Writing chemical reactions in general and inorganic chemistry is not a trivial task. However, writing reactions for chemical processes correctly is a clear indicator of proficiency and competence in a subject. Unfortunately, very few students grasp the concept of the correct writing of chemical reactions quickly, and so are unable to move through topics of general, analytical, and inorganic chemistry freely. Because the ability to write and balance different types of chemical reactions is a fundamental issue, this becomes a key question of chemical literacy. The successful writing of chemical reactions includes two components: the prediction of products of these reactions and their possible variations, and balancing these reactions providing a material balance between starting compounds and reactions’ products. This book explores that element of the teaching of the fundamentals of chemical literacy: writing complete equations of chemical reactions and balancing them. It contains 49 figures, 22 schemes and 12 tables, and 93 problems (with answers). This book will be very useful for high school students interested in chemical sciences, higher education teachers, students in colleges and universities majoring in chemistry and biochemistry, and chemistry professional working in industry. It also contains information about properties of the most common elements and applications of a variety of their chemical compounds.
Author(s): Gerasimchuk N.
Publisher: Cambridge Scholars Publishing
Year: 2022
Language: English
Pages: 271
City: Newcastle upon Tyne
Cover
Half Title
Chemical Literacy and Writing Chemical Reactions
Copyright
Contents
Preface
1. Periodic Table as basis for understanding of chemical properties of elements
2. Types of chemical reactions
3. Directions of chemical reactions
3.1. Reactions in solutions: ionic equations
3.2. Solubility of species
3.3. Common volatile compounds as reaction products
Citations
Part 1. Acid-base reactions
4. Main classes of inorganic compounds
4.1. Oxides
4.1.1. Salt-forming oxides
4.1.2. Methods of obtaining oxides
4.1.3. Non-salt-forming oxides
4.1.4. Natural occurrence of oxides
4.1.5. Practicality of oxides
4.1.6. Other binary compounds
4.2. Hydroxides
4.2.1. Methods of obtaining of bases
4.2.2. Natural occurrence of hydroxides
4.2.3. Aspects of practical uses of bases
4.3. Acids
4.3.1. Oxo-acids
4.3.2. Practical applications of acids
4.3.3. Other inorganic acids
4.4. Amphoteric species
4.5. Salts
4.5.1. Chemical properties of normal salts
4.5.2. Basic salts
4.5.3. Oxo-salts
4.5.4. Acid salts
4.5.5. Mixed and double salts
4.5.6. Complex salts
4.5.7. Natural occurrence of normal salts
4.5.8. Practical applications of some normal salts
5. Practice problems for writing and balancing acids-bases reactions
5.1. Identification of classes of compounds and their properties
5.2. Reactions of oxides and hydroxides (bases and acids)
5.3. Formation and reactions of salts
5.4. Hydrolysis
Cited Literature
Figure I-XIII
Figure I. Representative images of some minerals oxides that are used for metals recovery
Figure II. Pictures of samples of several non-metallic oxides and quartz
Figure III. Photographs of hydroxide minerals: bases, basic salts and acid
Figure IV. Representative images of normal salts as minerals
Figure V. Precipitation reactions: A – C insoluble hydroxides; D - G – insoluble salts
Figure VII. Single displacement reaction: Fe + CuCl2 = FeCl2 + Cu ↓
Figure VIII. Decomposition reactions: A – oxide to metal, and B – “chemical volcano” result of ignition of ammonium dichromate
Figure IX. Combustion reactions: burning of phosphorous (A) and sulfur (B) in oxygen gas in dark
Figure XI. Reduction of orange dichromate with sodium sulfite at acidic condition to green Cr(III)
Figure XIII. Displacement of I2 by bubbling gaseous Cl2 in KI solution.
Part 2. Redox reactions
6. Fundamentals of reduction and oxidation
6.1 The concept of losing and gaining electrons in chemical reactions
6.2. Types of redox reactions
6.3. Activity of metals series
7. Quantitative aspects of redox reactions: the Nernst equation
8. Pictorial representation of redox properties of elements: Frost diagrams
9. Qualitative aspects of redox reactions: common reducers and their reactions
I. Electric current at cathode (negatively charged electrode)
II. Hydrides of Li, Na, Ca, NaBH4 and LiAlH4
III. Active metals such as Li, Na, K, Rb, Cs, Ba, Ca
IV. Molecular hydrogen
V. Electron-rich nonmetals in the following monoatomic anions
VI. Other metals (Zn, Al, Fe, Mg, etc.)
VII. Non-metals in intermediate oxidation states in anions
10. Qualitative aspects of redox reactions: common oxidizers and their reactions
I. Electric current at anode (positively charged electrode)
II. Free halogens: F2, Cl2, Br2, I2
III. Ozone and oxygen
IV. Other oxygen-containing species: superoxide and peroxides
V. Nitric acid, HNO3
VI. Metals in high positive oxidation state
VII. Non-metals in high positive oxidation states
11. The role of solutions’ media on the outcome of redox reactions: effect of bases and acids
12. Other factors that affect redox reactions
13. Strategy for prediction of products of redox reactions and worked-out examples
Reaction 1
Reaction 2
Reaction 3
Reaction 4
14. Introductory general problems for practice of writing redox reactions
15. Some specific selected redox reactions for main group chemical elements in the Periodic Table
15.1. Groups I and II
15.2. Group III: B, Al
15.3. Group IV: C, Si, Sn and Pb
15.3.1. Problems for practice on group IV elements
15.4. Chemistry of pnictogens (N, P, As)
Thermal decomposition of ammonium salts
Reactions of pnictogens with other elements
Redox active oxo-compounds of nitrogen
Thermal decomposition of nitrates
Other reactions involving P and As
15.4.1. Practice exercises on redox chemistry of pnictogens
15.5. Chemistry of chalcogens (O, S, Se)
15.5.1. Problems for practice on redox chemistry of group VI elements
15.6 Chemistry of halogens (F, Cl, Br, I)
15.6.1. Practice exercises on redox chemistry of halogens
16. Some selected redox reactions for 3d transition metals series
16.1. Titanium
16.2. Vanadium
16.3. Chromium
16.4. Manganese
16.5. Iron
16.6. Cobalt
16.7. Nickel
16.8. Copper
17. Combined exercises on both types of chemical reactions: acid/base and redox
Chemistry of C
Chemistry of Si
Chemistry of N
Chemistry of P
Chemistry of O
Chemistry of S
Chemistry of F
Chemistry of Cl
Chemistry of Br
Chemistry of I
Chemistry of 3d-transition metals
Chemistry of Mn
Chemistry of Ni
Chemistry of Fe
Chemistry of Cu
Chemistry of Co
Chemistry of Cr
Cited literature
Acknowledgement
Answers to practice problems
5.1. Basic concepts
5.2. Reactions of oxides and hydroxides (bases and acids)
5.3. Formation and reactions of salts
5.4. Hydrolysis
11. Introductory general problems for practice of writing redox reactions
12.3.1. Problems for practice on group IV elements
12.4.1. Practice exercises on redox chemistry of pnictogens
12.5.1. Problems for practice on redox chemistry of group VI elements
12.6.1. Practice exercises on redox chemistry of halogens
14. Combined exercises on both types of chemical reactions: acid/base and redox
Chemistry of C
Chemistry of Si
Chemistry of N
Chemistry of P
Chemistry of O
Chemistry of S
Chemistry of F
Chemistry of Cl
Chemistry of Br
Chemistry of I
Chemistry of 3d-transition metals
Chemistry of Mn
Chemistry of Ni
Chemistry of Fe
Chemistry of Cu
Chemistry of Co
Chemistry of Cr
