6. Molecular vs. Ionic Equations Na + Na + Cl - Cl - Cl - Na + H + OH -1 OH -1 H + H + 3 NaCl 3 H 2 O OH -1
7.
8.
9.
10.
11.
12. SALTS The Solubility Table p. 344 Ion Solubility Exceptions NO 3 – soluble none ClO 4 – soluble none Cl – soluble except Ag + , Hg 2 2+ , *Pb 2+ I – soluble except Ag + , Hg 2 2+ , *Pb 2+ SO 4 2- soluble except Ca 2+ , Ba 2+ , Sr 2+ , Hg 2+ , Pb 2+ , Ag + CO 3 2- insoluble except Group IA and NH 4 + PO 4 3- insoluble except Group IA and NH 4 + OH – insoluble except Group IA, *Ca 2+ , Ba 2+ , Sr 2+ S 2- insoluble except Group IA, IIA and NH 4 + Na + soluble none K + soluble none NH 4 + soluble none
13.
14.
15.
16.
Editor's Notes
To understand why a pickle will glow when electricity is passed through it, you need to understand today’s lesson. Earlier in the year you discussed writing molecular equations, today we are going to discuss how to write net ionic equations, and talk about all the terminology associated. Movie Explanation: When energy is added to electrons in an atom they give off visible light (in waves). Soduim Chloride (NaCl) emits a yellow / orange color Ok what does all this have to do with a glowing pickle??? Well what is in a pickle? Salt - NaCl. So if you add energy to the sodium atoms in the pickle, the pickle will glow
Solute – the substance present in smaller amount in a solution Solvent – the substance present in larger amount in a solution Solution – A homogeneous mixture of two or more substances Homogeneous Mixture – A mixture that is the same throughout. Mixture – a combo of two or more substances in which the substances retain their identity. Dissolve – To pass into solution, or break into component parts.
In many cases, reactants and/or products will exist in solution as ions so its more accurate to write an ionic equation for a reaction. Molecular equation represents a chemical reaction of two or more substances and shows reactants and products in their molecular form Ionic equation shows soluble salts, acids, and bases that ionize (break apart) completely as ions, their true form in solution.
If phase labels are persent, soluble salts, acids, and bases that ionize completely are labeled aqueous Pure liquids, solids, and gases to not ionize If phase labels are not given, you must use the solubility table to determine which salts are soluble. Watch for Exceptions on the table You will also need to determine if acids and bases present will ionize. Only strong acids and bases ionize completely.
![Stuff you already know! ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)