Канал: Mike Sugiyama Jones (MSJ Chem)

R3.4.3 Heterolytic bond fission

R3.4.3 Heterolytic bond fission

R3.3.1 / R3.3.2 Homolytic bond fission

R3.3.1 / R3.3.2 Homolytic bond fission

S2.3.2 Factors that affect the strength of the metallic bond

S2.3.2 Factors that affect the strength of the metallic bond

S2.3.1 Metallic bonding and properties of metals

S2.3.1 Metallic bonding and properties of metals

S2.1.3 Factors that affect lattice enthalpy

S2.1.3 Factors that affect lattice enthalpy

R1.2.5 Born Haber cycle for sodium oxide (Na2O)

R1.2.5 Born Haber cycle for sodium oxide (Na2O)

R1.2.5 Born-Haber cycle for calcium oxide (CaO)

R1.2.5 Born-Haber cycle for calcium oxide (CaO)

R1.2.5 Born-Haber cycle for magnesium chloride (MgCl2)

R1.2.5 Born-Haber cycle for magnesium chloride (MgCl2)

R1.2.5 Born Haber cycles part one (HL)

R1.2.5 Born Haber cycles part one (HL)

S1.4.4 Percentage composition by mass

S1.4.4 Percentage composition by mass

S2.4.1 / S2.4.2 The bonding triangle

S2.4.1 / S2.4.2 The bonding triangle

S1.3.7 Successive ionisation energies (HL)

S1.3.7 Successive ionisation energies (HL)

S1.2.3 Mass spectra of elements (HL)

S1.2.3 Mass spectra of elements (HL)

S1.3.1 The Electromagnetic Spectrum

S1.3.1 The Electromagnetic Spectrum

S1.3.3 / S1.3.4 Atomic orbitals and sub-levels

S1.3.3 / S1.3.4 Atomic orbitals and sub-levels

S1.3.5 Electron configurations and the Aufbau principle (part two)

S1.3.5 Electron configurations and the Aufbau principle (part two)

S1.3.5 Electron configurations and the Aufbau principle (part one)

S1.3.5 Electron configurations and the Aufbau principle (part one)

S1.2.2 Calculating relative atomic mass

S1.2.2 Calculating relative atomic mass

S1.2.2 Isotopes

S1.2.2 Isotopes

S1.3.2 The hydrogen emission spectrum

S1.3.2 The hydrogen emission spectrum

S1.2.1 Atomic number and mass number

S1.2.1 Atomic number and mass number

R3.2.14 Cell potential and Gibbs free energy (HL)

R3.2.14 Cell potential and Gibbs free energy (HL)

R3.2.13 Calculating cell potential (HL)

R3.2.13 Calculating cell potential (HL)

R3.2.12 Standard electrode potentials (HL)

R3.2.12 Standard electrode potentials (HL)

R3.1.16 Buffer solutions (HL)

R3.1.16 Buffer solutions (HL)

R3.1.12 Salt hydrolysis (HL)

R3.1.12 Salt hydrolysis (HL)

R3.1.11 Ka, pKa, Kb, pKb, Kw, pKw (HL)

R3.1.11 Ka, pKa, Kb, pKb, Kw, pKw (HL)

S3.1.4 Properties of metals and non-metals

S3.1.4 Properties of metals and non-metals

S3.1.1 The metalloids

S3.1.1 The metalloids

R2.2.6 Intermediates and catalysts (HL)

R2.2.6 Intermediates and catalysts (HL)

R2.2.8 Molecularity (HL)

R2.2.8 Molecularity (HL)

R2.2.13 Calculating activation energy (HL)

R2.2.13 Calculating activation energy (HL)

R2.2.11 The rate constant k (HL)

R2.2.11 The rate constant k (HL)

R2.2.12 The Arrhenius equation (HL)

R2.2.12 The Arrhenius equation (HL)

R3.2.5 Comparison of electrochemical cells

R3.2.5 Comparison of electrochemical cells

R3.2.6 Voltaic cells

R3.2.6 Voltaic cells

R3.2.1 Oxidizing and reducing agents

R3.2.1 Oxidizing and reducing agents

$1.2 Mole fraction and mole percent$

1.2 Mole fraction and mole percent

10.1 Naming amides (SL)

10.1 Naming amides (SL)

10.1 Naming nitriles (SL)

10.1 Naming nitriles (SL)

S1.4.5 Concentration of solutions

S1.4.5 Concentration of solutions

S1.4.6 Avogadro's law

S1.4.6 Avogadro's law

S2.2.1 The octet rule

S2.2.1 The octet rule

Bonding and electrcial conductivty

Bonding and electrcial conductivty

S2.2.7 Structure and properties of covalent compounds

S2.2.7 Structure and properties of covalent compounds

1.2 Calculating empirical formula from percent composition

1.2 Calculating empirical formula from percent composition

S1.4.4 Empirical and molecular fomulas

S1.4.4 Empirical and molecular fomulas

S1.4.2 Relative atomic mass and molecular mass

S1.4.2 Relative atomic mass and molecular mass

S1.4.3 Molar mass

S1.4.3 Molar mass

S1.4.1 The mole concept

S1.4.1 The mole concept

S1.5.1 and S1.5.2 Ideal gases and deviation from ideal gas behaviour

S1.5.1 and S1.5.2 Ideal gases and deviation from ideal gas behaviour

S1.5.3 The gas laws (part 2)

S1.5.3 The gas laws (part 2)

S1.5.3 The gas laws (part 1)

S1.5.3 The gas laws (part 1)

S1.5.4 The Ideal gas equation

S1.5.4 The Ideal gas equation

R3.4.9 SN1 and SN2 mechanisms (HL)

R3.4.9 SN1 and SN2 mechanisms (HL)

R3.2.1 Disproportionation reactions

R3.2.1 Disproportionation reactions

S1.5.3 Molar volume of a gas

S1.5.3 Molar volume of a gas

S1.4.3 Calculating mass in grams from amount (in mol)

S1.4.3 Calculating mass in grams from amount (in mol)

S1.4.3 Calculating amount (in mol) of substance

S1.4.3 Calculating amount (in mol) of substance

R2.1.4 Theoretical yield and percent yield

R2.1.4 Theoretical yield and percent yield

R2.1.3 Limiting and excess reactants

R2.1.3 Limiting and excess reactants

R3.2.10 Reduction of carbonyl compounds

R3.2.10 Reduction of carbonyl compounds

R3.4.13 Nitration of benzene (HL)

R3.4.13 Nitration of benzene (HL)

R2.2.2 Collision theory

R2.2.2 Collision theory

R2.2.4 Activation energy

R2.2.4 Activation energy

20.1 Comparison of SN1 and SN2 reactions (HL)

20.1 Comparison of SN1 and SN2 reactions (HL)

R3.4.2 Nucleophilic substitution reactions

R3.4.2 Nucleophilic substitution reactions

R3.4.1 / 3.4.4 Electrophiles and nucleophiles

R3.4.1 / 3.4.4 Electrophiles and nucleophiles

R3.4.11 Electrophilic addition reactions (HL)

R3.4.11 Electrophilic addition reactions (HL)

14.1 Catalytic destruction of ozone (HL)

14.1 Catalytic destruction of ozone (HL)

8.5 Effects and reduction of acid deposition (SL)

8.5 Effects and reduction of acid deposition (SL)

18.1 Lewis theory vs Bronsted-Lowry theory (HL)

18.1 Lewis theory vs Bronsted-Lowry theory (HL)

R3.4.6 / R3.4.7 Lewis theory of acids and bases (HL)

R3.4.6 / R3.4.7 Lewis theory of acids and bases (HL)

S3.2.2 Diols and dicarboxylic acids

S3.2.2 Diols and dicarboxylic acids

S3.1.5 Acid deposition

S3.1.5 Acid deposition

S2.2.15 Sigma and pi bonds (HL)

S2.2.15 Sigma and pi bonds (HL)

14.1 Calculating wavelength from bond enthalpy values (O2 and O3) (HL)

14.1 Calculating wavelength from bond enthalpy values (O2 and O3) (HL)

R2.2.9 Reaction mechanisms (HL)

R2.2.9 Reaction mechanisms (HL)

4.4 Group 16 hydrides (SL)

4.4 Group 16 hydrides (SL)

R2.2.10 Orders of reaction (HL)

R2.2.10 Orders of reaction (HL)

R2.2.6 Rate expressions (rate equations) (HL)

R2.2.6 Rate expressions (rate equations) (HL)

5.3 The ozone layer (SL)

5.3 The ozone layer (SL)

13.2 The Spectrochemical series (HL)

13.2 The Spectrochemical series (HL)

13.2 Factors that affect the colour of complex ions (HL)

13.2 Factors that affect the colour of complex ions (HL)

S3.1.10 Colour of complex ions (HL)

S3.1.10 Colour of complex ions (HL)

S3.1.9 Oxidation states of the transition elements (HL)

S3.1.9 Oxidation states of the transition elements (HL)

R3.4.5 Test for unsaturation

R3.4.5 Test for unsaturation

R3.4.8 Deduce the charge and oxidation state of a central metal ion (HL)

R3.4.8 Deduce the charge and oxidation state of a central metal ion (HL)

S3.1.8 Ligands (HL)

S3.1.8 Ligands (HL)

S3.1.8 Complex ions (HL)

S3.1.8 Complex ions (HL)

S3.1.8 Introduction to the transition elements (HL)

S3.1.8 Introduction to the transition elements (HL)

S3.1.3 Trends in ionic radii

S3.1.3 Trends in ionic radii

R3.2.2 Writing net ionic equations

R3.2.2 Writing net ionic equations

S1.3.5 Electron configurations of ions

S1.3.5 Electron configurations of ions

S3.2.5 Naming halogenoalkanes

S3.2.5 Naming halogenoalkanes

S3.1.2 Electron configurations and the periodic table

S3.1.2 Electron configurations and the periodic table

S3.2.2 Identifying functional groups

S3.2.2 Identifying functional groups

S3.2.2 Functional groups

S3.2.2 Functional groups

S3.2.2 Esters

S3.2.2 Esters

S3.2.6 Classification of organic compounds

S3.2.6 Classification of organic compounds

S3.2.4 Factors that affect the boiling points of organic compounds

S3.2.4 Factors that affect the boiling points of organic compounds

9.1 The Winkler method (SL)

9.1 The Winkler method (SL)

R3.2.3 The activity series

R3.2.3 The activity series

S2.1.2 Writing formulas of ionic compounds

S2.1.2 Writing formulas of ionic compounds

S2.2.6 Polar and non-polar molecules

S2.2.6 Polar and non-polar molecules

S2.2.5 Polar and non-polar covalent bonds

S2.2.5 Polar and non-polar covalent bonds

S2.2.1 / S2.2.2 Covalent bonding

S2.2.1 / S2.2.2 Covalent bonding

S2.2.8 / S2.2.9 Intermolecular forces

S2.2.8 / S2.2.9 Intermolecular forces

4.1 Electronegativity and bonding (SL)

4.1 Electronegativity and bonding (SL)

15.1 Enthalpy change of solution and hydration (HL)

15.1 Enthalpy change of solution and hydration (HL)

S3.2.2 Ethers

S3.2.2 Ethers

20.1 Comparison of SN1 and SN2 reactions (HL)

20.1 Comparison of SN1 and SN2 reactions (HL)

S2.1.2 Polyatomic ions

S2.1.2 Polyatomic ions

20.3 Diastereomers (HL)

20.3 Diastereomers (HL)

S3.2.7 The use of a polarimeter (HL)

S3.2.7 The use of a polarimeter (HL)

S3.2.7 Optical isomerism part 1 (HL)

S3.2.7 Optical isomerism part 1 (HL)

R3.4.11 / R3.4.12 Markovnikov's rule (HL)

R3.4.11 / R3.4.12 Markovnikov's rule (HL)

15.1 Enthalpy change of solution and hydration (HL)

15.1 Enthalpy change of solution and hydration (HL)

C.7 Calculating energy released in nuclear reactions (HL)

C.7 Calculating energy released in nuclear reactions (HL)

Organic acids and bases (HL)

Organic acids and bases (HL)

S3.2.1 Structural formulas of organic compounds

S3.2.1 Structural formulas of organic compounds

S3.2.6 Structural isomerism

S3.2.6 Structural isomerism

S3.2.5 Naming aldehydes and ketones

S3.2.5 Naming aldehydes and ketones

S3.2.5 Naming carboxylic acids

S3.2.5 Naming carboxylic acids

S3.2.5 Naming alcohols

S3.2.5 Naming alcohols

S3.2.5 Naming alkynes

S3.2.5 Naming alkynes

S3.2.5 Naming alkenes

S3.2.5 Naming alkenes

S3.2.5 Naming alkanes (straight-chain and cyclic alkanes)

S3.2.5 Naming alkanes (straight-chain and cyclic alkanes)

S2.2.8 Solubility and intermolecular forces

S2.2.8 Solubility and intermolecular forces

S3.1.3 Trends in atomic radii

S3.1.3 Trends in atomic radii

R2.3.4 Le Chatelier's principle (changes in temperature)

R2.3.4 Le Chatelier's principle (changes in temperature)

R2.3.4 Le Chatelier's principle (changes in pressure)

R2.3.4 Le Chatelier's principle (changes in pressure)

R2.3.4 Le Chatelier's principle (changes in concentration)

R2.3.4 Le Chatelier's principle (changes in concentration)

Areas of difficulty (HL)

Areas of difficulty (HL)

Areas of difficulty (SL)

Areas of difficulty (SL)

1.3 Back titration

1.3 Back titration

Exam tips for the IB chemistry exam (SL/HL)

Exam tips for the IB chemistry exam (SL/HL)

Exam overview (HL)

Exam overview (HL)

Exam overview (SL)

Exam overview (SL)

R2.3.1 Physical equilibrium

R2.3.1 Physical equilibrium

R2.3.1 Chemical equilibrium

R2.3.1 Chemical equilibrium

S2.2.11 Molecules and ions with delocalised pi electrons (HL)

S2.2.11 Molecules and ions with delocalised pi electrons (HL)

S3.2.5 Naming branched-chain alkanes

S3.2.5 Naming branched-chain alkanes

R2.2.1 Rate of reaction

R2.2.1 Rate of reaction

R2.2.3 Factors that affect the rate of reaction

R2.2.3 Factors that affect the rate of reaction

R3.1.10 Calculating pH of weak acids and bases (HL)

R3.1.10 Calculating pH of weak acids and bases (HL)

R3.1.10 Calculating the Ka or Kb of a weak acid or base (HL)

R3.1.10 Calculating the Ka or Kb of a weak acid or base (HL)

R3.1.5 Ionic product constant of water, Kw

R3.1.5 Ionic product constant of water, Kw

R3.1.6 Distinguish between strong and weak acids and bases

R3.1.6 Distinguish between strong and weak acids and bases

R3.1.6 Strong and weak acids and bases

R3.1.6 Strong and weak acids and bases

R3.1.4 The pH scale

R3.1.4 The pH scale

R3.1.4 Calculating the pH of strong acids

R3.1.4 Calculating the pH of strong acids

R3.1.10 Acid and base dissociation constants Ka and Kb (HL)

R3.1.10 Acid and base dissociation constants Ka and Kb (HL)

R3.1.7 / R3.2.4 Reactions of acids and bases

R3.1.7 / R3.2.4 Reactions of acids and bases

D.2 Solubility and bioavailability of aspirin (SL)

D.2 Solubility and bioavailability of aspirin (SL)

6.1 Activation energy (SL)

6.1 Activation energy (SL)

6.1 Collision theory (SL)

6.1 Collision theory (SL)

S1.2.1 Atomic structure

S1.2.1 Atomic structure

S3.2.7 Cis-trans isomerism (HL)

S3.2.7 Cis-trans isomerism (HL)

20.3 E/Z isomerism (HL)

20.3 E/Z isomerism (HL)

20.3 Conformational isomers of the alkanes (HL)

20.3 Conformational isomers of the alkanes (HL)

20.1 Reduction of nitrobenzene (HL)

20.1 Reduction of nitrobenzene (HL)

R3.1.3 Amphiprotic species

R3.1.3 Amphiprotic species

R3.1.2 Conjugate acid-base pairs

R3.1.2 Conjugate acid-base pairs

R3.1.1 Brønsted–Lowry theory of acids and bases

R3.1.1 Brønsted–Lowry theory of acids and bases

R3.1.11 Temperature dependence of Kw (HL)

R3.1.11 Temperature dependence of Kw (HL)

R1.4.3 The effect of temperature on the spontaneity of a reaction. (HL)

R1.4.3 The effect of temperature on the spontaneity of a reaction. (HL)

R1.4.1 Entropy and spontaneity (HL)

R1.4.1 Entropy and spontaneity (HL)

R1.4.1 Predicting entropy changes (HL)

R1.4.1 Predicting entropy changes (HL)

2.2 Flame tests (SL)

2.2 Flame tests (SL)

1.3 Determine the molar mass of a gas experimentally

1.3 Determine the molar mass of a gas experimentally

R1.4.1 Entropy (HL)

R1.4.1 Entropy (HL)

R1.4.4 / R2.3.7 Equilibrium and Gibbs free energy (HL)

R1.4.4 / R2.3.7 Equilibrium and Gibbs free energy (HL)

R1.4.2 Calculating ∆G° using ∆G°f values (HL)

R1.4.2 Calculating ∆G° using ∆G°f values (HL)

S2.2.16 Hybridisation (HL)

S2.2.16 Hybridisation (HL)

S1.3.6 Calculating ionisation energy (HL)

S1.3.6 Calculating ionisation energy (HL)

S3.1.3 Electron shielding and effective nuclear charge

S3.1.3 Electron shielding and effective nuclear charge

S2.2.12 Evidence for the structure of benzene (HL)

S2.2.12 Evidence for the structure of benzene (HL)

R3.4.5 Addition reactions of the alkenes

R3.4.5 Addition reactions of the alkenes

R1.4.2 Gibbs free energy (HL)

R1.4.2 Gibbs free energy (HL)

R1.2.3 / R1.2.4 Standard enthalpy change of combustion (HL)

R1.2.3 / R1.2.4 Standard enthalpy change of combustion (HL)

R1.4.1 Standard entropy change of reaction (HL)

R1.4.1 Standard entropy change of reaction (HL)

R3.2.8 Electrolytic cells

R3.2.8 Electrolytic cells

R2.3.5 Reaction quotient, Q (HL)

R2.3.5 Reaction quotient, Q (HL)

20.1 Stereochemistry of SN reactions (HL)

20.1 Stereochemistry of SN reactions (HL)

R2.3.2 / R2.3.3 Equilibrium constant, Kc

R2.3.2 / R2.3.3 Equilibrium constant, Kc

Areas of difficulty 2018 (HL)

Areas of difficulty 2018 (HL)

Areas of difficulty 2018 (SL)

Areas of difficulty 2018 (SL)

B.9 Anthocyanins (HL)

B.9 Anthocyanins (HL)

R3.2.15 Electrolysis of aqueous solutions (HL)

R3.2.15 Electrolysis of aqueous solutions (HL)

Introduction to my channel

Introduction to my channel

S2.2.12 Reactions of benzene (HL)

S2.2.12 Reactions of benzene (HL)

R3.4.2 Reactions of the halogenoalkanes

R3.4.2 Reactions of the halogenoalkanes

S2.4.5 Addition polymers

S2.4.5 Addition polymers

R1.3.1 / R1.3.2 Combustion reactions of the alcohols

R1.3.1 / R1.3.2 Combustion reactions of the alcohols

R3.2.9 Oxidation reactions of the alcohols

R3.2.9 Oxidation reactions of the alcohols

10.2 Addition reactions of the alkenes (SL)

10.2 Addition reactions of the alkenes (SL)

10.2 Test for unsaturation (SL)

10.2 Test for unsaturation (SL)

19.1 Standard electrode potential (HL)

19.1 Standard electrode potential (HL)

R3.3.1 / R3.4.3 Homolytic and heterolytic bond fission

R3.3.1 / R3.4.3 Homolytic and heterolytic bond fission