Download Lab № 8. Redox Reactions.

«Kazakh national technical research university »
«APPROVED»
Head of the department of
“Applied Chemistry”
______________Kalenova A.S.
“___”_____________2017y.
SILLABUS
Discipline: «Chemistry»
Credits: 2
Academic year: 2016-2017
Semestr: II
Teacher: Abildina Ainaz Kairatovna
Office: Lab 1002 MEB (Main educational building)
Date about
teacher
Tutor
Time and place of
Classes
Office hours
Lecture:
Monday:
10.00-10.50
1007, MEB;
Labs:
Monday:
07.50-09.45
Lab 1002,
MEB
Friday:
15.10-16.00
Lab 1002,
MEB
Contact information
Telephone
e-mail
numbers
Work number:
[email protected]
2-57-71-94;
[email protected]
Internal phone:
7194
Cell number:
8-707-39-86531
Prerequisites of course:
Basic school course of chemistry, mathematics (elements of algebra and geometry), physics.
Course Description:
“Chemistry” course gives wide amount of theoretical knowledge in chemistry and helps acquiring
experimental skills for conducting physical and chemical research required to solve problems in various
industrial branches that require a basic knowledge.
The knowledge gained during the course are the foundation for studying Inorganic chemistry II,
Analytical, Physical, Rare earth chemistry as well as core courses related to technology of inorganic
substances.
Aims and Objectives:
The aim of discipline is to deliver fundamental chemical knowledge and skills for application of
the basic concepts and laws of chemistry in the further study of general engineering and technological
courses or directly in practical activities.
As a result of the course, students are expected to be able to operate with the basic concepts and
laws of chemistry; have and understanding of the matter structure; theory of chemical bonds; properties of
solutions of non-electrolytes and electrolytes; mechanism and laws of dissociation processes; the essence
of chemical equilibrium and ways of its shifting; modern theory of acids and bases; reactions in electrolyte
solutions; fundamentals of chemical thermodynamics and kinetics; concepts of basic electrochemical
processes; properties of simple substances and chemical compounds of various elements (metals and
nonmetals).
Students are expected to acquire skills of applying obtained knowledge in solving engineering
problems; based on the periodic law and the theory of matter structure predict the physical and chemical
properties of elements and their compounds.
Textbooks
Recommended:
1. Raymond Chang. "CHEMISTRY", New York: Williams College, 10th EDITION, 2010, 1170 p.
2. Raymond Chang, Jason Overby. "General Chemistry. The Essential concepts",6th EDITION,
2011, 853 p.
Calendar-thematic plan
Week
1.
2.
3.
Classes (hour)
Lect
Name of lesson
ure
Lecture 1. Introduction. Basic
2
concepts and laws in the chemistry.
The Study of Chemistry. The
Scientific Method. Classifications of
Matter. Physical and Chemical.
Properties of Matter Measurement.
Handling Numbers. Dimensional
Atomic Mass. Avogadro’s Number
and the Molar Mass of an Element.
Molecular Mass. Percent Composition
of
Compounds.
Experimental
Determination of Empirical Formulas.
Chemical Reactions and Chemical
Equations. Substances That Exist as
Gases. Pressure of a Gas. The Gas
Laws. The Ideal Gas Equation. Gas
Stoichiometry.
Dalton’s Law of Partial Pressures.
The Kinetic Molecular Theory of
Gases. Deviation from Ideal
Behavior.
Lecture 2. The Electronic Structure of
2
Atoms.
From Classical Physics to Quantum
Theory. The Photoelectric Effect.
Bohr’s Theory of the Hydrogen
Atom. The Dual Nature of the
Electron. Mechanics. Quantum
Numbers. Orbitals. Electron
Configuration. The Building-Up
Principle
Lecture 3. The Periodic Table. .
2
Development of the Periodic Table.
Periodic Classification of the
Elements . Periodic Variation in
Physical Properties. Ionization
Energy. Electron Affinity. Variation
Lab
work
2
Chapter
2
1[2,7,8];
2[2,7,8]
Lab № 2. Determination of the
equivalent weight of zinc.
2
1[9]; 2[9]
Lab № 3 The rate of a
chemical reaction
1[1,5];
2[1,5]
SWS (SWST)
Typeof tasks and deadline
Introduction. General safety
rules
in
the
chemical
laboratory.
Lab № 1. The classes of
inorganic compound
2
4.
5.
6.
7.
8.
9.
in Chemical Properties of the
Representative.
Lecture 4. Chemical Bonding I: The
Covalent Bond.
Lewis Dot Symbols. The Ionic Bond.
Lattice Energy of Ionic Compounds.
The Covalent Bond.
Electronegativity. Writing Lewis
Structures. Formal Charge and Lewis
Structure. The Concept of Resonance.
Exceptions to the Octet Rule. Bond
Enthalpy..
Lecture 5. Chemical Bonding II:
Molecular Geometry.
and Hybridization of Atomic Orbitals.
Molecular Geometry.
Moments. Valence Bond Theory.
Hybridization of Atomic Orbitals.
Hybridization in Molecules
Containing Double and Triple Bonds.
Orbital Theory
Lecture 6 Thermochemistry.
The Nature of Energy and Types of
Energy. Energy Changes in Chemical
Reactions.
Introduction
to
Thermodynamics.
Enthalpy
of
Chemical Reactions. Calorimetry.
Standard Enthalpy of Formation and
Reaction. Heat of Solution and
Dilution..
Lecture 7. Chemical Kinetics.
Chemical Equilibrium.
The Rate of a Reaction.
The Rate Laws. Relation Between
Reactant Concentrations and Time.
Activation Energy and Temperature
Dependence of Rate Constants.
Reaction Mechanisms. Catalysis. The
Concept of Equilibrium. Ways of
Expressing Equilibrium Constants.
Factors That Affect Chemical
Equilibrium..
Lecture 8. Physical Properties of
Solutions.
Types of Solutions. Molecular View
of the Solution Process.
Concentration Units. The Effect of
Temperature on Solubility. The Effect
of Pressure on the Solubility of Gases.
Colligative Properties of
Nonelectrolyte Solutions
Lecture 9 Acid-Base Equilibria and
Solubility Equilibria
Homogeneous versus Heterogeneous
Solution Equilibria. The Common Ion
Effect. Buffer Solutions. Acid-Base
Titrations. Acid-Base Indicators.
2
2
1[10];
2[10]
Lab № 4 The shift of chemical
equilibrium in the reaction
between the iron (III) chloride
with potassium thiocyanate.
2
2
1[6,18];
2[6,18]
Quizzes №1.
Lab № 5. Preparing solutions
2
2
1[13,14];
2[14,15]
Lab № 6.
dissociation.
2
2
1[12];
2[13]
Protection of SIS №1.
2
2
1[15];
2[16]
Midterm Control №1
2
2
1[19.1]
2[19.1]
Lab № 7. Hydrolysis of salts
Electrolytic
3
10.
11.
12.
13.
14.
15.
Solubility Equilibria Separation of
Ions by Fractional Precipitation. The
Common Ion Effect and Solubility. pH
and
Solubility.
Complex
Ion
Equilibria and Solubility.
Lecture
10
Redox
Reactions.
Balancing. Redox Equations.
Balancing Redox Equations using the
Oxidation Number Method. Oxidizing
agents. Reducing agents.
Lecture 11 Electrochemistry.
Galvanic Cells. Standard Reduction
Potentials. Thermodynamics of
Redox Reactions. The Effect of
Concentration on Cell. Batteries.
Corrosion. Electrolysis.
Electrometallurgy.
Lecture 12. Transition Metals
Chemistry and Coordination
Compounds.
Properties of the Transition Metals.
Chemistry of Iron and Copper.
Coordination Compounds. Structure
of Coordination Compounds.
Bonding in Coordination
Lecture 13. Transition Metals
Chemistry and Coordination
Compounds
Compounds: Crystal Field. Reactions
of Coordination Compounds.
Coordination Compounds in Living
Systems. Applications of
Coordination Compounds.
Lecture 14. Nonmetallic Elements and
Their Compounds.
General Properties of Nonmetals.
Hydrogen. Carbon.
Nitrogen and Phosphorus. Oxygen
and Sulfur. The Halogens. Metallurgy
and the
Lecture 15. Chemistry in the
Atmosphere.
Earth’s Atmosphere. Phenomena in
the Outer Layers of the Atmosphere.
Depletion of Ozone in the
Stratosphere. Volcanoes. The
Greenhouse Effect. Rain.
Photochemical Smog.
Total
Final Exam
2
2
1[19.219.8];
2[19.219.9]
Lab № 8. Redox Reactions.
2
2
1[22.122.5];
2[20.120.4]
Lab № 9. Galvanic Cells.
Standard Reduction Potentials
of metals.
Lab № 10. Electrolysis of salt
solution.
2
2
1[22.522.7];
2[20.5,20
.6]]
Lab №11.
metals.
2
2
1[21]
Quizzes № 2.
Lab №12. Coordination
Compounds.
2
2
1[20]
Protection of SIS № 2.
2
2
1[17]
Midterm Control № 2
30
30
Corrosion
of
15
Types of assessment:
Midterm / End-of-term Exams: 2 per semester
Quizzes: 2 per semester
SIS (student’s independent study): 2 per semester
Final Exam: during exam session
4
Evaluation, %
Laboratory work
Problem solving
Quizzes
SIS
Midterm Exam
End-of-term Exam
Final Exam
Total
24%
8%
8%
10 %
10 %
40 %
100 %
100 %
Schedule for assessment
№
1.
2.
3.
4.
5.
6.
Types of assessment and
class activities
Laboratory work
Quizzes
SIS
Midterm/ End-of-term Exams
Final Exam
Total
1
2
3
*
4
*
5
6
*
WEEKS
8 9 10
* *
7
*
*
*
Total
11
12
*
13 14
*
*
*
*
15
*
24
8
8
20
40
100
Grading scales
Grade
Excellent
Good
Satisfactory
Unsatisfactory
Alphabetic
А
АВ+
В
ВС+
С
СD+
D
F
Percentage, %
95-100
90-94
85-89
80-84
75-79
70-74
65-69
60-64
55-59
50-54
0-49
GPA
4
3,67
3,33
3,0
2,67
2,33
2,0
1,67
1,33
1,0
0
Grading policy
Attendance and activity at lectures and laboratory classes are mandatory. Due to the large volume of
study material, the student must come prepared for a lecture. Lectures will cover the basic theoretical
principles of the course, as well as their practical value. At 20% (9 hours) missed classes student will be
withdrawn from the discipline receiving an “F (Fail)” grade regardless of the previous marks. In cases of
constant violations of the discipline, fixed deadlines or frequent lateness to the classes will lead to the
appropriate measures to be taken according to the Credit system.
Laboratory work helps with acquiring practical knowledge and problem solving skills, as well as
elucidation of theoretical material. Lab Reports are defended by a student at the next lab class. Also during
the time free of laboratory work we will solve problems and conduct quizzes, Midterm and End-of-term
Examinations.
Quizzes will be carried out in the form of tests and / or problem solving and will be used to assess
your progress in understanding the material as well as keeping you prepared for the following exams.
Students’ Independent Study (SIS) will be given in the form of 1 presentation on a given subject
during the semester and is expected to consist of 10-15 slides designed freeform and defended within the
fixed deadline.
Midterm and End-of-term Exams cover all the lectures, laboratory work and SIS studied during the
middle and end of term. They will contain tests and / or theoretical questions and problems to solve.
5
The Final Exam covers and generalizes all course material. Examination papers divided into three
parts: tests, problems and theoretical questions. The duration of the Final Exam will not exceed 3 academic
hours.
Students who scored 30 points or more by the result of Midterm and End-of-term Exams are
permitted to take the Final Exam.
To receive positive marks the student must score at least 20 points (out of 40) on the Final Exam
otherwise, he/she will be graded with “F” mark.
Cheating, plagiarism and holding cellphones and course materials (on paper or electronic devices) at
the Mid/End-of-term or the Final Examinations will lead to an “F” mark for the entire discipline regardless
of the marks received previously.
The case of being late for the Final Exam will lead to “F” grade.
The Syllabus have been discussed at a meeting of "Applied Chemistry" Department
“__”_________ 2017y, Protocol №__.
Tutor
Abildina A.K.
6