Grade 10
  1. Mechanics  1.1. Dynamics  1.1.1. Motion in one dimension  1.1.2. Motion in two dimensions  1.1.3. Displacement and Distance  1.1.4. Speed and Velocity  1.1.5. Acceleration  1.1.6. Graphical representation of motion  1.1.7. Equations of motion  1.1.8. Free fall and acceleration due to gravity  1.1.9. Projectile motion  1.1.10. Relative speed  1.2. Dynamics  1.2.1. Newton's Laws of Motion  1.2.2. Inertia and mass  1.2.3. Force and its types  1.2.4. action and reaction force  1.2.5. Friction and its effects  1.2.6. Coefficient of friction  1.2.7. Circular motion  1.2.8. Centripetal force and centripetal acceleration  1.2.9. Momentum and Impulse  1.2.10. Conservation of momentum  1.2.11. Newton's third law and applications  1.3. Work, Energy and Power  1.3.1. Work done by the force  1.3.2. Work–energy theorem  1.3.3. Kinetic energy  1.3.4. Potential energy  1.3.5. Mechanical energy  1.3.6. Energy Conservation  1.3.7. Power and efficiency  1.3.8. Renewable and non-renewable energy sources  1.4. Gravitational force  1.4.1. Newton's law of universal gravitation  1.4.2. Gravitational field and field strength  1.4.3. Acceleration due to gravity on different planets  1.4.4. Kepler's laws of planetary motion  1.4.5. Orbits and satellites  1.4.6. Weight and apparent weight  1.4.7. Gravitational potential energy
  2. Properties of matter  2.1. States of matter  2.1.1. Solid, liquid and gas  2.1.2. Molecular structure of matter  2.1.3. Intermolecular forces  2.1.4. Plasma and Bose–Einstein condensate  2.2. Pressure  2.2.1. Definition of Pressure  2.2.2. Pressure in liquids  2.2.3. Atmospheric pressure  2.2.4. Pascal's principle  2.2.5. Archimedes' Principle and Buoyancy  2.2.6. Surface tension and capillarity  2.3. Elasticity  2.3.1. Hooke's law  2.3.2. Stress and strain  2.3.3. Elastic Limit and Modulus of Elasticity  2.3.4. Applications of Elasticity
  3. Thermal physics  3.1. heat and temperature  3.1.1. Difference Between Heat and Temperature  3.1.2. Temperature scale  3.1.3. Thermal expansion  3.1.4. Thermal equilibrium  3.2. Heat transfer  3.2.1. Conductivity  3.2.2. Convection  3.2.3. Radiation  3.2.4. Insulation and its applications  3.3. Thermal properties of matter  3.3.1. Specific heat capacity  3.3.2. Latent heat and phase change  3.3.3. Boiling and Melting Point  3.3.4. Heat engines and refrigeration  3.4. Laws of Thermodynamics  3.4.1. Zeroth law of thermodynamics  3.4.2. First law of thermodynamics  3.4.3. Second law of thermodynamics  3.4.4. Carnot cycle
  4. Waves and optics  4.1. Nature and properties of waves  4.1.1. Types of waves in nature and properties of waves  4.1.2. Transverse and longitudinal waves  4.1.3. Wave parameters  4.1.4. Reflection and refraction of waves  4.1.5. Superposition and Interference  4.1.6. Standing Waves and Resonance  4.1.7. Doppler effect  4.2. Sound waves  4.2.1. Characteristics of sound waves  4.2.2. Speed of sound in different mediums  4.2.3. Applications of sound waves  4.2.4. Ultrasound and its uses  4.3. Light Waves and Optics  4.3.1. Nature of light  4.3.2. Reflection of light  4.3.3. Laws of reflection  4.3.4. Mirrors and Image Formation  4.3.5. Refraction of light  4.3.6. Snell's Law  4.3.7. Lenses and Image Formation  4.3.8. Total internal reflection and critical angle  4.3.9. Optical fibre  4.4. Optical Instruments  4.4.1. Microscope  4.4.2. Telescope  4.4.3. Human eye and vision defects  4.4.4. Camera and its working principle
  5. Electricity and Magnetism  5.1. Electrostatics  5.1.1. Electric charge and its properties  5.1.2. Conductors and Insulators  5.1.3. Coulomb's law  5.1.4. Electric field and field lines  5.1.5. Electric potential and potential difference  5.1.6. Capacitors and Capacitance  5.2. Current Electricity  5.2.1. Electric current and its measurement  5.2.2. Ohm's law  5.2.3. Resistance and resistivity  5.2.4. Series and Parallel Circuits  5.2.5. Electric power and energy  5.2.6. Kirchhoff's Laws  5.3. Magnetism and Electromagnetism  5.3.1. Magnetic field and field lines  5.3.2. Magnetic effects of electric current  5.3.3. Electromagnetic induction  5.3.4. Faraday's laws of electromagnetic induction  5.3.5. Transformers and Applications  5.3.6. AC and DC current
  6. Modern Physics  6.1. Nuclear physics  6.1.1. Structure of the atom  6.1.2. Bohr's atomic model  6.1.3. Electron Energy Levels  6.1.4. X-rays and applications  6.2. Radioactivity  6.2.1. Types of radiation  6.2.2. Half-life and radioactive decay  6.2.3. Nuclear reactions and applications  6.2.4. Fission and Fusion  6.3. Quantum physics  6.3.1. Wave–particle duality  6.3.2. Photoelectric effect  6.3.3. Energy quantization  6.3.4. Heisenberg's uncertainty principle
  7. Electronics and Communication  7.1. Semiconductors  7.1.1. Conductors, Insulators and Semiconductors  7.1.2. Diodes and their applications  7.1.3. Transistors and Logic Gates  7.1.4. LEDs and photodiodes  7.2. Communication Systems  7.2.1. Basics of communication  7.2.2. Analog and digital signals  7.2.3. Wireless and optical fibre communication  7.2.4. Radio Waves and Modulation

Grade 10 → Properties of matter → States of matter ↓


Solid, liquid and gas


Matter exists everywhere around us. The phone or computer you use, the water you drink and the air you breathe are all examples of matter. In physics, matter is everything that has mass and occupies space. Matter exists in different states, and the three most common states are solid, liquid and gas. Understanding these states and their properties is fundamental in physics and helps us understand how different substances behave under different conditions.

Solids

Solids are one of the fundamental states of matter. Atoms in solids are tightly packed together in a definite arrangement. This close packing of atoms gives solids the unique property of having a definite shape and volume.

Imagine a wooden chair. No matter where you place it in the room, its shape remains the same and it occupies the same amount of space. This stability and rigidity is a characteristic of solids.

In terms of particle arrangement, the particles in a solid are closely packed in a regular pattern. This highly ordered structure is the reason why solids do not flow like liquids or gases and have fixed shapes.

Examples of solids

  • Ice cubes: Ice cubes keep their shape no matter what container they're in.
  • Table salt: Each grain of salt retains its shape even when poured onto a table.
  • Bricks: Bricks have a fixed structure and do not change their shape.

Liquids

Liquid is another state of matter that has a definite volume but an indefinite shape. This means that while a liquid occupies a definite space, its shape changes depending on the container it is in.

Imagine a glass full of water. Water can fill glasses of different sizes, but the volume of water always remains the same. This is because the molecules in liquids are not as tightly packed as those in solids, but are still close enough together to maintain volume.

Particles in liquids are close to each other but not in a fixed position. They can move and slide over each other, allowing liquids to flow and take the shape of their container.

Examples of liquids

  • Water: Water takes the shape of any bottle or glass, but the volume of water remains unchanged.
  • Oil: When oil is poured, it goes into any shape of the vessel, but its volume remains the same.
  • Milk: When milk is poured from a can into a bowl, its shape changes but the volume does not change.

Gases

Gases are a state of matter that has neither a definite shape nor a definite volume. The particles in gases are spread out and move around freely, allowing gases to completely fill any container, regardless of its size and shape.

Imagine a balloon being inflated. The air inside the balloon expands to fill the entire space inside. Unlike solids and liquids, gases will continue to expand indefinitely to occupy any given space due to the high energy and dispersed nature of their particles.

The particles in gases have a lot of space between them and are constantly moving at high speeds in all directions. This freedom of movement of the particles is the reason why gases can easily compress or expand.

Examples of gases

  • Air: The air we breathe can fill any room, no matter its size.
  • Helium: When used to fill balloons, helium conforms completely to the shape of the balloon.
  • Steam: Steam from boiling water fills the air space around it.

Understanding changes between states

Matter can change from one state to another through physical processes. These changes often involve the transfer of energy, such as heating or cooling. Understanding these changes is essential to understanding how matter interacts in different environments.

Melting and freezing

When a solid substance gains enough energy, its particles begin to move around faster and break free from their fixed positions. This process is called melting, and it turns solids into liquids. An everyday example is ice melting into water at 0°C (32°F).

Conversely, when a fluid loses energy, its particles slow down and settle into a fixed structure, forming a solid. This is called freezing. Water freezing into ice is an example of this.

Evaporation and condensation

Liquids can become gases through a process called evaporation, which occurs when liquid molecules gain enough energy to break free and become a gas. This can be observed when water slowly evaporates from a wet surface.

Condensation is the opposite process, in which gas molecules lose energy and change to a liquid state. This can be observed when steam comes in contact with a cold surface, forming water droplets.

Sublimation and deposition

Some substances can change directly into a solid and a gas without becoming a liquid. Sublimation is when a solid changes directly into a gas, such as dry ice changing into carbon dioxide gas. Deposition is the opposite, where a gas changes directly into a solid, such as water vapor forming frost.

Exploration of the particle model

The particle model makes it easier to understand the states of matter. This model helps to see how particles interact and move through different states.

        
            
            Solids: 
            Liquids: 
            Gases: 
            [•][•][•] [•] [•] [•] [•] [•] 
            [•][•][•] [•] [•] [•] [•] [•] 
            [•][•][•] [•] [•] [•] [•] [•]
  • Solid particles are tightly packed in a regular, stable structure.
  • The liquid particles are close to each other, but they do not have a fixed arrangement so that they can flow.
  • The gas particles are far apart and move around freely, completely filling their container.

Use of knowledge of states

Recognizing the states of matter and how they change is important in a variety of fields, including construction, food production, and scientific research. For example, understanding how water expands when it freezes helps engineers design frost-resistant structures.

Practical applications

  • In the kitchen: Cooking often involves a change of state. Boiling water changes from a liquid to a gas, and melting chocolate changes from a solid to a liquid.
  • In nature: The formation of ice from water vapor involves deposition, and the water cycle is driven by phase changes between evaporation and condensation.
  • In industry: Metal forging and glass manufacturing rely on controlling the phase changes of the material to create the desired shape.

Conclusion

Understanding solids, liquids, and gases, as well as how matter changes between these states, is the basis for many theories of physics and everyday life. The particle model provides a framework for visualizing these differences and predicting how matter behaves under different conditions.

By examining examples and applications of state changes, we get a deeper understanding of how important these concepts are in various fields and daily activities.


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Solid, liquid and gas

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