Unit 4 atoms and the periodic table ppt video online download average atomic mass urtaz Image collections
{"Image DocumentName": "Average Atomic Mass", "Image ImageDescription": "The weighted average of the masses of all the naturally occurring isotopes of an element (forms of an element with different number of neutrons) The average considers the percent abundance of each isotope in nature. Found on the periodic table of elements. Example. What would be the atomic mass (\u2248) of Hydrogen if these three isotopes. were found in the following percentages (99.9, 0.015, 0) respectively? Hydrogen (Protium) Mass # = 1 amu. Hydrogen (Deuterium) Mass # = 2 amu. Hydrogen (Tritium) Mass # = 3 amu. If you simply average the three, 2 amu (1 amu + 2 amu + 3 amu/3) would be the atomic mass, but since 99.9% of the Hydrogen is Protium, the atomic mass is around 1 amu (.999 x 1 amu)", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}