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 → Periodic table ↓


Noble gases and their chemical inertness


Introduction to noble gases

The noble gases form a group of chemical elements with similar properties found in group 18 (also called group 8A) of the periodic table. These elements are: helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). Each of these elements is colorless, odorless, tasteless, and non-flammable. One characteristic they all have in common is chemical inertness, which means they are not very reactive.

H He by AR Sl Ze R N

Why are noble gases inert?

The main reason for the noble gases being inert is their electronic configuration. The noble gases have a full valence shell, which means they have the maximum number of electrons in their outer shell. This configuration is very stable and gives them a very low tendency to gain or lose electrons, making them unlikely to react with other elements.

For example, helium (He) has a full valence shell with 2 electrons, while neon (Ne) and argon (Ar) have full shells with 8 electrons. Normally, chemical reactions occur in such a way that atoms can achieve stable electron configurations similar to those of the noble gases. However, since the noble gases already have these configurations, they do not need to react with other elements.

Electronic configuration of noble gases

Let us look at the electronic configuration of noble gases:

Helium (He): 1s 2
Neon (Ne): 1s 2 2s 2 2p 6
Argon (Ar): 1s 2 2s 2 2p 6 3s 2 3p 6
Krypton (Kr): 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6
Xenon (Xe): 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6
Radon (Rn): 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6

Unique properties of noble gases

Each noble gas has unique properties that make it useful for various applications in industries and scientific research. Here is a brief overview:

  • Helium (He): This is the second lightest element and is non-flammable, making it ideal for use in balloons and as a protective gas in welding.
  • Neon (Ne): Known for its distinctive glow when electrically stimulated, perfect for use in neon signs.
  • Argon (Ar): It is used in incandescent and fluorescent lighting and as a protective atmosphere for arc welding due to its inertness.
  • Krypton (Kr): Often used in high performance lighting products and photography.
  • Xenon (Xe): It is used in light emitting devices and as a general anesthetic.
  • Radon (Rn): Due to its radioactivity, it is used in radiotherapy for the treatment of cancer.
Full valence shell

Exploring the applications of noble gases

Noble gases have important applications due to their chemical inertness and unique properties. Let us find out how these gases are used in various fields:

Helium

Helium is commonly known for its use in balloons, due to its low density and inertness, which makes it safer than hydrogen. It also plays an important role in cryogenics, particularly in cooling superconducting magnets used in medical imaging equipment such as MRI machines. Its non-reactive property also makes it ideal for use in protective gas mixtures for arc welding.

Neon

Neon is known globally for neon lights, which are famous in advertising and art because of their bright and distinctive glow. This gas emits different colors when used in various types of glass tubes excited by electricity. Neon is also used in high-voltage testers and as a cryogenic refrigerant.

Argon

Argon is used in the lighting industry, particularly in fluorescent tubes and incandescent lighting because of its inertness, which protects the filament in the bulb and reduces its evaporation. This gas is also used as an inert shield for arc welding and in the production of titanium and other reactive elements.

Krypton

Krypton is used in high-performance flashlights used in photography because of its white light. It is also used in fluorescent lamps in combination with other gases to improve efficiency and brightness.

Xenon

Xenon is used in a variety of light emitting devices. Because of its fast response time, xenon gas is used in xenon flash lamps for photographic flashes and aircraft landing lights. It is also used in ion propulsion systems for spacecraft because of its ability to produce a high thrust-to-weight ratio.

Radon

Although radon is radioactive, it has some applications, especially in the field of medicine. It was historically used in the treatment of cancer, but its use has declined due to safety concerns. Nowadays, radon is commonly used for geological research, as its presence can be an indicator of underlying radioactive minerals.

Example:

If the noble gases are placed under certain conditions where they are forced to react, they do so with difficulty. For example, xenon can form compounds such as XeF 4 or xenon tetrafluoride. However, these conditions are not usually found in nature, which is why noble gases are considered inert in everyday occurrences.

Conclusion

The chemical inertness of the noble gases makes them extremely valuable in many industrial and scientific applications. Their unique ability to avoid reacting with other elements under standard conditions is primarily due to their full valence electron shell, which gives them a stable configuration. As a result, these gases have created their own specialized roles that exploit their stability, safety, and distinctive electrical or visual properties. Understanding the noble gases makes the incredible diversity and complexity of the elements within the periodic table even more clear, illustrating how specific properties can drive an element's functionality and application in our world.


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Noble gases and their chemical inertness

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