That depends on which element you are speaking of. I'm going to give you an example for the hydrogen isotope protium, which has one proton and one electron.
The Atomic Mass for the protium isotope of hydrogen is 1.008*
We use the relative atomic mass in conjunction with a special term called a mole, which is defined as being Avogadro's number of atoms (which is a special number discovered by Avogadro).
Avogadro's number is 602,214,150,000,000,000,000,000; or 6.0221415 x 1023
This is useful because 1 mole of an element is as many grams as the element's relative atomic mass.
So 1 mole of protium is 1.008g and consists of an equivalent number of atoms as Avogadro's number.
So 1.008g of protium is 602,214,115,000,000,000,000,000 atoms of protium!!!
Using this we can find how much one hydrogen atom weighs in grams:
1.008 / 6.0221415 x 1023 = 0.0000000000000000000000016738g
Or 0.0000000000000000000016738mg (milligrams)
Or 0.0000000000000000016738μg (micrograms)
Or 0.0000000000000016738ng (nanograms)
Or 0.0000000000016738pg (picograms)
Or 0.0000000016738fg (femtograms)
Or 0.0000016738ag (attograms)
Or 0.0016738zg (zeptograms)
Or 1.6738yg (yoctograms)
The average mass of a single silicon atom in grams is the ratio 28,085/6,022140857.10e23.
1 atom of carbon refers to a single carbon atom, which is the basic unit of carbon element. 1 gram atom of carbon, in contrast, refers to the molar mass of carbon, which is approximately 12 grams per mole, representing Avogadro's number of carbon atoms. Essentially, 1 gram atom of carbon is equivalent to Avogadro's number of carbon atoms, which is a large number.
To find the mass of 4350000 atoms of carbon, first calculate the molar mass of carbon (12.01 g/mol). Then, divide the molar mass by Avogadro's number to find the mass of one carbon atom. Finally, multiply the mass of one carbon atom by 4350000 to find the total mass of 4350000 carbon atoms.
One mole of 12C has a mass of 12.00000 grams (exactly, by definition).One mole of 13C has a mass of 13.00335 grams.One mole of 14C has a mass of 14.00324 grams.One mole of natural carbon - i.e. a sample with the ration of isotopes equal to that in nature - has a mass of 12.0107 grams.
the atomic mass carbon is 12.011 g/mol 12.011/mol = the mass of one atom 12.011/6.022x10 raised to the power of 23 this equals 1.994520093 x 10 raised to the power of -23 this is the mass of one atom of carbon in grams.
The average mass of a single silicon atom in grams is the ratio 28,085/6,022140857.10e23.
1 atom of carbon refers to a single carbon atom, which is the basic unit of carbon element. 1 gram atom of carbon, in contrast, refers to the molar mass of carbon, which is approximately 12 grams per mole, representing Avogadro's number of carbon atoms. Essentially, 1 gram atom of carbon is equivalent to Avogadro's number of carbon atoms, which is a large number.
The atomic mass of Ne (neon) in grams is approximately 20.180 grams per mole. This means that a single Ne atom would have a mass of about 3.35 x 10^-23 grams.
The mass of a single copper atom is the same as the mass of a nickel atom.
To find the mass of 4350000 atoms of carbon, first calculate the molar mass of carbon (12.01 g/mol). Then, divide the molar mass by Avogadro's number to find the mass of one carbon atom. Finally, multiply the mass of one carbon atom by 4350000 to find the total mass of 4350000 carbon atoms.
Let us use the usual example, carbon, to show you the process.1 atom Carbon (1 mole carbon/6.022 X 1023)(12.01 grams/1 mole carbon)= 2 X 10 -23 grams in one atom carbon==========================(compare to mass of electron and proton )
One mole of 12C has a mass of 12.00000 grams (exactly, by definition).One mole of 13C has a mass of 13.00335 grams.One mole of 14C has a mass of 14.00324 grams.One mole of natural carbon - i.e. a sample with the ration of isotopes equal to that in nature - has a mass of 12.0107 grams.
the atomic mass carbon is 12.011 g/mol 12.011/mol = the mass of one atom 12.011/6.022x10 raised to the power of 23 this equals 1.994520093 x 10 raised to the power of -23 this is the mass of one atom of carbon in grams.
35.5 grams per mole or 5.90*10^-23 for a single atom
Since Argon has a relative atomic mass of 39.95, and mols = grams / RAM, one could calculate 39.95 / (6.02*10^23) = 6.63 * 10^-23 grams [0.00000000000000000000006634g] for a single argon atom, where 6.022 * 10^23 is roughly Avogadro's constant (the count of atoms in a mole). IF my math is correct.
The mass of an avogadro number of atoms in grams is numericaly equivalent to the amu mass of the atom. 6.023 * 10^23.
The mass of a carbon atom is approximately 12 atomic mass units.