Explain why the following ground-state electron configurations are not possible: a. 1s22s32p3 b. 1s22s22p33s6 c. 1s22s22p73s23p8 d. 1s22s22p63s23p14s23d14

Answer 1

For a): Can't have more than two electrons in an orbital 2s³ not possible

b). Need to fill the three 2p orbitals before 3s, can't have 3s⁶

c). maximum number of electrons in p orbitals is 6

d) need to fill 3p orbitals before 4s and only 10 electrons in d orbitals

Answer 2

a. 1s2 2s3 2p3 The s orbital can only hold 2 electrons, so 2s3 is not possible.

b. 1s2 2s2 2p3 3s6 There are 2 issues here: a p orbital can hold 6 electrons, so you would fill the 2p orbital before starting to fill 3s. Also, an s orbital can only hold 2 electrons, so 3s6 is not possible.

c. 1s2 2s2 2p7 3s2 3p8 2 issues here: both are that p can only hold 6 electrons, so 2p7 and 3p8 are not possible.

d. 1s2 2s2 2p6 3s2 3p1 4s2 3d14 The 3p orbital would be filled with 6 electrons before moving to 4s, and d orbitals only hold 10 electrons so 3d14 is not possible.