Grade 7
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Scientific Method in Chemistry  1.5. Laboratory Safety Rules and Precautions  1.6. Common Laboratory Equipment and Their Uses  1.7. Units of measurement in chemistry
  2. Matter and its properties  2.1. Definition of Matter  2.2. Classification of matter  2.3. Properties of matter  2.3.1. Physical properties  2.3.2. Chemical properties  2.4. States of matter  2.4.1. Solid state  2.4.2. Fluid state  2.4.3. Gaseous state  2.4.4. Plasma and Bose–Einstein condensates  2.5. Changes in the states of matter  2.5.1. Melting and freezing  2.5.2. Evaporation and Condensation  2.5.3. Sublimation and deposition  2.6. Density and its applications  2.7. Diffusion and its importance
  3. Elements, Compounds, and Mixtures  3.1. Definition of the element  3.2. Classification of elements  3.3. Metals, Nonmetals and Metalloids  3.4. Noble gases and their properties  3.5. Introduction to the Periodic Table  3.6. Definition of Compound  3.7. Properties of Compounds  3.8. Introduction to Chemical Formulas  3.9. Definition of Mixture  3.10. Types of mixtures  3.10.1. Homogeneous mixture  3.10.2. Heterogeneous mixtures  3.11. Difference Between Compounds and Mixtures  3.12. Solutions, Colloids and Suspensions
  4. Separation of mixtures  4.1. Need for separation of mixtures  4.2. Separation methods  4.2.1. Filtration  4.2.2. Sedimentation and decantation  4.2.3. Evaporation  4.2.4. Crystallization  4.2.5. Distillation  4.2.6. Chromatography  4.2.7. Magnetic Separation  4.2.8. Centrifugation
  5. Atomic Structure  5.1. Introduction to Atoms  5.2. Structure of the atom  5.2.1. Nucleus and electron cloud  5.3. Subatomic particles  5.3.1. Proton  5.3.2. Neutron  5.3.3. Electrons  5.4. Atomic number and mass number  5.5. Isotopes and their uses  5.6. Ions and ion formation
  6. Periodic table  6.1. Introduction to the Periodic Table  6.2. Groups and periods  6.3. Trends in the Periodic Table  6.3.1. Atomic Size  6.3.2. Metallic and non-metallic character  6.3.3. Electronegativity  6.3.4. Reactivity of the elements  6.4. Alkali metals and their properties
  7. Chemical bond  7.1. Why do atoms form bonds?  7.2. Types of chemical bonds  7.2.1. Ionic bond  7.2.2. Covalent bond  7.2.3. Metal Bond  7.3. Properties of Ionic and Covalent Compounds  7.4. Intermolecular forces
  8. Chemical reactions  8.1. Introduction to Chemical Reactions  8.2. Signs of a chemical reaction  8.3. Types of Chemical Reactions  8.3.1. Combination Reactions  8.3.2. Decomposition reactions  8.3.3. Displacement reactions  8.3.4. Double displacement reactions  8.3.5. Combustion reactions  8.4. Law of conservation of mass  8.5. Balancing simple chemical equations
  9. Acids, Bases and Salts  9.1. Definition of Acid and Base  9.2. Properties of Acids  9.3. Properties of bases  9.4. pH Scale and Indicators  9.5. Neutralization reactions  9.6. Common Acids and Bases in Everyday Life  9.7. Preparation and use of salts  9.8. Strong and weak acids and bases
  10. Solutions and Solubility  10.1. Definition of Solution  10.2. Components of the solution  10.2.1. Solvent  10.2.2. solute  10.3. Factors Affecting Solubility  10.4. Concentration of solutions  10.5. Saturated and unsaturated solutions  10.6. Colloids and suspensions  10.7. Solubility curve and its interpretation
  11. Air and atmosphere  11.1. Composition of air  11.2. Properties of gases in the air  11.3. Importance of Oxygen and Carbon Dioxide  11.4. Air pollution and its effects  11.5. Greenhouse effect and global warming  11.6. Ways to reduce air pollution  11.7. Ozone layer and its importance
  12. Water and its importance  12.1. Properties of Water  12.2. Water as the universal solvent  12.3. Importance of water for life  12.4. Water pollution and its effects  12.5. Water Purification  12.5.1. Filtration  12.5.2. boil  12.5.3. Chlorination in water purification  12.5.4. reverse osmosis  12.6. Hard and soft water  12.7. Water cycle and its importance
  13. Fuel and energy  13.1. Types of fuel  13.1.1. Fossil fuels  13.1.2. Renewable energy sources  13.2. Combustion and energy release  13.3. Global warming and its effects  13.4. Alternative sources of energy  13.5. Ways to conserve energy
  14. Metals and Nonmetals  14.1. Physical and chemical properties of metals  14.2. Physical and Chemical Properties of Non-Metals  14.3. Difference Between Metals and Nonmetals  14.4. Uses of metals and nonmetals  14.5. Corrosion of metals and its prevention  14.6. Alloys and their importance
  15. Plastics and polymers  15.1. Natural and synthetic polymers  15.2. Properties of plastics  15.3. Biodegradable and Non-Biodegradable Plastics  15.4. Environmental impact of plastic  15.5. Recycling and waste management in plastics and polymers  15.6. Daily Uses of Polymers
  16. Introduction to Organic Chemistry  16.1. Basic definitions of organic chemistry  16.2. Carbon Compounds in Daily Life  16.3. Hydrocarbons  16.4. Simple functional groups (alcohols and carboxylic acids)  16.5. Importance of organic compounds in industry

Grade 7 → Chemical bond → Types of chemical bonds ↓


Metal Bond


When we dive into the world of chemistry, we find how different atoms connect to each other. One of the fascinating types of connection or bond between atoms is called metallic bonding. Understanding metallic bonding helps us know why metals have unique properties such as the ability to conduct electricity, shine, and take shape in different forms. Let us learn about metallic bonding in detail.

What is metallic bonding?

Metallic bonding occurs in metals. It is different from other types of bonding such as ionic and covalent bonding. In metallic bonding, metals share a "sea of electrons." These electrons are not attached to any particular atom. Instead, they move freely throughout the structure. Imagine the atoms in the metal as positive ions in a sea, with the electrons flowing like water in an ocean.

Because these electrons can move, they are called "delocalized electrons." They enable metals to transmit electricity and heat, to bend without breaking, and to shine.

Structure of metallic bonds

Metallic bonds form a unique kind of lattice structure. In a metal crystal, atoms are arranged in a dense and ordered pattern. This close packing allows a sea of electrons to flow freely around the metal ions.

Visualizing metallic bonding

, , , , ,

In this simplified diagram, the blue boxes represent metal atoms as positive ions, while the circles within them represent electrons moving freely in a delocalized way. The larger circles around them symbolize the collective "sea of electrons." This shows how electrons can move freely around many atoms.

How metallic bonding works

Metals have a small number of electrons in their outer shell. For example, sodium (Na) has one electron in its outer shell. It is easy for metals to lose these electrons to become stable. When metal atoms come together, they donate electrons to the common sea, which allows the atoms to stick together, thus forming strong bonds.

Na (s) → Na + + e −

This equation shows how sodium donates electrons to the sea. It then becomes a positively charged ion. Many such ions form a lattice structure held together by delocalized electrons, forming a solid metal object.

More examples of metals

Let's take a closer look at other examples, such as iron (Fe) and copper (Cu):

Fe → Fe 2+ + 2e −
Cu → Cu 2+ + 2e −

In these equations, the iron and copper atoms lose electrons and form a sea of electrons around the positive ions, forming metallic bonds.

Properties of metallic bonds

The unique properties of metallic bonds are a result of the movement of free electrons. Let's take a look at some of these properties.

Conductivity

Metals are known for their ability to conduct electricity. This is because free moving electrons can carry electric current. When an electric field is applied to a metal, it moves the electrons in a directed flow, thereby conducting electricity.

Similarly, metals are good conductors of heat because they have moving electrons, which transfer energy quickly through the material.

Malleability and ductility

Metals can be hammered or pressed into thin sheets (malleability) and drawn into wires (ductility). This is because metal atoms can slide over one another without breaking the metallic bonds, thanks to the sea of electrons that constantly flow to maintain the bonds.

Aura

The shiny appearance of metals, known as lustre, is due to their ability to reflect light. Free electrons on the metal surface can absorb and re-emit energy in the form of light, giving metals their shiny appearance.

Conclusion

Metallic bonding is a fascinating aspect of chemistry. It is a bridge to understanding why metals behave the way they do and are important to so many everyday applications. From electrical wiring to cooking utensils, the principles of metallic bonding ensure that metals remain indispensable in our world. By exploring the concepts of metallic bonding, one gains a better understanding of the fundamental nature of the materials that shape our lives.


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Covalent bond
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Properties of Ionic and Covalent Compounds

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Metal Bond

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