. Final structure: replace each bonding e- pairs with a line
H
HC = O
Clarification: the structural formula shows bonds as lines and the lone pairs aren’t ALWAYS included. A dot diagram represents bonding electrons pairs as dots. A Lewis structure can technically be either, we are not too particular.
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Simple Structures Practice
CH4
HF
H2
H2O
HF and H2O are polar
molecules (uneven
distribution of electrons)
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More Practice
CH3Br
NH3
SF6
BCl3
WEIRDNESS!!!!
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expanded octetSulfur usually makes 2 bonds but can
make up to 6 H
S
H
H2S
SF F
F F
F F
SF6
Phosphorus can also expand it’s octet. Nitrogen cannot.
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Incomplete Octet
BCl3 BeF2 B
Cl
Cl
Cl
Violation
Be FF
Violation
on
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More Practice OH-
Total e-
6 + 1 + 1
NH4+
Total e-
5 + 4 – 1
N2
10 e- total, but
double or
triple bond?
H O [ ]-1
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Some orbitals are full and don’t have to
overlap (lone pairs!)CCOO OO
A bond is not ACTUALLY 2 dots (or 4 or 6) in between two atoms!!!!!!!!!!!!!!!!!!!!
A bond is formed when one orbital (containing an electron) overlaps with an orbital from another atom. The electrons are shared and travel within the two orbitals….they are SHARED.
2e-
2e-
1e-
1e-1e-
1e-
1e-1e-
You will not need to draw
something like this!!!