Explain the formation of the following molecules using hybridization a)becl2 & b)bf3
Answers
Explanation:
becl2:-
->There are different types of hybridization that usually occur in BeCl2. However, beryllium dichloride in the gaseous state -exists in a linear form and is sp hybridized.
Name of the Molecule :Beryllium Dichloride
Molecular Formula :BeCl2
Hybridization Type :sp
Bond Angle :1800
Geometry :Linear
What is the Hybridization of Beryllium Dichloride?
BeCl2 (Beryllium Dichloride) central atom which is Be. Its electronic configuration is 1s2, 2s2, where two electrons are present in the valence shell. During the formation of BeCl2, beryllium atom bonds with two chlorine atoms via single covalent bonds. The number of electron pairs around the central atom will be two. No lone pair is found in the molecule. If we analyze this information then we can conclude that BeCl2 has sp hybridization.
Hybridization of BeCl2
In the BeCl2 molecule, beryllium dichloride forms single covalent bonds with two chlorine atoms each.
The central atom Be will consist of two bond pair.
No lone pair exists.
BeCl2Molecular Geometry And Bond Angles
BeCl2 molecular geometry is said to be a linear one with a bond angle of 180o. It is a non-polar molecule because they have less attraction between each other.
bf3
->hybridization for this molecule, it is sp2 hybridized. To explain it in simple terms, Boron’s atomic p orbitals and s orbitals in the outer shell usually combine together to form three sp2 hybrid orbitals which are all of the equivalent energy.
Name of the Molecule :Boron Trifluoride
Molecular Formula :BF3
Hybridization Type :sp2
Bond Angle :120°
Geometry :Trigonal Planar
What is the Hybridization of Boron Trifluoride?
Hybridization of BF3
BF3 has a boron atom with three outer-shell electrons in its ground state and three fluorine atoms containing seven outer electrons. Further, if we observe closely, one boron electron is unpaired in the ground state. During the formation of this compound, the 2s orbital and two 2p orbitals hybridize. Only one of the empty p-orbital is left behind as the lone pair. In short, Boron needs 3 hybridised orbitals to make bonds with 3 atoms of F where the 2pz orbitals get overlapped with these hybridised sp2 orbitals and bonds are formed.
The three hybridised sp2 orbitals are usually arranged in a triangular shape.
BF3 molecule is formed by bonding between three sp2 orbitals of B and p of 3 F atoms.
All the bonds in BF3 are sigma bonds.
BF3 Molecular Geometry and Bond Angles
BF3 Molecular Geometry
Normally, boron forms monomeric covalent halides which have a planar triangular geometry. This shape is mainly formed by the overlap of the orbitals between the two compounds. To be more precise, the BF3 molecular geometry is trigonal planar. It further has symmetric charge distribution on the central atom and is nonpolar.
The bond angle is 120o where all the atoms are in one plane. Each of them also makes an equilateral triangle.
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