Atomic weight.
The atomic mass (ma) is the mass of a specific isotope, most often expressed in unified atomic mass units.[1] The atomic mass is the total mass of protons, neutrons and electrons in a single atom.[2]The atomic mass is sometimes incorrectly used as a synonym of relative atomic mass, average atomic mass and atomic weight; these differ subtly from the atomic mass. The atomic mass is defined as the mass of an atom, which can only be one isotope at a time and is not an abundance-weighted average as in the case of atomic weight. In the case of many elements that have one dominant isotope the actual numerical similarity/difference between the atomic mass of the most common isotope and the relative atomic mass or standard atomic weights can be very small such that it does not affect most bulk calculations-but such an error can be critical when considering individual atoms. For elements with more than one common isotope the difference even to the most common atomic mass can be half a mass unit or more (e.g. chlorine). The atomic mass of an uncommon isotope can differ from the relative atomic mass or standard atomic weight by several mass units.
The atomic mass unit is used to express the measure of the atomic mass.
There is none.
The atomic mass of magnesium is approximately 24.305 atomic mass units (amu).
The atomic mass of iodine is less than the atomic mass of all elements with greater atomic number.
The atomic mass (ma) is the mass of a specific isotope, most often expressed in unified atomic mass units.[1] The atomic mass is the total mass of protons, neutrons and electrons in a single atom.[2]The atomic mass is sometimes incorrectly used as a synonym of relative atomic mass, average atomic mass and atomic weight; these differ subtly from the atomic mass. The atomic mass is defined as the mass of an atom, which can only be one isotope at a time and is not an abundance-weighted average as in the case of atomic weight. In the case of many elements that have one dominant isotope the actual numerical similarity/difference between the atomic mass of the most common isotope and the relative atomic mass or standard atomic weights can be very small such that it does not affect most bulk calculations-but such an error can be critical when considering individual atoms. For elements with more than one common isotope the difference even to the most common atomic mass can be half a mass unit or more (e.g. chlorine). The atomic mass of an uncommon isotope can differ from the relative atomic mass or standard atomic weight by several mass units.
Atomic no.=no. of protons Atomic mass=no. of protons+no. of neutrons Hence, atomic mass is greater
The atomic mass is the mass of a molecule, atomic particle or sub-atomic particle.
The atomic mass unit is used to express the measure of the atomic mass.
Atomic no.=no. of protons Atomic Mass=no. of protons+no. of neutrons Hence, atomic mass is greater
== The equation of atomic mass is protons+nuetrons== atomic mass. ===
Cobalt is an atomic mass of 58.93 atomic mass units
Atomic Bomb
There is none.
The atomic mass of magnesium is approximately 24.305 atomic mass units (amu).
The atomic mass unit is not a SI unit. An atomic mass unit is equal to 1/12 from the atomic mass of the isotope 12C.
Atomic number 6, atomic mass 12.