1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (e) aluminum metal is added to a solution of 
cobalt(II) sulfate.

Lesson 29 - Activity Series, Part 1 (Chemistry Tutor)

Based on your understanding of activities determine if a reaction occurs and if so provide the products formed.&nbsp;Zn (s) + NiCl2 (aq) →

Write the balanced chemical equation for the reaction of solid
potassium with liquid water.

The most strongly reducing elements are listed at the top of the partial activity series table provided. Use the activity series to predict which reaction will occur. (LO 4.20) 
(a) 
(b) 
(c) 
(d) <img class="fr-dib" src="https://lightcat-files.s3.amazonaws.com/problem_images/d61409dd4f51d14c-1677161864520.jpg" style="width: 174px;">

Activity Series

Reactivity Series of Metals | Environmental | Chemistry | FuseSchool

Assume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (d) chromium metal is immersed in an aqueous 
solution of cobalt(II) chloride

Predicting Products of Single Replacement Reactions

Based on your understanding of activities determine if a reaction occurs and if so provide the products formed.&nbsp;Ba (s) + H2O (g) →

The Activity Series (Explanation & Examples)

Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals 
like this that are solids are called alloys. There is a range 
of compositions over which the solution is considered a 
bronze. Bronzes are stronger and harder than either copper or 
tin alone. (c) Suggest a reaction 
that you could do to remove all the tin from this bronze 
to leave a pure copper sample. Justify your reasoning.

Metal Reactivity Series Menomics

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (a) Nickel metal is added to a solution of copper(II) nitrate

8.3 Activity Series of the Elements

(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:

Determine if HNO3 can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HNO3 and determine the minimum volume of 6.0 M HNO3 required to completely dissolve the sample.
a. 5.90gAu

Nickel metal is added to a solution of copper(ii) nitrate.

The following reactions (note that the arrows are pointing
only one direction) can be used to prepare an activity series
for the halogens:
Br21aq2 + 2 NaI1aq2¡2 NaBr1aq2 + I21aq2
Cl21aq2 + 2 NaBr1aq2¡2 NaCl1aq2 + Br21aq2
(a) Which elemental halogen would you predict is the most
stable, upon mixing with other halides?

Using the activity series (Table 4.5), write balanced chemical
equations for the following reactions. If no reaction occurs,
write NR. (b) zinc metal is added to a solution of magnesium sulfate

Chlorine dioxide gas 1ClO22 is used as a commercial bleaching
agent. It bleaches materials by oxidizing them. In the
course of these reactions, the ClO2 is itself reduced. 
(b) Why do you think that ClO2 is reduced so readily?<img src="https://lightcat-files.s3.amazonaws.com/problem_images/9b350e62cc52767a-1660740626958.jpg" alt="" />

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR.
(a)

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. 
(d)

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. 
(b)

Making Predictions Using Reactivity Series | Reactions | Chemistry | FuseSchool

Suppose you have 3.00 g of powdered zinc metal, 3.00g of
powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate
solution. (a) Which metal will react with the copper(II)
nitrate solution?

Consider the following reagents: zinc, copper, mercury (density
13.6 g/mL), silver nitrate solution, nitric acid solution.
(a) Given a 500-mL Erlenmeyer flask and a balloon, can you
combine two or more of the foregoing reagents to initiate a
chemical reaction that will inflate the balloon? Write a balanced
chemical equation to represent this process. What
is the identity of the substance that inflates the balloon?

Activity Series of Metals and Reaction Prediction

(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

Write balanced molecular and net ionic equations for the
reactions of (d) acetic acid, CH3COOH, with zinc.

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample.
a. 2.15gAl

If the activity of halogens is stated as:Fluorine &gt; Chlorine &gt; Bromine &gt; Iodine, determine if a reaction occurs and if so provide the products formed.&nbsp;Cl2 (g) + AlBr3 (aq) →

The metal cadmium tends to form Cd2+ ions. The following 
observations are made: (i) When a strip of zinc metal is placed 
in CdCl21aq), cadmium metal is deposited on the strip. (ii) 
When a strip of cadmium metal is placed in Ni1NO3221aq), 
nickel metal is deposited on the strip. 
(b) Which elements more closely define the position of cadmium 
in the activity series?

A sample of metal (M) reacted with both steam and aqueous HCl to release H2 but did not react with water at room tem-perature. When 1.000 g of the metal was burned in oxygen, it formed 1.890 g of a metal oxide, M2O3. What is the iden-tity of the metal?

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (e) hydrogen gas is bubbled 
through a solution of silver nitrate.

Chromium metal is immersed in an aqueous solution of cobalt(ii) chloride.

Write the balanced chemical equation for the reaction of solid strontium with iodine gas.

Some metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by
(c) heating its oxide with coke?

Write balanced molecular and net ionic equations for
the reactions of (d) aluminum with formic acid, HCOOH.

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample.
b. 4.85gCu

Write the balanced chemical equation for the reaction of solid
lithium with liquid water.

Activity Series Example 1

Write balanced molecular and net ionic equations for the 
reactions of (b) dilute sulfuric acid with iron

Write the balanced equation for the reaction of hydrogen gas
with bromine gas.

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample.
c. 2.42gAg

Some metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by
(a) finding it in its elemental state?

An unknown metal (M) was found not to react with either water or steam, but its reactivity with aqueous acid was not investigated. When a 1.000 g sample of the metal was burned in oxygen and the resulting metal oxide converted to a metal sulfide, 1.504 g of sulfide was obtained. What is the identity of the metal?

The following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain.
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/0922bbd3a5291d7c-1668708050814.jpg" alt="" />
(b) <img src="" alt="" />
(c) <img src="" alt="" />
(d) <img src="" alt="" />

Using the activity series (Table 4.5), write balanced chemical
equations for the following reactions. If no reaction occurs,
write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate

Based on the positions in the periodic table, which of the following reactions would you expect to occur?
(a) Red+ + Green ---> Red + Green+
(b) Blue + Green+ ---> Blue+ + Green 
(c) Red + Blue+ ---> Red+ + Blue
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/251c89c4b3bbd48b-1668701887644.jpg" alt="" />

Suppose you have 3.00 g of powdered zinc metal, 3.00g of 
powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate 
solution. (d) What is the molarity of Cu2+ ions in the 
resulting solution?

Using the activity series (Table 4.5), write balanced chemical 
equations for the following reactions. If no reaction occurs, 
write NR. (c) hydrobromic acid is added to tin metal

Use the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR.
(c)

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Solutions

Solutions represent homogeneous mixtures made of 2 or more components that form a uniform composition.&nbsp;

Osmolarity

Osmolarity (ionic molarity) represents the number of moles of ions per liter of solution.&nbsp;

Gas Evolution Equations

A Gas Evolution Equation is a molecular equation that involves the creation of specific gases.&nbsp;

Molecular Equations

Molecular Equations show reacting molecules involved in a chemical reaction.&nbsp;

Complete Ionic Equations

Complete Ionic Equations show aqueous compounds as fully dissociated ions.&nbsp;

Solubility Rules

The Solubility Rules are a convenient set of guidelines to help us determine if a compound will be soluble or insoluble.

Molarity

Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.&nbsp;

Electrolytes

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.&nbsp;

Solution Stoichiometry

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Calculate Oxidation Numbers

Calculating Oxidation Numbers is the first pivotal step in understanding redox reactions.&nbsp;

Dilutions

In Dilutions, a solvent (usually water) is added to a concentrated solution.&nbsp;

Redox Reactions

Redox Reactions (oxidation-reduction reactions) involve transference of an electron(s) between reactants.

Activity Series is a list of single displacement reactions in order of reactivity.

Balancing Redox Reactions: Acidic Solutions

Balancing Redox Reactions requires a new approach that accounts for the transfer of electrons between reactants.

Balancing Redox Reactions: Basic Solutions

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.