answersLogoWhite

Top Answer
User Avatar
Wiki User
Answered 2008-05-06 17:55:53

Carbone / 12

001
๐Ÿ™
0
๐Ÿคจ
0
๐Ÿ˜ฎ
0
๐Ÿ˜‚
0
User Avatar

Your Answer

Loading...

Still Have Questions?

Related Questions

Relative atomic masses are measured in?

AMU's


An isotope of which element is used as the standard for the relative mass scale for atoms?

Carbon-12 is used as the standard by which the atomic masses of other nuclides are measured.


Why are gram formula masses called relative masses?

They are called relative masses because all of the masses of the elements are measured relative to the mass of an isotope of carbon called carbon-12. Carbon-12 has been assigned a mass of exactly 12 atomic mass units. One atomic mass unit has an actual value of 1.660538782(83)ร—10^โˆ’27 kg.


What atom is used as the standared in the relative scale for atomic masses?

This is the isotope carbon-12.


True or false relative atomic masses sre measured in amus?

true


What are the units for average relative atomic masses?

The unit is such that the isotope Carbon 12 is exactly 12 by definition.


Relative atomic masses are expressed in atomic mass units?

Yes, relative atomic masses are expressed in atomic mass units


Is this statement true or false The isotope hydrogen-1 is the standard used for the relative scale of atomic masses?

true


Is 20Ne and 21N an isotope?

Yes, neon has three isotopes and they have relative atomic masses of 20, 21 and 22 respectively.


How you calculate the relative atomic weight of uranium?

The atomic weight of an element is derived from the atomic masses of the isotopes of this element and from the percentage of these isotopes. The correct terms are: - atomic weight for elements - atomic mass for an isotope


What is the average atomic mass of an element is the average atomic masses of what kind of isotopes?

average atomic massof an element=(Atomic mass of first isotope X % of that isotope) + (Atomic mass of second isotope X % of the second isotope)


True or false relative mass is a system of comparing atomic masses to carbon?

True. The unit for the atomic weights of chemical elements is the relative atomic mass unit (1/12 from the atomic mass of the isotope 12C). Note that atomic weights is used for elements and atomic mass for isotopes.


What is an isotope and why are atomic masses usually in decimal form?

An isotope is a variant of the atom with the same number of protons but more or fewer neutrons. The atomic mass is an average of the isotopes of the element. The average is weighted according to the relative abundance of such isotopes.


What is the standard for comparison for the relative masses listed n the periodic table?

The standard comparison for atomic weights on the periodic table is carbon 12. This is a common isotope of carbon which has 6 protons and 6 neutrons. Carbon 12 is assigned an atomic mass of 12, and other elements' atomic masses are all relative to this value.


The nucleus of an isotope is called?

Surely it's just a nucleus, as every version of an element is an isotope in its own right, and the atomic and molar masses are just an average made by relative abundance...hope this helps.


How do you calculate the atomic mass of an element with different isotopes?

To calculate average atomic mass from different isotopes of an element, we take into account the relative atomic masses of isotopes and their relative abundance on Earth. The following formula is used to calculate the needful : atomic mass = mass of isotope x percent abundance + mass of isotope x percent abundance / 100 (whole expression divided by 100)


What atoms has different masses but the same atomic number?

They are called Isotope.


What is an element that has the same chemical properties but different atomic masses?

an isotope


Is atomic masses measured in amus?

Yes it is true.


What is necessary to calculate the atomic mass of an element?

You need to know the atomic # or the masses of each isotope of the element.


How is the existence of isotopes related to atomic masses not being whole numbers?

Atomic masses are the weighted average of all the isotopes of an element. The average is based on the relative abundance of each isotope. Let say we have an element with two isotopes, the first isotope has a mass of 6 and the second has a mass of 8. If we took a straight average of the atomic masses then the element would have a mass of 7. But a weighted average based on the abundance of each isotope would be different (unless both isotopes are found to be in equal amounts ie. both 50% abundance) If the isotope with a mass of 6 had a relative abundance of 75% (meaning that 3/4 of all atoms of that element had a mass of 6) then the other isotope would have a relative abundance of 25% (relative abundance must add up to 100%). The atomic mass of the elements would be calculated by multiplying each isotopes mass my the relative abundance and then adding the two results together. 75% (6) = 4.5 25% (8) = 2.0 4.5 + 2.0 = 6.5 The atomic mass for this element would have an atomic mass of 6.5 amu (atomic mass units)


Which are the two important particles in an isotope?

The atomic particles of an isotope are the proton, electron and neutron


The average atomic mass of an element is the average of the atomic masses of its?

The average atomic mass of an element is the average of the atomic masses of its isotopes (that is a weighted average). You have to take into account the abundance of each isotope when they do your averaging.


Who is credited for the determination of standard relative atomic masses?

Italian chemist Stanislao Cannizzaro is credited for the determination of standard relative atomic masses. pg.133 modern chemistry textbook


Is the atomic mass equal to the number of atoms in the elements?

No. Atomic mass is the mass of all of the protons, neutrons, and electrons in a single atom of an element at rest. This is not the same as the atomic weight, or relative atomic mass, given for each element on the periodic table. The atomic weights, or relative atomic masses, are the relative atomic masses of the elements in the crust of the earth and atmosphere.