Final answer:
The options that are isoelectronic with the oxide ion are F- and O-.
Step-by-step explanation:
An ion is said to be isoelectronic when it has the same number of electrons as another ion or atom. The oxide ion (O2-) has 10 electrons. To determine which of the given options is isoelectronic with the oxide ion, we need to compare the number of electrons in each option:
a. P3-: Phosphorous has the electron configuration 1s2 2s2 2p6 3s2 3p3, which gives it 5 valence electrons. When it gains 3 electrons to become P3-, it would have a total of 8 electrons, which is not isoelectronic with the oxide ion.
b. F-: Fluorine has the electron configuration 1s2 2s2 2p5, which gives it 7 valence electrons. When it gains 1 electron to become F-, it would have a total of 8 electrons, which is isoelectronic with the oxide ion.
c. O: Oxygen has the electron configuration 1s2 2s2 2p4, which gives it 6 valence electrons. It already has the same number of electrons as the oxide ion and is therefore isoelectronic.
d. O-: This is the same as the oxide ion, which means it is isoelectronic.
e. S2-: Sulfur has the electron configuration 1s2 2s2 2p6 3s2 3p4, which gives it 6 valence electrons. When it gains 2 electrons to become S2-, it would have a total of 8 electrons, which is isoelectronic with the oxide ion.
Therefore, the options that are isoelectronic with the oxide ion are: b. F- and d. O-.