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General and Bioinorganic Chemistry - GAF390
Title: General and Bioinorganic Chemistry
Guaranteed by: Department of Organic And Bioorganic Chemistry (16-16120)
Faculty: Faculty of Pharmacy in Hradec Králové
Actual: from 2025
Semester: winter
Points: 0
E-Credits: 6
Examination process: winter s.:combined
Hours per week, examination: winter s.:28/20, C+Ex [HS]
Capacity: unlimited / 90 (unknown)
Min. number of students: unlimited
4EU+: no
Virtual mobility / capacity: no
Key competences:  
State of the course: taught
Language: English
Teaching methods: full-time
Level:  
Note: course can be enrolled in outside the study plan
enabled for web enrollment
Guarantor: doc. PharmDr. Jaroslav Roh, Ph.D.
Interchangeability : GAF124
Is co-requisite for: GAF411, GAF299, GAF293
Is interchangeable with: GAF124
Annotation -
General Chemistry is fundamental to understanding other chemical disciplines. The subject deals with atomic structure, the theory of chemical bond, the periodic character of physical and chemical properties of elements and compounds and with the course of chemical reactions. Bioinorganic chemistry gives a systematic survey of chemical elements and their compounds on the basis of the location of the elements in the periodic table; special emphasis is put on biological and pharmaceutical importance.
Last update: Palát Karel, PharmDr., CSc. (27.09.2025)
Course completion requirements -

Requirements for getting the credit:

1. Attendance at all seminars
2. More than 60% of points from the credit tests



Conditions for the examination

 

1. The credit getting shall be the condition for the exam taking. The credit must be got one day before the exam’s taking at the latest.

2. Registration for an examination shall be done electronically through Internet in the Student Information System (SIS). The student may not be registered for more terms of the same exam concurrently.

3. The list of themes for the exam is placed in the study materials on the faculty website.

4. The examination will start in the form of a written test.

5. Students will have 50 minutes for solving the problems.

6. Students will use only a calculator and a pen. It will be strictly forbidden to use a mobile phone during the exam.

7. When student obtains 10 points and more from this part (maximum is 16 points), he or she will continue with the oral part where a student answers two questions – one in General Chemistry and one in Inorganic Chemistry.

8. The list of oral exam questions is placed in the study materials on the faculty website

9. The examiner shall record the result of the examination in the student’s record (Student Information System).

10. The student may take the examination from the registered subject for maximum three times, i.e. he has the right for two corrective dates; an extraordinary corrective date is not allowed.

11. If the student passes the written part and fails in the oral part, the next time he or she will continue only with the oral part.

 

Written exam test:

 

Students will find:

6 questions without given answers – they will obtain 2 points per one correct answer = 12 points

and

4 question with given 4 answers – they will obtain 1 point per correct answer = 4 points.

The maximum amount of points = 16.

 

The successful written examination passing means acquiring more than 10 points.

 

Oral exam questions:

General Chemistry

 

  1. The structure of the atom, atomic nucleus, chemical elements.
  2. Electronic shell of the atom. Models of the atom. The quantum mechanical model of the atom - atomic orbitals, quantum numbers.
  3. Chemical periodicity. Periodic chart of elements. Electron configurations, valence electrons. Atomic parameters – atomic radii, ionization energy, electron affinity, electronegativity, periodicity of these parameters.
  4. Chemical bonding (preconditions of its formation, types of bonding), molecular orbitals. LCAO-MO theory.
  5. Nonpolar and polar covalent bonding, MO diagrams of two-atomic molecules, bond order. Coordinate covalent bonding.
  6. Parameters of the bond - length, energy. Molecular geometry. VSEPR theory.
  7. Valence bond theory. Hybridization - types and examples.
  8. Ionic bonding. Polarizing activity of ions. Metallic bonding. Bond delocalization. Three-center two-electron (3c,2e) bond.
  9. Weak bonding interactions. Hydrogen bond.
  10. Types of chemical formulas, models of molecules.
  11. Chemical reactions, types of chemical reactions, chemical equations, heat of reaction, Gibbs energy, activation energy, catalysis.
  12. Chemical equilibria and their affection, the principle of action and reaction, solubility product constant.
  13. Electrolytic dissociation, electrolytes. Dissociation constant.
  14. Theories of acids and bases (Arrhenius, Brønsted-Lowry, Lewis).
  15. Quantitative evaluation of acids and bases, pH of a solution.
  16. Relationships between the structure and acid-base properties of compounds.
  17. Acid-base reactions. Hydrolysis of salts.
  18. Oxidation-reduction reactions, oxidation number, oxidizing and reducing agents.
  19. Reactions in electrolytic cells. Electromotive series (Activity series) of the elements. Reduction and oxidation potentials. Electrolysis.
  20. Coordination compounds. Basic terms, types of coordination compounds, nomenclature, preparation, properties, importance, usage.

 

Bioinorganic Chemistry

 

  1. Periodic system of elements, chemical periodicity, occurrence, types of elements.
  2. Hydrogen (structure, properties, reactivity, occurrence, production, usage).
  3. Binary compounds of hydrogen.
  4. Noble (inert) gases and their compounds.
  5. Group VIIA (17) – general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage. Hydrogen halides, halides, compounds of halogens and oxygen.
  6. Group VIA (16) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage. Hydrides, hydrogen peroxide.
  7. Compounds of sulfur and oxygen – oxides, acids. Derivatives of sulfur oxoacids (halides, peroxoacids, amides).
  8. Group VA (15) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage.
  9. Compounds of the group VA (15) elements with hydrogen (generally), halogens. Compounds of nitrogen and hydrogen.
  10. Oxides of nitrogen and phosphorus. Oxoacids of nitrogen and phosphorus, their salts, derivatives.
  11. Group IVA (14) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage. Compounds with hydrogen, halogens. Compounds of carbon and oxygen, nitrogen, and/or sulfur.
  12. Compounds of carbon and silicon with oxygen, organosilicon compounds.
  13. Group IIIA (13) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage. Compounds with hydrogen, halogens, nitrogen, and oxygen.
  14. Group IIA (2) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage, compounds (hydrides, oxides, hydroxides, halides, oxo salts, organometallic compounds, complexes).
  15. Group IA (1) - general characteristic, physical properties, reactivity, occurrence, production, biological importance, usage, compounds (hydrides, oxides, hydroxides, halides, oxo salts).
  16. Groups IIIB, IVB, and VB (3, 4, 5), lanthanoids, actinoids – general characteristics of groups, elements and their compounds.
  17. Groups VIB, and VIIB (6,7) - general characteristics of groups, elements and their compounds.
  18. Group VIIIB (8, 9, 10) – general characteristic, elements and their compounds.
  19. Group IB (11) – general characteristic of the group, elements and their compounds.
  20. Group IIB (12) – general characteristic of the group, elements and their compounds.

 

 

Last update: Palát Karel, PharmDr., CSc. (27.09.2025)
Literature -

Recommended:

  • 1. G.W. Daub, W.S. Seese: Basic Chemistry, 7th ed., Prentice Hall, Upper Saddle River, 1996

    2. D.D. Ebbing, S.D. Gammon: General Chemistry, Houghton Mifflin Company, Boston 2009.

    3. J.E. House, K.A. House: Descriptive Inorganic Chemistry, Elsevier, San Diego 2010

    4. G. Rayner-Canham, T. Overton: Descriptive Inorganic Chemistry, W. H. Freeman and Company, New York 2010

    5. P.W. Atkins, T.L. Overton, J.P. Rourke, M.T. Weller, F.A. Armstrong: Shriver and Atkins Inorganic Chemistry, 5th ed., W. H. Freeman and Company, New York 2010.

    6. Connelly N.G., Gamhus T., Hartshorn R.M., Hutton A.T.: Nomenclature of Inorganic Chemistry. IUPAC Recommendations 2005. RSC Publishing, Cambridge 2005

    7. R. M. Hartshorn, K.-H. Hellwich, A. Yerin, T. Damhus), A. T. Hutton: Brief Guide to the Nomenclature of Inorganic Chemistry. IUPAC, Pure Appl. Chem. Doi: 10.1515/pac-2014-0718.

    . . : , , s. ISBN .

Last update: prepocet_literatura.php (14.08.2025)
Syllabus -

Lectures:

 

General chemistry

1. Basic terms and categories

1.1 the subject and development of chemistry, its differentiation, interdisciplinary relations. Chemistry in the study of pharmacy

1.2 matter, field, motion and its forms, compounds, elements

1.3 basic empirical chemical laws, chemical notation, basic terms concerning elements and compounds

1.4 nomenclature of inorganic compounds

 

2. Atomic theory

2.1 development of atomic theory

2.2 contemporary atomic theory, subatomic particles, arrangement of electrons, protons, and neutrons, atomic models)

2.3 atomic nucleus (proton number, nucleon number, nuclides, natural and artificial radioactivity, physical, chemical, and biological effects of nuclear radiation, applications of radioactive nuclides to pharmacy and medicine)

2.4 arrangement of electrons (Bohr's atomic model, dualistic nature of electron, the quantum mechanical model of the atom)

 

3. Theory of chemical bonding

3.1 ionic relation (origin of ions, ionisation energy, electronic affinity, structure of ionic compounds)

3.2 the covalent bond (theory of valence bonds, theory of molecular orbitals, hybridization of atomic orbitals, orientation of bonds in space, bond order, bond energy, polarity of covalent bonds, dipole moment, donor-acceptor bond)

3.3 metallic bond

3.4 weak (non-)bonding interactions (hydrogen bridge, van der Waals forces)

3.5 molecular structure and shape– valence bond (VB) theory (hybridization of orbitals), valence shell electron pair repulsion (VSEPR) theory

 

4 Dispersion systems

4.1 basic terms, classification, importance for pharmaceutical sciences and practice

4.2 solutions (preparation, properties of solutions, importance in biology and pharmacy)

4.3 ionisation in solutions

4.4 acids and bases (theories of acids and bases, relations between structure and acid-basic properties of compounds)

4.5 ionic product of water, pH

4.6 protolytic reactions

4.7 solubility product constant

 

5 Chemical reactions and their intercourse

5.1 reaction kinetics and thermodynamics

5.2 oxidation-reduction reactions

5.3 electrochemistry

 

6. Co-ordination compounds

6.1  basic terms

6.2 co-ordinate theory, Werner's approach, contemporary theory

6.3 types of co-ordination compounds, stereochemistry of co-ordination compounds

6.4 bioinorganic, pharmaceutical, medical, and selected technological aspects of chemistry of co-ordination compounds

6.5 nomenclature of co-ordination compounds

 

7. The periodic law and the periodic table of elements

7.1 classification of elements, importance of D. M. Mendeleev's periodic law

7.2 the periodic table of elements

7.3 the periodic law  and the periodic table in relation to contemporary atomic theory

 

Bioinorganic chemistry

 

8. Chemistry of s- and p- elements and their  compounds with regard to the biological and pharmaceutico-medical aspects

8.1 hydrogen, water

8.2 the noble gases

8.3 the alkali metals

8.4 the alkaline earth metals

8.5 the boron group

8.6 the carbon group

8.7 the nitrogen group

8.8 the chalcogens

8.9 the halogens

 

9 Chemistry of d- and f- transition elements and their  compounds with regard to the biological and pharmaceutico-medical aspects

9.1 the scandium subgroup, lanthanides, actinides

9.2 the titanium subgroup

9.3 the vanadium subgroup

9.4 the chromium subgroup

9.5 the manganese subgroup

9.6 the iron triad

9.7 the palladium triad; the platinum triad

9.8 the copper subgroup

9.9 the zinc subgroup

 

Seminars:

 

1 Basic chemical terms, empirical formulas

2 Nomenclature and formulas of inorganic compounds

3 Structural (Lewis dot) formulas

4 Solutions - calculation of concentrations

5 Stoichiometric calculations

6 Acids and bases, acid-base reactions, calculations of pH, Ka, hydrolysis of salts

7 Oxidation number, oxidation and reduction - balancing of equations

 

Last update: Palát Karel, PharmDr., CSc. (27.09.2025)
Learning outcomes

  

General and Bioinorganic Chemistry

The subject of General and Bioinorganic Chemistry unifies and expands the knowledge and skills acquired during secondary school chemistry studies in the area of general principles and laws governing chemical processes, including chemical calculations, which apply to all chemical substances regardless of their specific composition or classification within a compound type or group. In the field of inorganic chemistry, it extends high school knowledge and skills regarding biologically significant elements and their inorganic compounds.

Based on the acquired knowledge and skills, students will be able to:

  • Explain and characterize fundamental principles of the microscopic world relevant to general chemistry, including the structure and properties of atoms and selected subatomic particles, the quantum-mechanical model of the atom, and derive the structure of the electron shell (including orbital types) and its electron occupancy.

  • Explain the principles behind the construction and classification of the periodic table of elements (PTE), characterize basic atomic parameters and their dependence on the element’s position in the PTE, define the valence shell and its importance for chemical behavior of atoms.

  • Explain the nature of chemical bonding and its parameters as well as weak intermolecular interactions, define the different types of bonds and weak interactions, and derive physical and physico-chemical properties of compounds based on their characteristics and molecular polarity.

  • Explain the principles of hybridization and the VSEPR model, and use them to determine the spatial structure of a given particle.

  • Define a chemical process (chemical reaction) and apply various criteria for its classification.

  • Explain the basic rules and laws of chemical thermodynamics, including state functions and the energetic feasibility of chemical reactions, chemical (reaction) kinetics, reaction rates and ways to influence them, including catalysis.

  • Explain the basic rules and laws related to chemical equilibria and equilibrium constants, perform related calculations, and describe ways to influence chemical equilibrium.

  • Define acids and bases according to different theories, derive their behavior in various environments and with each other, and describe and compare acid and base strength (according to Brønsted–Lowry theory) both verbally and mathematically. Explain the nature of hydrolysis, its effect on solution pH, and ways to influence it.

  • Explain oxidation and reduction in a broader context, including reagents, galvanic cells, and electrolysis, and balance various types of redox reactions.

  • Identify coordination compounds, define their nature, individual types of complexes, their isomerism, significance, and uses of common representatives in analytical chemistry, pharmacy, and in biochemical processes.

  • Use general characteristics of elements to classify them into groups according to various criteria, including their occurrence.

  • Apply the properties of main group elements and their compounds to their reactivity, preparation/production, and use.

  • Apply the properties of transition elements and their important compounds to their reactivity and use.

  • Apply the properties of both main and transition group elements and their compounds to their biological properties and related applications.

  • Explain the nature of chemical formulas, their types, properties, and usage. Construct a formula (empirical, molecular, functional, structural-electronic) of an inorganic and organometallic compound from its name and name an inorganic compound according to IUPAC rules.

  • Calculate the composition of a mixture (especially solutions, including saturated ones) from given data, including the state after dilution, mixing, or evaporation of the solvent, and express the final composition mathematically.

  • Calculate the empirical formula of a compound from given data and determine the percentage composition of individual elements in a compound, the anhydrous substance in a hydrate, or the pure substance in a mixture.

  • Write and balance an equation for an inorganic process (including redox reactions) and apply the relationship between stoichiometric coefficients and the amount of substances to calculate the amounts of reactants, yields, products, and other relevant data that can be derived from the chemical equation.

Last update: Palát Karel, PharmDr., CSc. (27.09.2025)
 
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