SiCl2Br2 Lewis Structure: Drawings, Hybridization, Shape, Charges, Pair And Detailed Facts

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In this article, “sicl2br2 lewis structure”, lewis structure drawing, hybridization, shape, formal charge calculation with some detailed explanations are discussed briefly.

SiCl2Br2 is a tetrahedral compound with sp3 hybridization. In this compound, one silicon atom is attached with two chlorine and two bromine atoms. It has a molar mass 258.8 g/mol and having a bond angle 109.50.

The main outlook of this article is to discuss the below mentioned relevant topics on SiCl2Br2 structure and hybridization.

How to draw lewis structure of SiCl2Br2?

Lewis structure also known as electron dot structure was first introduced by scientist Gilbert. N. Lewis in the year of 1916. It is one type of special structural representation of any molecule keeping the nonbonded electrons around the respective species.

The following steps should be followed to draw the lewis structure of any molecule.

  1.  As valance shell electrons play a significant role in this structural representation, counting of valance electrons should be completed firstly. In SiCl2Br2, silicon, chlorine (Cl) and bromine (Br) have 4,7 and 7 electrons respectively in their valance shell.
  2. Next, number of bond connectivity (covalent or ionic) present in the molecule will be determined. In this molecule, total four covalent (two sigma bonds between Si and two chlorine and another two sigma bond is between Si and two bromine atoms) bonds are present.
  3. Calculate the number of nonbonding electrons or lone pairs who do not take part in bond formation. Si has no nonbonded electron but both the chlorine and bromine have 6 electrons as nonbonded.
sicl2br2 lewis structure
SiCl2Br2 Lewis Structure

SiCl2Br2 Lewis Structure Shape

Shape of any molecule can be determined by two following factors-

  • Hybridization
  • Repulsive factor

Hybridization is the key point to decide the structure and shape. But if any molecule does not show its actual geometrical structure, then repulsive factor must be present in that molecule. Repulsive factor can be different types but here only three factors are included.

  • Lone pair-lone pair repulsion
  • Lone pair-bond pair repulsion
  • Bond pair-bond pair repulsion

The increasing order of this repulsion is-

Lone pair-lone pair repulsion > Lone pair-bond pair repulsion > bond pair-bond pair repulsion.

But in SiCl2Br2 shows its actual geometrical structure due to absence of any lone pair on central atom (silicon). Bond pair-bond pair repulsion cannot deviate the actual structure much more. From hybridization we can conclude that Si is sp3 hybridized with a tetrahedral structure.

SiCl2Br2 shape
Shape of SiCl2Br2

 

SiCl2Br2 Lewis Structure Formal Charges

Formal charge is an outcome of lewis structure. The overall charge as well as the charge of individual atom can also be calculated from formal charge calculation.

Formal charge is calculated using the following formula-

  • Formal charge = Total number of valance electrons – number of electrons remain as nonbonded – (number of electrons involved in bond formation/2)
  • Formal charge of Silicon (Si) = 4 – 0 – (8/2) = 0
  • Formal charge on chlorine (Cl) = 7 – 6 – (2/2) = 0
  • Formal charge on bromine (Br) = 7 – 6 – (2/2) = 0

SiCl2BR2 Lewis structure Lone Pairs

Lone pairs are those electrons who are not participating in bond formation with another atoms. Number of lone pairs or nonbonding electrons can be calculated from the following formula using total valence shell electrons and number of electrons participate in bond formation.

  • Lone pair or nonbonded electron = Total number of valance electron – number of bonded electrons.
  • Nonbonded electrons of silicon = 4 – 4 = 0
  • Nonbonded electrons of each of the chlorine atom = 7 – 1 = 6
  • Nonbonded electrons of each of the bromine atom = 7 – 1 = 6

Valance electron of chlorine is 7 (3s2 3p5) and bromine also 7 (4s2 4p5). Silicon has total 4 electrons in its outer most shell (3s2 3p2).

SiCl2Br2 Hybridization

When two or more than two atomic orbitals mix with each other and form new hybrid orbitals for the purpose of gaining extra stability then this process is called hybridization.

The term “SiCl2Br2 hybridization” means the hybridization of central atom (silicon). Si is sp3 hybridized in this molecule with the four sigma bond connectivity with two chlorine and two bromine atoms.

SiCl2Br2 hybridization
SiCl2Br2 Hybridization

In this type of hybridization, bromine and chlorine share their one valance electron with silicon. In sp3 hybridization, silicon uses its one s orbital and three p orbital with chlorine and bromine and generate the bond angle 109.50. Due to this hybridization and bond angle, this molecule shows tetrahedral structure.

SiCl2Br2 lewis Structure Octet Rule

Octet rule is one of the most useful and important rule in Chemistry which states that an atom should have eight electrons in its valance shell like the nearest noble gas electron configuration. Octet rule is only applicable for main group elements.

Full filled valance shell has an extra stability because they hardly participate in any reaction. For this electron configuration noble gas are inert in nature.

Silicon, chlorine, bromine do not obey octet rule because their valance shell contains more than eight electrons. Silicon and chlorine is group three element and they need 18 electrons to get full filled valance shell. Bromine is group four element and it needs 32 electrons to achieve nearest noble gas electron configuration.

SiCl2Br2 Polar or Nonpolar

Polarity of any molecule depends upon the polarity of the substituents and the orientation or direction of the substituent atoms or groups. If the polar groups are in anti position with each other then the molecule does not show any polarity.

SiCl2Br2 is definitely a polar compound because the substituent atoms are not exactly in anti position with each other. The bond angle between them is 109.50. Thus, it has a strong net dipole moment.

SiCl2Br2 Polarity
 SiCl2Br2, a polar molecule.

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