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Chemical Bonding and Molecular Structure Class 11 Notes Chemistry Chapter 4

  • Chemical Bond

    The force responsible for holding different atoms together in a molecule is termed as a chemical bond.

  • Octet Rule

    Atoms engage in chemical combinations to achieve a stable octet or noble gas configuration.

  • Valence Electrons

    Valence electrons are the outermost shell electrons involved in chemical bonding.

  • Facts Stated by Kossel in Relation to Chemical Bonding

    • In the periodic table, halogens and alkali metals are separated by noble gases.
    • Formation of anions and cations involves gain and loss of electrons.
    • Negative and positive ions attain noble gas configuration.
    • Ions are stabilized by electrostatic attraction.

  • Modes of Chemical Combination

    • Transfer of electrons results in an electrovalent or ionic bond.
    • Sharing of electrons leads to a covalent bond.
    • Coordinate bond forms when one atom contributes electrons shared by both.

  • Ionic or Electrovalent Bond

    • Complete electron transfer between atoms forms an ionic bond.
    • Typically occurs between metals and non-metals.
    • Compounds formed through this bond are electrovalent compounds.
Chemical Bonding Concepts:
  • Chemical Bond: The force that holds atoms together in a compound.
  • Octet Rule: Atoms tend to combine in such a way that they each have a full outer shell of eight electrons.
  • Valence Electrons: Electrons in the outermost energy level of an atom that are involved in bonding.
  • Facts Stated by Kossel in Relation to Chemical Bonding: Principles related to the arrangement of electrons in atoms.
  • Modes of Chemical Combination: Various ways in which atoms can combine to form compounds.
  • Ionic and Covalent Bonds:
  • Ionic or Electrovalent Bond: Formed by the transfer of electrons from one atom to another.
  • Factors Affecting the Formation of Ionic Bonds: Influences on the strength and stability of ionic compounds.
  • General Characteristics of Ionic Compounds: Properties shared by substances with ionic bonds.
  • Covalent Bond—Lewis-Langmuir Concept: Sharing of electron pairs between atoms to achieve stability.
  • Structural Aspects of Bonds:
  • Bond Length: Distance between the nuclei of two bonded atoms.
  • Bond Angle: The angle between two bonds originating from the same atom.
  • Bond Enthalpy: Energy required to break a bond between two atoms.
  • Bond Order: The number of chemical bonds between a pair of atoms.
  • Molecular Structures and Theories:
  • Resonance Structures: Different ways to depict the same molecule using Lewis structures.
  • Valence Shell Electron Pair Repulsion (VSEPR) Theory: Predicts the geometry of molecules based on electron pairs repelling each other.
  • Valence Bond Theory: Describes covalent bonding as the overlap of atomic orbitals.
  • Orbital Overlap Concept: Interaction of atomic orbitals to form molecular orbitals.
  • Hybridization and Molecular Behavior:
  • Hybridization: Mixing of atomic orbitals to form new hybrid orbitals.
  • Salient Features of Hybridization: Key characteristics of hybrid orbitals.
  • Formation of Molecular Orbitals: Combination of atomic orbitals to form bonding and antibonding orbitals.
  • Stability of Molecules: Factors influencing the stability of molecules in different bonding scenarios.
  • Special Bonding Cases:
  • Hydrogen Bonding: Attraction between a hydrogen atom and a highly electronegative atom.
  • Types of H-Bonds: Different classifications based on the nature of hydrogen bonding.
  • Bonding in Some Homonuclear Molecules: Bonding behavior in diatomic molecules like O2 and N2.
  • Magnetic Nature: Influence of electron spin on the magnetic properties of molecules.
  • The document Understanding Covalent Bonds | Chemistry for EmSAT Achieve is a part of the EmSAT Achieve Course Chemistry for EmSAT Achieve.
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