Inorganic Chemistry

Code:

Q212

Acronym:

Q212

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2013/2014 - 2S

Active?	Yes
Web Page:	https://moodle.up.pt/course/view.php?id=734
Responsible unit:	Department of Chemistry and Biochemistry
Course/CS Responsible:	Bachelor in Chemistry

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
L:Q	77	Plano de estudos Oficial	1	-	7,5	-

Teaching language

Suitable for English-speaking students

Objectives

Introduction to chemical bonds and molecular geometry. Use of chemical thermodynamic, acid-base and oxidation-reduction concepts to the characterization of chemical reactivity and stability of inorganic compounds. Introduction to transition metal complexes.

Learning outcomes and competences

1. Knowledge on chemical bonding and structure for molecular compounds,

2. Knowledge on chemical bonding and structure for covalent, ionic and molecular solids,

3. Reactivity vs structure: electrical, oxidation-reduction and acid-base properties.

 

Working method

Presencial

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

No previous specific background is need

Program

1 The electronic structure of the atom and overview of the periodic table - overview 2 Covalent bonding: Lewis theory, valence shell electron pair repulsion theory (VSEPR), valence bond theory/ orbital hybridization and molecular orbital theory (diatomic molecules) 3 Metallic bonding: bonding models and structures of metals. 4 Ionic bonding. Polarization and covalency. Ionic crystal structures 5 Inorganic thermodynamics. Thermodynamics of the formation of ionic and covalent compounds. Thermodynamics of the solution process for ionic compounds. 6 Solvents systems and Acid-base behavior. Bronsted-Lowry Acids and Lewis Theory. Trends in acid-base behavior. Hard-soft acid base concepts. 7 Oxidation-reduction in inorganic compounds. Periodic variation of oxidation numbers. Electrode potentials as thermodynamic functions. Latimer, Frost and Pourbaix diagrams. 8 Introduction to transition metal complexes. Ligands and their properties. Isomerism in metallic complexes. An overview of bonding theories of transition metal complexes: crystal field theory; ligand spectrochemical series. Introduction of electronic spectra: high spin complexes.

Mandatory literature

Geoff Rayner-Canham e Tina Overtin; Descriptive Inorganic Chemistry , Freeman, 2006

Complementary Bibliography

Peter Atkins, Loretta Jones; Chemical Principles: the quest for insight ,, Freeman, 2008

Teaching methods and learning activities

The lectures (3 x 1 h /week) were given using multimedia methods. Teh lectures will be available in the Moodle UP page of the discipline. During the lectures some sites in the internet were given to the students in order to complement their formation in specific subjects.These will be also available in the Moodle UP page of the discipline.

In the tutorial lectures (2h x 1 / week) several exercises will be done in order to strengthen the theoretical concepts . This was done in groups (2-3 students) after their preparation at home.

An inetrmediate test will be made by March/April

keywords

Physical sciences > Chemistry > Inorganic chemistry
Physical sciences > Chemistry > Molecular chemistry
Physical sciences > Chemistry > Structural chemistry

Evaluation Type

Distributed evaluation with final exam

Assessment Components

designation	Weight (%)
Exame	70,00
Participação presencial	30,00
Total:	100,00

Amount of time allocated to each course unit

designation	Time (hours)
Estudo autónomo	140,00
Frequência das aulas	70,00
Total:	210,00

Eligibility for exams

The students can not miss more than 4 tutorial classes - this corresponds to 1/4 of the expected number of tutorial sessions.

The final mark in the tutorial sessions have to be equal ou higher than 9.5.

Calculation formula of final grade

NOTA FINAL= (0,70 x Exame) + (0,30 x aulas TP)

1 -Teste intermédio (TI)  + exame final (época normal): Se o aluno tiver uma nota igual ou superior a 8,0 valores poderá ficar dispensado de realizar no exame final da  época normal a avaliação sobre a matéria do TI. A avaliação será: (nota TI + nota do ex época normal) / 2. As notas não poderão ser inferior a 8,0 valores nos dois casos. A NOTA DO TI SÓ PODERÁ SER USADA NA ÉPOCA NORMAL

 2 Exame final Se o aluno tiver uma nota infeiror a 8,0 valores no TI terá de realizar o exame final (época normal ou recurso) .Para o aluno obter aprovação, a nota de exame terá de ser igual ou superior a 8,0 valores.

 AULAS TEÓRICO-PRÁTICAS: nota mínima de 9,5

Special assessment (TE, DA, ...)

With frequency in the TPs = ordinary students

Without frequency in the TPs = the final mark of the UP corresponds to the exam mark

Classification improvement

By Final exam