General Inorganic Chemistry

Course Information
TitleΓΕΝΙΚΗ ΑΝΟΡΓΑΝΗ ΧΗΜΕΙΑ / General Inorganic Chemistry
Cycle / Level1st / Undergraduate
Teaching PeriodWinter
Course ID40000973

Class Information
Academic Year2018 – 2019
Class PeriodWinter
Faculty Instructors
Class ID
Course Type 2016-2020
  • General Knowledge
Course Type 2011-2015
General Foundation
Mode of Delivery
  • Face to face
Digital Course Content
The course is also offered to exchange programme students.
Language of Instruction
  • Greek (Instruction)
Learning Outcomes
Upon completion of the course students should be able: •To understand basic principles governing various physicochemical phenomena. •To correlate macroscopic observation processes with those at the molecular level.
General Competences
  • Apply knowledge in practice
  • Retrieve, analyse and synthesise data and information, with the use of necessary technologies
Course Content (Syllabus)
Matter and energy, mass and weight. Units, measurement and equations. Distinguish elements, compounds, mixtures. Atomic and molecular mass. Calculate a percentage composition from formula. Empirical and molecular formulae. Balance chemical equations. Mole, molarity, normality, Avogadro's number. Characteristic properties of solids, liquids and gases. Endothermic and exothermic reactions. Structure of the nuclear atom and isotopes. Atomic structure, electronic shells and subshells, and orbitals. Energy level diagram for the hydrogen atom, and spectrum of atomic hydrogen. Quantum numbers for the hydrogen atom, and for other elements. Interpret orbitals in terms of probability s, p, and d electrons. Aufbau principle, Pauli principle and Hund's rules to build up electron configurations of the elements of the Periodic Table. Periodicity from configuration across and down the Table, and explain trends in radii, ionisation enthalpies, electron affinities and electronegativities. IUPAC Nomenclature of Inorganic Compounds. Classification of Inorganic Compounds. Ionic and covalent bonding. Metallic bonding and relate to metallic properties. Hybridisation of an atom in a given molecule. Lewis structures for simple molecules. Distinguish sigma and pi bonds. Orbital overlap of s, p, and d electrons, bond order. Molecular orbital energy-level diagram. Non-bonding and antibonding orbitals from s, p, and d combinations. Theories of resonance and p-orbital overlap. Dipoles in polar molecules. Covalent or ionic bonds. Occurrence of intermolecular interactions (van der Waals forces, and hydrogen-bonding). Inter- and intra-molecular hydrogen bonding and van der Waals (London) forces in a molecule. State the Bronsted and Lewis acid-base theory and its applications to salt hydrolysis, buffers and solubility. The theory of redox reactions.
Atomic structure, Molecules, Chemical bond, Nomenclature, Chemical equilibrium, Thermochemistry, Acids-bases, Red-ox
Educational Material Types
  • Slide presentations
  • Book
Use of Information and Communication Technologies
Use of ICT
  • Use of ICT in Course Teaching
  • Use of ICT in Communication with Students
Course Organization
Student Assessment
Student Assessment methods
  • Written Exam with Short Answer Questions (Summative)
  • Written Exam with Problem Solving (Summative)
Course Bibliography (Eudoxus)
«Γενική Χημεία», D.D. Ebbing, S.D. Gammon (Μετάφραση Νικόλαος Δ. Κλούρας), Κωδικός 5697, ISBN 960- 7990-66-8.
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