MGF2 Lewis Structure: Drawings, Hybridization, Shape, Charges, Pairs


In this article, we will discuss about mgf2 lewis structure, molecular geometry, formal charge calculation, hybridization and its applications.

Each Magnesium atom and each Fluorine atom have two single bonds in the Lewis structure of MgF2. Two Fluorine atoms surround the Magnesium atom. There are no lone pairs on magnesium, however there are three lone pairs on both fluorine atoms.

1. How to draw MGF2 lewis structure:

The Lewis structure of magnesium fluoride must be studied in conjunction with the Lewis structure of magnesium and fluorine atoms. The atomic number of magnesium is 12 and its electronic configuration is 1s2 2s2 2p6 3s2. This gives magnesium a total valence electron count of 2. Fluorine, on the other hand, has an atomic number of 9 and an electronic configuration of 1s2 2s2 2p5. In this case, fluorine has 9 valence electrons.

Steps to draw the Lewis structure of magnesium fluoride (MgF2):

Step 1: Determine the maximum number of valence electrons accessible in a single magnesium fluoride molecule

There are sixteen because two have magnesium atoms and fourteen have two fluorine atoms.

Step 2: Determine how many valence electrons one magnesium fluoride molecule needs to complete its octet

It is eight since both the fluorine and magnesium atoms require one and the magnesium atom requires six. It’s vital to remember that the magnesium atom will supply two valence electrons, while each fluorine atom will get one.

Step 3: Identify the main atom

Because this atom exists as a single thing, it is magnesium.

Step 4: Determine the sort of link that forms between the atoms that are involved

Between each magnesium and fluorine link, only single bonds develop.

Step 5Merge all of the given facts to form the Lewis structure

Simple structure of MgF2 from wikipedia

2. Molecular Geometry of Magnesium Fluoride:

The molecular geometry of the magnesium fluoride is studied with the help of the VSEPR theory. According to this idea, the magnesium fluoride molecule must meet the following criteria in order to have a linear structure:

  • Two bonding electron pairs
  • Electron domains are two 
  • Lone pairs are zero

The Lewis structure reveals that magnesium fluoride (MgF2) has a linear molecular geometry. The tri-atomic MgF2 molecule has the simplest structure since all of the involved atoms are aligned in a straight line at an angle of 180°.

3. MGF2 lewis structure formal charge:

The formal charge present on the magnesium atom in the MgF2 molecule is same as the real charge on the magnesium atom.

By applying following formula, we can find out the formal charge on the magnesium atom in the MgF2 molecule:

MgF2 molecule’s formal charge on the magnesium atom = (V. E (Mg) – L.E (Mg – ½ (B.E))

V.E (Mg) = the magnesium atom in the MgF2 molecule has a valence electron.

L.E (Mg) = Lone pairs of electrons in the MgF2 molecule’s magnesium atom.

B.E = the Mg atom in the MgF2 molecule has a bond pair electron.

In the MgF2 molecule, the formal charge on the magnesium atom is calculated.

The MgF2 molecule contains two valence electrons, and four bonding electrons on the magnesium atom resulted from the two single bonds coupled with the fluorine atoms and no lone pair of electrons.

MgF2 molecule’s formal charge on the magnesium atom was found to be = (2- 0-(4/2)) = 0

4. MGF2 hybridization:

There will be no hybridization structure in the Magnesium Fluoride (MgF2) molecule since magnesium fluorine is not a covalent compound. Because magnesium has a low electronegativity, it loses two valence electrons when it combines with a non-metal, resulting in a +2 charge.

5. MGF2 lewis structure octet rule:

This rule limits the number of valence electrons in an atom’s outermost shell to a maximum of eight. The maximum number of valence electrons that can be accommodated in the outermost shell according to this rule is interesting to note since several groups in the periodic table defy this norm and enlarge their outermost shell to accept additional valence electrons.

6. MGF2 Uses:

  • Multi-layer anti-reflective optical coatings on glass
  • As a long-lasting lens material that eliminates birefringence in UV and IR radiation.
  • In the deep and vacuum UV areas, MgF2 windows are commonly utilised. They are long-lasting and create few abnormalities.

Conclusion:

Magnesium fluoride (MgF2) is an ionic compound, we study its lewis structure, shape, formal charge calculation, hybridization and its uses.

Madhusudan DN

Hi....Myself D N Madhusudan, I have completed my Masters in General Chemistry at University of Mysore. Mysore. Apart from this, I like to read, and listen to Music. Let's connect through LinkedIn:https://www.linkedin.com/in/madhusudan-d-n-b83a05156

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