📦 haribo's box

          • 1.1.1 elements, compounds and mixtures
          • 1.1.2 the kinetic molecular theory
          • 1.1.3 kinetic energy and temperature
          • 1.2.1 the atomic model
          • 1.2.2 isotopes
          • 1.2.3 mass spectra (HL)
          • 1.3.1 and 1.3.2 emission spectra
          • 1.3.3, 1.3.4, and 1.3.5 electron configuration
          • 1.3.6 and 1.3.7 ionisation energies (HL)
          • 1.4.1 the mole as the unit of amount
          • 1.4.2 relative atomic mass and relative formula mass
          • 1.4.3 molar mass
          • 1.4.4 empirical and molecular formulas
          • 1.4.5 molar concentration
          • 1.4.6 Avogadro's law
          • 1.5.1 the ideal gas model
          • 1.5.2 real gases
          • 1.5.3 and 1.5.4 the ideal gas laws
          • 2.1.1 and 2.1.2 the ionic bond
          • 2.1.3 ionic structures and properties
          • 2.2.1 covalent bonding, octet rule and Lewis formulas
          • 2.2.2 single, double and triple covalent bonds
          • 2.2.3 coordination bonds
          • 2.2.4 the valence shell electron pair repulsion (VSEPR) model
          • 2.2.5 bond polarity
          • 2.2.6 molecular polarity
          • 2.2.7 covalent network structures
          • 2.2.8 and 2.2.9 intermolecular forces
          • 2.2.10 intermolecular forces and chromatography
          • 2.2.11 resonance structures (HL)
          • 2.2.12 benzene (HL)
          • 2.2.13 molecules with an expanded octet (HL)
          • 2.2.14 formal charge (HL)
          • 2.2.15 sigma and pi bonds (HL)
          • 2.2.16 hybridisation (HL)
          • 2.3.1 and 2.3.2 metallic bond
          • 2.3.3 transition elements (HL)
          • 2.4.1 the bonding triangle
          • 2.4.2 application of the bonding triangle
          • 2.4.3 alloys
          • 2.4.4 polymers
          • 2.4.5 addition polymers
          • 2.4.6 condensation polymers (HL)
          • 3.1.1 periods, groups and blocks
          • 3.1.2 periodicity and electron configuration
          • 3.1.3 periodicity in properties of elements
          • 3.1.4 periodicity in reactivity
          • 3.1.5 metal and non-metal oxides
          • 3.1.6 oxidation states
          • 3.1.7 discontinuities in patterns of first ionisation energy (HL)
          • 3.1.8 characteristic properties of transition elements (HL)
          • 3.1.9 variable oxidation states (HL)
          • 3.1.10 coloured complexes (HL)
          • 3.2.1 structural representations of organic molecules
          • 3.2.2 functional groups and classes of compounds
          • 3.2.3 and 3.2.4 homologous series
          • 3.2.5 IUPAC nomenclature
          • 3.2.6 structural isomers
          • 3.2.7 stereoisomers (HL)
          • 3.2.8 mass spectrometry (HL)
          • 3.2.9 infrared spectroscopy (HL)
          • 3.2.10 and 3.2.11 nuclear magnetic resonance (NMR) spectroscopy (HL)
          • 3.2.12 combining analytical techniques
          • 1.1.1 chemical reactions involve heat transfers
          • 1.1.2 endothermic and exothermic reactions
          • 1.1.3 energetic stability and the direction of change
          • 1.1.4 measuring enthalpy changes
          • 1.2.1 bond enthalpy
          • 1.2.2 Hess's law
          • 1.2.3 standard enthalpy changes of combustion and formation (HL)
          • 1.2.4 calculating enthalpy changes (HL)
          • 1.2.5 Born-Haber cycles (HL)
          • 1.3.1 combustion reactions
          • 1.3.2 incomplete combustion of organic compounds
          • 1.3.3 fossil fuels
          • 1.3.4 biofuels
          • 1.3.5 fuel cells
          • 1.4.1 entropy (HL)
          • 1.4.2 Gibbs energy (HL)
          • 1.4.3 ∆G and spontaneity (HL)
          • 1.4.4 ∆G and equilibrium (HL)
          • 2.1.1 chemical equations
          • 2.1.2 using mole ratios in equations
          • 2.1.3 limiting reactant and theoretical yield
          • 2.1.4 percentage yield
          • 2.1.5 atom economy
          • 2.2.1 rate of reaction
          • 2.2.2 collision theory
          • 2.2.3, 2.24 and 2.25 factors that influence the rate of reaction
          • 2.2.6, 2.2.7 and 2.2.8 reaction mechanisms
          • 2.2.9 and 2.2.10 rate equations
          • 2.2.11 the rate constant, k
          • 2.2.12 and 2.2.13 the Arrhenius equation
          • 2.3.1 dynamic equilibrium
          • 2.3.2 and 2.3.3 equilibrium law
          • 2.3.4 Le Chatelier's principle
          • 2.3.5 the reaction quotient, Q
          • 2.3.6 quantifying the composition of equilibrium
          • 2.3.7 measuring position of equilibrium
          • 3.1.1 and 3.1.2 Bronsted-Lowry acids and bases
          • 3.1.3 amphiprotic species
          • 3.1.4 the pH scale
          • 3.1.5 the ionic product constant of water
          • 3.1.6 strong and weak acids and bases
          • 3.1.7 neutralisation reactions
          • 3.1.8 pH curves
          • 3.1.9 the pOH scale (HL)
          • 3.1.10 and 3.1.11 acid and base dissociation constants (HL)
          • 3.1.12 pH of salt solutions (HL)
          • 3.1.13 pH curves revisited (HL)
          • 3.1.14 and 3.1.15 acid-base indicators (HL)
          • 3.1.16 buffer solutions (HL)
          • 3.1.17 buffer composition (HL) and pH
          • *3.2.10 reduction of functional groups in organic compounds
          • *3.2.11 reduction of unsaturated compounds
          • 3.2.1 redox reactions
          • 3.2.2 half-equations
          • 3.2.3 trends in ease of oxidation and reduction of elements
          • 3.2.4 oxidation of metals by acids
          • 3.2.5 comparing voltaic and electrochemical cells
          • 3.2.6 primary (voltaic) cells
          • 3.2.7 secondary (rechargeable) cells
          • 3.2.8 electrolytic cells
          • 3.2.9 oxidation of functional groups in organic compounds
          • 3.2.12 the standard hydrogen electrode (HL)
          • 3.2.13 standard electrode potentials
          • 3.2.14 electrode potentials and Gibbs energy changes (HL)
          • 3.2.15 electrolysis of aqueous solutions (HL)
          • 3.2.16 electroplating (HL)
          • 3.3.1 radicals
          • 3.3.2 homolytic fission
          • 3.3.3 radical substitution reactions of alkanes
          • 3.4.1 nucleophiles
          • 3.4.2 nucleophilic substitution reactions
          • 3.4.3 heterolytic fission
          • 3.4.4 electrophiles
          • 3.4.5 electrophilic addition of alkenes
          • 3.4.6 lewis acids and lewis bases (HL)
          • 3.4.8 complex ions (HL)
          • 3.4.9 and 3.4.10 sn1 and sn2 nucleophilic substitution mechanisms (HL)
          • 3.4.11 electrophilic substitution mechanism (HL)
          • 3.4.12 addition of hydrogen halides to asymmetrical alkenes (HL)
          • 3.4.13 electrophilic substitution of benzene (HL)
          • conventions
      • Equations and physical constants
      • eyes go wow
      • Green Chemistry
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    ❯

    1 Structure

    ❯

    3 classification of matter

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    3.2 functional groups classification of organic compounds

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    3.2.12 combining analytical techniques

    3.2.12 combining analytical techniques

    27 Feb 20251 min read

    chem classificationsofmatter

    Structure 3.2.12 - data from different techniques are often combined in structural analysis

    see 3.2.8 mass spectrometry (HL)
    see 3.2.10 and 3.2.11 nuclear magnetic resonance (NMR) spectroscopy (HL)
    see 3.2.9 infrared spectroscopy (HL)

    practice!


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