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Ionic Bond

Learn about the formation of ionic bonds between sodium and chlorine atoms, the role of electron transfer, and the creation of stable configurations. Explore covalent bonds, orbitals, and Lewis dot symbols in chemical bonding processes.

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Ionic Bond

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  1. Ionic Bond A sodium atom loses an electron from its last shell and forms a cation. The cation, now, has the neon configuration, [Ne]. This configuration is very stable since it corresponds to a noble-gas configuration. The chlorine atom, on the other hand, receives the electron from the sodium atom, itself attaining the argon configuration [Ar]. This configuration is also very stable, corresponding to a noble-gas configuration. It is the stability of the ions that ultimately lead to the formation of the ionic solid, NaCl. Once a cation or an anion is formed, it starts to attract oppositely charged ions immediately. This attraction improves stability furthermore, attaining the crystal structure ultimately. The ionic solid represents the lowest energy level, and therefore maximum stability.

  2. Covalent Bond

  3. Orbitals in Covalent Bond

  4. Bond Energies

  5. Lewis Dot Symbols Each element is shown by its elemental symbols and valence electrons only

  6. : : : H Cl : Formation of Hydrogen Chloride 1bonding pair • Cl H 3 lone pairs When the atoms combine, they form a stable covalent bond. This bond is a single bond, denoted by a single line between the two atoms. Each single bond represents a pair of electrons. By sharing a pair of electrons, hydrogen is surrounded by two and chlorine is surrounded by eight valence electrons.

  7. Electronegativities of Elements

  8. Formation of Hydrogen Fluoride

  9. Interference of Waves Constructive Destructive

  10. Shapes of Orbitals

  11. Structure of Methane

  12. sp3 Hybridisation

  13. Common Hybridisations

  14. Arrangement of Electron Pairs

  15. Molecular Shapes

  16. Molecular Shapes

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