types of reaction homework answer key

Unit 7 - Chemical Reactions

• Due: March 26/27
• Partial Key - make sure you check your answers! 
• Intervention Review Sessions:  TBA
• Assignment #1 - % composition , Empirical vs. molecular formula , Calculations for EF and MF
• Assign #2 -  Oxidation/ Reduction Reactions

Worksheets & Notes

• Unit 7 PowerPoint Slides
• Language of Chemistry Lab
• Chemical vs. Physical Reactions
• Naming and Formula Writing
• Identifying 5 Types of Rxn + Activity
• Mixed Naming & Formula Writing + Sweet 16 Tournament
• Balancing Chemical Reactions (Online Exploration + Practice WS)
• Writing & Predicting Products of a Reaction
• Unit 7 Study Guide     (key)

Online Practice Tests

Naming & Formulas ( online practice ) (choose scatter/ test/ or space race)

       a)   Writing compound formulas  (in real life, you don't leave charges on the ions)        b)   Practice with Polyatomic Ions        c)   Practice with Colvalent Molecules

Phet Online- Balancing Equations ( click here  for site)

Balancing Chemical Equations (Online practice)

Identifying the reaction type (online practice)

Online practice test  (Entire Unit...skip volume of gas questions)

Interesting Links

• Rising Acidity of the Ocean

Day 1: March 6/9

• Finish  Language of Chemistry Lab
• Review Test and clear ESA's
• Worksheet:  Chemical vs. Physical changes
• Finish wkst: Chemical vs. Physical Changes

Day 2: March 10/11

• Notes: Naming and formula writing 
• Wkst:  Naming and Formula writing
• Online Practice game
• Finish Wkst:   Naming and Formula Writing

Day 3: March 12/13

• Notes: 5 types of Chemical reactions
• Wkst:  Identifying 5 Types of Chemical Reactions
• Activity:  Reaction Types
• Finish Wkst:  Identifying 5 Types of Chemical Reactions

Day 4: March 16/17

• Finish Types of Reactions Activity
• Mixed Naming & Formula Writing
• Naming Relay (if time)
• Sweet 16 Tournament

Day 5: March 18/19

• Online Exploration: Balancing Chemical Equations
• U se Phet online balancing   ( click here  for site)...Use HTML 5 for phones/ chromebooks
• Notes: Balancing
• Practice:  Balancing & Types of Reactions WS
• Intro to Activity Series & Solubility Rules
• Handout  Study Guide
• Finish  Balancing & Types of Reactions WS  (back)
• Study guide Due Tues/ Weds 3/24 & 3/25

Day 6: March 20/23

• Review types of rxn activities 
• Notes/Discussion: Predicting Products
• WS-   Writing, Balancing, & Identifying Chemical Reactions (front)
• Single & Double Replacement Activity 
• Honors lab 
• Unit 7 Study Guide     (Key)

Day 7: March 24/25

• Review study guide  Key
• Unit 7 HW packet

Day 8: March 26/27

• Turn in Homework Packet
• Unit 7 Multiple Choice Test

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4.E: Chemical Reactions and Equations (Exercises)

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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 → ?  
• Na 2 CO 3 + Sr(NO 2 ) 2 → ?
• (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  
• 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)  
• NiCl 3  
• NaH (sodium hydride)
• NO 2 −
• AgNO 3  
• 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 + .

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