Electrochemistry Lesson 1

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Presentation transcript:

Electrochemistry Lesson 1 Net Ionic Equations

Electrochemistry Electrochemistry is the interconnection between electricity and chemical reactions. Examples include: Cars rusting (oxidation of metals) Why Mars is red (the soil is rich in iron, which quickly oxidizes and turns red) How batteries work (chemicals inside create electrical energy) Why your skin goes green wearing some jewellery (the moisture in your skin causes a reaction)

Review - Charges What is the charge when these metals become ions? Sodium Copper Gold Magnesium Zinc Potassium Aluminum Silver Hydrogen A reminder that when ions have a positive charge, it is because they have LOST electrons. If they have a negative charge, it is because they have GAINED electrons.

Review - Charges Write the charge on each ion in the compound: a) Al(OH)3 d) Cu(NO3)2 b) Fe2S3 e) Au2(CO3)3 c) K2O f) MgO

Review - Single Displacement Word Equation: Zinc + Copper (II) Sulfate → Balanced Equation:

Review - SD Physical Observations: Zinc is grey, and copper sulfate is a blue solution. When zinc is added to the copper solution, it appears to fizz and seems to dissolve. The blue solution turns grey, and a reddish precipitate starts to appear.

Review - SD Analysis: zinc is displacing the copper – it bonds with sulfate in solution, leaving solid copper to form Activity Series: activity series predicts that this reaction does occur, because zinc is a more active metal than copper. If it wasn’t, no changes would occur when the two are mixed.

NEW: Net Ionic Equations A net ionic equation is when a chemical equation is written with all the aqueous ionic or polyatomic compounds written in their ionic form. Solids and liquids and gases cannot be written in ionic form – only aqueous.

Example from Before: Write as a net ionic equation: Zn (s) + CuSO4 (aq) → Cu (s) + ZnSO4 (aq)

Example: Complete the following equation, balance it, and write the total and net ionic equations, and spectator ions: Mg (s) + Ag3PO4 (aq) →