NO2 Lewis structure shows several chemical properties of the compound. Many facts about its internal structure can be obtained from the drawing of Lewis did structure. This article will represent those facts such as:
- Drawing NO2 Lewis structure
- NO2 Lewis structure molecular geometry
- NO2 Lewis structure resonance
- NO2 Lewis structure shape
- NO2 Lewis structure formal charge
- NO2 Lewis structure angle
- NO2 Lewis structure octet rule
- NO2 Lewis structure lone pairs
- NO2 valence electrons
- NO2 hybridization
- NO2 uses
Drawing NO2 Lewis structure
Drawing Lewis structure of Nitrogen dioxide is simple and followed by the fundamental steps of Lewis structure formation. Those steps give specific structure with proper geometric knowledge.
In the first place calculating the number of Valence electron is the most significant step to follow. Then placing g the suitable atom in the centre of the compound one can draw the basic Sketch of the NO2 Lewis structure.
Moreover, several factorial characteristics can be represent by the following the steps of drawing. The most electronegative atom is placed in the centre that is the Nitrogen in NO2 is considered as centre atom of this compound.
The number of valance electrons decides formation of bond pairs and existence of lone pairs in the compounds. After drawing the complete Lewis structure of NO2, it has been found that one oxygen atom holds one extra valance electron, which cannot get scope to undergo bonding.
VSEPR (Valence Shell Electron Pair Repulsion) theory relates with this structure in the case of describing the internal facts about NO2. This theory delivers tremendous valuable knowledge about the bond pair and lone pair in the compound and their effect on its shape.
NO2 Lewis structure molecular geometry
The molecular geometry can be represented by counting the number of bond and lone pairs in the compound. It is important to identify the molecular geometry of a compound to illustrate the internal facts about it.
In Nitrogen dioxide, it has been found that the compound has three bond pairs and one lone pair. It possessed Trigonal planner structure for electron geometry. Nitrogen is bonded with one oxygen by double bond (one sigma and one π bond).
NO2 Lewis structure resonance
Resonance is notable in the compound, which holds one or more π bonds in the molecular structure. NO2 has one π bond that helps the compound in posing resonating structure.
There is one extra electron present on one oxygen atom that creates bond with the centre atom in NO2 that is Nitrogen. The π bond opens up and generates negative charge on another oxygen atom and vice versa. Therefore, NO2 has two consecutive resonating structures.
NO2 Lewis structure shape
The shape of compound depends on few factors such as the present of bond pairs and lone Pairs in the compound impacts on the sculpture of the compounds. VESPR theory is responsible for deciding the presence of bond pairs and lone pairs in compounds and its effect on the shape.
NO2 has Trigonal planner geometry with bent shape. The shape of the compound is bent due to the presence of lone pairs in oxygen. This bent geometry of Nitrogen dioxide is represented by VESPR (Valence Shell Electron Pair Repulsion) theory as well.
NO2 Lewis structure formal charge
The Lewis structure of any compound delivers the idea about charges hold by each element. It is important to calculate the charges to identify overall charge of the compound.
A specific formula is there to calculate the formal charges of the elements that are (valence electrons – nonbonding electrons – ½ bonding electrons).
The formal charge of Nitrogen atom is (5-2-(1/2)*3) = 1.5
The formal charge of Oxygen with only one Sigma bond is (6-5-(1/2)*1) = 0.5
The formal charge of Oxygen with one Sigma and one pi bond is (6-6-(1/2)*2) = -1
The overall charge of NO2 comes out as -1. It indicates the presence of one free electron on one of the oxygen atom inside the molecular geometry.
NO2 Lewis structure bond angle
Bond angle is another physical feature identified by the Lewis structure of any compound. Bond angle also can be obtained with the help of VSEPR (Valence Shell Electron Pair Repulsion) theory.
The bond angle of NO2 is 115 °, which indicates its bent shape due to strong repulsion in the lone pairs present in the overall compound. The extra electron in the compound has impact on the angle of the Nitrogen dioxide.
NO2 Lewis structure octet rule
Octet rule refers to the phenomenon regarding filling the last energy level of the periodic element exactly the similar way of nearest noble gas. It gives ultimate stability to the elements. Therefore, for having similar electronic configuration like the nobles gases the elements undergo electron sharing or transferring process.
In NO2, nitrogen needs three electrons to fill its octet and each of the oxygen atoms need two electrons for the same reason. Therefore, nitrogen partially shares its two electrons with one oxygen atom for getting two electrons in its last energy level and share one electron with another oxygen atom.
The oxygen atoms also share their electron on the needs of having electron partially from nitrogen. One oxygen atom gets one electron only and shares one electron with the centre atom. Therefore, there is an excess electron on one oxygen atom, which makes the compound unstable in case of filling octet.
NO2 Lewis structure lone pairs
The number of lone pair hold by the centre atom in any compound is considered as the number of lone pair of the entire compound. The number of lone pair is significant to recognise for delivering complete description about the Lewis electronic structure.
The number of lone pair in Nitrogen dioxide is one. Therefore, the total number of lone pair is considered as one. Otherwise, the oxygen atoms also hold lone pairs on their octet. Each oxygen atom holds 3 lone pairs in this structure.
These lone pairs are responsible for giving bent structure to geometry of the Nitrogen dioxide. The ideal bond angle of the compound differs and gets lowered by the factor lone pair bond pair repulsion.
NO2 valence electrons
The total number of valence electron can be found by calculating the number of electron in individual atoms. Valence electron refers to the electrons, which is remained in the last energy level of the atoms.
In NO2, the number of valence electron in Nitrogen is five and both the oxygen have six valence electron for each. Valence electrons provides the facts about the requirement of electron in the octet of the elements, Nitrogen needs three electrons and each of oxygen needs two electrons.
The total number of valance electron in NO2 is (5+6) = 11. Nitrogen can share only three electrons therefore; one electron of an oxygen atom remains unshared, which supports the valence of the elements. Now that electron responsibly provides a resonating structure of the compound.
Hybridisation can be obtained by drawing Lewis structure and this electron structure gives internal knowledge about the electronic geometry of the compounds after undergoing electron share methods.
The hybridization of NO2 is sp2. It is supportive to represent the Trigonal planner shape of the compound. Sp2 hybridization means that one electron from the s orbital of Nitrogen atom shift to the vacant shell of p orbital of the atom.
Every chemical; compound holds some specific utilities in chemistry. Similarly, NO2 is chemical compound that shoes utilisable properties as well.
NO2 is used in several chemical methods. Such as:
- NO2 is great compound to use in the industrial production of Nitric acid.
- It acts as catalyst in the chemical reactions.
- The immediate production of sulphuric acid is also regulated by NO2
- In the rocket fuels, NO2 is used as oxidiser.
- Oxidised cellulose compounds are manufactured with the help of nitrogen dioxide.
This article has described the electronic facts about the chemical compound Nitrogen dioxide matters evaluate by NO2 Lewis structure have been illustrated in this article to bring forth effective knowledge about the compound and its internal sculpture.