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Appendix III. Nomenclature of inorganic compounds: the rules

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Inorganic Chemistry
This chapter is in the book Inorganic Chemistry
Appendix IIINomenclature of inorganic compounds: the rulesIntroductionThe standards of nomenclature in chemistry are the rules published by theInternational Union of Pure and Applied Chemistry (IUPAC) from time to time.Based on these rules, the universal adoption of an agreed chemical nomenclature is akey tool for communication in the chemical sciences, computer-based searching indatabases and regulatory purposes, such as those associated with health and safetyor commercial activity. The IUPAC provides recommendations on the nature and useof chemical nomenclature which are freely available at http://www.iupac.org-/publications/pac/ and http://www.chem.qmul.ac.uk/iupac/. An overall summary of chem-ical nomenclature can be found inPrinciples of Chemical Nomenclature(Leigh 2011).Further details can be found inNomenclature of Inorganic Chemistry, colloquiallyknown asThe Red Book(Connelly et al. 2005).It should be noted that many compounds may have non-systematic or semi-systematic names (some of which are not accepted by IUPAC for several reasons)and IUPAC rules allow more than one systematic name in many cases. IUPAC isworking towards identification of single names which are to be preferred for regula-tory purposes.In this appendix, the nomenclature types described are applicable to com-pounds, molecules and ions that do not contain carbon, and to many structuresthat do contain carbon.(i) Atomic symbols, mass, atomic number and so on of elementsThe approved symbols and names of the elements are given in Appendix I. Theatomic number, mass number, number of atoms and atomic charges are to be repre-sented as follows:Mass number:Left upper indexAtomic number: Left lower indexNumber of atoms: Right lower indexIonic charge:Right upper indexFor example,20080Hg22+represents the doubly charged ion containing two mercuryatoms each of which has mass number 200 and atomic number 80. The charge is tobe written as Hg22+, not Hg2+2.https://doi.org/10.1515/9783110727289-013
© 2021 Walter de Gruyter GmbH, Berlin/Munich/Boston

Appendix IIINomenclature of inorganic compounds: the rulesIntroductionThe standards of nomenclature in chemistry are the rules published by theInternational Union of Pure and Applied Chemistry (IUPAC) from time to time.Based on these rules, the universal adoption of an agreed chemical nomenclature is akey tool for communication in the chemical sciences, computer-based searching indatabases and regulatory purposes, such as those associated with health and safetyor commercial activity. The IUPAC provides recommendations on the nature and useof chemical nomenclature which are freely available at http://www.iupac.org-/publications/pac/ and http://www.chem.qmul.ac.uk/iupac/. An overall summary of chem-ical nomenclature can be found inPrinciples of Chemical Nomenclature(Leigh 2011).Further details can be found inNomenclature of Inorganic Chemistry, colloquiallyknown asThe Red Book(Connelly et al. 2005).It should be noted that many compounds may have non-systematic or semi-systematic names (some of which are not accepted by IUPAC for several reasons)and IUPAC rules allow more than one systematic name in many cases. IUPAC isworking towards identification of single names which are to be preferred for regula-tory purposes.In this appendix, the nomenclature types described are applicable to com-pounds, molecules and ions that do not contain carbon, and to many structuresthat do contain carbon.(i) Atomic symbols, mass, atomic number and so on of elementsThe approved symbols and names of the elements are given in Appendix I. Theatomic number, mass number, number of atoms and atomic charges are to be repre-sented as follows:Mass number:Left upper indexAtomic number: Left lower indexNumber of atoms: Right lower indexIonic charge:Right upper indexFor example,20080Hg22+represents the doubly charged ion containing two mercuryatoms each of which has mass number 200 and atomic number 80. The charge is tobe written as Hg22+, not Hg2+2.https://doi.org/10.1515/9783110727289-013
© 2021 Walter de Gruyter GmbH, Berlin/Munich/Boston

Chapters in this book

  1. Frontmatter I
  2. Preface VII
  3. Contents IX
  4. Chapter I. Valence shell electron pair repulsion (VSEPR) theory: principles and applications 1
  5. Chapter II. Delocalized π-bonding in polyatomic molecules: molecular orbital approach 27
  6. Chapter III. Chemistry of borane and related compounds: structure, bonding and topology 71
  7. Chapter IV. Synthesis and reactivity of metal clusters, and their bonding based on molecular orbital approach 117
  8. Chapter V. Stability constants of metal complexes: some aspects 137
  9. Chapter VI. Principles of magnetochemistry and its multiple applications in coordination compounds 173
  10. Chapter VII. Mechanism of inorganic reactions: a study of metal complexes in solution 261
  11. Chapter VIII. Bonding in transition metal complexes: molecular orbital theory approach 349
  12. Chapter IX. Bonding in organometallic sandwich compounds: molecular orbital theory approach 409
  13. Chapter X. Some aspects of safe and economical inorganic experiments at UG and PG levels 451
  14. Appendix I. Some aspects of modern periodic table 563
  15. Appendix II. Units, fundamental physical constants and conversions 577
  16. Appendix III. Nomenclature of inorganic compounds: the rules 583
  17. Appendix IV. Symmetry operations and point groups in molecules 605
  18. Appendix V. Prediction of infrared and Raman active modes in molecules belonging to icosahedral (Ih) point group 625
  19. Bibliography 637
  20. Index 641
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https://doi.org/10.1515/9783110727289-013

Chapters in this book

  1. Frontmatter I
  2. Preface VII
  3. Contents IX
  4. Chapter I. Valence shell electron pair repulsion (VSEPR) theory: principles and applications 1
  5. Chapter II. Delocalized π-bonding in polyatomic molecules: molecular orbital approach 27
  6. Chapter III. Chemistry of borane and related compounds: structure, bonding and topology 71
  7. Chapter IV. Synthesis and reactivity of metal clusters, and their bonding based on molecular orbital approach 117
  8. Chapter V. Stability constants of metal complexes: some aspects 137
  9. Chapter VI. Principles of magnetochemistry and its multiple applications in coordination compounds 173
  10. Chapter VII. Mechanism of inorganic reactions: a study of metal complexes in solution 261
  11. Chapter VIII. Bonding in transition metal complexes: molecular orbital theory approach 349
  12. Chapter IX. Bonding in organometallic sandwich compounds: molecular orbital theory approach 409
  13. Chapter X. Some aspects of safe and economical inorganic experiments at UG and PG levels 451
  14. Appendix I. Some aspects of modern periodic table 563
  15. Appendix II. Units, fundamental physical constants and conversions 577
  16. Appendix III. Nomenclature of inorganic compounds: the rules 583
  17. Appendix IV. Symmetry operations and point groups in molecules 605
  18. Appendix V. Prediction of infrared and Raman active modes in molecules belonging to icosahedral (Ih) point group 625
  19. Bibliography 637
  20. Index 641
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