Write the molecular, ionic, and net ionic equation for the above

Honors Chemistry Macroscopic vs. Submicroscopic “Particulate Diagrams”

Double Replacement Reactions

Complete the following word equation for a reaction of two aqueous solutions:

magnesium chloride and silver nitrate  ____________________ + _____________________

Write the molecular, ionic, and net ionic equation for the above reaction. (Include states of matter)

Molecular equation:

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Ionic equation:

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Net ionic equation:



Draw a particulate model of this reaction, before the reaction and after as much precipitate can form. In each drawing

include 6 of each of the ions, magnesium, chloride, silver and nitrate. Identify ions with charges. Be sure to show a

difference when a substance is dissolved in solution or precipitated out of solution.

Before reaction: When reaction stops:

Which ions are the spectator ions? Why are they not written in the net ionic equation?

If you started with 6 ions of silver and 3 ions of chloride, how would this affect the amount of precipitate you would get?

What other ion (besides the spectator ions) would still be in the solution after the reaction is complete?

MACROSCOPIC

What do the solutions look like before they are combined?

What does this reaction look like after they are combined?