Nitrogen trifluoride is a colorless gas with a smell of moldy. That is non-flammable through the chemical formula NF3. It is slightly dissolve in water and an extremely toxic by inhalation.

In this article, we will comment on NF3 lewis dot structure, molecule geometry or VSEPR shape, link angle, hybridization, etc. We will additionally discuss is NF3 polar or non-polar?

NF3 is provided to make chemicals or likewise used together a ingredient of rocket fuels. That is a solid greenhouse gas and also it has the potential to reduce an international warming better than co2. That is also used for making chemistry lasers favor deuterium fluoride and also hydrogen fluoride laser.

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Properties the Nitrogen trifluoride

It has a molar massive of 71.00 g/mol.NF3 boiling point is −129.06 °C and also melting allude is −207.15 °C.It has actually a low dipole moment.The density of NF3 is 3.003 kg/m3Its refractive index is 1.0004.It is Corrosive to tissue.
Name that MoleculeNitrogen trifluoride
Chemical formulaNF3
Molecular geometry that NF3Trigonal pyramid
Electron geometry of NF3Tetrahedral
Bond angle101.9º
Total Valence electron for NF326
The formal fee of NF30

Page Contents present
1 just how to attract NF3 lewis structure?
2 an easy steps for illustration the NF3 lewis dot structure
3 What are the electron and also molecular geometry the NF3?
4 Nitrogen trifluoride polarity: is NF3 polar or nonpolar
5 Three components that indicate the polarity that NF3
6 What is the formal charge in NF3 lewis dot structure and also how to calculate it?
8 an introduction

How to attract NF3 lewis structure?

NF3 lewis structure has actually 3 fluorine and 1 nitrogen atom linked with three single bonds. This structure is very comparable to NCl3 and NH3. Over there is a complete of 10 lone pairs and also 3 bonded pairs present in the NF3 lewis structure.

Let’s see how to draw lewis dot structure for NF3 with simple steps.

Simple measures for illustration the NF3 lewis period structure

1. Count total valence electron in NF3

In the very first step, we need to calculate the total number of valence electrons existing in the NF3 molecule. Together nitrogen current at 15th group in periodic table and Fluorine in group 17th.

⇒ complete valence electron in Nitrogen = 5

⇒ full valence electron in Fluorine = 7

∴ total valence electron accessible for drawing the NF3 lewis structure = 5 + 7*3 = 26 valence electrons  <∴NF3 has three fluorine atom and one nitrogen>


2. Discover the the very least electronegative atom and also placed it in ~ center

After recognize the total valence electron following step is to recognize which atom has less electronegativity.

For this mental electronegativity boost from left to appropriate in the regular table. Clearly, nitrogen is in the left position to fluorine in the regular table.

Nitrogen is the the very least electronegative atom in the NF3 molecule. So, put it at the center, and also fluorine spaced evenly approximately it.


3. Affix nitrogen and fluorine through a single bond

In this step, us start illustration NF3 skeletal framework by bonding together Nitrogen and Fluorine through a single bond.


Now look in ~ this structure and also count how many electrons we used till now and also how numerous are left. 

As three single bonds are provided in the above structure that has 6 electrons and we have actually a total of 26 valence electron are available for NF3 lewis structure.

∴ (26 – 6) = 20 valence electrons

So, we room left v 20 valence electrons.

4. Put remaining valence electrons beginning from external atom first

In this step, we need to place the remaining valence electrons starting from the an ext electronegative atom or indigenous the external atoms.

So, fluorine is an ext electronegative 보다 nitrogen and it requirements 8 electrons to finish its octet rule.

Fluorine already shares 2 electrons v the help of a solitary bond so that only needs 6 more electrons to complete its octet rule.


As you view in the over structure, every fluorine use 6 electron to finish its octet. Now discover how many valence electrons space left.

Three fluorine in the above structure supplied 18 electrons from a full of 20 remaining valence electrons.

∴ (20 – 18) = 2 valence electrons

So, we left v 2 electrons.

Placed these 2 electrons around the main atom(Nitrogen).

5. Complete central atom octet and use covalent bond if necessary

After placing two electrons about the main atom, nitrogen likewise completes that octet rule because it already shares three single bonds through fluorine i beg your pardon contain 6 electrons.


NF3 lewis structure

As you see in this NF3 lewis period structure, nitrogen and fluorine already complete their octet preeminence so no need to make any covalent bond.

We acquired our correct Nitrogen trifluoride lewis structure.

What room the electron and molecular geometry the NF3?

The molecule geometry the NF3 is a trigonal pyramid and its electron geometry is tetrahedral due to the fact that nitrogen has actually Sp³ hybridization through 5 valence electrons in the valence shell and also it makes three bond pairs, one v each fluorine atom.

And one lone pair is current on the nitrogen atom that tries come repel the bonded bag of electrons, as a result, the nearby atoms push apart giving its geometry trigonal pyramid.


As you see in the above structure, the lone pair ~ above the nitrogen atom defeat the adjacent electron pairs, as a result, the two fluorine atom in equatorial place pushes much apart giving the NF3 molecule geometry exact same as a trigonal pyramid.

Let’s see how to uncover the molecular and also electron geometry of NF3 this action by step.

1. Uncover the variety of lone pairs existing on the main atom the the NF3 lewis structure

To uncover the variety of lone pairs, you can use the Nitrogen trifluoride lewis structure. So, according to it, NF3 central atom has 1 lone pair. 

Or find lone pair by utilizing the formula.

∴ L.P = (V.E. – N.A.)/2

where L.P. = Lone pair ~ above the main atom

V.E. = valence electron the that central atom

N.A. = variety of atoms attached to that main atom

∴ So, Nitrogen is the main atom, it has 5 valence electrons and the number of atoms attached come nitrogen is 3

So, L.P. = (5 – 3)/2

= 1

Hence, lone pair top top the central atom nitrogen is 1.

2. Uncover hybridization variety of NF3

Use the formula to find the hybridization of NF3.

∴ H = N.A. + L.P.

where H = hybridization number

N.A. = variety of atoms attached to the main atom

L.P. = lone pairs on that main atom

So, the central atom (nitrogen) attached to 3 fluorine atoms and it has 1 lone pair.

So, H = 3 + 1 

= 4

Hence the hybridization variety of the NF3 main atom is 4 which method it has Sp³ hybridization.

3. Usage VSEPR concept or AXN method to identify NF3 molecular shape

According come Valence covering electron pair repulsion theory if the molecule has Sp³ hybridization and 1 lone pair of electrons, climate the form of the molecule is trigonal pyramidal.


NF3 molecule geometry or Shape

You deserve to use the AXN method likewise to determine the molecular geometry or electron geometry the NF3.

A to represent the main atom.X represents the bonded atom to the main atom.N to represent the lone bag on the main atom

So, nitrogen is the main atom that has actually 1 lone pair and also 3 bonded pair electrons according come the NF3 lewis period structure.

Hence the formula the NF3 i do not care AX3N1

So, according to the VSEPR chart, if the molecule has actually the formula that AX3N1, it has actually a molecular form of trigonal pyramid and electron geometry the tetrahedral.


The bond angle of Nitrogen trifluoride (NF3) is 101.9°.

NF3 is polar because of the asymmetric shape and also electronegativity difference between nitrogen and also fluorine which cause non-zero dipole moment.

For knowing, is NF3 polar or non-polar? us will talk about three determinants 1. electronegativity 2. dipole minute 3. Geometrical or molecule shape.

Three components that suggest the polarity that NF3 

1. Electronegativity: 

The difference in between the electronegativity of Nitrogen and also fluorine is straight proportional come the Polarity that the NF3 molecule.

The electronegativity that the fluorine atom is 3.98 and also for the nitrogen atom, its worth is 3.04.

So, being an ext electronegativity that fluorine help it come attract an ext bonded electron 보다 nitrogen. As such fluorine profit a partial negative charge and nitrogen profit a partial optimistic charge.

Positive and an unfavorable charges cause non-uniform fee distribution about the NF3 structure. Thus it also causes NF3 to come to be polar in nature.

Also, the electronegativity difference of fluorine and nitrogen atom is greater than 0.5 which ensures the NF3 is very polar in nature.

2. Dipole moment

The network dipole moment of the NF3 molecule is 0.24 D. Dipole minute measure the strength of polarity. 

The bigger the electronegativity differences of atoms greater is the polarity and dipole moment.

The dipole that the NF3 molecule originates in the downward and also upward direction due to the fact that of the lone pair present in Nitrogen. Hence it reasons a non-zero dipole minute which reasons the polar nature the NF3.

⇒ Dipole moment formula = charge on the atom * the distance between them 

∴ D = Q × R

3. Geometrical or molecular shape

The geometrical shape is also a large factor to identify is NF3 polar or non-polar.

As we understand NF3 molecule geometry is trigonal pyramidal i beg your pardon is asymmetric and when the form of the molecule is asymmetric or distorted it doesn’t cancel the dipole moment across the molecule. Hence reason polar nature of the molecule

All these determinants are sufficient to recognize whether NF3 is polar or non-polar.

What is the formal fee in NF3 lewis dot structure and also how to calculate it?

To calculation the formal charge in NF3. Use this equation:

⇒ formal charge = (Valence electrons – unbonded electron – 1/2 bonded electrons)

⇒ We will certainly calculate the formal charge on Nitrogen i m sorry is the central atom in the Nitrogen trifluoride lewis diagram.

⇒ Valence electron that nitrogen = 5

⇒ Non-bonding electrons = 2

⇒ Bonding electron = 6

∴ 5 – 2 – 6/2

= 0 is the formal charge on Nitrogen.


Why bond angle in NF3 much less than the in NH3?

The bond edge is inversely proportional come electronegativity. So, in the situation of NF3, fluorine is more electronegative 보다 nitrogen hence it attracts more electrons. Hence repulsion between the link of nitrogen decreased and it provides NF3 bond edge lower.

In the case of NH3, nitrogen is an ext electronegative 보다 hydrogen. For this reason it attracts more electrons and also repulsion between the bond of nitrogen increased. Therefore it reasons the bond angle of NH3 greater than NF3.

∴ l.p.-l.p. > l.p-b.p >b.p-b.p.

where l.p. = lone pairs

b.p. = bond pairs

How many lone pairs and also bond pairs room present about Nitrogen in the NF3 lewis structure?

Nitrogen includes 1 lone pair and also 3 external inspection pair i beg your pardon is attached with fluorine atoms according come the NF3 lewis structure.

why NF3 is much less polar 보다 NH3?

N-F bond is an ext polar 보다 N-H yet NF3 is less polar 보다 NH3. In NF3, polarity is attracted in the direction of fluorine since of more electronegativity. Thus some the the dipole moments room cancelled out since polarity is attractive opposite to the center atom.

The dipole moment of NF3 is 0.24 D.

In NH3, nitrogen is an ext electronegative 보다 hydrogen for this reason dipole minute will add up since polarity is attracted in the direction of the center from hydrogen to nitrogen.

The dipole moment of NH3 is 1.47 D.

Hence higher is the dipole minute of the Molecule more is the polarity of the molecule.

Hence NH3 is an ext polar than NF3.

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Let’s take a quick overview that what us learnt about the NF3 molecules in this article.