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 answer is approx. 2.10ex-23 grams.
5.8x10^-23
The average mass of a single silicon atom in grams is the ratio 28,085/6,022140857.10e23.
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 mass of an avogadro number of atoms in grams is numericaly equivalent to the amu mass of the atom. 6.023 * 10^23.
The molar mass of bromine is approximately 79.9 grams/mol. Since one mole of any substance contains Avogadro's number of particles (6.022 x 10^23), the mass of a single bromine atom is approximately 79.9 grams/mol divided by 6.022 x 10^23, which is approximately 1.33 x 10^-22 grams.
The average mass of a single silicon atom in grams is the ratio 28,085/6,022140857.10e23.
mother earth
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
The mass of an avogadro number of atoms in grams is numericaly equivalent to the amu mass of the atom. 6.023 * 10^23.
1.055 × 10-25 kg.
The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless). Relative isotopic mass is the relative mass of a given isotope scaled with carbon-12 as exactly 12.
The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless). Relative isotopic mass is the relative mass of a given isotope scaled with carbon-12 as exactly 12.
The molar mass of bromine is approximately 79.9 grams/mol. Since one mole of any substance contains Avogadro's number of particles (6.022 x 10^23), the mass of a single bromine atom is approximately 79.9 grams/mol divided by 6.022 x 10^23, which is approximately 1.33 x 10^-22 grams.
The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless). Relative isotopic mass is the relative mass of a given isotope scaled with carbon-12 as exactly 12.