SCH3U Isotope Exercise

SCH3U Isotope Exercise 1. What are the names, symbols, electrical charges, and masses (expressed in amu) of the three subatomic particles? 2. Where is nearly all of the mass of an atom located? Explain your answer in terms of what contributes to this mass. 3. Define the terms atomic number and mass number. 4. How are isotopes of the same element alike? How do they differ? 5. The composition of ordinary neon is: neon-20, 90.92 %; neon-21, 0.26 %; neon-22, 8.82 %. Calculate the average atomic mass of neon. (20.04u) 6. Natural lithium comes in only two isotopes of Li-6 (7.42%) and Li-7 (92.58%). Determine the average atomic mass for Lithium. (6.93u) 7. Boron occurs as two natural isotopes of B-10 (19.78%) and B-11 (80.22%). Determine the average atomic mass for boron. (10.80u) 8. Calculate the relative atomic mass of gallium given that the relative abundance of its two isotopes are: 60.5% of Ga-69 and 39.5% of Ga-71. (69.79u) 9. Oxygen occurs as one major isotope and two minor isotopes. O-16 (99.759%), O-17 (0.037%) and O-18 (0.204%). Calculate the average atomic mass of oxygen. (16.00u) 10. Iron has four isotopes; Fe-54 (5.82%); Fe-56 (91.66%); Fe-57 (2.19%) and Fe-58 (0.33%). Determine the average atomic mass for natural iron. (55.91u) 11. Nickel has five naturally occurring isotopes. We will exclude all the special isotopes synthetically made in nuclear reactors. The isotopes are: Ni-58 67.88% Ni-60 26.23% Ni-61 1.19% Ni-62 3.66% Ni-64 1.08% Calculate the average atomic mass of nickel. (58.79u) 12. Iridium (a metal rather like platinum) occurs with only two isotopes of mass number 191 and 193. The atomic weight of iridium is 192.2. Deduce the relative abundance of the two isotopes of this element. (There must be more Ir-193 since the average mass is 192.2u which is closer to 193 that 192) 13. A recently discovered element has been given the symbol Hh (recently unknown). It has an average atomic mass of 255.84 amu. There are only two isotopes of Hh, these being Hh-253 and Hh-259. Determine the relative percentages of these two isotopes. This is tricky!!! (Hh-253 = 52.67%; Hh-259 = 47.33%) 14. Natural Rubidium consists solely of the isotopes Rb-85 and Rb-87. From the atomic mass of Rb (85.4678) calculate the relative percentages of these two isotopes. (Rb-85 = 76.61%; Rb-87 = 23.39%) 15. There are only two naturally occurring isotopes of Mattrothium (Mr). There are Mr-335 and Mr-338. (The first person to make a joke about Mattrothium being a heavy element will be summarily flogged.) Mr-335 makes up 69.00% of all know Mattrothium. Determine the average atomic mass of Mattrothium. (335.95u)