Bayburt University Lifelong Learning Programme

Description of Individual Course Units

Course Unit Code	Course Unit Title	Type of Course Unit	Year of Study	Semester	Number of ECTS Credits
G109B2	General Chemistry	Compulsory	1	1	5

Level of Course Unit

First Cycle

Objectives of the Course

To understand the molecular nature of all phases of matter, to understand the various ways of depicting chemical compounds and chemical reactions, to develop an ability to solve basic quantitative problems regarding the properties of molecules, chemical equilibria, and chemical kinetics, and to develop the ability to appropriately apply this knowledge to general scientific problems in various fields of science and engineering.Introduction to atomic structure, periodic trends, chemical bonding, molecular structure Basic principles of chemistry including stoichiometry. Introduction to solution phase chemistry. Gas phase chemistry. Introduction to thermodynamics, including enthalpies of formation and reaction.

Name of Lecturer(s)

Doç. Dr. İbrahim Hakkı KARAKAŞ

Learning Outcomes

1	to learn the basic structures of atoms, ions, and molecules, and ways to quantitatively describe the properties of atoms and molecules in the various phases of pure matter and in mixtures
2	to learn the reactivity of atoms, ions, and molecules, and the various qualitative and quantitative methods for describing or depicting chemical reactions
3	to learn the concept of chemical equilibrium, and the energies that drive chemical reactions: an introduction to the field of thermodynamics
4	to learn the relationship between the electronic configurations of atoms and molecules and their chemical properties: an introduction to the field of quantum chemistry
5	to learn gas laws, kinetic-molecular theory of gases
6	to learn intermolecular forces, states of matter, properties of liquids and solids
7	to learn concentration, solubility, solutions, colligative properties
8	to learn chemical Reactions: Reactions in Aqueous Solutions
9	to learn general properties of solutions and regulations related to solutions

Mode of Delivery

Normal Education

Prerequisites and co-requisities

None

Recommended Optional Programme Components

None

Course Contents

Electronic Structure of Atoms., Dalton’s Atom Model, Electromagnetic Radiation , Atomic Spectra, Hydrogen Atom (The Bohr Atom), Quantum Theory, Quantum Numbers, Energy Levels and Electron Orbitals, Electron, Pauli Principle, Electronic Configurations of atoms.Periodic Table of Chemical Compounds, Classifying the Elements, Oxidation states of elements, Sizes of Atoms and Ions, Elektronegativity, Electron Affinity.Types of Chemical Compounds, Formulas of Chemical Compounds, Chemical Bonding ,Classification of Bonds, Ionic Bonding, Covalent Bonding, Coordinate Covalent Bonds, Multiple Covalent Bonds, Polar Covalent Bonds-Electronegativity, Writing Lewis Structures, Formal Charge, Resonance, Exceptions to the Octet Rule

Weekly Detailed Course Contents

Week	Theoretical	Practice	Laboratory
1	Elements, compounds, and mixtures; physical and chemical properties; SI system, units, measurements, accuracy and precision, significant figures, unit analysis Electronic Structure of Atoms, Dalton’s Atom Model,	Laboratory . Presentation of laboratory Woking regulations in General chemistry equipments,heating procedures.
2	Electromagnetic Radiation , Atomic Spectra, Hydrogen Atom (The Bohr Atom)	Measuring,precipitation,filitration and washing procedures .
3	Quantum Theory, Quantum Numbers, Energy Levels and Electron Orbitals, Electron, Pauli Principle, Electronic Configurations of atoms.	seperation , purification and crystallization procedures .
4	Periodic Table; classification of elements Oxidation states of elements, Sizes of Atoms and Ions, Electronegativity, Electron Affinity. Types of Chemical Compounds, Formulas of Chemical Compounds,	normal,fractionated,and vacuum distillation
5	Oxidation states of elements, Sizes of Atoms and Ions, Elektronegativity, Electron Affinity. Types of Chemical Compounds, Formulas of Chemical Compounds, The Mole Concept and Chemical Compounds, Composition of Oxidation states of elements, . The Mole Concept and Chemical Compounds, Composition of Chemical Compounds, Oxidation States: A Useful Tool in Describing Chemical Compounds,	chemical properties of matter.Law of conservation of mass
6	Chemical Bonding -I Classification of Bonds, Ionic Bonding, Covalent Bonding, Coordinate Covalent Bonds, Multiple Covalent Bonds, Polar Covalent Bonds-Electronegativity, Writing Lewis Structures, Formal Charge, Resonance, Exceptions to the Octet Rule	Extractions procedures Liquid-liquid extraction solid –liquid extraction
7	Chemical Bonding -II The Shapes of Molecules-VSEPR, Hybridization of Atomic Orbitals, Bond Energies, Valence Bond Theory , Multiple Covalent Bonds and Valence Bond Theory, Molecular Orbital Theory, Bonding in Metals, Metallic Bonding	definition of chemical solvents
8	Midterm Exam	Midterm Exam
9	Gases Introduction, Gas Pressure, The Simple Gas Laws, The Ideal Gas Equation and the General Gas Equation, Applications of the Ideal Gas Law, Gases in Chemical Reactions, Gases in Chemical Reactions, Mixtures of Gases and Partial Pressures, Kinetic-Molecular Theory of Gases, Gas Properties Relating to the Kinetic-Molecular Theory , Nonideal (Real) Gases	pH indicators
10	Liquids, Solids, and Intermolecular Forces Liquids, Intermolecular Forces and Some Properties of Liquids, Vaporization of Liquids: Vapor Pressure, Clausius – Clapeyron Equation	To Precipitate and filitration
11	Some Properties of Solids, Phase Diagrams (H2O, CO2, I2 ), Van der Waals Forces, Hydrogen Bonding , Crystal Structures, X-Ray Diffraction, Chemical Bonds as Intermolecular Forces, Energy Changes Involving Ionic Crystal Formation.	Chemical synthesis and calculation of chemical reaction yield.
12	Chemical Reactions: Reactions in Aqueous Solutions Balancing Chemical Equations, Chemical Equations and Stoichiometry, Chemical Reactions in Solutions, Molarity, Dilution of Solutions, Determining the Limiting Reactant in Chemical reactions, Other Practical Matters in Reaction Stoichiometry.	The effect of temperature on the rate of chemical reactions
13	The Nature of Aqueous Solutions, Precipitation Reactions and Net Ionic Equations, Acid-Base Reactions, Writing neutralization reactions, Oxidation-Reduction Reactions, Stoichiometry of Reactions in Aqueous Solutions	Qualitative analysis of cations
14	Solutions and Their Physical Properties Types of Solutions: Some Terminology, Solution Concentration, Mass%, Volume%, Mass/Volume%, ; ppm, ppb, Mole Fraction, Mole %, Molality, Intermolecular Forces, Solution Process and Enthalpy, Effect of Pressure and Temperature on Solubility, Solubilities of Gases (Temperature, Pressure Effect, Henry`s Law, Vapor Pressures of Solutions (Ideal Solutions and Non-Ideasl Solutions)	Qualitative analysis of anions
15	Osmotic Pressure, Freezing-Point Depression and Boiling-Point Elevation of Nonelectrolyte Solutions, Solutions of Electrolytes.	Qualitative analysis of carbon compounds