Chemistry

Code:

Q1007

Acronym:

Q1007

Level:

100

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2017/2018 - 2S

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

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:CTA	63	Plano estudos a partir do ano letivo 2016/17	1	-	6	56	162

Teaching language

Portuguese

Objectives

Learning outcomes and competences

Ability to apply knowledge obtained in real situations. Ability to understand simple chemical problems and to use chemical tools for understanding chemical systems.

Working method

Presencial

Program

Chemistry, the study of transformation: matter, physical and chemical properties and transformation

Atoms, molecules, ions: atomic theory, structure of the atom, the periodic table. Molecules and ions, chemical formulas and compound nomenclature.

Mass relations in chemical reactions: atomic mass, molecular mass, chemical reactions and chemical equations, limiting reactants and reaction yields.

Gases: Pressure of a gas, ideal gas equation of state; Dalton's Law of Partial Pressures; Molecular kinetic theory of gases, real gases and van der Waals' equation of state.

Thermochemistry: types of energy, energy variations in chemical reactions, enthalpy and thermochemistry; Standard enthalpy of formation and reaction, heats of reaction.

Quantum theory and electronic structure of atoms: from classical physics to quantum theory; photoelectric effect; Bohr's theory of the hydrogen atom; Duality of the nature of the electron; Quantum numbers; Orbitals, electronic configuration

Periodic relations between the elements: development of the Periodic Table; Periodic classification of the elements; Periodic variation of physical properties; Ionization energy; Electronic affinity

Chemical bonding, basic concepts: Lewis symbols; Ionic bonding; Network energy of ionic compounds; covalent bond; Electronegativity; Formal charge and Lewis structure; Concept of resonance; Exceptions to the octet rule;
Molecular geometry; Dipole moments; Theory of valence bonding.

Intermolecular, liquid and solid forces: Molecular kinetic theory of liquids and solids; Intermolecular forces; Properties of liquids.

Physical properties of solutions: Types of solutions; Molecular approach to the dissolution process; Concentration units; Effect of temperature on solubility; Effect of the pressure on the solubility of the gases.

Chemical equilibrium: Concept of equilibrium and equilibrium constant; Expressions for the equilibrium constant; Relationship between chemical kinetics and chemical equilibrium; Factors that affect the chemical balance.


Pratical activities at the laboratory.

Mandatory literature

Raymond Chang e Kenneth A. Goldsby; Química, AMGH EDITORA LTDA, 2013. ISBN: 0073402680 / 9780073402680

Teaching methods and learning activities

Theoretical classes essentially expositive. Support materials are made available to students on the course platform. A set of laboratorial activities are done in practical classes

Evaluation Type

Distributed evaluation with final exam

Assessment Components

designation	Weight (%)
Exame	75,00
Trabalho prático ou de projeto	25,00
Total:	100,00

Calculation formula of final grade

The assessment of knowledge will be done through a mandatory final exam and by the student's performance in the practical classes. The final grade will be calculated by: 0.75 x exam mark + 0.25 x mark practice

The student can dismiss the final exam by performing two tests (T1, T2) throughout the semester, provided that the final grade calculated (according to 1) from the arithmetic mean of both tests and the practical note, is positive. Performing these tests is optional.

The final exam of the normal period will consist of two modules corresponding to the subject of the tests referred to in point 2. Students who have carried out the tests provided for in point 2 may choose to carry out the modules that best fit the final exam of the normal period, Sense of improving classification. The final grade of this exam will be obtained through the arithmetic mean of the classifications obtained in the two modules. In the case of students who have opted to take the test and then repeat the module under examination, the note considered will be the more favorable of the two.

The final exam of the period of recourse and special time will involve all the subjects taught. The final classification will be obtained from the note obtained by the student in this exam and the practical note.