Question

use the periodic table in the tools bar to complete the electron - configurations for the following elements. lithium (li): 1s^a2s^b a = 2 b = 1 complete beryllium (be): 1s^c2s^d c = 2 d = 2 complete boron (b): 1s^e2s^f2p^g e = 2 f = 2 g = 1 complete carbon (c): 1s^h2s^i2p^j h = i = j = done

Explanation:

Step1: Recall electron - filling rules

Electrons fill orbitals in order of increasing energy: 1s before 2s, 2s before 2p. The 1s orbital can hold a maximum of 2 electrons, the 2s orbital can hold a maximum of 2 electrons, and the 2p orbital can hold a maximum of 6 electrons.

Step2: Determine electrons for carbon

Carbon has an atomic number of 6, which means it has 6 electrons. The first 2 electrons fill the 1s orbital, so $H = 2$. The next 2 electrons fill the 2s orbital, so $I = 2$. The remaining $6-(2 + 2)=2$ electrons go into the 2p orbital, so $J = 2$.

Answer:

$H = 2$
$I = 2$
$J = 2$