<p> Name: ______Date: ______Period: ______Page: _____</p><p>Nomenclature Review (Honors)</p><p>1. Classify the reaction. Predict the products. Balance the equation and write the order of coefficients. Assume all reactions occur</p><p>Type of Order of Predict the products Reaction Coefficients Single Chlorine + Potassium bromide  potassium chloride + bromine 1,2,2,1 Replacem Cl2 + KBr  KCl + Br2 ent K+ Br- K+ Cl- Cl & Br are diatomics</p><p>Double AgNO3 + KCl  AgCl + KNO3 1,1,1,1 Replacem + - + - ent Ag Cl K NO3 (+ and – cancel out)</p><p>Double HCl + NaOH  H2O + NaCl 1,1,1,1 Replacem H+ Cl- H+ OH- Na+ Cl- ent **when an acid and a hydroxide combine, one product will always be water</p><p>Combusti Methane (CH4) and oxygen  1,2,1,2 on CH4 + O2  CO2 + H2O</p><p>Carbon dioxide and water are the products of ALL combustion reactions Single Potassium metal reacts with barium chloride  2,1,2,1 Replacem K + BaCl2  KCl + Ba ent Ba2+ Cl- K+ Cl-</p><p>Single Magnesium reacts with iron(II) oxide  1,1,1,1 Replacem Mg + FeO  MgO + Fe ent Fe2+ O2- Mg2+ O2-</p><p>Double Sodium phosphate and calcium chloride react  2,3,6,1 Replacem Na3PO4 + CaCl2  NaCl + Ca3(PO4)2 + 3- 2+ - + - 2+ 3- ent Na PO4 Ca Cl Na Cl Ca PO4</p><p>2. Identify the reaction type for each of the following reactions.</p><p> a. 2Ba + O2  2BaO combination</p><p> b. 2H3PO4  P2O5 + 3H2O decomposition</p><p> c. 2Fe + 6HCl  2FeCl3 + 3H2 single replacement</p><p> d. CaO + CO2  CaCO3 combination 3. Write the correctly spelled name for each of the following.</p><p> a. NO2 nitrogen dioxide e. Al2S3 aluminum sulfide</p><p> b. NiI2 nickel(II) iodide f. Fe(NO3)3 iron(III) nitrate</p><p> c. N2O5 dinitrogen pentoxide g. Na3(PO4) sodium phosphate</p><p> d. SF6 sulfur hexafluoride h. CoCl3 cobalt(III) chloride Refer to the following set of equations to answer question43.</p><p>Ca + ZnCl2 → CaCl2 + Zn Ca > Zn Zn + MgCl2 → No Reaction Mg > Zn Mg + KCl → No Reaction K > Mg 2 K + CaCl2 → 2 KCl + Ca K > Ca Ca + MgCl2 → CaCl2 + Mg Ca > Mg</p><p>4. Place the metals in order of decreasing activity.</p><p>K, Ca, Mg, Zn</p><p>Refer to the following set of equations to answer question 5 & 6.</p><p>Cr + SrF2 → No Reaction Sr > Cr 3 Li + AlF3 → 3 LiF + Al Li > Al Sr + LiF → No Reaction Li > Sr</p><p>2 Al + 3 CrF2 → 2 AlF3 + 3 Cr Al > Cr 3Sr + 2AlCl3  3SrCl2 + 2Al Sr > Al</p><p>5. Place the metals in order of decreasing activity.</p><p>Li, Sr, Al, Cr</p><p>6. A strip of strontium is added to the solution containing a compound of each metal. Which of the metals would strontium replace? Aluminum & chromium</p><p>7. Why must a chemical equation be balanced? Matter cannot be created or destroyed. The same number of atoms of each element must appear on both sides of the reaction arrow. 8. Will all single replacement reactions occur? Explain. No. Only if the metal by itself is more reactive/higher on the activity series than the metal in the ionic compound. 9. Will all double replacement reactions occur? Explain. No. Only if both reactants are soluble and only one product is soluble in water.</p>