Question

With nn representing the outermost energy level, the electron configuration for that level for elements in Group 14 is :

A) 1s² 2s² 2p².
B) 2s² 2p² 3s² 3p².
C) 3s² 3p² 4s² 3d².
D) 4s² 3d² 4p².

Answer 1

The correct electron configuration for the outermost energy level of Group 14 elements is ns² np². For carbon in Group 14, which is in the second period, the configuration is 2s² 2p², corresponding to option A) 1s² 2s² 2p².

Step-by-step explanation:

The student asked about the electron configuration for elements in Group 14 and which of the listed configurations correctly represents the outermost energy level of these elements. The elements in Group 14 of the periodic table include carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). These elements have four electrons in their outermost energy level.

Considering the energy order of orbitals as 1s, 2s, 2p, 3s, 3p, 4s etc., the correct answer for the configuration of the outermost energy level of Group 14 elements is ns² np². Where 'n' represents the principal quantum number corresponding to the period number the element is in. For carbon (in the second period), the configuration would be 2s² 2p², which is represented by option A) 1s² 2s² 2p². This is the correct configuration for the valence electrons of carbon specifically, which is the second element in Group 14.