unit ix ppt #1 solution chemistry. ix.1 solutions and solubility definitions: solution: solvent:...
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UNIT IX PPT #1Solution Chemistry
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IX.1 SOLUTIONS AND SOLUBILITY
Definitions: Solution:
Solvent:
Solute:
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IX.1 SOLUTIONS AND SOLUBILITY
Saturated:
Unsaturated:
Solubility:
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IX.1 SOLUTIONS AND SOLUBILITY
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IX.1 SOLUTIONS AND SOLUBILITY
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IX.2 THE CONDUCTIVITY OF AQUEOUS SOLUTIONS
A conducting solution contains ions; the greater the concentration of ions, the greater the conductivity.
A compound made up of a METAL and NONMETAL is IONIC, and forms a conducting solution in water.
A substance made up of a NONMETAL and a NONMETAL is COVALENT, and will NOT form a conducting solution in water.
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IX.2 THE CONDUCTIVITY OF AQUEOUS SOLUTIONS
The "+" and "-" ions are now free to move around. The "+" ions would be attracted to a negative electrode and the "-" ions would be attracted to a positive electrode. In this way, the ionic solution conducts a current.
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IX.2 THE CONDUCTIVITY OF AQUEOUS SOLUTIONS
Compounds whose formulae start with a CARBON ATOM are usually ORGANIC and normally DO NOT form a conducting solution in water.
ACIDS and BASES form conducting solutions in water.
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IX.2 THE CONDUCTIVITY OF AQUEOUS SOLUTIONS
**TO CONDUCT or NOT CONDUCT??? that is the question.....
CONDUCT DOESN’T CONDUCT ionic - solid acidic - covalent basic - starts with C CH3COOH (exception)
http://www.youtube.com/watch?v=UHYWIM8AbPE Hebden p. 198 # 6-8
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IX.3 MOLECULAR POLARITY
Van der Waals Forces:
THREE main types:
A.DIPOLE-DIPOLE FORCESB.LONDON FORCESC.HYDROGEN BONDING
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IX.3 MOLECULAR POLARITY
A. DIPOLE-DIPOLE FORCES Dipole:
*a permanent dipole results from atoms with
different ELECTRONEGATIVITY! Dipole-Dipole Forces:
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IX.3 MOLECULAR POLARITY
Polar:
Nonpolar:
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IX.3 MOLECULAR POLARITY
Ex: Which of the following are expected to be polar and which are expected to be nonpolar??
nonpolar = symmetrical polar = assymetrical (if one end of the molecule
differs from the other)
Methane Hydrogen fluoride
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IX.3 MOLECULAR POLARITY
B. LONDON FORCES London Forces:
*if a permanent dipole is ABSENT….LONDON FORCES!
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IX.3 MOLECULAR POLARITY
IONIC BOND DIPOLE – DIPOLE ==LONDON FORCE
Intramolecular Intermolecular *the attraction between polar molecules is much less
than the attraction between ions
*polar molecules have a higher boiling temp then nonpolar
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IX.3 MOLECULAR POLARITY
C. HYDROGEN BONDING Hydrogen Bond: strong dipole – dipole attraction
between molecules containing a H – N, H – O, or H – F *intermolecular bond
*strongest van der Waals bonds – but still weaker than covalent and ionic
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IX.3 MOLECULAR POLARITY
Hebden p. 199 #9, p. 202 # 11-12, p. 203 # 13-16
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IX.4 POLAR AND NONPOLAR SOLVENTS
BOND TYPE WHAT TO LOOK FOR...
INTRAMOLECULAR BONDS:
IONIC BOND Made up of metal and nonmetal (or recognizable ions)
COVALENT BOND Made up of nonmetal and nonmetal
INTERMOLECULAR BONDS:
HYDROGEN BOND Look for HF or any molecule having OH or NH in its formula
DIPOLE-DIPOLE FORCE Look for an asymmetric molecule
LONDON FORCE Always present
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IX.4 POLAR AND NONPOLAR SOLVENTS
Common solvents: p.204 water methanol ethanol benzene ethoxyethane acetone acetic acid chloroform carbon tetrachloride heptane liquid ammonia
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IX.4 POLAR AND NONPOLAR SOLVENTS
“LIKE DISSOLVES LIKE”
POLAR dissolves ------- POLAR------- IONIC------- NONPOLAR
NONPOLAR dissolves ------- NONPOLAR
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IX.4 POLAR AND NONPOLAR SOLVENTS
Dissolving Process – 3 ATTRACTIONS:
attraction of solvent molecule to surrounding solvent molecules
attraction of solvent molecule to particles of solute
attraction of one solute particle to other solute particles
*when no CHARGE ==== no attraction
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IX.4 POLAR AND NONPOLAR SOLVENTS
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IX.4 POLAR AND NONPOLAR SOLVENTS
POLAR and IONIC solutes have low solubilities in nonpolar solvents.
POLAR and IONIC solutes tend to dissolve in polar solvents.
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IX.4 POLAR AND NONPOLAR SOLVENTS
NON POLAR solutes tend to be soluble in nonpolar solvents. *only attracted to solute particles by London
Forces
NONPOLAR substances tend to have at most a low solubility in polar solvents.
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IX.4 POLAR AND NONPOLAR SOLVENTS
**WATER is one of the most polar solvents known and tends to dissolve both polar and ionic solutes.
Hebden p. 207 # 18-22, p. 208 # 23-27
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IX.5 THE NATURE OF SOLUTIONS OF IONS
The formation of a solution depends on the ability of the solute to dissolve in the solvent.
SOLVATION:
IONIC SOLID:
MOLECULAR SOLID:
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IX.5 THE NATURE OF SOLUTIONS OF IONS
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IX.5 THE NATURE OF SOLUTIONS OF IONS
Ex: NaCl dissolving in water http://www.northland.cc.mn.us/biology/biolog
y1111/animations/dissolve.html
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IX.5 THE NATURE OF SOLUTIONS OF IONS
DISSOCIATION:
ex: NaCl ----> Na + Cl
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IX.5 THE NATURE OF SOLUTIONS OF IONS
IONIZATION:
ex: CH3COOH + H2O ------> CH3COO- + H3O
+
Hebden p. 210 # 28 & 29