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# Isotopes & AvgMass

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On the periodic table, the column to the far right is called the [...] gases.   On the periodic table, the column to the far right is called the noble gases.
Isotopes of the same element vary in the number of [...] they contain.   Isotopes of the same element vary in the number of neutrons they contain.
Some isotopes have unstable nuclei and radioactive; they are called [...].   Some isotopes have unstable nuclei and radioactive; they are called radioisotopes.
The mass of an atom is measured in [...] mass units (amu).   The mass of an atom is measured in atomic mass units (amu).
*Technically*, an atomic mass unit is 1/12th the mass of an atom of [...]... for practical purposes, it's the mass of one proton or neutron.   *Technically*, an atomic mass unit is 1/12th the mass of an atom of carbon-12... for practical purposes, it's the mass of one proton or neutron.
Not all isotopes are found in the same [...] in nature.   Not all isotopes are found in the same abundance in nature.
The periodic table gives us the [...]mass of all the atoms of each element instead of giving us the individual mass and abundance of each known isotope.   The periodic table gives us the average mass of all the atoms of each element instead of giving us the individual mass and aboundance of each known isotope.
If you know the masses and abundances (as a percent) of each isotope of an element, the average atomic mass is the sum of the [...] of each isotope.   If you know the masses and abundances (as a percent) of each isotope of an element, the average atomic mass is the sum of the mass times the abundance of each isotope.
The isotopes of an atom have the same number of [...] but different numbers of [...].   The isotopes of an atom have the same number of protons but different numbers of neutrons.
An [...] is a different form of the same atom of the element.   An isotope is a different form of the same atom of the element.
By definition, an atom of any element has a set number of [...].   By definition, an atom of any element has a set number of protons.
Each isotope has a different atomic [...], and each occurs in nature in a different [...].   Each isotope has a different atomic mass, and each occurs in nature in a different abundance.
*Technically*, an atomic mass unit is 1/12th the mass of an atom of carbon-12... for practical purposes, it's the mass of one [...] or [...].   *Technically*, an atomic mass unit is 1/12th the mass of an atom of carbon-12... for practical purposes, it's the mass of one proton or neutron.
If you know the masses and abundances (as a percent) of each isotope of an element, the average atomic mass is the [...] of the mass times the abundance of each isotope.   If you know the masses and abundances (as a percent) of each isotope of an element, the average atomic mass is the sum of the mass times the abundance of each isotope.
To find the average atomic mass of an element, just take the [...] for each isotope and [...] those numbers all together.   To find the average atomic mass of an element, just take the mass times abundance% for each isotope and add those numbers all together.
If an element has two isotopes ( 20% 5 amu; 80% 10 amu) how do you find it's average atomic mass?   average atomic mass = (0.2 * 5 amu) + (0.8 * 10 amu) = 1 amu + 8 amu = _9 amu_

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