Question

1. Does the sample contain identical atoms of copper? No, the sample contains both 63Cu and 65Cu 2. Use the picture above to determine the percent of 63Cu in the sample. What is the percent of 65Cu? 63Cu = 14/20 = 70% 65Cu = 6/20 = 30% 3. a) What is the average atomic mass of copper on the periodic table? 63.546 u b) Is it closer to 63 amu or 65 amu? It is closer to 63 amu. c) How does the information from the picture above explain the answer to the previous question? There are more coppers with 63 amu, so it makes sence that the atomic mass would be closer to 63 than 65. It is an average between the two, with 63 being the majority. 4. Consider the data given in the table below. Determine the average mass of an element based on the isotopic abundance and the mass of each isotope Isotope % Abundance 20Ne 90.48 21Ne 0.27 22Ne 9.25

          1. Does the sample contain identical atoms of copper?
No, the sample contains both 63Cu and 65Cu
2. Use the picture above to determine the percent of 63Cu in the sample. What is the percent of 65Cu?
63Cu = 14/20 = 70%
65Cu = 6/20 = 30%
3. a) What is the average atomic mass of copper on the periodic table?
63.546 u
b) Is it closer to 63 amu or 65 amu?
It is closer to 63 amu.
c) How does the information from the picture above explain the answer to the previous question?
There are more coppers with 63 amu, so it makes sence that the atomic mass would be closer to 63 than 65. It is an average between the two, with 63 being the majority.
4. Consider the data given in the table below. Determine the average mass of an element based on the isotopic abundance and the mass of each isotope
Isotope % Abundance
20Ne 90.48
21Ne 0.27
22Ne 9.25

1. Does the sample contain identical atoms of copper?
No, the sample contains both 63Cu and 65Cu
2. Use the picture above to determine the percent of 63Cu in the sample. What is the percent of 65Cu?
63Cu = 14/20 = 70%
65Cu = 6/20 = 30%
3. a) What is the average atomic mass of copper on the periodic table?
63.546 u
b) Is it closer to 63 amu or 65 amu?
It is closer to 63 amu.
c) How does the information from the picture above explain the answer to the previous question?
There are more coppers with 63 amu, so it makes sence that the atomic mass would be closer to 63 than 65. It is an average between the two, with 63 being the majority.
4. Consider the data given in the table below. Determine the average mass of an element based on the isotopic abundance and the mass of each isotope
Isotope % Abundance
20Ne 90.48
21Ne 0.27
22Ne 9.25

Added by Gina F.

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