The nitronium ion chemical formula is NO2+. Drawing NO2+ Lewis Structure is very easy to by using the following method. Here in this post, we described step by step method to construct NO2+ Lewis Structure. The nitrogen and oxygen elements come as the member of the nitrogen and oxygen family groups from the periodic table respectively. The valence electrons in nitrogen and oxygen are five and six respectively. The branch of nitronium ion chemistry is used to make chemicals reagents for nitrating reactions.
Key Points To Consider When Drawing The NO2+ Electron Dot Structure
A three-step approach for drawing the NO2+ Lewis structure can be used. The first step is to sketch the Lewis structure of the NO2+ molecule, to add valence electrons around the nitrogen atom; the second step is to add valence electrons to the two oxygen atoms, and the final step is to combine the step1 and step2 to get the NO2+ Lewis Structure.
The NO2+ Lewis structure is a diagram that illustrates the number of valence electrons and bond electron pairs in the NO2+ molecule. The geometry of the NO2+ molecule can then be predicted using the Valence Shell Electron Pair Repulsion Theory (VSEPR Theory), which states that molecules will choose the NO2+ geometrical shape in which the electrons have from one another.
Finally, you must add their bond polarities to compute the strength of the two N-O double bonds (dipole moment properties of the NO2+ molecule). The nitrogen-oxygen bonds in nitronium ion(NO2+), for example, are polarised toward the more electronegative oxygen in NO2+ molecule, and because both bonds have the same size and are located around two oxygen terminals of the linear molecular geometry with no lone pairs (in positive charge resonating around) on the nitrogen atom, their sum of dipole moment is zero due to the NO2+ molecule’s bond dipole moment and more electron polarity to the oxygen atoms. Because each two N-O bonds polarity canceled each other in the NO2+ molecule due to the presence of no lone pairs of electrons. The nitronium ion(NO2+) molecule is classified as a nonpolar molecule.
The molecule of nitronium ion (with linear structured molecular geometry) is tilted, the bond angles between nitrogen and oxygen are 180 degrees. It has a difference in electronegativity values between nitrogen and oxygen atoms, with central nitrogen’s pull being less than terminal oxygen’s in the NO2+ molecule. But they canceled each other due to the symmetrical linear structure with no lone pairs in the molecular geometry of the NO2+ molecule.
As a result, it has the zero dipole moment. The NO2+ molecule has a nonzero dipole moment due to an equal charge distribution of negative and positive charges. But both nitrogen and oxygen atoms fall on the nitrogen and oxygen family groups in the periodic table respectively. The oxygen atom is a more electronegative value than nitrogen in the NO2+ molecule. The NO2+ molecule has the net dipole moment of 0D value in the ground state energy level.
NO2+ molecule has two N-O double bonds. Its dipole moment in the ground state is totally different as compared with the excited state. If it absorbs light may be from visible or UV light. It undergoes pi to pi star and n to pi star transition from ground state energy level to excited state energy level. In the excited state energy level, the NO2+ molecule shows a definite dipole moment. But it is very dynamics.
Molecules can be classified as polar or nonpolar. The molecule polar behaves in a different manner as compared to nonpolar.
Overview: NO2+ Lewis Structure
The central atom is nitrogen, which is bordered on two terminals with oxygen atoms( in linear geometry), and no lone pairs on the central nitrogen atom in the linear molecular geometry. Nitrogen has five outermost valence electrons, indicating that it possesses five electrons in its outermost shell, whereas oxygen also has six valence electrons in its outermost shell. To complete the octet of the nitrogen and oxygen atoms requires three and two valence electrons on each of their outermost shell respectively.
Two oxygen atoms establish covalent connections with the central nitrogen atom as a result, leaving the nitrogen atom with no lone pairs. But the positive charge is on the central nitrogen atom. There are no lone pairs of electrons on the nitrogen central atom that don’t resist the bond pairs of the two N-O bonds. According to VSEPR theory, the single N-O bond pairs polarity lead the NO2+ molecule to take on the linear geometry structure.
The NO2+ molecule’s two N-O bonds are arranged in symmetrical polarity order around the linear molecular geometry, giving rise to the NO2+ molecular shape. The NO2+ molecule has a linear molecular geometry because there is an electrical repulsion between the lone pairs of electrons in nitrogen and two double bond pairs(N-O) of the NO2+ molecule.
Lewis structure of NO2+ has dot electron representative structure. Valence electrons of atoms undergo orbitals mixing in the chemical reactions, gives new types of molecular species of NO2+. The molecule is nothing but a bundle of valence electrons from the atoms. But it is converted to bond pairs and lone pairs in the molecular structure.
Electronegative value Difference Calculation of NO2+ Molecule:
Nitrogen and oxygen Electronegative difference in NO2+:
The nitrogen atom has an electronegativity value of 3.04, while oxygen has an electronegativity value of 3.44 in the NO2+ molecule. The difference in electronegativity of nitrogen and oxygen can be estimated using the method below.
The electronegative value difference between nitrogen and oxygen in NO2+ molecule
Electronegativity value of nitrogen = 3.04
Electronegativity value of oxygen= 3.44
Difference of electronegativity value between nitrogen and oxygen in NO2+ molecule = 3.44 – 3.04 = 0.40Electronegativity difference between N-O bond calculation of NO2+ molecule
The electronegative difference between nitrogen and oxygen is less than 0.5. This indicated the bond polarity moves near to a slightly polar nature. N-O bond polarity in the NO2+ molecule is less polar.
Because of this difference in electronegativity of nitrogen and oxygen atoms, the NO2+ molecule’s NO2+ bond becomes nonpolar. The total net dipole moment of the NO2+ molecule is zero due to the cancellation of the bond dipole moment in the linear structural geometry. The electronegativity of an atom is the strength with which it may attract bound electron pairs to its side. The polarity of NO2+ is discussed in our previous post.
As a result, the N-O bond’s dipole moment is none due to the polarization of the bonds( negligible) and no lone pairs of electrons on nitrogen, and all N-O bonds’ dipoles are arranged in the symmetrical NO2+ molecular geometry. The NO2+ molecule has a zero net dipole moment.
The electron dot structure of the NO2+ molecule is also known as the NO2+ Lewis structure. It determines the number of outermost valence electrons as well as the electrons engaged in the NO2+ molecule’s bond formation. The outermost valence electrons of the NO2+ molecule must be understood while considering the Lewis structure of the molecule.
The nitrogen atom is the middle element in NO2+ molecular geometry, with five electrons in its outermost valence electron shell, whereas the oxygen atom has six electrons in its outermost valence electron shell. The oxygen atom has six valence electrons.
The NO2+ has a total of 16 valence electrons as a result of the foregoing above-said reasoning. With the core central nitrogen atom, the two terminals with two oxygen atoms form covalent bonds, leaving the nitrogen atom with no lone pairs in the middle of linear geometry.
Because lone pairs on the terminal oxygen atoms create interaction with N-O bond pairs(but it is negligible in the ground state of the NO2+ molecule). The bond angle of the O-N-O bond in the linear molecular geometry is approximately 180 degrees. This angle is greater than the CH4 molecule bond angle. The N-O bond length is 136pm(picometer).
To sketch the NO2+ Lewis structure by following these instructions:
Step-1: NO2+ Lewis dot Structure by counting valence electrons on the nitrogen atom
To calculate the valence electron of each atom in NO2+, look for its periodic group from the periodic table. The nitrogen and oxygen group families, which are the 15th and 16th groups in the periodic table, are both made up of nitrogen and oxygen atoms respectively. In their outermost shells, nitrogen and oxygen have five and six valence electrons respectively.
Calculate the total number of valence electrons in the NO2+ molecule’s outermost valence shell. The first step is to determine how many electrons are in the NO2+ Lewis structure’s outermost valence shell. An electron in an atom’s outermost shell is known as a valence electron. It is represented by dots in the NO2+ Lewis diagram. The NO2+ molecule’s core nitrogen atom can be represented as follows:
Total outermost valence shell electron of nitrogen atom in NO2+= 5
Total outermost valence shell electron of oxygen atom in NO2+= 6
The NO2+ molecule has one central nitrogen and two oxygen atoms. Then the total outermost valence shell electrons can be calculated as follows
∴ Total outermost valence shell electrons available for NO2+ Lewis structure( dot structure) = 5+2*6= 17 valence electrons in NO2+.
Postive nature of NO2+ molecule gives one electron less, then total valence electron=16calculation of total valence electron of NO2+ molecule
Choose the atom with the least electronegative value atom and insert it in the center of the molecular geometry of NO2+. We’ll choose the least electronegative value atom in the NO2+ molecule to place in the center of the NO2+ Lewis structure diagram in this phase. The electronegativity value in periodic groups grows from left to right in the periodic table and drops from top to bottom.
The first step is to put five valence electrons around the nitrogen atom as given in the figure.
Step-2: Lewis Structure of NO2+ for counting valence electrons around the terminal oxygen atoms
As a result, nitrogen is the first atom in the periodic table’s nitrogen family group. Oxygen is the first member of the oxygen family. The electronegative value of the oxygen atom is higher than that of the nitrogen atom in the NO2+ molecule. Furthermore, oxygen has a six electrons limit since nitrogen is the less electronegative element in the NO2+ molecule.
In the NO2+ Lewis structure diagram, the nitrogen atom can be the center atom of the molecule. As a result, central nitrogen in the NO2+ Lewis structure, with all two oxygen atoms arranged in a linear geometry.
Add valence electrons around the oxygen atom, as given in the figure.
Step-3: Lewis dot Structure for NO2+ generated from step-1 and step-2
Connect the exterior and core central atom of the NO2+ molecule with two double N-O bonds. In this stage, use two oxygen atoms on the outside of the NO2+ molecule to the central nitrogen atom in the middle.
Count how many electrons from the outermost valence shell have been used in the NO2+ structure so far. Each N-O double bond carries four electrons because each nitrogen atom is connected to two oxygen atoms by two N-O double bonds. Bond pairings of N-O are what they’re called.
So, out of the total of 16 valence electrons available for the NO2+ Lewis structure, we used eight electrons for the NO2+ molecule’s two N-O double bonds. The NO2+ molecule has no lone pairs of electrons in the central nitrogen atom.
Place the valence electrons in the N-O bond pairs starting with the core nitrogen, two oxygen atoms in the NO2+ molecule. In the NO2+ Lewis structure diagram, we always begin by introducing valence electrons from the central nitrogen atom(in step1). As a result, wrap around the central nitrogen atom’s bond pair valence electrons first (see figure for step1).
The nitrogen atom in the molecule gets only 8 electrons around its molecular structure. This central nitrogen atom is octet stable. But it has no lone pairs. The positive charge is resonating around the central nitrogen atom of NO2+. Nitrogen molecule(N2) is a colorless and odorless gas. It is available in a higher percentage in the atmosphere. It is one of the main essential micronutrients in plants growth.
Oxygen molecule(O2) is in the gaseous state at normal temperature and pressure. It is essential for life on earth. Most of our oxygen demands come from plants and trees. All types of combustion reactions are carried out with the help of oxygen gas.
Nitrogen requires 8 electrons in its outermost valence shell to complete the molecular octet stability, 8 electrons bond pairs in two N-O double bonds, and no lone pairs in the central nitrogen atom. Then lone pairs of electrons on the oxygen atoms of the NO2+ molecule are placed in a linear geometry. Nitrogen already shares 8 electrons to the two N-O double bonds. Then place the valence electron in the oxygen atoms, it placed around six electrons on each atom(step-2). 8 valence electrons were placed around two oxygen atoms as lone pairs of electrons.
We’ve positioned 8 electrons around the two terminal oxygen atoms(step-3), which is represented by a dot, in the NO2+ molecular structure above. The nitrogen atom completes its molecular octet stability in the NO2+ molecule because it possesses 8 electrons in its (two N-O double bonds) bond pairs with two oxygen in the outermost valence shell.
Count how many outermost valence shell electrons have been used so far using the NO2+ Lewis structure. Two electron bond pairs are shown as dots in the NO2+ chemical structure, whereas two double bonds each contain eight electrons. The outermost valence shell electrons of the NO2+ molecule(bond pairs) are 8 as a result of the calculation. The total valence electron in a nitrogen atom is 8.
So far, we’ve used 16 of the NO2+ Lewis structure’s total 16 outermost valence shell electrons. No lone pairs of electrons on the nitrogen atom in the linear geometry of the NO2+ molecule.
Complete the middle nitrogen atom stability and, if necessary, apply a covalent bond. The central nitrogen atom undergoes octet stability(due to two double bond pairs of electrons).
The core atom in the NO2+ Lewis structure is nitrogen, which is bonded to the two oxygen atoms by double bonds (two N-O). With the help of two double bonds, it already shares 8 electrons. As a result, the nitrogen follows the octet rule and has 8 electrons surrounding it on the two terminals of the NO2+ molecule’s linear geometry.
How to calculate the formal charge on nitrogen and oxygen atoms in NO2+ Lewis Structure?
Calculating formal charge on the nitrogen of NO2+ molecule:
The formal charge on the NO2+ molecule’s nitrogen central atom often corresponds to the actual charge on that nitrogen central atom. In the following computation, the formal charge will be calculated on the central nitrogen atom of the NO2+ Lewis dot structure.
To calculate the formal charge on the central nitrogen atom of the NO2+ molecule by using the following formula:
The formal charge on the nitrogen atom of NO2+ molecule= (V. E(N)– L.E(N) – 1/2(B.E))
V.E (N) = Valence electron in a nitrogen atom of NO2+ molecule
L.E(N) = Lone pairs of an electron in the nitrogen atom of the NO2+ molecule.
B.E = Bond pair electron in S atom of NO2+ moleculecalculation of formal charge on nitrogen atom in NO2+ molecule
The nitrogen core atom (two double bonds connected to two oxygen atoms ) of the NO2+ molecule has five valence electrons, no lone pairs of electrons(zero electrons), and 8 bonding pairing valence electrons. Put these values for the nitrogen atom in the formula above.
Formal charge on nitrogen atom of NO2+ molecule = (5- 0-(8/2)) = +1
In the Lewis structure of NO2+, the formal charge on the central nitrogen atom is +1.
Calculating formal charge on the oxygen atom of NO2+ molecule:
The formal charge on the NO2+ molecule’s oxygen terminal atoms often corresponds to the actual charge on that oxygen terminal atoms. In the following computation, the formal charge will be calculated on the terminal oxygen atom of the NO2+ Lewis dot structure.
To calculate the formal charge on the terminal oxygen atom of the NO2+ molecule by using the following formula:
The formal charge on the oxygen atom of NO2+ molecule= (V. E(O)– L.E(O) – 1/2(B.E))
V.E (O) = Valence electron in a oxygen atom of NO2+ molecule
L.E(Cl) = Lone pairs of an electron in the oxygen atom of the NO2+ molecule.
B.E = Bond pair electron in O atom of NO2+ moleculecalculation of formal charge on oxygen atom in NO2+ molecule
The oxygen terminal atoms of the NO2+ molecule have six valence electrons, two lone pairs of electrons(four electrons), and four bonding pairing valence electrons(double bond). Put these values for the oxygen atom in the formula above.
Formal charge on oxygen atom of NO2+ molecule = (6- 4-(4/2)) =0
In the Lewis structure of NO2+, the formal charge on the terminal oxygen atom is zero.
In this post, we discussed the method to construct the NO2+ Lewis structure. First, the valence electrons are placed around the nitrogen atom. Second, place the valence electron on the oxygen atoms. Finally, when we combined the first and second steps. It gives NO2+ Lewis structure. Need to remember that, if you follow the above-said method, you can construct molecular dot structure very easily.
What is the NO2+ Lewis structure?
NO2+ Lewis structure is dot representation
What is the formal charge on the NO2+ Lewis structure?
Zero charges on the NO2+ molecular structure
The polarity of the molecules
The polarity of the molecules are listed as follows
- Polarity of BeCl2
- Polarity of SF4
- Polarity of CH2Cl2
- Polarity of NH3
- Polarity of XeF4
- Polarity of BF3
- Polarity of NH4+
- Polarity of CHCl3
- Polarity of BrF3
- Polarity of BrF5
- Polarity of SO3
- Polarity of SCl2
- Polarity of PCl3
- Polarity of H2S
- Polarity of NO2+
- Polarity of HBr
- Polarity of HCl
- Polarity of CH3F
- Polarity of SO2
- Polarity of CH4
Lewis Structure and Molecular Geometry
Lewis structure and molecular geometry of molecules are listed below
- CH4 Lewis structure and CH4 Molecular geometry
- BeI2 Lewis Structure and BeI2 Molecular geometry
- SF4 Lewis Structure and SF4 Molecular geometry
- CH2I2 Lewis Structure and CH2I2 Molecular geometry
- NH3 Lewis Structure and NH3 Molecular geometry
- XeF4 Lewis Structure and XeF4 Molecular geometry
- BF3 Lewis Structure and BF3 Molecular geometry
- NH4+ Lewis Structure and NH4+ Molecular geometry
- CHCl3 Lewis Structure and CHCl3 Molecular geometry
- BrF3 Lewis Structure and BrF3 Molecular geometry
- BrF5 Lewis Structure and BrF5 Molecular geometry
- SO3 Lewis Structure and SO3 Molecular geometry
- SI2 Lewis structure and SI2 Molecular Geometry
- PCl3 Lewis structure and PCl3 Molecular Geometry
- H2S Lewis structure and H2S Molecular Geometry
- NO2+ Lewis structure and NO2+ Molecular Geometry
- HBr Lewis structure and HBr Molecular Geometry
- CS2 Lewis structure and CS2 Molecular Geometry
- CH3F Lewis structure and CH3F Molecular Geometry
- SO2 Lewis structure and SO2 Molecular Geometry
- HCl Lewis structure and HCl Molecular Geometry
- HF Lewis structure and HF Molecular Geometry
- HI Lewis structure and HI Molecular Geometry
- CO2 Lewis structure and CO2 Molecular Geometry
- SF2 Lewis structure and SF2 Molecular Geometry
- SBr2 Lewis structure and SBr2 Molecular Geometry
- SCl2 Lewis structure and SCl2 Molecular Geometry
- PF3 Lewis structure and PF3 Molecular Geometry
- PBr3 Lewis structure and PBr3 Molecular Geometry
- CH3Cl Lewis structure and CH3Cl Molecular Geometry
- CH3Br Lewis structure and CH3Br Molecular Geometry
- CH3I Lewis structure and CH3I Molecular Geometry
- SCl4 Lewis structure and SCl4Molecular Geometry
- SBr4 Lewis structure and SBr4 Molecular Geometry
- CH2F2 Lewis structure and CH2F2 Molecular Geometry
- CH2Br2 Lewis structure and CH2Br2 Molecular Geometry
- XeCl4 Lewis structure and XeCl4 Molecular Geometry
- BCl3 Lewis structure and BCl3 Molecular Geometry
- BBr3 Lewis structure and BBr3 Molecular Geometry
- CHF3 Lewis structure and CHF3 Molecular Geometry
- CHBr3 Lewis structure and CHBr3 Molecular Geometry
- ClF3 Lewis structure and ClF3 Molecular Geometry
- IF3 Lewis structure and IF3 Molecular Geometry
- ICl3 Lewis structure and ICl3 Molecular Geometry
- IBr3 Lewis structure and IBr3 Molecular Geometry
- ClF5 Lewis structure and ClF5 Molecular Geometry
- IF5 Lewis structure and IF5 Molecular Geometry
- PH3 Lewis structure and PH3 Molecular Geometry
- AsH3 Lewis structure and AsH3 Molecular Geometry
- AsCl3 Lewis structure and AsCl3 Molecular Geometry
- AsF3 Lewis structure and AsF3 Molecular Geometry
- NCl3 Lewis structure and NCl3 Molecular Geometry
- NF3 Lewis structure and NF3 Molecular Geometry
- NBr3 Lewis structure and NBr3 Molecular Geometry
- AlCl3 Lewis structure and AlCl3 Molecular Geometry
- AlF3 Lewis structure and AlF3 Molecular Geometry
- AlBr3 Lewis structure and AlBr3 Molecular Geometry
- CCl4 Lewis structure and CCl4 Molecular Geometry