Is NF3 polar or nonpolar - Polarity of NF3
NF3 is the chemical formula for nitrogen trifluoride. It is a synthetic inorganic chemical formed by the reaction of HCl with NH3 and has a molar mass of 71 g/mol. NF3 is toxic, odorless, colorless, and non-flammable gas. It is primarily used in manufacturing semiconductor devices such as LCD displays, thin-film solar cells, etc.
To find out whether the nitrogen trifluoride (NF3) molecule is polar or non-polar, continue reading this article.
Is NF3 polar or non-polar?
Nitrogen trifluoride (NF3) is a polar molecule. NF3 consists of a nitrogen (N) atom and three fluorine (F) atoms. The nitrogen atom is present at the center of the molecule, while three fluorine (F) atoms occupy terminal positions, one on each side, making a trigonal pyramidal molecular shape.
An electronegativity difference of 0.94 units exists between nitrogen and fluorine atoms in each N-F bond in the NF3 molecule. Thus, all three covalent bonds are individually polar in NF3 and possess a specific dipole moment value (symbol µ).
The asymmetrical trigonal pyramidal shape and geometry of NF3 further enhance the polarity effect. The N-F dipole moments do not get canceled. The electron cloud distribution does not stay uniform thus, NF3 is overall polar (net µ =0.24 D).
|Name of molecule||Nitrogen trifluoride (NF3)|
|Bond type||Polar covalent|
|Molecular geometry||Trigonal pyramidal|
|Polar or Non-polar?||Polar molecule|
|Dipole moment||0.24 Debye|
What makes a molecule polar or non-polar?
A molecule is polar if there is a non-uniform charge distribution present in it. If the charge distribution gets equally balanced in different parts, then that molecule or molecular ion is considered non-polar.
The following three factors mainly influence the polarity of a molecule or molecular ion:
- The electronegativity difference between two or more covalently bonded atoms
- Dipole moment
- Molecular geometry or shape
Now, let us discuss the effect of the above three factors one by one to prove that the nitrogen trifluoride (NF3) molecule is overall polar.
Factors affecting the polarity of NF3
It is defined as the ability of an atom to attract a shared pair of electrons from a covalent chemical bond.
Electronegativity decreases down the group in the Periodic Table of elements while it increases across a period.
Greater the electronegativity difference between bonded atoms in a molecule, the higher the bond polarity.
Nitrogen (N) is present in Group V A (or 15) of the Periodic Table. The electronic configuration of nitrogen is 1s2 2s2 2p3. As per this electronic configuration, an N-atom has a total of 5 valence electrons. It is thus short of 3 valence electrons that are required so that a nitrogen atom can achieve a complete octet electronic configuration.
Conversely, fluorine (F) is a halogen that belongs to a Group of VII A (or 17) of the Periodic Table. The electronic configuration of a fluorine atom is 1s2 2s2 2p5. Valence electrons in fluorine are total 7 in number. Therefore, an F-atom has a deficiency of only a single electron to complete its octet.
Hence in NF3, three F-atoms are single covalently bonded with the central N-atom, one on each side of the trigonal pyramidal shape. In this way, all four bonded atoms attain a complete octet configuration via chemical bonding in NF3.
One lone pair of electrons is present on the nitrogen atom that tries to repel the bonded pairs of electrons. Consequently, the adjacent atoms are pushed apart giving NF3 a trigonal pyramidal shape and geometry.
|Atom||Electronic configuration||Valence electrons|
|Fluorine (9F)||1s2 2s2 2p5||7|
The electronegativity of the F-atom is 3.98 and of N-atom is 3.04. The electronegativity difference of 0.94 units is present between the bonded N-atom and F-atoms.
The more electronegative F-atom strongly attracts the shared electron cloud away from the central N-atom in each of the N-F single bonds present in NF3.
Thus, the nitrogen atom present at the center of NF3 gains a partial positive (Nδ+) charge, while each terminal fluorine atom obtains a partial negative (Fδ-) charge. As a result, each N-F bond is individually polar in the nitrogen trifluoride molecule.
The dipole moment is the product of electrical charge (Q) and bond length (r) between two bonded atoms. It is a vector quantity expressed in Debye (D) units.
It is represented by a Greek symbol µ and measures the polarity of a bond.
The dipole moment of a polar covalent bond conventionally points from the positive center to the center of the negative charge. So in NF3, the dipole moment of each N-F bond points from Nδ+ to Fδ- (as shown below).
According to the valence shell electron pair repulsion (VSEPR) theory of chemical bonding, NF3 is an AX3E1 molecule. To one N-atom at the center (A), three F-atoms (X) are attached, and there is one lone pair (E) on the central atom.
A lone pair of electrons on the central N-atom leads to strong lone pair-bond pair repulsions in addition to the N-F bond pair-bond pair repulsive effect. The strong repulsive effect distorts the shape and geometry of the molecule.
Thus, NF3 adopts an asymmetric trigonal pyramidal shape and molecular geometry. Each F-N-F bond angle is 101.9° in NF3.
It is due to this asymmetrical shape that the dipole moments of individually polar N-F bonds do not get canceled. The electron cloud stays non-uniformly distributed over the molecule. Thus, NF3 is overall polar (net µ = 0.24 Debye).
Difference between polar and nonpolar?
|Polar molecule||Non-polar molecule|
|Atoms must have a difference in|
|Atoms may have the same or different electronegativity values|
|Unequal charge distribution overall||Equal charge distribution overall|
|Net dipole moment greater than zero||Net dipole moment equals to zero|
|Examples include water (H2O), ethanol (CH3CH2OH), ammonia (NH3), sulfur dioxide (SO2), bromine trifluoride (BrF3), nitrogen trichloride (NCl3), nitrogen trifluoride (NF3), etc.||Examples include oxygen (O2), nitrogen (N2), methane (CH4), nitrate [NO3]– ion, etc.|
Also, check –
- NF3 lewis structure, molecular geometry, bond angle, hybridization
- How to tell if a molecule is polar or nonpolar?
- Is NCl3 polar or nonpolar?
- Is NO3– polar or nonpolar?
- Is BrF5 polar or nonpolar?
- Is SF4 polar or nonpolar?
- Is CO2 polar or nonpolar?
- Is NH3 polar or nonpolar?
- Is SO2 polar or nonpolar?
- Is SO3 polar or nonpolar?
- Is H2O polar or nonpolar?
- Is H2S polar or nonpolar?
- Is HCN polar or nonpolar?
- Is CCl4 polar or nonpolar?
- Is XeF4 polar or nonpolar?
- Is CH2O polar or nonpolar?
- Is CHCl3 polar or nonpolar?
- Is SF6 polar or nonpolar?
- Is BF3 polar or nonpolar?
- Is PCl5 polar or nonpolar?
Why is NF3 a polar molecule?
Thus, NF3 is overall polar with the net dipole moment of µ = 0.24 Debye.
What causes the NF3 molecule to be trigonal pyramidal in shape, and how this shape affects the molecular polarity?
Bond polarity depends on the electronegativity difference between bonded atoms, while molecular polarity is governed by the overall shape of the molecule.
In NF3, there is a lone pair of electrons on the central N-atom that distorts the shape and geometry of the molecule.
It thus adopts an asymmetric trigonal pyramidal shape, which leads to an unequal charge distribution overall, thus contributing to overall molecular polarity.
Why NF3 is polar, but BF3 a non-polar molecule?
Nitrogen trifluoride (NF3) has an asymmetrical trigonal pyramidal The dipole moments of individually polar N-F bonds do not get canceled in NF3; thus, it is polar (net µ > 0).
Boron trifluoride (BF3) has a symmetrical trigonal planar shape and geometry as there is no lone pair of electrons on the central B-atom. The dipole moments of individually polar B-F bonds get canceled in BF3. Hence it is overall non-polar (net µ = 0).
What are the formal charges present on bonded atoms in NF3?
Formal charge on an atom = [ valence electrons – non-bonding electrons- ½ (bonding electrons)]
For the central N-atom
∴ Formal charge on N-atom = 5 – 2 – 6/2 = 5 – 2 – 3 = 5 – 5 = 0
For single-bonded F-atoms
∴ Formal charge on each single-bonded F-atom = 7 – 6 – 2/2 = 7 – 6 – 1 = 7 – 7 = 0
Zero formal charges is present on the central N-atom and also on each of the terminal F-atoms.
Thus, the overall charge present on the nitrogen trifluoride molecule is Zero.
- Nitrogen trifluoride NF3 is a polar molecule.
- It consists of polar N-F bonds due to the electronegativity difference of 0.94 units between nitrogen and a fluorine atom.
- Nitrogen trifluoride NF3 has an asymmetrical trigonal pyramidal shape with a 101.9° bond angle due to a lone pair of electrons on the central N-atom in NF3.
- The dipole moments of individually polar N-F bonds do not get canceled due to this asymmetrical shape.
- The net dipole moment in NF3 is 0.24 Debye, so it is overall polar.
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