Fundamentals of Chemistry

Code:

Q1014

Acronym:

Q1014

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2022/2023 - 2S

Active?	Yes
Web Page:	https://moodle.up.pt/course/view.php?id=243
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	Bachelor in Physics

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:F	66	Official Study Plan	1	-	6	48	162

Teaching language

Suitable for English-speaking students

Objectives

The main objective of this course is to show the importance of Chemistry and its pervasive influence in other branches of Science. For that, fundamental topics will be addressed that allow students to understand the structure and properties of matter and to interpret the phenomena of chemical transformation.

Learning outcomes and competences

At the end of this course students are able to:

• Acknowledge that all matter is made up of atoms and that the immense variety of materials that occurs in the Universe is a consequence of different ways the atoms are able to link to each other.
• Know the principles of atomic structure and interpret the periodic table of chemical elements.
• Know the basics of valence bond theory and predict molecular geometry.
• Understand the basis of stoichiometry and the thermodynamics of chemical reactions.
• Identify different types of chemical reactions and put them in the context of a wide variety of phenomena observed in Nature.
• Describe the main interactions between molecules and relate them to the macroscopic physical properties of substances.
• Solve quantitatively and discuss critically a set of selected problems related with specific areas of chemistry.
• Know how to extrapolate the knowledge acquired in this course and apply it in other contexts.

Working method

Presencial

Program

Chemistry, the Study of Change

Atoms, Molecules, Ions and Chemical reactions: the structure of atoms, the periodic table; from the atom to molecules and ions;inorganic nomenclature; mass relationships in chemical reactions.
 
Chemical bonding, molecular geometry and carbon compounds: the Lewis model, covalent bonding and molecular geometry; hybridization of atomic orbitals in carbon compounds; main families of organic  compounds; natural polymers-proteins, lipids, nucleic acids

Stoichiometry: Avogadro's number and molar mass of an element; mass percentage composition ; chemical reactions and chemical equations; relation of masses in chemical equations; limiting reactant.

States of matter and intermolecular interactions: Gases: ideal gas equation, Dalton´s law of partial pressures, real gas equation of van der Waals; Intermolecular interactions in liquids and solids.

Thermodynamics: internal energy and 1st Law; enthalpy and thermochemistry; entropy , 2nd and 3rd Laws.; Gibbs energy, spontaneity of a reaction and chemical equilibrium.

Physical equilibria: properties of solutions: Types of solutions; phase transitions; phase diagrams; hydrofobic effect.

Chemical equilibria: chemical reactions in equilibrium; equilibrium constant and thermodynamics; response of equilibria to changes in experimental conditions.

Acid base equilibrium in aqueous solution; acid and bases concept; pH scale; strength of acids and bases; buffers; acid-base titration.

Electrochemistry.: redox reactions; standard reduction potentials; galvanic cells; spontaneity of redox reactions; Nernst equation. Illustration of the importance of electrochemistry in industry and technology. 

 

Mandatory literature

Peter William Atkins; Chemical principles. ISBN: 0-7167-3596-2

Teaching methods and learning activities

Presentation of topics in the theoretical classes. Once a week, at the end of the theoretical class there is a simple practical demonstration followed by discussion of the observed phenomena. 

Practical classes where the students solve quantitative problems.

B-learning component is implemented by means of the Moodle digital platform, where the students have access to texts, videos and interactive exercises. 

keywords

Physical sciences > Chemistry

Evaluation Type

Evaluation with final exam

Assessment Components

designation	Weight (%)
Exame	100,00
Total:	100,00

Amount of time allocated to each course unit

designation	Time (hours)
Estudo autónomo	114,00
Frequência das aulas	48,00
Total:	162,00

Eligibility for exams

The students must attend at least 3/4 of the number of practical classes planned for the academic semester.

Calculation formula of final grade

T1 and T2 are two assessment tests that correspond roughly to two halves of the course syllabus. These tests are taken during both exam periods. The final grade, NF, is obtained by the average of T1 and T2 (NF = 0.50 T1 + 0.50 T2), in which T1 and T2 are the best classification obtained by the student in each assessment test.