2BSBS:
9. Active metals are more difficult to process and refine than less active metals because active metals tend to corrode more easily and are less durable.
10. We did not complete this lab.
11. Most metals exist in nature as minerals rather than pure metallic elements because the metals are found combined with other elements within more stable compounds which then can be refined to produce free metal.
12. A calcium metal with chromium (III) chloride is more likely to react together because calcium is is more reactive than chromium (III) chloride.
13. Zn2+ (aq) + 2 Ag(s) --> Zn(s) + 2 Ag+ (aq) is more likely to occur.
14. It is a poor idea to stir a solution of lead (II) nitrate with an iron spoon because lead is less reactive than iron.
15. Reduction is what chemists classify any chemical change in which a reactant can be considered to gain one or more electrons. Oxidation is when any reactant appears to lose one or more electrons. Oxidation-reduction occur together because whenever one reactant loses electrons, another reactant must gain them.
16. a. Au2+ + 2 e- --> Au
b. V --> V2+ + 2 e-
c. Cu2+ --> Cu + e-
17. a. Reduction reaction
b. Oxidation reaction
c. Reduction reaction
18. a. Zn2 + has been oxidized because it loses 2 electrons
b. Ni has been reduced gains 2 electrons
c. Zn
19. a. Al + Cr3+ ---> Al3 + Cr
b. Mn2+ + Mg ---> Mn + Mg2+
20. a. Al + Cr3 --> Al3 + Cr
b. Mn2 + Mg --> Mn + Mg2+
21. a. Electrometallurgy- using an electrical current to supply electrons to metal ions, thus reducing them. This process is used when no adequate chemical reducing agents are available or when a very high purity metal is sought
b. Pyrometallurgy- treating metals and their ores with heat. Carbon and carbon monoxide are common reducing agents
c. Hydrometallurgy- treating ores and other metal-containing materials with reactants in a water solution. Used to recover silver and gold from old mine tailings by a process called leaching
22. a. Magnesium- electrometallurgy
b. Lead- pyrometallurgy
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