Honors 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 Tuesday before exams start.
Major topics covered
Chapter 1 Chemistry an Introduction
Theory
Law
Scientific Method
Lab safety
Chapter 2 Measurements and Calculations
Sig figs
Dimensional analysis (field goals)
Metric system
Density
Chapter 3 Matter
Elements
Compounds
Mixture
Homogeneous/heterogeneous
Chapter 4 Chemical Foundations
Subatomic particles
Proton
Neutrons
Electrons
Nucleus
Rutherford
Thomson
Periodic Table
Periodic trends
Metals
Nonmetals
Metalloids
Alkali metals
Alkaline Earth Metals
Transition metals
Halogens
Noble gases
Chapter 5 Nomeclature
Ions
Cations
Anions
Ionic bonding
Polyatomic ions
Naming ionic compounds
Determining ionic formulas
Ionic dissociation
Molar mass
Covalent Naming
Covalent Prefixes
Naming Acids
Chapter 6 Chemical Reactions
Products
Reactants
Energy
Exothermic
Endothermic
Balancing Equations
Chapter 7 Reactions in an aqueous solution
Preciptiate
Redox reaction
Combustion Reaction
Single Replacement Reaction
Double Replacement reaction
Synthesis Reaction
Double Replacement Reaction
Net Ionic Equation
Spectator Ions
Acid Base Reactions
Chapter 8 Chemical Composition
Mole
Molar Mass
Mole gram conversion
Mole atom conversion
Chapter 9 Chemical Quantities
Stoichiometry
Limiting reactants
Percent Yield
Mole atom conversion
Chapter 11 Modern Atomic Theory
Bohr
Heisenberg
Orbitals
Energy levels
Electron configuration
Quantum numbers
Chapter 12 Chemical Bonding
Covalent bonding
Electronegativity
Polar Covalent Bond
Nonpolar covalent bond
Determining the type of bond
Lewis dot structures
VSEPR
Shapes of Molecules
Chapter 13 Gases
Boyle’s Law
Charles’ Law
Avagadro’s Law
Gay Lussac’s Law
Pressure
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
Cu- 2,1,-1 –½
Rb- 3, 2, 2, +½
Element
Symbol
Zirconium
Bromine
Magnesium
Silicon
Atomic number
Ion
Iron (II)
Chloride
Calcium
Atomic number
Symbol
Fe2+
ClCa2+
Mass Number protons
40
12
14
26
17
20
80
24
neutrons
51
electrons
35
14
Mass Number protons
56
36
41
neutrons
electrons
Determine the formula of the following compound and show the ionic dissociation.
Potassium sulfide
Magnesium chlorate
Ammonium iodide
Net Ionic Equations
Write out and balance the net ionic equation for each reaction
CaCl2 + NaOH  Ca(OH)2 + NaCl
Na3PO4 + Sr(NO3)2  NaNO3 + Sr3(PO4)2
Li3PO4 + NH4F  LiF + (NH4)3PO4
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
name the shape.
Mg(NO2)2 (shape of nitrite)
C2H3F
NH4OH (shape of hydroxide and shape
of ammonium)
SiO2
NI3
CaF2
Mg + HNO3  Mg(NO3)2 + H2
Calculate how many grams of Magnesium nitrate Mg(NO3)2 will be made from 32.1 g of
HNO3 and 15.4 g of Mg with a 79.3% yield.
CH4 + O2  H2O +
CO2
If 22 g of water is produced from 18 g of CH4 (methane) and 49 g of O2, what is the
percent yield?