IB Chemistry Higher Level

This subject is broken down into 83 topics in 15 modules:

  1. Stoichiometric relationships 3 topics
  2. Atomic structure 3 topics
  3. Periodicity 4 topics
  4. Chemical bonding and structure 7 topics
  5. Energetics/thermochemistry 5 topics
  6. Chemical kinetics 3 topics
  7. Equilibrium 2 topics
  8. Acids and bases 8 topics
  9. Redox processes 2 topics
  10. Organic chemistry 5 topics
  11. Measurement and data processing 3 topics
  12. Option A: Materials 10 topics
  13. Option B: Biochemistry 11 topics
  14. Option C: Energy 8 topics
  15. Option D: Medicinal chemistry 9 topics
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  • 15
    modules
  • 83
    topics
  • 29,175
    words of revision content
  • 3+
    hours of audio lessons

This page was last modified on 28 September 2024.

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Chemistry

Stoichiometric relationships

Introduction to the particulate nature of matter and chemical change

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Introduction to the particulate nature of matter and chemical change

Introduction to the Particulate Nature of Matter

Fundamental Concepts

  • Comprehend that all matter is composed of tiny, discrete particles known as atoms which combine to form molecules.
  • Understand that these particles are in constant motion and the speed of their motion is determined by the temperature of the system.
  • Familiarize yourself with the three states of matter: solid, liquid, and gas, and how the arrangement and motion of particles differ in each state.
  • Learn that changing between these states involves either absorption or release of energy, known as latent heat.

Chemical Change

  • Recognise that during a chemical change or reaction, the bonds between atoms in a molecule break and new bonds are formed, creating new substances.
  • Realise that atoms are neither created nor destroyed in a chemical reaction, in accordance with the law of conservation of matter.
  • Comprehend that a chemical equation represents a chemical change, with the reactants and their stoichiometric coefficients on the left and the products and their coefficients on the right.
  • Understand that the balanced chemical equation ensures the law of conservation of matter is obeyed.

Kinetic Particle Theory

  • Learn that Kinetic Particle Theory describes the behaviour of matter in terms of particles in motion. This theory helps explain properties of solids, liquids and gases, as well as changes of state.
  • Note that increased temperature corresponds to increased kinetic energy of particles, and hence greater rates of diffusion.

Practical Tips

  • Gain proficiency in writing and balancing chemical equations to get a firm grasp of the concept of stoichiometric relationships in a reaction.
  • Understand the impacts of changes in temperature, pressure, and concentration on the system by relating them to the movement and interaction of particles.
  • Familiarise yourself with common physical changes like melting, freezing, boiling, etc., and how changes in energy play a role in these processes.
  • Make sure to remember the essential concepts of atomic theory, states of matter, and the chemical change process.

Course material for Chemistry, module Stoichiometric relationships, topic Introduction to the particulate nature of matter and chemical change

Chemistry

Measurement and data processing

Uncertainties and errors in measurement and results

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Uncertainties and errors in measurement and results

Uncertainties and Errors in Measurements and Results

Understanding Uncertainties

  • Uncertainty refers to the estimate of how much a measured or calculated value may deviate from the true value.
  • Uncertainty may be due to systematic errors (errors that consistently affect results in the same way) or random errors (errors that vary in an unpredictable manner).
  • Common sources of uncertainty include limitations of measuring instruments, operator error, and changes in the experimental environment.

Expressing and Quantifying Uncertainty

  • Uncertainty is usually expressed as a range of values, e.g., 7.5 ± 0.2, where the reading is 7.5 and the uncertainty is ± 0.2.
  • Absolute uncertainty refers to the magnitude of the uncertainty, without considering the size of the measurement. It is usually expressed as ± some value.
  • Percentage uncertainty is absolute uncertainty expressed as a percentage of the measured value. It helps to compare uncertainties of different measurements.

Propagation of Uncertainty

  • Uncertainty propagation refers to how uncertainties of individual measurements combine to affect the uncertainty of the final result.
  • In addition or subtraction, absolute uncertainties add up.
  • In multiplication or division, percentage uncertainties add up.
  • In raising to a power, the percentage uncertainty multiplies by the power.

Systematic and Random Errors

  • Systematic errors consistently affect outcomes in a predictable direction. Causes include poorly calibrated equipment, biased observers, or environmental conditions.
  • Random errors vary unpredictably, balancing out in the long term. Causes include fluctuations in readings, or environmental changes.
  • Systematic errors cause a lack of accuracy, while random errors cause a lack of precision. Accuracy reflects how close measurements are to the true value, while precision reflects how close repeated measurements are to each other.

Reducing and Managing Uncertainty and Errors

  • Minimising uncertainties and errors can be achieved by repeating measurements, improving experimental techniques, or using better measuring equipment.
  • Statistical analysis can also help manage uncertainties, such as calculating the mean and standard deviation of multiple measurements.
  • It’s important to consider uncertainties and errors when interpreting results, and always express final results with the appropriate level of uncertainty.

Course material for Chemistry, module Measurement and data processing, topic Uncertainties and errors in measurement and results

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