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GERİ DÖN
Ders Öğretim Planı
| Dersin Kodu | Dersin Adı | Dersin Türü | Yıl | Yarıyıl | AKTS | Kredi |
|---|---|---|---|---|---|---|
| ECVL107 | Chemistry | Ders | 1 | 1 | 0 | 3.00 |
Dersin Seviyesi
Lisans
Dersin Sunulduğu Dil
İngilizce
Dersin Amacı
To introduce the main subjects of chemistry, to give the fundamentals of chemistry to the engineering students.
Dersi Veren Öğretim GörevlisiGörevlileri
Öğrenme Çıktıları
| 1 | Students will learn the basic concepts of chemistry. |
| 2 | Students will learn to associate concepts learned in the class with chemical engineering topics |
| 3 | Students will draw the structures of simple molecules and learn basic information about the structure of atoms. |
| 4 | Students will write simple chemical reactions and complete it. They will evaluate the status of a reaction in terms of energy. |
| 5 | 1. Students will learn the basic concepts of chemistry. 2. Students will learn to associate concepts learned in the class with chemical engineering topics 3. Students will learn to make experiment related with lecture topic on laboratory. 4. Students will draw the structures of simple molecules and learn basic information about the structure of atoms. 5. Students will write simple chemical reactions and complete it. They will evaluate the status of a reaction in terms of energy. |
Öğrenim Türü
Birinci Öğretim
Dersin Ön Koşulu Olan Dersler
Ders İçin Önerilen Diğer Hususlar
Yok
Dersin İçeriği
The properties of material and measurements, atoms and atomic theory, periodic table chemical compounds, chemical reactions stoichiometry, gases and gas mixtures, chemical thermodynamics
Haftalık Ayrıntılı Ders İçeriği
| Hafta | Teorik | [OgretimYontemVeTeknikleri] | [OnHazirlik] |
|---|---|---|---|
| 1 | Properties of Matter, Classification of Matter, Measurement of Matter: SI (Metric) Units, Significant Figures Law of Conservation of Mass, Law of Constant Composition, Dalton’s Atomic Theory, Discovery of Electrons, The Nuclear Atom, Representation of Chemical Elements by Symbols, Atomic Mass, The Concept of The Mole and The Avogadro Constantt | ||
| 2 | Types of Chemical Compounds and Their Formulas, The Mole Concept, The Composition of Chemical Compounds, Oxidation States in Describing Chemical Compounds, Balancing Oxidation Reduction Equations Chemical Reactions and Chemical Equations, Chemical Equations and Stoichiometry, Determining the Limiting Reactant and Yield in Chemical Reactions | ||
| 3 | Properties of Gases, Gas Pressure, The Simple Gas Laws, The Ideal Gas Equation and the General Gas Equation, Applications of the Ideal Gas Equation, Gases in Chemical Reactions, Law of combining volumes (Gay-Lussac’s Law) Mixtures of Gases and Partial Pressures, Kinetic-Molecular Theory of Gases, Gas Properties Relating to the Kinetic-Molecular Theory, Nonideal (Real) Gases and The van der Waals Equation | ||
| 4 | Some Terminology in Thermochemistry, Heat, Heats of Reaction and Calorimetry, Work, The First Law of Thermodynamics, Heats of Reaction, ΔU ve ΔH, Hess’s Law, Standard Enthalpies of Formation | ||
| 5 | Midterm I | ||
| 6 | Electromagnetic Radiation, Atomic Spectra, Quantum Theory, The Bohr Atom, New Quantum Mechanics, Quantum Numbers and Electron Orbitals, Electron spin, Electron Configurations | ||
| 7 | The Periodic Table, Classification of elements, relation between Electron Configurations and periodic table, atomic radius, ionization energy, electron affinity | ||
| 8 | Introduction, Lewis Theory and Classification of Bonds, Ionic Bonding, Covalent Bonding, Multiple Covalent Bonds, Polar Covalent Bonds, Electronegativity, Writing Lewis Structures, Lewis Structures, Formal Charge, Exceptions to the Octet Rule, Resonance, Shapes of Molecules, VSEPR Theory, Molecule Examples | ||
| 9 | Intermolecular Forces and Some Properties of Liquids, Viscosity, SurfaceTension, Vapor Pressure, Clasius –Clapeyron Equation, Critical Point, Phase Diagrams (water), van der Waals Forces, Hydrogen bond | ||
| 10 | Midterm II | ||
| 11 | Solutions, Solution Concentrations, Solution Process and Solution Enthalpy, Calculation of Solution heat for Ionic Solutions, Effects of Temperature and Pressure on Solubility, Solubility of Gases, Vapor Pressures of Solutions, Osmotic Pressure, Freezing Point-Depression, Boiling point-Elevation, Electrolyte Solutions | ||
| 12 | Dynamic Equilibrum, Equilibrium Constant Expression, Relationship Involving Equilibrium Constants, The Magnitude of an Equilibrium Constant, Predicting the Direction of Net Change, Altering Equilibrium Conditions: Le Chatelier’s Principle | ||
| 13 | Arrhenius Theory, Bronsted-Lowry Theory, Self-Ionization of Water and the pH Scale, Strong Acids and Strong Bases, Weak Acids and Weak Bases, Acid-Base Equilibrum Calculations | ||
| 14 | Spontaneity, Entropy, The Second Law of Thermodynamic, Gibbs Energy Change, ΔG, Gibbs Energy Change and Equilibrium. . | ||
| 15 | Final |
Ders Kitabı Malzemesi Önerilen Kaynaklar
Planlanan Öğrenme Aktiviteleri ve Metodları
Değerlendirme
| Yarıyıl (Yıl) İçi Etkinlikleri | Adet | Değer |
|---|---|---|
| Ara Sınav | 1 | 100 |
| Toplam | 100 | |
| Yarıyıl (Yıl) Sonu Etkinlikleri | Adet | Değer |
| Final Sınavı | 1 | 100 |
| Toplam | 100 | |
| Yarıyıl (Yıl) İçi Etkinlikleri | 40 | |
| Yarıyıl (Yıl) Sonu Etkinlikleri | 60 | |
Staj Durumu
İş Yükü Hesaplaması
| Etkinlikler | Sayısı | Süresi (saat) | Toplam İş Yükü (saat) |
|---|---|---|---|
| Ara Sınav | 1 | 3 | 3 |
| Final Sınavı | 1 | 3 | 3 |
| Derse Katılım | 14 | 3 | 42 |
| Ara Sınav İçin Bireysel Çalışma | 1 | 25 | 25 |
| Final Sınavı içiin Bireysel Çalışma | 1 | 25 | 25 |
| Ev Ödevi | 3 | 5 | 15 |
| Toplam İş Yükü (saat) | 113 | ||
Program ve Öğrenme Çıktıları İlişkisi
| PÇ 1 | PÇ 2 | PÇ 3 | PÇ 4 | PÇ 5 | PÇ 6 | PÇ 7 | PÇ 8 | PÇ 9 | PÇ 10 | PÇ 11 | |
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| ÖÇ 5 |
* Katkı Düzeyi : 1 Çok düşük 2 Düşük 3 Orta 4 Yüksek 5 Çok yüksek