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Presentation
Presentation
Field of action: Understand the fundamental principles and concepts of physical chemistry, including gas laws, thermodynamic laws, and chemical equilibrium. Field of activity: Interpret and explain the behaviour of chemical systems and the properties of matter in different states. Integrate the concepts covered with a focus on application and illustration of real examples. Intervention: Apply the knowledge acquired and physical chemistry principles to solve problems and analyse biomedical scenarios. Analyse and evaluate experimental data and observations to draw meaningful conclusions about chemical processes. Integrate various physical chemistry concepts to propose solutions to more complex problems. This CU constitutes a relevant knowledge base for progression in training and future professional practice. It assists in the critical evaluation of problems and the analysis of scientific literature and research on topics related to physical chemistry.
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Class from course
Class from course
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Degree | Semesters | ECTS
Degree | Semesters | ECTS
Bachelor | Semestral | 5
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Year | Nature | Language
Year | Nature | Language
1 | Mandatory | Português
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Code
Code
ULHT7037-16914
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Prerequisites and corequisites
Prerequisites and corequisites
Not applicable
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Professional Internship
Professional Internship
Não
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Syllabus
Syllabus
Description of contents Particle mechanics revisited Review of forces, motion, work and energy Introduction to Physical Chemistry. Scope and basic concepts Basic concepts, states of matter, gases, phase transitions Chemical Thermodynamics and Biochemistry Laws of thermodynamics, thermodynamic potentials, and applications. Atomic structure, intermolecular forces and chemical bonding Chemical bonding, molecular geometry Chemical kinetics Reaction rates, order and molecularity, enzyme kinetics Chemical equilibrium: acid-base equilibrium Acids and bases, pH scales Solutions and Colloids Solutions and colloids, colligative properties. Electrochemistry Redox equations, active and passive transport, sodium and potassium pump Introduction to Quantum Chemistry Molecular Symmetry Spectroscopy and Analytical Techniques Introduction to Biophysical Chemistry Introduction to Computational Chemistry.
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Objectives
Objectives
This course aims to continue the content discussed in the previous semester's general chemistry course and to explore some fundamental topics in physical chemistry in greater depth, namely, topics in the area of equilibrium such as equilibrium thermodynamics, chemical equilibrium, equations of state, and the concept of thermodynamic potential. Fundamental concepts on the structure of matter and atomic and molecular interactions will also be addressed, as well as basic knowledge of molecular symmetry and spectroscopic techniques. From a more evolutionary perspective, principles of chemical kinetics will be discussed. Whenever possible, the skills that students acquire are linked to biological and biomedical systems.
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Teaching methodologies
Teaching methodologies
In the theoretical component classes, in addition to introducing the fundamental concepts and relationships in each chapter, 'Case Studies' are analysed, based on concrete systems and focusing on solving practical issues related to the concepts or relationships discussed previously. In some classes that conclude a chapter or subchapter, students are challenged to take a conceptual quiz focused on understanding the basic concepts. About the practical application and mastery of the process of solving concrete problems, students are challenged to solve a set of proposed exercises in class, and those that are not solved in class due to different speeds of execution can be solved by students at home and self-corrected. In certain chapters, students will conduct research and present group work. The work is developed throughout the semester, integrating the knowledge that is being taught.
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References
References
Serway, R.A. & Jewett, J.W., Physics for Scientists and Engineers, Vol.1, 10th Edition. Cengage Learning, 2018. ISBN: 9781337553278 Atkins, P., de Paula, J., & Keeler, J., Physical Chemistry, 11th Edition. Oxford University Press, 2017. iSBN :9780198769866 Chang, R., Physical Chemistry for the Chemical Sciences, 2nd Edition. University Science Books, 2000. ISBN: 1891389068
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Assessment
Assessment
Avaliação Contínua:
1) Dois testes durante o semestre, cada um com ponderação de 40% para a nota final de avaliação contínua e com nota mínima de 6 em cada teste. Possibilidade de recuperação de um dos testes ou de realização de uma prova global no final do semestre, caso a média dos testes juntamente com o trabalho autónomo não atinja o requisito mínimo de aprovação ou algum dos testes tenha nota mínima inferior a 6 valores.
2) Média das notas da componente de trabalho autónomo avaliado realizado pelos estudantes. Esta componente não tem nota mínima e tem ponderação de 20%. Nesta componente estão incluídos problemas propostos para entrega, análise de papers e apresentação de trabalhos, quizzes, trabalhos práticos de laboratório e correspondentes relatórios.
Exemplo:
Descrição
Data limite
Ponderação
Teste de avaliação 1
Data a definir
40%
Teste de avaliação 2
Data a definir
40%
Recuperação de um dos testes
data a definir
Para a média conta a melhor nota
Prova Global (substitui sempre a nota dos testes feitos anteriormente) Data a definir 80% e substitui os testes Vários elementos de trabalho autónomo avaliado a indicar ao longo do semestre A definir 20 % (média) A nota final por avaliação contínua é calculada como a média ponderada dos itens de avaliação de acordo com a seguinte fórmula:
Nota final = 0.40 * F1 + 0.40 * F2 + 0.20*TA
Para que haja aprovação à Unidade Curricular, a Nota Final não pode ser inferior a 9,5 valores e a média aritmética das duas frequências não pode ser inferior a 8,0 valores, com nota mínima individual de 6 valores em F1 e F2 .
2. Avaliação não contínua:
Os alunos podem optar por realizar o exame final com ponderação de 100%, sendo necessária uma nota mínima de 9,5 valores para a aprovação.
NOTA MUITO IMPORTANTE: Todos os elementos de avaliação escritos referidos anteriormente (testes, prova global, exame, relatórios, quizes, etc) implicam sempre a realização de uma prova oral associada e a nota desse elemento de avaliação é a média da prova escrita com a oral correspondente. Caberá aos docentes decidir em cada momento de avaliação se a oral é realizada. Caso a oral não seja realizada, a componente escrita corresponderá à totalidade da nota nesse momento de avaliação.
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Mobility
Mobility
Yes
