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 → Carbon and its compounds ↓


Isomerism in organic chemistry (structural and geometrical)


Introduction

In organic chemistry, isomers are compounds that have the same molecular formula but different structural or spatial arrangements. This phenomenon is known as isomerism. Isomerism is an essential concept because it explains the diversity in the chemical properties and behavior of organic compounds.

Types of isomerism

Isomerism is broadly classified into two types:

  • Structural isomerism
  • Stereo isomerism, which includes geometric isomerism

Structural isomerism

Structural isomerism, also known as constitutional isomerism, occurs when compounds have the same molecular formula but different structural formulas, that is, the atoms are connected in different ways.

Example of structural isomerism

Consider the molecular formula C4H10. This formula can represent two different alkenes:

1. CH3-CH2-CH2-CH3 (butane)
2. CH3-CH(CH3)-CH3 (2-methylpropane)

These are structural isomers because the arrangement of their atoms is different.

Stereoisomerism

Stereo isomerism occurs when two or more compounds have the same structural formula but differ in the orientation of their atoms in space. Geometrical isomerism is a type of stereo isomerism.

Geometrical isomerism

Geometrical isomerism is usually found in compounds containing carbon-carbon double bonds. The double bond shows restricted rotation, leading to different spatial arrangements called cis and trans isomers.

Cis-trans isomerism

The terms cis and trans are used to describe the relative positions of the substituents attached to the double-bonded carbon.

  • Cis isomer: The substituents are on the same side of the double bond.
  • Trans isomer: The substituents are on opposite sides of the double bond.

Example of geometrical isomerism

Consider the molecule C2H2Cl2:

1. cis-dichloroethene: Cl and H on one side, Cl and H on the other side.
2. trans-dichloroethene: Cl and H are opposite each other at the double bond.
C C Chlorine Sis C C Chlorine Trans

Importance of isomerism

The study of isomers is important because different isomers often have different chemical and physical properties. For example, cis- and trans- isomers can have different reactivities, boiling points, and states of matter.

Conclusion

Isomerism reflects the diversity of organic compounds beyond the basic molecular formulas. Understanding structural and geometric isomerism helps us understand more about the behavior and properties of substances, which is fundamental in the field of chemistry and opens up new application possibilities in various scientific disciplines.

Now that you understand isomerism, try to identify the different isomers in the compounds you come across to solidify your understanding of this concept.


Grade 10 → 9.5


U
username
0%
completed in Grade 10

← Prev (9.4)
Nomenclature of organic compounds (IUPAC system)
Next (9.6) →
Important organic reactions (combustion, addition, substitution, polymerization)

Comments 



Isomerism in organic chemistry (structural and geometrical)

https://www.chemistryelite.com/g10/9.5?ceal=en