정하은T – 1:1 Q&A

S1.1.1 Elements, compounds and mixtures

S1.1.2 The kinetic molecular theory

S1.1.3 Temperature and average kinetic energy

S1.2.1 The atomic structure

S1.2.2 Isotopes & S1.2.3 Mass spectrometer (HL)

S1.3.1 Emission spectrum & S1.3.2 The hydrogen atom spectrum

S1.3.3 The main energy level & S1.3.4 Detailed model of an atom

S1.3.5 Electron configuration

S1.3.6 First ionization energy (HL) & S1.3.7 Successive ionization energy (HL)

S1.4.1 The mole & S1.4.2 Relative atomic mass and relative formula mass & S1.4.3 Molar mass

S1.4.4 Empirical and molecular formulas

S1.4.5 Molar concentration & S1.4.6 Avogadro’s law

S1.5.1 The ideal gas model & S1.5.2 Real gases

S1.5.3 Molar volume of an ideal gas & S1.5.4 Ideal gas equation and combined gas law

S2.1.1 Cation and anion & S2.1.2 Ionic bond

S2.1.3 Ionic structures and properties

S2.2.1 Covalent bond & S2.2.2 Multiple bonds & S2.2.3 Coordination bond

S2.2.4 Valence Shell Electron Pair Repulsion (VSEPR) model

S2.2.5 Bond polarity & S2.2.6 Molecular polarity

S2.2.7 Covalent network structures

S2.2.8 Types of intermolecular forces & S2.2.9 Strengths of intermolecular forces

S2.2.10 Chromatography

S2.2.11 Resonance structure (HL) & S2.2.12 Benzene (HL)

S2.2.13 Expanded octet (HL) & S2.2.14 Formal charge (HL)

S2.2.15 Sigma and pi bonds (HL) & S2.2.16 Hybridization (HL)

S2.3.1 Metallic bond & S2.3.2 Strength of a metallic bond

S2.3.3 Transition elements (HL)

S2.4.1 Bonding triangle & S2.4.2 Application of the bonding triangle

S2.4.3 Alloys

S2.4.4 Polymers & S2.4.5 Addition polymers

S2.4.6 Condensation polymers (HL)

S3.1.1 Periodic table & S3.1.2 Periodicity and electron configuration

S3.1.3 Periodicity in properites of elements

S3.1.4 Periodicity in reactivity

S3.1.5 Metal and non-metal oxides

S3.1.6 Oxidation states

S3.1.7 Discontinuities in patterns of first ionization energy (HL)

S3.1.8 Characteristic properties of transition elements (HL) & S3.1.9 Variable oxidation states (HL)

S3.1.10 Colored complexes (HL)

S3.2.1 Structural representations of organic compounds

S3.2.2 Functional groups and classes of compounds

S3.2.3 Homologous series & S3.2.4 Trends in physical properties within a homologous series

S3.2.5 IUPAC nomenclature

S3.2.6 Structural isomers

S3.2.7 Stereoisomers (HL)

S3.2.8 Mass spectrometry (HL) & S3.2.9 Infrared spectroscopy (HL)

S3.2.10, 11 Nuclear magnetic resonance spectroscopy (HL) & S3.2.12 Combining analytical techniques (HL)

R1.1.1 Chemical reactions involve heat transfers

R1.1.2 Endothermic and exothermic reactions & R1.1.3 Energetic stability and the direction of change

R1.1.4 Measuring enthalpy changes

R1.2.1 Bond enthalpy

R1.2.2 Hess’s law

R1.2.3 Standard enthalpy changes of combustion and formation (HL) & R1.2.4 Calculating enthalpy changes (HL)

R1.2.5 Born-Haber cycles (HL)

R1.3.1 Combustion reactions & R1.3.2 Incomplete combustion of organic compounds

R1.3.3 Fossil fuels

R1.3.4 Biofuels

R1.3.5 Fuel cells

R1.4.1 Entropy (HL)

R1.4.2 Gibbs energy (HL) & R1.4.3 ∆G and spontaneity (HL)

R1.4.4 ∆G and equilibrium (HL)

R2.1.1 Chemical equilibrium

R2.1.2 Using mole ratios in equations

R2.1.3 The limiting reactant and theoretical yield & R2.1.4 Percentage yield

R2.1.5 Atom economy

R2.2.1 Rate of reaction & R2.2.2 Collision theory

R2.2.3, 4, 5 Factors that influence the rate of reaction

R2.2.6, 7, 8 Reaction mechanisms (HL)

R2.2.9, 10 Rate equations (HL)

R2.2.11 The rate constant, k (HL)

R2.2.12, 13 The Arrhenius equation (HL)

R2.3.1 Dynamic equilibrium

R2.3.2, 3 Equilibrium law

R2.3.4 Le Châtelier’s principle

R2.3.5 The reaction quotient, Q (HL)

R2.3.6 Quantifying the composition of equilibrium (HL)

R2.3.7 Measuring the position of equilibrium (HL)

R3.1.1, 2 Brønsted-Lowry acids and bases & R3.1.3 Amphiprotic species

R3.1.4 The pH scale

R3.1.5 The ion product constant of water

R3.1.6 Strong and weak acids and bases

R3.1.7 Neutralization reactions

R3.1.8 pH curves

R3.1.9 The pOH scale

R3.1.10, 11 Acid and base dissociation constants (HL)

R3.1.12 pH of salt solutions (HL)

R3.1.13 pH curves revisited (HL)

R3.1.14, 15 Acid-base indicators (HL)

R3.1.16 Buffer solutions (HL)

R3.1.17 Buffer composition and pH (HL)

R3.2.1 Redox reactions

R3.2.2 Half-equations

R3.2.3 Trends in ease of oxidation and reduction of elements & R3.2.4 Oxidation of metals by acids

R3.2.5 Comparing voltaic and electrolytic cells

R3.2.6 Primary (voltaic) cells

R3.2.7 Secondary (rechargeable) cells

R3.2.8 Electrolytic cells

R3.2.9 Oxidation of functional groups in organic compounds & R3.2.10 Reduction of functional groups in organic compounds

R3.2.11 Reduction of unsaturated compounds

R3.2.12 The standard hydrogen electrode (HL)

R3.2.13 Standard electrode potentials (HL)

R3.2.14 Electrode potentials and Gibbs energy changes (HL)

R3.2.15 Electrolysis of aqueous solutions (HL)

R3.2.16 Electroplating (HL)

R3.3.1 Radicals & R3.3.2 Homolytic fission

R3.3.3 Radical substitution reactions of alkanes

R3.4.1 Nucleophiles & R3.4.2 Nucleophilic substitution reactions

R3.4.3 Heterolytic fission

R3.4.4 Electrophiles & R3.4.5 Electrophilic addition of alkenes

R3.4.6, 7 Lewis acids and Lewis bases (HL)

R3.4.8 Complex ions (HL)

R3.4.9, 10 SN1 and SN2 nucleophilic substitution mechanisms (HL)

R3.4.11 Electrophilic addition reaction mechanism (HL)

R3.4.12 Addition of hydrogen halides to asymmetrical alkenes (HL)

R3.4.13 Electrophilic substitution of benzene (HL)