GENERAL AND INORGANIC CHEMISTRY I AND LAB EXPERIENCES 2

Module Module 1

The course introduces the fundamental principles of the atomic structure of matter, chemical bonding, the states of matter, its properties, and transformations. Learning outcomes include a thorough understanding of: i) the atomic model and its application to electronic configurations and the periodic table; ii) the aspects of thermochemistry and kinetics covered; iii) the theory of acids and bases; and iv) chemical equilibrium. The ability to: i) develop Lewis formulas; ii) predict stereochemistry using VSEPR theory; iii) perform stoichiometry calculations (including balancing reactions); VI) Knowledge of the reactivity of compounds

Knowledge and understanding

Knowledge of the physical principles and fundamental concepts of general chemistry, and the chemistry of s-p elements in relation to their electronic and structural properties.

Ability to apply knowledge and understanding

At the end of the course, students will be able to apply the knowledge acquired to problems of practical interest, often related to both basic research and processes of industrial interest.

Making judgments

Students will be able to process what they have learned and recognize "real-world" cases and specific problems in which the learned chemical principles can be applied.

Communication skills

Develop the ability to express themselves using appropriate terminology, both verbally and in writing. Group discussions and the ability to arrive at a conclusion through a process of synthesis of the contributions emerging from the discussion will be encouraged during the exercises. At the end of the course, students will be able to describe the topics of general and inorganic chemistry with language proficiency and confidence in their presentation.

Learning ability

Learning ability. At the end of the course, students will be able to analyze, apply, and integrate the knowledge acquired with what will be learned in subsequent courses, with particular reference to scientific disciplines based on aspects and processes governed by chemical-molecular phenomena.

Frontal lessons in the classroom, supported by slides, in which exercises will be carried out to consolidate the quantitative aspects of general chemistry. The teaching is held in Italian.

To ensure equal opportunities and in compliance with current laws, interested students can request a personal interview in order to plan any compensatory and/or dispensatory measures, based on the educational objectives and specific needs. It is also possible to contact the CInAP (Center for Active and Participatory Inclusion - Services for Disabilities and/or DSA) referent teachers of our Department.

If the conditions require the delivery of teaching in mixed or distance mode, the necessary changes may be introduced with respect to what was previously declared, in order to respect the planned program and reported in the syllabus.

Introduction to chemistry - Matter and its states of aggregation*, the scientific method, the three levels of chemistry, matter and its units of measurement*, significant figures, pure elementary substances* and compounds* and homogeneous* and heterogeneous mixtures*. Chemical nomenclature* - Elements* and their representation, oxidation number*, classification of inorganic compounds*, ionic* and molecular compounds*, traditional nomenclature* and IUPAC.* Chemical reactions* - Representation*, Lavosier's law of conservation of mass*, balancing*, combustion reactions, precipitation reactions,* reactions that develop gas, acid-base reactions*, redox reactions* and their balancing*.

Atom Generalities- Rutherford experiment, planetary atomic model, atomic number*, mass number*, isotopes*, isotopic abundance, mass defect, atomic mass unit* (amu), relative atomic mass*, molecular mass*, mole*, minimal formula*, molecular formula*, extended formula, structural formula, weight percentages.

Structure of matter- Bohr atomic model,* quantum mechanical model, quantum numbers, Pauli principle,* Hund's rule*, electronic configuration*.

Periodic table- Periodicity*, atomic radius,* ionic radius, ionization 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,* dative bond,* hydrogen bond,* valence orbital theory,* hybridization, resonance.

The gaseous state- Pressure*, Boyle's law, Charles's law, Gay-Lussac's law, Avogadro's hypothesis, the ideal gas law*, gas mixtures and Dalton's law*, kinetic-molecular theory*, Graham's law, real gases*.

The liquid state- Properties, viscosity, surface tension and vapor pressure.* State transitions- Water state diagram*

Thermodynamics- State functions, first law*, second law*, entropy* and 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 coefficient

Chemical equilibrium*-Law of mass action*, equilibrium constant*, dependence of the equilibrium constant on Temperature, factors that influence equilibrium*. Acids and bases*- Strength of acids and bases, dissociation constant*, amphoteric electrolytes, ionic product of water*, pH calculation*, pH indicators. Salt hydrolysis- Hydrolysis constant, pH of hydrolysis, Buffer solutions*, strong acid-strong base titrations*, , solubility product*, effect of the common ion on solubility.

Notes on chemical kinetics-order and molecularity of reaction, reaction rate*.

Notes on electrochemistry - conductivity of aqueous solutions*, batteries, redox potential series, Nerst equation.

Inorganic - The elements of the sp* group: presence in nature, preparation of the elements and their chemical properties, binary and ternary compounds. Notes on the chemistry of transition metals ‘d’ and ‘f’.

Organic - Properties and reactivity of aliphatic and aromatic hydrocarbons, alcohols, aldehydes and ketones, carboxylic acids and their derivatives*

STOICHIOMETRY

Stoichiometry: Stoichiometry of chemical reactions. Chemical reactions. Chemical equations and their balancing. Stoichiometric calculations. Percentage composition and elemental analysis. Yield of reactions and limiting agent. Reactions in aqueous solution. Net ionic equations. Concentration expressions. Dilution. Oxidation-reduction and their balancing

1) Petrucci, Herring, Madura, Bissonnette - Chimica Generale-Principi ed applicazioni moderne

2) M Schiavello, L. Palmisano - Fondamenti di Chimica - EdiSes 

N.B.: Although the lessons are based on 1 or 2 texts for each section, it should be noted that all the texts listed above are equally valid and the student is free to choose the one he/she deems most suitable for his/her training. The 

Any texts not listed can be submitted to the teacher for examination.

The final exam consists of a two-hour written exam (the exam date is the one indicated on the official calendar). The exam is based on a sufficient number of open-ended questions to cover all the topics covered in class, including the stoichiometry exercises and the nomenclature and reactivity of organic molecules covered during the course. Only those who pass the written exam will be admitted to the oral exam. The final grade will be the average of the written and oral scores.

The grade follows the following scheme:

Not suitable:

Knowledge and understanding of the topic: Important deficiencies. Significant inaccuracies

Analysis and synthesis skills: Irrelevant. Frequent generalizations. Inability to synthesize

Use of references: Completely inappropriate

18-20:

Knowledge and understanding of topic: At threshold level. Evident imperfections

Analysis and synthesis skills: Barely sufficient ability

Use of references: Barely appropriate

21-23

Knowledge and understanding of topic: Routine knowledge

Analysis and synthesis skills: Is capable of correct analysis and synthesis. Argues logically and coherently

Use of references: Uses standard references

24-26

Knowledge and understanding of topic: Good knowledge

Analysis and synthesis skills: Has good analysis and synthesis skills. The topics are expressed coherently

Use of references: Uses standard references

27-29

Knowledge and understanding of the topic: More than good knowledge

Analysis and synthesis skills: Has notable analysis and synthesis skills

Use of references: Has studied the topics in depth

30-30 cum laude

Knowledge and understanding of the topic: Excellent knowledge

Analysis and synthesis skills: Has notable analysis and synthesis skills.

Use of references: Important insights.

Chemical nomenclature

Describe the periodic properties of the elements

Electronic configuration of the elements and atomic number

Molecular geometry of inorganic acids based on the VSEPR theory

VB theory and hybrid orbitals

Chemical bonding

Reaction balance

Redox reactions

Intermolecular interactions

Solutions

Calculating the concentration of a solution

Colligative properties

Main thermodynamic state functions

Gibbs energy

Chemical kinetics

Solution equilibria

Calculating pH

Buffer solutions

Hydrolysis of salts