College Board AP Chemıstry

AP Kimya Konuları
AP Chemistry Syllabus 2025–2026

AP Kimya, öğrencileri üniversite seviyesinde genel kimya bilgisiyle tanıştıran yoğun ve kapsamlı bir derstir. Bu sayfada AP Kimya müfredatında yer alan AP Kimya konuları ve detaylı içerikleri bulabilirsiniz.

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Bu rehberde

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9 ana üniteAtomic Structure, Kinetics, Thermodynamics, Equilibrium, Acids/Bases, Electrochemistry
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Türkçe konu özetleriHızlı başvuru için
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Detaylı İngilizce syllabusLearning objectives & essential knowledge
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AP Kimya özel dersBirebir destek ile 5 hedefi
26 yılKimya deneyimi
ODTÜMezunu
AP ChemistryUzmanı
ÜcretsizTanışma dersi
AP Kimya Konuları (Türkçe)

AP Kimya Konuları — 9 Ana Ünite

1. Atomic Structure and Properties

Atom modelleri, proton-nötron-elektron yapısı, izotoplar, ortalama atom kütlesi, elektron konfigürasyonları ve periyodik eğilimler

2. Molecular and Ionic Compound Structure

İyonik ve kovalent bağlar, Lewis yapıları, formal yük, rezonans, moleküler geometri, VSEPR modeli

3. Intermolecular Forces and Properties

London, dipol-dipol, hidrojen bağları, madde halleri, buharlaşma, çözünürlük, IMF etkileri

4. Chemical Reactions

Tepkime türleri, net iyon denklemleri, yükseltgenme-indirgenme tepkimeleri, stokiyometri

5. Kinetics

Tepkime hızları, hız yasaları, mekanizmalar, enerji profilleri, Arrhenius denklemi

6. Thermodynamics

Endotermik/ekzotermik tepkimeler, entalpi (ΔH) hesaplamaları, Hess yasası, entropi, Gibbs serbest enerji

7. Equilibrium

Kimyasal denge kavramı, Kc ve Kp sabitleri, Le Châtelier ilkesi, asit-baz dengeleri, Ksp

8. Acids and Bases

Brønsted-Lowry tanımı, pH/pOH hesaplamaları, zayıf/kuvvetli asit ve bazlar, titrasyon, tampon çözeltiler, Henderson-Hasselbalch

9. Applications of Thermodynamics

Elektrokimya: galvanik hücreler, elektroliz, hücre potansiyeli ve ΔG, redoks tepkimeleri, serbest enerji ve denge bağlantısı

📘 Tüm bu konular, AP sınavının hem çoktan seçmeli hem de serbest yanıt (free response) kısımlarında sorulmaktadır. Öğrencilerimizin bu konularda tam hakimiyet kazanabilmesi için bire bir özel derslerde hem teorik temelleri hem de soru çözüm tekniklerini işliyoruz.

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AP Chemıstry Syllabus (Englısh)

AP Chemistry Topics — Detailed Syllabus

Complete breakdown based on the official College Board AP Chemistry Course and Exam Description.

Unit 1: Atomic Structure and Properties▼
  • 1.1 Moles and Molar Mass – Avogadro's number, mole concept, n = m/Ma
  • 1.2 Mass Spectra of Elements – Isotopes, relative abundance, average atomic mass
  • 1.3 Elemental Composition of Pure Substances – Empirical formula, law of definite proportions
  • 1.4 Composition of Mixtures – Pure substances vs mixtures, elemental analysis
  • 1.5 Atomic Structure and Electron Configuration – Coulomb's law, shells/subshells, core/valence electrons, ionization energy
  • 1.6 Photoelectron Spectroscopy (PES) – Electron energies, subshell identification
  • 1.7 Periodic Trends – Ionization energy, atomic/ionic radii, electron affinity, electronegativity
  • 1.8 Valence Electrons and Ionic Compounds – Bond formation, typical ionic charges
Unit 2: Molecular and Ionic Compound Structure and Properties▼
  • 2.1 Types of Chemical Bonds – Electronegativity, nonpolar/polar covalent, ionic bonds, metallic bonding
  • 2.2 Intermolecular Forces and Potential Energy – Bond length, bond energy, Coulomb's law
  • 2.3 Structure of Ionic Solids – 3D lattice, electrostatic attractions
  • 2.4 Structure of Metals and Alloys – Sea of electrons, interstitial/substitutional alloys
  • 2.5 Lewis Diagrams – Lewis structures construction
  • 2.6 Resonance and Formal Charge – Resonance structures, formal charge calculations
  • 2.7 VSEPR and Hybridization – Molecular geometry, bond angles, dipole moment, sp/sp²/sp³ hybridization, sigma/pi bonds
Unit 3: Properties of Substances and Mixtures▼
  • 3.1 Intermolecular Forces – London dispersion, dipole-dipole, hydrogen bonding, ion-dipole
  • 3.2 Properties of Solids – Ionic, covalent network, molecular, metallic solids; alloys
  • 3.3 Solids, Liquids and Gases – Particulate models, phase changes
  • 3.4 Ideal Gas Law – PV = nRT, partial pressures, mole fraction
  • 3.5 Kinetic Molecular Theory – Maxwell-Boltzmann distribution, KE = ½mv²
  • 3.6 Deviation from Ideal Gas Law – Real gases, interparticle attractions, particle volumes
  • 3.7 Solutions and Mixtures – Molarity, homogeneous/heterogeneous mixtures
  • 3.8 Representations of Solutions – Particulate models
  • 3.9 Separation of Solutions and Mixtures – Chromatography, distillation
  • 3.10 Solubility – "Like dissolves like"
  • 3.11 Spectroscopy and EM Spectrum – Microwave (rotational), IR (vibrational), UV/Vis (electronic)
  • 3.12 Properties of Photons – c = λν, E = hν
  • 3.13 Beer-Lambert Law – A = εbc, absorbance, concentration
Unit 4: Chemical Reactions▼
  • 4.1 Introduction to Reactions – Physical vs chemical changes, evidence of reaction
  • 4.2 Net Ionic Equations – Balanced molecular, complete ionic, net ionic equations
  • 4.3 Representations of Reactions – Particulate representations
  • 4.4 Physical and Chemical Changes – Bond breaking/forming, intermolecular interactions
  • 4.5 Stoichiometry – Reacting amounts, limiting reactant, theoretical yield
  • 4.6 Introduction to Titration – Equivalence point, endpoint, titrant, analyte
  • 4.7 Types of Chemical Reactions – Acid-base, redox, precipitation, combustion
  • 4.8 Introduction to Acid-Base Reactions – Brønsted-Lowry acids/bases, conjugate pairs
  • 4.9 Oxidation-Reduction (Redox) Reactions – Half-reactions, oxidation numbers
Unit 5: Kinetics▼
  • 5.1 Reaction Rates – Rate = Δ[concentration]/Δt, factors affecting rate
  • 5.2 Introduction to Rate Law – Rate = k[A]^m[B]^n, order of reaction, rate constant
  • 5.3 Concentration Changes Over Time – Integrated rate laws, half-life t₁/₂ = 0.693/k (first order)
  • 5.4 Elementary Reactions – Molecularity, rate law from elementary step
  • 5.5 Collision Model – Activation energy, orientation, Maxwell-Boltzmann distribution
  • 5.6 Reaction Energy Profile – Activation energy, transition state, ΔE
  • 5.7 Introduction to Reaction Mechanisms – Elementary steps, intermediates, catalysts
  • 5.8 Reaction Mechanism and Rate Law – Rate-determining step
  • 5.9 Pre-Equilibrium Approximation – Fast equilibrium before rate-determining step
  • 5.10 Multistep Reaction Energy Profile – Multiple activation energies
  • 5.11 Catalysis – Homogeneous/heterogeneous catalysts, enzymes, lower activation energy
Unit 6: Thermodynamics▼
  • 6.1 Endothermic and Exothermic Processes – Heat transfer, system/surroundings
  • 6.2 Energy Diagrams – Endothermic vs exothermic profiles
  • 6.3 Heat Transfer and Thermal Equilibrium – Molecular collisions, thermal equilibrium
  • 6.4 Heat Capacity and Calorimetry – q = mcΔT, first law of thermodynamics
  • 6.5 Energy of Phase Changes – Enthalpy of fusion/vaporization, constant temperature during phase change
  • 6.6 Introduction to Enthalpy of Reaction – ΔH, exothermic/endothermic
  • 6.7 Bond Enthalpies – ΔH = Σ(bonds broken) – Σ(bonds formed)
  • 6.8 Enthalpies of Formation – ΔH°rxn = ΣΔHf°products – ΣΔHf°reactants
  • 6.9 Hess's Law – Enthalpy change independent of pathway
Unit 7: Equilibrium▼
  • 7.1 Introduction to Equilibrium – Dynamic equilibrium, reversible reactions
  • 7.2 Direction of Reversible Reactions – Kc and Kp expressions
  • 7.3 Reaction Quotient and Equilibrium Constant – Q vs K, predicting direction
  • 7.4 Calculating the Equilibrium Constant – From experimental data
  • 7.5 Magnitude of the Equilibrium Constant – K > 1 favors products, K < 1 favors reactants
  • 7.6 Properties of the Equilibrium Constant – Reversing reactions, multiplying coefficients, adding reactions
  • 7.7 Calculating Equilibrium Concentrations – ICE tables, approximations
  • 7.8 Representations of Equilibrium – Particulate models
  • 7.9 Le Châtelier's Principle – Effect of concentration, pressure, temperature changes
  • 7.10 Reaction Quotient and Le Châtelier – Q vs K response to stress
  • 7.11 Introduction to Solubility Equilibria – Ksp, molar solubility
  • 7.12 Common Ion Effect – Reduced solubility in presence of common ion
Unit 8: Acids and Bases▼
  • 8.1 Introduction to Acids and Bases – pH, pOH, Kw, neutral solutions
  • 8.2 pH and pOH of Strong Acids and Bases – Complete dissociation
  • 8.3 Weak Acid and Base Equilibria – Ka, Kb, pKa, percent ionization
  • 8.4 Acid-Base Reactions and Buffers – Strong/weak combinations, buffer solutions
  • 8.5 Acid-Base Titrations – Titration curves, equivalence point, half-equivalence point, polyprotic acids
  • 8.6 Molecular Structures of Acids and Bases – Electronegativity, inductive effects, resonance stabilization
  • 8.7 pH and pKa – Relationship between pH, pKa, and protonation state
  • 8.8 Properties of Buffers – Resistance to pH change
  • 8.9 Henderson-Hasselbalch Equation – pH = pKa + log([A⁻]/[HA])
  • 8.10 Buffer Capacity – Concentration ratio effects
  • 8.11 pH and Solubility – Effect of pH on solubility of salts
Unit 9: Applications of Thermodynamics▼
  • 9.1 Introduction to Entropy – ΔS, dispersal of matter and energy
  • 9.2 Absolute Entropy and Entropy Change – ΔS°rxn = ΣS°products – ΣS°reactants
  • 9.3 Gibbs Free Energy and Thermodynamic Favorability – ΔG° = ΔH° – TΔS°, ΔG° < 0 is thermodynamically favored
  • 9.4 Thermodynamic and Kinetic Control – Kinetics vs thermodynamics
  • 9.5 Free Energy and Equilibrium – ΔG° = –RT ln K, relationship between K and ΔG°
  • 9.6 Free Energy of Dissolution – Factors affecting solubility
  • 9.7 Coupled Reactions – Using favorable reactions to drive unfavorable ones
  • 9.8 Galvanic (Voltaic) and Electrolytic Cells – Oxidation at anode, reduction at cathode, salt bridge, electron flow
  • 9.9 Cell Potential and Free Energy – ΔG° = –nFE°, E°cell = E°cathode – E°anode
  • 9.10 Cell Potential Under Nonstandard Conditions – Nernst equation (qualitative), Q vs K
  • 9.11 Electrolysis and Faraday's Law – I = q/t, stoichiometry of electrolysis

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