Nitrogen and oxygen base compounds are very different in nature. Nitronium ion has the chemical formula NO2+. All atoms belong to the non-metal family groups in the periodic table and possess a high electronegativity value. Students used to ask “Is NO2+ polar or nonpolar?”, “NO2+ Lewis Structure”, “NO2+ molecular geometry”, “NO2+ bond angle”, and “NO2+ polarity”. In this blog post, we are going to discuss the polarity of NO2+ ions in a detailed manner.
NO2+ is commonly appearing at ordinary temperatures and pressures, it exists as a gas with stable salt form. NO2+ contains one nitrogen atom, cation resonate on nitrogen, and two oxygen atoms. Nitronium ion (NO2+) is corrosive to biological tissue and metals, and it can induce a corrosive effect on metal, nitrate the cotton, and other organic materials. The nitrogen atom stays the center of the molecule ion and the remaining two oxygen atoms. “Is NO2+ polar or nonpolar?”, to answer this question, we need a detailed analysis of the polarity of the NO2+ molecule.
Because of the linear structural form of nitronium ion (NO2+). 0xygen has atomic number 8 in the modern periodic table and six outermost valence shell electrons. It comes under the oxygen family group. Similarly, nitrogen has atomic numbers 7 and five outermost valence shell electrons. It contains a +1 charge on the nitrogen dioxide molecular species.
NO2+ molecule ion species are formed by elements of the nitrogen and oxygen family group in the periodic table. When NO2+ ion is exposed to air, it absorbs water quickly and produces white vapors that have a distinct odor and are toxic to breathe. nitronium ion (NO2+) can generate nitric acid when it reacts with water and undergoes hydrolysis.
Is NO2+ polar or nonpolar, then? nitronium (NO2+) is nonpolar due to its linear geometrical shape caused by the presence of the two oxygen atoms, opposite to each other. Second, the difference in electronegativity between nitrogen and oxygen atoms causes the N-O bonds to become polar, causing the entire molecule ion to become nonpolar as well, resulting in a net dipole moment of the NO2+ molecule is 0 D.
Preparation of NO2+ ion
Nitronium ion(NO2+) is a bright yellow color liquid with a strong intense odor. It is created primarily through the mixing of sulphuric and nitric acid. It is the homogeneous reaction, mixing of concentrated sulfuric acid and nitric acid. Initially, This gives hydrogen sulfate and nitronium ion(NO2+). A nitronium ion is known as an electrophile. This first reaction step is exothermic in nature.
The chemical equation of mixing of concentrated sulfuric and nitric acid, exothermic reaction is shown below.
H2SO4 + HNO3 → HSO−4 + NO+2 + H2OPreparation of nitronium ion(NO2+)
NO2+ Molar Mass Calculation
NO2+ has a molecular mass of 46.005 g·mol−1, which may be computed as follows.
Mol mass of NO2+ = 1 * 14 (atomic mass of N) + 2 * 16 (atomic mass of O) = 46.005 g·mol−1.NO2+ molar mass calculation
The chemical composition of the nitrogen dioxide ion(NO2+) molecule is 2 oxygen atoms and a positive charge resonates on the nitrogen atom in the middle.
NO2+ Lewis Structure: Is NO2+ polar or nonpolar?
The core atom is nitrogen, which is flanked by two oxygen atoms. nitrogen contains five outermost valence electrons, which means it contains five electrons in its outermost shell, whereas oxygen has six outermost electrons. An oxygen atom is required two electrons to complete the octet of oxygen atoms. If you want to know about the octet rule, please see in our previous post.
As a result of this, both two oxygen atoms form covalent bonds with the nitrogen atom, leaving the nitrogen atom with a positive charge. The double bond pairs of N–O are linear in nature by the positive charge on the nitrogen atom. According to VSEPR theory, a positive charge resonating on nitrogen causes the molecule’s shape to linear.
The positive charge resonating on NO2+ ion both two N-O bonds linear, resulting in the linear form of the NO2+ molecule. Because they generate electrical repulsion among the NO2+ molecule, Resonating positive ions on NO2+ have shaped NO2+ in a linear structure.
Electronegative difference calculation NO2+:
When it comes to the electronegativity value of the NO2+ molecule, Oxygen has an electronegativity of 3.44, while nitrogen has an electronegativity of 3.04. The electronegativity difference of the N-O bond in NO2+ molecule can be calculated by the following method.
Electronegativity value of oxygen = 3.44
Electronegativity value of nitrogen = 3.04
Difference of electronegativity value between nitrogen and oxygen = 3.44- 3.04=0.40Electronegativity difference calculation of NO2+ molecule
The N-O bond of the NO2+ molecule becomes nonpolar in nature due to this difference in electronegativity value. The power with which an atom can attract bound electron pairs towards its side is known as the electronegativity of the atom.
As a result of this, the dipole moment of the N-O bond is near zero, and the dipoles of both N-O bonds are negated due to the linear structure of the NO2+ molecule. The total dipole moment of the NO2+ molecule is calculated to be 0 D. Nitrogen atoms receive a positive charge on it, while oxygen atoms receive a partial negative charge on it.
NO2+ molecule’s electron dot structure is also known as NO2+ Lewis structure. It determines the number of outermost valence electrons and the electrons involved in the formation of the NO2+ molecule’s bonds. When discussing the Lewis structure of the NO2+ molecule, it is necessary to understand the outermost valence electrons of NO2+ ion.
Nitrogen is the middle element of the molecule, with five electrons in its outermost valence electron shell, while the oxygen atom is the outermost valence electron shell, with six electrons and two electrons missing in the shell to complete its octet.
As a result of this above explanation, the NO2+ molecule contains a total of 16 valence electrons. The two oxygen atoms establish covalent connections with the nitrogen atom, leaving the nitrogen atom with the resonating positive charge on it.
The resonating positive charge of nitrogen atoms causes repulsion and stability with N-O bond pairs, causing the N-O bonds to linear structure and the shape of the molecules resonating between nitrogen and oxygen. The 0-N-O bond has a bond angle of roughly 180 degrees. N-O bond has a bond length of 115 pm (picometer).
To sketch the NO2+ Lewis structure by following these instructions:
Step-1: Determine the total number of outermost valence shell electrons in the NO2+ molecule. The first step is to figure out how many outermost valence shell electrons there are in the NO2+ Lewis structure. A valence electron is one of an atom’s outermost shell electrons. In the Lewis diagram, it is represented by dots. The central nitrogen atom of the NO2+ molecule can be represented as follows
Look for the periodic group of each atom in NO2+ to determine its valence electron. Nitrogen and oxygen are both members of the nitrogen and oxygen family, which is the 15th and 16th groups in the periodic table respectively. Nitrogen and oxygen have five and six valence electrons in their outermost shell respectively.
Because nitrogen and oxygen belong to the nitrogen and oxygen family group in the periodic table, their valence electrons are five and six respectively.
Total outermost valence shell electron of oxygen atom in NO2+ = 6
Total outermost valence shell electron of the nitrogen atom in NO2+= 5
The NO2+ molecule has one central nitrogen atom 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) = 6 + 5*2 = 16 valence electrons in NO2+calculation of total valence electron of NO2+ molecule
Step-2: Locate the atom with the least electronegative charge and place it in the center of the NO2+ molecular geometry. In this phase, we’ll select the least electronegative atom in the NO2+ molecule to place in the Lewis structure diagram’s center. In the periodic table, the electronegativity value increases in order from left to right and decreases in order from top to bottom in periodic groups.
As a result, Oxygen is the first atom in the oxygen family group in the periodic table. The nitrogen atom comes as the first element in the nitrogen family group. A nitrogen atom has a lower electronegative value than an oxygen atom. Furthermore, because oxygen is the most electronegative element in NO2+ molecule, it can never be the central atom in a NO2+ Lewis structure diagram. As a result of this, place nitrogen at the center of the NO2+ Lewis structure, with oxygen uniformly around the two terminals of linear NO2+ molecule.
Step-3: Use two double bonds (N-O) to connect the outside and core atoms in the NO2+ molecule. Connect all outside atoms (oxygen) to the core central atom (nitrogen) with two double bonds in this stage.
Count how many outermost valence shell electrons we’ve used so far in the NO2+ structure. Because each nitrogen atom is connected to an oxygen atom by two double (N-O) bonds, each connection contains four electrons. Those are called bond pairs of double bonds.
So, from the total of 16 valence electrons available for the NO2+ Lewis structure, we employed 8 electrons for two double (N-O) bonds in the NO2+ molecule. There are still 8 valence electrons left in the NO2+ molecule. Where do we need to place them in NO2+ molecular geometry?
Step-4: Starting with the outer two oxygen atoms in the NO2+ molecule, place the remaining valence electrons. We always start inserting valence electrons from the exterior oxygen atom first in the Lewis structure diagram. As a result, first, wrap around the leftover valence electrons on each oxygen atom.
To complete its octet, oxygen requires 8 electrons in its outermost valence shell. With the help of a double bond, each oxygen already shares four electrons. Put 4 electrons around each oxygen atom and you’re done with the oxygen atoms in NO2+ molecule.
In the NO2+ molecule structure above, we’ve put 8 electrons around the oxygen atoms, represented by a dot. As all oxygen atoms have 8 electrons in their outermost valence shell, each oxygen atom comfortably completes its octet stability in the NO2+ molecule.
Using the Lewis structure, count how many outermost valence shell electrons have been consumed so far. In the NO2+ molecular structure, 16 electrons are represented as dot structure, whereas two double bonds each contain 4 electrons. As an outcome of the calculation, the outermost valence shell electrons are 8 + 8= 16.
So far, we’ve used 16 of the total 16 outermost valence shell electrons available for the NO2+ Lewis structure. But now the question is, “How to fix the remaining four valences in nitrogen atom?”. We also have four valences in the central nitrogen atom to spare in the NO2+ molecule.
Step-5: Complete central nitrogen atom octet and use covalent bond if necessary. In the NO2+ Lewis structure, nitrogen is the central atom and it is connected with two double bonds (N-O) to the oxygen atoms. It means it already sharing 8 electrons with the help of 2 double bonds.
So, Nitrogen is obeying the rule of the octet with 8 electrons around it. Place the resonating positive charge around the nitrogen center atom, which is acting as an octet stabilization in this case.
What are NO2+ electron and molecular geometry?
NO2+ has a linear molecular geometry and resonating electron geometry, according to the VSEPR theory. Because the core central atom, nitrogen, has two N-O bonds with the surrounding two oxygen atoms. In the same plane, the O-N-O bond forms a 180-degree angle. Because two oxygen atoms are in the same plane, they form a linear shape.
Above that plane, there is a positive charge on nitrogen. It maintains the linear-like form after connecting the resonating charges along with the NO2+ molecule form. The bond pair is located just opposite to central nitrogen atom in the linear geometry. The positive charge on the nitrogen atom resonating in the linear NO2+ molecule.
Because of the resonating positive charge, it gives linear electron geometry. But the NO2+ molecular geometry is a linear form in nature. It is the symmetrical geometry of the NO2+ molecule. That makes, NO2+ molecule is nonpolar.
How to find NO2+ molecular geometry
- Determine the number of lone pairs on the NO2+ Lewis structure’s core Nitrogen atom.
We need to figure out how many lone pairs there are on the central nitrogen atom of the NO2+ Lewis structure because the lone pairs on nitrogen are primarily responsible for the linear NO2+ molecule geometry.
Use the formula below to find the lone pair on the NO2+ molecule’s center nitrogen atom.
L.P(N) = V.E(N) – N.A(N-O)/2
Lone pair on the central nitrogen atom = L.P(N )
The core central nitrogen atom’s valence electron = V.E(S)
Number of N-O bonds = N.A (N-O)calculation for nitrogen atom lone pair in NO2+ molecule
In the case of NO2+, the center atom, nitrogen, has four outermost valence shell electrons(positive charge on it)and two oxygen atoms(double bond) connected to it.
As a result of this, L.P(S) = (4 – 4)/2=0
The lone pair on the center nitrogen atom of the NO2+ electron geometry structure is equal to zero. It means, the central nitrogen atom contains no lone pairs.
- Determine the number of NO2+ molecular hybridizations.
How to find the hybridization of the NO2+ molecule?. Now we need to figure out what NO2+ molecular hybridization number is.
The formula of NO2+ molecular hybridization is as follows:
No. Hyb of NO2+ = N.A(N-O) + L.P(N)
No. Hy= the number of hybridizations of NO2+
Number of N-O bonds = N.A (N-O)
Lone pair on the central nitrogen atom = L.P(N)Calculation for hybridization number for NO2+ molecule
Nitrogen, then, is a central atom with two oxygen atoms linked to it and no lone pairs in the NO2+ molecule. Then the number of hybridization of NO2+ (No. Hyb) can be calculated as follows
No. Hyb of NO2+= 2+0 =2
The number of hybridization for NO2+ molecule is two. one S orbital, and one p orbitals combine together to form the sp hybridization.
3. Use VSEPR theory to determine NO2+ molecular geometry shape
When the VSEPR theory is utilized to calculate the shape of the NO2+ molecule, the AXN approach is typically used.
The AXN notation is as follows:
The center nitrogen atom in the NO2+ molecule is denoted by the letter A.
The bound pairs (N-O) of electrons to the core atom are represented by X.
The lone pairs of electrons on the center nitrogen atom are denoted by the letter N.Notation for NO2+ molecular geometry
We know nitrogen is the center atom with two bound (N-O) pairs of electrons and zero lone pairs. because of the NO2+ Lewis structure. NO2+ has the general molecular geometry formula AX2.
If the molecule has an AX2 generic formula, the molecular and electron geometry will be linear form, according to the VSEPR theory.
|Name of Molecule||Nitronium ion|
|Chemical molecular formula||NO2+|
|Molecular geometry of NO2+||linear form|
|Electron geometry of NO2+||Linear resonance structure|
|Hybridization of NO2+||SP|
|Bond angle (O-N-O) and Bond order||180º degree and 2|
|Total Valence electron for NO2+||16|
|The formal charge of NO2+ on nitrogen||+1|
How to calculate the formal charge in NO2+ Lewis Structure?
The formal charge on the nitrogen central atom of the NO2+ molecule often represents the actual charge on that nitrogen central atom. The formal charge will be found on the central nitrogen atom of the NO2+ Lewis dot structure in the following calculation.
To calculate the formal charge on the central nitrogen atom of 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 (S) = Valence electron in nitrogen atom of NO2+ molecule
L.E(S) = Lone pairs of an electron in nitrogen atom of NO2+ molecule.
B.E = Bond pair electron in N atom of NO2+ moleculecalculation of formal charge on nitrogen atom in NO2+ molecule
We have 5 valence electrons, 0 lone pair electrons, and eight bonding electrons in the nitrogen central atom (two double bonds attached to oxygen) of the NO2+ molecule. Now put these value of the nitrogen atom in the above formula
Formal charge on nitrogen atom of NO2+ molecule = (5- 0-(8/2)) =+1
The formal charge on central nitrogen atom of NO2+ Lewis structure is +1.
Dipole moment of NO2+
The dipole moment of the NO2+ molecule can assist us in determining the polarity’s strength. The polarity of any molecule is proportional to its dipole moment of bonds. Because the form of NO2+ is symmetric. The dipole moment of NO2+ does cancel each other as a result of this.
The dipole moment of NO2+ can be calculated as follows
D(N-O) = Q(N-O) * R(N-O)
D(N-O) = Dipole moment of N-O bond in NO2+ molecule
Q(N-O) = Charge distribution in N and O atom of NO2+ molecule
R(N-O)= Bond length of N-O bond in NO2+ moleculeDipole moment calculation of NO2+ molecule
Net dipole moment of NO2+ molecule is 0 D.
Why is NO2+ polar molecule?
Due to the existence of resonating positive charge on the nitrogen atom, the nitronium ion (NO2+) molecule has a linear structural form. According to the VSEPR hypothesis, zero lone pairs on nitrogen and bond pairs stabilize with each other, causing the N-O bonds to form the linear molecular structure, resulting in a linear shaped NO2+ molecule.
The dipole moment of N-O bonds does cancel out as it does in symmetric NO2+ molecules. NO2+ has a dipole moment of 0 D across the entire molecule. The formation of a nonpolar molecule is caused by the geometrical structure and the difference in electronegativity value of atoms in the NO2+ molecule.
Because of the symmetric shape of the NO2+ molecule, the positive charge is dispersed uniformly resonating among the nitrogen and oxygen atoms, resulting in the formation of positive and negative poles resonating across the NO2+ molecule.
Properties of NO2+
The properties of NO2+ molecule are listed below
- NO2+ has a molar mass of 46.005 g/mol.
- It is soluble in non-polar solvents but not polar solvents. Non-polar solvents include benzene, carbon tetrachloride, and others, while polar solvents include water, ammonia, and others.
- NO2+ gas is extremely poisonous and can cause death in humans.
- The nitrogen atom has a high electrical affinity due to its +1 charge and is utilized as an electrophoresis reagent in the titration process.
Uses of Nitronium ion (NO2+)
The uses of nitronium ion are listed below
- In the nitration process, it acts as an electrophile.
- NO2+ is used to make fertilizers like slurry, worm castings, and peat, among other things.
- It’s used to make fluorinated nitrile (NO2F) and nitrile chloride, which are both commercially accessible salts (NO2Cl).
- It loves electron in the reaction. It is called an electrophile reagent.
Because of its strong electron affinity, NO2+ (Nitronium ion) is a linear molecule and an electrophile in an organic reaction. Oxygen atoms are more electronegative than nitrogen atoms in the NO2+ ion. As a result, the NO bond is slightly polar, but the dipoles in opposite directions cancel each other out due to the symmetric linear geometry of NO2+, resulting in a net-zero dipole moment for the entire NO2+ molecule. As a result, NO2+ (Nitronium ion) is nonpolar.
It showed the sp molecular hybridization. The O-N-O bond angle of NO2+ is 180 degrees. The N-O bond length of NO2+ is 115 pm. It has a positive resonating charge on NO2+ molecules.
If you have any doubts and queries on this post, please leave comment. We will reply back as soon as possible.
FAQ on “Is NO2+ polar or nonpolar?”
What is the shape of NO2+?
The molecule NO2 is twisted, but when an electron is removed from it, making it NO2+, the molecule becomes linear due to the loss of a single electron. There is no repulsion between the two O atoms and the single electron on the centre atom in NO2+.
Is NO2+ polar or nonpolar atom closest to negative side?
NO2+ is a nonpolar molecule with the Oxygen atom closest to the negative side because Oxygen’s electronegativity value (3.44) is higher than Nitrogen’s (3.04), causing Oxygen atoms to attract an electron from the Nitrogen atom, resulting in a partial positive charge on the Nitrogen atom and a negative charge on the Oxygen atoms.
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