The relative atomic mass and molecular mass Relative

The relative atomic mass and molecular mass Relative

TOPICS: relative atomic mass and molecular mass Relative


The relative atomic mass and molecular mass Relative

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Atoms are very small particles. Because the atomic mass is also too small when expressed in units of grams so that the chemists created a way to measure the mass of an atom, namely the relative atomic mass. The relative atomic mass (Ar) is the ratio of the average mass of an atom with one-twelfth times the mass of one atom of carbon-12.

Ar

The smallest unit of a substance can also be a molecule. Molecules composed by two or more atoms held together by chemical bonds. Relative molecular mass (Mr) adalahperbandingan average mass of a molecule with one-twelfth times the mass of one atom of carbon-12.

Mr

In the above formulas used atomic mass and molecular mass on average. Why use an average atomic mass? Because the elements in nature have beberapaisotop. For example, the carbon in nature has two pieces of stable isotopes is C-12 (98.93%) and C-13 (1.07%). If the abundance and mass of each isotope is known, the relative atomic mass of an element can be calculated by the formula:

isotope
Given the relative atomic mass of each element making up the molecule, relative molecular mass equal to the amount of relative atomic masses of all the atoms making up the molecule. Molecules that have a formula in one molecule AmBn means there tersbut m n atom atom A and B. Thus AmBndapat relative molecular mass is calculated as follows.

Mr-AmBn