Equations - -1 - Inorganic Chemistry Writing (Net Ionic)...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
- 1- Inorganic Chemistry Writing (Net Ionic) Equations for Various Reactions On the AP examination you will encounter a question in which you will be required to write net ionic equations for various reactions. In past years, students have been required to choose 5 of 8 reactions. Some of the reactions you will undoubtedly recognize; others you will not! Hopefully, at least of them will be familiar to you! On the examination you will be given reactions that actually occur - you will not be required to figure out whether or not the reaction actually works, as you did in ‘Introductory’ Chemistry. You will be required to write equations in ionic form - i.e. for ionic compounds you write the anions (-) and cations (+) as separate entities. You also omit the spectator ions - those ions that do not take part in the reaction. You wrote several different types of net ionic equations in ‘INTRODUCTORY’ Chemistry. On this handout, an attempt has been made to summarize the most important types of reactions. It will not be possible, or useful, for you to learn dozens of specific reactions. Learn the general reactions, and figure out the specifics on the examination! FOR THE EXAMINATION YOU WILL NEED TO KNOW: Formulae For Common Ions Refer to the Table of Ionic Charges - hopefully all the polyatomic ions that you will encounter on the examination are on this chart. Refer also to the Table of Standard Reduction Potentials , which you will be given on the examination. Formulae For Common Acids Again, refer to the Table of Ionic Charges General Solubility Rules Refer to the Solubility Table - you will need to know the general “trends”. ON THIS HAND-OUT REFERENCE IS MADE TO: ELEMENTS - both metals and non-metals ACIDS - both dilute and concentrated BASES - soluble metal hydroxides (NaOH and KOH being the most common, by far) - soluble carbonates (Na 2 CO 3 and K 2 CO 3 being the most common) - an aqueous solution of ammonia , NH 3 (aq) SALTS - ionic compounds that are neither acids nor bases. In general, MX , where M is a metal and X is an anion such as Cl - , So 4 2- , PO 4 3- WATER OXIDES PEROXIDES COMBUSTION REACTIONS REDOX REACTIONS
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
- 2- Precipitation (Double Displacement) Reactions If you have two salts reacting, and a reaction occurs, the chances are excellent that it will be a precipitation (double displacement) reaction. The precipitate will, obviously, be the insoluble salt . Example Write the net ionic equation for the reaction that occurs when an aqueous solution of silver nitrate is added to an aqueous solution of copper(II) chloride. Answer Ag + (aq) + Cl - (aq) ---> AgCl(s) Refer back to the hand-out on precipitation reactions which you were given in Term 2. There could be
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 07/15/2011 for the course CHEM 2045 taught by Professor Gower during the Spring '11 term at University of Florida.

Page1 / 11

Equations - -1 - Inorganic Chemistry Writing (Net Ionic)...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online