Chemistry I

Code:

Q1009

Acronym:

Q1009

Level:

100

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2022/2023 - 1S

Active?	Yes
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	Bachelor in Chemistry

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:BQ	121	Official Study Plan	1	-	9	70	243
L:Q	51	study plan from 2016/17	1	-	9	70	243

Teaching language

Portuguese

Objectives

The course "Química I (1st year, 1st semester) is the first chemistry course in the Chemistry and Biochemistry B.Sc's. The main objective is to provide a solid understanding of the essential chemistry concepts necessary for further applications in other more specialized courses and multidisciplinary courses.

The program covers the general principles about atoms and molecules, constituents of matter, their transformations, either by chemical reaction or by phase transition, and also the thermodynamic principles that govern these transformations of matter and energy associated with them.

Learning outcomes and competences

Ability to apply concepts acquired in practical situations. Ability to analyze simple chemical situations and select the necessary tools to obtain additional chemical information.
The main objective is that the students will be able to identify and interpret simple problems in general chemistry. The presentation and discussion of the topics in the theoretical classes followed by classes where the students solve problems with the assistance of the professor allows them to acquire the necessary knowledge and problem solving skills.

Working method

Presencial

Program

1. Chemistry: the study of matter and its transformation
Matter and energy; physical and chemical, intensive and extensive properties of matter; physical and chemical changes; the scientific method; Measurement in science and significant figures; physical quantities and SI units.
2. Atoms, molecules and ions
Atomic Theory; Structure of the atom; Isotopes and elements; Periodic table; Monatomic ions, ionic and molecular compounds; Chemical formulas and nomenclature of inorganic compounds.

3. Stoichiometry
Atomic mass and Avogadro's constant; Molecular mass; Chemical reactions and stoichiometry; reaction yield.

4. Reactions in aqueous solution
General properties of aqueous solutions; main type of reactions in aqueous solution; precipitation reactions, acid base reactions, oxidation-reduction reactions.

5. Gases
The gas laws; equation of state of an ideal gas; Mixtures of gases: Dalton laws; kinetic theory of gases; deviations from ideality

6. Energy, Enthalpy and Thermochemistry
Nature and types of energy;  Work, heat and internal energy; Introduction to Thermodynamics; the 1st Principle of Thermodynamics; calorimetry; standard enthalpies of formation and of reaction; Hess´s law

7.Quantum theory and electronic structure of atoms
Quantum theory; Photoelectric effect; dual nature of the electron; quantum numbers; orbital quantum numbers, obtained from solving the Schrodinger equation; atomic orbitals and their spatial visualization; electronic configuration of chemical elements and construction of the Periodic Table.

8. Periodic relations between the elements
The Periodic Table; periodic variation of physical properties; ionization energy and electron affinity; variation of the chemical properties of representative elements

9. Chemical Bonding, an introduction
Lewis notation; ionic bond; covalent bond; electronegativity; Formal charge and Lewis structure; resonance; Exceptions to the octet rule; molecular geometry; dipole moment. Valence bond theory (brief reference); multiple bonds-sigma and pi-type bonds,

10. Intermolecular Forces-liquids and solids,
Intermolecular forces, their nature and magnitude; main physical states of matter; physical properties of liquids: viscosity and surface tension; types of interactions in crystalline (crystalline structures will be discussed in Chemistry II), semi-crystalline and amorphous solids and a brief reference to some of their physical properties

11. Spontaneity , Entropy and Gibbs energy
Entropy: Spontaneity and Equilibrium in Chemical Reactions and Physical Processes - 2nd and 3rd Laws of Thermodynamics; Gibbs energy of the system as a criterion for transformation spontaneity, at constant temperature and pressure; spontaneity and coupling of biological processes.molar Gibbs energy of a pure substance, its variation with pressure and temperature; equilibrium phases and phase transitions, mesophases - thermotropic liquid crystals; phase diagramsof pure substances; water, a unique substance.The standard Gibbs energy and the equilibrium constant. Determining the standard Gibbs energy of a reaction from standard Gibbs energies of standard formation of reactants and products.

12. Physical properties of the solutions
Types of solutions; molecular and thermodynamic view of the dissolution process; effect of temperature on solubility; effect of pressure on solubility of gases in liquids; colligative properties of solutions of non-electrolytes and electrolytes; macromolecules in water- micelles, lamellar phases and cell membranes

Mandatory literature

Chang Raymond; Química. ISBN: 84-481-4527-5
Chang Raymond e Goldsby Kenneth; Química, McGraw Hill, 2013. ISBN: 978-97172-7-5

Complementary Bibliography

Atkins Peter William 1940-; Chemical principles. ISBN: 0-7167-3596-2

Teaching methods and learning activities

Teorethical classes are essentially lectures. The support materials are available to students in the course platform.

A set of issues/problems are discussed/solved in the theoretical-practical classes

keywords

Physical sciences > Chemistry

Evaluation Type

Distributed evaluation with final exam

Assessment Components

designation	Weight (%)
Teste	50,00
Exame	50,00
Total:	100,00

Amount of time allocated to each course unit

designation	Time (hours)
Estudo autónomo	173,00
Frequência das aulas	70,00
Total:	243,00

Eligibility for exams

The students must have no more absences than 1/4 of the total number of the theorethical-practical classes.

Calculation formula of final grade

The  evaluation is the average of the grade obtained in TWO tests: T1  during the semester, and T2 will take place during the normal examination period.


NF = (T1+T2)/2

Examinations or Special Assignments

Exam

Special assessment (TE, DA, ...)

Working students may opt for a comprehensive examination.

Classification improvement

Examination of appeal