J2: Unit Study Guide/Chapter 8 Review Sheet/Solubility Chart

VOCABULARY/CONCEPTS

As mentioned in the unit outline, you must be able to define and apply your understanding of the following terms:

J1-1 / chemical reaction (8-1)
J1-2 / reactants, products (8-1)
J1-3 / chemical equation (8-1)
J1-4 / indications of a chemical reaction vs physical change (8-1)
J1-5 / word equation (8-1)
J1-6 / formula equation (8-1)
J1-7 / exothermic, endothermic (revisited, 8-1)
J1-8 / phase designations and other symbols used in chemical equations (8-1)
J2-1 / significance of a balanced chemical equation (8-2)
J2-2 / coefficients (8-2)
J2-3 / balanced equation (8-2)
J2-4 / conservation of mass (8-2)
J2-5 / procedures for balancing chemical equations (8-2)
J3-1 / combustion reactions (8-3)
J3-2 / synthesis reactions—reactions of elements or simpler compounds to form more complex species (8-3)
J3-3 / decomposition reactions through electrolysis (8-3)
J3-4 / decomposition through heating—metal carbonates, metal hydroxides, and metal chlorates (8-3)
J3-5 / decomposition of acids (8-3)
J4-1 / single displacement reactions—replacing a metal with another metal in a compound, replacement of hydrogen in water with a metal, replacement of hydrogen in an acid with a metal, replacement of halogens (8-3)
J4-2 / activity of an element—the activity series—determining if a hypothetical single displacement or synthesis reaction occurs (8-3, Table A-9, p 832)
J5-1 / double displacement reactions in aqueous solutions and requirements for them to occur (8-3)
J5-2 / solubility of cations in the presence of other ions—how to determine if a precipitate forms (class notes, solubility rules on p. 284)

It is likely that questions concerning vocabulary will take the form of multiple choice or matching questions.

  • You must be able to prove your ability to determine if an equation is balanced by showing all work leading to your conclusion. THIS MEANS THAT YOU MUST SHOW THE ATOM COUNTING METHOD THAT WE HAVE USED IN CLASS.
  • You must be able to balance any equation to conform to the Law of Conservation of Mass given the chemical formulas of the reactants and products. This will involve supplying coefficients when necessary while leaving subscripts unchanged.
  • You must be able to determine the type of reaction (synthesis/direct combination, decomposition/analysis, single replacement, double replacement) given the chemical formulas of the reactants and products.
  • Given the relative activities of elements, you should be able to determine if a single replacement reaction will take place.
  • You must show that you understand the conditions for a double replacement reaction to take place (formation of a gas, formation of water, formation of a precipitate) given solubility data and the understanding of which elements form diatomic gas molecules (for example, hydrogen, nitrogen, oxygen, fluorine, chlorine)
  • Given an interpretation or word equation and the naming compounds flow sheet, you should be able to write the formulas of reactants and products of an unbalanced equation.

Please turn over 

On a separate sheet of paper do the following for each reaction:

a)State whether the equation represents a synthesis (S), decomposition (D), single replacement (SR), or double replacement (DR) reaction.

b)Balance any reactions that need to be balanced.

c)If the equation represents a single or double replacement reaction, use the activity of elements chart on page 281 (SR reactions), the solubility rule on page 284, and the conditions that must be satisfied (DR reactions) to determine if a reaction will (or will not ) occur. State the reason for how you know. Remember that knowing whether a product substance is a solid, liquid, gas, or an aqueous solution is very important. Don’t forget to use your ion charge sheet or the chart on page 155 if you forget how to name the ions.

  1. CO(g) C + O2
  2. FeCl3 (aq) + AgNO3 (aq) Fe(NO3)3 + AgCl
  3. Al + Cl2 AlCl3
  4. BaCl2(aq) + NaOH(aq) NaCl + Ba(OH)2
  5. ZnSO4(aq) + Cu(s) Cu2SO4 + Zn
  6. CH4 C + H2
  7. Pb(NO3)2(aq) + Mg(s) Mg(NO3)2 + Pb
  8. MgCl2(aq) + H2(g) HCl + Mg
  9. H2SO4 H2 + S + O2
  10. O2 + N2 N2O4
  11. CaBr2(aq) + NaNO3(aq) Ca(NO3)2 + NaBr
  12. KI +Br2 KBr + I2
  13. C6H12O6 C + O2 + H2
  14. NaF  Na + F2
  15. Si + Cl2 SiCl4
  16. Na(C2H3O2)(aq) + Pb(NO3)2(aq) Pb(C2H3O2)2 + NaNO3
  17. NaI(aq) + Ca(s) CaI2 + Na
  18. H2 + CO + O2 H2CO3
  19. Li3PO4 Li + P + O2
  20. AlI3(aq) + Br2(l)AlBr3(aq) + I2(s)