Unit 4: Chemical Reactions.
4.1 Introduction for Reactions.
Use indications of change to distinguish between physical and chemical
changes.
Differentiate between a physical change or a chemical change.
Classify common processes as physical or chemical changes.
4.2 Net Ionic Equations.
Represent a physical change (i.e., dissolving) using a net ionic
equation.
Write a balanced net ionic equation for a chemical change, considering
both number of atoms and charge.
4.3 Representations of Reactions.
Represent a physical change with a particle diagram showing a difference
in particle spatial arrangement.
Draw a particle diagram for a chemical process with equal numbers of
atoms before and after the change.
Draw a particle diagram for a chemical change that balances charge.
4.4 Physical and Chemical Changes.
Justify a change as either a physical or chemical process based on
bonding changes.
Compare and contrast physical changes involving only IMFs (such as phase
changes) with those that involve bond breaking (such as dissolving an
ionic solid).
4.5 Stoichiometry.
Balance a chemical equation.
Clearly denote the mole ratio for a chemical process given a chemical
reaction.
Apply the Law of Conservation of Mass to determine theoretical yield
given mass amounts.
Use the ideal gas law or molarity to perform stoichiometric calculations
for reactions with gases and solutions.
4.6 Introduction to Titration.
Label a titration setup with terminology: analyte, titrant, indicator,
buret.
Use titration terminology to identify known, unknown, consumed, and
excess species at various titration points.
Perform a titration to the endpoint.
Use MacidVacid = MbaseVbase
at the equilavence point to calculate the molarity of an unkown acid or
base.
4.7 Types of Chemical Reactions.
Classify a reaction by identifying the transferring species: protons,
electrons, or ions.
Determine if a species is oxidized, reduced, or neither by assigning
oxidation numbers.
Complete a combustion reaction of a hydrocarbon.
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Write the balanced chemical reaction for the combustion of octane
(C8H18).
Identify the product of a precipitation reaction using the SNAP
mnemonic: sodium (Na+), nitrate (NO3+),
ammonia (NH4+), potassium (K+) ions are
always soluble
4.8 Introduction to Acid-Base Reactions.
Label the Brønsted-Lowry acid, base, conjugate acid, and conjugate base
in a reaction.
Recognize that water is amphoteric and label it as either an acid or a
base given the overall reaction.
List the strong acids and strong bases.
Compare the relative strengths of acids and bases based on dominant
species after the reaction.
Draw a particle diagram of a weak or strong acid and label
Brønsted-Lowry acid/base in reactants and conjugate acid/base in
products.
4.9 Oxidation-Reduction (Redox) Reactions.
Balance a redox reaction given a table of half-reactions, ensuring
conservation of atoms and electrons.