Chemistry Review Topics for Mid-Year Exam
REVIEW UNIT (formerly called Module 1, not included in Student Study Guide)
The review unit contains much that was learned in previous courses, such as models of the atom,
valence and periodic properties. These will be assumed to be known, but will not be directly tested.
Some new material is important and will find its way into the examination, either directly or indirectly.
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Understanding Significant Figures can gain you a few extra points.
Knowing how to name compounds and find formulas is necessary for doing some
problems
Knowing how to balance chemical equations is vital to do stoichiometry
Understanding the mole concept and molar masses from formulas is also important in
stoichiometry.
Basic stoichiometry is necessary to understand stoichiometry of gases as well as excess
and limiting type problems
UNIT ONE , Gases (formerly called Module 2, as in the Student Study Guide)
Chapter 1
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Know the properties, uses, environmental risks and formulas of many common gases,
including O2, O3, H2, He, Cl2, NH3, CH4, CO2, CO, SO2.
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Know what the Kinetic theory is, and be able to relate many of the properties of gases
to the motion of their particle (including such properties as compressibility, expansion,
diffusion, temperature, and pressure)
Know what atmospheric pressure is, and how it is measured (in atmospheres,
kilopascals and millimetres(Hg).
Know how to find pressure using a manometer
Know how to convert from Celsius to Kelvins and vice-versa.
Know how to use Graham’s Law to find rates of diffusion or effusion.
Know the Simple Gas Laws, being able to solve problems and represent the laws
graphically.
o Boyles law relating pressure and volume
o Charles law relating Temperature and volume
o Gay-Lussac’s law relating pressure and temperature
o Avogadro’s observations regarding the amount of gas
Know the combined (general) gas law and how to solve problems using it.
Know the Ideal Gas Law (PV=nRT) and how to use it to solve problems.
Know Dalton’s Law of Partial Pressures and how to use it to find the pressure or
amount of a gas within a mixture of gases.
Know how to deal with the stoichiometry of gases, especially when you can use
volumes of gas to find the number of moles.
Chapter 2
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UNIT TWO: Energy Changes in Reactions (formerly called Module 3, as in the Student Study Guide)
Chapter 3
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Difference between energy, heat, work and temperature
Law of conservation of energy
Types of Thermodynamic Systems
Calorimeters and Calorimetry. The Calorimeter formula: Q=mcΔT
Calculating Energy Transfer: -Q = Q or –m1c1ΔT1 = m2c2ΔT2
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Enthalpy and Enthalpy Change
Endothermic and Exothermic chemical changes
Endothermic and Exothermic physical changes (staircase analogy)
Phase Diagram (Temperature vs. Heat) and five things you should know from them
o Melting/Freezing Point
o Boiling / Condensation Point
o Heat of Fusion
o Heat of Vaporization
o Specific Heat Capacity
Simple Enthalpy Diagrams for Endothermic and Exothermic reactions.
Chapter 4
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Material for Mid-Year exam ends on page 155 of your textbook.
Review materials in the Student Study Guide go from the page labelled 2-1 to page 3-16