Oxygen has several isotopes, the most abundant being oxygen-16 (816O^{16}_{8}\text{O}816O) and oxygen-18 (818O^{18}_{8}\text{O}818O).
Which statement correctly describes the divalently charged anions 16O2−^{16}\text{O}^{2-}16O2− and 18O2−^{18}\text{O}^{2-}18O2−?
Both ions have a total of 8 electrons and different specific charges.
Both ions have a total of 10 electrons, but the 16O2−^{16}\text{O}^{2-}16O2− ion has a greater specific charge than the 18O2−^{18}\text{O}^{2-}18O2− ion.
Both ions have the same number of neutrons but different numbers of electrons.
Both ions have the same specific charge because they carry the same net charge of −2e-2e−2e.