00088 - Chemistry

Learning outcomes

The objective of the course is to provide the essential elements relative to the composition and behaviour of the various substances that constitute the Universe. At the same time, the course is intended to give the necessary information for a critical analysis on the following topics:

- the composition of the material objects in the surrounding world;

- the dependence of the macroscopic properties of substances on their microscopic composition and structure;

- the ability of substances to combine together, or to decompose, giving rise to other substances.

Course contents

Mod. 1 -Theory

1) atoms

2) molecules

3) transformations of substances

PART I: macroscopic and microscopic structure of matter

The atomic structure of matter. Atoms. Chemical formulas and molecular weight. Mole. Qualitative and quantitative meaning of chemical formulas.

The electronic structure of atoms. Bohr's atomic model. Quantization of energy. Dual nature of the electron and Heisenberg's principle. Wave theory, quantum numbers and atomic orbitals. Energy levels for atomic hydrogen. Atomic orbitals in atoms with many electrons. Pauli's principle and Hund's rule. Electronic configuration of atoms (aufbau) and periodic classification of chemical elements (Periodic Table).

Periodic change of the physical properties of atoms. Atomic size, ionization energy and electron affinity.

PART II: the chemical bond

The chemical bondand the energy of the system. Bond energy. Classification of chemical bonds.

The covalent bond. Valence bond theory. Polarity of covalent bonds, electronegativity. Stoichiometry of covalent compounds. Molecular geometry and VSEPR model. Polar and apolar molecules. Laboratory exercise on molecular geometry and polarity. Molecular orbital theory. Energy diagram of the molecular orbitals and electronic configuration of some simple biatomic molecules.

The chemical bond in the solid state. Ionic bond. Structure and properties of ionic compounds. Metallic bond. Short account on band theory for solids. Conductors, insulators and semiconductors.

Attractive forces between molecules in condensed phases. Van der Waals interactions. Hydrogen bonds. Factors determining the aggregation state of a substance.

Periodic behaviour of bond properties. Relationship between bond types and atom position in the Periodic Table. Prediction of the bond nature.

Chemical properties of the elements relative to their position in the Periodic Table. Periodic chemical properties. Properties of the compounds between the various elements and oxygen (oxides, hydroxides, oxoacids) or hydrogen (hydrides). Salts. Solutions: properties and composition. Gaseous solutions. Solubility. Electrolytic solutions.

PART III. Chemical reactions

Chemical equations. Energy involved in chemical reactions: internal energy and entalpy. Spontaneity of a chemical process: entropy and free energy.

Chemical equilibria. Homogeneous and heterogeneous equilibria. Equilibrium constant and its temperature dependence. Predictions on the evolution of a chemical system. Principle of Le Chatelier. Choice of the best reaction conditions.

Chemical kinetics. Rate of a chemical reaction. Factors affecting the reaction rate. Rate constants, order of reactions and lifetimes. Reaction mechanism and elementary steps. Activation energy. Catalysis.

Thermodynamic and kinetic aspects of a reactive chemical system.

Mod. 2 - Laboratory

- General rules of safety and behavior in the chemical laboratory.

- Experiences: (i) molecular models: from the crude formula to the molecular structure, (ii) chemical reactions of precipitation, redox, and reducing power scale, (iii) batteries and determination of equilibrium constants by electrochemical measurements.

The teacher will make the teaching material necessary to carry out the experiences (laboratory handouts and presentations) available.

The student will have to produce a written report for each practical laboratory exercise which will then be evaluated using a judgment (insufficient, sufficient, good). For module 2, there is no final exam; however, it will be necessary to obtain a positive evaluation of at least 75% of the reports to pass module 2.

 

Readings/Bibliography

It is essential to use the provided teaching material, including slides, worked examples, and exercises available on Virtuale – Unibo [https://virtuale.unibo.it/], together with lecture notes.

It is recommended to supplement your study with a university-level textbook dedicated to General and Inorganic Chemistry for first-year courses.

Here are some suggestions among the many available options:

• J. Overby, R. Chang, Chemistry, 4th ed., McGraw-Hill, 2024.

• T. L. Brown, H. E. LeMay, B. E. Bursten, C. J. Murphy, P. M. Woodward, M. W. Staltzfus, M. W. Lufaso, Chemistry: The Central Science, Edises, 2023.

Exercise books / practice materials

• The above-mentioned textbooks contain a large number of exercises. In addition, the instructor will solve and upload further exercises and exam samples on the course webpage (Virtuale).

Note
Students who already possess other study materials are encouraged to consult with the instructor to verify their suitability and content.

Teaching methods

The course is mainly structured around lectures, delivered at the blackboard and supported by PowerPoint presentations.

It also includes classroom exercises (problem-solving, use of molecular models) and some laboratory activities, totaling 16 hours.

Depending on the time available, topical issues or subjects of particular interest (for example, technological developments) related to the course content will be explored in greater depth.

Assessment methods

The assessment will normally take place through a written exam lasting two hours (2h).
The exam typically includes:

• an open-ended question related to theory,

• a question on molecular structure or chemical bonding,

• two stoichiometry exercises.

Students may request, in advance of the written exam, to take the exam orally, only in exceptional and well-justified cases.

The exam is considered passed with an overall score of 18/30 or higher.

Students with learning disabilities or temporary or permanent disabilities: please contact the relevant University office promptly (https://site.unibo.it/studenti-con-disabilita-e-dsa/itStudents with learning disabilities or temporary or permanent disabilities: please contact the relevant University office promptly (https://site.unibo.it/studenti-con-disabilita-e-dsa/it). The office will advise students of possible adjustments, that will be submitted to the professor for approval 15 days in advance. He/she will evaluate their suitability also in relation to the academic objectives of the course. ). The office will advise students of possible adjustments, that will be submitted to the professor for approval 15 days in advance. He/she will evaluate their suitability also in relation to the academic objectives of the course.

Starting from a score of 27/30 (achieved in the written exam), it is possible to improve the grade through an oral interview (1 question, lasting 10 minutes).

During the oral exam, questions will be asked that may cover all syllabus topics, including those covered in the practical laboratory experiences.

If the preparation is thorough and the candidate demonstrates an excellent ability to independently conduct critical analysis and make connections
between the various topics covered in the course, with full command of terminology and argumentative ability, the
grade will be 30 or 30 cum laude.

Note:

• Students must bring a photo ID or their university badge to the written exam.

• Working students are invited to arrange the exam date with the instructor well in advance.

During the written exam, the use of the following is allowed:

• the periodic table of elements;

• a scientific calculator.

The use of textbooks, notes, or handouts is not permitted.
During the exam, the use of any electronic device other than a calculator is prohibited.

 

IMPORTANT: Your exam grade can be rejected a maximum of two times!

Teaching tools

The slides used during the lectures and the handouts related to the laboratory exercises are provided by the instructor and can be downloaded from the course website (Virtual Learning Environment).

Links to further information

https://www.unibo.it/sitoweb/simone.dagostino2/didattica

Office hours

See the website of Simone D'Agostino