{"id":159253,"date":"2024-10-31T14:24:15","date_gmt":"2024-10-31T14:24:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=159253"},"modified":"2024-10-31T14:24:59","modified_gmt":"2024-10-31T14:24:59","slug":"which-of-the-following-is-the-correct-electron-configuration-for-se2%e2%88%92","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/31\/which-of-the-following-is-the-correct-electron-configuration-for-se2%e2%88%92\/","title":{"rendered":"Which of the following is the correct electron configuration for Se2\u2212"},"content":{"rendered":"\n

Which of the following is the correct electron configuration for Se
2\u2212
?
A. [Ar] 4s
2
3d
10
4p
6
B. [Ar] 4s
2
3d
10
4p
2
C. [Ar] 4s
2
3d
10
4p
4
D. [Ar] 4s
2
4d
10
4p
6<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct answer is: A: [Ar] \\, 4s^2 \\, 3d^{10} \\, 4p^6<\/strong><\/p>\n\n\n\n

To determine the correct electron configuration for the selenium ion ( \\text{Se}^{2-} ), we start with the electron configuration of neutral selenium (( \\text{Se} )), which has an atomic number of 34. The electron configuration for neutral selenium is:<\/p>\n\n\n\n

[
\\text{Se}: [\\text{Ar}] \\, 4s^2 \\, 3d^{10} \\, 4p^4
]<\/p>\n\n\n\n

The notation ([\\text{Ar}]) represents the electron configuration of the noble gas argon, which accounts for the first 18 electrons (1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076).<\/p>\n\n\n\n

Selenium typically gains two electrons to achieve a stable octet configuration, particularly in its common oxidation state of -2. Therefore, the electron configuration for ( \\text{Se}^{2-} ) will include these additional two electrons. We add these electrons to the highest energy sublevel, which is the 4p sublevel:<\/p>\n\n\n\n

Starting from the neutral configuration:<\/p>\n\n\n\n