12 amu
Boron.
34.98008 AMU
The isotope with a mass of 32 amu is the most abundant. This can be determined by comparing the atomic mass of sulfur (32.06 amu) to the masses of the isotopes. Since the atomic mass is closest to 32 amu, this isotope is the most abundant.
Doofus. Atomic # - 128 Atomic mass - 320.04 amu
If the atomic mass of a carbon is 12 amu, 1 mole of pure carbon will have a mass of 12 g. (that's the way an a.m.u. is defined: 1 a.m.u. = 1/12th of the mass of C-12 isotope atom)
amu is an anime character in shugo chara ------------------------------------------------- The atomic mass unit (amu) is 1/12 from the atomic mass of the isotope 12C in his ground state.
Boron.
34.98008 AMU
IUPAC credited seaborgium with the mass [269]; the atomic mass of this isotope is 269,128 63(39) amu.
The isotope with a mass of 32 amu is the most abundant. This can be determined by comparing the atomic mass of sulfur (32.06 amu) to the masses of the isotopes. Since the atomic mass is closest to 32 amu, this isotope is the most abundant.
Hydrogen's atomic mass (1 amu for the most stable isotope) is less than that of helium (4 amu).
248.90
Doofus. Atomic # - 128 Atomic mass - 320.04 amu
If the atomic mass of a carbon is 12 amu, 1 mole of pure carbon will have a mass of 12 g. (that's the way an a.m.u. is defined: 1 a.m.u. = 1/12th of the mass of C-12 isotope atom)
The mass number of an isotope of an element is defined as the sum of the numbers of protons and neutrons in the nucleus of each atom of the isotope. The atomic number is defined as the number of protons only in the nucleus. Therefore, an atom with an atomic number. Since neutrons have no electric charge, the nuclear charge of the specified atom is 17 amu.
the atomic mass is -(248.90)
The mass of the isotope multiplied by its relative abundance plus the the mass times abundance of other isotopes.(mass of isotope)(relative abundance) + (mass of isotope)(relative abundance) = average atomic massExample: Carbon can be naturally found as carbon- 12 or carbon- 13. The mass of carbon- 12 is 12 amu and it makes up 98.93% of naturally found carbon. The mass of carbon- 13 is 13.00335 amu, and it makes up 1.07% of naturally found carbon. So the equation to calculate the average atomic mass of carbon is:(0.9893)(12 amu) + (0.0107)(13.00335 amu) = 12.01 amu