All the atoms have octets except the Nitrogen in the center: it only has 6 valence electrons. To give an octet to the Nitrogen, let's take 2 valence electrons from the Oxygen, since it's less electronegative than the Fluorine and is more likely to give them up, and form a double bond.
So now in our Lewis structure for NO2F, we have an octet on the Oxygen, still, but the Nitrogen, now it has 8 valence electrons so its outer shell is full. So we've used all 24 valence electrons.
Each of the atoms has an octet, so we're done. That's the Lewis structure for NO2F. This is Dr. The oxygen atom will share its electrons instead of the fluorine atom as it is less electronegative than the fluorine atom. There will be two resonance structures of nitryl fluoride as any oxygen atom can share its electron pair.
Now, every atom has eight electrons but nitrogen can form only three bonds owing to the absence of d-orbitals. Hence, there is a need to estimate the formal charge on every atom in the molecule. For getting further insight into the nature of chemical bonding in nitryl fluoride, we need to understand its molecular geometry, which can be anticipated from Valence Shell Electron Pair Repulsion VSEPR theory.
This theory has been established the concept of repulsion of valence shell electrons, as they create a negatively charged atmosphere around the atom. These valence shell electrons can be bonding as well as nonbonding electrons. The lone pair — lone pair repulsion is higher than lone pair-bond pair repulsion, which in turn higher than bond pair-bond pair repulsion.
The molecule becomes more stable by minimizing the repulsion between valence electrons and hence, increasing the distance between them. As the nitrogen atom does not have nonbonding electrons, hence, the shape of the nitryl fluoride can be predicted from the following table. Here, the nitrogen atom is a central atom with three bond pairs of electrons, as can be observed from the Lewis structure. Hence, the general formula of nitryl fluoride will be AX3 and it will have a trigonal planar geometry around the nitrogen atom.
All X atoms are not the same in NO2F and the nitrogen atom forms one double bond with the oxygen atom and two single bonds with another oxygen atom and a fluorine atom. According to this theory, the atomic orbitals of the central atom cannot overlap directly with other orbitals because they cannot explain the directional property of the structure. Hence, these atomic orbitals combine and form hybrid orbitals of equivalent energy. Then, the covalent bond is formed by overlapping these hybrid orbitals with the atomic orbitals of the surrounding atoms.
The steps for the determination of hybridization of the nitrogen atom in Nitryl Fluoride by VBT are given below. The nitrogen atom has ground state electronic configuration: [He] 2s22p3. As nitrogen atom has a positive charge, therefore, electronic configuration of nitrogen ion cation in its ground state: [He] 2s22p2. The electronic configuration of the nitrogen ion by excitation of 2s electron to 2p orbital i.
According to the VSEPR theory as well as the lewis structure, nitryl fluoride constitutes one pi bond three sigma bonds from the nitrogen atom. Hence, the one 2s orbital and two 2p orbitals of the nitrogen atom will fuse, which take place in the following manner:. Hence, three sp2 hybrid orbitals are formed whereas the 2pz orbital remains unchanged and hence, 2pz orbital is used for the formation of a pi bond with the oxygen atom. The sideways overlapping of atomic orbitals results in the formation of a pi bond.
The orbital diagram of nitryl fluoride, representing only the sigma bonds, is shown below. Therefore, the hybridization of the nitrogen atom in Nitryl Fluoride is sp2 hybridization with trigonal planar geometry. The polarity of any compound depends upon the net dipole moment and distribution of charges around the central atom in that compound.
If the compound has a net dipole moment and asymmetric charge distribution around the central atom, then it is a polar molecule. From the Pauling Electronegativity chart, the electronegativity values of the nitrogen atom, fluorine atom, and oxygen atom are 3. These electronegativity values confirm that electronegativity increases across the period. Hence, the N-F bond is polar and acts as a dipole with a partial positive charge and a partial negative charge on the nitrogen atom and the fluorine atom, respectively.
However, the N-O bond has a completely negative and positive charge on the oxygen atom and nitrogen atom, respectively.
The electronegativity difference generates the net dipole moment in the molecule and therefore, nitryl fluoride is a polar molecule. The nitryl fluoride has trigonal planar geometry with asymmetric charge distribution around the nitrogen atom and hence, it is a polar molecule. The bonding nature of one of the inorganic compounds, the nitryl fluoride, NO2F, is discussed here. The nitrogen atom is present at the center of the structure of nitryl fluoride.
In the Lewis structure of the nitryl fluoride, there is a positive and a negative formal charge on the nitrogen atom and the oxygen atom, respectively. The nitryl fluoride has trigonal planar geometry with asymmetric charge distribution.
Hence, it is a polar molecule. The nitryl fluoride shows sp2 hybridization at the nitrogen atom. November 9, November 9, November 8, November 7, Your email address will not be published.
Save my name, email, and website in this browser for the next time I comment. Here, we are going to learn about the chemical bonding of Nitryl Fluoride.
NO2F Lewis Structure We need to depict the Lewis structure of nitryl fluoride to understand the nature of chemical bonding in it.
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