Environmental Chemistry I

Code:

EA0007

Acronym:

QA I

Keywords
Classification	Keyword
OFICIAL	Physical Sciences (Chemistry)

Instance: 2019/2020 - 1S

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

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
MIEA	50	Syllabus since 2006/07	1	-	6	56	162

Teaching language

Portuguese

Objectives

1. Background: using the principles of chemistry, environmental engineers develop ways to solve problems related to the environment. These principles are present in important environmental issues such as air and water pollution control, waste disposal, recycling, ozone depletion, global warming and others. Many of these issues involve understanding chemical reactions. 2. Specific aims: this basic course intends (i) to pass on fundamental knowledge of chemistry that will support the student’s education regarding environmental chemistry and (ii) to give a global vision of fundamental chemistry in an interface framework with environment and environmental chemistry. 

Learning outcomes and competences

It is expected that students have: (i) deepen and consolidated their previous acquired knowledge on chemistry; (ii) developed a scientific reasoning and a critical mind, avoiding the primary acceptance of results; (iii) increased their auto-sufficiency by valuing the search and use of recently published data.

 

Specifically, it is expected that students learn the following technical competences:

Identify organic or inorganic compounds and give their name. In the case of organic compounds, the students should recognize a simple haloalkane, alcohol, ether, phenol, aldehyde, ketone, carboxylic acid, amine, amide or ester.

Describe the composition of carbohydrates, fats and proteins. In the latter, distinguish their structures (from primary to quaternary).

Know how to: (i) use the gas laws to calculate P, T, V and number of moles; (ii) calculate the total pressure of a mixture and the partial pressures of gases in a mixture; (iii) use the Graham´s law to determine molar mass; (iv) explain the differences between real and ideal gases.

Know how to: (i) predict the relative strengths of the ion-dipole interactions; (ii) explain how London forces arise and how they vary with polarizability of an atom and the size and shape of a molecule; (iii) describe the structure of a liquid and explain how viscosity and surface tension vary with temperature and the strength of intermolecular forces.

 

Working method

Presencial

Pre-requirements (prior knowledge) and co-requirements (common knowledge)

Knowledge of chemistry at the 11th level of the secondary school.

Program

1. Revision of basic concepts 1.1 Elements an atoms 1.2 Compounds 1.3 Nomenclature of inorganic compounds 1.4 Unities and measurements 1.5 Moles e molar weights 1.6 Determination of chemical formulas 1.7 Mixtures and solutions 1.8 Chemical equations 1.9 Aqueous solutions (concentration and dilution).

2. Concepts of organic chemistry 2.1 Common functional groups. Nomenclature of organic compounds. 2.2 Aliphatic hydrocarbons. Physical and chemical properties. 2.3 Aromatic hydrocarbons. Physical and chemical properties. 2.4 Properties and reactions of compounds with different functional groups: haloalkanes, alcohols, ethers, aldehydes and ketones; carboxylic acids, esters and amines. 2.5 Proteins, polysaccharides and lipids.

3. The Properties of Gases 3.1 The nature of gases 3.1.1 Pressure and its unities 3.2 The gas laws 3.2.1 Boyle’s law 3.2.2 Charles’s law 3.2.3 Avogadro’s principle 3.2.4 The ideal gas law 3.2.5 Gas density 3.2.6 The stoichiometry of gaseous reactions 3.2.7 Mixtures of gases 3.3 Real gases 3.3.1 Deviations from ideality 3.3.2 The liquefaction of gases 3.3.3 Equation of state of real gases.

4. The Properties of Liquids. 4.1 Intermolecular forces 4.1.1 The formation of condensed phases.4.1.2 Ion-dipole forces. 4.1.3 Dipole-dipole forces. 4.1.4 London forces. 4.1.5 Hydrogen bonding. 4.2 Liquid structure. 4.2.1 Order in liquids. 4.2.2 Viscosity and surface tension. 

Mandatory literature

Theodore L. Brown, ... [et al.]; Chemistry. ISBN: 978-0-321-74983-3

Complementary Bibliography

Peter Atkins, Loretta Jones, leroy Laverman; Chemical principles. ISBN: 978-1-4641-2467-9

Teaching methods and learning activities

General theoretical lectures (T): presentations supported by audiovisual media, and illustrated with the solution of problems related with practical examples, included in tutorial handouts to be delivered to the students. Special attention will be given to the application of knowledge in quotidian life issues, with interfaces with environment and Environmental Engineering. Students will be strongly stimulated to participate during the classes. Presences will be registered.

Theoretical-practical lectures (TP): besides the problems solved in T, the handouts will include proposals for problems to be solved in TP, and other problems to be solved outside class, to facilitate learning and to consolidate knowledge. Special attention will be given to the critical analysis of results and to the search of data in tables delivered to the students. Absences will be registered.

Evaluation Type

Distributed evaluation without final exam

Assessment Components

Designation	Weight (%)
Teste	100,00
Total:	100,00

Amount of time allocated to each course unit

Designation	Time (hours)
Estudo autónomo	80,00
Frequência das aulas	62,00
Total:	142,00

Eligibility for exams

Application of SPECIFIC REGULATION OF ASSESSMENT OF STUDENTS of FEUP.

Repeating students who attended the course in the previous academic year are exempted from class attendance

Calculation formula of final grade

Two evaluation assays. The final classification (CF) of students, as long as they reach the minimum level of attendance to classes, will be calculated through the following equation: CF = k*[ 0,40 * T1 + 0,60 * T2], where  k - performance factor in T and TP (0.90 < k < 1.05) where T1 and T2 correspond to the classification of the two evaluation assays. A minimum of 7.0/20.0 in each assay is required for approval. For the students, who obtain a final mark below 10 in the distributed evaluation and obtained frequency, the final mark will be that obtained in a special exam.

 

The dates of the tests are:

T1- 24th of October;
T2-7th of January.

The missing information about timetable and rooms, not yet available, will be announced to the students by dynamic email.

Examinations or Special Assignments

Not applicable.

Internship work/project

No special assignments, beyond those indicated herein, are provided.

Special assessment (TE, DA, ...)

Not applicable.

Classification improvement

In agreement with section 10.1 of Article 10 Improvement of the SPECIFIC REGULATION OF ASSESSMENT OF STUDENTS of FEUP, students may make improvements classification examination performed only once, at one of two times of the final examination mentioned in alinea a) of paragraph 1, Article 9, immediately after they passed and when the course has examination provided. 

Observations

The students, who miss any of the components of the distributed evaluation, a classification of zero values will be assigned in this component.

In all classes, students must have the following materials: calculating machine, problems, data tables, paper and pen.