TutorPeak’in AP Kimya kursu, öğrencilere maddenin yapısını, kimyasal tepkimeleri ve kimyasal prensiplerin günlük hayattaki etkilerini öğretmeyi amaçlar. College Board müfredatına tam uyumlu bu kurs, hem teorik kimya bilgilerini hem de laboratuvar temelli uygulamaları kapsar.
Öğrenciler, kimyasal denklemleri analiz eder, matematiksel çıkarımlarda bulunur ve deneysel verileri yorumlar. Kurs boyunca kavramsal anlayış, problem çözme ve kanıta dayalı açıklama becerileri öne çıkar – bu da öğrencileri üniversite düzeyindeki bilim ve laboratuvar eğitimine hazırlar.
Kazanımlar:
Atom yapısı, periyodik eğilimler ve bağ kuramları
Stokiyometri, kinetik ve termodinamik süreçler
Kimyasal denge, asit-baz tepkimeleri ve elektrokimya
Moleküler ve iyonik bileşiklerin yapısı ve özellikleri
Deney verilerini analiz etme ve FRQ (açık uçlu soru) stratejileri
Öne Çıkan Özellikler:
AP müfredatına uygun bilimsel düşünme temelli dersler
Sanal laboratuvar simülasyonları ve uygulamalı problem setleri
Kavramsal anlatım ve görsel destekli öğrenme materyalleri
AP formatına uygun çoktan seçmeli ve açık uçlu sorularla pratik
Konu bazlı ilerleme takibi ve sınav hazırlık değerlendirmesi
Kimler İçin Uygun:
10–12. sınıf öğrencileri için uygundur. AP Kimya sınavına hazırlanan ve üniversite düzeyinde fen, mühendislik veya tıp eğitimi planlayan öğrenciler için idealdir.
Sunulan Diller:
Türkçe | İngilizce
Eğitim Özellikleri
- Dersler 69
- Sınav 0
- Süre 25 weeks
- Yetenek seviyesi Expert
- Dil English
- Öğrenciler 35
- Başarı Belgesi Hayır
- Değerlendirme Evet
- 6 Sections
- 69 Lessons
- 25 Weeks
- Atomic Structure and Properties- Master atomic theory, electron configuration, and periodic trends - Apply quantum mechanical principles to explain atomic behavior - Analyze periodic properties and predict chemical behavior from atomic structure8
- 1.11.1 Moles and Molar Mass Calculations
- 1.21.2 Mass Spectroscopy and Elemental Composition
- 1.31.3 Elemental Composition of Pure Substances
- 1.41.4 Composition of Mixtures
- 1.51.5 Atomic Structure and Electron Configuration
- 1.61.6 Photoelectron Spectroscopy (PES)
- 1.71.7 Periodic Trends: Atomic Radius, Ionization Energy, Electronegativity
- 1.81.8 Valence Electrons and Ionic Compounds
- Molecular and Ionic Compound Structure and Properties- Construct and interpret Lewis structures, VSEPR models, and molecular geometry - Explain intermolecular forces and their effects on physical properties - Apply bonding theories to predict molecular behavior and properties13
- 2.12.1 Types of Chemical Bonds (Ionic, Covalent, Metallic)
- 2.22.2 Intramolecular Force and Potential Energy
- 2.32.3 Structure of Ionic Solids
- 2.42.4 Structure of Metals and Alloys
- 2.52.5 Lewis Diagrams and Resonance Structures
- 2.62.6 Octet Rule Exceptions
- 2.72.7 VSEPR and Bond Hybridization
- 2.82.8 Molecular Geometry and Polarity
- 2.92.9 Intermolecular Forces (London Dispersion, Dipole-Dipole, Hydrogen Bonding)
- 2.102.10 Properties of Solids (Network Covalent, Metallic, Ionic, Molecular)
- 2.112.11 Ideal Gas Law and Kinetic Molecular Theory
- 2.122.12 Deviations from Ideal Gas Behavior
- 2.132.13 Phase Diagrams and Phase Changes
- Intermolecular Forces and Properties- Analyze solutions, solubility, and colligative properties - Apply gas laws and kinetic molecular theory to real-world problems - Predict and explain phase changes and physical property variations9
- 3.13.1 Solutions and Mixtures
- 3.23.2 Representations of Solutions (Molarity, Molality, Percent Composition)
- 3.33.3 Solubility Rules and Solution Formation
- 3.43.4 Solubility Equilibria and Solubility Product (Ksp)
- 3.53.5 Spectroscopy and Light Absorption (Beer-Lambert Law)
- 3.63.6 Colligative Properties: Vapor Pressure Lowering
- 3.73.7 Colligative Properties: Boiling Point Elevation and Freezing Point Depression
- 3.83.8 Colligative Properties: Osmotic Pressure
- 3.93.9 Chromatography and Separation Techniques
- Chemical Reactions- Master stoichiometry, reaction types, and balanced equations - Analyze oxidation-reduction reactions and electrochemistry - Apply titration techniques and acid-base chemistry principles12
- 4.14.1 Introduction to Chemical Reactions and Net Ionic Equations
- 4.24.2 Physical and Chemical Changes
- 4.34.3 Stoichiometry and Limiting Reactants
- 4.44.4 Reaction Yield and Percent Yield
- 4.54.5 Types of Chemical Reactions (Synthesis, Decomposition, Single/Double Replacement)
- 4.64.6 Acid-Base Reactions and pH
- 4.74.7 Oxidation-Reduction (Redox) Reactions
- 4.84.8 Balancing Redox Reactions (Half-Reaction Method)
- 4.94.9 Electrochemistry: Galvanic and Electrolytic Cells
- 4.104.10 Standard Reduction Potentials
- 4.114.11 Quantitative Titration Analysis
- 4.124.12 Gravimetric and Spectrophotometric Analysis
- Kinetics- Determine reaction rates and analyze factors affecting reaction speed - Interpret experimental kinetic data and rate laws - Apply collision theory and reaction mechanisms to explain rate behavior11
- 5.15.1 Introduction to Reaction Rates
- 5.25.2 Rate Laws and Reaction Order (Zero, First, Second Order)
- 5.35.3 Concentration-Time Relationships and Half-Life
- 5.45.4 Integrated Rate Laws
- 5.55.5 Experimental Determination of Rate Laws
- 5.65.6 Effect of Concentration on Reaction Rates
- 5.75.7 Elementary Reactions and Reaction Mechanisms
- 5.85.8 Collision Theory and Activation Energy
- 5.95.9 Energy Profiles and Transition States
- 5.105.10 Catalysts and Reaction Rate Enhancement
- 5.115.11 Steady-State Approximation and Multi-Step Mechanisms
- Thermodynamics and Equilibrium- Calculate energy changes in chemical reactions using thermodynamic principles - Analyze equilibrium systems and apply Le Chatelier's Principle - Predict spontaneity using entropy, enthalpy, and Gibbs free energy16
- 6.16.1 Endothermic and Exothermic Processes
- 6.26.2 Enthalpy of Formation and Hess’s Law
- 6.36.3 Bond Energies and Reaction Energy Calculations
- 6.46.4 Heat Transfer and Calorimetry
- 6.56.5 Introduction to Entropy
- 6.66.6 Gibbs Free Energy and Spontaneity
- 6.76.7 Thermodynamic Favorability and Temperature
- 6.86.8 Reversible Reactions and Equilibrium
- 6.96.9 Equilibrium Constants (Kc, Kp, Ksp, Ka, Kb)
- 6.106.10 Le Chatelier’s Principle and Stress on Equilibrium Systems
- 6.116.11 Calculations Involving Equilibrium Constants
- 6.126.12 Acid-Base Equilibria and Buffer Solutions
- 6.136.13 pH, pOH, and the Henderson-Hasselbalch Equation
- 6.146.14 Titration Curves and Acid-Base Indicators
- 6.156.15 Solubility Equilibria and the Common Ion Effect
- 6.166.16 Relationship Between Gibbs Free Energy and Equilibrium
