Complete the following table, showing the number of protons, neutrons, and electrons for the two most common isotopes of mercury (Hg200and Hg202) in both the elemental and ion forms.

Question

In this compound, mercury forms an ion with a charge of +2, and sulfur forms an ion with a charge of −2. Complete the following table, showing the number of protons, neutrons, and electrons for the two most common isotopes of mercury (200^Hg and 202^Hg) in both the elemental and ion forms.

Isotopes Form Protons Neutrons Electrons

200^Hg Atom (charge=0)

Ion (charge=+2)

202^Hg Atom (charge=0)

Ion (charge=+2)

1. 200^Hg (atom; charge=0): ? protons
2. 200^Hg (atom; charge=0): ? neutrons
3. 200^Hg (atom; charge=0): ? electrons
4. 200^Hg (ion; charge=+2): ? protons
5. 200^Hg (ion; charge=+2) : ? neutrons
6. 200^Hg (ion; charge=+2): ? electrons

Answer 1

Instead of giving you the answers, I will tell you how to answer the questions.

1. Get a periodic table and find the element mercury (Hg).
2. In the block containing the elemental symbol, you should find the atomic number which is the number of protons in the nucleus. This will be 80. The atomic mass is around 200 because it takes into account the relative amounts of various isotopes of mercury.
3. The questions in the problem indicate that the isotope to be considered is the one whose mass number is 200.
4. The number of neutrons is obtained by subtracting the atomic number from the mass number.
5. In a neutral atom, the number of electrons is equal to the number of protons.
6. For the ion, the number of protons and neutrons do not change from the neutral atom, but the number of electrons in this case will be 2 less than the number of protons.

This should be enough information to answer the questions.