The image contains two mass spectrometry graphs, each illustrating the relative abundance of various isotopes of an element.### Graph Analysis:#### Left Graph:- **Axes:** - Y-axis: Relative Abundance, ranging from 0 to 100. - X-axis: Mass-to-charge ratio (m/z), with values ranging from 0 to 12.- **Details:** - This graph shows several peaks, with a prominent peak around m/z = 12, indicating the most abundant isotope.#### Right Graph:- **Axes:** - Y-axis: Relative Abundance (%), ranging from 0 to 100. - X-axis: Mass-to-charge ratio (m/z), with values from 88 to 98.- **Details:** - This graph displays multiple peaks, with a notable peak at m/z = 90, suggesting the most prevalent isotope.### Educational Task:For each of the two Mass Spec Graphs:1. Determine the average atomic mass.2. Identify the element.3. Write the symbol for each isotope.4. Indicate the number of protons, electrons, and neutrons for each isotope.This exercise helps students understand how to interpret mass spectrometry data to identify elements and their isotopic composition.

1.) Average atomic mass is calculated using formula : Average Atomic mass : X1 M1 + X2 M2 + X3 M3 +…

100 100 relative abundance relative abundance (%) 50 50- 10 12 mlz 06 88 94 92 For each of the two Mass Spec Graphs above: 1. Determine the average atomic mass 2. Identify the element 3. Write the symbol for each isotope 4. Indicate the number of protons, electrons, and neutrons for each isotope

100 100 relative abundance relative abundance (%) 50 50- 10 12 mlz 06 88 94 92 For each of the two Mass Spec Graphs above: 1. Determine the average atomic mass 2. Identify the element 3. Write the symbol for each isotope 4. Indicate the number of protons, electrons, and neutrons for each isotope

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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An element has the following natural abundance and isotopic masses: 90.92% abundance with 19.99amu, 0.26% abundance with 20.99amu and 8.82% abundance with 21.99amu. Calculate the average atomic mass of this element.
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