Question

enter full electron configurations for each ion.

part a

f-

express your answer in complete form, in order of increasing orbital. for example, 1s²2s² would be entered as 1s^22s^2.

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part b

p³-

express your answer in complete form, in order of increasing orbital. for example, 1s²2s² would be entered as 1s^22s^2.

Explanation:

Step1: Determine the number of electrons for \(F^-\)

Fluorine (\(F\)) has an atomic number of \(9\). The \(F^-\) ion has gained one electron, so it has \(9 + 1=10\) electrons.
Using the Aufbau principle (\(1s<2s<2p\)), the electron configuration is \(1s^22s^22p^6\).

Step2: Determine the number of electrons for \(P^{3 -}\)

Phosphorus (\(P\)) has an atomic number of \(15\). The \(P^{3-}\) ion has gained three electrons, so it has \(15+ 3 = 18\) electrons.
Using the Aufbau principle (\(1s<2s<2p<3s<3p\)), the electron configuration is \(1s^22s^22p^63s^23p^6\).

Answer:

Part A: \(1s^22s^22p^6\)
Part B: \(1s^22s^22p^63s^23p^6\)