General and Inorganic Chemistry

Course Code:

Π1 1060


1st Semester

Specialization Category:

Required ( ΜΓΥ )

Course Hours:





Course Theory

I – STRUCTURE OF MATTER: Forms of matter: The gaseous state. Laws of gases. The liquid state. Evaporation and boiling. – The solid state. Crystalline and amorphous solids. Mixtures. Homogeneous systems: solutions. Colloidal systems. Heterogeneous systems. – Atoms and molecules. – Atomic and mass number. The mass of atoms and molecules. Chemical Formulas: Molecular, structural, electronic and stereochemical formula. Electronic structure of atoms. Single-electron atom: the Bohr atom. Polyelectronic atoms: their electron structure. The Periodic Table of the elements. Metals and nonmetals. Transition metals. Electronegativity, ionization energies and electron affinity. The electronic structure of molecules. Types of chemical bonds: the covalent bond. The Lewis model for the covalent bond; bond energies, bond lengths and dipole moments; polarity of molecules. Ionic bonds. – Intermolecular interactions. Intermolecular bonding: the hydrogen bond. Types of bonds in crystalline solids (ionic and molecular solids, metals, semiconductors). Iron and copper: their physical and chemical properties. Coordination compounds (complexes) of transition metals. – Specific elements and compounds: molecular oxygen. Water. Silicates and aluminosilicates.

II – IONIC EQUILIBRIA IN AQUEOUS SOLUTIONS: Electrolytes. Acids and bases. Bronsted-Lowry and Lewis acids and bases. Dissociation of acids and bases in aqueous solutions. – Definition of pH. Conjugate pairs of acids and bases. Definition of the pK of acids and bases. Salts. Salt hydrolysis. Buffer solutions. Buffer capacity. Solubility of salts. Solubility product.

III – OXIDATION AND REDUCTION. Redox reactions. The method of redox half-reactions. Oxidation number of atoms in ions and molecules. Electrolysis. The Nernst equation. Electrode potentials; standard reduction potentials. Reference electrodes. The electrochemical series: redox properties of metals according to their electrode potentials; connections with metal corrosion.

Course Practicals

The laboratory part of the course will include practicals on the structure of chemical compounds, preparation, dilution and mixing solutions, the acid-base properties of certain chemical compounds, the titration of weak acids and bases and buffer solutions; the redox properties and the solubility product of salts.


The Scope of the Course

To convey a solid chemical background so that students are able to qualify and quantify various stimuli from the entire body of natural science.

Course objectives

The students are expected to understand the basic concepts related to the structure of matter at the atomic and molecular level; to clarify the chemical basis of the physical states of matter: solids, liquids and gases; to elucidate the acid/base and oxidative/reductive behavior of certain compounds and elements; to develop the requisite laboratory skills for safe handling of common chemicals and using these for the study of chemistry-related issues.

The student’s final grade results from 50% of the grade of the theoretical part and 50% of the grade of laboratory practice.
Language of evaluation: Greek
ΤΗΕΟRY (50%): Written exams:
• Open-ended questions
• Multiple-choice questionnaires
• Short-answer questions
LAB PRACTICES (50%): Written essays

Greek and Translated into Greek
1. Μανουσάκης Γεώργιος, Γενική και Ανόργανη Χημεία, Εκδ. Κυριακίδη Α.Ε., 2006
2. Ξένος Κωνσταντίνος Δ., Ξένου Ευγενία, Γενική και ανόργανη χημεία, Εκδ. ΠΑΡΙΚΟΥ, 2009
3. Λάλια – Καντούρη Μ., Παπαστεφάνου Στέργιος, Γενική και ανόργανη χημεία, Εκδ. Ζήτη, 1995
4. Ebbing, Gammon, Γενική Χημεία, εκδ. Τραυλός, 2006
5. Cotton, Darlington, Lynch, Χημεία, εκδόσεις Ευγενίδου (μτφρ. Ν. Γιάννοβιτς)
6. Caret, Denniston, Topping, Αρχές και Εφαρμογές της Ανοργάνου, Οργανικής και Βιολογικής Χημείας, Ιατρικές εκδόσεις Κ. Πασχαλίδης (μτφρ. Ι. Σέκερης)
7. Ν. Λυδάκης-Σημαντήρης, Γενική Χημεία και Ενόργανη Ανάλυση, εκδόσεις Τζιόλα, 2007
1. Catherine Housecroft and Edwin Constable, Chemistry, Prentice Hall 2009
2. Steven S. Zumdahl and Susan A. Zumdahl, Chemistry; Brooks Cole; 7th edition (January 9, 2006).
3. Raymond Chang, General Chemistry: The Essential Concepts, McGraw-Hill Science/ Engineering/Math; 5th edition (February 23, 2007).