How did I get the percentage abundance of
And it is likely that we got the element neon. How did I know this?
The atomic mass is the weighted average of the atomic masses of each isotope. In a weighted average, we multiply each value by a number representing its relative importance. In...
1 Answers 1 viewsThe idea here is that each isotope will contribute to the average of the element proportionally to their respective abundance. Now, the key to this problem lies in how you...
1 Answers 1 views$""^63Cu$ has $69.2%$ abundance. $""^65Cu$ has $30.8%$ abundance. So, the weighted average is $62.93xx69.2%$ $+$ $64.93xx30.8%$ $=$ $63.55$ $"amu"$. If we look at , copper metal (a mixture of isotopes...
1 Answers 1 viewsThe average of an element is determined by taking the weighted average of the atomic masses of its naturally occurring . Now, weighted average simply means that each...
1 Answers 1 viewsMultiply the percentage (in decimal form) of each isotope times its mass in amus and add. $"Atomic weight"=(0.81xx99"amu")+(0.19xx114"amu")="101.85 amu"$
1 Answers 1 viewsThe weighted average is the sum of each individual nuclide, multiplied by its isotopic abundance. So, we simply do the arithmetic: $0.7577xx34.969+0.2423xx36.966 = ???$ amu Then look at to...
1 Answers 1 viewsNow I hope you have been exposed to the concept of weighted average; If not here is a video Now lets get our data; Lets call our element...
1 Answers 1 viewsThe $"Average Atomic Mass"$ of an element is defined as "the weighted average mass of all naturally-occurring (occasionally radioactive) of the element." (and hence the name "average") [1] Dividing the...
1 Answers 1 viewsAnd thus the $"weighted average"$ is: $(62.93xx69.2%+64.93xx30.8%)*"amu"$ $=$ $63.55$ $"amu"$
1 Answers 1 viewsThe is the weighted average of the individual isotopic masses: $(23.99xx78.99%+24.99xx10.00%+25.98xx11.01%)*g=24.31*g$ I have given you answer in $g$ which here is equivalent to $"amu"$.
1 Answers 1 views