Info
Course Code CCC207
Semester 1
Category Basic
Points 3
ECTS Units 4
Eclass
Lecturer
No items found
Recommended Reading

1. «General Chemistry», Darrell D. Ebbing & Steven D. Gammon

Houghton Mifflin Company, New York, 1999 (6th Edition). Translated into Greek by N. Klouras

Publisher: P. Travlos, Athens 2007 (3rd Edition).

2. «Basic Inorganic Chemistry», N. Klouras

Publisher: P. Travlos, Athens 2003 (6th Edition).

3. «Inorganic Chemistry – Basic Principles», G. Pnevmatikakis, Χ. Mitsopoulou, Κ. Methenitis

Publisher: A. Stamoulis, Athens 2005

4. «General Chemistry», Darrell D. Ebbing & Steven D. Gammon

Houghton Mifflin Company, New York, 2009 (9th Edition).

5. «General Chemistry: Principles and Modern Applications»,

Ralf H. Petrucci, William S. Hawood, Geoff E Herring, & Jeffry Madura, Prentice Hall, 2006 (9th Edition).

6. «General Chemistry: The Essential Concepts», Raymond Chang

McGraw-Hill Science Engineering, 2007

7. «Chemistry: The Central Science»,Theodore E. Brown, Eugene H. LeMay, & Bruce E. Bursten, Prentice Hall, 2006 (10th Edition)

8. «Chemistry», John McMurry, Robert C. Fay, & Logan McCarty

Prentice Hall, 2003 (4th Edition)

9. «Chemistry», Steven S. Zumdahl, Houghton Mifflin College Div

2007 (7th Edition).

Course Description

1. Calculations with Chemical Formulas and Equations

Molecular weight and formula weight. The mole concept. Mass percentages from the formula. Elemental analysis: Percentages of carbon, hydrogen and oxygen. Determining formulas. Molar interpretation of a chemical equation. Amounts of substances in a chemical reaction. Limiting reactant: Theoretical and percentage yields.

2. Chemical Reactions: An Introduction

Ionic theory of solutions. Molecular and ionic equations. Precipitation reactions. Acid – base reactions. Oxidation – reduction reactions. Balancing simple oxidation – reduction reactions. Molar concentration. Diluting solutions. Gravimetric analysis. Volumetric analysis.

3. Thermochemistry

Energy and Its Units. Heat of reaction. Enthalpy and Enthalpy Change. Thermochemical Equations. Applying Stoichiometry to Heats of Reaction. Measuring Heats of Reaction. Hess’s Law. Standard Enthalpies of Formation. Fuels-Foods, Commercial Fuels and Rocket Fuels.

4. Ionic and Covalent Bond

Describing ionic bonds. Electron configuration of ions. Ionic radii. Describing covalent bonds. Polar covalent bonds. Electronegativity. Writing Lewis electron-dot formulas. Delocalized bonding – Resonance. Exceptions to the octet rule. Formal charge and Lewis formulas. Bond length and bond order. Bond energy.

5. Molecular Geometry and Chemical Bonding Theory

The VSEPR model. Dipole moment and molecular geometry. Valence bond theory. Description of multiple bonding. Principles of molecular orbital theory. Electron configurations of diatomic molecules of the second-period elements. Molecular orbitals and delocalized bonding.

6. Solutions

Types of solutions. Solubility and the Solution Process. Effects of Temperature and Pressure on Solubility. Ways of Expressing Concentration. Vapor Pressure of a Solution. Boiling-Point Elevation and Freezing-Point Depression. Osmosis. Colligative Properties of Ionic Solutions. Colloids.

7. Rates of Reaction

Definition of Reaction Rate. Experimental Determination of Rate. Dependence of Rate on Concentration. Change of Concentration with Time. Temperature and Rate; Collision and Transition-State Theories. Arrhenious Equation. Elementary Reactions. The Rate Law and the Mechanism. Catalysis.

8. Chemical Equilibrium

Chemical Equilibrium-A dynamic Equilibrium. The Equilibrium Constant. Heterogeneous Equilibria; Solvents in Homogeneous Equilibria. Qualitatively Interpreting the Equilibrium Constant. Predicting the Direction of Reaction. Calculating Equilibrium Concentations. Removing Products of Adding Reactants. Changing the Pressure and Temperature. Effect of a Catalyst.

9. Acids and Bases

Arrhenius concept of acids and bases. Brønsted–Lowry concept of acids and bases. Lewis concept of acids and bases. Relative strengths of acids and bases. Molecular structure and acid strength. Self ionization of water. Solutions of a strong acid or base. The pH of a solution.

10. Acid-Base Equilibria

Acid-Ionization Equillibria. Polyprotic Acids. Base-Ionization Equillibria. Acid-Base Properties of Salt Solutions. Common-Ion Effect. Buffers. Acid-Base Titration Curves.