NCl2+ is the halogenated covalent salt of N having a molar mass of 84.03 g/mol. Let us explain the NCl2+ lewis structure and covalent property in the following article.
The central N of NCl2+ is sp2 hybridized. It is a cation of nitrogen dichloride. The positive charge is present over the N center only. N makes two sigma bonds with two Cl and two lone pairs are present over N, so it carries one positive charge. The shape of the molecule is trigonal planar.
NCl2+ consists of two atoms N and Cl. So, the property of the molecule is depending on these two atoms. The bond angle of the molecule is perfect at 1200. Let us discuss some important topics of NCl2+ like lewis structure, valence electrons, and hybridization in the following section with proper explanations
1. How to draw NCl2+lewis structure?
Lewis structure of NCl2+ can give us a clear picture of the bonding nature of the molecule. Now we try to draw the lewis structure of NCl2+ in the following steps.
Counting the valence electrons
The total valence electrons for the NCl2+ is 18. This is the total number of valence electrons of an individual atom present. The valence electrons of N are 5 and for Cl are 7 because those numbers of electrons are present in the valence shell. One electron will be subtracted due to the positive charge.
Choosing the central atom
For every covalent molecule, it is very important to select the central atom, because the central atom can decide different properties. The central atom is to be chosen based on the electronegativity and size of the atom. O is the central atom here because it is less electronegative than Cl and larger.
Satisfying the Octet
We should check all the atoms present in the molecule obeys the octet rule. To follow the octet rule every atom present in the NCl2+ should complete its valence electron by a total number of eight electrons. So, they accept electrons to fulfill their octet and try to gain the noble gas electronic configuration.
Satisfying the valency
According to the octet, the total electrons required for NCl2+ are (8*3)-1 = 23. But the total valence electrons for the molecule are 18. So, the required number of electrons should be accumulated by the respective valency of atoms, 5/2 =2.5 bonds. N formed two single bonds and one positive charge.
Assign the lone pairs
N and Cl both contain lone pairs here. N has one and each Cl has three pairs of lone pairs. These lone pairs are the counting in the valence electrons but are not involved in the valency of the respective atoms. They only exist as non-bonded electrons.
2. NCl2+valence electrons
Valence electrons are present in the outermost or valence shell of every atom. Now we calculate the total valence electrons for NCl2+ in the following section.
The total valence electrons for NCl2+ are 18. This number is the summation of valence electrons of individual atoms present in the NCl2+. The valence electrons of each atom are counted by the electrons present in the valence orbital of each atom. For N and Cl, the outermost orbitals are 2s and 2p.
- Now we count the total valence electrons for NCl2+
- The valence electrons for N are 5
- The valence electrons for Cl are 7
- For the positive charge, there will be 1 electron subtracted from the total value.
- So, the total valence electrons for NCl2+ are 5+7+7-1 = 18.
3. NC2+lewis structure shape
The molecular shape is dependent on the VSEPR theory. Every molecule has its shape or geometry basis on the environment. Let us discuss the shape of NCl2+ in brief.
The molecular shape of the NCl2+ is trigonal planar. The geometry is thought to be about the same as NCl3, here one Cl is missing and the positive charge appears on the missing part of Cl. The central atom has three surrounded by two atoms and one vacant site is filled with lone pairs.
We can think of the molecule as AX3 type, so the best-fitted geometry for AX3 type molecule is trigonal planar as per VSEPR (Valence Shell Electrons Pair Repulsion) theory. One surrounded molecule will be replaced by the lone pairs of the N. There is no such repulsion present that the geometry will be changed.
4. NCl2+lewis structure angle
A bond angle is that angle that can be made by the atoms present in a molecule depending on the surrounding environment. Let’s discuss the bond angle of NCl2+ in detail.
The Cl-N-Cl bond angle is near about 1200. It is the best angle for a tri-coordinated molecule. Although it is not a tri-coordinated there is a lone pair present over the N and it can be thought of as a tri-coordinated molecule. So, the bond angle for trigonal planar geometry is 1200.
The bond angle is according to the geometry of the molecule. The best geometry for the molecule NCl2+ is trigonal planar. So, the bond angle for trigonal planar is 1200. There is no such lone pairs or bond pairs repulsion so there is no chance of deviation of the bond angle for the NCl2+ molecule.
5. NCl2+lewis structure lone pairs
Lone pairs are the non-bonded electrons present in the valence orbitals of the respective atoms of a molecule. Let us calculate the lone pairs over the NCl2+.
The lone pairs are situated over the N and Cl atoms. N has two more valence electrons after the two bond formation. Those two electrons are present in the valence shell of N and they exist as one pair of lone pairs. Again, for the Cl, they have six extra non-bonded electrons lie as lone pairs over each Cl.
- Let us calculate the total number of lone pairs over the NCl2+ calculated by the formula, lone pairs = valence electrons – bonded electrons.
- The lone pairs over the N atom = 4-2 = 2 (As N contains one positive charge)
- The lone pairs over the Cl atom = 7-1 = 6 (each Cl form one single bond)
- So, the total lone pairs present over the NCl2+ are 1+(3*2) =7 pairs of lone pairs.
6. NCl2+lewis structure formal charge
The formal charge is the hypothetical concept of every molecule to predict the appearance of charge within the molecule. Let us predict the formal charge of NCl2+.
The formal charge of NCl2+ cannot be zero. Because there is already a positive charge present over the molecule. With the help of the formal charge, we can be proved that the charge is present over N only not Cl. So, from the formal charge value, we can predict the charge of the molecule.
- The formula being used for the formal charge is, F.C. = Nv – Nl.p. -1/2 Nb.p.
- The formal charge present over the N atom is, 5-2-(4/2) = +1
- The formal charge over each Cl atom is, 7-6-(2/2) = 0
- So, from the above data, it is proved that the formal charge is present over the N atom only and the value is +1.
7. NCl2+lewis structure octet rule
The octet rule is completing the valence orbital by accepting a suitable number of electrons to gain stability like a noble gas. Let us talk about the NCl2+ octet.
The electronic configuration of N and Cl are [He]2s22p3 and [He]2s22p5 respectively. But here N is exist as N+, so one electron will be removed from its outermost 2p orbital. Now N has 4 electrons in 2s and 2p orbital. N and Cl both need eight electrons in their valence shell to complete the octet.
N needs 4 more electrons in its valence orbital to complete its octet. So, N shares two bonds with Cl via four electrons sharing and two electrons already present in the s orbital as non-bonded electrons. So, now it has six electrons and N does not complete its octet although it paired four electrons in its p orbital.
8. NCl2+lewis structure resonance
Resonance is the delocalization of excess electrons cloud within the molecule by the different skeleton forms of that molecule. Now discuss the resonance of the NCl2+.
There is no such resonance occurred in the NCl2+ molecule. As there is a lack of electrons in the central atom N. On the other hand, Cl is a more electronegative atom and it cannot lose electrons from its site. So, there is no such option for the elections of delocalized.
Resonance occurred in the anionic form of that molecule which is NCl2-. There will be excess electron density present over N which can be delocalized with Cl throughout the molecule. But here no resonance occurred although N and Cl are present in the molecule bearing a positive charge.
9. NCl2+hybridization
Hybridization is the mixing of the atomic orbitals to form a new hybrid orbital of equivalent energy. Let us discuss the hybridization of N in NCl2+.
From the below table we can predict the hybridization of N is sp2.
| Structure | Hybridization value | State of hybridization of central atom | Bond angle |
| 1. Linear | 2 | sp /sd / pd | 1800 |
| 2. Planner trigonal | 3 | sp2 | 1200 |
| 3. Tetrahedral | 4 | sd3/ sp3 | 109.50 |
| 4. Trigonal bipyramidal | 5 | sp3d/dsp3 | 900 (axial), 1200(equatorial) |
| 5. Octahedral | 6 | sp3d2/ d2sp3 | 900 |
| 6. Pentagonal bipyramidal | 7 | sp3d3/d3sp3 | 900,720 |
The s and p orbital of N are involved in the hybridization here. We can calculate the hybridization by the formula, H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, and M = monovalent atoms surrounded. From the above formula, the value is sp2.
10. Is NCl2+a solid?
Solid is a physical state of a molecule depending on the crystal structure or temperature. Let’s discuss whether NCl2+ is solid or not.
NCl2+ is liquid because the van der Waal’s force of attraction between atoms is moderate to stay it is in a liquid state at room temperature.
Why and how NCl2+ is not solid?
NCl2+ is not solid because the van der Waal’s force of attraction will be not so high. The entropy of the molecule is not zero. So, it can exist in liquid at room temperature.
11. Is NCl2+ soluble in water?
Polar or charge-containing species can be soluble in water. Let’s see whether NCl2+ is soluble in water or not.
NCl2+ is soluble in water, as it contains a charge over it. It can be ionized in the water solution, resulting in soluble in water. Although it is polar it has a solubility in water by the ionic interaction.
Why and how NCl2+ is soluble in water?
NCl2+ is soluble in water because it is a polar molecule. The N-Cl bond is much polar and can be dissociated in the water solution and gets dissolved. Although there is a charge present over the molecule, so there will be an ionic interaction occurring between water and the cation making it water-soluble.
N is electronegative and the size is also small, so it can easily form H-bonding with a water molecule. Due to this H-bonding, it makes it more soluble in water.
12. Is NCl2+ polar or nonpolar?
The polarity of a molecule depends on the dipole-moment value and the difference in electronegativity. Let’s see if NCl2+ is polar or not.
NCl2+ is polar due to there is a permanent dipole-moment value is present. Also, there is an electronegativity difference observed between N and Cl, which makes the N-Cl bond more polar. The positive charge present over the molecule also makes it polar.
Why and how NCl2+ is polar?
The permanent dipole moment makes the NCl2+ polar. Now discuss the polarity of NCL2+ in brief.
There is a dipole-moment flow from less electronegative N to more electronegative Cl atoms. The direction of the dipole moment is not opposite and the magnitude is equal, so there is no chance of canceling out the dipole moment. So, in the NCl2+ molecule, there is observed a permanent dipole-moment value.
13. Is NCl2+a molecular compound?
A molecular compound is the combination of two or more atoms maintaining the proper valency of each atom. Now see whether NCl2+ is a molecular compound or not.
NCl2+ is a molecular compound because there is a combination of N and Cl atoms. Here the valency of the N as well as Cl is maintained properly. The property of the NCl2+ is not similar to N or Cl and this is the sign of a compound. Also, molecular compounds are held by the covalent bond between two atoms.
Why and how NCl2+ is a molecular compound?
NCl2+ is made by the fixed ratio of N and Cl by 1:2. This ratio is fixed and also N and Cl both maintained their respective valency here. To maintain the trivalency of N here a positive charge is also added. NCl2+ is consist of the covalent interaction of N and Cl, which makes it a compound.
The stable mono-valency of Cl is also maintained here by the forming of one single bond.
14. Is NCl2+ an acid or base?
Acidity or basicity is depending upon the ability to release the proton or OH– in an aqueous solution. Let us see whether NCl2+ is acid or base.
NCl2+ is neither acid nor base according to the Arrhenius theory. It could not be released H+ or OH– in an aqueous solution. Because it has not any acidic proton or OH– for donating. But we can predict its acidity according to lewis’s acid-base concept.
Why and how NCl2+ is a lewis acid?
Accepting electrons ability makes NCl2+ lewis acid. Now explain the lewis acidity of NCl2+ in the following section.
The N contains a positive charge in NCl2+, so it is lack electrons. So, N can accept the extra electron density of lone pairs from the suitable lewis base. After accepting an electron, N will be stabilized so the process of accepting of electron for N is favorable and makes the NCl2+ lewis acid.
15. Is NCl2+ an electrolyte?
The species can get dissolved in water to ionize and carry electricity is known as electrolyte. Let us talk about whether NCl2+ is an electrolyte or not.
NCl2+ is an electrolyte. It can soluble in water and get dissolved to ionize to respective cation and anion. So, the solution becomes charged and can conduct electricity very easily. The process of ionization of NCl2+ in water is very fast and makes a strong electrolyte.
Why and how NCl2+ is a strong electrolyte?
Strong electrolytes are those electrolytes that can be ionized in water very fast and conduct electricity. Now discuss the NCl2+ about its strong electrolytic nature.
NCl2+ also carries a positive charge so it can be ionized in water in a very faster way to form N+ and Cl–. The magnitude of those cation and anion is very high and the mobility of the ions is also very fast. So, it can carry electricity very faster way.
The higher the charge density, the higher the ion’s mobility and the stronger the electrolytic nature will be.
16. Is NCl2+ a salt?
Salt is formed by the ionic interaction of the cation and anion and conducts electricity. Now learn about the NCl2+ whether it is salt or not.
NCl2+ is a salt because it can conduct electricity in an aqueous solution, although there is weak ionic interaction occurred between N and Cl. NCl2+ is a covalent compound rather than salt. But it has some properties similar to salt.
Why and how NCl2+ is salt?
NCl2+ can be ionized and get dissolved in water to carry electricity. Although it is a covalent molecule the charge present makes it ionic and for this ionic interaction, it can behave as a salt.
17. Is NCl2+ ionic or covalent?
No molecule is purely covalent, it has some ionic character depending on its ionic potential – Fajan’s rule. Now discuss the ionic or covalent nature of NCl2+ in brief.
NCl2+ is a covalent molecule. It can form by the electrons shared between N and Cl atoms. Sharing the electrons makes the bond between N and Cl covalent in nature, although it carries a positive charge.
Why and how NCl2+ is covalent?
The bond between N and Cl is formed by the shared electrons. Now discuss the covalent nature of NCl2+ in the following section.
The ionic potential of N is not so high and the polarizability of Cl is also lower. So, it cannot be polarized properly. Although there is a charge present over the N that makes the molecule partial ionic but nature of the bond makes the molecule pure covalent.
18. Is NCl2+ protic or aprotic?
Species that carry an H atom able to form H-bonding with another subsequent are called protic. Now talk about whether NCl2+ is protic or aprotic.
NCl2+ is aprotic because it does not contain any proton or H atom in the molecule. So, it is unable to form H-bonding with another subsequent. Mainly protic molecules will be polar but polar molecules are not necessarily protic.
Why and how NCl2+ is aprotic?
Absence of proton makes a molecule aprotic. Let us discuss the aprotic nature of NCl2+.
There is no proton present over NCl2+, so it is aprotic but due to its small size and higher electronegativity of N, it can able to form H-bonding with protic solvent or polar molecule. But NCl2+ is itself an aprotic but can form H bonding with water molecule makes water-soluble.
19. Is NCl2+ a strong or weak nucleophile?
Nucleophiles are those substances that can donate electrons to an electron-deficient site or can react with electrophiles. Now see whether NCl2+ is nucleophile or not.
NCl2+ is not a nucleophile. It does not contain extra electron density that can be donated to the electron-poor site. Rather it can accept an electron from the nucleophile and acts as an electrophile. It is a strong electrophile in the case of electron-accepting reactions.
Why and how NCl2+ is a strong electrophile?
Electrophiles are those species having electron acceptor sites and can accept electron density from the nucleophile. Let us discuss the electrophilicity of NCl2+.
NCl2+ is a strong electrophile because the positive charge present over N makes a more electron deficient center. So, it can accept an electron from the electron-rich center or from the suitable nucleophile in any organic reaction.
Again, electronegative Cl atoms pull electron density from the N site, so it becomes a more electron deficient center and also makes a strong electrophile.
Conclusion
NCl2+ is an sp2 hybridized molecule having geometry trigonal planar. It is the cationic form of the NCl3 molecule. NCl2+ is a lewis acid and a strong electrophile. So, in an acid-base reaction or any organic reaction, it can participate.
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Hi……I am Biswarup Chandra Dey, I have completed my Master’s in Chemistry from the Central University of Punjab. My area of specialization is Inorganic Chemistry. Chemistry is not all about reading line by line and memorizing, it is a concept to understand in an easy way and here I am sharing with you the concept about chemistry which I learn because knowledge is worth to share it.