Structure 1

Title

Chemistry for the IB Diploma Programme

Authors and Publication

  • Catrin Brown, Mike Ford, Oliver Canning, Andreas Economou, Garth Irwin

  • Published by Pearson Education Limited, 2023

Contents Overview (Page 4)

  • Syllabus roadmap

  • Authors' introduction to the third edition

  • Skills in the study of chemistry

  • Structure chapters covering:

    • Structure of matter

    • Models of bonding and structure

    • Classification of matter

    • Reactivity concepts

Syllabus Roadmap (Page 8)

  • Focus on integration of concepts and inquiry

  • Students encouraged to personalize their approach

Authors' Introduction (Page 9)

  • New edition aligns with IB curriculum for assessments from 2025.

  • Structured around themes of Structure and Reactivity.

Chapter Summaries

Structure 1.1 - Particulate Nature of Matter (Pages 20-23)

  • Introduction: Matter consists of atoms, the building blocks of all substances.

  • Elements, Compounds, and Mixtures:

    • Elements: Pure substances that cannot be broken down.

    • Compounds: Consist of atoms from different elements.

    • Mixtures: Combinations of elements or compounds not chemically bonded.

Structure 1.2 - The Nuclear Atom (Pages 43-50)

  • Atomic Structure:

    • Atoms consist of protons, neutrons (nucleus) and electrons.

    • Atomic number (Z) = number of protons.

  • Mass Number (A) = number of protons + neutrons.

  • Isotopes: Atoms of the same element with different numbers of neutrons.

Structure 1.3 - Electron Configurations (Pages 66-88)

  • Electron Configuration: Determines an atom's chemical behavior, derived from energy levels.

  • Energy Levels:

    • Each main level can hold a maximum of (2n^2) electrons.

    • Sublevels: s, p, d, and f.

    • Aufbau principle: Electrons fill orbitals of lowest energy first.

    • Hund's rule: Electrons fill degenerate orbitals singly before pairing.

Counting Particles by Mass: The Mole (Pages 105-116)

  • Mole Concept: Unit of amount; one mole contains (6.022 imes 10^{23}) entities.

  • Calculating Molar Mass: Relates mass of a substance to the amount of substance in moles.

  • Empirical vs. Molecular Formulas: Empirical formulas give the simplest ratio of elements, while molecular formulas denote the actual number of atoms.

Ideal Gases (Pages 136-157)

  • Gas Laws: Relationships between pressure, volume, and temperature of gases.

  • Ideal Gas Model: Assumes particles have negligible volume and no intermolecular forces.

  • Real Gases: Deviate from the ideal at low temperatures and high pressures due to particle volume and intermolecular attractions.

Advanced Concepts (Pages 158-173)

  • Ionization Energies: Patterns in ionization energies provide insights into electron configurations and chemical properties.

Important Formulas

  • Ideal Gas Equation: (PV = nRT)

  • Converting Moles to Mass: (mass = n \times M)

  • Molar Concentration: (c = \frac{n}{V})

  • Empirical Formula Calculation: Convert mass percent to mole ratios, derive formula.

Experimental Techniques • Laboratory Practices (Pages 109-113)

  • Titration: Used to determine solution concentrations.

  • Serial Dilutions: Generates a series of solutions of known concentration.

  • Combustion analysis: Determines compositions from combustion products.