Question

part 2. in the box to the right. construct the lewis dot structure of the neutral element with an electron - configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p²

Explanation:

Step1: Determine valence electrons

The valence - shell electrons are the electrons in the outermost shell. The electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{2}$. The outermost shell is the 5th shell with electrons in $5s^{2}5p^{2}$. The number of valence electrons is $2 + 2=4$.

Step2: Draw Lewis - dot structure

Place the symbol of the element in the center. Then, place one dot at a time around the symbol for each valence electron. We can place the dots on the four sides (top, bottom, left, right) of the symbol.

Answer:

Draw the symbol of the element (let's assume it's Sn, tin, which has this electron - configuration in its neutral state). Place 4 dots around the symbol, one on each of the four sides (top, bottom, left, right).