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Rank the following elements in order from least to most number of moles of atoms in a 10.0 g sample: Sn, Si, Se, S

, , , .

Explanation:

The relative atomic mass of an element is numerically equal to the mass (in grams) of one mole of its atoms. This quantity can help estimate the number of moles of atoms in each of these four samples.  

Look up the relative atomic mass for each of these four elements (on a modern periodic table.)

: .: .: .: .

The relative atomic mass of is (approximately) . Therefore, the each mole of silicon atoms would have a mass of approximately . How many moles of silicon atoms would there be in a sample?

Given:

. .

Number of mole of silicon atoms in the sample: .

Similarly:

.

.

.

Therefore, among these samples:

.

It is not a coincidence that among these four samples, the one with the fewest number of atoms corresponds to the element with the largest relative atomic mass.

Consider two elements, with molar mass and each. Assume that moles and moles of atoms of each element were selected, such that the mass of both samples is . That is:

.

.

Equate the right-hand side of these two equations:

.

.

In other words, the number of moles atoms in two equal-mass samples of two elements is inversely proportional to the molar mass of the two elements (and hence inversely proportional to the formula mass of the two elements.) That explains why in this question, the sample containing the smallest number of atoms corresponds to element with the largest relative atomic mass among those four elements.

Ido not understand. 

(no3)⁻n has oxidation number x,o has oxidation number -2.(x*1 -2*3) charge of the nitrate ion, and we know that charge of the nitrate ion =-1.so,(x*1 -2*3) =-1x-6=-1x=+5answer a. +5.