Fundamentals of Chemistry

Code:

Q1002

Acronym:

Q1002

Level:

100

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2023/2024 - 2S

Active?	Yes
Web Page:	https://moodle2324.up.pt/course/view.php?id=2144
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	Bachelor in Biology

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:B	0	Official Study Plan	3	-	6	42	162
L:CC	0	study plan from 2021/22	2	-	6	42	162
			3
L:F	59	Official Study Plan	1	-	6	42	162
			2
L:G	67	study plan from 2017/18	1	-	6	42	162
			2
L:M	3	Official Study Plan	2	-	6	42	162
			3

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 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

Introduction: Chemistry, the Study of Change.

Stoichiometry: Avogadro's number and concept of mole, molecular and molar masses; elemental composition of compounds; empirical formula, molecular formula and structural formula; chemical reactions and chemical equations; limiting reactant; stoichiometric calculations; chemical reaction yield.

Atoms and Ions: isotopes and ions; electromagnetic radiation; interaction of radiation with matter; wave-particle duality; Heisenberg's Uncertainty Principle; Schrödinger equation; electronic structure and emission spectrum of atomic hydrogen; electronic structure and emission spectra of polyelectronic atoms; periodicity of atomic properties and periodic table of elements.
 
Chemical bonding and molecular geometry: covalent bonding and ionic bonding; Lewis model; Valence Shell Electron Pair Repulsion model (VSEPR); valence bond theory; prediction of molecular geometries; theory of molecular orbitals.

Intermolecular interactions: types of intermolecular interactions: electrostatic interactions, van der Waals interactions; ion-dipole interactions; short-range repulsive interactions and hydrogen bonds; nature of intermolecular interactions: polarity and polarizability; correlation between the value of certain physical properties and the magnitude of intermolecular interactions.

Gases: pressure and temperature of a gas; ideal gas model;equation of state of an ideal gas; Dalton's law of partial pressures; Avogadro's principle; real gas and intermolecular interactions; compressibility factoras a descriptor of the ideality of a gas; van der Waals equation of state.

Thermodynamics (1st principle): thermodynamic systems and their surroundings; work and heat; internal energy; 1st principle of thermodynamics; state functions; standard state, enthalpy; endothermic and exothermic processes; standard molar enthalpies of  formation and of combustion for a chemical substance; standard molar enthalpy of reaction; Hess law; heat capacities.

Thermodynamics (2nd and 3rd principles): entropy and spontaneity; 2nd principle of thermodynamics; interpretative models for the entropy; 3rd principle of thermodynamics; molar and standard molar entropies for a chemical substance; Gibbs' energy and spontaneity; standard molar Gibbs energy of  formation for a chemical substance; molar and standar molar Gibbs energies of reaction.

Chemical equilibrium (general principles): thermodynamic formulation of the chemical equilibrium; alternative forms for expresing the equilibrium constant; variation of the equilibrium constant with temperature; chemical equilibrium and stoichiometry; perturbations of the equilibrium state.

Chemical equilibria in aqueous solution: acid-base equilibria; precipitation equilibria.

Redox equations and electrochemistry: balancing redox equations; galvanic and electrolitic cells; schematic representation of a galvanic cell; standard state in electrochemistry; standard reduction potentials; thermodynamics of cell reactions; Nernst equation.

Physical equilibria: thermodynamic formulation of physical equilibrium; vapor pressure; Clausius-Clapeyron equation; phase diagrams.

 

Mandatory literature

Chang Raymond; Química. ISBN: 972-9241-68-6
Atkins Peter; Chemical principles. ISBN: 0-7167-5701-X

Complementary Bibliography

Chang Raymond; Physical chemistry for the biosciences. ISBN: 1-891389-33-5
Lehninger Albert L.; Biochemistry. ISBN: 0-87901-047-9

Teaching methods and learning activities

Presentation of topics in the theoretical classes.Whenever possible, at the end of the theoretical class, there is a brief practical demonstration followed by a 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

Distributed 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)
Frequência das aulas	49,00
Estudo autónomo	113,00
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.

Classification improvement

At the time of appeal the student will take an overall exam.

Observations

UC jury

Alexandre Lopes de Magalhães
André Alberto de Sousa Melo
Pedro Manuel Azevedo Alexandrino Fernandes