In the case of the carbon atom, one s orbital and 3p orbitals from the same shell mix and overlap to produce four new orbitals of similar energy. This is because of the reason that the lone pairs of electrons are present in proportion due to which they cancel out overall neutralizing the effect.įrom the molecular geometry, it is clear that the nitromethane (CH3NO2) molecule is following the ideal conditions, by which it is clear that the carbon atom is sp3 hybridized whereas the nitrogen atom is sp2 hybridized. It might interest you that even after the presence of lone pairs of electrons, there exist distortion from the ideal shape and bond angle. It says the -CH3 end is tetrahedral whereas the -NO2 end is trigonal planar because of the bond angle they are making. The molecular geometry of nitromethane (CH3NO2) can be studied with the help of the Valence Shell Electron Pair Repulsion (VSEPR) theory. Here it is important to understand that the hydrogen-carbon-nitrogen bond is linear meaning 180° so it won’t hold much substance in this discussion. The bond angle between the hydrogen-carbon-hydrogen atoms is 109.5° and that in the carbon-nitrogen-oxygen atom is 120°. So, there will be two molecular geometry for separate entities of -CH3 and -NO2. Step 5: Now, assemble all the steps and draw the Lewis structure of Nitromethane:įrom the Lewis structure, we have got to know about two central atoms in a single nitromethane molecule. Each participating atom is forming a single covalent bond whereas between nitrogen and one oxygen atom, a double covalent bond is forming. In methyl nitrite, one oxygen atom bonds with the carbon which is not the case in nitromethane. The confusion may occur as the molecular formula of the compounds is the same.īut it is important to realize how each of the participating atom form which type of bond. It is important to understand that we are talking about nitromethane, not methyl nitrite. Step 4: Look for the type of bond-forming among the participating atoms in one nitromethane (CH3NO2) molecule: With this information, it is clear that there will be two central atoms bonded together with a single bond. Step 3: Find the central atom in one nitromethane (CH3NO2) molecule:įrom the molecular formula, it is clear that the hydrogen atoms are bonded to the carbon atom whereas the oxygen atoms are bonded to the nitrogen atom. It is 14 as 4 are needed by the carbon atom, 1 each by the hydrogen atom, 3 by the nitrogen atom, and 2 by each oxygen atom. Step 2: Find how many more valence electrons are needed by a single nitromethane molecule (CH3NO2): It is 24 as 4 are coming from the carbon atom, 1 from each hydrogen atom, 5 from the nitrogen atom, and 6 from each oxygen atom.
Step 1: Find the total number of valence electrons present in a single nitromethane molecule (CH3NO2): Steps to Draw the Lewis structure of Nitromethane (CH3NO2) This makes the total number of valence electrons in oxygen 6.īelow is the image of the lewis structure of Carbon, Nitrogen, and Oxygen atom. Here, it is important to know that the valence electrons are also those, present in the highest principal energy level which are s and p for the oxygen atom. Lastly, in the case of oxygen, its atomic number is 8 by which its electronic configuration is 1s2 2s2 2p4. Due to this, the valence electrons in the nitrogen atom are 5. Because p shell needs 6 valence electrons, there exists a scarcity of 5 electrons. In the case of the nitrogen atom, its atomic number is 7 where its electronic configuration is 1s2 2s2 2p3. Due to this, the total number of valence electrons for hydrogen is 1.
As the s shell needs 2 electrons to complete its octet, there is a need for 1 electron. Now, for the hydrogen atom, its atomic number is 1 which makes its electronic configuration 1s1. Due to this, the total number of valence electrons in one carbon atom is 4. The atomic number of Carbon is 6 which makes it electronic configuration 1s2 2s2 2p2.Īs we know, the p shell needs 6 valence electrons to complete its octet, there is a need for 4 more valence electrons. In order to start with the Lewis structure of nitromethane, it is crucial to study the individual participating atoms first.
Conclusion The Lewis Structure of Nitromethane (CH3NO2)
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