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Chemistry Ch. 10 & Final Exam Review Mary Strangler Center for Academic Success This review is meant to highlight basic concepts from the units covered in this course. It does not cover all concepts
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How to fill out 1s22s22p63s23p64s24d8 form
To fill out the electron configuration 1s22s22p63s23p64s24d8, follow these steps:
01
Start by identifying the principal energy level. In this case, the principal energy level is 4 because the highest value in the electron configuration is 4d8.
02
Next, determine the number of electrons in each sublevel. The sublevels within the 4th principal energy level are 4s, 4p, and 4d.
2.1
The 4s sublevel can hold a maximum of 2 electrons, so it is filled with 2 electrons: 4s2.
2.2
The 4p sublevel can hold a maximum of 6 electrons, so it is filled with 6 electrons: 4p6.
2.3
The 4d sublevel can hold a maximum of 10 electrons, but in this case, only 8 electrons are present: 4d8.
03
Moving to the lower principal energy levels, we fill the remaining sublevels:
3.1
The 3s sublevel is filled with 2 electrons: 3s2.
3.2
The 3p sublevel is filled with 6 electrons: 3p6.
04
Finally, we fill the 2s sublevel with 2 electrons: 2s2.
In conclusion, the electron configuration 1s22s22p63s23p64s24d8 represents an atom with 2 electrons in the 1s sublevel, 2 electrons in the 2s sublevel, 6 electrons in the 2p sublevel, 2 electrons in the 3s sublevel, 6 electrons in the 3p sublevel, 2 electrons in the 4s sublevel, and 8 electrons in the 4d sublevel.
As for who needs this electron configuration, it is often used in the field of chemistry and physics when studying the electronic structure of atoms and molecules. It provides valuable information about the arrangement of electrons and helps determine various properties and behaviors of these entities.
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