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Ionic Bonds

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Vocabulary

  • Vocabulary: ionic bond, cation, anion, crystal lattice

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Ionic Compounds

An ionic bond  is the complete transfer of valence electrons between atoms. It is a type of chemical bond that generates two oppositely charged ions.

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Electronegativity

    • A bond where there is a large electronegativity difference between the elements is an ionic bond. Metals have low electronegativity and nonmetals have high electronegativity, so when they form a bond there is a large difference.

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Electronegativity

  • Nonmetals attract outside electrons well. When a nonmetal is near a metal, it will attract/pull its valence electrons. This is because nonmetals have a strong force of attraction in their nucleus.

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ionic compounds are made up of

a positively charged metal (cation)

negatively charged non-metal (anion)

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  • Atoms form ions because they have available spots in their valence shell. They will gain or lose electrons to make sure they have a full valence shell. (OCTET RULE)

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Properties of Ionic Compounds

1. Most ionic compounds exist as crystalline solids.

    • These are a network of positive and negative ions known as a crystal lattice.

2. Ionic bonds are very strong due to the crystal lattice structure.

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Properties of Ionic Compounds

3. The strength of this bond leads to ionic compounds having a higher melting point, boiling point, and hardness.

4. Ionic compounds easily dissolve in water.

5. In solution, ionic compounds are good electrical conductors because the ions move freely to carry a current.

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Example

  • Use electron-dot notation to demonstrate the formation of the following ionic compounds:
    • Li and Cl
    • Ca and I

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Recap

  • Properties of ionic compounds:
    • Balance positive and negative charges
    • Strong bonds
    • High melting point, boiling point, conductivity
    • Exist as a “crystal lattice”
  • Draw Lewis structures to depict ionic compounds
    • Start with LDS for each element.
    • Determine which will gain electrons and which will lose electrons.
    • Draw arrows to show movement of electrons.