In oxide X2O7 element X has the highest oxidation state. This element in a compound with hydrogen makes up 99.219%. What is this element?
Here's what I got.
The idea here is that for two atoms that are covalently bonded, oxidation numbers are assigned by assuming that the more electronegative of the two atoms "takes" all the bonding electrons shared by two atoms.
For a given element, the highest oxidation state occurs when all of its valence electrons are "taken" by the atoms to which it is covalently bonded.
In this case, element
#stackrel(color(blue)(?))("X")_ 2 stackrel(color(blue)(-2))("O")_ 7#
#2 xx color(blue)(?) + 7 xx (-2) = 0#
#color(blue)(?) = 14/2 = color(blue)(+7)#
Now, what this means is that your unknown element has
The first thing to do here is check the halogens by using the fact that element
Since halogens and hydrogen form compounds that have the general form
If you take
#(M_Mcolor(red)(cancel(color(black)("g mol"^(-1)))))/((1 xx M_M + 1 xx 1.00794) color(red)(cancel(color(black)("g mol"^(-1))))) xx 100 = 99.219%#
This will get you
#100 * M_M = 99.219 * M_M + 99.219 * 1.00794#
Rearrange to find
#0.781 * M_M = 100.0068 implies M_M = 100.0068/0.781 = 128.05#
This means that you element has a molar mass of
#M_("M I") = "126.9045 g mol"^(-1)#
So my guess would be that your unknown element is iodine, which would make your oxide
#"I"_2"O"_7 ->#diiodine heptoxide
The problem here is that this is a hypothetical compound, meaning that it doesn't really exist, at least as far as I know.
For example, dehydrating periodic acid,