iiiiiiiv ch. 8-9 – molecular formulas …and lewis structures ii. molecular compounds (p. 212-229,...
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I II III IV
Ch. 8-9 – Molecular Formulas …and Lewis Structures
II. Molecular Compounds(p. 212-229, 237-245, p. 268-286)
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A. Energy of Bond Formation
Potential Energy based on position of an object low PE =
high stability
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no interaction
attraction vs. repulsion
increased attraction
A. Energy of Bond Formation
Potential Energy Diagram
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balanced attraction & repulsion
increased repulsion
attraction vs. repulsion
A. Energy of Bond Formation
Potential Energy Diagram
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Bond Energy
A. Energy of Bond Formation
Bond Length
Bond Energy
Energy required to break a bond
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A. Energy of Bond Formation
Bond Energy Short bond = high bond energy
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B. Lewis Structures
Electron Dot Diagrams show valence e- as dots distribute dots like arrows
in an orbital diagram 4 sides = 1 s-orbital, 3 p-orbitals EX: oxygen
2s 2pO
X
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B. Lewis Structures
Octet Rule Most atoms form bonds in order to obtain 8 valence
e-
Full energy level stability ~ Noble Gases
Ne
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+ -
+
B. Lewis Structures
Nonpolar Covalent - no charges
Polar Covalent - partial charges
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C. Molecular Nomenclature
Prefix System (binary compounds)
1. Less e-neg atom comes first.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the second element to -ide.
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PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-
NUMBER123456789
10
C. Molecular Nomenclature
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CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride
C. Molecular Nomenclature
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arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10
C. Molecular Nomenclature
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N O F
Cl
Br
I
H
C. Molecular Nomenclature
There are Seven Diatomic Elements which do not exist as monoatomic elements like the others do
Br2 I2 N2 Cl2 H2 O2 F2
Memory Trick: “The Seven of 7 go to H eaven”