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Electronegativity

Electronegativity is a key concept in chemistry, particularly in understanding ionic bonds. When the difference in electronegativity between two atoms exceeds 1.6, the bonding electrons are completely transferred to the more electronegative atom, resulting in the formation of ions. For example, in sodium chloride (NaCl), sodium loses one electron to become a positively charged ion, while chlorine gains an electron to become a negatively charged ion. The electrostatic attraction between these oppositely charged ions forms an ionic bond, creating a structured lattice in ionic compounds like table salt.

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Electronegativity

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  1. Electronegativity Sometimes the difference in electronegativity between two atoms is so vast (greater than 1.6) that the bonding electrons are fully transferred to the most electronegative atom.

  2. Electronegativity Sometimes the difference in electronegativity between two atoms is so vast (greater than 1.6) that the bonding electrons are fully transferred to the most electronegative atom. E.g. Na Cl

  3. Electronegativity Lost one (1) electron: Becomes positively charged by one; therefore +1. Gained one (1) electron: Becomes negatively charged by one; therefore -1. Na Cl

  4. Ionic bonds The oppositely charged ions attract to each other. The electrostatic attractive force between these ions is called an ionic bond. Na Cl

  5. Ionic bonds The oppositely charged ions attract to each other. The electrostatic attractive force between these ions is called an ionic bond. Bonding Ionic Covalent Lewis structures Polarity Electronegativity

  6. Ionic bonds For ionic compounds the positive and negative ions are arranged in a lattice. For example, table salt (NaCl). Na Cl Na Cl Na Cl Na Na Cl Na Cl

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