Grade 6
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Safety rules in chemistry laboratory  1.5. Common Laboratory Equipment and Their Uses
  2. Matter and its states  2.1. Definition of Matter  2.2. Properties of matter  2.3. States of matter  2.4. Solid state  2.5. Fluid state  2.6. Gaseous state  2.7. Plasma state  2.8. Changes in the states of matter  2.9. Melting and freezing  2.10. Evaporation and Condensation  2.11. Sublimation  2.12. Deposit
  3. Physical and chemical changes  3.1. Definition of Physical Change  3.2. Examples of physical change  3.3. Definition of Chemical Change  3.4. Examples of chemical change  3.5. Difference Between Physical and Chemical Changes  3.6. Indicators of Chemical Change
  4. Elements, Compounds, and Mixtures  4.1. Definition of the element  4.2. Classification of elements  4.3. Metals  4.4. Non metallic  4.5. Metalloids  4.6. Noble gases  4.7. Definition of compound  4.8. Properties of Compounds  4.9. Definition of Mixture  4.10. Types of mixtures  4.11. Homogeneous mixture  4.12. Heterogeneous mixtures
  5. Separation of mixtures  5.1. The need for isolation  5.2. Separation methods  5.3. Handpicking and winnowing  5.4. Filtration  5.5. Sedimentation and decantation  5.6. Evaporation  5.7. Crystallization  5.8. Distillation  5.9. Magnetic Separation  5.10. Chromatography
  6. Air and its composition  6.1. Components of air  6.2. Importance of Oxygen  6.3. The importance of nitrogen in the air and its composition  6.4. Carbon dioxide in the atmosphere  6.5. The role of water vapor and other gases in air and its composition  6.6. Properties of Air  6.7. Uses of air  6.8. Air pollution and its effects
  7. Water and its properties  7.1. Importance of Water  7.2. Sources of water  7.3. Properties of water  7.4. Water as the universal solvent  7.5. Water Purification  7.6. Water purification methods (boiling, filtration, chlorination)  7.7. Water cycle  7.8. Water conservation  7.9. Water pollution and its effects
  8. Acids, Bases and Salts  8.1. Definition of Acid  8.2. Properties of Acids  8.3. Examples of Acids  8.4. Definition of Bases  8.5. Properties of bases  8.6. Examples of Bases  8.7. Definition of Salt  8.8. Neutralization reaction  8.9. pH Scale and Indicators  8.10. Uses of Acids, Bases and Salts
  9. Introduction to the Periodic Table  9.1. History of the Periodic Table  9.2. Arrangement of elements in the periodic table  9.3. Groups and periods  9.4. Importance of periodic table  9.5. First 10 elements and their symbols
  10. Metals and Nonmetals  10.1. Properties of Metals  10.2. Properties of Non-Metals  10.3. Difference Between Metals and Nonmetals  10.4. Uses of metals and nonmetals  10.5. Corrosion of metals and its prevention
  11. chemical reactions  11.1. Introduction to Chemical Reactions  11.2. Types of Chemical Reactions  11.3. combustion reaction  11.4. Oxidation and Reduction  11.5. Simple chemical equations  11.6. Rusting of iron
  12. Fuel and energy  12.1. Types of fuel  12.2. Fossil fuels  12.3. Renewable and non-renewable sources of energy  12.4. Energy Conservation  12.5. Alternative sources of energy (solar, wind, hydropower)
  13. Plastic and fiber  13.1. Natural and synthetic fibers  13.2. Properties of plastics  13.3. Advantages and disadvantages of plastic  13.4. Recycling of plastic  13.5. Biodegradable and non-biodegradable materials

Grade 6 → Matter and its states ↓


States of matter


Matter is anything that occupies space and has mass. Everything around us is made of matter, from the air we breathe to the food we eat. Matter exists in different forms, often called "states." In this longer lesson, we'll explore the different states of matter and what makes each state unique.

What is the matter?

Matter is made up of tiny particles called atoms and molecules. These particles are so small that we cannot see them without a powerful microscope. Matter can combine and rearrange in countless ways, forming everything in the universe.

General properties of matter

Here are some basic properties that apply to all substances:

  • Volume: The space occupied by an object.
  • Mass: The amount of matter in an object.
  • Density: This is a measure of how much mass is contained in a given volume.

Three main states of matter

Matter is usually found in three states: solid, liquid, and gas. Each state has different properties and can change from one state to another under certain conditions. Let's look at each state more closely.

Solids

The characteristic of solids is that they have a definite shape and volume. The atoms or molecules in a solid are adjacent to each other in a definite arrangement, due to which solids become rigid and maintain their shape.

Example of solids: A wooden table, a steel beam and a piece of ice each represent the solid state of matter. Despite differences in structure and appearance, they all retain their shape without requiring any container.
Block A Block B Block C

Liquids

Liquids have a definite volume, but they do not have a definite shape. This means that the liquid will take the shape of its container. The atoms or molecules in liquids are more loosely packed than those in solids, allowing them to move more freely even while still being in contact with each other.

Examples of fluids: Water in a glass, juice in a bottle, and milk in a carton are all examples of fluids. When you pour water from one container into another, it will flow and change shape to conform to the container.

Gases

Gases have neither a definite shape nor a volume. They expand to fill the entire space of their container. The atoms or molecules in a gas are much more spread out than those in solids and liquids, allowing them to move freely and rapidly.

Example of gases: Earth's atmosphere, helium in a balloon, and steam from boiling water represent gases. When you open a soda bottle, carbon dioxide gas forms bubbles and escapes quickly.

Changing states of matter

Matter can change from one state to another when energy, usually in the form of heat, is added or removed. Here are some of the processes through which states of matter change:

Melting

Melting is the process of changing from a solid to a liquid. When we heat a solid, its atoms or molecules gain energy and pass past each other more freely, turning it into a liquid.

Example of melting: Ice melting into water is a classic example. If you take a piece of ice out of the freezer and leave it at room temperature, it slowly melts into liquid water. 
        H 2 O (solid) + heat → H 2 O (liquid)

Solidify

Freezing is the change from a liquid to a solid. It occurs when we remove heat from a liquid, causing its particles to lose energy and bond more tightly, forming a solid.

Freezing example: Water turning into ice is a simple example. Place a tray of water in the freezer, and as it cools, it will freeze and form ice cubes. 
        H 2 O (liquid) → H 2 O (solid) + heat loss

Evaporation

Evaporation is the conversion of a liquid into a gas, which occurs at the surface of the liquid. It occurs when particles in the liquid gain enough energy that they break free from the liquid and become gas particles.

Example of evaporation: It is a common sight on a hot day for water to evaporate into water vapor. Puddles also become smaller as the water evaporates into the air. 
        H 2 O (liquid) + heat → H 2 O (gas)

Condensation

Condensation is the change from a gas to a liquid. It occurs when gas particles lose energy and come closer to each other to form a liquid.

Example of condensation: Dew forming on grass in the early morning, or water droplets forming on the outside of a cold glass are examples of condensation. 
        H 2 O (gas) → H 2 O (liquid) + heat loss

Sublimation and deposition

Sublimation is the process in which a solid substance changes directly into a gas, bypassing the liquid state. Deposition is the opposite process in which a gas changes directly into a solid.

Example of sublimation and deposition: Dry ice (solid carbon dioxide) sublimes into a gas without becoming a liquid. Frost forms on cold surfaces through deposition as water vapor turns directly into ice. 
        CO 2 (solid) → CO 2 (gas) (sublimation)
        H 2 O (gas) → H 2 O (solid) (deposition)

Unusual states of matter

In addition to the three main states, there are also some less common states that matter can take under special circumstances. These include plasma and Bose-Einstein condensates.

Plasma

Plasma is often called the fourth state of matter. Plasma is gases heated to very high temperatures, causing the atoms to lose their electrons. Plasmas are found in stars, including our Sun.

Examples of plasma: Neon signs and lightning are familiar examples of plasma on Earth. 
        Gas + intense heat → Plasma + free electrons

Bose–Einstein condensates

A Bose-Einstein condensate (BEC) is a state of matter that occurs at temperatures close to absolute zero. At such low temperatures, a group of atoms cool down and behave as if they were a single particle.

Example of Bose-Einstein condensates: This state of matter is complex and not found in everyday life, it is usually studied in advanced scientific laboratories.

Understanding matter and everyday life

States of matter are part of our everyday experiences. Knowing how and why states of matter change can help us understand natural processes and even design technologies that make our lives easier.

Everyday uses: Refrigerators use the condensation and evaporation of liquid to keep food cold. The natural water cycle relies on evaporation and condensation to form clouds and produce precipitation.

Conclusion

Matter is all around us, and understanding its various states enhances our understanding of science and the world. Solids, liquids, gases, and even plasma and Bose-Einstein condensates each have unique properties and behaviors. By learning about the states of matter, we are able to better understand the complex fabric of science we encounter in our daily lives.


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States of matter

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