General Chemistry

Recommended Prerequisites

Physics and Chemistry A (High School). 

Teaching Methods

The teaching methodology includes T, TP and PL classes.

In T classes is taught the programme of the discipline, with the aid of notes in the form of photocopies and electronically, as well as audio-visual aids. The aim of TP classes, always with the active individual participation of the students, is to reinforce the students’ knowledge acquired in T classes through problem solving.

The objectives of the PL classes are to illustrate the concepts shown in T classes, illustrate the chemical and physical phenomena discussed and demonstrate how chemistry is an experimental science.     

Learning Outcomes

The principal objective is to learn the fundamentals of chemistry necessary for the future curricular units in the Bachelor in Chemical Engineering in relation to its chemistry and engineering aspects.

Specific objectives including learning the fundamentals of chemical bonding, the composition of matter (gas, liquid and solid phases), thermodynamics and kinetics of chemical reactions and processes.

Competences to be developed are:

- Knowledge and capacity for comprehension: recognise and use theories and concepts, analyse and summarise information

- Application of knowledge and comprehension: apply concepts to solve problems, know how to undertake laboratory practical work in safety conditions

- Perform judgements / take decisions: process and interpret quantitative data

- Communication: understand and use information sources, transmit acquired knowledge adequately

- Self-learning competences: develop competences sufficiently to be autonomous.

Work Placement(s)

No

Syllabus

Revision of concepts: fundamental quantities and units; types of errors. Introduction to the chemical laboratory.

Periodic Table.

Atomic electronic structure and quantum theory. Schrödinger equation. Atomic and molecular orbitals. Electronic configurations and periodic classification.

Ionic and covalent bonds. Valence theory and molecular orbitals; hybridization. Electronegativity. Intermolecular forces. Polarity and dipole moment. Molecular geometry.

The gaseous state: perfect and real gases, gas mixtures. The liquid state: properties, liquids as solvents. The solid state: Properties, types of solid and structures, defects

Chemical thermodynamics: Energy and enthalpy; Hess’s law, Born-Haber cycles.. Enthalpies of formation and reaction. Entropy and absolute entropy. Chemical potential and free energy. Chemical equilibrium: response to changes in temperature, pressure and concentration; phase diagrams

Chemical kinetics: Reaction order and molecularity; rate constants. Catalysis - hom.

Head Lecturer(s)

João Manuel Ferreira Pita Batista Pina

Assessment Methods

Assessment
Mini Tests: 20.0%
Laboratory work or Field work: 20.0%
Exam: 60.0%

Bibliography

Chang, R. Química, 11ª ed., McGraw Hill, NY, 2012.

Chang R., Overby J., Chemistry, 13ª ed., McGraw Hill, NY, 2019.

Burdge J., Chemistry, 5ª ed., McGraw Hill, NY, 2020.

Atkins, P., Jones, L. Chemical Principles. The Quest for Insight, 5ª ed., Freeman, NY, 2010.

Kotz, J.C., Treichel, P. Chemistry and Chemical Reactivity, 10ª ed., Brooks Cole, EUA, 2019.