Oxygen Difluoride or OF2 is a chemical compound formed by the reaction between halogen fluorine and dilute aqueous equipment of NaOH ( sodium hydroxide ).

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The equation because that the ready of Oxygen Difluoride:

2F2 + 2NaOH ——> OF2 + 2NaF + H2O

It is a colorless gaseous link exhibiting a solid peculiar odor and acts together an oxidizer. It has a boiling allude of 128.40 K and a melting point of 49.3 K. It has a molar massive of 53.996 g/mol and also a thickness of 1.88 g/l as a gas at room temperature.

Although it has actually its usage as a strong oxidizing agent, because that example, in propellants the rocket fuels, this property also makes the compound unsafe.

OF2 deserve to explode on contact with water and also is stated to be extremely corrosive come the skin. It deserve to also impact the eyes and also the cardiovascular system.

Let us have a quick however detailed look into the within of the molecule and also discuss the nature of chemistry bonding.

OF2 Lewis Structure

Do you understand that several determinants make atoms come together and combine to kind several different chemical compounds?

When atoms come together and also create bonds, a brand-new molecule is created.

Usually, the electron in the outermost shell of one atom, also known together valence electrons, take part in chemical bonding.

Lewis Structure, thus, is a straightforward and constructive procedure to map out a diagrammatic representation of a molecule v the help of electron-dot structures.

It offers us a 2D figure and helps us have actually a brief idea around the electron arrangement and the kind of bond formation without going much right into detail.

Now, we will comment on the procedures to form the Lewis structure of OF2.

Steps to kind OF2 Lewis framework Diagram

Step 1: Find the Total variety of Valence Electrons.

The an initial and foremost step is to calculation the total variety of valence electron in an OF2 molecule.

Oxygen belong to group 16, the chalcogen family, and has a valency that 6. Fluorine belongs come the household of halogen in group 17 and also has a valency that 7.

Therefore, the total number of valence electron = 6 + 7*2 = 20.

Step 2: Identify the central Atom

Now, we have to decipher the central atom in this molecule. If we look in ~ the Pauling Electronegativity chart, we can uncover out that the least electronegative element amongst oxygen and fluorine is Oxygen (O).


The central atom in an oxygen difluoride molecule is Oxygen.

Step 3: Sketch the skeleton Diagram the the Molecule

In Lewis Structure, we usage atomic symbols favor C for carbon, H because that hydrogen to stand for the constituent atoms, and also electron period notation to represent the valence covering electrons.

Let us look in ~ the listed below skeletal sketch:

The atomic symbols:


Atomic symbols in addition to dot notations:


Step 4: Octet rule 

The key group elements ( group 1 to group 17 ) of the routine table have actually a tendency to attain the octet construction of the noble gas aspects present in team 18 that the very same period. This is known as octet fulfillment due to the fact that the facets want to achieve eight electrons in their valence shells.

For example, Carbon tends to obtain a Neon configuration.

Exception: Hydrogen often tends to achieve Helium configuration, for this reason only 2 electrons in the outer shell.

Here, if we look in ~ the octet rule, both the fluorine atom have achieved a valency the eight. The same goes because that the main oxygen atom.

Step 5: Formal charge Concept

Before we continue to confirm any sketch to be the perfect Lewis framework for a given molecule or ionic structure, we require to check the formal fee values.


For Oxygen: Formal charge = 6 – 0.5*4 – 4 = 6 – 2 – 4 = 0.

For every Fluorine atom: Formal fee = 7 – 0.5*2 – 6 = 7 – 1 -6 = 0.

Since the elements are existing in their least possible formal fee values, we have completed our suitable Lewis structure configuration.

Let us see:


Here, oxygen creates a solitary bond v each of the fluorine atom (O-F).

OF2 molecule Geometry

We have currently found the 2D Lewis structure diagram of the Oxygen Difluoride molecule.

Now, we space going to decipher the 3D molecule shape. Via Lewis Structure, we have actually realized the kind of link formed and the variety of lone or unbonded bag of valence electrons present in one OF2 molecule.

Our next step is to usage Valence covering Electron Pair Repulsion theory (VSEPR) to discover the specific molecular geometry along with the bond angles.

Like fee electrons develop a negatively fee cloud surrounding the atom nuclei and also repulsion is created. The VSEPR design tends to minimize or minimization the repulsive forces and also balance the stability of any given molecule, in this case, OF2.

Let us look at this VSEPR chart reflecting AXN notations:


According to AXnEx notation that VSEPR theory,

A: central atom ( Oxygen )

X: no. Of bordering atoms, ‘n’ = 2 ( Fluorine )

E: no. Of lone bag of electrons of the central atom, ‘X = 2.

The VSEPR notation for the OF2 molecule is AX2E2. Follow to the over chart, we have actually a bent molecule structure.

The bond angle is around 103 degrees (due come the repulsion that the lone pair).



In chemistry, one orbit is a fixed path roughly the nucleus in i m sorry electrons often tend to move or revolve. An orbital, on the various other hand, is characterized to be the probability of the existence of an electron in any type of given regional space.

Atomic orbitals are of numerous shapes favor spherical, dumb-bell, clover-leaf, or doughnut to surname a couple of of the complex varieties. We have actually s,p,d,f atomic orbitals ( AOs ).

Electrons deserve to be explained via their wave attributes in quantum mechanics. If us take into account the mix of wave functions of numerous atomic orbitals, us come throughout the procedure of hybridization.

For example, the wave functions of the s and a 2px orbitals provide rise to sp hybridization which usually outcomes in a direct geometry.

Hybridization in OF2

Let united state look in ~ the electronic configuration of oxygen and also fluorine in your ground states.

O: 1s2 2s2 2p4

F: 1s2 2s2 2p5


After creating bonds v halogen F and also attaining octet configuration, the electronic structure of O looks like this:


We, therefore, have in the outermost covering of the central oxygen atom, four hybridized orbitals: 2s, 2px, 2py, 2pz.

Steric number = number of atoms bonded to central atom inside a molecule + number of lone pair of electron attached to the main atom

Also, steric number = 2 + 2 = 4.

Therefore, we have actually sp3 hybridization for the central oxygen atom in a molecule of oxygen difluoride ( OF2 ).

OF2 Polarity

Let us know at very first what we typical by the an extremely famous and common terminology: Polarity.

Polarity have the right to be defined as the physical property of any type of molecule or chemical compound wherein the constituent atomic aspects can own either optimistic or negative charges or both.

We have already seen the Pauling Electronegativity chart. Each and every aspect of the main groups in the periodic table has a certain value that electronegativity.

When atoms of the same facet come together in same ratio, the charge worths neutralize themselves and the net dipole is zero, because of this the molecule is non-polar. Linear or symmetrical chemistry molecules are usually non-polar. ( e.g. : H2 )

However, if molecule consist of uneven partial charge distributions because of a difference in electronegativity or the molecular form is asymmetrical, the net dipole no cancel or becomes zero and also we have a polar molecule.( e.g. : H3PO4, HCl ).

You can likewise refer to the polarity of HCl.

Is OF2 a polar molecule?

Let us have a quick look into the molecular form of Oxygen Difluoride. That is almost similar to H2O and also in both cases, the central O has two lone bag on the top.

The electronegativity value of Oxygen is 3.44. And, that of fluorine is 3.98.

Since oxygen is an ext electropositive 보다 fluorine atoms, it will certainly possess a partial optimistic charge ( δ+ ) and also each of the F atoms will possess a an unfavorable partial charge ( δ- ).

So, we can see that there is an electronegativity difference and henceforth the net dipole minute is no equal to zero.

Again, OF2 is not a symmetrical straight structure. The lone bag on the central Oxygen atom provide it a bent molecule geometry which resembles the English letter V.

We have actually gone with both the uneven charge distribution and the asymmetry the Oxygen Difluoride.The molecule is polar in nature.

For in-depth information, girlfriend must likewise read out the write-up written around the polarity the OF2.

OF2 Molecular orbit (MO) Diagram

Valence Bond theory is essential for explaining chemical bonding within a molecule structure however it has several restrictions or drawbacks.

Here, come the molecule Orbital theory or MOT.

In MOT, we take into account the ide of molecule orbitals (MOs) which room orbitals the the molecule as a whole and also not just those that constituent separation, personal, instance atoms.

It considers electrons to be delocalized and results in producing bonding and also anti-bonding interaction in orbitals.

To showcase the relative energy levels the the AOs and the resultant MOs, we have actually the Molecular orbit diagrams.

The lower power molecular orbital is the bonding and also the higher energy is the anti-bonding orbital.

The below-mentioned diagram provides us the separation, personal, instance MO diagrams that Oxygen and also Fluorine separately, the atoms that make up a molecule that OF2.



In this article, us have debated the kind of chemistry bonding emerging inside one OF2 molecule. Oxygen Difluoride is an interesting molecule that was found accidentally and later had several applications although it was toxicity in nature.

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We have covered Lewis Structure, VSEPR concept to identify molecular geometry, Hybridization, Polar nature, and a short discussion top top MO diagram about oxygen difluoride.