By successfully completing the course the students are expected to be able to:
Locate the position in the table of periodicity of elements by their atomic number.
Write the electronic structure of elements and monoatomic ions.
Write the correct Lewis structures for simple and moderately compex compounds.
Determine the hybridization of atoms and consequently the structure of small and medium sized molecules.
Determine the bonding and the possible intermolecular interactions between small and medium sized molecules.
Understand the basics of thermodynamics and spectroscopy.
Course Content (Syllabus)
Atomic model: Initial atomic models – quantum description – current state of atomic theory. Atomic wave functions for hydrogen atom and simple applications of the atomic theory.
Periodic properties of the atoms: Periodic table. Periodic properties of the elements – atomic radius – ionization energy – electron affinity – electronegativity. Understanding of the periodic properties through atomic theory. Determination of the electronic configuration of atoms – stable electronic structures.
Description of the chemical bond: Formation of simple molecules. Valence bond approximation. Bond description based on molecular orbitals. Covalent bonds. Description of polyatomic molecules – hybridization – VSEPR theory. Molecules with π bonds – aromatic systems. Energy and polarization of a covalent bond. Structure and interactions of macromolecules. Ionic bond – hydrogen bond – other electrostatic interactions.
Metal compounds: General considerations. Classification of metal coordination compounds. Bond theories in coordination compounds. Optical and magnetic properties of coordination compounds. Isomerism in coordination compounds.
Elements of molecular spectroscopy: General principles of spectroscopy. Electronic, vibrational, magnetic resonance and photoelectron spectroscopy. Principles and applications in the identification of chemical compounds.
Description of the gaseous state: Brief description of the laws of gases and the kinetic theory of gases. Reactions in the gas state.
Elements of chemical thermodynamics: General considerations. Enthalpy, entropy and free energy.
Chemical properties of elements in groups: Elements of the S, P and D blocks of the periodic table. Descriptive presentation of their general chemical properties and some physical properties of their compounds.
The course is accompanied by a set of laboratory experiments which include:
Rules of good laboratory practice.
Categories of chemical reactions – product identification.
Chemical equilibrium in solution. Homogeneous and heterogeneous reactions and means to alter their equilibrium.
Weak electrolyte dissociation, determination of the pK of a weak acid. pH indicators and their use. Preparation and study of a buffer solution.
Elements of redox chemistry. Oxidative and reductive properties of some compounds. Galvanic cells.
Principles of visible spectroscopy. Application of visible spectroscopy in the identification and quantification of chemical compounds.
Principles of volumetric analysis. Volumetric techniques in the determination of acid-base or metal content of a solution.
Course Bibliography (Eudoxus)
Στοιχεία Γενικής Χημείας, Κωδικός Βιβλίου στον Εύδοξο: 22766674, Έκδοση: 1η έκδ./2012, Συγγραφείς: Ακρίβος Περικλής Δ., Χατζηδημητρίου Αντώνης, ISBN:978-960-456-333-3, Τύπος: Σύγγραμμα, Διαθέτης (Εκδότης): Ζήτη Πελαγία & Σια Ο.Ε.