NH3BF3 Structure & Characteristics (13 Helpful Facts)

Ammonia Trifluoroborane or NH3BFare a chemical compound. Let us study the fact about NH3BF3 in more detail.

Ammonia Trifluoroborane(NH3BF3) belongs to the borane-nitrogen-hydride family. The molecular weight of NH3BF3 is 84.84g/mol. Azaniumyl(trifluoro)boranuide is the IUPAC name for NH3BF3.

Let us discuss some other facts like hybridisation, valence electrons, structure, polarity and lewis structure of NH3BF3 in more detail below.

How to draw NH3BF3 structure?

Lewis structures use the chemical symbol for each atom to show where it is located within the molecule’s structure. Let us draw the step of the lewis structure of NH3BF3.

Count the valence electron in NH3BF3:

In total, NH3BF3 has 32 valence electrons. Boron has 3 valence electrons (1s22s1), Fluorine has 7 valence electrons (2s22p5), Nitrogen has 5 valence electrons (2s22p3), and H has 1 (1s1). The sum of the valence electrons is 32 (5 + 3 + 3 + 21).

Select the central atom in NH3BF3:

Two central atoms, one each of nitrogen and boron, are present in NH3BF3. Atoms in the surroundings include hydrogen and fluorine. As a result, this molecule is stable by dative bonding.

Complete the octet of NH3BF3:

In NH3BF3, NH3, N has 3 single bonds to H and 1 pair of electrons, filling its octet. In BF3, F completes their octets by forming 3 single bonds with B, whereas B is unable to complete its octet. Therefore, B needs 2 more electrons to complete the octet. Atoms of boron follow a sextet rule.

Draw the final NH3BF3 lewis structure:

Lewis structures are not very good at describing boron-containing compounds and ions. A far better way to consider such organisms is through the view of molecular orbital theory. However, the Lewis structure for NH3BF3 can be shown as follows:

nh3bf3  structure
 Lewis structure for NH3BF3

NH3BF3 structure formal charge

In a molecule, formal charge is based on the idea that all chemical bonds have uniformly distributed electrons in atoms. Let us calculate NH3BF3 formal charge.

The formal charge on overall NH3BF3  is 0. Using the formula F.C can be calculated. Formal charge in NH3BF3 = Number of valence electrons in NH3BF3 – non-bonding electrons in NH3BF3 -1/2 bonding electrons in NH3BF3.

A formal charge table for NH3BF3 is as follows:

Atoms involved
in NH3BF3
Valence
Electrons
(V.E)
Non-bonding
Electrons
(N.E)
Bonding
Electrons
(B.E) 
Formal
charge
(F.C)
Central Atom
(N)
508/2(5- 0- 8/2)
=+1
Outer Atom
 (3H)
102/2(1- 0- 2/2)
=0
Central Atom 
(B)
308/2(3 -0 – 8/2)
=-1
Outer Atom
(3F)
762/2(7-6-2/2)
=0
 The formal charge on NH3BF3 lewis structure, N= +1, H=0, B =-1, F=0, NH3BF3=0

NH3BF3 valence electrons

In valence electron is one of the outer shells of an atom created during chemical bond synthesis. Let us calculate the valence electrons in NH3BF3.

NH3BF3 has overall 32 valence electrons present. The periodic table places hydrogen in group 1 and nitrogen in group 15. In the periodic table, fluorine and boron fall into groups 13 and 17, respectively.

The following table details the valence electron:

Atoms involved
in NH3BF3
Valence
Electrons
(V.E)
Electronic
configuration 
of atoms
Total valence 
electrons
Central Atom
(N)
51s22s22p35*1
=5
Outer Atom 
(H)
11s13*1
=3
Central Atom 
(B)
31s22s22p13*1
=3
Outer Atom
(F)
71s22s22p57*3
=21
Total valence electron in NH3BF3 =32

NH3BF3 structure lone pairs

A lone pair of electrons lacks a covalent bond and is referred to as a pair of electrons. Now let us see how many lone pairs are in NH3BF3.

In NH3BF3 there is one lone pair present on NH3. This is because these lone pairs are shared via a coordinate connection to create the adduct with BF3. The bond between B and N is created using the single pair of N, completing the octet of B. 

NH3BF3 hybridization

Molecules contain hybrid orbitals that distribute an atom’s orbital energy. Let us check hybridisation in NH3BF3.

NH3BF3 has Sp3 hybridisation on both Nitrogen and Boron. This is because the boron atom in BF3  has three bond pairs of electrons and no lone pairs. It has been Sp2 hybridised. The nitrogen atom in NH3 has Sp3 hybridised, on the other hand.

  • The boron atom in NH3BF3 possesses 4 bond pairs of electrons and zero nonbonding electrons. 
  • BF3 is hybridised with Sp3.  
  • As a result, the boron’s hybridization changes from Sp2 to Sp3 as a result of the development of the molecule(NH3BF3)complex.

NH3BF3 structure shape

Molecule shape affects chemical and physical properties, including its colour, reactivity, and biological activity. Let us look at the shape of NH3BF3.

NH3BF3 has a tetrahedral shape. Because each hydrogen will create a single covalent bond with nitrogen in NH3, which contains 5 valence electrons. It has 4 bonds because it has 3 bonding pairs and 1 lone pair, which results in a tetrahedral structure.

Boron geometry shifts from trigonal planar to tetrahedral due to a change in the hybridization process(Sp2 to Sp3).

NH3BF3 structure angle

The angles between neighbouring lines that form bonds are known as bond angles. Let us find out the angle between NH3BF3

NH3BF3 structure has 109.5° bond angles because the B and N atoms each have four single bonds. This may be because of their Sp3 hybridizations, which have bond angles of 109° for H-N-H, N-B-F, and F-B-F, respectively.

NH3BF3 solubility

The maximum quantity of a component that will dissolve at a specific temperature in a given volume of solvent. Let us check the solubility of NH3BF3.

NH3BF3 is soluble in water and other polar coordinating organic solvents like NH3BH3. The solubility of NH3BH3 or NH3BF3 is temperature-dependent. Here is a solvent list table in which ammonia-borane is soluble at room temperature.

SolventSolubility/g
(100g/solvent)-1
Ammonia260g
Water 33.6g
Tetrahydrofuran 25g
Diethyl ether0.7g
Ethanol6.5g
Isopropanol4g
isobutanol1g
Solubility of NH3BH3or NH3BF3

Is NH3BF3 solid or liquid?

There is no regular arrangement of liquids next to one another but solids are regularly arranged and closely packed. Let us check whether NH3BF3 is solid or not.

NH3BF3 is a white or colorless crystalline solid. It is because the solid structure suggests that the NH and BH centres are closely related. When compared to the B-F bonding distance of 131.1pm, the closest B-F distance is 136.7 pm. The image is shown below:

nh3bf3  structure
Distance of  B-F bond= 131.1 pm,136.7 pm

Is NH3BF3 polar or nonpolar?

Determine if molecules are polar or nonpolar by looking at the electronegativities of the associated atoms. Let us find out whether NH3BF3 is polar or not.

NH3BF3 is relatively high polar properties. It is because of being consistent with this difference. Although the B-F bond in BF3 is polar, due to symmetry they arrange themselves in a trigonal planar geometry and so cancel each other out. There is no net dipole moment as a result.

  • While the molecule of NH3 has a net dipole moment due to its trigonal pyramidal structure and lack of symmetry.
  • Trifluroamine boron (III) adduct is the product of this reaction, which occurs at a temperature lower than 0°C. 
  • The relationship between these atoms is a covalent bond or dative bond.
  • The reaction image is shown below:
nh3bf3  structure
Trifluroamine boron (III) adduct

Is NH3BF3 acidic or basic?

Acidity is indicated with the aid of using pH values beneath 7, while baseness is proven with the aid of using pH values above 7. Let us discover whether or not NH3BF3 is acidic or not.

NH3BF3 is an “adduct” molecule because there is the occurrence of a reaction between BF3(electron-deficient species) and NH3(electron-rich species). Despite lacking a proton, BF3 behaves like acid and interacts with NH3 by taking on its single pair of electrons. 

The equation for the response is as follows: BF3 +:NH3 → BF3:NH3

Is NH3BF3 electrolyte?

Chemical that dissociates into ions, which are positively and negatively charged particles, and as a result conducts electric current. Let us find out whether NH3BF3 is an electrolyte or not.

NH3BF3  behaves as an electrolyte because different chemicals with unique identities and properties are BF3 and NH3. A dative bond or Coordinate covalent bond connects the N of NH3 to the electron-poor B of BF3. It can therefore be easily divided into its constituent components.

Is NH3BF3 ionic or covalent?

A bond in which both electrons are coordinated and linked or covalent bonding. Let us find out whether NH3BF3 is ionic or covalent.

NH3BF3 is neither ionic nor covalent but shows “Coordinate” or dative bonding. This is because ammonia is electron-rich and it contains a lone pair while BF3 is electron deficient. By forming a coordinating bond, NH3 can give BF3 its electron pair because it has an empty orbital.

  • A single bond between N and H, along with one pair of electrons, fills the octet in NH3. This molecule is stable as a result.
  • A single bond between B and F, but the octet of boron is not completed. So, for B to complete its octet, it requires 2 extra electrons.  
  • It acquired 6 electrons by making just 3 simple connections to F. But, the F octet can be completed by 3 single bonds.
  • To create NH3BF3, BF3 coordinately covalently bonds with NH3 and accepts its single pair of electrons.

Conclusion

NH3BF3 is known as trifluroamine boron (III) adduct. A covalent or dative bond was created by the union of the boron and nitrogen atoms. A coordinate covalent bond is another name for the bond that exists between these atoms. The hybridization is Sp3 on both N and B.