Fundamentals of Chemistry

Code:

EQ102

Acronym:

EQ102

Keywords
Classification	Keyword
OFICIAL	Basic Sciences

Instance: 2018/2019 - 2S

Active?	Yes
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	First Degree in Engineering Sciences

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:CE	21	PE2007- Perfil Engenharia Alimentar	1	-	7,5	-
		PE2007- Perfil Engenharia Agronómica	1	-	7,5	-

Teaching language

Suitable for English-speaking students

Objectives

It is intended to enable students with knowledge about some essential principles and concepts of Chemistry, as well as how to apply this knowledge in practical situations.

Learning outcomes and competences

As a result of learning, students should be able to continue their studies in more advanced Chemistry disciplines or in need of fundamental Chemistry knowledge.

Working method

Presencial

Program

1 - Chemistry: The study of matter and its transformations
Matter and energy; Physical and chemical, intensive and extensive properties of matter; physical and chemical transformations; Scientific method; Measurement in science and significant figures; Physical quantities and SI units;
 
2 - Atoms, Molecules and Ions
Structure of the atom; Isotopes and elements; Periodic table; Monatomic ions, ionic compounds; Chemical formulas and nomenclature of inorganic compounds.

3 - Stoichiometry
Atomic mass, Avogadro's number and molecular mass; Chemical reactions and stoichiometry; Yield of chemical reactions.

4 - Reactions in Aqueous Solution
Properties of aqueous solutions; Reactions of precipitation, acid-base, and oxidation-reduction.

5 - Gases
The laws of gases; state equation of ideal gases; Gas mixtures: Dalton's laws; kinetic theory of gases; deviations from ideality - some state equations for real gases.

6 - Thermochemistry
Nature and types of energy; Work, heat and internal energy; Introduction to Thermodynamics; the 1st Principle of Thermodynamics; Calorimetry; Enthalpy; Standard states; Enthalpy pattern formation and reaction

7 - Intermolecular Forces and Liquid and Solid 
Intermolecular forces; Properties of liquids; Crystalline structure; Types of crystals; Amorphous solids; Phase changes; Phase diagrams.

8 - Physical Properties of Solutions
Types of solutions; Effect of temperature on solubility; Effect of pressure on gas solubility; Colligative properties of non-electrolyte solutions; Colligative properties of electrolyte solutions.

9 - Chemical Kinetics
Rate ​​of reaction and its dependence on concentrations and time; Activation energy and specific rate variation with temperature; The law of Arrhenius; Influence of temperature on food degradation; Reactions mechanisms; Catalysis.

10 - Chemical Equilibrium
Concepts of equilibrium and of equilibrium constant; Relationship between kinetics and chemical equilibrium; Factors affecting chemical equilibrium.

11- Acids and Bases
Bronsted acids and bases. Acid-base properties of water. PH as a measure of acidity; Force of acids and bases and ionization constants; Diprotic and polyprotic acids; Acid-base properties of salts, oxides and hydroxides.

12 - Acid-Base Equilibria and Solubility Equilibria
Homegeneral equilibria versus heterogeneous equilibria in solution; Effect of common ion and solubility: buffer solutions; Acid-base titrations; Solubility equilibrium.

13 - Entropy, Gibbs Energy and Equilibrium
The three laws of thermodynamics; Spontaneous processes and reversible processes; Entropy; The second law of thermodynamics; Gibbs energy and chemical equilibrium; The third law of thermodynamics.

14 - Nuclear Chemistry and Radioativity
Nature of nuclear reactions; Nuclear stability and natural radioactivity; Nuclear transmutation; Nuclear fission; Nuclear fusion; Applications of radioactive isotopes - Food irradiation; Biological effects of radiation.

Mandatory literature

Chang Raymond; Química. ISBN: 84-481-4527-5
Chang Raymond e Goldsby Kenneth; Química, 11ª edição, McGraw-Hill, 2013. ISBN: 978-989-97172-7-5

Complementary Bibliography

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

Teaching methods and learning activities

Theoretical classes are essentially expositive. Support materials are made available to students on the MOODLE platform.
Several questions / exercises are discussed / solved in theoretical-practical classes

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)
Frequência das aulas	28,00
Total:	28,00

Eligibility for exams

In order to obtain frequency, the maximum number of absences in theoretical-practical classes (1/4 of the number of classes planned) can not be exceeded.
Students with a valid frequency in the previous school year may, at their request, be exempted from attending TP classes.

Calculation formula of final grade

Normal Season:
NF = [(T1 or E1) * + (T2 or E2) **] / 2
Where N1 and N2 represent the 1st and 2nd marks (optional), respectively, and E1 and E2 represent the marks of parts 1 and 2 of the normal period test.

If (T1 + T2) / 2> 9.45, students are exempt from the exam, but may take one or both parts of the normal exam if they wish.

* the best of the grades between T1 and E1; ** the best of grades between T2 and E2.

Time of appeal
NF = exam grade (global)

Final scores above 18 may require a supplemental oral test.

Special assessment (TE, DA, ...)

Classification improvement

Appeal assessment (global examination)