A hypothetical element has three main iso- topes with mass numbers of 81, 83, and 84. If 17.00% of the isotopes have a mass number of 81 amu and 35.00% of the isotopes have a mass of 83 amu, what atomic weight should be listed on the periodic table for this element?
17% is h1
35% is 83
Then 48% is 84
(0.17)*81 + (0.35)*83 + (0.48)*84 = ?
To calculate the atomic weight of the element, we need to consider the relative abundance of each isotope.
Let's assume that the remaining percentage, 100% - (17% + 35%), is the abundance of the isotope with a mass number of 84 amu.
Abundance of isotope with mass number 81 amu = 17.00% = 0.17
Abundance of isotope with mass number 83 amu = 35.00% = 0.35
Abundance of isotope with mass number 84 amu = Remaining percentage = 100% - (17% + 35%) = 48.00% = 0.48
To calculate the atomic weight, we multiply the mass of each isotope by its relative abundance and then sum them up:
Atomic Weight = (Mass of isotope 1 × Relative abundance 1) + (Mass of isotope 2 × Relative abundance 2) + (Mass of isotope 3 × Relative abundance 3)
Assuming the mass of the isotope with a mass number of 81 amu is 81 amu, the mass of the isotope with a mass number of 83 amu is 83 amu, and the mass of the isotope with a mass number of 84 amu is 84 amu:
Atomic Weight = (81 amu × 0.17) + (83 amu × 0.35) + (84 amu × 0.48)
Atomic Weight = 13.77 + 29.05 + 40.32
Therefore, the atomic weight that should be listed on the periodic table for this element is approximately 83.14 amu.
To calculate the atomic weight of the element, we need to take into account the abundance of each isotope. The atomic weight is a weighted average of the masses of each isotope, where the abundance is the proportion or percentage of each isotope in the element.
Let's break down the information provided in the question:
1. Isotope 1: Mass Number = 81 amu, Abundance = 17.00%
2. Isotope 2: Mass Number = 83 amu, Abundance = 35.00%
3. Isotope 3: Mass Number = 84 amu
Since the question doesn't explicitly provide the abundance of Isotope 3, we can assume that the remaining 48% (100% - 17% - 35%) is the abundance for Isotope 3.
Now, let's calculate the atomic weight:
Atomic weight = (Mass1 x Abundance1) + (Mass2 x Abundance2) + (Mass3 x Abundance3)
Atomic weight = (81 amu x 17.00%) + (83 amu x 35.00%) + (84 amu x 48%)
Calculating this expression will give us the atomic weight of the element.