Science help? Gaining or losing electrons to become stable?

Question

These are the eletrons for some atoms. How many electrons will these atoms gain or lose to become stable?
rubidium(37)
argon(18)
sodium(11)
helium(2)
francium(87)
radon(86)
astatine(85)
bromine(35)
xanon(54)
neon(10)
lithium(3)
krypton(36)
cesium(55)
iodine(53)
boron(5)
chlorine(17)
flourine(9)
potassium(19)

any help would definately be appreciated, and please explain on how you found this out.

Answer 1

You need a periodic table of elements for this. Depending on the group that each element is in, you can find out how many electrons it gains or loses. If it is in the first group, it will lose 1 electron. second, group, 2 electrons. And so on. The line that divides nonmetals from metals (it's the diagonal line near the top right of the table) tells you whether it gains or loses. To the left of that loses, and to the right of the line gains electrons. The far right group stays the same. They are the Noble gases and are the most stable. Therefore in order to become stable, elements will either gain or lose electrons in order to have the same electron configuration. The atom will gain or lose depending on how much energy it takes to do so. It goes with the path that takes the least energy. This is what the line tells you, whether it is easier to lose electrons to become stable, or to gain electrons to become stable.

Answer 2

in case you look into the periodic table of aspects you will see that the two helium and neon are in the some distance splendid column, helium in the 1st row and neon in the 2nd row. This vertical column is composed of the inert aspects that have an fairly constrained ability to react chemically. Neither helium nor neon will easily combine with different aspects and there are no longer any prevalent compounds that incorporate the two helium or neon. the reason of this, as you stated on your question, is that the outer electron shells are complete. The electron shells denote potential tiers and the optimal form of electrons for each point is as follows: 1st = 2; 2d = 8; third = 18; 4th = 32. I’ll stop at this point because it’s no longer mandatory to bypass further for the reason. The atomic type for an element is the style of protons or the style of electrons in the independent state of an atom. Helium is atomic type 2 meaning it has purely 2 electrons. in view that potential point you will incorporate purely 2 electrons and helium has purely 2, that time is complete which might make helium virtually impossible to be reactive with the different element. As for neon, its atomic type is10 which might recommend it has 10 electrons in its shells. the 1st point has 2 and the 2nd point has 8 for a entire of 10. in view that its outer shell (point 2) has the optimal allowed (8), it like helium is extremely inert and virtually impossible to be reactive with any yet another element. consequently, by way of fact the outer shells (potential tiers) for the two aspects are complete, you could infer that neither helium nor neon will react with different aspects.

Answer 3

I would have done it but on second tought ............do your home work!!!!!!!!!!