practice: predicting products of chemical reactions\nuse your knowledge of the types of chemical reactions…

practice: predicting products of chemical reactions\nuse your knowledge of the types of chemical reactions and of bond formation in compounds to complete each reaction below. after, balance the equation if needed. show all work for balancing on a separate sheet of paper. place coefficient final answers in the blanks provided. you can leave coefficients of \1\ blank.\npart 1: synthesis reactions\n1. ___ na + ___ o₂ →\n2. ___ mg + ___ f₂ →\n3. ___ na + ___ cl₂ →\n4. ___ al + ___ s →\n5. ___ ca + ___ p →\npart 2: decomposition reactions (hint: oxygen is always o₂ on its own, and metals tend to stand alone.)\n6. ___ hgo →\n7. ___ al₂o₃ →\npart 3: single replacement reactions (hint: like elements always switch!)\n8. ___ al + ___ niso₄ →\n9. ___ f₂ + ___ nacl →\npart 4: double replacement reactions\n10. ___ koh + ___ nacl →\n11. ___ bacl₂ + ___ na₃po₄ →\n12. ___ agno₃ + ___ cacl₂ →\npart 5: combustion reactions\n13. ___ ch₄ + ___ o₂ →\n14. ___ c₂h₂ + ___ o₂ →

practice: predicting products of chemical reactions\nuse your knowledge of the types of chemical reactions and of bond formation in compounds to complete each reaction below. after, balance the equation if needed. show all work for balancing on a separate sheet of paper. place coefficient final answers in the blanks provided. you can leave coefficients of \1\ blank.\npart 1: synthesis reactions\n1. ___ na + ___ o₂ →\n2. ___ mg + ___ f₂ →\n3. ___ na + ___ cl₂ →\n4. ___ al + ___ s →\n5. ___ ca + ___ p →\npart 2: decomposition reactions (hint: oxygen is always o₂ on its own, and metals tend to stand alone.)\n6. ___ hgo →\n7. ___ al₂o₃ →\npart 3: single replacement reactions (hint: like elements always switch!)\n8. ___ al + ___ niso₄ →\n9. ___ f₂ + ___ nacl →\npart 4: double replacement reactions\n10. ___ koh + ___ nacl →\n11. ___ bacl₂ + ___ na₃po₄ →\n12. ___ agno₃ + ___ cacl₂ →\npart 5: combustion reactions\n13. ___ ch₄ + ___ o₂ →\n14. ___ c₂h₂ + ___ o₂ →

Answer

Explanation:

Step1: Identify synthesis reaction rules

Synthesis reactions combine elements to form compounds. For metal - non - metal reactions, we form ionic compounds.

  1. (4Na+O_2\rightarrow2Na_2O)
  2. (Mg + F_2\rightarrow MgF_2)
  3. (2Na+Cl_2\rightarrow2NaCl)
  4. (2Al + 3S\rightarrow Al_2S_3)
  5. (3Ca+2P\rightarrow Ca_3P_2)

Step2: Identify decomposition reaction rules

Decomposition reactions break a compound into its elements or simpler compounds. 6. (2HgO\rightarrow2Hg + O_2) 7. (2Al_2O_3\rightarrow4Al+3O_2)

Step3: Identify single - replacement reaction rules

In single - replacement reactions, a more reactive element replaces a less reactive element in a compound. 8. (2Al + 3NiSO_4\rightarrow Al_2(SO_4)_3+3Ni) 9. (F_2 + 2NaCl\rightarrow2NaF+Cl_2)

Step4: Identify double - replacement reaction rules

In double - replacement reactions, the cations and anions of two compounds switch places. 10. (KOH+NaCl\rightarrow KCl + NaOH) (no precipitate, gas or water formed, so it's often considered no reaction in practice) 11. (3BaCl_2+2Na_3PO_4\rightarrow Ba_3(PO_4)_2\downarrow + 6NaCl) 12. (2AgNO_3+CaCl_2\rightarrow2AgCl\downarrow+Ca(NO_3)_2)

Step5: Identify combustion reaction rules

Hydrocarbon combustion reactions produce carbon dioxide and water. 13. (CH_4 + 2O_2\rightarrow CO_2+2H_2O) 14. (2C_2H_2+5O_2\rightarrow4CO_2 + 2H_2O)

Answer:

  1. (4Na+O_2\rightarrow2Na_2O)
  2. (Mg + F_2\rightarrow MgF_2)
  3. (2Na+Cl_2\rightarrow2NaCl)
  4. (2Al + 3S\rightarrow Al_2S_3)
  5. (3Ca+2P\rightarrow Ca_3P_2)
  6. (2HgO\rightarrow2Hg + O_2)
  7. (2Al_2O_3\rightarrow4Al+3O_2)
  8. (2Al + 3NiSO_4\rightarrow Al_2(SO_4)_3+3Ni)
  9. (F_2 + 2NaCl\rightarrow2NaF+Cl_2)
  10. (KOH+NaCl\rightarrow KCl + NaOH) (no real - world reaction in most cases)
  11. (3BaCl_2+2Na_3PO_4\rightarrow Ba_3(PO_4)_2\downarrow + 6NaCl)
  12. (2AgNO_3+CaCl_2\rightarrow2AgCl\downarrow+Ca(NO_3)_2)
  13. (CH_4 + 2O_2\rightarrow CO_2+2H_2O)
  14. (2C_2H_2+5O_2\rightarrow4CO_2 + 2H_2O)