This has to do with the reactivity series for metals (K,Na,Ca,Mg,Al,Zn,Fe,Pb,Cu,Au,Ag)

Which metal is most likely to undergo the conversion M(s)->M(n+)(aq)+ne-
What type of reaction is this?-oxidation ?

Which metal ion is most likely to undergo the conversion M(n+)(aq)+ne-
->M(s)
What type of reaction is this?- reduction ?

Which metal, from the list, is most likely to exist as metal ions rather than metal atoms?
Which metal, from the list, reacts with acids more slowly?

Please, please help!

Look up the activity series. This is not a complex concept but you need to be able to think it through. Some hints.

The metals at the top of the list are the most active and will displace any metal ion below it in the series. The metals at the bottom of the list are the least active and will not displace a metal ion above it in the series.
Two definitions will get you through all oxidation/reduction questions. Oxidation is the loss of electrons and reduction is the gain of electrons; LEO the lion goes GER
"Loss electrons oxidation" and "Gain electrons reduction" is a mnenomic that may help you remember. Now you have a try. Post again if you have trouble BUT tell us in detail what you don't understand.

To determine which metal is most likely to undergo the conversion M(s) -> M(n+)(aq) + ne-, we need to look at the reactivity series. In general, metals become more reactive as we go down the series. Therefore, metals higher up in the series are more likely to undergo oxidation.

Looking at the list, potassium (K) is at the top of the reactivity series. It is highly reactive and will readily lose an electron to form K+ ions. Therefore, potassium is the metal most likely to undergo the conversion M(s) -> M(n+)(aq) + ne-.

Regarding the type of reaction, this is an oxidation reaction. Oxidation refers to the loss of electrons from a species. In this case, the metal atom (M) loses electrons (ne-) to form metal ions (M(n+)(aq)).

Now, let's determine which metal ion is most likely to undergo the conversion M(n+)(aq) + ne- -> M(s). Again, we need to refer to the reactivity series. In general, metals become less reactive as we go down the series. Therefore, metals lower down in the series are more likely to undergo reduction.

Looking at the list, gold (Au) and silver (Ag) are at the bottom of the reactivity series. They are the least reactive metals. Therefore, they are most likely to undergo the conversion M(n+)(aq) + ne- -> M(s). In other words, gold and silver ions (Au(n+)(aq) and Ag(n+)(aq)) are more likely to gain electrons and be reduced to form their respective metal atoms (Au and Ag).

Regarding the type of reaction, this is a reduction reaction. Reduction refers to the gain of electrons by a species. In this case, the metal ion (M(n+)(aq)) gains electrons (ne-) to form the metal atom (M).

Now, let's identify the metal that is most likely to exist as metal ions rather than metal atoms. This can be determined by looking at the reactivity series. Generally, metals higher up in the reactivity series are more likely to exist as metal ions because they readily lose electrons.

Based on the list, potassium (K) is at the top of the reactivity series. As mentioned earlier, it is highly reactive and readily loses electrons to form K+ ions. Therefore, potassium is the metal most likely to exist as metal ions rather than metal atoms.

Lastly, let's identify the metal that reacts with acids more slowly. This can also be determined by referring to the reactivity series. Generally, metals lower down in the reactivity series react with acids more slowly because they are less reactive.

Based on the list, gold (Au) is at the bottom of the reactivity series, making it the least reactive metal. Therefore, gold would react with acids more slowly compared to the other metals listed.

I hope this explanation helps! Let me know if you have any further questions.