Atomic Mass Units.atomic mass unit
12. The number 12 refers to the atomic mass. More precisely, to the sum of neutrons + protons; but this is usually close to the atomic mass. In the case of carbon-12, it is exact, by definition.
The atomic mass is the mass of a molecule, atomic particle or sub-atomic particle.
Cobalt is an atomic mass of 58.93 atomic mass units
== The equation of atomic mass is protons+nuetrons== atomic mass. ===
the answer is the atomic mass unit
Atomic Mass Units.atomic mass unit
The atomic mass unit (AMU) of carbon is approximately 12.01 AMU.
the atomic mass is the mass of an atomin the table of elements each element has its own specific box. the atomic mass is listed under the elemnts symbolEX. 2HE4.00
12 by definition.
12. The number 12 refers to the atomic mass. More precisely, to the sum of neutrons + protons; but this is usually close to the atomic mass. In the case of carbon-12, it is exact, by definition.
Element - Atomic Mass # Example: Carbon - 12
By definition, one mole would be the same as the atomic mass. You take the number of moles and multiply it by the atomic mass. So if you have just 1 mole, the number of grams will be the atomic mass. Nitrogen's atomic mass is 14.007 grams.
The relative atomic mass is the mean mass of the isotopes of an element. Since, by definition, these have different numbers of neutrons, their masses are different. This results in fractional values.
By definition, one mole would be the same as the atomic mass. You take the number of moles and multiply it by the atomic mass (divide by one mole for units to cancel). So if you have just 1 mole, the number of grams will be the atomic mass. Helium's atomic mass is 4.003 grams.
1 atomic mass unit is equivalent to the 1/12 the mass of a carbon-12 atom at rest. This is not considered an si unit because it is defined by a definition and not experimentally
The atomic mass of an element is the average mass of an element's isotopes, weighted by their natural abundance. It is expressed in atomic mass units (u) and is often close to the mass number of the most abundant isotope of the element.