IB Chemistry HL: Part 1, 2, 3 (Full Set)

이재훈 선생님 


10% 할인
로그인
무엇을 배울까요?
IB Chemistry의 1~11 단원
1. Stoichiometry
2. Atomic Structure
3. Periodicity
4. Bonding
5. Thermodynamics
6. Kinetics
7. Equilibrium
8. Acid & Base
9. Reduction & Oxidation
10. Organic Chemistry
11. Spectral Analysis
커리큘럼
  • 1.2.1 Mole 1: mole to particles
    40:12
  • 1.2.2 Mole 2: balancing chemical equation
    23:56
  • 1.2.3 Mole 3: mole to mass
    36:24
  • 1.2.4 Mole 4: mole to volume of gas
    35:28
  • 1.2.5 Mole 5: mole to concentration
    40:06
  • 1.2.6 Mole 6: dilution
    27:11
  • 1.2.7 Mole 7: Titration
    35:35
  • 1.2.8 Mole 8: Back Titration
    33:38
  • 1.2.9 Limiting reactant, Excess reactant, Yield
    36:52
  • 1.3.1 Empirical & Molecular formula
    22:32
  • 1.3.2 Determining empirical formula 1: Using mass percentage composition
    26:54
  • 1.3.3 Determining empirical formula 2: Combustion analysis
    28:05
  • 1.4.1 Conditions of Ideal Gas, Pressure, Temperature
    42:58
  • 1.4.2 Gas Laws
    38:53
  • 1.4.3 Ideal gas law & Dalton's law of partial pressure
    30:45
  • 2.1.1 Atomic Structure
    37:11
  • 2.1.2 Isotope
    48:11
  • 2.1.3 History of Atomic models
    11:07
  • 2.2.1 Bohr's model of Hydrogen atom
    1:17:20
  • 2.2.2 Electronic Configuration
    1:07:50
  • 2.2.3 Electronic Configuration Q&A
    18:47
  • 12.1.1 Ionization energy 1: Definition of First Ionization energy
    27:50
  • 12.1.2 Ionization energy 2: Calculation of Ionization Energy
    30:26
  • 12.1.3 Ionization energy 3: Trend of First Ionization energy
    47:32
  • 12.1.4 Ionization energy 4: Successive Ionization energy
    34:52
  • 3.1.1 Composition of periodic table
    43:11
  • 3.1.2 Metal and Nonmetal, Melting & Boiling point across period
    27:56
  • 3.2.1 Seven Periodic Trend 1: Effective Nuclear Charge & Shielding Effect
    46:23
  • 3.2.2 Seven Periodic Trend 2: Electronegativity
    34:33
  • 3.2.3 Seven Periodic Trend 3: Atomic & Ionic Radius
    49:56
  • 3.2.4 Seven Periodic Trend 4: Ionization Energy 1
    1:14:29
  • 3.2.5 Seven Periodic Trend 4: Ionization Energy 2
    38:00
  • 3.2.6 Seven Periodic Trend 5: Electron Affinity, Metallic character, Nonmetallic character
    31:22
  • 3.2.7 Acid-Base Characteristic of Period 3 Oxide & Acid Rain
    51:42
  • 13.1.1 Transition metal core: Physical & Chemical properties of transition metal
    17:59
  • 13.1.2 Transition metal core: Atomic radius of transition metals
    11:26
  • 13.1.3 Transition metal core: Variable oxidation state
    24:01
  • 13.1.4 Chemical property: Metal Complex 1
    34:06
  • 13.1.5 Chemical property: Metal Complex 2
    13:24
  • 13.1.6 Transition metal: Catalyst
    21:52
  • 13.2.1 Colored Transition Metal Complex 1
    32:25
  • 13.2.2 Colored Transition Metal Complex 2: Factors affecting the splitting of d-orbital
    24:01
  • 4.1.1 Ionic bond 1: Formation and Strength of Ionic Bond
    1:08:16
  • 4.1.2 Ionic bond 2: Structure and Properties of Ionic Compound
    45:53
  • 4.1.3 Ionic bond 3: Naming of Ionic Compound
    20:21
  • 4.2.1 Metallic Bond: Metallic Bond & Properties
    31:02
  • 4.2.2 Metallic Bond: Alloy
    09:18
  • 4.3.1 Covalent bond 1: Formation of covalent bond
    18:44
  • 4.3.2 Lewis structure 1: Drawing Lewis structure
    59:44
  • 4.3.3 Lewis structure 2: Resonance structure
    30:44
  • 4.3.4 Covalent bond 2: Dative(coordinate) covalent bond
    33:16
  • 4.3.5 VSEPR Theory (SL)
    48:28
  • 4.3.6 VSEPR Theory (HL)
    36:56
  • 4.3.7 Polarity of covalent Bond & covalent Molecule
    1:07:16
  • 4.3.8 Structure and properties of covalent molecule
    15:38
  • 4.3.9 Giant covalent molecule
    49:20
  • 4.3.10 Nomenclature of covalent molecule
    12:57
  • 4.4.1 London Dispersion Force
    49:34
  • 4.4.2 Dipole-Dipole
    44:25
  • 4.4.3 Hydrogen bond
    1:17:29
  • 4.4.4 Naming Organic Molecules
    21:09
  • 14.1.1 Hybridization of Orbitals
    37:43
  • 14.1.2 Covalent Bond Type: Sigma bond & Pi bond
    29:31
  • 14.2.1 Formal charge
    44:02
  • 14.2.2 Ozone depletion
    43:00
  • 5.1.1 Laws of thermodynamics
    42:55
  • 5.1.2 Definition of enthalpy
    21:36
  • 5.1.3 Endothermic & Exothermic reaction
    51:00
  • 5.2.1 Calorimetry 1: Heat Calculation
    38:30
  • 5.2.2 Calorimetry 2: Enthalpy change of combustion
    43:02
  • 5.2.3 Calorimetry 3: Enthalpy change of neutralization
    45:47
  • 5.3.1 Enthalpy change of formation 1: Definition
    50:30
  • 5.3.2 Enthalpy change of formation 2: Calculation
    37:13
  • 5.4.1 Hess's Law 1
    22:00
  • 5.4.2 Hess's Law 2
    38:51
  • 5.4.3 Enthalpy change of combustion
    27:31
  • 5.5.1 Bond enthalpy 1: Definition
    40:11
  • 5.5.2 Bond enthalpy 2: Calculation & Source of error
    52:50
  • 5.5.3 Naming Organic Molecules
    21:09
  • 5.5.4 Bond enthalpy 3: Ozone depletion
    52:09
  • 15.1.1 Further types of enthalpies related to ionic compound
    54:03
  • 15.1.2 Born-Haber Cycle 1: Ionic solid to gas
    42:57
  • 15.1.3 Born-Haber Cycle 2: Ionic solid to solution
    39:14
  • 15.2.1 Entropy 1: Prediction of entropy change
    30:10
  • 15.2.2 Entropy 2: Absolute entropy and Calculation of entropy change
    22:46
  • 15.2.3 Gibb's Free Energy 1: Definition and Prediction of Spontaneity
    57:05
  • 15.2.4 Gibb's Free Energy 2: Gibb's Free Energy of formation
    12:52
  • 6.1.1 Definition of Reaction Rate
    1:09:24
  • 6.1.2 Techniques for measuring Rates
    1:11:58
  • 6.2 Collision Theory
    32:16
  • 6.3.1 Factors affecting Rate
    1:08:25
  • 6.3.2 Factors affecting Rate Questions
    35:18
  • 16.1.1 Rate Expression 1: Writing rate expression
    37:47
  • 16.1.2 Rate Expression 2: Determining Order of reactant
    29:59
  • 16.1.3 Rate Expression 3: Graphical Representation
    24:03
  • 16.2.1 Reaction Mechanism & Molecularity
    27:15
  • 16.2.2 Rate Determining Step
    28:11
  • 16.3 Calculation of Activation Energy
    53:10
  • 7.1.1 Reversible & Irreversible Reactions
    18:19
  • 7.1.2 Definition of Equilibrium
    34:24
  • 7.2.1 Equilibrium Constant (Kc)
    40:17
  • 7.2.2 Mathematical Relationship of Kc
    19:30
  • 7.3 Reaction Quotient (Q)
    25:22
  • 7.4.1 Le Chatelier's Principle
    1:00:52
  • 7.4.2 Le Chatelier's Principle Q&A
    22:21
  • 17.1 ICE Table
    45:11
  • 17.2.1 Relationship of Equilibrium Constant & Gibbs Free Energy
    30:05
  • 17.2.2 Extra: Relationship of Equilibrium constant & Rate constant
    08:49
  • 8.1 Characteristics of Acid & Base
    29:51
  • 8.2.1 Arrhenius Acid & Base: Definition
    17:12
  • 8.2.2 Bronsted Lowry Acid & Base 1: Definition
    30:53
  • 8.2.3 Bronsted Lowry Acid & Base 2: Conjugate Acid-Base pair
    29:06
  • 8.2.4 Bronsted Lowry Acid & Base 3: Amphiprotic species & Amphoteric species
    27:57
  • 8.2.5 Lewis Acid & Base 1: Definition
    28:24
  • 8.2.6 Lewis Acid & Base 2: Further application
    17:13
  • 8.3.1 Strong Acid & Base 1: Definition
    23:29
  • 8.3.2 Strong Acid & Base 2: Property of Different Strength
    25:56
  • 8.3.3 Strong Acid & Base 3: Conjugates of Strong & Weak species
    24:41
  • 8.3.4 Hydrolysis of Salt
    25:11
  • 8.4.1 Definition of pH & pOH
    36:55
  • 8.4.2 Auto Ionization of Water
    34:08
  • 8.4.3 Titration Calculation
    35:35
  • 8.4.4 Titration Curve
    29:05
  • 8.4.5 Titration of Strong Acid & Strong Base
    41:13
  • 8.5.1 Anthropogenic formation of acid rain
    18:41
  • 8.5.2 Problems of acid deposition
    14:23
  • 8.5.3 Solution to acid deposition
    09:42
  • 18.2.1 Titration of Weak acid - Strong base
    1:12:52
  • 18.2.2 Titration of Strong acid - Weak base
    30:18
  • 18.3 Common Ion Effect & Buffer solution
    45:46
  • 18.4.1 Indicator 1: Definition of Indicator
    16:46
  • 18.4.2 Indicator 2: Different types of indicators
    32:15
  • 9.1.1 Definition of Oxidation & Reduction
    21:04
  • 9.1.2 Oxidation State
    44:08
  • 9.1.3 Balancing Redox Reaction
    32:51
  • 9.2.1 Redox Titration 1: Iron with Permanganate ions
    16:05
  • 9.2.2 Redox Titration 2: Winkler Method
    20:02
  • 9.3.1 Activity Series
    36:17
  • 9.3.2 Voltaic Cell
    55:27
  • 9.3.3 Electrolytic Cell
    50:52
  • 19.1.1 Standard Electrode Potential
    48:57
  • 19.1.2 Cell Potential (E)
    21:04
  • 19.1.3 Spontaneity of Cell
    19:42
  • 19.2.1 Electrolysis of aqueous electrolyte
    50:02
  • 19.2.2 Electrolysis of aqueous electrolyte in series
    20:58
  • 19.2.3 Stoichiometry of Electrolysis
    30:47
  • 10.2.1 Homologous Series
    16:05
  • 10.2.2 Structural Isomer
    35:10
  • 10.2.3 Classification of Species
    39:57
  • 10.2.4 Types of Reaction, Bond Fission, Movement of electrons
    18:06
  • 10.2.5 Structure of Benzene (Kekule's Structure)
    34:43
  • 10.3.1 Alkane: Free Radical Substitution Reaction
    54:02
  • 10.3.2 Alkene: Addition Reaction
    51:21
  • 10.3.3 Alcohol: Oxidation Reaction
    51:45
  • 10.3.4 Halogenoalkane: Nucleophilic Substitution Reaction
    19:29
  • 10.3.5 Benzene: Electrophilic Substitution Reaction
    16:52
  • 10.3.6 Overall review of functional group chemistry
    15:58
  • 20.1.1 Halogenoalkane 1: Nucleophilic Substitution Reaction
    1:03:43
  • 20.1.2 Halogenoalkane 2: Q&A
    16:37
  • 20.1.3 Halogenoalkane 3: Rate of Nucleophilic Substitution Reaction
    25:37
  • 20.1.4 Alkene 1: Electrophilic Addition Reaction
    23:49
  • 20.1.5 Alkene 2: Markovnikov's Rule
    23:29
  • 20.1.6 Benzene: Electrophilic Substitution Reaction
    34:25
  • 20.1.7 Alcohol & Nitrobenzene: Reduction Reaction
    31:44
  • 20.1.8 Overall review of functional group chemistry
    16:53
  • 20.2 Synthetic Route
    31:08
  • 20.3.1 Geometrical Isomer 1: Cis & Trans Isomerism
    42:51
  • 20.3.2 Geometrical Isomer 2: E & Z Isomerism
    17:17
  • 20.3.3 Optical Isomer
    59:00
  • 11.1.1 Index of Hydrogen Deficiency
    17:43
  • 11.1.2 Mass Spectrometry
    21:11
  • 11.1.3 Infrared Spectrometry
    07:04
  • 11.1.4 HNMR Spectrometry: Low Resolution
    19:58
  • 21.1.1 HNMR Spectrometry: High Resolution
    22:57
설명

이재훈 선생님의 IB Chemistry (HL) 강좌입니다. 

다루는 단원은 Chapter 1~11 입니다. (SL과 HL 포함)

 

*이재훈 선생님의 강좌는 각 단원별 기본 문제풀이도 포함되어 있습니다!

*얼라이언스 에듀의 모든 IB 과목의 HL 과정 강좌는 SL 내용을 포함하고 있습니다!

 

일시정지 기간: 15일 3회

 

 

교재 다운받는 방법:

인강 수강 시에 선생님의 핵심 노하우가 담긴 필기용 교재를 학생분께 PDF로 드립니다. 

1) 인강 결제 후에 왼쪽 상단에 있는 "내 강의실"에서 구매한 강의를 누르면 아래 사진과 같은 수강 페이지가 보이게 됩니다. 

2) 각 단원의 첫 번째 영상을 보면 "첨부파일" 버튼이 있는데, 이를 누르면 PDF가 열려서 다운이 가능합니다^^

 

 

질문하기 방법:

인강 수강 시에 강의에서 궁금한 내용을 올리시면 다음날 까지는 답변을 드려요~

선생님의 빠르고 정확한 답변을 위해 학생분들은 아래 형식을 꼭 지켜주세요! 

 

1. 궁금한 부분의 강의 영상 번호 (1.1.1) 

2. 강의 영상의 시간

3. 궁금한 내용을 구체적으로!

 

 

강사 평점

★★★★★ 5.0

코멘트

    더보기