Question detail
In a mass spectrum, an element shows a peak at m/z = 16 with a relative intensity of 100% and another peak at m/z = 18 with a relative intensity of 50%. What can be inferred about the isotopes of this element?
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At a glance
Question
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Topic
Atomic structure
Question
In a mass spectrum, an element shows a peak at m/z = 16 with a relative intensity of 100% and another peak at m/z = 18 with a relative intensity of 50%. What can be inferred about the isotopes of this element?
Answer
The presence of peaks at m/z = 16 and m/z = 18 suggests that the element has two isotopes. The isotope with m/z = 16 is the most abundant, while the one with m/z = 18 is less common, indicating it has two additional neutrons.
Explanation
The evidence indicates that the peak at m/z = 16 is the most abundant isotope, while the peak at m/z = 18 represents a less common isotope. This implies that the element has isotopes with different neutron counts, affecting their mass numbers. Consequently, the conclusion is that the element has isotopes with mass numbers 16 and 18, with the former being more prevalent.
Common mistake
Misunderstanding Mass Spectra Peaks
Students often misinterpret the peaks in a mass spectrum, thinking that each peak represents a different element rather than different isotopes of the same element.
To correct this, students should focus on understanding that each peak corresponds to isotopes of the same element, with the height of the peak indicating the relative abundance of each isotope.
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