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Which of the following is the correct electron configuration for the iodide ion, I⁻?
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10. Periodic Properties of the Elements
The Electron Configuration: Ions
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Which of the following particles has the same electron configuration as a potassium ion (K^+)?
A
Cl^-
B
Ar
C
Na^+
D
Ca^2+
Guida verificata passo dopo passo1
Step 1: Identify the electron configuration of a neutral potassium (K) atom. Potassium has an atomic number of 19, so its electron configuration is \$1s^2 2s^2 2p^6 3s^2 3p^6 4s^1$.
Step 2: Determine the electron configuration of the potassium ion $K^+$. Since it has lost one electron, remove one electron from the outermost shell (4s orbital), resulting in \$1s^2 2s^2 2p^6 3s^2 3p^6$.
Step 3: Recognize that the electron configuration \$1s^2 2s^2 2p^6 3s^2 3p^6$ corresponds to the electron configuration of argon (Ar), which has 18 electrons.
Step 4: Compare the electron configurations of the other ions: $Cl^-$ has gained one electron (18 electrons), $Na^+$ has lost one electron (10 electrons), and \(Ca^{2+}\) has lost two electrons (18 electrons).
Step 5: Conclude that the particles with the same electron configuration as $K^+$ are those with 18 electrons, which includes \(Ar\), $Cl^-$, and \(Ca^{2+}\). Among the given options, \(Ar\) is the correct answer as it is a neutral atom with the same electron configuration.
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