Chemistry 30

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Redox Reactions & Electrochemistry

Assignment 1: Redox Reactions - Oxidation Numbers

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1. Define oxidation and reduction.
2. Determine the oxidation number of nitrogen in each of the following compounds:
  a. NH3
  b. NO2
  c. Ca3N2
  d. NI3
3. Determine the oxidation numbers of the requested element in the following compounds:
  a. S in SO2
  b. Mn in MnO2
  c. Cr in Cr3+
  d. S in SO42-
  e. B in H3BO3
  f. O in Na2O2 (hint: this is a peroxide)
  g. Sn in Sn
  h. Cr in K2Cr2O7
4. Determine the oxidation of each element in (NH4)2CO3
5. The following reactions are not complete reactions. Determine if each of the following changes is an oxidation, a reduction, or neither:
  a. SO32- → SO42-
  b. CaO → Ca
  c. CrO42- → Cr2O72-
  d. 2 I- → I2
6. For each of the following reactions, complete the summary table below the equation. If an element does not undergo any change, leave the last two columns blank. Also provide the formula of the oxidizing or reducing agent. An example is shown.
  a. CuO + H2 → Cu + H2O
   

element

Initial
Ox. No

 

Final
Ox. No.

e - gained or lost

Oxidized or reduced

Oxidizing or
Reducing Agent

Cu

+2

0

gain 2

reduced

oxidizing agent - CuO

O

 

 

 

 

 

H

 

 

 

 

 

  b. CH4 + 2 O2 → CO2 + 2 H2O
   

element

Initial
Ox. No

 

Final
Ox. No.

e - gained
or lost

Oxidized or reduced

Agent

C

 

 

 

 

 

H

 

 

 

 

 

O

 

 

 

 

 

  c. 2 Na + Br2 → 2 NaBr
   

element

Initial
Ox. No

 

Final
Ox. No.

e - gained
or lost

Oxidized or reduced

Agent

Na

 

 

 

 

 

Br

 

 

 

 

 

7. Not all of the following reactions are redox reactions. Place a check mark in the appropriate column for each reaction.
     
Redox

 
Not Redox
  a. Na2S + FeCl2 → 2 NaCl + FeS      
  b. 2 Na + 2 H2O → 2 NaOH + H2      
  c. 2 KClO3 → 2 KCl + 3 O2      
  d. SO2 + H2O → H2SO3      
  e. 2 Al + 6 HCl → 2 AlCl3 + 3 H2      
     
Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 31-May-2006