In relative oxidizing and reducing agents table ;

1) Is Al oxidized by Ni+2
2) Is Cu oxidized by Ag+
3) Is Pb oxidized by Na+
4) Is F2 reduced by Cl-
5) Is Br2 reduced by Cl-
and if you or no , how it is as a rule to predict any ?

thank you

You look at the activity series. Here is one on the web.

http://www.cod.edu/people/faculty/jarman/richenda/1551_hons_materials/Activity%20series.htm

Any metal will displace any ion BELOW it in the activity series.
So Al(s) + Ni^2+(aq) ==> Ni(s) + Al^3+(aq) then balance it; 2Al + 3Ni^2+ ==> ?

Cu(s) + Ag^+(aq) ==> Cu^2+(aq) + Ag(s) and balance it.

But Pb(s) + Na^+ ==> no reaction because Pb is BELOW Na^+
+ Ag^+

To determine if a specific reaction will occur, whether it involves oxidation or reduction, you can apply the "activity series" or "electrochemical series" table. This table is a list of metals and non-metals, ordered based on their tendency to undergo oxidation or reduction.

For the given reactions, let's determine the possibility of oxidation or reduction:

1) Al oxidized by Ni+2: To determine if Al will be oxidized by Ni+2, we can look at the activity series. If Ni is higher than Al in the series, then the reaction may occur. However, if Al is higher in the series than Ni, the reaction is not likely to occur.
- If the activity series shows Ni below Al, that means Al is more easily oxidized and Ni cannot oxidize it. Therefore, Al is not oxidized by Ni+2.

2) Cu oxidized by Ag+: Similarly, we need to compare Cu and Ag in the activity series. If Ag is above Cu in the series, then Cu can be oxidized by Ag+.
- If the activity series shows Ag above Cu, that means Cu can be oxidized by Ag+. Therefore, Cu is oxidized by Ag+.

3) Pb oxidized by Na+: Again, we compare Pb and Na in the activity series. If Na is above Pb, then Pb can be oxidized by Na+.
- If the activity series shows Na below Pb, that means Pb is more easily oxidized and Na cannot oxidize it. Therefore, Pb is not oxidized by Na+.

4) F2 reduced by Cl-: Here, we are looking at the reduction potential of F2 by Cl-. If the reduction potential of Cl- is higher than that of F2, then F2 can be reduced by Cl-.
- Unfortunately, the activity series only considers metals, not halogens like F2 and Cl-. So, we cannot determine if F2 is reduced by Cl- using the activity series alone.

5) Br2 reduced by Cl-: Again, we need to compare the reduction potentials of Br2 and Cl-. If the reduction potential of Cl- is higher than that of Br2, then Br2 can be reduced by Cl-.
- Unfortunately, the activity series only considers metals, not halogens like Br2 and Cl-. So, we cannot determine if Br2 is reduced by Cl- using the activity series alone.

In summary, to predict the likelihood of oxidation or reduction, you can compare the elements involved in the reaction using the activity series. However, for non-metals or halogens, the activity series is not applicable, and you may need additional information or other methods to determine if the reaction will occur.