General and inorganic chemsitry

NAME OF THE COURSE General and inorganic chemsitry

Code

KTL101

Year of study

1.

Course teacher

Asst Prof Marijo Buzuk

Credits (ECTS)

7.0

Associate teachers

Type of instruction (number of hours)

P S V T

30

15

30

0

Status of the course

Mandatory

Percentage of application of e-learning

0 %

COURSE DESCRIPTION

Course objectives

This course provides an introduction to chemistry as a quantitative and qualitative science. The course will provide students with the core chemistry skills and knowledge recommended for understanding of other fields of chemistry (organic, analytic, physics) and will provide knowledge needed for engineering study. Course will present fundamental concepts of chemistry including atomic structure, history of the atom, development of the periodic table, nuclear chemistry, chemical
nomenclature and formula, types of reactions, stoichiometry, gas laws, liquids and solids, thermodynamics, chemical equilibrium, acids and bases. Core topics include base theories in chemistry needed for understanding and recognizing problems in chemistry and provide the student with a basic foundation of laboratory inquiry and develop problem solving skills.

Course enrolment requirements and entry competences required for the course

 

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students successfully completing this course will:
1. Understand and apply concepts to solve problems by knowledge of the matter and measurement and atoms, molecules and ions.
2. Describe and calculate quantities for gas behaviour, stoichiometry and calculations with chemical formulas and equations, reactions in aqueous solution.
3. Use the following to predict, depict and describe electronic structure of atoms, elemental periodic properties, basic properties of chemical bonding, molecular geometry and theory of bonding.
4. Understand and apply concepts to solve problems using knowledge of properties of solutions and chemical kinetics.
5. Describe and calculate quantities for general chemical equilibria, acid-base equilibria, precipitation equilibria.

Course content broken down in detail by weekly class schedule (syllabus)

1. Introduction to chemistry and matter and mathematics of chemistry. Physical and chemical properties of the matter.
2. Dalton`s theory of atom. Gases and their laws. Molar mass of molecules.
3. Atoms, the atomic theory and structure.
4. The periodic law, properties, and trends.
5. Compounds, bonding, ionic and covalent bonding, formula, nomenclature. Geometry of molecules. Lewis structure.
6. Intermolecular forces and interactions.
7. Chemical reactions, redox reactions, oxidation and reduction.
8. Solution chemistry. Properties and kind of solutions. Electrolytes.
9. Collligative properties. Henry`s and Rault`s law. Dissolution of gasses in liquids.
10. Chemical equilibrium. Heterogonous and homogenous equilibrium. Acid-base equilibrium. Buffers. pH.
11. Elements of 18. and 17. group. Hydrogen and water.
12. p-elements. Elements of 16. i 15. group. Characteristic reaction. Characteristic compounds and oxidation number. Water. Water hardness. Acid and basic oxides.
13. p-elements. Elements of 14. i 13. group. Carbonates, hydrogencarbonates. Aluminium-amphoteric properties of aluminium and its oxides.
14. s-elements. Elements of 1. and 2. group. Hydrides and oxides. Peroxides, superoxides, oxides. Basic character of s-elements and their compounds.
15. Overview.

Format of instruction:

Student responsibilities

Attendance to all lab courses.

Screening student work (name the proportion of ECTS credits for eachactivity so that the total number of ECTS credits is equal to the ECTS value of the course):

Class attendance

2.0

Research

0.0

Practical training

0.0

Experimental work

1.0

Report

0.0

 

 

Essay

0.0

Seminar essay

0.0

 

 

Tests

1.0

Oral exam

2.0

 

 

Written exam

1.0

Project

0.0

 

 

Grading and evaluating student work in class and at the final exam

During semester two exams will be performed. Final examinations will be administered during formal examination periods. The following percentage equivalents apply to final grade: <55% Failure; 56%-66% (2); 67%-78% (3); 79%-90% (4);> 90% (5). After written exam, student will attend to oral exam. Lecturers do not give grades. Students earn grades.

Required literature (available in the library and via other media)

Title

Number of copies in the library

Availability via other media

Filipović, I., Lipanović, S., Opća i anorganska kemija I i II dio, Školska knjiga, Zagreb, 1995

10

Sikirica, M., Stehiometrija, Školska knjiga, Zagreb

0

Vježbe iz Opće kemije (interna skripta), Kemijsko-tehnološki fakultet, Split, 2013.

0

Optional literature (at the time of submission of study programme proposal)

Darrell D. Ebbing and Steven D. Gammon, General Chemistry, 9th edition, Houghton Mifflin Company, Boston, 2009.
Raymond Chang, Chemistry, 10th edition, McGraw-Hill, New York, 2010.

Quality assurance methods that ensure the acquisition of exit competences

- monitoring of students suggestions and reactions during semester
- students evaluation organized by University

Other (as the proposer wishes to add)