Question
An atom consists of a small positively charged nucleus surrounded by negatively charged electrons. We organize the electrons in a logical manner. As the atomic number increases, electrons are added to the subshells according to their energy. Lower energy subshells fill before higher energy subshells The order of filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. The periodic table can be used to help you remember the order. Give the ground-state electron configuration for silicon (Si). Express the complete electron configuration using superscripts where appropriate. For example, the configuration for Li would be entered as 1s^22s^1. Try Again; 3 attempts remaining submit hints my answer show answer review part Give the actual ground-state electron configuration for copper (Cu). Express the electron configuration using superscripts where appropriate. For example, the configuration for Li would be entered as 1s^22s^1.
Explanation / Answer
silicon is having atomic number = 14 so its electronic configuration is: 1s22s22p63s23p2 copper is having atomic number = 29 its actual electronic configuration is: 1s22s22p63s23p64s23d9 but as we know from hund`s rule that half filled or fullfilled orbital is more stable so here one elctron from 4s moves to 3d which makes 4s halffilled orbital and 3d full filled orbital so now the real configuration is: 1s22s22p63s23p64s13d10 but as we know from hund`s rule that half filled or fullfilled orbital is more stable so here one elctron from 4s moves to 3d which makes 4s halffilled orbital and 3d full filled orbital so now the real configuration is: 1s22s22p63s23p64s13d10