Intermolecular Forces. Bonding Ionic Covalent Polar covalent.
IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)
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Transcript of IIIIIIIV Ch. 8 - Covalent Bonding I. The Covalent Bond (p. 240 – 247)
I II III IV
Ch. 8 - Covalent Bonding
I. The Covalent Bond(p. 240 – 247)
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
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
Examples:
Which of the following are covalent compounds?
NaBr SiO2
CO2
AlCl3 CH4
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
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
N O F
Cl
Br
I
H
D. Diatomic Elements
The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2
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
E. Lewis Structures
Octet Rule Most atoms form bonds in order to obtain 8 valence
e-
Full energy level stability ~ Noble Gases
Ne
E. Lewis Structures
Example Electron Dot Notations:
Ca
P
H
C
CaP
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
How would you draw the Lewis structure for fluorine?
Diatomic!
F – F
E. Lewis Structures
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
E. Lewis Structures
Double Bonds Sharing two pairs of
electrons between two atoms
Draw Lewis Structures for 2 oxygen atoms
E. Lewis Structures
Triple Bonds Sharing three pairs of
electrons between two atoms
Draw Lewis Structures for 2 nitrogen atoms
I II III IV
Naming Molecules
Section 8.2
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.
PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-
NUMBER12345678910
C. Molecular Nomenclature
CCl4
N2O
SF6
carbon tetrachloride
dinitrogen monoxide
sulfur hexafluoride
C. Molecular Nomenclature
arsenic trichloride
dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10
C. Molecular Nomenclature
+ -
+
B. Lewis Structures
Nonpolar Covalent - no charges
Polar Covalent - partial charges