COURSE SYLLABUS

Course title : Chemistry
Credit hours : 6
Theory : 5 credits
Experiment : 1 credit
Objects : Undergraduate students in Processing Technology and Food Technology
Prerequisite : Analytics 1, 2
Evaluation methods :
( Midterm exam : 1 paper (multiple-choice test)
( Final exam (applied at the end of trimester) : writing
( Weighting of midterm exam : 30 %
6. Description of course content :

PART I : GENERAL CHEMISTRY

CHAPTER I
ATOMIC STRUCTURE AND PERIODIC TABLE
1.1 Atomic structure
Atomic structure according to quantum concepts
The Hydrogen atom : Results from solving the Schrödinger equation for hydrogen atom
1.2 Many-electron atoms
1.2.1 Wave function and atomic energy. Shells, sub-shell and orbitals.
1.2.2 Principal quantum number. Orbital quantum number. Magnetic quantum number.
1.2.3 Principles and rules of electron distribution in multi-electron atoms
1.2.4 Electron configuration of elements. Concepts of s, p, d, f elements and valence electrons.
1.3 The Periodic System of the chemical elements
Periodic Law and structure of the Periodic table of chemical elements.
Periods, Groups
The periodic change in properties of elements: Atomic radius. Ionic radius. The first ionization energy. Electron affinity. Electronegativity

CHAPTER II
CHEMICAL BONDS AND MOLECULAR STRUTURE
Classical theories of bonds
Ionic bonds
Covalent bonds
Valence bond theory (VSEPR-Valence Shell Electron Pair Repulsion Theory)
Theorems of VB theory
The rule of spinning valence
( bond, ( bond. Geometries of molecules with maximum hybridization rule
Theory of hybridization: Hybrid rules. sp, sp2, sp3,sp3d2 hybridization
Coordinate bonds and formation of complexes
Molecular structure
Molecular polarity: Polar and non polar molecules. Dipole moment. Dipole moment and molecular structure. Relationship between molecular polarity and their physical and chemical properties.
Ionic and molecular polarization
2.4 Weak bonds : Hydrogen bond. Van der Waals forces

CHAPTER III
THE BASICS OF CHEMICAL THEMODYNAMICS

3.1 Basic concepts: Systems and Surroundings. State functions. Process functiosn. Energy. Internal energy. Work. Heat.
3.2 First Law of Thermodynamics
3.2.1 Statements of the first law of thermodynamics
3.2.2 Equation of the first law of thermodynamics
3.2.3 Heat effect at constant pressure. Heat effect at constant volume
3.3 Themochemistry
3.3.1 Heat effect of reaction: Heat of formation. Heat of combustion. Heat of state transition
3.3.2 Hess’s Law and the results
3.4 Second Law of Thermodynamics
Statements of the second law of thermodynamics
Equation of the first law of thermodynamics
Criterion for spontaneous processes in isolated systems
Criterion for spontaneous processes in constant-pressure-temperature closed systems
Criterion for spontaneous processes in constant-volume-temperature closed systems

CHAPTER IV
CHEMICAL KINETICS

4.1 Basic concepts: Chemical reactions. Homogeneous reactions. Heterogeneous reactions. Mechanisms of reactions ….
4.2. Reactions Rates
4.2.1 Reaction rates: Definition. Average rate. Simultaneous rate
4.2.3 Effect of concentration on reaction rate ( Law of mass action
4.2.4 Effect of temperature on reaction rate: The Van’t Hoff Rule. The Arrhenius Equation
4.3 Kinetics of chemical reactions
4.3.1 Reaction Order. Molecularity.
Kinetics of First-Order Reactions and Second-Order Reactions
4.4 Catalysis
4.4.1 Concepts and definition of catalysis
4.4.2 General mechanisms of catalysis processes
4.4.3 Classification of catalysis processes
4.5 Reversible reactions
4.5.1 Reversible reactions and equilibrium state
4.5.2 Equilibrium constants and the evolvement of a reaction
4.5.3 Displacement of Equilibrium ( Le Chatelier’s Principle

CHAPTER V
SOLUTIONS
5.1 Generality of solution
Solution : Solvent. Solute. Solubility. Concentrations ( C%, CM, Cm, Ni)
Dissolution process : Interaction between solvent and solute. Heat of dissolution. Factors affecting the solubility of solid, liquid, gas solute in liquid solvent
Solution of nonelectrolyte. Concentration properties of nonelectrolyte solution
Lowering of saturated vapour pressure of solution versus pure solvent
Elevation of Boiling Point of solution versus pure solvent
Depression of Freezing Point of solution versus pure solvent
Osmotic phenomenon
Solution of electrolytes
Electrolytic dissociation. Degrre of dissociation (. Strong electrolytes. Weak electrolytes
Equilibrium in solution of a weak electrolyte. Dissocation constant. Relationship between dissocation constant and degrre of discociation.. Displacement of electrolytic equilibrium
Proton equilibrium in aqueous solution
Equilibrium in solution of sparingly soluble electrolytes
Solubility Product
Relationship between solubility product and solubility
Rule for dissociation and precipitation
Equilibrium displacement in solution of a sparingly soluble electrolyte
Direction of reactions in electrolytic solutions

CHAPTER VI
ELECTROCHEMISTRY

Oxidation- reduction