![]() Average atomic weight for boron in the periodic table is a)10.8b)10.2c)11.2d)10.0Correct answer is option 'A'. Besides giving the explanation ofīoron has two stable isotopes, 10B (19%) and 11B (81%). Can you explain this answer? defined & explained in the simplest way possible. Here you can find the meaning of Boron has two stable isotopes, 10B (19%) and 11B (81%). Therefore, the correct answer is option 'A' (10.8). ![]() Rounding to the nearest whole number, the average atomic weight of boron is approximately 11. Now we can substitute this value into the equation for the atomic weight of 10B:Ītomic Weight of 10B = (1990 - (0.81 * 0)) / 0.19 Therefore, the atomic weight of 11B is 0. Since the atomic weight of an isotope is the sum of the number of protons and neutrons, we can set up the following equation: We can do this by setting up a system of equations. To find the atomic weight of 10B, we need to solve for x. We can now substitute the atomic weight of 11B, which is not given, with the variable x:Ītomic Weight of 10B = (1990 - (0.81 * x)) / 0.19 We can rearrange the equation to solve for the Atomic Weight of 10B:Ītomic Weight of 10B = (Average Atomic Weight - (0.81 * Atomic Weight of 11B)) / 0.19Ītomic Weight of 10B = (1990 - (0.81 * Atomic Weight of 11B)) / 0.19 To calculate the average atomic weight, we can use the following formula:Īverage Atomic Weight = (Abundance of Isotope 1 * Atomic Weight of Isotope 1) + (Abundance of Isotope 2 * Atomic Weight of Isotope 2)Īverage Atomic Weight = (0.19 * Atomic Weight of 10B) + (0.81 * Atomic Weight of 11B) The abundance of 10B is given as 19% and the abundance of 11B is given as 81%. In this case, boron has two stable isotopes: 10B and 11B. The average atomic weight of an element is calculated by taking into account the abundance of each isotope and its respective atomic weight.
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