Chemistry - End of Third Trimester Exam Review (Chapters 11 – 13)
Chapter 11 – Chemical Reactions
11.1
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To write a word equation, write the names of the reactants to the left of the arrow separated by
plus signs; write the names of the products to the right of the arrow, also separated by plus
signs.
To write a skeleton equation, write the formulas for the reactants to the left of the yields sign
and the formulas for the products to the right.
After writing the skeleton equations, use coefficients to balance the equation so that is obeys
the law of conservation of mass.
11.2
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The five general types of reactions are combination, decomposition, single-replacement,
double-replacement, and combustion.
The number of elements and/or compounds reacting is a good indicator of possible reaction
type and thus possible products.
In a combination reaction, there is always a single product.
A decomposition reaction involves the breakdown of a single compound into two or more
simpler substances.
In a single-replacement reaction, both the reactants and the products are an element and a
compound.
A double-replacement reaction generally takes place between two ionic compounds in aqueous
solution.
A combustion reaction always involves oxygen as a reactant.
11.3
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A net ionic equation shows only those particles involved in the reaction and is balanced with
respect to mass and charge.
You can predict the formation of a precipitate by using the general rules for solubility of ionic
compounds.
Vocabulary:
Balanced Equation
Combustion Reaction
Net Ionic Equation
Catalyst
Complete Ionic Equation
Single-Replacement Reaction
Chemical Equation
Decomposition Reaction
Skeleton Equation
Coefficients
Double-Replacement
Reaction
Spectator Ion
Combination Reaction
Chemistry - End of Third Trimester Exam Review (Chapters 11 – 13)
Chapter 12 – Stoichiometry
12.1
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A balanced chemical equation provides the same kind of quantitative information that a recipe
does.
Chemists use balanced chemical equations as a basis to calculate how much reactant is needed
or product is formed in a reaction.
A balanced chemical equation can be interpreted in terms of different quantities, including
numbers of atoms, molecules, or moles; mass; and volume.
Mass and atoms are conserved in every chemical reaction.
12.2
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In chemical calculations, mole ratios are used to convert between moles of reactant and moles
of product, between moles of reactants, or between moles of products.
In a typical stoichiometric problem, the given quantity is first converted to moles. Then the mole
ratio from the balanced equation is used to calculate the moles of the wanted substance.
Finally, the moles are converted to any other unit of measurement related to the unit mole.
12.3
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In a chemical reaction, an insufficient quantity of any of the reactants will limit the amout of
product that forms.
The percent yield is a measure of the efficiency of a reaction performed in the laboratory.
Vocabulary:
Actual Yield
Mole Ratio
Excess Reagent
Percent Yield
Limiting Reagent
Stoichiometry
Theoretical Yield
Chapter 13 – States of Matter
13.1
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Particles in a gas are considered to be small, hard spheres with an insignificant volume. The
motion of the particles in a gas is rapid, constant, and random. All collisions between particles in
a gas are perfectly elastic.
Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a
gas with an object.
The Kelvin temperature of a substance is directly proportional to the average kinetic energy of
the particles of the substance.
Chemistry - End of Third Trimester Exam Review (Chapters 11 – 13)
13.2
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The interplay between the disruptive motions of particles in a liquid and the attractions among
the particles determines the physical properties of liquids.
During evaporation, only those molecules with certain minimum kinetic energy can escape from
the surface.
In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the
liquid. The rates of evaporation and condensation are equal.
At a temperature at which particles throughout a liquid have enouch kinetic energy to vaporize,
the liquid begins to boil.
13.3
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The general properties of solids and the shapes of crystals reflect the orderly arrangement and
the fixed locations of particles within the solids.
13.4
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Sublimation occurs in solids that have vapor pressures that exceed atmospheric pressure at or
near room temperature.
Conditions of pressure and temperature at which two phases exist in equilibrium are indicated
on a phase diagram by a line separating the two regions representing the phases.
Vocabulary:
Allotrope
Glass
Sublimation
Amorphous Solid
Kinetic Energy
Triple Point
Atmospheric Pressure
Kinetic Theory
Unit Cell
Barometer
Melting Point
Vacuum
Bioling Point
Normal Boiling Point
Vaporization
Crystal
Pascal (Pa)
Vapor Pressure
Evaporation
Phase Diagram
Gas Pressure
Standard Atmosphere