Hence it causes a non-zero dipole moment which causes the polar nature of NF3. The dipole of the NF3 molecule originates in the downward and upward direction because of the lone pair present in Nitrogen. The larger the electronegativity differences of atoms greater is the polarity and dipole moment. Dipole moment measure the strength of polarity. The net dipole moment of the NF3 molecule is 0.24 D.
Hence it also causes NF3 to become polar in nature.Īlso, the electronegativity difference of fluorine and nitrogen atom is greater than 0.5 which ensures that NF3 is highly polar in nature. Positive and negative charges cause non-uniform charge distribution around the NF3 structure. Therefore fluorine gains a partial negative charge and nitrogen gains a partial positive charge. So, being more electronegativity of fluorine help it to attract more bonded electron than nitrogen. So, according to it, NF3 central atom contains 1 lone pair. To find the number of lone pairs, you can use the Nitrogen trifluoride lewis structure. Find the Number of lone pairs present on the central atom of the NF3 lewis structure
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Let’s see how to find the molecular and electron geometry of NF3 this step by step. The molecular geometry of NF3 is a trigonal pyramid and its electron geometry is tetrahedral because nitrogen has Sp³ hybridization with 5 valence electrons in its valence shell and it makes three bond pairs, one with each fluorine atom.Īnd one lone pair is present on the nitrogen atom that tries to repel the bonded pairs of electrons, as a result, the adjacent atoms push apart giving its geometry trigonal pyramid.Īs you see in the above structure, the lone pair on the nitrogen atom repel the adjacent electron pairs, as a result, the two fluorine atom in equatorial position pushes far apart giving the NF3 molecular geometry same as a trigonal pyramid.
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