Understanding Isotopes and Atomic Mass in Chemistry
Explore the world of isotopes and average atomic mass in chemistry through detailed explanations and informative images. Learn about the differences between isotopes, their impact on atomic mass, and how to calculate average atomic mass. Discover the significance of isotopes versus ions and delve into the essential concepts in the periodic table. Courtesy of Christy Johannesson.
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Isotopes and Average Atomic Mass Subtitle
Isotopes Atoms of the same element with different mass numbers. Nuclear symbol: Mass # 12 6C Atomic # Hyphen notation: carbon-12
Isotopes Neutron + + + Electrons Nucleus + + + Nucleus Proton Proton + Nucleus + Neutron + Carbon-12 Neutrons 6 Protons Electrons + Electrons + 6 6 + Carbon-14 Neutrons 8 Protons Electrons 6 6 Nucleus
6Li 7Li 3 p+ 3 n0 3 p+ 4 n0 2e 1e 2e 1e Neutron Neutron Electrons Electrons + + Nucleus Nucleus + + + + Proton Proton Nucleus Nucleus Lithium-6 Neutrons 3 Protons Electrons Lithium-7 Neutrons 4 Protons Electrons 3 3 3 3
17 Cl 37 Isotopes Chlorine-37 17 atomic #: 37 mass #: 17 # of protons: 37 17Cl 17 # of electrons: 20 # of neutrons:
Average Atomic Mass weighted average of all isotopes on the Periodic Table round to 2 decimal places Avg. Atomic Mass =(mass)(%) + (mass)(%) 100 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Average Atomic Mass EX: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16O, 0.04% 17O, and 0.20% 18O. Avg. Atomic Mass (16)(99.76) + (17)(0.04) + (18)(0.20) =16.00 amu = 100 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Isotopes vs. Ions Isotopes vary in the number of neutrons so mass is affected Ions vary in the number of electrons so charge is affected
