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Chemical bonding

Chemical bonding

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🔬 Chapter 4: Chemical Bonding 🔬

  • Learning Outcomes 🎯:

    • Describe different types of bonding using dot-and-cross diagrams, including ionic, covalent, and co-ordinate (dative covalent) bonding.

    • Explain shapes and bond angles in molecules using electron-pair repulsion.

    • Describe covalent bonding in terms of orbital overlap, sigma and pi bonds, and hybridization.

    • Explain terms like bond energy, bond length, and bond polarity.

    • Describe intermolecular forces based on permanent and induced dipoles, hydrogen bonding, and metallic bonding.

    • Deduce the type of bonding present from given information. (Page 48)

  • Van der Waals’ Forces 💨:

    • Van der Waals’ forces are weak forces of attraction between atoms or molecules.

    • They arise due to temporary dipoles set up by the movement of electron charge clouds.

    • These forces increase with the increasing number of electrons and contact points between molecules.

    • They play a significant role in the boiling points of noble gases and other substances. (Page 14)

  • Bond Length and Bond Energy ⚛️:

    • Double bonds are shorter and stronger than single bonds.

    • Bond energy is the energy needed to break one mole of a given bond in a gaseous molecule.

    • Bond strength influences the reactivity of a compound. (Page 6)

  • Metallic Bonding 🧲:

    • Metals have a giant metallic structure with positive ions surrounded by a sea of delocalized electrons.

    • This structure explains why metals are good conductors of electricity and have high melting points. (Page 22)

  • Hydrogen Bonding and Boiling Point 🌡️:

    • Hydrogen bonding can cause compounds to have higher boiling points than expected.

    • Water has a much higher boiling point and enthalpy change of vaporization due to extensive hydrogen bonding. (Page 17)

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