Question

oxygen, $^{16}_{8}o$ $1s^{2}2s^{2}2p^{4}$ what would happen to this oxygen - 16 atom if two protons and two neutrons were removed? a nitrogen - 14 would be the end product. b it would become the isotope oxygen - 12. c it would transform into the atom carbon - 12 with an electrical charge of 2. d the oxygen - 16 would have an electrical charge of 2.

Explanation:

Step1: Determine initial properties of oxygen - 16

Oxygen - 16 has 8 protons (atomic number of oxygen is 8) and 8 neutrons (mass number 16 - 8 protons = 8 neutrons), and 8 electrons to be neutral.

Step2: Calculate changes after removal

If 2 protons and 2 neutrons are removed: Protons become 8 - 2=6, neutrons become 8 - 2 = 6. The mass number is 6+6 = 12, and the atomic number is 6. The element with atomic number 6 is carbon. Since the number of electrons is still 8 and the number of protons is 6, the net electrical charge is + 2 (8 electrons - 6 protons).

Answer:

C. It would transform into the atom carbon - 12 with an electrical charge of 2.