General Chemistry

Code:

EQ102

Acronym:

QGI

Instance: 2005/2006 - 1S

Active?	Yes
Responsible unit:	Department of Chemical and Biological Engineering
Course/CS Responsible:	Chemical Engineering

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
LEQ	98	Plano Oficial EQ a partir 2003	1	4,5	5,5	-

Teaching language

Portuguese

Objectives

-To develop the capacity to use the knowledge as interpretation instrument and intervention in the real.
- To develop the capacities to formulate and to solve problems, of communicating, as well as the memory, the rigidity, the critical spirit and the creativity.
- To promote the thoroughly of a scientific culture, technique and humanistic that constitute cognitive and methodological support so much for the pursuit of studies as for the insert in the active life.
- To contribute for an attitude positive face to the Science.
- To promote the personal accomplishment by means of the development of autonomy attitudes and solidarity.

Program

REVISIONS
1. MATTER: concept; matter types; states of the matter; physical and chemical properties of the matter; precision and accuracy; measurement; manipulation of numbers.

2. ATOMS, MOLECULES AND IONS: the atomic theory; the structure of the atom; quantitative chemical relationships; molecules; ions and ionic compounds; experimental determination of atomic and molecular masses; elementary composition of compounds; nomenclature of the inorganic compounds.

3. CHEMICAL EQUATIONS AND REACTIONS IN AQUEOUS PHASE: chemical equations; properties of the aqueous solutions; precipitation reactions; acid-base reactions; oxidation-reduction reactions.

4. STOICHIOMETRY: QUANTITATIVE CHEMICAL RELATIONSHIPS: amounts of reactants and products; limited reactants; theoretical yield and percentage yield; concentration and dilution of the solutions; gravimetric analysis; acid-base titrations; redox titrations.
NEW MATTER
5. QUANTUM THEORY AND ELECTRONIC STRUCTURE OF THE ATOMS: from the classic physics to the quantum theory; photoelectric effect; theory of Bohr of the hydrogen atom: the duality of the nature of the electron; quantum mechanics; the Schrödinger equation applied to the hydrogen atom; quantum numbers; atomic orbital; electronic configuration; Hund rule.

6. PERIODIC RELATIONSHIPS AMONG THE ELEMENTS: development of the Periodic Table; the periodic classification of the elements; periodic variation of the physical properties; ionization energy; electronic affinity; variation of the chemical properties.

7. CHEMICAL BOND: Lewis notation; the ionic bond; reticular energy of ionic compounds ; the covalent bond; electronegativity; drawing Lewis structures; formal charge and the selection of Lewis structure; the resonance concept when a single Lewis structure fails; exceptions to the octet rule; energy of covalent bond.

8. MOLECULAR ORBITALS AND MOLECULAR GEOMETRY: molecular geometry; dipole moments; valence bond theory; hybridization of atomic orbitals; hybridization in molecules with double and triple bonds; orbital molecular theory; delocalized molecular orbitals.

9. GASEOUS STATE: example of gases; pressure of a gas; the laws of the gases; the equation of the perfect gases; stoichiometry involving gases; the law of Dalton of the partial pressures; The kinetic theory of the gases; the laws of Graham of the diffusion and effusion; deviations to the behaviour of perfect gas.


10. INTERMOLECULAR FORCES, LIQUIDS AND SOLIDS: kinetic theory of liquids and solids; intermolecular forces; the liquid state; crystalline structures; diffraction of X-ray for crystals; types of crystals; amorphous solids; changes of phases.

11. PHYSICAL PROPERTIES OF SOLUTIONS: types of solutions; molecular perspective of the dissolution process; solutions of liquids in liquids; solutions of solids in liquids; units of concentration; effect of the temperature in the solubility; effect of the pressure in the solubility of gases; coligative properties of non-electrolytes solutions; coligative properties of electrolyte solutions.

Mandatory literature

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

Complementary Bibliography

Russell, John B.; Química geral. ISBN: 0-07-450371-5
Chang, Raymond; Química. ISBN: 972-9241-68-6

Teaching methods and learning activities

- The structure of the classes is divided in theoretical classes and theoretical - practices classes, where they are resolved problems and they can also happen brief theoretical exhibitions, or still, presentation of subjects for audiovisual or of small experiences that the knowledge form sediment.
- Consolidation of concepts and basic beginnings with thoroughly of knowledge taught essentially in the 10 and 11st years of the Secondary Teaching.
- Investigation through the macroscopic world as the domain of the microscopic (atoms, molecules) allowing the discussion of the properties and chemical relationships, as well as the analysis of the mechanisms associated to chemical alterations.
- It is done the accomplishment of individual works and in group, dynamically, questioning, making syntheses and allowing information.
- It is fallen back upon the use of work records distributed the students in the beginning of the class for the discussion and resolution of the problems.
- Private attention is given to the analysis capacity and of synthesis, trying to stimulate the creativity and the horizontal integration of knowledge.

Evaluation Type

Distributed evaluation without final exam

Assessment Components

Description	Type	Time (hours)	Weight (%)	End date
Subject Classes	Participação presencial	65,00
	Total:	-	0,00

Eligibility for exams

a) The assiduity to the theoretical and theoretical-practices classes.
b) Interest and diligence in classes.

Calculation formula of final grade

The classification (CF) end is obtained starting from the results of the records and of the tests.

CF = Tests x 0.6 + Records x 0.4

When there are other works, these will enter in the final classification with the value of 20%, being the component of tests and records to be worth 80%.

Examinations or Special Assignments

Possibility of reports or project works to weigh in the mind in face of the level and interest manifested by the students.

Special assessment (TE, DA, ...)

Final exam.

Classification improvement

Final exam

Observations

For the teaching of these contents it will be necessary to appeal to pré-requirements, basic concepts of chemistry essentially of the 10 and 11th years of the Secondary Teaching, that will be consolidated in the own heights and deepened.
That basic knowledge is:
1 - AMOUNT OF MATTER: mole, molar mass and molar volume; chemical formulas; concentration of solutions; chemical equations; calculations based on the chemical equations; the chemical analysis.
2 - STRUCTURES OF THE ATOMS: absorption and light emission for the matter; the emission spectrum of the hydrogen atom and the energy of the respective electron, the effect photoelectric of the electrons in the atoms; ionization energy; Periodic Table and the properties of the metals, metalloids, non-metals and transition elements.
3 - STRUCTURES OF THE MOLECULES: chemical bond in diatomic molecules; chemical bond in polyatomic molecules; properties of the metals.
4 - CHEMICAL EQUILIBRIUM: reversible physical and chemical transformations; balance in homogeneous systems; factors that affect the equilibrium state of a system; practical applications of the beginning of the Chatelier's Principle; balance in heterogeneous systems.
5 - ENERGY IN GAME IN CHEMICAL REACTIONS: reaction heats; the reaction heats and the structure of the reactants and products; electric energy in game in the oxidation-reduction reactions; extension of the chemical reactions and the entropy.
6 - RATE OF REACTIONS: concept of reaction rate; effect of the concentrations of the reactants; chemical reactions at molecular level, mechanisms; effect of the temperature and catalysts in the reaction rate.
7 - REACTIONS OF ACID-BASE: strong and weak acids, monoprotics and polyprotics, pH of the solutions; qualitative characterization of the acid-base balance; reactions between acids and bases in aqueous solution, neutralization.