CHEMISTRY AND BIOCHEMISTRY (1S-F)

GENERAL AND INORGANIC CHEMISTRY

Introduction and atomic structure
Properties of matter. Elements and compounds. Sub-atomic particles. Atomic number, mass number, isotopes. Atomic and molecular weight, gram atom, gram molecule. Atomic structure; atomic orbitals and quantum numbers. Electronic configuration of the elements.

Periodic trends in the chemical properties of the elements
Periodic table. Periodic properties of the elements: atomic size, ionization energy, electron affinity, electronegativity. Electronic structure and chemical properties.

Chemical bonding
Ionic bond; covalent bond (pure, polar, dative) and molecular orbitals. Intermolecular bonding: dipole-dipole interactions, hydrogen bonding, van der Waals forces.

Inorganic chemical compounds
Hydrurs, binary acids, oxides and anhydrides, peroxides, hydroxides, acids, neutral and acidic salts: formation reactions, reaction balancing, nomenclature, structural formulas.

Chemical kinetics
Rates of chemical reactions, rate laws. The factors that affect chemical reaction rate: chemical nature of the reactants, concentration of the reactants (order of a reaction), temperature and catalysts. Molecular collision theory and transition state theory.

Chemical equilibria
Chemical equilibrium is a dynamic process. The general expression of the equilibrium constant. Factors that affect the chemical equilibrium: variations of concentration, volume, pressure, temperature. Le Chatelier’s principle.

Chemical thermodynamics
First principle of thermodynamics, the concept of enthalpy. Second principle of thermodynamics, the concept of entropy. Third law of thermodynamics. Free energy and spontaneity of chemical reactions; free energy and equilibrium constant.

Solutions
Concentrations units: percent fraction w/w and w/v, molarity, molality, normality.
Colligative properties of solutions: boiling point elevation, freezing point depression; origin and significance of the osmotic pressure, van’t Hoff factor and osmolarity.
Acids and bases: Arrhenius theory, Bronsted and Lowry theory, Lewis theory. Acid-base equilibria. Strong acids and bases, weak acids and bases.
Water ionization. Concept of pH. Calculating the pH of acid and base (strong and weak) solutions. Hydrolysis of salts in water. Buffer solutions: properties and pH calculation.
Acid-base titrations.

Stoichiometry
Stoichiometric calculations. Balancing chemical equations. Oxidation state and oxidation number; balancing ox-red reactions. Chemistry exercises: concentrations of solutions, pH calculation of aqueous solutions containing different compounds, colligative properties.

ORGANIC CHEMISTRY

Introduction
Hybrid orbitals of carbon. Molecular and structural formulas. Types of reaction: substitution, addition, elimination. Electrophiles and nucleophiles reagents. Functional groups.

Hydrocarbons
Hydrocarbons classification. Alkanes: nomenclature, physical properties and characteristic reactions. Structural isomerism. Cycloalkanes: structure and nomenclature. Alkenes and alkynes: nomenclature, physical properties and characteristic reactions.
Benzene: concept of aromaticity and properties. Benzene reactivity and most important substitution reactions. Substituents effect on reactivity and orientation.

Alcohols and phenols
Structure, classification and nomenclature. Physical and chemical properties; the acid-base behaviour. Characteristic reactions. Formation of ethers.

Aldehydes and ketones
Structure and nomenclature. Physical properties. Characteristic reactions and their mechanism: addition of water, alcohols, amine; aldol condensation.

Carboxylic acids and related carbonyl derivatives
Carboxylic acids: structure and nomenclature. Physical properties and acidity of