GCSE Physics A (Combined) OCR
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56 topics in 6 modules
☑️ Matter 7 topics
- The History of the Atom and Atomic Structure
- Density
- Particle Theory
- States of Matter
- Specific Heat Capacity
- Specific Latent Heat
- Pressure of Gases
☑️ Forces 17 topics
- Speed and Velocity
- Acceleration
- Motion
- Distance-Time Graphs
- Velocity-Time Graphs
- Forces and Free Body Force Diagrams
- Scale Diagrams and Forces
- Newton's First and Second Laws of Motion
- Friction and Terminal Velocity
- Inertia and Newton's Third Law of Motion
- Momentum
- Conservation of Momentum
- Mass, Weight and Gravity
- Mechanical Energy Stores
- Work Done and Power
- Forces and Elasticity
- Hooke's Law
☑️ Electricity and Magnetism 11 topics
- Static Electricity
- Current and Potential Difference
- Circuits
- Resistance
- Circuit Devices
- Series and Parallel Circuits
- Energy and Power in Circuits
- Magnets and Magnetic Fields
- Electromagnetism
- Magnetic Forces
- Motors
☑️ Waves and Radioactivity 9 topics
- Wave Basics
- Reflection
- Refraction
- Electromagnetic Waves
- Isotopes and Radioactive Decay
- Radiation Properties and Decay Equations
- Electron Energy Levels
- Half-Life
- Dangers of Radioactivity
☑️ Energy 6 topics
- Conservation of Energy
- Efficiency
- Energy Transfer by Heating
- Reducing Unwanted Energy Transfers
- Mechanical Energy Transfers
- Electrical Energy Transfers
☑️ Global Challenges 6 topics
- Everyday Speeds and Accelerations
- Stopping Distances and Reaction Times
- Non-Renewable Energy Sources
- Renewable Energy Sources
- Electricity and the National Grid
- Home Wiring
GCSE Physics A (Combined) OCR Revision Content
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GCSE Physics A (Combined) OCR - Matter - The History of the Atom and Atomic Structure Content Preview
Matter
The History of the Atom and Atomic Structure
The History of the Atom
- Democritus proposed the first atomic theory in 400BC, suggesting that matter is composed of small, indestructible particles.
- English chemist John Dalton further developed the atomic theory in the 1800s, claiming all matter is made up of atoms, which are indestructible and can't be divided.
- Towards the end of the 19th century, J.J. Thomson discovered the electron using cathode rays, leading to the 'plum-pudding' model.
- In 1911, Ernest Rutherford conducted his gold foil experiment, discovering the nucleus of the atom, which led to the 'planetary' model of the atom.
- Later, Niels Bohr revised Rutherford’s model to include distinct electron shells, a theory which partially stands today.
Atomic Structure
- Atoms are comprised of protons, neutrons, and electrons.
- The nucleus at the centre of the atom contains both protons and neutrons. It is positively charged due to the protons.
- Electrons are negatively charged particles that orbit the nucleus within energy levels or electron shells.
- Atoms are electrically neutral, meaning the number of protons (positive) equals the number of electrons (negative).
- The number of protons an atom possesses defines the atomic number and the type of element it is.
- The mass number (or atomic mass) of an atom is the sum of protons and neutrons.
Atomic Models
- Plum-pudding model: J.J. Thomson suggested the atom was a positively charged sphere with negative electrons embedded within it.
- Planetary model: Following his discovery of the nucleus, Rutherford compared atoms to a mini solar system, with electrons orbiting the nucleus.
- Bohr model: Bohr improved upon Rutherford’s model by organising the electrons into fixed orbits or 'shells'.
Isotopes
- Isotopes are atoms of the same element (having the same number of protons) but with different numbers of neutrons, leading to different mass numbers.
- Isotopes of the same element share chemical properties but may have different physical properties.
- Some isotopes are unstable, or radioactive, and can emit radiation through alpha, beta, and gamma decay.
Question: Explain the key differences between the plum-pudding model, the planetary model, and the Bohr model of the atom.
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