2.1.1 atomic structure and isotopes

• Isotope - are atoms of same elements with same number of protons, but different number of neutrons
• relative isotopic mass - mass of one isotope compared to 1/12th of the mass of one atom of carbon 12
• relative atomic mass - weighted mean mass of one atom compared to 1/12 th of the mass of an atom of carbon 12
• relative molecular mass - average mass of molecule compared to 1/12 th of mass of one atom of carbon 12
• isotopes have similar chemical properties because they have the same electronic structure. they may have slightly varying physical properties because they have different masses
• RAM =$\frac{\sum_{ }^{ }\left(isotopic\ mass\ \times\%\ abundance\right)}{100}$
• RAM - relative atomic mass
• RAM = $\frac{\sum_{ }^{ }\left(isotopic\ mass\ \times relative\ abundance\right)}{total\ relative\ abundance}$
• relative atomic mass - weighted mean mass of one atom compared to 1/12 th of the mass of an atom of carbon 12
• relative molecular mass - average mass of molecule compared to 1/12 th of mass of one atom of carbon 12
• whats the weighted mean mass?

  taking into account the relative abundancies of the isotopes