How di I write the Lewis structure of magnesium chloride?

Question

How di I write the Lewis structure of magnesium chloride?

1 Answer

Impact of this question

26605 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-07-29T01:58:26

See below.

Explanation:

${MgCl}_{2}$ $"MgCl"_2$ is an ionic compound.

The electron configuration of $Mg$ $"Mg"$ is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}$ $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2$ .

$Mg$ $"Mg"$ can get a noble gas $s^{2} p^{6}$ $s^2p^6$ configuration by losing its two $4 s$ $4s$ electrons and forming a magnesium ion, ${Mg}^{2 +}$ $"Mg"^(2+)$ .

The electron configuration of $Cl$ $"Cl"$ is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$ $1s^2 2s^2 2p^6 3s^2 3p^5$ .

$Cl$ $"Cl"$ can get a noble gas $s^{2} p^{6}$ $s^2p^6$ configuration by gaining an electron and forming a chloride ion, ${Cl}^{-}$ $"Cl"^"-"$ .

The Lewis structure of ${MgCl}_{2}$ $"MgCl"_2$ is therefore

Lewis structure
(From www.superteachertools.net)

The compound is held together by electrostatic attractions between the positively charged magnesium ion and the negatively charged chloride ions.

Science

Math

Humanities

... and beyond

How di I write the Lewis structure of magnesium chloride?

1 Answer

Explanation:

Related questions

Impact of this question