Homework #4 week one semester two

1. Active metals are more difficult to process because they react to readily with other elements and are very unstable in their pure forms. Less active metals do not readily share electrons with other elements making them easier to process and keep in their pure forms.
2. The metals involved int the investigation that were the easiest to process where silver and copper because they are both less reactive than any of the other metals used in the experiment and do not readily share electrons making them harder to oxidize.
3. Most metals exist in nature as minerals rather than as pure metallic elements because most metals react readily with other substances in order to stabilize themselves; in nature most metals are too unstable in their pure form.
4. The reaction that is most likely to occur is chromium metal with calcium chloride because calcium is more likely to combine and share its electrons with chloride because it is more reactive then chromium.
5. The equation that is most likely to occur is 2Ag⁺ + Zn to 2Ag + Zn ²⁺ because zinc is more reactive then silver and therefore will readily lose 2 electrons to silver, which is less reactive.
6. It would be a poor idea to stir a solution of lead(II)  nitrate with an iron spoon because Iron is more reactive and will lose electrons to the lead nitrate; therefore, the solution will become an iron lead nitrate solution rather than just a lead nitrate solution.
1. PbN ²⁺+ Fe to Fe²⁺ PbN
7. Define”
1. Oxidation- losing electrons to another element and becoming a positive ion
2. Reduction- stabilizing by gaining two electrons from another element.
8. Au³⁺ + 3e^- to become Au.
1. Iv – 1e^- to become Iv⁺
2. Cu⁺- 1e^_ to become Cu²⁺
9. A.  is a reduction
1. Is an oxidation
2. Is an reduction
10. The reactant that has been oxidized is Zn because it became an ion by losing two of its electrons to Ni.
1. The reactant that has been reduced is the Ni because it became the  pure metal by gaining two electrons from Zn.
2. The reducing agent is Zn because it provides the electrons.
11. After considering equation:
1. The reactant that has been oxidized is K because it loses an electron to Hg.
2. The reactant that has been reduced is Hg because it gained an electron from K in order to make it stable.
3. The oxidizing agent in this reaction is Hg because it gains electrons.
12. Al + Cr³⁺ becomes Al³⁺ + Cr
1. Mn²⁺ +Mg becomes Mg²⁺ + Mn
13. How each of the following processes converts metal cations to metal atoms:
1. Electrometallurgy- A process that converts metal cations to metal atoms through an electric current that is shot through it.
2. Pyrometallurgy- the process in which the metal cations are heated until they become metal atoms.
3. Hydrometallurgy- The process where the metal cations are suspended in a water solution with different other substances in it in order to make the cations gain electrons to make them metal atoms.
14. The process that would be most useful in obtaining the following elements from theier metal ores are:
1. Magnesium- electrometallurgy
2. Lead- pyrometallurgy