Unit 7 Outline Chemical Reactions

KEY Unit 7 Outline– Chemical Reactions Study Guide (This is only a partial review- use your labs, book assignments, and worksheets too) 1. Given the following equations, determine if a physical change or chemical change has occurred & explain how you know: ESA!! a) CO2 (s) + H2O → H2CO3 (g) b) CO2 (s) → CO2 (g) Chemical- different substances in reactants and products Physical – Same substance in reactants and products, it just had a faze change. 2. Can you read a chemical equation? Identify the reactants, products & all the bolded symbols below: AgNO3 (aq) + Reactants MgBr2 (aq) 🡪 ESA!! AgBr (s) + __ Mg(NO3)2 Products (aq) = aqueous… means dissolved in water += combined with 🡪turns into/ produces (s) = solid 3. On the image, identify: a) the bonds that break during a chemical reaction & also name. _____ = strong bonds that break in chemical reactions and separate atoms from each other. Ex: water is broken into H & O b) the bonds that break during a physical reaction & also name. …. = hydrogen bonds that are weak, these break during physical changes When something changes from a solid to a liquid. Ex: water molecules break away from each other. ESA!! 4. Name Rule? (ex: 2 non-metals) Formula a. barium hydroxide metal + polyatomic ion b. trisulfur tetraoxide 2 nonmetals S3O4 c. diarsenic trisulfide 2 nonmetals As2S3 d. sodium carbonate metal + polyatomic ion e. ammonium sulfate both polyatomic ions f. Bromine g. Gold (I) phosphate Diatomic molecule Transition metal + polyatomic ion metal + polyatomic ion h. Barium Carbonate 5. Formula Total # of atoms Total number of ions Ba(OH)2 Na2CO3 (NH4)2SO4 BaCO3 Mg(NO3)2 9 3 Mg 2+ Charge on anion (NO3)-1 Al(OH)3 7 4 Al 3+ (OH)-1 6. What are 4 potential indicators of a chemical reaction? ● ● ● ● 2 liquids make a solid (precipitate) color change gas heat or light given off Charge on cation Br2 Au3PO4 Molar mass 148g/ mole (periodic table) 78 g/ mole 7. ESA!!Balance the following equations & ID the type of reaction: a. 2 CO + O2 🡪2 CO2 b. 2 Na + 2 H2O 🡪 2 NaOH + H2 Will the reaction occur? Why? synthesis Yes, always do Single Yes, Na is higher on activities series than H c. 2 AgNO3 + MgCl2 🡪 2 AgCl + Mg(NO3)2 double Yes, AgCl is solid d. 2P2O5 🡪 4 P + Decomp Yes, always do Combustion Yes, always do 5 O2 e. CH4 + 2 O2 🡪____ CO2 + 2 H2O 8. Chem. Reaction Type: a. What law in nature requires that chemical reactions be balanced? How does it work? The Law of conservation of matter/ mass. “What goes in must come out.” b. For: 2 Al(OH)3 What is the 2 called & why is it there? What is the 3 called & why is it there? ● 2 is a coefficient, these are written in order to balance and equation ● 3 is a subscript that is used to correctly write the formula. Swap and drop the charge of 3 from Al. 9. List the 7 diatomic elements & explain why they are diatomic. H2, N2, O2, I2, F2, Cl2, Br2… All these elements bond with themselves to make the octet rule instead of being a single, monoatomic atom like the noble gases and metals. 10. Write the correct formulas, state of matter, and equations, & balance: a. Aqueous iron (III) nitrate reacts with a solution of ammonium sulfate to yield aqueous ammonium nitrate and aqueous iron (III) sulfate. 2Fe(NO3)3 (aq) + 3(NH4)2SO4 🡪 6NH4 NO3 (aq) + Fe2(SO4)3 (aq) (double replacement) b. Solid mercury (I) oxide breaks down to form liquid mercury and oxygen gas. 2Hg2O (s) 🡪 4Hg (l) + O2 (g) (decomposition) 11. Complete the following chart. Reactants Predict the Products (make sure to balance equations) a. ___2_ Fe(NO3)3 + _3___ Pb 🡪 (Pb 2+ is most common) b. ___1_ C5H12 + __8__ O2 🡪 3Pb(NO3)2 + 2Fe c. __3_NaNO3 + _1__FeBr3 🡪 Fe(NO3)3 + 3 NaBr 6 H2O + 5 CO2 12. Based on the solubility chart, identify if the substances are a solid (precipitate) or aqueous: a. ZnCO3 b. K3PO4 c. Ca(OH)2 d. Al2(SO4)3 solid aq solid aq 13. Based on the activity series which element is more likely to replace the other in a compound? a. K and Na b. Al and Ni c. I and F