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Suppose that a newly discovered element called centium has three isotopes that occur in nature. These are centium- 200 cenitum- 203 and centium- 209. Assume that the isotopes occur in equal amounts in?
If centium has three isotopes—centium-200, centium-203, and centium-209—occurring in equal amounts, the average atomic mass can be calculated by averaging the mass numbers of the isotopes. Since they are present in equal proportions, the average atomic mass would be (200 + 203 + 209) / 3 = 204. The average atomic mass of centium would therefore be approximately 204 atomic mass units (amu).
Why cant you add the average masses of each of the isotopes and divide to get overall average of the atoms?
Because the isotopes do not appear in equal amounts. This is hardly surprising since many isotopes experience radioactive decay and change to other elements after decay while stable isotopes persist - thus stable isotopes will usually dominate as the most common isotopes for individual elements with those with the longest half-lifes being more common than those with shorter half-lifes. Of course when you get into the heaviest elements there don't seem to be any stable isotopes so those with longest half life dominate.
Why is the average atomic mass included in the periodic table?
The average atomic mass is included in the periodic table because elements exist as a mix of isotopes with different atomic masses. The average atomic mass accounts for the abundance of each isotope in nature, providing a more accurate representation of the actual mass of an element in a given sample.
What would cause the average atomic mass to be close to a whole number?
The average atomic mass of an element is close to a whole number when the element has nearly equal amounts of its isotopes, with atomic masses that are close to whole numbers themselves. This occurs in elements with only one stable isotope or with stable isotopes that have similar abundances.
Why is the atomic mass of copper not exactly equal to 64 midway between the mass numbers of copper-63 and copper-65?
Because copper has isotopes. All Copper atoms have exactly the same number of protons, but not all of them have the same number of neutrons. The ones with different numbers of neutrons are known as isotopes. A given sample of Copper will contain various amounts of each of its isotopes. The atomic mass (weight) is an average weight, based on the percentages of the isotopes
Suppose that a newly discovered element called centium has three isotopes that occur in nature. These are centium- 200 cenitum- 203 and centium- 209. Assume that the isotopes occur in equal amounts in?
If centium has three isotopes—centium-200, centium-203, and centium-209—occurring in equal amounts, the average atomic mass can be calculated by averaging the mass numbers of the isotopes. Since they are present in equal proportions, the average atomic mass would be (200 + 203 + 209) / 3 = 204. The average atomic mass of centium would therefore be approximately 204 atomic mass units (amu).
What is the average mass of the mixture of an elements isotopes?
All of the isotopes in an element's atomic masses divided by the amount of isotopes there are is the weighted-average mass of the mixture of an elements isotopes.
Why cant you add the average masses of each of the isotopes and divide to get overall average of the atoms?
Because the isotopes do not appear in equal amounts. This is hardly surprising since many isotopes experience radioactive decay and change to other elements after decay while stable isotopes persist - thus stable isotopes will usually dominate as the most common isotopes for individual elements with those with the longest half-lifes being more common than those with shorter half-lifes. Of course when you get into the heaviest elements there don't seem to be any stable isotopes so those with longest half life dominate.
Why is the average atomic mass included in the periodic table?
The average atomic mass is included in the periodic table because elements exist as a mix of isotopes with different atomic masses. The average atomic mass accounts for the abundance of each isotope in nature, providing a more accurate representation of the actual mass of an element in a given sample.
What would cause the average atomic mass to be close to a whole number?
The average atomic mass of an element is close to a whole number when the element has nearly equal amounts of its isotopes, with atomic masses that are close to whole numbers themselves. This occurs in elements with only one stable isotope or with stable isotopes that have similar abundances.
What is weighted average mass of an element isotopes?
average atomis mass
What is the average of all the naturally occurring isotopes of a particular element?
The average of all the naturally occurring isotopes of a particular element are an element's atomic Mass.
Is the reason that an element's average atomic mas is often a decimal number stems from the fact that elements have isotopes?
Yes, the reason that an element's average atomic mass is often a decimal number is the fact that most elements have more than one isotope stable against radioactive decay and that these isotopes, each of which individually has an integral mass number, occur naturally in amounts that do not lead to integral average gram atomic masses.
What is the average mass of the isotope of an element?
the average mass numbers of the isotopes of an element
Why is the atomic mass of copper not exactly equal to 64 midway between the mass numbers of copper-63 and copper-65?
Because copper has isotopes. All Copper atoms have exactly the same number of protons, but not all of them have the same number of neutrons. The ones with different numbers of neutrons are known as isotopes. A given sample of Copper will contain various amounts of each of its isotopes. The atomic mass (weight) is an average weight, based on the percentages of the isotopes
Is an average mass of the different isotopes of the element?
The average atomic mass of an element is the weighted average of the masses of its isotopes, based on their abundance in nature. It is calculated by multiplying the mass of each isotope by its relative abundance, then summing these values together. This average mass is given on the periodic table.
What is an average of the masses of all the isotopes that occur in nature For an element?
The weighted average for all isotopes that occur in nature for an element is its atomic weight listed on the Periodic Table of the elements.
