Calculate the atomic mass of element "X" if it has 2 naturally occurring isotopes with the following masses and natural abundances. X−107 106.90509 amu 51.84%X−109 108.90476 amu 48.46%

Using my (not very precise) periodic table, I get the mass of Ag as 107.87

Explanation:

This must be a combination of these two isotopes. So the % of the other isotope must be 48.16%.

To work with these percentages in an equation I'll use them as decimals.

So now I can start putting them into an equation:

107.87  =  ( 106.905 ⋅ 0.5184 )  +  ( x ⋅ 0.4816 )  

Because both of the isotope masses, multiplied by their percentage, would give us the overall average mass.

107.87  =  55.419552  ⋅  (  x  ⋅  0.4816 )  

Worked out the brackets that we can work out, and then rearrange to give:

107.87  −  55.419552  =  (  x  ⋅  0.4816  )

Again rearrange:

52.450448 =  (  x  ⋅  0.4816  )  

And final rearranging:

x  =  52.450448  - 0.4816

x

=

108.909

(using same sig figs as given in question)

You probably want to work through that again using your periodic table value for Ag.

omg

I needed to hear that. Your so kind. Thank you!