c# barcode reader from image U STEP 4 Review the Knowledge You Need to Score High in Visual C#.NET

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70 U STEP 4 Review the Knowledge You Need to Score High
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Writing the equation in the ionic form shows clearly which species are really reacting + and which are not In the example above, Na and NO3 appear on both sides of the equation They do not react, but are simply there in order to maintain electrical neutrality of the solution Ions like this, which are not actually involved in the chemical reaction taking place, are called spectator ions The net ionic equation is written by dropping out the spectator ions and showing only those chemical species that are involved in the chemical reaction: Pb2+ ( aq ) + SO2 ( aq ) PbSO 4 ( s) 4 This net ionic equation focuses only on the substances that are actually involved in the 2+ reaction It indicates that an aqueous solution containing Pb (any solution, not just Pb(NO3)2(aq)) will react with any solution containing the sulfate ion to form insoluble lead(II) sulfate If this equation form is used, the spectator ions involved will not be known, but in most cases this is not a particular problem since the focus is really the general reaction, and not the specific one You will be expected to write the balanced net ionic equation for many of the reactions on the test
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Precipitation Reactions
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Precipitation reactions involve the formation of an insoluble compound, a precipitate, from the mixing of two soluble compounds Precipitation reactions normally occur in aqueous solution The example above that was used to illustrate molecular equations, ionic equations, etc, was a precipitation reaction A solid, lead(II) sulfate, was formed from the mixing of the two aqueous solutions In order to predict whether or not precipitation will occur if two solutions are mixed, you must:
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1 Learn to write the correct chemical formulas from the names; on the AP exam names are frequently given instead of formulas in the reaction section 2 Be able to write the reactants and products in their ionic form, as in the ionic equation example above Be sure, however, that you do not try to break apart molecular compounds such as most organic compounds, or insoluble species 3 Know and be able to apply the following solubility rules by combining the cation of one reactant with the anion of the other in the correct formula ratio, and determining the solubility of the proposed product Then do the same thing for the other anion/cation combination 4 On the AP exam, you will be expected to explain why a substance is soluble/insoluble Simply quoting the solubility rule is not sufficient Learn the following solubility rules: Salts containing the following ions are normally soluble:
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+ All salts of Group IA (Li+, Na+, etc) and the ammonium ion (NH4 ) are soluble All salts containing nitrate (NO3 ), acetate (CH3COO ), and perchlorates (ClO4 ) are soluble All chlorides (Cl ), bromides (Br ), and iodides (I ) are soluble, except those of Cu+, Ag+, 2+ 2+ Pb , and Hg2 All salts containing sulfate (SO42 ) are soluble, except those of Pb2+, Ca2+, Sr2+, and Ba2+
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Reactions and Periodicity 71
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Salts containing the following ions are normally insoluble:
G G G
2 3 Most carbonates (CO3 ) and phosphates (PO4 ) are insoluble, except those of Group IA and the ammonium ion Most sulfides (S2 ) are insoluble, except those of Group IA and IIA and the ammonium ion Most hydroxides (OH ) are insoluble, except those of Group IA, calcium, and barium Most oxides (O2 ) are insoluble, except for those of Group IA, and Group IIA which react with water to form the corresponding soluble hydroxides
Let s see how one might apply these rules Suppose a solution of lead(II) nitrate is mixed with a solution of sodium iodide Predict what will happen Write the formulas: Pb(NO3 )2 (aq ) + NaI(aq ) Convert to the ionic form:
Pb2+ ( aq ) + 2NO3 (aq ) + Na + (aq ) + I (aq )
Predict the possible products by combining the cation of one reactant with the anion of the other and vice versa: PbI2 + NaNO3 Apply the solubility rules to the two possible products: PbI2(s) NaNO3(aq) Insoluble, therefore a precipitate will form Soluble, no precipitate will form
Complete the chemical equation and balance it: Pb(NO3 )2 (aq ) + 2NaI(aq ) PbI2 ( s) + 2NaNO3 (aq ) Pb2+ (aq ) + 2I (aq ) PbI2 ( s) If both possible products are soluble, then the reaction would be listed as NR (No Reaction) In the reaction question part of the AP exam, there will be a possible reaction for every part of the question If at least one insoluble product is formed, the reaction is sometimes classified as a double displacement (replacement) or metathesis reaction
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