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 → Elements, Compounds, and Mixtures ↓


Properties of Compounds


Compounds are a core part of chemistry. Unlike elements, which are pure substances made of only one type of atom, compounds form when two or more elements combine chemically. Understanding the properties of compounds helps us understand how substances interact in the world around us.

What is a compound?

A compound is a substance that is formed when two or more elements are chemically joined together. This means that the atoms of these elements are linked by chemical bonds, forming a new substance that has its own unique properties.

For example, water (H2O) is a compound made of hydrogen and oxygen. Although hydrogen and oxygen are gases at room temperature, water is a liquid. This new property of being a liquid comes from the combination of hydrogen and oxygen.

H2 + O → H2O

Characteristics of compounds

  • Fixed structure: The proportion of each element in a compound is fixed. For example, water is always made up of two hydrogen atoms and one oxygen atom.
  • Distinctive properties: The properties of a compound are different from those of the elements that make it up.
  • Chemical changes: Compounds can be separated into their elements only by chemical changes, such as heating or chemical reactions.

Visual example: formation of sodium chloride

Let's learn about the formation of table salt, a common compound known as sodium chloride (NaCl). Below is a simplified illustration of how sodium and chlorine atoms combine to form sodium chloride:

Na , Cl NaCl

In this response:

  • Sodium (Na) loses one electron to become positively charged.
  • Chlorine (Cl) gains that electron and becomes negatively charged.
  • Sodium chloride is formed by the attraction between positively charged sodium and negatively charged chlorine.

Types of compounds

Compounds may be broadly classified into two types:

Molecular compounds

Molecular compounds are formed by sharing electrons between non-metal atoms. A good example of this is water.

H2 + O → H2O

Each hydrogen atom shares electrons with the oxygen atom, resulting in a covalent bond.

Ionic compounds

Ionic compounds form when electrons transfer from one atom to another, creating ions. These ions attract each other and form a bond. Sodium chloride (table salt) is an example of an ionic compound.

Na + Cl → NaCl

In sodium chloride, sodium loses an electron to become a positively charged ion, and chlorine gains an electron to become a negatively charged ion.

Examples of compounds

Water (H2O)

Water is perhaps the most well-known compound. It is essential to life and covers about 71% of the Earth's surface. Water's unique properties, such as its boiling and freezing point, surface tension, and ability to dissolve many substances, are quite different from those of its constituent elements hydrogen and oxygen.

Carbon dioxide (CO2)

Carbon dioxide is a compound made of carbon and oxygen. It is a gas at room temperature and is used by plants to make oxygen during photosynthesis.

C + O2 → CO2

Methane (CH4)

Methane is a simple hydrocarbon compound consisting of one carbon atom bonded to four hydrogen atoms. It is widely used as a fuel and is a primary component of natural gas.

C + H4 → CH4

How are compounds different from mixtures

It's important to distinguish between compounds and mixtures. Compounds are made up of elements combined in chemically definite proportions, while mixtures are made up of two or more substances that are mixed together without any chemical bonds.

For example, if you mix sand and salt, you get a mixture. Each component retains its properties and can be easily separated, such as with a sieve or water.

Sand , Salt Mixture

Conclusion

Understanding compounds and their properties helps us understand how they make up the world around us. From the water we drink to the air we breathe, compounds are essential to life and a variety of natural processes. By learning about compounds, you can better understand how chemistry plays an important role in our daily lives.


Grade 6 → 4.8


U
username
0%
completed in Grade 6

← Prev (4.7)
Definition of compound
Next (4.9) →
Definition of Mixture

Comments 



Properties of Compounds

https://www.chemistryelite.com/g6/4.8?ceal=en