Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 → Chemical bond ↓


Metallic bond and its properties


Chemistry is a fascinating subject that delves deep into the nature of the various bonds that join atoms together. Among these various bonds, the metallic bond is particularly unique and plays a vital role in the structure and properties of metals. In this long article, we will explore the metallic bond, its characteristics, and its applications. Keep in mind that we will use simple language so that even beginners in chemistry can easily understand the concept.

What is metallic bonding?

Metallic bonding is a type of chemical bond that occurs between atoms of metallic elements. It is characterized by the sharing of free electrons between lattices of metal atoms. This bond explains many of the physical properties of metals, such as their ability to conduct electricity and heat, their malleability, and their lustre.

To better understand metallic bonding, let's consider how metals are arranged. In a metal, the atoms are packed closely together in a specific pattern. This forms a solid structure called a "metal lattice." The unique aspect of metallic bonding is that the electrons from the outer shells of the metal atoms do not stick to any particular atom. Instead, they become "delocalized," meaning they are free to move throughout the structure. These freely moving electrons are often referred to as a "sea of electrons."

Visualizing metallic bonding

To better understand this concept, let's take a look at a simple diagram of a metallic bond:

<svg width="200" height="200" xmlns="http://www.w3.org/2000/svg">
    <circle cx="60" cy="60" r="15" fill="blue"/> 
    <circle cx="140" cy="60" r="15" fill="blue"/> 
    <circle cx="60" cy="140" r="15" fill="blue"/> 
    <circle cx="140" cy="140" r="15" fill="blue"/> 
    <text x="60" y="60" font-family="Arial" font-size="10" fill="white" text-anchor="middle" dy=".3em">M</text> 
    <text x="140" y="60" font-family="Arial" font-size="10" fill="white" text-anchor="middle" dy=".3em">M</text> 
    <text x="60" y="140" font-family="Arial" font-size="10" fill="white" text-anchor="middle" dy=".3em">M</text> 
    <text x="140" y="140" font-family="Arial" font-size="10" fill="white" text-anchor="middle" dy=".3em">M</text> 
    <circle cx="100" cy="100" r="5" fill="yellow"/> 
    <circle cx="80" cy="80" r="5" fill="yellow"/> 
    <circle cx="120" cy="80" r="5" fill="yellow"/> 
    <circle cx="80" cy="120" r="5" fill="yellow"/> 
    <circle cx="120" cy="120" r="5" fill="yellow"/> 
    <line x1="65" y1="70" x2="100" y2="100" stroke="black" stroke-width="1"/> 
    <line x1="135" y1="70" x2="100" y2="100" stroke="black" stroke-width="1"/> 
    <line x1="65" y1="150" x2="100" y2="100" stroke="black" stroke-width="1"/> 
    <line x1="135" y1="150" x2="100" y2="100" stroke="black" stroke-width="1"/> 
    </svg>

In this diagram, the blue circles represent metal atoms, while the yellow circles represent delocalized electrons. Note that the electrons are not attached to any one atom, but move freely around the metal lattice.

Main characteristics of metallic bond

Understanding metallic bonding is incomplete without discussing its special characteristics. Let us look at these characteristics one by one:

1. Electrical conductivity

One of the most remarkable properties of metals is their ability to conduct electricity. This ability can be attributed to delocalized electrons. When a voltage is applied to a metal, these free electrons can move easily through the lattice, producing an electric current.

For example, consider copper (Cu), which is widely used in electrical wiring due to its excellent electrical conductivity. This property makes copper indispensable in construction, electronics, and even household appliances.

2. Thermal conductivity

Similar to electrical conductivity, metals also exhibit high thermal conductivity. When heat is applied to a metal, the free electrons can rapidly transfer thermal energy throughout the lattice. This rapid transfer results in a uniform distribution of heat across the metal surface.

Remember the last time you touched a metal spoon placed in a hot pot? The spoon heated up quickly due to its high thermal conductivity.

3. Malleability and ductility

Metals can be beaten into thin sheets (malleability) or drawn into wires (ductility) without breaking. This property arises because metal atoms can slide past one another within the lattice structure. The presence of free, mobile electrons allows easy rearrangement of metal atoms under stress.

Think of gold, for example. Gold is so malleable that one gram can be hammered into a thin sheet one square meter in size. Such malleability makes metals useful in industries such as construction, automotive and jewelry making.

4. Glossy appearance

Metals have luster, which means they can reflect light and appear shiny. This property is mainly due to the oscillation of free electrons on the metal surface, which interact with light waves, reflecting them evenly.

Examples of metallic bonding

To consider practical applications and examples, let's look at some commonly occurring metals and their uses:

1. Aluminium (Al)

Aluminum is a lightweight but strong metal, making it valuable in the aerospace and automotive industries. It has excellent corrosion resistance, which is why it is often used in outdoor structures.

2. Copper (Cu)

Copper's high electrical conductivity and corrosion resistance make it ideal for electrical wiring and plumbing. It is also used in making coins and, due to its antimicrobial properties, is also used in medical equipment.

3. Iron (Fe)

Iron is one of the most widely used metals due to its strength and abundance. It is a primary component in steel production and is used in construction, automobiles, and appliances.

4. Gold (Au)

Gold does not rust, which is why it is used in making jewelry. Its malleability and ductility means it can be formed into intricate designs. In addition, gold is used in electronics and aerospace for its corrosion resistance and conductivity.

Differences between metallic bond and other types of chemical bonds

It is important to distinguish between metallic bonds and other types of chemical bonds: ionic and covalent bonds.

Ionic bond

In ionic bonding electrons are transferred from one atom to another, creating positive and negative ions that attract each other. This is fundamentally different from metallic bonding, where electrons are shared between multiple atoms.

<svg width="200" height="100" xmlns="http://www.w3.org/2000/svg"> <circ...

Grade 10 → 4.4


U
username
0%
completed in Grade 10

← Prev (4.3)
Covalent Bond and Properties of Covalent Compounds
Next (4.5) →
Molecular geometry and VSEPR theory

Comments 



Metallic bond and its properties

https://www.chemistryelite.com/g10/4.4?ceal=en