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rspill6

Answer:

i)  The electron configuration for the magnesium ion, Mg²⁺, is 1s² 2s² 2p⁶.

ii)  The electron configuration for the oxide ion, O²⁻, is:  1s² 2s² 2p⁶

Explanation:

We will assume that the two atoms in question are [tex]Mg^{2+}[/tex] and [tex]O^{2-}[/tex].  Note the clarification on the charges for both atoms.

i)  The electron configuration for the magnesium ion, Mg²⁺, is 1s² 2s² 2p⁶, can be explained:

  • A neutral magnesium atom has 12 electrons.
  • When it loses two electrons to become Mg²⁺, it gets a positive charge because it loses two negatively charged electrons.
  • The two lost electrons come from the outermost 3s orbital, which originally held 2 electrons.
  • Therefore, the remaining electron configuration reflects the filled inner orbitals (1s and 2s) and the filled 2p orbitals, with the 3s orbital now empty.

ii)  The electron configuration for the oxide ion, O²⁻, is:  1s² 2s² 2p⁶

Here's why:

Neutral oxygen (O) has 8 electrons [Element 8]. Its electron configuration is typically written as [He] 2s² 2p⁴, using the noble gas helium (He) as a shorthand for the 1s² electrons in the inner shell.

When oxygen gains two electrons to become the oxide ion (O²⁻), it completely fills its outermost 2p subshell with 6 electrons (2p⁶). This configuration is similar to that of neon (Ne), which has a full outer shell and is very stable.

Therefore, O²⁻ achieves a stable octet configuration, meaning it has 8 electrons in its valence shell (the outermost energy level).

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