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.