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Lesson 4 Ionic and Molecular Compounds

  Interactive Activity

Ionic Bonding Tutorial @ ChemThink


Work through slides 1 to 27. At times, you will need to interact with simulations to continue the slideshow. https://quick.adlc.ca/IonicBonding

Click on the procedure tab to continue.
  1. Click on the play icon to open the tutorial.
  2. Read the content on slides 1 and 2.

    What happens when you drag the negative ions close together?

    They repel each other.
  3. Read slide 3.

    What happens when you drag the negative ion close to the positive ion?

    They attract each other.
  4. Read slides 4 to 19.

    Describe the structure on slide 19.

    The structure is an alternating arrangement of small red spheres and larger blue spheres, set up in a three-dimensional array.
  5. Read slides 20 and 21.

    Count the number of chloride ions and sodium ions.

    sodium ions = 3
    chloride ions = 3
  6. Read slides 22 to 24. On Slide 24, rotate the crystal.

    Count the number of calcium ions and fluoride ions. What is the formula for the ionic crystal?

    calcium ions = 4
    fluoride ions = 8
    formula = CaF2
  7. Read slides 25 to 27.

Read This

Please read pages 34, 35, and 40 to 41 in your Science 10 textbook. Make sure you take notes on your readings to study from later. You should focus on how electrons are transferred to form ionic bonds. Remember, if you have any questions or you do not understand something, ask your teacher!

  Practice Questions

Complete the following practice questions to check your understanding of the concept you just learned. Make sure you write complete answers to the practice questions in your notes. After you have checked your answers, make corrections to your responses (where necessary) to study from.

Fill in the blanks for each of the following questions.

  1. Ionic bonds are formed between a __ and a ___.

    2. Ionic bonds are formed between a metal and a non-metal.

  2. An ionic bond is formed by the __ of ___.

    An ionic bond is formed by the transfer of electrons.
  3. A metal atom __ electrons to form a ___, while a non-metal ___ electrons to become an ____.

    A metal atom loses electrons to form a cation, while a non-metal gains electrons to become an anion.
  4. The two oppositely charged ions ___ each other to form an ___ compound.

    The two oppositely charged ions attract each other to form an ionic compound.
  5. Using your own words, explain the formation of an ionic compound, starting with sodium atoms and chlorine atoms.

    Your answer should be a variation of the following. Remember that elements gain or lose electrons when forming compounds so that they achieve a full outer shell. Let's now look at the reaction between sodium and chlorine. A sodium atom loses one electron to achieve a full outer shell, and chlorine gains one electron to complete a full outer shell. So when a sodium atom reacts with a chlorine atom, the sodium atom loses its one electron to chlorine. The two ions formed are a sodium ion, Na+, and a chlorine ion, Cl–. The two ions have opposite charges, and they attract one another. The force of attraction between them is an electrostatic one. This type of attraction is strong. It is called an ionic, or electrovalent, bond.
  6. Explain why Mg25F52 would never be a chemical formula.

    Metals and non-metals join in an ionic structure that is expressed in lowest terms. MgF2 is the correct formula.