6. Chemical Quantities & Aqueous Reactions

Calculate Oxidation Numbers

How to Calculate the Oxidation State of Transition Metals in Coordination Compounds

Assign oxidation numbers to each element in the following compounds. 
(b) SO3

 The electrons lost in the oxidation must equal the electrons gained in the reduction. 

 can happen only in the presence of reduction. 

 Both the first and second statements are correct. 

 Both the first and third statements are correct. 

 Correct!  Both processes occur simultaneously. 

Assign oxidation numbers to each element in the following compounds.
(b) CuSO4

How to calculate oxidation numbers - Basic Introduction - Dr K

Assign oxidation numbers to each element in the following compounds. 
(c) CH2O

Assign oxidation numbers to each atom in Borax, Na2B4O7, a mineral used in laundry detergent. (LO 4.18)

How to calculate Oxidation Number or Oxidation State? Easy Trick

Aqueous solutions of ammonia 1NH32 and bleach (active
ingredient NaOCl) are sold as cleaning fluids, but bottles
of both of them warn: “Never mix ammonia and bleach, as
toxic gases may be produced.” One of the toxic gases that
can be produced is chloroamine, NH2Cl. 
(b) What is the 
oxidation number of chlorine in chloramine?

What is the oxidation state of Cl in each ion?
a. ClO-
b. ClO2- 
c. ClO3-
d. ClO4-

Assign oxidation numbers to each element in the following compounds. 
(c) COCl

Determine the oxidation number for the indicated element
in each of the following substances: (e) Pt in PtCl4

Assign oxidation numbers to each element in the following compounds. 
(d) CH2Cl2

Assigning Oxidation Numbers - Chemistry Tutorial

Assign oxidation numbers to each element in the following compounds.
(d) Mn2O7

Assign oxidation numbers to each element in the following ions. 
(e) BrO-

Assign oxidation numbers to each element in the following compounds. 
(a) NO2

Oxidation number of monoatomic ions equals to their charge.

Assign oxidation numbers to each element in the following ions. 
(d) MnO4 2-

Indicate whether the following balanced equations involve
oxidation–reduction. If they do, identify the elements that
undergo changes in oxidation number.
(a) 2 AgNO31aq2 + CoCl21aq2 ¡ 2 AgCl1s2 +
Co1NO3221aq2

How to Find Oxidation Numbers  (Rules and Examples)

Assign oxidation numbers to each element in the following compounds.
(a) VOCl3

Assign oxidation numbers to each element in the following ions. 
(c) C2O4 2-

Assign oxidation numbers to each element in the following compounds. 
(e) OsO4

Calculate Oxidation Numbers Example 4

Determine the oxidation number for the indicated element in 
each of the following substances: (c) P in AgPF6

Calculate Oxidation Numbers Example 2

Disulfides are compounds that have S ¬ S bonds, like peroxides have O ¬ O bonds. Thiols are organic compounds
that have the general formula R ¬ SH, where R is a generic
hydrocarbon. The SH- ion is the sulfur counterpart of
hydroxide, OH-. Two thiols can react to make a disulfide,
R ¬ S ¬ S ¬ R.
(b) What is the oxidation state of sulfur in a disulfide?

Calculating Oxidation Numbers

Determine the oxidation number for the indicated element in
each of the following substances: (a) S in SO3

Indicate whether the following balanced equations involve
oxidation–reduction. If they do, identify the elements that
undergo changes in oxidation number.
(a) PBr31l2 + 3 H2O1l2 ¡ H3PO31aq2 + 3 HBr1aq2

What is the oxidation state of Cr in each compound?
b. CrO3

Assign oxidation numbers to each element in the following ions.
(c) NO3-

Determine the oxidation number for the indicated element in 
each of the following substances: (d) N in HNO3

Assign oxidation numbers to each element in the following ions. 
(b) SO3

Assign oxidation numbers to each element in the following compounds. 
(e) KClO3

Assign oxidation numbers to each element in the following ions. 
(d) NO2-

What is the oxidation state of Cr in each compound?
c. Cr2O3

Assign oxidation states to each atom in each element, ion, or
compound.
Cl2, Fe3+, CuCl2, CH4, Cr2O720, HSO4-

Magnesium, the element, is produced commercially by
electrolysis from a molten salt (the “electrolyte”) using a
cell similar to the one shown here. (a) What is the most
common oxidation number for Mg when it is part of a salt?

Iron corrodes to produce rust, Fe2O3, but other corrosion
products that can form are Fe(O)(OH), iron oxyhydroxide,
and magnetite, Fe3O4. (a) What is the oxidation number
of Fe in iron oxyhydroxide, assuming oxygen’s oxidation
number is - 2?

Calculating Oxidation Number

Indicate whether the following balanced equations involve
oxidation–reduction. If they do, identify the elements that
undergo changes in oxidation number.
(b) NaI1aq2 + 3 HOCl1aq2 ¡ NaIO31aq2 + 3 HCl1aq2

Assign oxidation numbers to each element in the following compounds. 
(f) HNO3

For each of the following balanced oxidation–reduction
reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total
number of electrons transferred in each reaction.
(b) 2 Hg2+1aq2 + N2H41aq2 ¡ 2 Hg1l2 + N21g2 + 4 H+1aq2

Specific rules exist for calculating oxidation numbers of group 1A and 2A elements, F, H, O and Halogens.

Nitrogen can have several different oxidation numbers ranging in value from -3 to +5.
(a) Write the formula and give the name of the nitrogen oxide compound in which nitrogen has an oxidation number of +1, +2, +4, and +5.

Calculate Oxidation Numbers Example 3

Determine the oxidation number of sulfur in each of the following 
substances: (b) sulfurous acid, H2SO3

Assign oxidation numbers to each element in the following ions. 
(b) S2O3 2-

Elements in group 17 in the periodic table are called the halogens;
elements in group 16 are called the chalcogens. (a)
What is the most common oxidation state of the chalcogens
compared to the halogens?

Assign oxidation numbers to each element in the following ions.
(a) Cr(OH)4-

Calculate Oxidation Numbers Example 1

Determine the oxidation number for the indicated element
in each of the following substances: (f) Cl in NaClO4.

Determine the oxidation number of sulfur in each of the following 
substances: (f) Which region(s) of the periodic table 
contains elements that can adopt both positive and negative 
oxidation numbers?

Elements in Natural State have an oxidation number of zero:H2, N2, O2, F2, P4, S8, Cl2, Se8, Br2.

Assign oxidation numbers to each element in the following ions.
(a) ClO3-

Phosphorus can have several different oxidation numbers ranging in value from -3 to +5.
(a) When phosphorus burns in air or oxygen, it yields either tetraphosphorus hexoxide or tetraphosphorus decoxide. Write the formula and give the oxidation number for each compound.

The substances NaF and CaO are isoelectronic (have the 
same number of valence electrons). (a) What are the charges 
on each of the cations in each compound?

Nitrogen can have several different oxidation numbers ranging in value from -3 to +5.
(b) Based on oxidation numbers, which nitrogen oxide from part (a) cannot react with molecular oxygen?

For each of the following balanced oxidation–reduction
reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total
number of electrons transferred in each reaction.
(a) 2 MnO4-1aq2 + 3 S2 - 1aq2 + 4 H2O1l2 ¡ 3 S1s2 +
2 MnO21s2 + 8 OH-1aq2

How to Calculate Oxidation Number Practice Problems

Copper corrodes to cuprous oxide, Cu2O, or cupric oxide,
CuO, depending on environmental conditions. (a) What is
the oxidation state of copper in cuprous oxide?

Assign oxidation states to each atom in each element, ion, or
compound.
Ag, Ca2+, BaO, H2S, NO3-, CrO42-

Which of the following elements would have the lowest oxidation number?

 There is another compound with a larger positive oxidation number for nitrogen. 

 Correct, the oxidation number of nitrogen in this compound is +5. 

 Review the rules for determining oxidation numbers. 

 In which of the following does nitrogen have the largest positive value for its oxidation number? 

Determine the oxidation number of sulfur in each of the following
substances: (d) hydrogen sulfide, H2S

Assign oxidation numbers to each element in the following ions. 
(f) V2O7 4-

What is the oxidation state of Cr in each compound?
a. CrO

Assign oxidation numbers to each element in the following compounds. 
(f) H2PtCl6

Assign oxidation numbers to each element in the following ions. 
(e) HPO4 2-

Phosphorus can have several different oxidation numbers ranging in value from -3 to +5.
(b) Based on oxidation numbers, which phosphorus oxide compound from part (a) was formed by combustion with a limited supply of oxygen?

Assign oxidation numbers to each element in the following ions. 
(f) AsO4 3-

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

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

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.

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

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.