NH2F Lewis Structure& Characteristics: 17 Complete Facts


NH2F or fluoroamine, an analogous compound to monochloroamine, is an unstable gas with molar mass 35.021 g/mol. Let us explore the structure and some relevant facts about NH2F.

NH2F has a trigonal pyramidal geometrical structure with sp3 hybridization. It possesses bond angle slightly lesser than 109.50 with a permanent dipole moment. Due to presence of three covalent bonds between nitrogen and fluorine, it is considered as a covalent compound.

Let us discuss the shape, structure with some important characteristics briefly.

How to draw NH2F lewis structure?

Lewis structure is a structural representation in which nonbonding electrons are shown as the electron dots around each of the participating atoms. Let us discuss it in detail.

Determination of valence electrons:

The outer most shell electrons are considered as valence electrons. Nitrogen, hydrogen and fluorine have five, one and seven electrons in their outer most shell.

Finding out the bonding electrons:

In NH2F, total three covalent bonds are present. Therefore, (3×2) = 6 electrons are considered as bonding electrons.

Finding out the nonbonding electrons:

Rest of the electrons which are not involved in bonding, is regarded as nonbonding electrons. Nitrogen has two and each of the two fluorine has six electrons left as nonbonding.

NH2F Lewis Structure Resonance

Resonance structures are sets of lewis structures which shows the delocalization of electrons between the atoms. Let us discuss about it.

Different resonance structures of NH2F are not possible because none of the participating atoms (N,H,F) have any energetically accessible vacant orbital. The lone pairs of nitrogen cannot be delocalized with fluorine as well as hydrogen because F has 2p5 and H has 1s1 electron configuration.

Minimum one vacant orbital is required to accommodate the electron pairs. Therefore, nitrogen also cannot accept electron pairs from fluorine because it has already 2p3 electron configuration and has no vacant place for the electron pairs coming from fluorine.

NH2F Lewis Structure Shape

Lewis structure shape is the three-dimensional arrangement of the atoms present in the molecule. Let us talk about it in detail.

The shape of NH2F lewis structure is trigonal pyramidal with the tetrahedral geometry. The lone pairs of nitrogen deviate the shape of NH2F from its ideal geometrical structure.

The shape of NH2F is involved in these following repulsions-

  • Lone pair-lone pair repulsion – Nitrogen has only one lone pair. So, lone pair-lone pair repulsion is not applicable for NH2F.
  • Lone pair-bond pair repulsion – The lone pair of nitrogen and the N-F with two N-H bonding electrons face repulsion from each other and the shape is distorted from its ideal geometrical structure. Therefore, it shows trigonal pyramidal shape rather than tetrahedral shape.
Shape of NH2F

NH2F Lewis Structure Formal Charge

Calculation of formal charge is very much significant in chemistry because it helps to determine the most stable lewis structure. Let us calculate the formal charge.

The calculation of NH2F ‘s formal charge is = Total number of valance electrons – number of electrons remain as nonbonded – (number of electrons involved in bond formation/2).

  • Formal charge of nitrogen = 5 – 2 – (6/2) = 0
  • Formal charge of fluorine = 7 – 6 – (2/2) = 0
  • Formal charge of each of the hydrogen = 1 – 0 – (2/2) = 0

NH2F Lewis Structure Angle

Bond angle is defined as the angle between two covalent bonds connecting central atom. Let us determine the bond angle in NH2F.

The bond angle of NH2F Lewis structure is nearly equals to 109.50 as the central atom, nitrogen is sp3 hybridized. The bond angle should be exactly 109.50 but the lone pair of nitrogen deviates the bond angle from 109.50 and show slightly lesser than the ideal bond angle.

The nonbonding electrons of nitrogen face repulsion from the N-F and N-H bonding electrons. Thus, the bond angle is deviated from its ideal bond angle. NH2F can possess its actual bond angle according its sp3 hybridization in absence of any lone pair in central atom.

NH2F Lewis Structure Octet Rule

Octet rule states that any atom should possess electron configuration (8 electrons in valence shell) like its nearest noble gas. Let us discuss it.

All the atoms in NH2F lewis structure except hydrogen obeys octet rule in this way-

  • Nitrogen obeys octet rule. It has five electrons in its n=2 orbital. After three covalent bond formation with two hydrogen and one fluorine atom, it gains three more electrons and the number of total electrons in its valence shell becomes eight.
  • Fluorine has seven valence electrons and when it forms covalent bond with nitrogen, it also gets eight electrons in its outer most shell. Therefore, octet rule is also satisfied for fluorine.
  • Hydrogen does not obey octet rule because it cannot accommodate eight electrons in its 1s orbital. Rather it can have two electrons after formation of one covalent bond which resembles with its nearest noble gas, helium.

NH2F Lewis Structure Lone Pairs

Lone pairs are the rest of the valence electrons which have no contribution in bond formation.

Nitrogen and fluorine have lone pairs in NH2F lewis structure. Number of lone pairs can be determined by using the following formula- Formula of calculation of nonbonded electron is = Total number of valance electron – number of bonded electrons.

  • Nonbonding electrons of nitrogen = 5 – 3 = 2
  • Nonbonding electrons of fluorine = 7 – 1 = 6
  • Nonbonding electrons of hydrogen = 1 – 1 = 0
  • Therefore, total number of lone pairs in NH2F is = 6 + 2 = 8

NH2F Valence Electrons

Valence electrons are the outer most shell electrons of any atom and most reactive due to having lesser attraction force of nucleus. Let us explain it.

The valence electrons of NH2F are actually the outermost shell electrons of nitrogen, fluorine and hydrogen. Nitrogen, fluorine and hydrogen contains five, seven and one electrons in their respective valence shell. Therefore, total number of valence electrons in NH2F is {5 + 7 +(2×1)} = 14.

Nitrogen and fluorine have electron configuration 1s2 2s2 2p3 and 1s2 2s2 2p5 respectively. The 2s and 2p electrons are considered as valence electrons. Due to having only one electron in hydrogen, that electron is counted as valence shell electron of hydrogen.

NH2F Hybridization

Mixing of two atomic orbitals to generate a new orbital for the purpose of chemical bond formation is defined as hybridization. Let us discuss it in detail.

The hybridization of the central atom, nitrogen in NH2F is sp3. Four electrons from 2s and 2p orbitals participate in sp3 hybridization with the valence electrons of hydrogen and fluorine. NH2F attains the trigonal pyramidal shape due to the sp3 hybridization of central atom.

According to sp3 hybridization molecular shape should be tetrahedral. But due to presence of lone pair in central atom, it is deviated from its actual structure and shows trigonal pyramidal shape.

Is NH2F soluble in water?

Solubility of any molecule in a particular solvent depends upon the nature of the solute as well as solvent. Let us explore it.

It is considered that NH2F is soluble in water. Water is a polar solvent and fluoroamine is also a polar molecule.

Why NH2F is soluble in water?

To become soluble in a solvent, the nature of solute and solvent should be same. Let us discuss it.

NH2F is soluble in water because both water and NH2F is polar in nature. As polar solute always dissolves in water, thus, NH2F is dissolved in water due to having polar nature.

How NH2F is soluble in water?

Polar solute dissolves in a polar solvent through an interesting mechanism. Let us talk about this.

NH2F can be dissolved in water because the negative part of NH2F like nitrogen and fluorine get solvated by the positive end of water like hydrogen end. Whereas the hydrogen in NH2F gets hydrated by the oxygen end of water.

Is NH2F an acid or base?

Acidity and basicity of any molecule depends upon the capability of accepting or donating electron pairs respectively. Let us determine the acidity or basicity of NH2F.

NH2F is basic in nature. It can donate its nonbonding electrons to the vacant orbital of any atom, considered as lewis acid. Therefore, NH2F is a lewis base.

Why and how NH2F is basic in nature?

Lewis base is defined as those who can donate their nonbonding or excess electrons. Let us talk about this.

NH2F is a lewis base because nitrogen has nonbonding electrons which are not involved in bonding. Those electrons can be donated to such molecule or atom who has vacant orbital.

Is NH2F an electrolyte?

Electrolyte are those who can conduct electricity as a result of dissociation in positive and negative ions. Let us explain it.

NH2F is not an electrolyte as it is not an ionic compound and it cannot be dissociated into positive and negative ions.

Why and how NH2F is not an electrolyte?

Non-electrolytes cannot be dissociated into two oppositely charged ions when dissolved in water. Let us comment on it.

NH2F is not an electrolyte as when it is dissolved in water, the resultant aqueous solution does not contain any ions. This aqueous solution also does not conduct electricity due to no dissociation in any ions.

Is NH2F ionic or covalent?

Ionic and covalent bonds are formed due to permanent transferring of electrons and sharing of electrons between the atoms. Let us discuss it.

NH2F is a covalent compound as it contains three covalent bonds between nitrogen, fluorine and hydrogen atoms. Electrons are shared, not completely transferred between the atoms depending upon the electronegativity of respective atoms.

Why and how NH2F is a covalent compound?

Covalent bonds involve the sharing of electrons between atoms. Let us discuss the reason of being a covalent compound.

NH2F is covalent because the electrons between nitrogen, fluorine and hydrogen are mutually shared between them. Bonding electrons are not shared equally between the atoms due to having differences in electronegativity of nitrogen, hydrogen and fluorine.

The bonding electrons of two N-H bonds are shifted towards nitrogen side because of the greater electronegativity of nitrogen. Whereas the N-F bonding electrons are shifted towards fluorine as fluorine has greater electronegativity than nitrogen.

Conclusion

NH2F is a very much unstable gaseous compound. A lot of facts and uses about NH2F are still left to be discovered. Different type of scientific research is continuing with this compound and in future it will be considered as one of the most useful compounds.

Aditi Roy

Hello, I am Aditi Ray, a chemistry SME on this platform. I have completed graduation in Chemistry from the University of Calcutta and post graduation from Techno India University with a specialization in Inorganic Chemistry. I am very happy to be a part of the Lambdageeks family and I would like to explain the subject in a simplistic way. Let's connect through LinkedIn-https://www.linkedin.com/in/aditi-ray-a7a946202

Recent Posts