Università Roma Tre

Definition of substance, chemical elements and their symbols, atomic number, mass number, isotopes, periodic table, compounds, molecules and chemical formula.
Atomic mass unit, atomic weight, formula weight, mole, Avogadro's number; calculation of mass percent composition of a compound, calculation of the empirical formula of a compound. Chemical reactions (stoichiometry): symbolism, stoichiometric coefficients, balancing simple reactions, reaction yield, limiting reagent, indirect analysis. Electronegativity, definition of oxidation number and rules for its determination; oxidation-reduction reactions and their balancing.
Classification and nomenclature of inorganic compounds: elements, monoatomic ions, basic oxides, acid oxides, hydroxides, hydracides, oxoacids, salts and reactions producing them.
Atomic structure: Bohr model and quantization, quantum numbers and energy levels; stationary wave, wave-particle dualism for the electron, Heisenberg uncertainty principle, wave functions, orbitals, probability; shape of orbitals and graphical representation; energy of orbitals, electronic configuration and aufbau, periodic properties, atomic size, ionization energy, electronic affinity, electronegativity.
Chemical bonding: definition of chemical bonding according to Lewis theory, ionic bonding, covalent bonding, bond energy, bond distance, bond order; rules for constructing molecular structure (octet rule), formal charge, resonance and resonance energy, exceptions to octet rule; spatial arrangement of molecules, VSEPR theory; valence bonding (VB) theory, σ-type and π-type bonding, hybrid orbitals.
Crystalline and amorphous solids; metallic solids, metal bonding, properties; ionic solids, properties; molecular solids, intermolecular forces, hydrogen bonding; covalent solids.
Definition of pressure, volume and temperature and their units, perfect gas model and equation, molar volume, absolute and relative density; gas mixtures, Dalton's law, partial pressures.
Definition of thermodynamic system: type and state; thermodynamic variables; reversible and irreversible transformations; graphical representation; thermal equilibrium; heat capacity and specific heat.
First Principle of Thermodynamics: definition of state function; Internal Energy Function U; Energy transfers: heat and work; Mechanical work: expansion of a perfect gas, work for reversible and irreversible processes, graphical representation. Isochore and isobar transformations. Thermochemistry: definition of state function enthalpy H; the enthalpy of physical changes; Enthalpy of a chemical reaction; molar enthalpy and standard state; standard molar enthalpy of elements. Hess's law. Estimation of binding energy. Born-Haber cycle.
Second Principle of Thermodynamics: qualitative description; definition of Entropy; increase in entropy. Criterion for spontaneity (statistical interpretation). Definition of free energy G. Third principle of thermodynamics.
Liquid state: factors influencing aggregate state; vapor pressure: qualitative description and temperature dependence (Clapeyron's eq. and its thermodynamic demonstration). State diagrams for pure substances: transformations from one state to another, triple point, critical point, cooling curve at constant pressure, measurement of variance. Solutions: definition and types of solutions, Henry's law, definition of ideal liquid solution; measurement of concentration: molarity, molality, molar fractions, percentage by weight.
Properties of solutions: Raoult's law for mixtures of completely miscible liquids and temperature versus concentration state diagram (calculation of relative quantities); colligative properties for non-volatile solutes strong electrolytes and non-electrolytes, osmotic pressure, cooling curve for solutions.
Chemical equilibrium: definition of chemical equilibrium, equilibrium constant (Kp and Kc), thermodynamic definition of chemical equilibrium; reaction quotient, meaning of K, relationship between Kp and Kc, principle of mobile equilibrium (influence of pressure and concentrations), Van't Hoff's law (dependence of K on temperature); heterogeneous equilibrium. Dissociations: gas dissociation, degree of dissociation, weak electrolytes in solution.
Heterogeneous solid-liquid equilibrium in an aqueous environment: solubility of a salt, saturated solution, poorly soluble compounds, common ion effect.
Acids and bases according to Arrhenius and Brönsted-Lowry; strength of acids and bases; ionic product of water; definition of pH; conjugate acid-base pair and relationship between Ka and Kb; calculation of pH of a solution of a strong acid and a strong base (even very dilute), a weak acid and a weak base. Salt hydrolysis: calculation of pH for salts producing neutral solutions, salts producing acid solutions and salts producing basic solutions; buffer solutions.
Electrochemistry: galvanic cell, salt bridge, Nernst's Equation, calculation of cell potential, standard hydrogen electrode, standard reduction potentials, concentration cells and other types.