record total charge too
🧾AP CHEMISTRY STUDY GUIDE
Unit 4: Chemical Reactions
Review reaction evidence, equations, net ionic forms, stoichiometry, titration, oxidation, and reduction for AP Chemistry Unit 4.
8 key ideas8 flashcards5 practice questions
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Balance particles first, then calculate amounts.
coefficients only
matter and charge agree
Key ideas to know
Start with the relationships between ideas. Then close the notes and explain each one from memory.
- 01
A balanced equation conserves each element and total charge.
- 02
A net ionic equation includes only species that participate in the reaction.
- 03
Precipitation occurs when dissolved ions form a sparingly soluble solid.
- 04
Acid-base reactions transfer protons between donors and acceptors.
- 05
Oxidation is electron loss, while reduction is electron gain.
- 06
Stoichiometric coefficients give mole ratios among reactants and products.
- 07
A limiting reactant is consumed first and sets the maximum product amount.
- 08
Titration uses a known reactant amount to determine an unknown amount or concentration.
PART OF THE AP CHEMISTRY GUIDE
See every set in this course and follow a focused review order.
Open the full AP Chemistry guide →Two ideas worth correcting now
NOT QUITE
→Coefficients can alter subscripts inside formulas
USE THIS INSTEAD
Coefficients alter the number of formula units. Subscripts identify the substance and must remain fixed when balancing.
NOT QUITE
→The endpoint and equivalence point are always identical
USE THIS INSTEAD
The endpoint is the observed indicator signal, while the equivalence point is the stoichiometric condition.
Flashcards
Answer before opening each card. The effort to retrieve is part of the learning.
1What must a balanced chemical equation conserve?Show answer ＋
The number of each atom and the total charge.
2What is a spectator ion?Show answer ＋
An ion present in the same form before and after a reaction.
3What is a net ionic equation?Show answer ＋
An equation showing only species that undergo reaction.
4What is oxidation?Show answer ＋
Loss of electrons and an increase in oxidation number.
5What is reduction?Show answer ＋
Gain of electrons and a decrease in oxidation number.
6What is the limiting reactant?Show answer ＋
The reactant consumed first according to the available amounts and reaction ratio.
7What occurs at the equivalence point of a titration?Show answer ＋
Reactants have been combined in the stoichiometric ratio from the balanced equation.
8How is percent yield calculated?Show answer ＋
Actual yield divided by theoretical yield, multiplied by 100 percent.
Explain it in your own words
Use the answer as a check after you have written or spoken your response.
01How do you obtain a net ionic equation from a molecular equation?
Write strong aqueous electrolytes as ions, then cancel ions that appear unchanged on both sides.
02Why can mixing two clear ionic solutions produce a solid?
A cation and anion may form a compound with very low solubility, removing those ions from solution.
03How can oxidation numbers identify electron transfer?
An increased oxidation number marks oxidation, while a decreased oxidation number marks reduction.
04Why must the balanced equation come before a stoichiometric calculation?
Its coefficients supply the mole ratio needed to convert between substances.
05A titration overshoots its endpoint. How can that affect a calculated unknown concentration?
The recorded titrant volume is too large, so the calculated amount of analyte can be too large.
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