lOMoAR cPSD| 19857451
CHEM 120 INTRODUCTION TO GENERAL,
ORGANIC & BIOLOGICAL CHEMISTRY WITH
LAB EXAM 3 STUDY REVIEW CHAMBERLAIN
COLLEGE
, CHEM120 Exam 3 Review
Reduction/Oxidation (Redox Chemistry)
LEO the lion goes GER
Oxidation: Loss of Electrons is Oxidation (LEO)
Reduction: Gaining of Electrons is Reduction (GER)
Are each of the following oxidized or reduced?
Fe2+ → Fe0 Fe is reduced as the charge is becoming more negative (meaning that the Fe gained e-)
O2- → O0 O is being oxidized as the charge is becoming more positive (loosing e-)
Cu+1 → Cu2+ Cu is being oxidized as the charge is becoming more positive (loosing e-)
Agents
Oxidizing agent: Contains the species being reduced. Oxidizes another species in the reaction by
accepting electrons (becoming reduced in the process).
Reducing agent: Contains the species being oxidized. Reduces another species in the reaction by
donating electrons (becoming oxidized in the process).
What is the oxidizing agent in this redox reaction? Cu2+ + Zn0 → Cu0 + Zn2+
Answer:
Cu2+ is the oxidizing agent as this species accepted electrons from the Zn0, and in the processes, became
reduced. In other words, the Cu2+ oxidized the Zn0.
What is the reducing agent in this redox reaction: V4+ + Cu+ → Cu+5 + V0
Answer:
Cu+ is the reducing agent, as this species donated electrons to the V4+, and in the process, became
oxidized. In other words, the Cu+ reduced the V4+.
Assigning Oxidation Numbers
What are the oxidation numbers on: 2 H2 + O2 → 2 H2O
Answer:
2 H20 + O 20 → 2 H+12O2-
What is the reducing agent for the equation above?
Answer:
H2 is the reducing agent as this species reduced the O from 0 to -2.
CHEM 120 INTRODUCTION TO GENERAL,
ORGANIC & BIOLOGICAL CHEMISTRY WITH
LAB EXAM 3 STUDY REVIEW CHAMBERLAIN
COLLEGE
, CHEM120 Exam 3 Review
Reduction/Oxidation (Redox Chemistry)
LEO the lion goes GER
Oxidation: Loss of Electrons is Oxidation (LEO)
Reduction: Gaining of Electrons is Reduction (GER)
Are each of the following oxidized or reduced?
Fe2+ → Fe0 Fe is reduced as the charge is becoming more negative (meaning that the Fe gained e-)
O2- → O0 O is being oxidized as the charge is becoming more positive (loosing e-)
Cu+1 → Cu2+ Cu is being oxidized as the charge is becoming more positive (loosing e-)
Agents
Oxidizing agent: Contains the species being reduced. Oxidizes another species in the reaction by
accepting electrons (becoming reduced in the process).
Reducing agent: Contains the species being oxidized. Reduces another species in the reaction by
donating electrons (becoming oxidized in the process).
What is the oxidizing agent in this redox reaction? Cu2+ + Zn0 → Cu0 + Zn2+
Answer:
Cu2+ is the oxidizing agent as this species accepted electrons from the Zn0, and in the processes, became
reduced. In other words, the Cu2+ oxidized the Zn0.
What is the reducing agent in this redox reaction: V4+ + Cu+ → Cu+5 + V0
Answer:
Cu+ is the reducing agent, as this species donated electrons to the V4+, and in the process, became
oxidized. In other words, the Cu+ reduced the V4+.
Assigning Oxidation Numbers
What are the oxidation numbers on: 2 H2 + O2 → 2 H2O
Answer:
2 H20 + O 20 → 2 H+12O2-
What is the reducing agent for the equation above?
Answer:
H2 is the reducing agent as this species reduced the O from 0 to -2.
