1. Consider an isotope with 18 protons, a charge of +2, and a mass number of 38. Answer the following questions:
a. How many neutrons are in this isotope?
b. What is the atomic number of the isotope?
c. How many electrons 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 in the isotope, we subtract the number of protons from the mass number. Therefore, the isotope has 20 neutrons (38 - 18 = 20).
b. The atomic number of an isotope is equal to the number of protons. In this case, the atomic number is 18.
c. Since the isotope is charged +2, it means that it has lost 2 electrons. Therefore, the isotope has 16 electrons (18 - 2 = 16).
d. The total number of nucleons is equal to the sum of protons and neutrons. In this case, it would be 18 protons + 20 neutrons, which gives us 38 nucleons.
e. The total number of subatomic particles is the sum of protons, neutrons, and electrons. In this case, it would be 18 protons + 20 neutrons + 16 electrons, which gives us 54 subatomic particles.