Printable Chemistry Worksheets

Free pdf Worksheets to Download or Print

  • Chemical Laws
  • Periodic Table
  • Projects & Experiments
  • Scientific Method
  • Biochemistry
  • Physical Chemistry
  • Medical Chemistry
  • Chemistry In Everyday Life
  • Famous Chemists
  • Activities for Kids
  • Abbreviations & Acronyms
  • Weather & Climate
  • Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
  • B.A., Physics and Mathematics, Hastings College

This is a collection of chemistry worksheets in pdf format. The answers to the questions are available on separate worksheets so you can fill them out and then check your work. Please feel free to download these to your computer, print them, and use them as hand-outs.

  • Metals, Nonmetals, and Metalloids Worksheet
  • Metric to English Conversions Worksheet
  • Metric to English Conversions Answers
  • Metric to Metric Conversions Worksheet
  • Metric to Metric Conversions Answers
  • Temperature Conversions Worksheet
  • Temperature Conversions Answers
  • Temperature Conversions Worksheet #2
  • Temperature Conversions Answers #2
  • Moles to Grams Conversions Worksheet
  • Moles to Grams Conversions Answers
  • Formula or Molar Mass Worksheet
  • Formula or Molar Mass Worksheet Answers
  • Practicing Balancing Chemical Equations - Worksheet
  • Balancing Chemical Equations - Answers
  • Practicing Balancing Chemical Equations - Worksheet #2
  • Balancing Chemical Equations - Answers #2
  • Practicing Balancing Chemical Equations - Worksheet #3
  • Balancing Chemical Equations - Answers #3
  • Balancing Equations - Worksheet #4
  • Balancing Equations - Answer Key #4
  • Common Acid Names & Formulas - Worksheet
  • Acid Names and Formulas - Answers
  • Practice Calculations with Moles - Worksheet
  • Mole Calculations - Answers
  • Acid & Base pH - Worksheet
  • Acid & Base pH - Answers
  • Gas Laws Answers
  • Gas Laws Answers - Shown Work
  • Limiting Reagent - Worksheet
  • Limiting Reagent - Answers
  • Calculating Molarity - Worksheet
  • Calculating Molarity - Answers
  • Balancing Redox Reactions - Worksheet
  • Balancing Redox Reactions - Answers
  • Printable Element Crossword
  • Printable Element Crossword - Answers
  • Chemical Names to Chemical Formulas - Worksheet
  • Chemical Names to Chemical Formulas - Answer Key
  • Chemical Formulas to Chemical Names - Worksheet
  • Chemical Formulas to Chemical Names - Answer Key
  • Chemistry Element Word Search

Printable Periodic Tables

Here are some printable periodic tables to help you out, also in pdf format.

  • Color Printable Periodic Table - Pretty much everything you need that can fit on a page and still be readable. Color table with atomic numbers, element symbols, element names, atomic weights, periods, and groups. [ 2013 Edition ] [ 2012 Edition ]
  • Black/white Printable Periodic Table - Black/white table with atomic numbers, element symbols, element names, atomic weights, periods. [ 2013 Edition ] [ 2012 Edition ]
  • Blank Printable Periodic Table - Fill in the boxes yourself.
  • Electron Configuration Periodic Table - Periodic table that lists the electron configurations for each element.
  • Color Printable Periodic Table - Color table with atomic numbers, element symbols, atomic weights, periods, and groups. (no names)
  • Basic Printable Periodic Table - Black/white table with atomic numbers, element symbols, atomic weights, periods. (no names)
  • Basic Periodic Table with Element Names - Black/white table with element symbols, names, atomic numbers, and periods. (no weights)
  • Basic Periodic Table with Element Names (color) - Color periodic table with element symbols, names, atomic numbers, periods, and groups. (no weights)

The atomic weights given on these tables are the most recent (2007) values as accepted by the IUPAC.

Printable Scientific Method Flow Chart

This is a flow chart of the steps of the scientific method, available as a PDF file:

  • Scientific Method PDF

Also available is a PDF of a pie chart of the elemental composition of the human body .

  • A List of Common General Chemistry Problems
  • Printable Periodic Tables (PDF)
  • How to Balance Equations - Printable Worksheets
  • 20 Practice Chemistry Tests
  • Overview of High School Chemistry Topics
  • Molar Mass Example Problem
  • Periodic Table for Kids
  • Clickable Periodic Table of the Elements
  • Topics Typically Covered in Grade 11 Chemistry
  • Balancing Chemical Equations
  • Chemistry Elements Word Search Puzzles With Answers
  • Empirical Formula: Definition and Examples
  • Teach Yourself Chemistry Today
  • A List of the Elements of the Periodic Table
  • How to Use a Periodic Table of Elements
  • Why Is the Periodic Table Important?

Don't have Adobe Acrobat Reader? Click Here (You need Adobe Acrobat to read the files below.)

Physics Reviews for Final Exam - back to top

FR:2 - Final Review 2 ( Answer Key)

FR:V - Final Review Vocab Contains only the most important vocabulary from each chapter. Students were told to work on this at home.

FR:1 - Final Review 1 Students were challenged to take it like a test (with notes) in class. Solutions were given. It is recommended that students work the review again in preparation for the test. (Answer Key)

FR:GR - Final Review Guided Reading

11-15:Rev - Harmonic Motion and Light Review ( Answer Sheet )

15:2 - Misc Light Topics

15:1 - Optics

14:2 - Color

  • 14:1 - Light

Harmonic Motion and Waves (Ch 11-13) - back to top ( Bonus Skillsheet: "Harmonics" (see below) - typos fixed, now.

Important Notice Here About An Error Correction and TAKS information!

12:2 - Wave Actions NOTE: Yes, the worksheets numbers are out-of-order: it's a TAKS test thing! (Shorter class time that day.) This order will still work.

HME - Supplement: Harmonic Motion Equations

13:1 - Sound - Note: I removed the Mach number (660 mph). It didn't agree with the 340 m/s speed of sound in air I was using. Here's the deal: air's density and sound's speed in that air decreases with altitude. At 35,000 ft the speed of sound is 660 mph (only 293 m/s). I didn't have time on the worksheet to explain this, so I removed it. Sorry for any confusion.

12: 1 - Standing Waves

11: 2 - Waves

11: 1 - Harmonic Motion

Chapter 11-13 - Guided Reading over Harmonic Motion

6-9, 27:R - Electricity and Thermodynamics Review

8:1 - V, R, and I in Parallel Circuits

7:2 - V, R, and I in Series Circuits

7:1 - Types of Circuits and Ohm's Law

6:2 - Circuits and Symbols

6:1 - Electric Charge

  • 27:1 - Thermodynamics
  • Guided Reading for Chapter 27
  • 5and10:R - Review for Chapters 5 and 10
  • 10:1 - Magnetism
  • Chapter 10 Guided Reading .
  • 5:3 - Conservation of Energy

5:2 - Kinetic and Potential Energy

High School Chemistry Worksheets and Answer Keys, Study Guides and Vocabulary Sets.

CHEMISTRY is the study of matter, its properties, how and why substances combine or separate to form other substances, and how substances interact with energy. The five main branches of chemistry include analytical chemistry, physical chemistry, organic chemistry, inorganic chemistry and biochemistry.

Chemistry Worksheets and Study Guides High School

Atomic structure - set i, atomic structure - set ii, atoms and chemical bonding, chemical equations, rates and reactions, chemical equations, chemical reactions, kinetics and equilibrium, oxidation, reduction and electrochemistry, chemical formulas, mixtures and compounds, chemical compounds - set i, chemical compounds - set ii, chemical formulas and bonding, mixtures and compounds, gases and solutions, acids, bases and salts, matter and change, matter and energy, properties and states of matter, states of matter, the periodic law, elements - set i, elements - set ii, elements and the periodic table, the periodic table - set i, the periodic table - set ii, the science of chemistry, lab investigations/scientific method, measurements and calculations, nuclear chemistry, organic chemistry, newpath learning resources are fully aligned to us education standards. select a standard below to view aligned activities for your selected subject and grade:.

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Laboratory Safety

Handout - Laboratory Safety Activity - Understanding Chemical Hazard Labels & MSDS Activity - Disaster Demos

Atomic Structure - Ch. 3

Worksheet - Atomic Structure Project - Atomic Theory Timeline - Evaluation Sheet

Matter - Ch. 1

Worksheet - Matter Lab - Classifying Matter with Hardware Lab - Classification Rotation Lab - Chemical & Physical Changes (option 1) Lab - Chemical & Physical Changes (option 2) Activity - Categorizing Matter

Measurement - Ch. 2

Worksheet - Using Measurements Worksheet - Units & Unit Conversions Lab - Density of Pennies Article - "The Crash of Flight 143"

Electrons in Atoms - Ch. 4

Worksheet - Waves & Particles Worksheet - Bohr Model Worksheet - Quantum Model Worksheet - Electron Configuration Worksheet - Stability & Electron Configuration Lab - Emission Spectroscopy Lab - Electron Probability Activity - Patterns in Electron Configuration Activity - Electron Configuration Battleship

Periodic Table - Ch. 6

Worksheet - Periodic Trends Lab - Periodic Law Activity - Operation: Periodic Table Activity - What Element Am I? Activity - Periodically Puzzling

Chemical Bonding - Ch. 6 & 7 <

Worksheet - Molecular Compounds Worksheet - Ionic Compounds Worksheet - Acids Lab - Ionic vs. Covalent Activity - Formula Fun!

Molecular Structure - Ch. 6

Worksheet - Lewis Diagrams Worksheet - Molecular Geometry Lab - Molecular Structure Project - Molecular Model - Evaluation Sheet

The Mole - Ch. 3 & 7

Worksheet - Molar Conversions Worksheet - Molarity Worksheet - Formula Calculations Lab - Molar Conversions Lab - Empirical Formula Lab - Percentage of Water in Popcorn

Chemical Reactions - Ch. 8

Worksheet - Intro to Reactions Worksheet - Balancing Equations Worksheet - Types of Reactions Worksheet - Reaction Energy & Rate Lab - Types of Reactions (Design Lab) Lab - Types of Reactions Activity - Chemical Equations & Symbols

Stoichiometry - Ch. 9

Worksheet - Stoichiometry Worksheet - Limiting Reactants & Percent Yield Lab - Stoichiometry Lab - S'mores & Limiting Reactants

Gases - Ch. 10 & 11

Overview - Gases Worksheet - Gas Laws Worksheet - Ideal Gas Law & Stoichiometry Worksheet - Two More Gas Laws Lab - Boyle's Law Lab - Ideal Gas Law Article - Gas Laws & Scuba Diving

Liquids & Solids - Ch. 12

Worksheet - Liquids & Solids Worksheet - Changes of State Activity - Investigating Liquids & Solids

Solutions - Ch. 13 & 14

Worksheet - Nature of Solutions Worksheet - Concentration Worksheet - Colligative Properties Lab - Rate of Solution (Inquiry) Lab - Ice Cream Article - Ice Cream

Acids & Bases - Ch. 15 & 16

Worksheet - Introduction to Acids & Bases Worksheet - pH Worksheet - Titration Lab - Household Acids & Bases

Nuclear Chemistry - Ch. 22

Worksheet - The Nucleus & Radioactive Decay Lab - Understanding Half-life Project - Nuclear Applications  

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Chemistry LibreTexts

4.E: Chemical Reactions and Equations (Exercises)

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  • Page ID 64999

Exercises ( The Chemical Equation )

  • From the statement “nitrogen and hydrogen react to produce ammonia,” identify the reactants and the products.

From the statement “sodium metal reacts with water to produce sodium hydroxide and hydrogen,” identify the reactants and the products.

From the statement “magnesium hydroxide reacts with nitric acid to produce magnesium nitrate and water,” identify the reactants and the products.

From the statement “propane reacts with oxygen to produce carbon dioxide and water,” identify the reactants and the products.

Write and balance the chemical equation described by Exercise 1.

Write and balance the chemical equation described by Exercise 2.

Write and balance the chemical equation described by Exercise 3.

Write and balance the chemical equation described by Exercise 4. The formula for propane is C 3 H 8 .

Balance: ___NaClO 3 → ___NaCl + ___O 2

Balance: ___N 2 + ___H 2 → ___N 2 H 4

Balance: ___Al + ___O 2 → ___Al 2 O 3

Balance: ___C 2 H 4 + ___O 2 → ___CO 2 + ___H 2 O

How would you write the balanced chemical equation in Exercise 10 if all substances were gases?

  • How would you write the balanced chemical equation in Exercise 12 if all the substances except water were gases and water itself were a liquid?

1. reactants: nitrogen and hydrogen; product: ammonia

3. reactants: magnesium hydroxide and nitric acid; products: magnesium nitrate and water

5. N 2 + 3H 2 → 2NH 3

7. Mg(OH) 2 + 2HNO 3 → Mg(NO 3 ) 2 + 2H 2 O

9. 2NaClO 3 → 2NaCl + 3O 2

11. 4Al + 3O 2 → 2Al 2 O 3

13. N 2 (g) + 3H 2 (g) → 2NH 3 (g)

Exercises  (Types of Chemical Reactions - Single and Double Displacement Reactions )

  • What are the general characteristics that help you recognize single-replacement reactions?
  • What are the general characteristics that help you recognize double-replacement reactions?
  • Zn + Fe(NO 3 ) 2 → ?
  • F 2 + FeI 3 → ?
  • Li + MgSO 4 → ?
  • NaBr + Cl 2 → ?
  • Sn + H 2 SO 4 → ?
  • Al + NiBr 2 → ?
  • Mg + HCl → ?
  • HI + Br 2 → ?
  • FeCl 2 + Br 2 → ?
  • Fe(NO 3 ) 3 + Al → ?
  • Zn + Fe 3 (PO 4 ) 2 → ?
  • Ag + HNO 3 → ?
  • NaI + Cl 2 → ?
  • AgCl + Au → ?
  • Pt + H 3 PO 4 → ?
  • Li + H 2 O → ? (Hint: treat H 2 O as if it were composed of H + and OH − ions.)
  • Zn(NO 3 ) 2 + NaOH → ?
  • HCl + Na 2 S → ?
  • Ca(C 2 H 3 O 2 ) 2 + HNO 3 → ?
  • Na 2 CO 3 + Sr(NO 2 ) 2 → ?
  • Pb(NO 3 ) 2 + KBr → ?
  • K 2 O + MgCO 3 → ?
  • Sn(OH) 2 + FeBr 3 → ?
  • CsNO 3 + KCl → ?
  • K 2 O + Na 2 CO 3 → ?
  • (NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 → ?
  • K 3 PO 4 + SrCl 2 → ?
  • NaOH + MgCl 2 → ?
  • KC 2 H 3 O 2 + Li 2 CO 3 → ?
  • KOH + AgNO 3 → ?

1. One element replaces another element in a compound.

  • Zn + Fe(NO 3 ) 2 → Zn(NO 3 ) 2 + Fe
  • 3F 2 + 2FeI 3 → 3I 2 + 2FeF 3
  • Sn + H 2 SO 4 → SnSO 4 + H 2
  • 2Al + 3NiBr 2 → 2AlBr 3 + 3Ni
  • No reaction occurs.
  • Fe(NO 3 ) 3 + Al → Al(NO 3 ) 3 + Fe
  • 2NaI + Cl 2 → 2NaCl + I 2
  • Zn(NO 3 ) 2 + 2NaOH → Zn(OH) 2 + 2NaNO 3
  • 2HCl + Na 2 S → 2NaCl + H 2 S
  • Pb(NO 3 ) 2 + 2KBr → PbBr 2 + 2KNO 3
  • K 2 O + MgCO 3 → K 2 CO 3 + MgO
  • Pb(NO 3 ) 2 + 2KBr → PbBr 2 (s) + 2KNO 3
  • 2K 3 PO 4 + 3SrCl 2 → Sr 3 (PO 4 ) 2 (s) + 6KCl
  • 2NaOH + MgCl 2 → 2NaCl + Mg(OH) 2 (s)

Exercises (Ionic Equations - A Closer Look )

  • Write a chemical equation that represents NaBr(s) dissociating in water.

Write a chemical equation that represents SrCl 2 (s) dissociating in water.

Write a chemical equation that represents (NH 4 ) 3 PO 4 (s) dissociating in water.

Write a chemical equation that represents Fe(C 2 H 3 O 2 ) 3 (s) dissociating in water.

Write the complete ionic equation for the reaction of FeCl 2 (aq) and AgNO 3 (aq). You may have to consult the solubility rules.

Write the complete ionic equation for the reaction of BaCl 2 (aq) and Na 2 SO 4 (aq). You may have to consult the solubility rules.

Write the complete ionic equation for the reaction of KCl(aq) and NaC 2 H 3 O 2 (aq). You may have to consult the solubility rules.

Write the complete ionic equation for the reaction of Fe 2 (SO 4 ) 3 (aq) and Sr(NO 3 ) 2 (aq). You may have to consult the solubility rules.

Write the net ionic equation for the reaction of FeCl 2 (aq) and AgNO 3 (aq). You may have to consult the solubility rules.

Write the net ionic equation for the reaction of BaCl 2 (aq) and Na 2 SO 4 (aq). You may have to consult the solubility rules.

Write the net ionic equation for the reaction of KCl(aq) and NaC 2 H 3 O 2 (aq). You may have to consult the solubility rules.

Write the net ionic equation for the reaction of Fe 2 (SO 4 ) 3 (aq) and Sr(NO 3 ) 2 (aq). You may have to consult the solubility rules.

Identify the spectator ions in Exercises 9 and 10.

  • Identify the spectator ions in Exercises 11 and 12.

1. \(\mathrm{NaBr}(\mathrm{s}) \xrightarrow{\mathrm{H}_2 \mathrm{O}} \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq}) \)

3. \(\left(\mathrm{NH}_4\right)_3 \mathrm{PO}_4(\mathrm{~s}) \xrightarrow{\mathrm{H}_2 \mathrm{O}} 3 \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{PO}_4^{3-}(\mathrm{aq}) \)

5. \(\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{Cl}^{-}(\mathrm{aq})+2 \mathrm{Ag}^{+}(\mathrm{aq})+2 \mathrm{NO}_3^{-}(\mathrm{aq}) \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{NO}_3^{-}(\mathrm{aq})+2 \mathrm{AgCl}(\mathrm{s})\)

7. \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2^{-}(\mathrm{aq}) \rightarrow \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{K}^{+}(\mathrm{aq}) +\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2^{-}(\mathrm{aq}) \)

9. \(2 \mathrm{Cl}^{-}(\mathrm{aq})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow 2 \mathrm{AgCl}(\mathrm{s}) \)

11. There is no overall reaction.

13. In Exercise 9, \(\mathrm{Fe}^{2+}(\mathrm{aq})\) and \(\mathrm{NO}_3{ }^{-}(\mathrm{aq})\) are spectator ions; in Exercise 10, \(\mathrm{Na}^{+}(\mathrm{aq})\) and \(\mathrm{Cl}^{-}(\mathrm{aq})\) are spectator ions.

Exercises  (Composition, Decomposition, and Combustion Reactions )

  • NaCl + AgNO 3 → AgCl + NaNO 3
  • CaO + CO 2 → CaCO 3
  • H 2 + Cl 2 → 2HCl
  • 2HBr + Cl 2 → 2HCl + Br 2
  • 2SO 2 + O 2 → 2SO 3
  • 6C + 3H 2 → C 6 H 6
  • 4Na + 2C + 3O 2 → 2Na 2 CO 3
  • Na 2 CO 3 → Na 2 O + CO 2
  • HCl + NaOH → NaCl + H 2 O
  • CaCO 3 → CaO + CO 2
  • 3O 2 → 2O 3
  • 2KClO 3 → 2KCl + 3O 2
  • Na 2 O + CO 2 → Na 2 CO 3
  • H 2 SO 3 → H 2 O + SO 2
  • 2C 7 H 5 N 3 O 6 → 3N 2 + 5H 2 O + 7CO + 7C
  • C 6 H 12 O 6 + 6O 2 → 6CO 2 + 6H 2 O
  • 2Fe 2 S 3 + 9O 2 → 2Fe 2 O 3 + 6SO 2
  • CH 4 + 2F 2 → CF 4 + 2H 2
  • 2H 2 + O 2 → 2H 2 O
  • P 4 + 5O 2 → 2P 2 O 5
  • 2Al 2 S 3 + 9O 2 → 2Al 2 O 3 + 6SO 2
  • C 2 H 4 + O 2 → C 2 H 4 O 2
  • C 2 H 4 + Cl 2 → C 2 H 4 Cl 2
  • Is it possible for a composition reaction to also be a combustion reaction? Give an example to support your case.
  • Is it possible for a decomposition reaction to also be a combustion reaction? Give an example to support your case.
  • C 4 H 9 OH + O 2 → ?
  • CH 3 NO 2 + O 2 → ?
  • B 2 H 6 + O 2 → ? (The oxide of boron formed is B 2 O 3 .)
  • Al 2 S 3 + O 2 → ? (The oxide of sulfur formed is SO 2 .)
  • Al 2 S 3 + O 2 → ? (The oxide of sulfur formed is SO 3 .)
  • not composition
  • composition
  • not decomposition
  • decomposition

13. Yes; 2H 2 + O 2 → 2H 2 O (answers will vary)

  • C 4 H 9 OH + 6O 2 → 4CO 2 + 5H 2 O
  • 4CH 3 NO 2 + 3O 2 → 4CO 2 + 6H 2 O + 2N 2

Exercises ( Neutralization Reactions )

  • What is the Arrhenius definition of an acid?
  • What is the Arrhenius definition of a base?
  • HCl and KOH
  • H 2 SO 4 and KOH
  • H 3 PO 4 and Ni(OH) 2
  • HBr and Fe(OH) 3
  • HNO 2 and Al(OH) 3
  • HClO 3 and Mg(OH) 2
  • Write a balanced chemical equation for each neutralization reaction in Exercise 3.
  • Write a balanced chemical equation for each neutralization reaction in Exercise 4.
  • HI(aq) + KOH(aq) → ?
  • H 2 SO 4 (aq) + Ba(OH) 2 (aq) → ?
  • HNO 3 (aq) + Fe(OH) 3 (s) → ?
  • H 3 PO 4 (aq) + CsOH(aq) → ?
  • Write the net ionic equation for each neutralization reaction in Exercise 7.
  • Write the net ionic equation for each neutralization reaction in Exercise 8.
  • Write the complete and net ionic equations for the neutralization reaction between HClO 3 (aq) and Zn(OH) 2 (s). Assume the salt is soluble.
  • Write the complete and net ionic equations for the neutralization reaction between H 2 C 2 O 4 (s) and Sr(OH) 2 (aq). Assume the salt is insoluble.
  • Explain why the net ionic equation for the neutralization reaction between HCl(aq) and KOH(aq) is the same as the net ionic equation for the neutralization reaction between HNO 3 (aq) and RbOH.
  • Explain why the net ionic equation for the neutralization reaction between HCl(aq) and KOH(aq) is different from the net ionic equation for the neutralization reaction between HCl(aq) and AgOH.
  • Write the complete and net ionic equations for the neutralization reaction between HCl(aq) and KOH(aq) using the hydronium ion in place of H + . What difference does it make when using the hydronium ion?
  • Write the complete and net ionic equations for the neutralization reaction between HClO 3 (aq) and Zn(OH) 2 (s) using the hydronium ion in place of H + . Assume the salt is soluble. What difference does it make when using the hydronium ion?

1. An Arrhenius acid increases the amount of H + ions in an aqueous solution.

  • KCl and H 2 O
  • K 2 SO 4 and H 2 O
  • Ni 3 (PO 4 ) 2 and H 2 O
  • HCl + KOH → KCl + H 2 O
  • H 2 SO 4 + 2KOH → K 2 SO 4 + 2H 2 O
  • 2H 3 PO 4 + 3Ni(OH) 2 → Ni 3 (PO 4 ) 2 + 6H 2 O
  • HI(aq) + KOH(aq) → KI(aq) + H 2 O(ℓ)
  • H 2 SO 4 (aq) + Ba(OH) 2 (aq) → BaSO 4 (s) + 2H 2 O(ℓ)
  • H + (aq) + OH − (aq) → H 2 O(ℓ)
  • 2H + (aq) + SO 4 2 − (aq) + Ba 2 + (aq) + 2OH − (aq) → BaSO 4 (s) + 2H 2 O(ℓ)

11.    Complete ionic equation:

2H + (aq) + 2ClO 3 − (aq) + Zn 2 + (aq) + 2OH − (aq) → Zn 2 + (aq) + 2ClO 3 − (aq) + 2H 2 O(ℓ)

Net ionic equation:

2H + (aq) + 2OH − (aq) → 2H 2 O(ℓ)

13.  Because the salts are soluble in both cases, the net ionic reaction is just         H + (aq) + OH − (aq) → H 2 O(ℓ).

15.   Complete ionic equation:

H 3 O + (aq) + Cl − (aq) + K + (aq) + OH − (aq) → 2H 2 O(ℓ) + K + (aq) + Cl − (aq)

H 3 O + (aq) + OH − (aq) → 2H 2 O(ℓ)

17.    The difference is simply the presence of an extra water molecule as a product.

Exercises ( Oxidation-Reduction Reactions )

Is the reaction

2K (s) + Br 2 (ℓ) → 2KBr(s)

an oxidation-reduction reaction? Explain your answer.

    an oxidation-reduction reaction? Explain your answer.

In the reaction

    indicate what has lost electrons and what has gained electrons.

     indicate what has lost electrons and what has gained electrons.

     indicate what has been oxidized and what has been reduced.

    indicate what has been oxidized and what has been reduced.

What are two different definitions of oxidation?

  • What are two different definitions of reduction?  
  • SO 2 2 −
  • Ca(NO 3 ) 2
  • (NH 4 ) 2 S
  • Li 2 O 2 (lithium peroxide)
  • NaH (sodium hydride)
  • NO 2 −
  • Zn(C 2 H 3 O 2 ) 2
  • Identify what is being oxidized and reduced in this redox equation by assigning oxidation numbers to the atoms.

      2NO + Cl 2 → 2NOCl

     Fe + SO 3 → FeSO 3

     C 7 H 16 + 11O 2 → 7CO 2 + 8H 2 O

1. Yes; both K and Br are changing oxidation numbers.

3. Ca has lost electrons, and O has gained electrons.

5. Li has been oxidized, and O has been reduced.

7. loss of electrons; increase in oxidation number

  • S: +4; O: −2
  • S: +2; O: −2
  • Ca: 2+; N: +5; O: −2
  • C: +2; O: −2
  • C: +4; O: −2
  • Ni: +2; Cl: −1
  • Ni: +3; Cl: −1
  • C: 0; H: +1; O: −2
  • N: −3; H: +1
  • Rb: +1; S: +6; O: −2
  • Zn: +2; C: 0; H: +1; O: −2

15. N is being oxidized, and Cl is being reduced.

17. O is being oxidized, and Kr is being reduced.

19.K is being oxidized, and Mg is being reduced.

Additional Exercises

1. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the boiling of water, including the proper phase labels.

2. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the freezing of water, including the proper phase labels.

3. Explain why

4Na(s) + 2Cl 2 (g) → 4NaCl(s)

should not be considered a proper chemical equation.

4. Explain why

H 2 (g) + 1/2O 2 (g) → H 2 O(ℓ)

5. Does the chemical reaction represented by

3Zn(s) + 2Al(NO 3 ) 3 (aq) → 3Zn(NO 3 ) 2 (aq) + 2Al(s)

proceed as written? Why or why not?

6. Does the chemical reaction represented by

2Au(s) + 2HNO 3 (aq) → 2AuNO 3 (aq) + H 2 (g)

proceed as written? Gold is a relatively useful metal for certain applications, such as jewelry and electronics. Does your answer suggest why this is so?

7. Explain what is wrong with this double-replacement reaction.

NaCl(aq) + KBr(aq) → NaK(aq) + ClBr(aq)

8. Predict the products of and balance this double-replacement reaction.

Ag 2 SO 4 (aq) + SrCl 2 (aq) → ?

9. Write the complete and net ionic equations for this double-replacement reaction.

BaCl 2 (aq) + Ag 2 SO 4 (aq) → ?

10. Write the complete and net ionic equations for this double-replacement reaction.

11. Identify the spectator ions in this reaction. What is the net ionic equation?

NaCl(aq) + KBr(aq) → NaBr(aq) + KCl(aq)

12. Complete this reaction and identify the spectator ions. What is the net ionic equation?

3H 2 SO 4 (aq) + 2Al(OH) 3 (s) → ?

13. Can a reaction be a composition reaction and a redox reaction at the same time? Give an example to support your answer.

14. Can a reaction be a combustion reaction and a redox reaction at the same time? Give an example to support your answer.

15. Can a reaction be a decomposition reaction and a redox reaction at the same time? Give an example to support your answer.

16. Can a reaction be a combustion reaction and a double-replacement reaction at the same time? Give an example to support your answer.

17. Why is CH 4 not normally considered an acid?

18. Methyl alcohol has the formula CH 3 OH. Why would methyl alcohol not normally be considered a base?

19. What are the oxidation numbers of the nitrogen atoms in these substances?

20. What are the oxidation numbers of the sulfur atoms in these substances?

21. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating and indicate the initial and final oxidation numbers of that element.

2CuCl(aq) → CuCl 2 (aq) + Cu(s)

Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating and indicate the initial and final oxidation numbers of that element.

1. H 2 O(ℓ) → H 2 O(g)

3. The coefficients are not in their lowest whole-number ratio.

5. No; zinc is lower in the activity series than aluminum.

7. In the products, the cation is pairing with the cation, and the anion is pairing with the anion.

9. Complete ionic equation: Ba 2 + (aq) + 2Cl − (aq) + 2Ag + (aq) + SO 4 2 − (aq) → BaSO 4 (s) + 2AgCl(s)

    Net ionic equation: The net ionic equation is the same as the complete ionic equation.

11. Each ion is a spectator ion; there is no overall net ionic equation.

13. Yes; H 2 + Cl 2 → 2HCl (answers will vary)

15, Yes; 2HCl → H 2 + Cl 2 (answers will vary)

17. It does not increase the H + ion concentration; it is not a compound of H + .

  • Introduction
  • 1.1 Chemistry in Context
  • 1.2 Phases and Classification of Matter
  • 1.3 Physical and Chemical Properties
  • 1.4 Measurements
  • 1.5 Measurement Uncertainty, Accuracy, and Precision
  • 1.6 Mathematical Treatment of Measurement Results
  • Key Equations
  • 2.1 Early Ideas in Atomic Theory
  • 2.2 Evolution of Atomic Theory
  • 2.3 Atomic Structure and Symbolism
  • 2.4 Chemical Formulas
  • 3.1 Electromagnetic Energy
  • 3.2 The Bohr Model
  • 3.3 Development of Quantum Theory
  • 3.4 Electronic Structure of Atoms (Electron Configurations)
  • 3.5 Periodic Variations in Element Properties
  • 3.6 The Periodic Table
  • 3.7 Ionic and Molecular Compounds
  • 4.1 Ionic Bonding
  • 4.2 Covalent Bonding
  • 4.3 Chemical Nomenclature
  • 4.4 Lewis Symbols and Structures
  • 4.5 Formal Charges and Resonance
  • 4.6 Molecular Structure and Polarity
  • 5.1 Valence Bond Theory
  • 5.2 Hybrid Atomic Orbitals
  • 5.3 Multiple Bonds
  • 5.4 Molecular Orbital Theory
  • 6.1 Formula Mass
  • 6.2 Determining Empirical and Molecular Formulas
  • 6.3 Molarity
  • 6.4 Other Units for Solution Concentrations
  • 7.1 Writing and Balancing Chemical Equations
  • 7.2 Classifying Chemical Reactions
  • 7.3 Reaction Stoichiometry
  • 7.4 Reaction Yields
  • 7.5 Quantitative Chemical Analysis
  • 8.1 Gas Pressure
  • 8.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
  • 8.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions
  • 8.4 Effusion and Diffusion of Gases
  • 8.5 The Kinetic-Molecular Theory
  • 8.6 Non-Ideal Gas Behavior
  • 9.1 Energy Basics
  • 9.2 Calorimetry
  • 9.3 Enthalpy
  • 9.4 Strengths of Ionic and Covalent Bonds
  • 10.1 Intermolecular Forces
  • 10.2 Properties of Liquids
  • 10.3 Phase Transitions
  • 10.4 Phase Diagrams
  • 10.5 The Solid State of Matter
  • 10.6 Lattice Structures in Crystalline Solids
  • 11.1 The Dissolution Process
  • 11.2 Electrolytes
  • 11.3 Solubility
  • 11.4 Colligative Properties
  • 11.5 Colloids
  • 12.1 Spontaneity
  • 12.2 Entropy
  • 12.3 The Second and Third Laws of Thermodynamics
  • 12.4 Free Energy
  • 13.1 Chemical Equilibria
  • 13.2 Equilibrium Constants
  • 13.3 Shifting Equilibria: Le Châtelier’s Principle
  • 13.4 Equilibrium Calculations
  • 14.1 Brønsted-Lowry Acids and Bases
  • 14.2 pH and pOH
  • 14.3 Relative Strengths of Acids and Bases
  • 14.4 Hydrolysis of Salts
  • 14.5 Polyprotic Acids
  • 14.6 Buffers
  • 14.7 Acid-Base Titrations
  • 15.1 Precipitation and Dissolution
  • 15.2 Lewis Acids and Bases
  • 15.3 Coupled Equilibria
  • 16.1 Review of Redox Chemistry
  • 16.2 Galvanic Cells
  • 16.3 Electrode and Cell Potentials
  • 16.4 Potential, Free Energy, and Equilibrium
  • 16.5 Batteries and Fuel Cells
  • 16.6 Corrosion
  • 16.7 Electrolysis
  • 17.1 Chemical Reaction Rates
  • 17.2 Factors Affecting Reaction Rates
  • 17.3 Rate Laws
  • 17.4 Integrated Rate Laws
  • 17.5 Collision Theory
  • 17.6 Reaction Mechanisms
  • 17.7 Catalysis
  • 18.1 Periodicity
  • 18.2 Occurrence and Preparation of the Representative Metals
  • 18.3 Structure and General Properties of the Metalloids
  • 18.4 Structure and General Properties of the Nonmetals
  • 18.5 Occurrence, Preparation, and Compounds of Hydrogen
  • 18.6 Occurrence, Preparation, and Properties of Carbonates
  • 18.7 Occurrence, Preparation, and Properties of Nitrogen
  • 18.8 Occurrence, Preparation, and Properties of Phosphorus
  • 18.9 Occurrence, Preparation, and Compounds of Oxygen
  • 18.10 Occurrence, Preparation, and Properties of Sulfur
  • 18.11 Occurrence, Preparation, and Properties of Halogens
  • 18.12 Occurrence, Preparation, and Properties of the Noble Gases
  • 19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds
  • 19.2 Coordination Chemistry of Transition Metals
  • 19.3 Spectroscopic and Magnetic Properties of Coordination Compounds
  • 20.1 Nuclear Structure and Stability
  • 20.2 Nuclear Equations
  • 20.3 Radioactive Decay
  • 20.4 Transmutation and Nuclear Energy
  • 20.5 Uses of Radioisotopes
  • 20.6 Biological Effects of Radiation
  • 21.1 Hydrocarbons
  • 21.2 Alcohols and Ethers
  • 21.3 Aldehydes, Ketones, Carboxylic Acids, and Esters
  • 21.4 Amines and Amides
  • A | The Periodic Table
  • B | Essential Mathematics
  • C | Units and Conversion Factors
  • D | Fundamental Physical Constants
  • E | Water Properties
  • F | Composition of Commercial Acids and Bases
  • G | Standard Thermodynamic Properties for Selected Substances
  • H | Ionization Constants of Weak Acids
  • I | Ionization Constants of Weak Bases
  • J | Solubility Products
  • K | Formation Constants for Complex Ions
  • L | Standard Electrode (Half-Cell) Potentials
  • M | Half-Lives for Several Radioactive Isotopes

The spectrum consists of colored lines, at least one of which (probably the brightest) is red.

3.233 × × 10 −19 J; 2.018 eV

ν = 4.568 × × 10 14 s −1 ; λ = 656.3 nm; Energy mol −1 = 1.823 × × 10 5 J mol −1 ; red

(a) λ = 8.69 × × 10 −7 m; E = 2.29 × × 10 −19 J; (b) λ = 4.59 × × 10 −7 m; E = 4.33 × × 10 −19 J; The color of (a) is red; (b) is blue.

E = 9.502 × × 10 −15 J; ν = 1.434 × × 10 19 s −1

Red: 660 nm; 4.54 × × 10 14 Hz; 3.01 × × 10 −19 J. Green: 520 nm; 5.77 × × 10 14 Hz; 3.82 × × 10 −19 J. Blue: 440 nm; 6.81 × × 10 14 Hz; 4.51 × × 10 −19 J. Somewhat different numbers are also possible.

5.49 × × 10 14 s −1 ; no

Quantized energy means that the electrons can possess only certain discrete energy values; values between those quantized values are not permitted.

2.856 eV 2.856 eV

−8.716 × × 10 −18 J

−3.405 × × 10 −20 J

1.471 × × 10 −17 J

Both involve a relatively heavy nucleus with electrons moving around it, although strictly speaking, the Bohr model works only for one-electron atoms or ions. According to classical mechanics, the Rutherford model predicts a miniature “solar system” with electrons moving about the nucleus in circular or elliptical orbits that are confined to planes. If the requirements of classical electromagnetic theory that electrons in such orbits would emit electromagnetic radiation are ignored, such atoms would be stable, having constant energy and angular momentum, but would not emit any visible light (contrary to observation). If classical electromagnetic theory is applied, then the Rutherford atom would emit electromagnetic radiation of continually increasing frequency (contrary to the observed discrete spectra), thereby losing energy until the atom collapsed in an absurdly short time (contrary to the observed long-term stability of atoms). The Bohr model retains the classical mechanics view of circular orbits confined to planes having constant energy and angular momentum, but restricts these to quantized values dependent on a single quantum number, n . The orbiting electron in Bohr’s model is assumed not to emit any electromagnetic radiation while moving about the nucleus in its stationary orbits, but the atom can emit or absorb electromagnetic radiation when the electron changes from one orbit to another. Because of the quantized orbits, such “quantum jumps” will produce discrete spectra, in agreement with observations.

Both models have a central positively charged nucleus with electrons moving about the nucleus in accordance with the Coulomb electrostatic potential. The Bohr model assumes that the electrons move in circular orbits that have quantized energies, angular momentum, and radii that are specified by a single quantum number, n = 1, 2, 3, …, but this quantization is an ad hoc assumption made by Bohr to incorporate quantization into an essentially classical mechanics description of the atom. Bohr also assumed that electrons orbiting the nucleus normally do not emit or absorb electromagnetic radiation, but do so when the electron switches to a different orbit. In the quantum mechanical model, the electrons do not move in precise orbits (such orbits violate the Heisenberg uncertainty principle) and, instead, a probabilistic interpretation of the electron’s position at any given instant is used, with a mathematical function ψ called a wavefunction that can be used to determine the electron’s spatial probability distribution. These wavefunctions, or orbitals, are three-dimensional stationary waves that can be specified by three quantum numbers that arise naturally from their underlying mathematics (no ad hoc assumptions required): the principal quantum number, n (the same one used by Bohr), which specifies shells such that orbitals having the same n all have the same energy and approximately the same spatial extent; the angular momentum quantum number l , which is a measure of the orbital’s angular momentum and corresponds to the orbitals’ general shapes, as well as specifying subshells such that orbitals having the same l (and n ) all have the same energy; and the orientation quantum number m , which is a measure of the z component of the angular momentum and corresponds to the orientations of the orbitals. The Bohr model gives the same expression for the energy as the quantum mechanical expression and, hence, both properly account for hydrogen’s discrete spectrum (an example of getting the right answers for the wrong reasons, something that many chemistry students can sympathize with), but gives the wrong expression for the angular momentum (Bohr orbits necessarily all have non-zero angular momentum, but some quantum orbitals [ s orbitals] can have zero angular momentum).

n determines the general range for the value of energy and the probable distances that the electron can be from the nucleus. l determines the shape of the orbital. m 1 determines the orientation of the orbitals of the same l value with respect to one another. m s determines the spin of an electron.

(a) 2 p ; (b) 4 d ; (c) 6 s

(a) 3 d; (b) 1 s; (c) 4 f

(a) x. 2, y. 2, z. 2; (b) x. 1, y. 3, z. 0; (c) x. 4 0 0 1 2 , 1 2 , y. 2 1 0 1 2 , 1 2 , z. 3 2 0 1 2 ; 1 2 ; (d) x. 1, y. 2, z. 3; (e) x. l = 0, m l = 0, y. l = 1, m l = –1, 0, or + 1, z. l = 2, m l = –2, –1, 0, +1, +2

For example, Na + : 1 s 2 2 s 2 2 p 6 ; Ca 2+ : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 ; Sn 2+ : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 4 d 10 5 s 2 ; F – : 1 s 2 2 s 2 2 p 6 ; O 2– : 1 s 2 2 s 2 2 p 6 ; Cl – : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 .

(a) 1 s 2 2 s 2 2 p 3 ; (b) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 2 ; (c) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 6 ; (d) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 4 ; (e) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 6 6 s 2 4 f 9

The charge on the ion.

Rb + , Se 2−

Although both (b) and (c) are correct, (e) encompasses both and is the best answer.

1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 6 6 s 2 4 f 14 5 d 10

Co has 27 protons, 27 electrons, and 33 neutrons: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 7 . I has 53 protons, 53 electrons, and 78 neutrons: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 4 d 10 5 s 2 5 p 5 .

Rb < Li < N < F

Mg < Ca < Rb < Cs

Si 4+ < Al 3+ < Ca 2+ < K +

Mg 2+ < K + < Br – < As 3–

(a) metal, inner transition metal; (b) nonmetal, representative element; (c) metal, representative element; (d) nonmetal, representative element; (e) metal, transition metal; (f) metal, inner transition metal; (g) metal, transition metal; (h) nonmetal, representative element; (i) nonmetal, representative element; (j) metal, representative element

(a) He; (b) Be; (c) Li; (d) O

(a) krypton, Kr; (b) calcium, Ca; (c) fluorine, F; (d) tellurium, Te

(a) 11 23 Na 11 23 Na ; (b) 54 129 Xe 54 129 Xe ; (c) 33 73 As 33 73 As ; (d) 88 226 Ra 88 226 Ra

Ionic: KCl, MgCl 2 ; Covalent: NCl 3 , ICl, PCl 5 , CCl 4

(a) covalent; (b) ionic, Ba 2+ , O 2− ; (c) ionic, NH 4 + , NH 4 + , CO 3 2− ; CO 3 2− ; (d) ionic, Sr 2+ , H 2 PO 4 − ; H 2 PO 4 − ; (e) covalent; (f) ionic, Na + , O 2−

(a) CaS; (b) (NH 4 ) 2 SO 4 ; (c) AlBr 3 ; (d) Na 2 HPO 4 ; (e) Mg 3 (PO 4 ) 2

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  12. Mrs. J's Chemistry Page

    These materials were designed for my high school Chemistry I Honors class. Teachers, please feel free to use and modify them for your own classes. If you do so, I would appreciate ... The Mole - Ch. 3 & 7. Worksheet - Molar Conversions Worksheet - Molarity Worksheet - Formula Calculations Lab - Molar Conversions Lab - Empirical Formula ...

  13. PDF 5.3 questions ms 1. (1) [1]

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  14. 5.3 Chemistry Vocab Flashcards

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  15. Topic 5.3 Concentration Changes Over Time.pdf

    1. Complete the table below. How do you know? The half life is constant (7 sec.) Only first order reactions have a constant half-life rate. The slope of the line for the graph [A] vs. time is linear and slope=-k. The slope and half life rate are not constant. What must be plotted on the y-axis to give a straight line? ln[A] [A] 1/[A] 2. What is the order of the reaction with respect to NO 2 if ...

  16. Printable Chemistry Worksheets (with Answers)

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  18. 4.E: Chemical Reactions and Equations (Exercises ...

    Write the complete and net ionic equations for the neutralization reaction between HClO 3 (aq) and Zn(OH) 2 (s) using the hydronium ion in place of H +. Assume the salt is soluble. What difference does it make when using the hydronium ion? Answers. An Arrhenius acid increases the amount of H + ions in an aqueous solution. KCl and H 2 O; K 2 SO ...

  19. Pearson Chemistry

    Chapter 1: Introduction to Chemistry Section 1.1: The Scope of Chemistry Section 1.2: Chemistry and You Section 1.3: Thinking Like a Scientist Section 1.4: Problem Solving in Chemistry Page 28: Assessment Page 31: Standardized Test Prep Exercise 1 Exercise 2 Exercise 3 Exercise 4 Exercise 5 Exercise 6 Exercise 7 Chapter 2: Matter and Change

  20. Answer Key Chapter 3

    1. The spectrum consists of colored lines, at least one of which (probably the brightest) is red. 3. 3.15 m 5. 3.233 × 10 −19 J; 2.018 eV 7. ν = 4.568 × 10 14 s −1; λ = 656.3 nm; Energy mol −1 = 1.823 × 10 5 J mol −1; red 9.

  21. AP CHEMISTRY

    AP Chemistry Virtual Lessons from the College Board. AP Chemistry: 1.1-1.4 Moles, Mass Spectrometry, Elemental Composition, and Mixtures. AP Chemistry: 1.5-1.8 Atomic Structure, Electron Configuration, Spectroscopy, Periodic Trends. AP Chemistry: 2.1-2.4 Chemical Bonds, IMF, and Structure of Solids (WARNING - 1ST 30 SECONDS IS AN APRIL FOOLS JOKE)

  22. 5.3 Chemistry Flashcards

    Speed of lights is a constant that can be obtained by dividing the frequency of light by its wavelength. NT. Amplitude of a wave is the distance between the crest. NT. Energy of a body can change only in small discrete units. AT. Position and velocity of an electron in an atom can be determined with great certainty. NT.

  23. P3 Unit 5.3 Concentration Changes Over Time.docx

    Topic 5.3 Worksheet 1. Complete the table below. Paula Order? first zero second shallow curve line is. ... Topic 5.7, 5.8, 5.9 (Answer Key) Reaction Mechanisms, Reaction Mechanism and Rate Law, Steady-State ... Complete the table using the AP Chemistry Equations and Constants Sheet Michael Order of Reaction 0 1 2 Integrated Rate Law Equation ...