1 / 13

More on Reactions

More on Reactions. Predicting Products Solubility Rules. Synthesis. In a simple synthesis reaction, two elements can combine to form a binary ionic compound Remember to correctly write the ionic compound’s formula, you must balance charges Balance the equation when you finish. Decomposition.

kirkan
Download Presentation

More on Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. More on Reactions Predicting Products Solubility Rules

  2. Synthesis • In a simple synthesis reaction, two elements can combine to form a binary ionic compound • Remember to correctly write the ionic compound’s formula, you must balance charges • Balance the equation when you finish.

  3. Decomposition • In a simple decomposition reaction, we can predict that a binary compound will break down into its elements • Remember that some elements are diatomic in their elemental form • Balance the equation when you finish.

  4. Combustion • If a hydrocarbon (any compound with C and H) is combusted, it will react with oxygen gas (O2) to burn. • The products will be carbon dioxide (CO2)and water, usually in the form of water vapor or steam (H2O). • Then balance the equation with coefficients to have correct #’s of C,H, and O on both sides.

  5. Single Replacement One element replaces another in a compound • Cationic: a metal replaces the cation (another metal) in a compound • H can act as the cation in these reactions • Anionic: a nonmetal replaces the anion (another nonmetal) in a compound

  6. Single Replacement • For this class, you can assume a single replacement reaction will occur if you are asked to predict its product. • Don’t forget that some elements are diatomic when they are alone (not in a compound). You also must balance charges to write correct formulas for the compounds.

  7. Double Replacement • The cation of one compound switches places with the cation of the other compound • Don’t forget that you will need to balance charges to write the correct formula for each compound. • Balance the overall equation after you have written correct formulas.

  8. Types of Double Replacement • Production of a gas • Two compounds combine to form a gas and another product • Production of a precipitate • Two aqueous solutions combine to form a solid precipitate and another product • Acid/Base Neutralization* • An acid combines with a base to form a salt (any ionic compound) and water

  9. Acid/Base Neutralization Terms* • Remember, acids begin with H (not water) • Examples: HCl, HNO3 • Bases are ionic compounds with hydroxide (OH) as the anion • Examples: NaOH, Ba(OH)2 • The word “salt” refers to any ionic compound formed from reacting an acid with a base • Examples: CaBr2, NaCl

  10. Solubility Rules • Solubility Rules are used to give us a general idea of whether or not an ionic compound will dissolve in water to form an aqueous solution • These are very useful in determining states of matter for your compounds in reactions, especially double replacement precipitation reactions.

  11. What Solubility Rules Mean • Solubility Rules give you general guidelines based on cations and anions present in an ionic compound. • For each compound you have in the presence of water, look for a rule that will describe it.

  12. How to use the Solubility Rules • If the compound is insoluble in water, it will not dissolve and will fall out as a solid precipitate. • If the compound is soluble in water, it will dissolve and form an aqueous solution.

  13. Solubility Rules • Most nitrate salts are soluble. • Most salts of Na+, K+, and NH4+ are soluble. • Most chloride salts are soluble; notable exceptions are Ag+, Pb2+, and Hg2 2+. • Most sulfate salts are soluble; notable exceptions are Ba2+, Pb2+, and Ca2+. • Most hydroxide compounds are mostly insoluble; the important exceptions are Na+ and K+ and Ba2+ and Ca2+ are mostly soluble. • Most sulfide, carbonate, and phosphate salts are mostly insoluble except Na+, K+, and NH4+. • Most dichromate salts are soluble except Ag+ and Pb+2.  * insoluble compounds will fall out of solutions as precipitates

More Related