S1.2.3 Mass Spectrometry and Isotopes (AHL) | IB Chemistry

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S1.1 - Introduction to the particulate nature of matter S1.2 - The nuclear atom S1.3 - Electron configurations S1.4 - Counting particles by mass - The mole S1.5 - Ideal gases S2.1 - The ionic model S2.2 - The covalent model S2.3 - The metallic model S2.4 - From models to materials S3.1 - The periodic table - Classification of elements S3.2 - Functional groups - Classification of organic compounds R1.1 - Measuring enthalpy changes R1.2 - Energy cycles in reactions R1.3 - Energy from fuels R1.4 - Entropy and spontaneity AHL R2.1 - How much? The amount of chemical change R2.2 - How fast? The rate of chemical change R2.3 - How far? The extent of chemical change R3.1 - Proton transfer reactions R3.2 - Electron transfer reactions R3.3 - Electron sharing reactions R3.4 - Electron-pair sharing reactions

Course Menu

S1.1 - Introduction to the particulate nature of matter ▼

1.1.1 Elements, Compounds and Mixtures 1.1.2 Kinetics Intermolecular Theory and States of Matter 1.1.3 Temperature, Kinetics Energy, and Change of State

S1.2 - The nuclear atom ▼

1.2.1 Nuclear Atom and Sub-Atomic Particles 1.2.2 Isotopes and Atomic Mass 1.2.3 Mass Spectrometry and Isotopes (AHL)

S1.3 - Electron configurations ▼

1.3.1 Emission Spectra 1.3.2 Hydrogen Emission Spectrum and Energy Levels 1.3.3 Main Energy Levels 1.3.4 Sublevels and Atomic Orbital 1.3.5 Electron Configuration 1.3.6 Ionization Energy and Spectral Interpretation (AHL) 1.3.7 Successive Ionization Energies and Electron Configuration (AHL)

S1.4 - Counting particles by mass - The mole ▼

1.4.1 The Mole and Avagadro's Constant 1.4.2 Relative Atomic Mass (Ar) and Relative Formula Mass (Mr) 1.4.3 Molar Mass, Mass and The Mole 1.4.4 Empirical and Intermolecular Formulae 1.4.5 Molar Concentration and Solution Calculations 1.4.6 Avagadro's Law and Gas Volumes

S1.5 - Ideal gases ▼

1.5.1 Ideal Gas Model 1.5.2 Limitations of the Ideal Gas Model 1.5.3 Gas Laws and Molar Volumes of Ideal Gases 1.5.4 Ideal Gas Equation, pV=nRT

S2.1 - The ionic model ▼

2.1.1 Formation of Ions 2.1.2 Ionic Bonding and Compounds 2.1.3 Structure and Properties of Ionic Compounds

S2.2 - The covalent model ▼

2.2.1 Covalent Bonds and Lewis Formulas 2.2.2 Bond Types 2.2.3 Co-coordination (Dative) Bonds 2.2.4 VSEPR Molecular Shapes 2.2.5 Electronegativity and Bond Polarity 2.2.6 Molecular Polarity and Dipole Moments 2.2.7 Covalent Network Structures and Allotropes 2.2.8 Intermolecular Forces 2.2.9 Physical Properties of Covalent Substances 2.2.10 Chromatography and Intermolecular Forces 2.2.11 Resonance Structures (AHL) 2.2.12 Benzene and Resonance (AHL) 2.2.13 Expanded Octet and VSEPR (AHL) 2.2.14 Formal Charge (AHL) 2.2.15 Sigma and Pi Bonds (AHL) 2.2.16 Hybridization (AHL)

S2.3 - The metallic model ▼

2.3.1 Metallic Bonding and Properties of Metal 2.3.2 Strength of Metallic Bonding 2.3.3 Transition Metal (AHL)

S2.4 - From models to materials ▼

2.4.1 The Bonding Continuum 2.4.2 Using the Bonding Triangle 2.4.3 Alloys 2.4.4 Polymer and Plastic Properties 2.4.5 Addition Polymerization 2.4.6 Condensation Polymerization (AHL)

S3.1 - The periodic table - Classification of elements ▼

3.1.1 Periodic Table Structure 3.1.2 Periodic, Group and Electron Configuration 3.1.3 Periodicity of Elements 3.1.4 Group Trends 3.1.5 Metallic to Non-Metallic Oxide Behaviour 3.1.6 Oxidation States 3.1.7 Ionization Energy Trends Exceptions (AHL) 3.1.8 Transition Element Properties (AHL) 3.1.9 Transition Element Oxidation States (AHL) 3.1.10 Colour and Tran