ࡱ> kmj%` *bjbj *\̟̟"(3338&4Dj4|7A244444555@@@@@@@$iBhD@55555@44@<<<5h44@<5@<<?@44 (358?B@tA07A?,E;E@E@,55<55555@@<d5557A5555D/33 Significant Figures Worksheet How many significant figures are in each of the following numbers? 1) 5.40 ____ 6) 1.2 x 103 ____ 2) 210 ____ 7) 0.00120 ____ 3) 801.5 ____ 8) 0.0102 ____ 4) 1,000 ____ 9) 9.010 x 10-6____ 5) 101.0100 ____ 10) 2,370.0 ____ Periodic Trends Worksheet 1) Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium. 2) Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. 4) Why does fluorine have a higher ionization energy than iodine? 5) Why do elements in the same family generally have similar properties? Review Naming Chemical Compounds Write the formulas for the following chemical compounds: 1) sodium bromide 2) calcium acetate 3) lithium cyanide 4) Tin (IV) sulfate 5) iron (III) phosphate 6) potassium nitride 7) acetic acid 8) strontium hypochlorite 9) zinc nitrite 10) vanadium (III) sulfide 11) molybdenum (II) bisulfate 12) nickel (III) sulfide 13) manganese (II) phosphate 14) silver acetate 15) cobalt (III) oxalate 16) magnesium sulfate 17) potassium carbonate 18) ammonium oxide 19) tin (IV) selenide 20) hydroiodic acid Lots of Ionic Naming Practice Problems Name the following ionic compounds: 1) NaBr __________________________________ 2) Sc(OH)3 __________________________________ 3) V2(SO4)3 __________________________________ 4) NH4F __________________________________ 5) CaCO3 __________________________________ 6) NiPO4 __________________________________ 7) Li2SO3 __________________________________ 8) Zn3P2 __________________________________ 9) Sr(C2H3O2)2 __________________________________ 10) Cu2O __________________________________ 11) Ag3PO4 __________________________________ 12) YClO3 __________________________________ 13) SnS2 __________________________________ 14) Ti(CN)4 __________________________________ 15) KMnO4 __________________________________ 16) Pb3N2 __________________________________ 17) CoCO3 __________________________________ 18) CdSO3 __________________________________ 19) Cu(NO2)2 __________________________________ 20) Fe(HCO3)2 __________________________________ Write the formulas for the following ionic compounds: 21) lithium acetate __________________________________ 22) iron (II) phosphate __________________________________ 23) titanium (II) selenide __________________________________ 24) calcium bromide __________________________________ 25) gallium chloride __________________________________ 26) sodium hydride __________________________________ 27) beryllium hydroxide __________________________________ 28) zinc carbonate __________________________________ 29) manganese (VII) arsenide __________________________________ 30) copper (II) chlorate __________________________________ 31) cobalt (III) chromate __________________________________ 32) ammonium oxide __________________________________ 33) potassium hydroxide __________________________________ 34) lead (IV) sulfate __________________________________ 35) silver cyanide __________________________________ 36) vanadium (V) nitride __________________________________ 37) strontium acetate __________________________________ 38) molybdenum sulfate __________________________________ 39) platinum (II) sulfide __________________________________ 40) ammonium sulfate __________________________________ Naming Ionic Compounds Practice Worksheet Name the following ionic compounds: 1) NH4Cl _____________________________________ 2) Fe(NO3)3 _____________________________________ 3) TiBr3 _____________________________________ 4) Cu3P _____________________________________ 5) SnSe2 _____________________________________ 6) GaAs _____________________________________ 7) Pb(SO4)2 _____________________________________ 8) Be(HCO3)2 _____________________________________ 9) Mn2(SO3)3 _____________________________________ 10) Al(CN)3 _____________________________________ Write the formulas for the following compounds: 11) chromium (VI) phosphate _____________________________________ 12) vanadium (IV) carbonate _____________________________________ 13) tin (II) nitrite _____________________________________ 14) cobalt (III) oxide _____________________________________ 15) titanium (II) acetate _____________________________________ 16) vanadium (V) sulfide _____________________________________ 17) chromium (III) hydroxide _____________________________________ 18) lithium iodide_____________________________________ 19) lead (II) nitride _____________________________________ 20 silver bromide _____________________________________ Balancing Equations Practice Worksheet Balance the following equations: 1) ___ NaNO3 + ___ PbO ( ___ Pb(NO3)2 + ___ Na2O 2) ___ AgI + ___ Fe2(CO3)3 ( ___ FeI3 + ___ Ag2CO3 3) ___ C2H4O2 + ___ O2 ( ___ CO2 + ___ H2O 4) ___ ZnSO4 + ___ Li2CO3 ( ___ ZnCO3 + ___ Li2SO4 5) ___ V2O5 + ___ CaS ( ___ CaO + ___ V2S5 6) ___ Mn(NO2)2 + ___ BeCl2 ( ___ Be(NO2)2 + ___ MnCl2 7) ___ AgBr + ___ GaPO4 ( ___ Ag3PO4 + ___ GaBr3 8) ___ H2SO4 + ___ B(OH)3 ( __ B2(SO4)3 + ___ H2O 9) ___ S8 + ___ O2 ( ___ SO2 10) ___ Fe + ___ AgNO3 ( ___ Fe(NO3)2 + ___ Ag Word Equations Worksheet Write the word equations for each of the following chemical reactions: 1) When dissolved beryllium chloride reacts with dissolved silver nitrate in water, aqueous beryllium nitrate and silver chloride powder are made. 2) When isopropanol (C3H8O) burns in oxygen, carbon dioxide, water, and heat are produced. 3) When dissolved sodium hydroxide reacts with sulfuric acid (H2SO4), aqueous sodium sulfate, water, and heat are formed. 4) When fluorine gas is put into contact with calcium metal at high temperatures, calcium fluoride powder is created in an exothermic reaction. 5) When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. Types of Reactions Worksheet Balance the following equations and indicate the type of reaction taking place: 1) ____ NaBr + ____ H3PO4 ( ____ Na3PO4 + ____ HBr Type of reaction: ____________________ 2) ____ Ca(OH)2 + ____ Al2(SO4)3 ( ____ CaSO4 + ____ Al(OH)3 Type of reaction: ____________________ 3) ____ Mg + ____ Fe2O3 ( ____ Fe + ____ MgO Type of reaction: ____________________ 4) ____ C2H4 + ____ O2 ( ____ CO2 + ____ H2O Type of reaction: ____________________ 5) ____ PbSO4 ( ____ PbSO3 + ____ O2 Type of reaction: ____________________ 6) ____ NH3 + ____ I2 ( ____ N2I6 + ____ H2 Type of reaction: ____________________ 7) ____ H2O + ____ SO3 ( ____ H2SO4 Type of reaction: ____________________ 8) ____ H2SO4 + ____ NH4OH ( ____ H2O + ____ (NH4)2SO4 Type of reaction: ____________________ Fun With Predicting Reaction Products Predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not: 1) ____ Ag2SO4 + ____ NaNO3 ( 2) ____ NaI + ____ CaSO4 ( 3) ____ HNO3 + ____ Ca(OH)2 ( 4) ____ CaCO3 ( 5) ____ AlCl3 + ____ (NH4)PO4 ( 6) ____ Pb + ____ Fe(NO3)3 ( 7) ____ C3H6 + ____ O2 ( 8) ____ Na + ____ CaSO4 ( Fun With Predicting Reaction Products Answers Predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not: Before moving on, here are some general rules of thumb for how to figure out what will be made (and if the reaction will occur at all): 1) If something that has carbon and hydrogen reacts with oxygen, its probably a combustion reaction. The products will be CO2 and H2O. 2) If two elements or very simple molecules combine with each other, its probably a synthesis reaction. The products will probably be predictable using the octet rule to find charges. 3) If one compound has an arrow coming off of it, its probably a decomposition reaction. The products will either be a couple of very simple molecules, or some elements, or both. 4) If a pure element reacts with another compound (usually, but not always, ionic), its probably a single displacement reaction. The products will be the compounds formed when the pure element switches places with another element in the other compound. Important note: these reactions will only occur if the pure element on the reactant side of the equation is higher on the activity series than the element it replaces. 5) If two ionic compounds combine, its probably a double displacement reaction. Switch the cations and balance out the charges to figure out what will be made. Important note: These reactions will only occur if both reactants are soluble in water and only one product is soluble in water. 6) If an acid and a base combine, its an acid-base reaction. 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