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Student
Name

Mohammed Alnaimi

Student ID 48408
Lesson Oxidation-Reduction Activity Series
Institution Ocean County College
Session 2019L3 CHEM 182 DL1
Course CHEM 182 DL1
Instructor Nancy Marashi

Final Report

Exercise 1

CHEM 182 DL1
Oxidation-Reduction Activity Series

Oxidation is the process of being oxidized. Reduction is when a chemical, during a reaction, gains
electrons. The oxidation number is the number of electrons that is either gained or lost by the
element. The oxidation and reduction affect the oxidation number of an element is that when an
element is oxidized or reduced, the reduction number will either increase or decrease

1. Def ine oxidation, reduction, and oxidation number. Describe how oxidation and
reduction af fect the oxidation number of an element.

An oxidizing agent gains electrons and then reduces in the chemical reaction that is going on. The
reducing agent is when oxidation occurs when an element loses electrons during a reaction. A
spectator ion is both a reactant and a product in a chemical reaction.

2. Def ine oxidizing agent, reducing agent, and spectator ion.

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Data Table 1: Redox Reaction of Copper and Silver Nitrate

The new substance that appeared in the test tube during the reaction of copper and silver nitrate
was a silverish metallic looking substance. The chemical formula for the substance would be
Cu + 2AgNO3 = Cu(NO3)2 + 2 Ag. (This is if we assume the substance is silver or Ag.)

3. In the reaction of copper and silver nitrate, a new substance appeared in the test
tube. Describe the physical appearance of the substance and identif y its chemical
formula.

Copper would be listed above silver. The copper reacted more than the silver during the
experiment. That is why during the experiment the copper was the element that was oxidized was
also the oxidizing agent, whereas, the silver was the element that was reduced and was the
reducing agent.

4. Given an activity series in which the most active metals are at the top of the list and
the least active metals are at the bottom of the list, would copper be listed above silver
or would silver be listed above copper? Support your answer with data f rom Data Table 1.

The chemical equation that describes the reaction is: CuS (s) + 2AgNO3(aq) –> 2Ag2S (s) +
Cu(NO3)2 (aq). The oxidation number of each element, in order, are: (+2 -2), (+1 +5 -2), (+1 -2),
and (+2 +5 -2). This is a non-redox reaction.

5. Solid copper sulf ide and silver nitrate react to form copper (II) nitrate and solid silver
sulf ide. Write a balanced chemical equation that describes the reaction. Identif y the
oxidation number of each element in the reaction. (You do not need to include the total
contribution of charge.) Is this reaction a redox reaction or a non-redox reaction?
Explain your answer.

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Photo 1: Chemical Equation for Redox of Copper and Silver Nitrate. Note: Copper
has a +2 oxidation number in the products.Silver has its expected oxidation
number on the reactons side.

Initial
Observations
before
Beginning

Observations

Observations
after 30 min

Element that is
Oxidized

Element that is
Reduced

Spectator Ion

Oxidiz ing Agent

Reducing Agent

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Exercise 2

Metals: Cu, Pb, and Zn. Oxidation # – Pure: 0, 0, and 0. Oxidation # –
Compound: +2, +2, and +2.

1. List each of the metals tested in Exercise 2. Indicate the oxidation number when each
element is pure and the oxidation number when each element is in a compound.

The metal that was the strongest oxidizing agent was copper. I don’t think copper is the reducing
agent because it is more so the oxidizing agent during the reactions.

2. Which of the metals in Exercise 2 was the strongest oxidizing agent? Was there an
instance when this metal also acted as a reducing agent? Explain your answer using data
f rom Data Table 3.

The strongest reducing agent was zinc. There weren’t any instances when the metal also acted as
an oxidizing agent. The oxidization was done more by the copper.

3. Which of the metals in Exercise 2 was the strongest reducing agent? Was there an
instance when this metal also acted as an oxidizing agent? Explain your answer using
data f rom Data Table 3.

The ease of oxidation correlates with the activity because the more active, the easier it is to
oxidize. The highly active metals tend to donate electrons to other metals.

4. How does ease of oxidation correlate with activity? Do highly active metals tend to
donate electrons or accept electrons f rom other metals?

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Data Table 2: Redox Reactions of Copper, Lead, and Zinc

The most active metal at the top of the list would be Zn, the second would be Pb, and the third Cu.

5. Create an activity series for copper, lead, and zinc. Place the most active metal at the
top of the list.

Solid Metal Well ID

Cu A1

Cu A2

Pb B1

Pb B2

Zn C1

Zn C2

Solid Metal Solution

Cu Pb(NO )

Cu Zn(NO )

Pb CuSO

Pb Zn(NO )

Zn CuSO

Zn Pb(NO )

Solid Metal Immediate Observation

Cu

Cu

Pb

3 2

3 2

4

3 2

4

3 2

The liquid is clear while
the copper is bronze in
color.

The liquid is clear while
the copper is bronze in
color.

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Data Table 3: Potential Redox Reactions and Chemical Equations

Pb

Zn

Zn

Solid Metal 30 Minute Observation

Cu

Cu

Pb

Pb

Zn

Zn

There are a few
bubbles that form
around the lead, which
turns bronze in color.

The lead is silver in
color.

The z inc turned reddish
from the top.

The z inc turns black.

There was no change.

There was no change.

The lead starts to rust.

There was no change.

The z inc was black with
a little bit of red on the
top.

The z inc becomes dark
grey from the top.

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Photo 2: Chemical Equations and Redox Numbers for Reactions

Metal and Metallic Solution Reaction Occurred?

Cu + Pb(NO )

Cu + Zn(NO )

Pb + CuSO

Pb + Zn(NO )

Zn + CuSO

Zn + Pb(NO )

3 2

3 2

4

3 2

4

3 2

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