Question

Naturally occurring tellurium (Te) has the following isotopic abundances:

Isotope	Abundance	Mass(u)
${}^{120}\mathrm{Te}$	0.09%	119.90
${}^{122}\mathrm{Te}$	2.46%	121.90
${}^{123}\mathrm{Te}$	0.87%	122.90
${}^{124}\mathrm{Te}$	4.61%	123.90
${}^{125}\mathrm{Te}$	6.99%	124.90
${}^{126}\mathrm{Te}$	18.71%	125.90
${}^{128}\mathrm{Te}$	31.79%	127.90
${}^{130}\mathrm{Te}$	34.48%	129.91

Draw the mass spectrum of ${\mathbf{H}}_{\mathbf{2}}\mathbf{Te}$ , assuming that the only hydrogen isotope present is ${}^{\mathbf{1}}\mathbf{H}$ (mass 1.008).

Short answer

The mass spectrum is:

Step-by-step solution

The most abundant isotope

The most abundant ion has an intensity of 100% in the mass spectrum. So, to get the intensities of all other ions, multiply the abundance ion intensity with a common factor.

Calculation of mass spectrum

The multiplication of the abundance ion with a common factor:

$$\begin{gathered} {\mathrm{H}}_2{}^{122}\mathrm{Te}=7.135\% \\ {\mathrm{H}}_2{}^{123}\mathrm{Te}=2.52\% \\ {\mathrm{H}}_2{}^{124}\mathrm{Te}=13.37\% \\ {\mathrm{H}}_2{}^{125}\mathrm{Te}=20.27\% \\ {\mathrm{H}}_2{}^{126}\mathrm{Te}=54.26\% \\ {\mathrm{H}}_2{}^{128}\mathrm{Te}=92.2\% \\ {\mathrm{H}}_2{}^{130}\mathrm{Te}=100\% \end{gathered}$$

Mass spectrum figure

Mass spectrum figure