General Chemistry Midterm Review
100 Multiple choice problems
1 problem sheet (e configuration, lewis dot structures, molar mass etc.)
You may use a 3”x5” notecard on your exam provided that notecard is turned in prior to the end of class on the Monday before exams start.
Major topics covered
Unit 1 Introduction
Theory
Law
Scientific Method
Lab safety
Sig figs
Dimensional analysis (field goals)
Metric system
Density
Unit 2 Atomic theory
Subatomic particles
Proton
Neutrons
Electrons
Nucleus
Rutherford
Thomson
Bohr
Heisenberg
Orbitals
Energy levels
Electron configuration
Quantum numbers
Unit 3 Periodic Table
Elements
Compounds
Mixture
Homogeneous/heterogeneous
Periodic Table
Periodic trends
Metals
Nonmetals
Metalloids
Alkali metals
Alkaline Earth Metals
Transition metals
Halogens
Noble gases
Mole
Molar Mass
Mole gram conversion
Mole atom conversion
Unit 4 Nomenclature
Ions
Cations
Anions
Ionic bonding
Polyatomic ions
Naming ionic compounds
Determining ionic formulas
Ionic dissociation
Molar mass
Covalent Naming
Covalent Prefixes
Naming Acids
Unit 5 Chemical Reactions
Products
Reactants
Energy
Exothermic
Endothermic
Balancing Equations
Preciptiate
Redox reaction
Combustion Reaction
Single Replacement Reaction
Double Replacement reaction
Synthesis Reaction
Double Replacement Reaction
Spectator Ions
Acid Base Reactions
Unit 5 Chemical Bonding
Covalent bonding
Electronegativity
Polar Covalent Bond
Nonpolar covalent bond
Determining the type of bond
Lewis dot structures
Practice problems
Draw the orbital diagram, electron configuration for the following elements, draw the electron configuration and condensed electron configuration (circle electron w/ given quantum numbers, and circle your own)
W- 3, 2,1,+½ S- 2, 1, 0, –½
Rb- 3, 2, 2, +½ Cu 2,1,-1 –½
Element / Symbol / Atomic number / Mass Number / protons / neutrons / electronsZirconium / 40 / 51
Bromine / 80 / 35
Magnesium / 12 / 24
Silicon / 14 / 14
Ion / Symbol / Atomic number / Mass Number / protons / neutrons / electrons
Iron (II) / Fe2+ / 26 / 56
Chloride / Cl- / 17 / 36
Calcium / Ca2+ / 20 / 41
Determine the formula of the following compounds.
Potassium sulfide
Magnesium chlorate
Ammonium iodide
Equations
Balance the following equations
CaCl2 + NaOH ® Ca(OH)2 + NaCl
Na3PO4 + Sr(NO3)2 ® NaNO3 + Sr3(PO4)2
Li3PO4 + NH4F ® LiF + (NH4)3PO4
Mole Problems
How many moles are in 320 g of ammonium carbonate?
How many grams are in 5.23 mol of C3H8?
How many grams are in 5.1 mol of sulfur hexachloride?
How many moles are in 12.5 g of Nitrogen trichloride?
Empirical formulas and percent composition
Determine the percent composition of Li3BO3
Determine the percent composition of C2H5OH
What is the empirical formula of something that is 11.6% N and 88.4% Cl
What is the empirical formula of something that is 35.9 % Al and 64.1 % S
Name the compound, draw the Lewis dot structures for the following compounds and determine the shape.
Mg(NO2)2
NH4OH
NI3
C2H3F
SiO2
CaF2