iiiiiiiv ch. 8 - covalent bonding i. the covalent bond (p. 240 – 247)
TRANSCRIPT
![Page 1: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/1.jpg)
I II III IV
Ch. 8 - Covalent Bonding
I. The Covalent Bond(p. 240 – 247)
![Page 2: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/2.jpg)
A. Why Do Atoms Bond?
Gain stabilityLower potential energyAtoms that fulfill the octet rule are more
stable
balanced attraction & repulsion
increased repulsion
attraction vs. repulsion
![Page 3: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/3.jpg)
B. What is a covalent bond?
A chemical bond that results from the sharing of electrons
Molecule = two or more atoms
that are held together by
covalent bondsMajority of covalent bonds form between
nonmetals (CLOSE together on periodic table)
H2O
![Page 4: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/4.jpg)
Examples:
Which of the following are covalent compounds?
NaBr SiO2
CO2
AlCl3 CH4
![Page 5: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/5.jpg)
IONIC COVALENTBond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
e- are transferred from metal to nonmetal
high
yes (solution or liquid)
yes
e- are shared between two nonmetals
low
no
usually not
MeltingPoint
crystal lattice true molecules
Properties Table
Physical State solid liquid or gas
odorousForm electrolytes in
solution
![Page 6: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/6.jpg)
C. Covalent Bonding Formation
Diatomic molecule = molecule containing only two atoms
Some atoms exist this way because they are more stable than the individual atoms Cl2
![Page 7: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/7.jpg)
N O F
Cl
Br
I
H
D. Diatomic Elements
The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2
![Page 8: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/8.jpg)
E. 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
![Page 9: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/9.jpg)
E. Lewis Structures
Octet Rule Most atoms form bonds in order to obtain 8 valence
e-
Full energy level stability ~ Noble Gases
Ne
![Page 10: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/10.jpg)
E. Lewis Structures
Example Electron Dot Notations:
Ca
P
H
C
CaP
![Page 11: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/11.jpg)
E. Lewis Structures
Single Bonds When atoms share one pair of electrons The two shared electrons belong to both
atoms simultaneously Lewis Structure dots or a line symbolize a
single covalent bond (1 pair of shared e-)
H – H
![Page 12: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/12.jpg)
How would you draw the Lewis structure for fluorine?
Diatomic!
F – F
E. Lewis Structures
![Page 13: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/13.jpg)
E. Lewis Structures
Multiple Covalent Bonds When atoms share more
than one pair of electrons Have higher bond energies
and are shorter than single bonds
![Page 14: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/14.jpg)
E. Lewis Structures
Double Bonds Sharing two pairs of
electrons between two atoms
Draw Lewis Structures for 2 oxygen atoms
![Page 15: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/15.jpg)
E. Lewis Structures
Triple Bonds Sharing three pairs of
electrons between two atoms
Draw Lewis Structures for 2 nitrogen atoms
![Page 16: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/16.jpg)
I II III IV
Naming Molecules
Section 8.2
![Page 17: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/17.jpg)
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.
![Page 18: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/18.jpg)
PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-
NUMBER12345678910
C. Molecular Nomenclature
![Page 19: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/19.jpg)
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride
C. Molecular Nomenclature
![Page 20: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/20.jpg)
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10
C. Molecular Nomenclature
![Page 21: IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)](https://reader035.vdocuments.us/reader035/viewer/2022081416/5514ee8b55034693478b5d8d/html5/thumbnails/21.jpg)
+ -
+
B. Lewis Structures
Nonpolar Covalent - no charges
Polar Covalent - partial charges