GENERAL AND INORGANIC CHEMISTRY AND ELEMENTS OF ORGANIC CHEMISTRY

The aim of the course is to provide students with a general foundation in chemistry and to enable them to understand related topics addressed and further developed in other courses within the Degree Programme.

Based on the Dublin Descriptors, by the end of the course students will have achieved the following learning outcomes, with particular reference to the basic chemical knowledge required for the study of Geological Sciences.

• Knowledge and understanding: students will understand the fundamental principles of general, inorganic, and organic chemistry, including the structure of matter and the atom, the periodic table, chemical bonding, nomenclature, chemical reactions, states of matter, thermodynamics, solutions, chemical equilibrium, acids and bases, and kinetics. They will also understand the relationships among the structure, composition, and properties of substances, with particular emphasis on materials and processes of geological relevance.
• Applying knowledge and understanding: students will be able to use chemical formulae, nomenclature, and symbols correctly; balance simple chemical equations; perform calculations involving the mole, stoichiometry, concentrations, gases, pH, and equilibrium; and interpret electron configurations, Lewis structures, and periodic properties. They will be able to apply this knowledge to the description of minerals, natural solutions, chemical transformations, and basic geochemical processes.
• Making judgements: students will be able to select the most appropriate models and relationships for solving simple chemical problems, assess the correctness of the results obtained, and critically interpret quantitative and qualitative data concerning the composition and behaviour of matter.
• Communication skills: students will be able to describe concepts, procedures, and results using accurate scientific language, appropriate chemical terminology, and the main symbolic, graphical, and mathematical representations.
• Learning skills: students will acquire the methodological and conceptual foundations required to independently explore the chemical aspects of geological disciplines and to undertake subsequent courses in mineralogy, petrology, geochemistry, and environmental sciences.

Course structure includes frontal, collaborative and/or cooperative lessons.  Group works and individual research projects will be also encouraged.

Information for Students with Disabilities and/or Specific Learning Disorders (SLDs)

To ensure equal opportunities and in compliance with current legislation, students may request an individual meeting to arrange any appropriate compensatory measures and/or exemptions, in accordance with the learning objectives and their specific needs.

Basic knowledge of mathematics and physics is required, including operations with real numbers, solving first- and second-degree equations, and the equation of a straight line.

As specified in the Academic Regulations, attendance is a mandatory requirement for passing the final examination.

• Introduction to Chemistry – Matter and its states of aggregation*; the three levels of chemistry; matter and its units of measurement*; significant figures; pure substances, both elemental* and compound*; homogeneous* and heterogeneous* mixtures.
• Chemical Nomenclature* – Elements* and their representation; oxidation number*; classification of inorganic compounds*; ionic* and molecular* compounds; traditional* and IUPAC* nomenclature.
• Chemical Reactions* – Representation of chemical reactions*; Lavoisier’s law of conservation of mass*; balancing chemical equations*; combustion reactions; precipitation reactions*; gas-forming reactions; acid–base reactions*; redox reactions* and their balancing*.
• General Principles of Atomic Structure – Rutherford’s experiment; planetary atomic model; atomic number*; mass number*; isotopes*; isotopic abundance; atomic mass unit* (amu); relative atomic mass*; molecular mass*; mole*; empirical formula*; molecular formula*; expanded formula; structural formula.
• Structure of Matter – Bohr’s atomic model*; quantum-mechanical model*; quantum numbers*; wave interpretation of the atom; atomic orbitals*; Pauli exclusion principle*; Hund’s rule*; Heisenberg uncertainty principle*; electron configuration*.
• The Periodic Table – Periodicity*; atomic radius*; ionic radius; ionisation energy; electron affinity; electronegativity*.
• Chemical Bonding – Lewis structures* and the octet rule*; exceptions to the octet rule; molecular geometry; VSEPR theory*; bond energy; ionic bond*; covalent bond*; coordinate covalent bond*; hydrogen bond*; valence bond theory*; hybridisation*; resonance.
• The Gaseous State – Pressure*; Boyle’s law; Charles’s law; Gay-Lussac’s law; Avogadro’s hypothesis; ideal gas law*; gas mixtures and Dalton’s law*; kinetic molecular theory*; Graham’s law; real gases*.
• Introduction to the Solid State – Metallic and ionic crystalline solids*; close-packed structures*; molecular solids and covalent network solids*; glassy solids*.
• The Liquid State – Properties of liquids; viscosity; surface tension and vapour pressure.* Phase transitions: phase diagram of water.*
• Thermodynamics – State functions; first law of thermodynamics*; second law of thermodynamics*; entropy* and Gibbs free energy*; spontaneity of processes*.
• Solutions – Molarity*; mole fraction; molality; mass percentage; density*; Raoult’s law; colligative properties*; electrolytes*; degree of dissociation; van ’t Hoff factor.
• Chemical Equilibrium* – Law of mass action*; equilibrium constant*; dependence of the equilibrium constant on temperature; factors affecting chemical equilibrium*.
• Acids and Bases* – Strength of acids and bases; dissociation constant*; ionic product of water*; pH calculations*; pH indicators; salt hydrolysis; buffer solutions*; strong acid–strong base titrations; solubility product*; common-ion effect on solubility*.
• Introduction to Chemical Kinetics – Reaction order and molecularity; reaction rate*.
• Elements of Inorganic Chemistry – The elements of the s- and p-blocks.*
• Elements of Organic Chemistry – Organic compounds and properties of carbon.* Molecular formulas and representations; constitutional isomerism and stereoisomerism; saturated, unsaturated and aromatic hydrocarbons*: structure, nomenclature and main properties; functional groups and the main classes of organic compounds.

N.B. Knowledge of the topics marked with an asterisk is a necessary, but not sufficient, condition for passing the examination

Chemistry & Chemical Reactivity by Kotz, John C., Treichel, Paul M., Townsend, John, Treichel, David. A.

The examination consists of a written test followed, upon successful completion, by an oral examination.

The written test lasts 90 minutes and includes numerical exercises and open-ended and/or multiple-choice questions. Each exercise or question is assigned a specific score, for a maximum total of 30 points. The written test is considered passed with an overall score higher than 18/30.

During the test, students are not allowed to consult textbooks, formula sheets, course notes, or periodic tables, nor may they use mobile phones, even in calculator mode. Only a calculator may be used. Students must bring a valid identity document.

Students who have passed both mid-term tests are exempt from the written examination during the first examination session.