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Learning outcomes
The students, upon successful completion of the course, should be able to:
• correlate the wavelength with the frequency of light, calculate energy of a photon, determine the wavelength or frequency of a transition for the atom of H, apply the equation de Broglie, apply the rules for quantum numbers.
• apply Pauli’s principle, determine the structure of an atom by applying the Aufbau principle or by the period number and the group number, apply the Hund’s rule.
• identify chemicals that are acids or bases, according to Brønsted-Lowry or Lewis theory, predict whether an acid-base reaction favors the reactants or products, calculate H3O+ and OH–concentrations of a strong acid or base solution.
• define basic concepts such as solution and its characteristics, ways of expression of concentration (molarity, molality, formality, % by weight, etc.) and performs calculations to dilute, concentrate or mix solutions.
• apply relationships, that connect molecule and ion concentrations to weak acid and base solutions.
• perform the relevant calculations for the preparation of buffer solutions.
• know the factors that affect the rate of chemicals reactions.
• know the basic concepts of Thermodynamics and Thermochemistry and characterize a reaction as exothermic or endothermic, thermodynamically / entropically favored / unfavorable.
• define basic concepts such as oxidation and reduction and understands the operation of galvanic and electrolytic cells.
• describe all the safety rules in a chemical laboratory and recognize good laboratory practices.
SYLLABUS
THEORETICAL PART
1. Atomic structure
Atoms, Molecules and Ions (the atomic theory of matter, the nucleus of the atom, electrons, atomic masses, the concept of mole and the Avogadro number) – Electronic configuration (Electromagnetic radiation, atomic spectra, introduction to quantum theory- Bohr’s atomic model- Wave / particle dualism – The Uncertainty Principle- Quantum numbers and atomic orbitals – Multi-electronic atoms – Electronic devices and periodic table).
2. Periodic Table and Periodic Properties of Elements.
The Modern Periodic Table – Metals, non-metals and their ions – The atom and ion sizes- Ionization energy and electronic affinity – Magnetic properties – Periodicity in the properties of elements – Biological importance of certain elements.
3. Chemical Bonds.
The ionic bond- The covalent bond- Polar covalent bonds and electronegativity- Intermolecular forces- Van der Waals forces- Hydrogen Bond.
4. Solutions.
Solubility- Ways of expressing concentration- Relationships between expressions of Concentration – Dilution and mixing of solutions.
5. Chemical Equilibrium.
Equilibrium in Chemical Reactions- Homogeneous and Heterogeneous Reactions – Law of Mass Action- Direction and Stability of Chemical Equilibrium- Factors Affecting the Direction of Chemical Equilibrium.
6. Chemical Kinetics.
Reaction rate- Reaction rate equation – Factors affecting the rate and rate constant – Reaction order.
7. Chemistry of aqueous solutions
Acids and bases (Arrhenius theory, Brönsted-Lowry theory, Lewis theory, strong and weak acids and bases). Ionic equilibria in aqueous solutions (ionization of weak monoprotic acids and bases, ionization of water and pH, indicators, salt hydrolysis, acid-base titrations, buffer solutions, Henderson-Hasselbalch equation, ionization of polyprotic acids).
8. Thermochemistry.
Principles of Thermochemistry. Gibbs Free energy (G) – Enthalpy (H) – Entropy (S). The equation ΓG = ΓH-TΓS – Exothermic / endothermic reaction – Formation enthalpies of bonds (bond strengths) – Calculation of ΓH of reactions- Thermodynamically / entropically favored / unfavorable reaction.
9. Oxidation- Reduction.
Oxidation / Reduction- Oxidizing and reducing agents -Oxidation number- Balancing of oxidation / reduction half-reactions and redox reactions- Electrochemical series, Galvanic cells, Electrolytic cells.
10. Colligative properties of solutions.
Ideal and non-ideal solutions – Raoult’s law- Reduction of vapor pressure of the solvent- Elevation of the boiling point- Lowering of the freezing point, Osmosis, osmotic pressure- Operation of artificial kidney unit.
LABORATORY PART
- Chemical laboratory safety rules- Chemical laboratory instruments and operations.
- Preparation of solutions.
- Measurement of pH of solutions.
- Study of buffer solutions.
- Volumetric analysis- Acid-based titrations
- Chemical Kinetics
- Potentiometry
- Compleximetric titrations
- Redox titrations.