ENERGY SYSTEMS ENGINEERING
Bachelor	TR-NQF-HE: Level 6	QF-EHEA: First Cycle	EQF-LLL: Level 6

Course Introduction and Application Information

Course Code	Course Name	Semester	Theoretical	Practical	Credit	ECTS
CHE1001	General Chemistry I	Fall	3	2	4	7

Basic information

Language of instruction:	English
Type of course:	Must Course
Course Level:	Bachelor’s Degree (First Cycle)
Mode of Delivery:	E-Learning
Course Coordinator :	Dr. Öğr. Üyesi ÖMER LÜTFİ UYANIK
Course Lecturer(s):	Dr. Öğr. Üyesi ÖMER LÜTFİ UYANIK RA BESTENUR YALÇIN RA İBRAHİM ERTUĞRUL YALÇIN RA ÜMMÜGÜLSÜM ALYÜZ ÖZDEMİR
Recommended Optional Program Components:	None
Course Objectives:	The major purpose of this course is to help students learn some of the basic concepts in Chemistry. The course topics include the theory and applications. These contribute to the development of the student skills in analytical thinking and problem solving. The course aims to help them understand chemistry’s relevance and contribution to their career interests. The experiments that parallel the course topics provide opportunities to the students in making practice.

Learning Outcomes

The students who have succeeded in this course;
The student who succeeded in this course
1) Expresses experimental results with proper number of significant figures and in proper units.
2) Classifies compounds and determine the empirical and molecular formulas of a compound using experimental results.
3) Calculates the amount of product formed in a chemical reaction using stoichiometric relationships.
4) Lists the characteristics of chemical reactions occuring in aqueous solutions (precipitation reactions, acid-base reactions, and oxidation-reduction reactions) and writes molecular equation, ionic equation, and net ionic equation for these reactions.
5) Calculates state variables for a gas or gas mixture (pressure, volume, temperature, and number of moles) using ideal gas equation.
6) Using the results of kinetic-molecular theory of gases calculates average kinetic energies, average speeds, and effusion rates of gas molecules and also lists the conditions under which gas deviates from ideal behavior.
7) Knows the relationships among various forms of energy in physical changes and in chemical reactions and calculates the energies associated with chemical reactions.
8) Writes the Lewis structure of a molecule and based on this structure, determines the shape of this molecule, whether it is polar or nonpolar, the type of hybridization on the central atom, and the types of bonds in the molecule.
9) Classifies intermolecular forces of attraction and determines the type of intermolecular forces in the liquid and solid states of a given substance.
10) Defines each property of liquids related to intermolecular forces (surface tension, viscosity, molar enthalpy of vaporization, vapor pressure, and boiling point) and discusses how each of these properties by various factors.
11) Calculates the concentration of a solution in terms of various concentration definitions, defines solubility and knows how various factors affect solubility.
12) Calculates the colligative properties (vapor pressure lowering, osmotic pressure, boiling point elevation, and freezing point depression) of a solution of known concentration.

Course Content

Some Basic Concepts of Chemistry (Measurement, Units, Dimensional Analysis, Mole Concept, Compounds and their Formulas). Chemical Reactions. Introduction to Chemical Reactions in Aqueous Solutions. Gases. Thermochemistry. Chemical Bonding. Intermolecular Forces: Liquids and Solids. Solutions and their Physical Properties.

Weekly Detailed Course Contents

Week	Subject	Related Preparation
1)	SOME BASIC CONCEPTS IN CHEMISTRY. Measurement. SI (Metric) Units. Uncertainties in Scientific Measurements. Significant Figures. Dimensional Analysis in Unit Conversions. The Mole Concept. Chemical Compounds and Their Formulas.	Review of topics
2)	CHEMICAL REACTIONS Writing Chemical Reaction Equations. Stoichiometry in Chemical Equations. Stoichiometry of Chemical Reactions Occuring in Aqueous Solutions. Concentration Concept: Percent by Mass and Molarity. Limiting and Excess Reactants.	Review of topics
3)	Theoretical Yield, Actual Yield, and Percent Yield in Chemical Reactions. INTRODUCTION TO REACTIONS IN AQUEOUS SOLUTIONS The Nature of Aqueous Solutions: Solutions of Electrolytes and Nonelectrolytes. Precipitation Reactions. Some Properties of Acids and Bases. pH and pOH Concepts.	Review of topics
4)	Acid-Base (Neutralization) Reactions. Oxidation-Reduction (Redox) Reactions. GASES State Variables for Gases. Ideal Gas Equation.
5)	Gas Densities. Gas Mixtures. Kinetic Theory of Gases. Gas Properties Related to Kinetic Theory: Diffusion and Effusion. Nonideal (Real) Gases. THERMOCHEMISTRY Basic Terms in Thermochemistry.	Review of topics
6)	Heat. Experimental Determination of Heats of Reaction: Calorimeters. PressurexVolume Work in Chemical Reactions. First Law of Thermodynamics. The Concept of Enthalpy and Its Application to Chemical Reactions.	Review of topics
7)	Standard Enthalpies of Formation. Calculating Standard Enthalpy Changes of Chemical Reactions. CHEMICAL BONDING Electron Configurations of Elements. A General Look at the Periodic Table. Lewis Theory of Chemical Bonding. Ionic Bond and Covalent Bond. Lewis Symbols and Lewis Structures. 1st Mid-Term	Review of Topics
8)	Polar and Nonpolar Covalent Bonds. Writing Lewis Structures of Molecules and Ions Containing More than Two Atoms. Formal Charge Concept. Resonance.	Review of Topics
9)	Shapes of Molecules. Polarity of Molecules, the Concept of Dipole Moment. Hybridization and Hybrid Orbitals.	Review of the Previous Topics.
10)	Sigma and Pi Bonds. INTERMOLECULAR FORCES: LIQUIDS AND SOLIDS Intermolecular Forces. Surface Tension.	Review of topics
11)	Viscosity of Liquids. Vaporization, Enthalpy of Vaporization, Vapor Pressure of Liquids. Boiling of Liquids. 2nd Mid-Term	Review of Topics
12)	Critical Temperature and Critical Pressure. Liquefaction of Gases. Some Properties of Solids. Phase Diagrams.	Review of topics
13)	SOLUTIONS AND THEIR PHYSICAL PROPERTIES Concentration Concept in Solutions: Percent by Mass, Molarity, Mole Fraction, Molality, Parts Per Million. Intermolecular Forces and the Solution Process. Solubility. Colligative Properties of Solutions.	Review of topics
14)	Vapor Pressure Lowering, Osmotic Pressure, Boiling Point Elevation, Freezing Point Depression in Solutions of Nonelectrolytes. Vapor Pressure Lowering, Osmotic Pressure, Boiling Point Elevation, Freezing Point Depression in Solutions of Electrolytes. Colloidal Mixtures.	Review of Topics

Sources

Course Notes / Textbooks:	Petrucci, Ralph H. ; Harwood, William S. ; Herring, F. Geoffrey ; Madura Jeffry D. General Chemistry, Tenth Edition, Pearson.
References:	1) Chang, Raymond, Chemistry, 6th Ed. Mc Graw - Hill 2) Zumdahl, Steven S. Chemistry, 6th Ed. D.C. Heath and Company

Evaluation System

Semester Requirements	Number of Activities	Level of Contribution
Laboratory	8	% 20
Midterms	2	% 40
Final	1	% 40
Total		% 100
PERCENTAGE OF SEMESTER WORK		% 60
PERCENTAGE OF FINAL WORK		% 40
Total		% 100

ECTS / Workload Table

Activities	Number of Activities	Workload
Course Hours	14	42
Laboratory	8	16
Study Hours Out of Class	15	103
Midterms	2	4
Final	1	2
Total Workload		167

Contribution of Learning Outcomes to Programme Outcomes

No Effect	1 Lowest	2 Low	3 Average	4 High	5 Highest

	Program Outcomes	Level of Contribution
1)	Build up a body of knowledge in mathematics, science and Energy Systems Engineering subjects; use theoretical and applied information in these areas to model and solve complex engineering problems.	5
2)	Ability to identify, formulate, and solve complex Energy Systems Engineering problems; select and apply proper modeling and analysis methods for this purpose.	5
3)	Ability to design complex Energy systems, processes, devices or products under realistic constraints and conditions, in such a way as to meet the desired result; apply modern design methods for this purpose.	5
4)	Ability to devise, select, and use modern techniques and tools needed for solving complex problems in Energy Systems Engineering practice; employ information technologies effectively.	5
5)	Ability to design and conduct numerical or pysical experiments, collect data, analyze and interpret results for investigating the complex problems specific to Energy Systems Engineering.	5
6)	Ability to cooperate efficiently in intra-disciplinary and multi-disciplinary teams; and show self-reliance when working on Energy Systems-related problems
7)	Ability to communicate effectively in English and Turkish (if he/she is a Turkish citizen), both orally and in writing. Write and understand reports, prepare design and production reports, deliver effective presentations, give and receive clear and understandable instructions.
8)	Recognize the need for life-long learning; show ability to access information, to follow developments in science and technology, and to continuously educate oneself.	4
9)	Develop an awareness of professional and ethical responsibility, and behave accordingly. Be informed about the standards used in Energy Systems Engineering applications.
10)	Learn about business life practices such as project management, risk management, and change management; develop an awareness of entrepreneurship, innovation, and sustainable development.
11)	Acquire knowledge about the effects of practices of Energys Systems Engineering on health, environment, security in universal and social scope, and the contemporary problems of Energys Systems engineering; is aware of the legal consequences of Energys Systems engineering solutions.	4