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Electronegativity

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 . Electronegativity.

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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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