Environmental Chemistry I

Code:

EA0007

Acronym:

QA I

Keywords
Classification	Keyword
OFICIAL	Basic Sciences
OFICIAL	Design, Development, Implementation and Operation
OFICIAL	Interp/Personal professional attitudes and capac.

Instance: 2006/2007 - 1S

Active?	Yes
Responsible unit:	Department of Chemical 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	59	Syllabus since 2006/07	1	-	5,5	-

Teaching language

Portuguese

Objectives

Global aims:
• To pass on fundamental knowledge on chemistry that will support the student education regarding Environmental Chemistry;
• To give a global vision of fundamental chemistry in an interface framework with environment and Environmental Chemistry;
• To develop a scientific reasoning;
• To stimulate a critical mind, aiming to avoid the primary acceptance of results;
• To promote the student auto-sufficiency, valuing the search and use of recently published data.

Specific aims:
• To deep and consolidate the previously acquired knowledge on chemistry;
• To create capacities for: i) interpreting the characteristics of gases, liquids and solids; ii) quantifying the composition of systems on chemical equilibrium; iii) previewing and understanding the answer of systems to changes in equilibrium conditions; iv) calculating, for the systems, the time needed to reach determined chemical composition.

Program

1. Revision of basic concepts
1.1 Elements e 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 The Properties of Gases
2.1 The nature of gases
2.1.1 Pressure and its unities
2.2 The gas laws
2.2.1 Boyle’s law
2.2.2 Charles’s law
2.2.3 Avogadro’s principle
2.2.4 The ideal gas law
2.2.5 Gas density
2.2.6 The stoichiometry of gaseous reactions
2.2.7 Mixtures of gases
2.3 Real gases
2.3.1 Deviations from ideality
2.3.2 The liquefaction of gases
2.3.3 Equation of state of real gases
3 The Properties of Liquids and Solids
3.1 Intermolecular forces
3.1.1 The formation of condensed phases
3.1.2 Ion-dipole forces
3.1.3 Dipole-dipole forces
3.1.4 London forces
3.1.5 Hydrogen bonding
3.2 Liquid structure
3.2.1 Order in liquids
3.2.2 Viscosity and surface tension
3.3 Solid structures
3.3.1 Solid classification
3.3.2 Metallic solids
3.3.3 Unit cell
3.3.4 Ionic structures
3.3.5 Molecular solids
3.3.6 Network solids
3.3.7 Alloys
3.3.8 Liquid crystals
4 Termochemistry
4.1 Systems states and energies
4.1.1 Systems
4.1.2 Energy and work
4.1.3 Heat
4.1.4 The first law of thermodynamics
4.1.5 State functions
4.2 Enthalpy
4.2.1 Heat capacities of gases
4.2.2 Enthalpy of phase changes
4.2.3 Heating curves
4.2.4 Reaction enthalpies
4.2.5 The relation between enthalpy and internal energy
4.2.6 Standard reaction enthalpies
4.2.7 Hess’s law
4.2.8 The heat output of reactions
4.2.9 Influence of temperature on the reaction enthalpy
5 Spontaneous and Non-Spontaneous Changes
5.1 Entropy
5.1.1 Spontaneous change
5.1.2 Entropy and disorder
5.1.3 Entropy changes accompanying changes of physical state
5.1.4 Standard molar entropies
5.1.5 Standard reaction entropies
5.2 Global changes in entropy
5.2.1 The surroundings
5.2.2 The overall change in entropy
5.2.3 Equilibrium
5.3 Gibbs energy
5.3.1 Reaction Gibbs energy
5.3.2 The effect of temperature on the change of Gibbs energy
5.3.3 Change of Gibbs energy and equilibrium
6 Chemical Equilibrium
6.1 Reaction at equilibrium
6.1.1 The reversibility of reactions
6.1.2 Thermodynamic fundaments of chemical equilibrium
6.1.3 Equilibrium constants
6.1.4 Heterogeneous equilibrium
6.1.5 The extent of reaction
6.1.6 The direction of reaction
6.2 The Response of equilibrium to changes in conditions
6.2.1 Adding and removing reagents and products
6.2.2 Changes in pressure
6.2.3 Temperature and equilibrium
6.2.4 Presence of catalysts
7 Equilibrium in Aqueous Phase
7.1 Equilibrium in acid-base reactions
7.1.1 Acids and bases in aqueous solutions
7.1.2 Strong and weak acids and bases
7.1.3 The pH and pOH scales
7.1.4 Polyprotic acids e bases
7.1.5 Autoprotolysis and pH
7.1.6 Buffers
7.1.7 Titrations
7.2 Equilibrium of solubility and complexation
7.2.1 The solubility product
7.2.2 Non-ideal aqueous solutions
7.2.3 The common-ion effect
7.2.4 Predicting precipitation
7.2.5 Selective precipitation
7.2.6 Dissolving precipitates
7.2.7 Complex ion formation
7.3 Equilibrium in oxidation-reduction reactions
7.3.1 Half-reactions
7.3.2 Balancing oxidation-reduction reactions
7.3.3 The electrochemical series
7.3.4 Standard potentials and equilibrium constants
7.3.5 The Nernst equation
8 Chemical Kinetics
8.1 Reaction rates
8.1.1 Concentration and reaction rates
8.1.2 The instantaneous rate of reaction
8.1.3 Rate laws and reaction orders
8.2 Concentration and time
8.2.1 First-order integrated reaction laws
8.2.2 Half-lives for first-order reactions
8.2.3 Second-order integrated reaction laws
8.2.4 Zero-order integrated reaction laws
8.3 Models of reactions
8.3.1 The effect of temperature on reaction rate
8.3.2 Theories of collision and activated complex
8.4 Catalysis

Mandatory literature

Sawyer, Clair N.; Chemistry for environmental engineering and science. ISBN: 0-07-119888-1
Atkins, Peter; Chemical principles. ISBN: 0-7167-5701-X
Atkins, Peter; Princípios de química. ISBN: 85-7307-739-5

Complementary Bibliography

Stumm, Werner; Aquatic Chemistry. ISBN: 0-471-83495-5
Manahan, Stanley E.; Fundamentals of Environmental Chemistry

Teaching methods and learning activities

General theoretical-practical lectures (TPG)
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 for classes (TPT)
Besides the problems solved in TPG, the handouts will include proposals for problems to be solved in TPT, and other problems to be solved out of the classes, 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

Description	Type	Time (hours)	Weight (%)	End date
Subject Classes	Participação presencial	56,00
Evaluation assay T1	Exame	1,00
Evaluation assay T2	Exame	1,00
Evaluation assay T3	Exame	1,00
Evaluation assay T4	Exame	1,00
Evaluation assay T5	Exame	1,00
Evaluation assay T6	Exame	1,00
	Total:	-	0,00

Eligibility for exams

General rules

Calculation formula of final grade

The final classification (CF) of students, since they reach the minimum level of attendance to classes, will be calculated through the following equation:

CF = CT1x0,2 + (CT2 + CT3 + CT4 + CT5 + CT6)/5 x 0,8

where CTi corresponds to the classification of the different evaluation assays.

Examinations or Special Assignments

Not applicable.

Special assessment (TE, DA, ...)

Final examination according to general rules.

Classification improvement

Not applicable.