Download - Chemistry 103
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Chemistry 103
Lecture 17
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Bonds
Ionic Bonds - electron transfer process. Typically between a metal and a nonmetals
Covalent Bonds - electrons shared. Typically involving nonmetals.
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Chapter 5 & 6 - Ionic Compounds Ionic Radii
Ionic Bonds defined
Lewis Symbols Lewis Diagrams
Nomenclature Polyatomic Ions
NaCl (Sodium Chloride)
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Chapter 6 & 7 - Covalent Systems Molecules - Molecular
Compounds & Elements Covalent bonding
Lewis Structures Properties of Bonds Valence count
Nomenclature
Bond Polarity/Electronegativity
CH4 (methane)
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Lewis Structures/Nomenclature NH4Cl
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Bond Polarity
Which pair of atoms will form the most polar bonds?
a. C,N b. C,O c. C,F d. C,C e. all are equal
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Chapter 8 - Chemical Quantities Molecular and Formula
Masses
The Mole (Molar Mass &Avogadro’s number)
Percent Composition
Dalton’s law of Definite Proportions
Empirical/Molecular Formulas
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Mathematics of Chemistry
Which contains more oxygen atoms: 0.50 moles of H2O, 15 g of NO2, or 3.0 x 1023
molecules of SO3?
A. H2O
B. NO2
C. SO3
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Mole Problems
A sulfur oxide (contains only S and O) having 50.0% by mass sulfur might have which molecular formula(s)?
a. SO b. SO2 c. S2O
d. S2O4 e. both SO2 or S2O4
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Chapter 9 - Chemical Reactions Chemical Equations
Balancing Reactions
Types of Chemical Reactions
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Balancing Chemical Equations When the equation:
K(s) + H2O(l) --- KOH(aq) + H2(g) is
balanced, the sum of the coefficients is ___?
a. 4 b. 5 c. 6 d. 7 e. 8
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Chemical Reactions
Predict the products of the following (unbalanced) reaction:
Mg(NO3)2 + Al(OH)3 ----->
a. MgH2 and Al(ONO3)3
b. Mg(OH)2 , Al(NO2)3 and O2
c. Mg(OH)2 and Al(NO3)3
d. Mg(OH)2 , Al2O3 and NO2
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Chapter 10 - Stoichiometry
Basic Stoichiometry Moles Grams
Limiting Reactant BEFORE vs AFTER Left over Reactant
Percent Yield
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Stoichiometry
The overall chemical equation for the photosynthesis reaction in plants is
6CO2 + 6H2O -----> C6H12O6 + 6O2
a. How many grams of sugar can be produced from 25.0g of CO2 and 25.0g of H2O?
b. After the reaction has run to completion, how many grams of the remaining reactant are left over?
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Stoichiometry
Consider the reaction:
3K2MnO4 + 4CO2 + 2H2O -------->
2KMnO4 + 4KHCO3 + MnO2
When 9.50 moles of K2MnO4, 7.20 x 1024 molecules of CO2 and 90.0g of H2O are mixed, a 173g quantity of MnO2 is actually produced in the lab. What is the percent yield of MnO2 based on the limiting reactant concept?