QUESTION The mass spectra of sulfur is shown to the right. Each of their relative abundances (i.e.,each peak height) is measured and tabulated as shown. Using the peak height data given, calculate the abundance of each sulfur isotope in the unit of %. Using the isotopic abundances you will obtain, calculate the atomic mass of Sulfur (i.e., the average atomic mass). Hint: If you are not sure how to calculate the atomic mass of sulfur, refer to the previous Questions so far. DATA Isotope Peak height, cm 325 50.00 335 0.40 345 2.30 365 0.10 32 33 34 36 MASS, amu Copyright © All Rights Reserved by M.Han The abundance of 32s is %. The abundance of 33s is %. The abundance of 34s is %. The abundance of 36s is %. The atomic mass of sulfur is amu. Relative Abundance

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Can you give me explanations and only last two question

True or False...and why? a.) If you change number of protons, you have isotopes of an element b.) If you change number of neutrons, ions are created c.) If you change number of electrons, you have a different element

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I'm sturggling on the last question part c. I submitted what I though was correct (36 on top and  78 on bottom with the symbol Kr) if that makes sense. I was wondering if you could help me. Thank you. I have 10 attemps and already used 3 because I miss read the question at first and only submitted symbols instead of the atomic number and mass number as well like you see on a periodic table.

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Mendeleev left empty spaces in his periodic table for elements he suspected existed but had yet to be discovered. He left no spaces for the Noble gases that we now have in the modern periodic table.  Give at least two reasons on why this group was challenging to discover, based on what we now know about the atom including sub-atomic particles. Mendeleev had a group VIII but they are NOT the noble gases.