Consider an isotope with 38 electrons, an atomic number of 39, and a mass number of 86. Answer the following questions:
a. How many neutrons are in this isotope?
b. What is the charge of the isotope?
c. How many protons are in this isotope?
d. What is the total number of nucleons?
e. What is the total number of subatomic particles?
a. To find the number of neutrons, subtract the number of protons (atomic number) from the mass number: 86 - 39 = 47 neutrons.
b. The charge of an isotope is determined by the number of protons and electrons. In this case, there are 38 electrons and 39 protons, so the charge is +1.
c. The number of protons is given as 39.
d. The total number of nucleons is the sum of protons and neutrons, so it is 39 (protons) + 47 (neutrons) = 86 nucleons.
e. The total number of subatomic particles is the sum of protons, neutrons, and electrons. In this case, there are 39 protons, 47 neutrons, and 38 electrons, so the total number of subatomic particles is 39 + 47 + 38 = 124.