General and Inorganic chemistry with Basics of Organic Chemistry

Module General and Inorganic Chemistry

Candidates should be able to demonstrate knowledge and understanding of:  scientific phenomena, facts, laws, definitions, concepts and theories • scientific vocabulary, terminology and conventions (including symbols, quantities and units).

Furthermore, in reference to the so-called Dublin Descriptors, this course helps to acquire the following transversal skills.

Candidates should be able, in words or using other written forms of presentation (i.e. symbolic, graphical and numerical), to:

• locate, select, organise and present information from a variety of sources

• translate information from one form to another

• manipulate numerical and other data

• present reasoned explanations for phenomena

• make predictions and hypotheses

• solve problems, including some of a quantitative nature.

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

Should the circumstances require online or blended teaching, appropriate modifications to what is hereby stated may be introduced, in order to achieve the main objectives of the course.

The particular nature of the matter- Stoichiometry - Determination of relative atomic mass and relative molecular mass of atoms, molecules, and ions. Chemical equations and calculations based upon stoichiometry and the mole concept. Avogadro's hypothesis and calculations based on these concepts. Dalton's Law of partial pressures. Atomic structure and periodicity - A detailed understanding of the periodic table and the structure of the elements with reference to electron configuration, use of the periodic table to predict properties of elements and bonding behavior. General trends in ionization energies, electron affinities, etc. Bonding - The nature of covalent and ionic bonds, and the properties of compounds exhibiting these types of bonding. Simple Lewis structures and VSEPR theory. Oxidation and Reduction - Common oxidizing and reducing agents, balancing redox equations, the concept of oxidation number.  Gases and gas laws - Properties and behavior of ideal gases. Liquids. Solids. Changes of State. Chemical Equilibrium - Equilibrium constants, simple problems on gas equilibria, including the application of Le Chatelier's Principle. Simple equilibria in solution. Catalysis and rates of reaction. Acids bases and pH - Concept of Lowry Bronsted acids and bases, Kw, pH, pKa, pKb. Calculations based upon pH for simple systems. Main group elements sp - A basic systematic knowledge of the chemistry of main group elements.

TESTI DI RIFERIMENTO

T1. J.C. Kotz et al. - Chimica – EdiSES T2. P.W. Atkins, L. Jones - Chimica Generale - Zanichelli

The use of other textbooks is allows after evaluation of the Professor

The exam consists of a written test and, in case of a favorable outcome, a subsequent oral interview. The written test consists of numerical exercises and open and/or multiple choice questions to be completed in 2 hours. Textbooks, forms, course notes or periodic tables are not permitted in the written test, nor is the use of a mobile phone, not even in calculation mode. Only the use of a calculator is permitted. The student must present himself with a valid identity document.

Those who have passed both ongoing tests are exempt from the written exam of the first session.

The verification of learning can also be carried out electronically, should the conditions require it.

Examples of questions in the written test:

Write the formula of the following compounds: aluminum nitrate; hydrogen sulfide; sulfur dioxide; calcium nitrate; calcium hydroxide; sulfur hexafluoride, magnesium carbonate, sodium sulfide.

A gas in a closed container has a pressure of 20 atm at a temperature of 0°C. Calculate the pressure of the gas when it is heated to 100°C.

Balance the following oxidation-reduction reaction which occurs in acidic solution: MnO4- +SO2→Mn2+ + SO42-

Balance the given reaction and answer the following questions: How many grams of H2 are obtained from the reaction of 120 g of CaH2 with an excess of water? What mass of CaH2 must react with excess water to produce 28.3 g of H2?

Knowing that 11 g of an organic compound with the formula C12H10 that dissolves (without dissociating) in 100 g of benzene the boiling temperature rises by 1.8 °C, calculate the molal ebullioscopic constant Keb of benzene.

Calculate the pH of an aqueous solution obtained by dissolving 1.20 g of HCl in 500 mL of water.

Calculate the pH of a 0.056 M solution of acetic acid CH3COOH knowing that it is a weak acid and that its Ka = 1.8 × 10-5.

Calculate the molar solubility of CaCO3, Kps= 8.7 × 10-9

Examples of frequently asked questions during the oral test:

Describe an atomic model

Describe the dual nature of light and matter

Describe quantum numbers

Explain the octet rule and list some exceptions

State the VSEPR Theory and detail the molecular geometry of water and ammonia.

Explain the difference between compounds and mixtures.

Describe the solutions and their properties.

Describe the states of aggregation of matter and their properties.

Explain thermodynamically when a process can be defined as spontaneous.

Explain the amphoteric nature of water.

Influence of acids and bases on the pH of a solution.