Atomic Mass Isotopes Most elements found in nature occur as a mixture of isotope
ID: 912336 • Letter: A
Question
Atomic Mass Isotopes Most elements found in nature occur as a mixture of isotopes. The isotopic abundance can vary appreciably throughout the Universe, but here on Earth the abundance shows little variation from place to place. The most direct and accurate method for determining atomic masses and relative abundances is by a mass spectometer. The fraction of isotopic abundances is determined from the signal intensities reaching the detector of the mass spectrometer. Table 1 contains some selected isotopic abundance and atomic masses. Natural Abundance and Atomic Mass of Selected Isotopes. Critical Thinking Questions What element in Table 1 has the largest number of isotopes? Describe what all the isotopes of Neon have in common and how they are different. If you were to select one carbon atom at random, what would the mass of that atom most likely be in amu? What is the mass in amu of 100^12C atoms? Of 100^13C atoms? If you selected one hundred carbon atom at random, the total mass will be ___. 1200.0000 amu slightly more than 1200.0000 amu slightly less than 1200.0000 amu 1300.3355 amu slightly less than 1300.3355 amu Explain your reasoning.Explanation / Answer
1.Ne has three isotopes Ne-20 , Ne-21 and Ne-22.
2. Isotopes:
The atoms of an element with different mass number or atomic mass are called isotopes. They have same number of protons and electrons but different number of neutrons.
Hence Ne have same number of protons and electrons but different number of neutrons.
3.
Average atomic mass = (12.000000 amu)(0.9893) + (13.003355 amu)(0.0107)
= 11.8716+0.1391 amu
=12.0107 amu
4.
mass of 100 C-12 atoms in amu = 100* 12.00 amu
5.
mass of 100 C atoms in amu = 100* 12.0107 amu
= 1201.07 amu
measns slightly more than 1200.00 amu
= 1200 amu
mass of 100 C-13 atoms in amu = 100* 13.003355 amu
= 1300.3355 amu
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