Sf6 Lewis Structure Molecular Geometry

In this commodity, "SF6 lewis structure", hybridization, geometry, formal charge forth with some detailed explanations are discussed briefly.

SF_vi is an inorganic colorless greenhouse non-flammable gas with an octahedral geometry in which i sulfur atom is fastened with 6 fluorine atoms. It has an orthorhombic crystalline structure and hypervalent in nature. In SF₆, the S-F unmarried bond length is 156.iv pm.

Allow's focus on the structure, hybridization, formal charge and some relevant topics on sulfur hexafluoride.

How to draw lewis construction for SF₆?

Lewis structure known as electron dot structure was get-go introduced by eminent scientist Gilbert. N Lewis in the yr of 1916 in his periodical named as "The Cantlet and the Molecule". Lewis structure has a bully significance in Chemistry because number of bonds, nonbonding also as bonding electrons, construction tin be predicted from this construction.

In that location are some points should be kept in mind to draw lewis dot construction.

Valance electron has an important role in cartoon lewis structure. Thus, no of electrons in valance trounce should be counted first. In SF₆, sulfur has six and fluorine has seven valance electrons respectively.
Octet rule (having viii electrons in valance shell to achieve noble gas electron configuration) should exist applied if possible. For SF₆, octet dominion is simply applicable for fluorine but not in sulfur. Fluorine needs one more electron to be octet filled upward.
Number of covalent or ionic bonds should be calculated to know nigh the bonding electrons. After calculating bonding electrons, nonbonded electrons can be easily determined.

Afterwards maintaining all the to a higher place rules lewis dot construction is drawn (shown beneath).

SF₆ Lewis Structure Shape

Shape of any molecule tin exist decided by the presence of different repulsion factor similar bail pair-bail pair repulsion, lone pair-solitary pair repulsion and lone pair-bond pair repulsion because the shape of the molecular species is deviated from its bodily shape (geometry) due to the repulsion factor present in that molecule. The increasing club of this repulsion is-

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

In SF_six, sulfur has no lone pair, and so lonely pair-lone pair repulsion between the lone pair of central atom (sulfur) and substituent atom (fluorine) is absent. Thus, the geometry of SF_six is the shape of SF₆ that is octahedral. No departure is occurred from geometry to shape in SF_{half dozen}.

SF₆ Lewis Structure Formal Charges

Lewis structure helps to determine the formal charge of each of the atom in the molecular species. Formal accuse has a huge significance to determine if the molecule is a charged species or neutral in nature.

Information technology can exist 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/two)
Formal charge of sulfur = half-dozen – 0 – (12/2) = 0
Formal charge of each of the fluorine atom = 7 – 6 – (2/2) = 0

Valance electron of sulfur and fluorine is six and seven respectively. Number of nonbonding electrons for sulfur and fluorine is zero and 6 respectively.

SF_{half dozen} Lewis Structure Alone Pairs

Number of lone pairs or nonbonded electrons tin can be determined from the full valance electron and number o electrons participate in bond formation.

Lone pair or nonbonded electron = Total number of valance electron – number of bonded electrons.
Nonbonded electrons on sulfur = 6 – vi = 0
Nonbonded electrons on each of the fluorine atom = 7 – 1 = 6

In SF₆ sulfur has total six valance electrons (3s² 3p⁴) and fluorine has seven outer most shell electrons (2s² 2p^five).

Thus, central cantlet has no nonbonded electrons merely substituent atom has 6 nonbonded electrons or iii solitary pairs in SF₆ construction.

So, total nonbonded electrons in SF_vi is {0 + ( 4×half-dozen)} = 24 or 12 lone pairs.

SF_{half dozen} Hybridization

Hybridization occurs or hybrid orbitals are formed due to mixing of two or more than two atomic orbitals for the purpose of chemical bonding and stability.

In SF6, the hybridization of key cantlet sulfur is sp3d2. Lewis structure also helps to decide the hybridization.

Sulfur has total six electrons in its valance shell. All the valance electrons are getting paired by the valence electron from each of the six fluorine and the hybridization arises equally sp³d^two. What nosotros state in lewis construction point that sulfur has no electrons remain every bit nonbonded is proved through the hybridization epitome. In that location is six bail pairs and no lone pairs in SF₆. In this hybridization one s orbital, 3 p orbital and two d orbitals of sulfur are involved. Due to absenteeism of lone pair the actual geometry (octahedral) is shown by SF₆. The <FSF bond bending is ninety⁰ in SF₆ and the bond length of S-F bond is 156.4 pm.

SF₆ Lewis Structure Octet Rule

Octet rule is very much known and one of the important rules in chemistry. Just this dominion is only applicable for main group element. Ionic or covalent molecule are also included in this octet rule.

Octet dominion tells about the stability of any atom or molecule. It states that the valance crush of any atom should take eight electrons to achieve the nearest element of group 0 electron configuration.

This configuration gives any atom an extra stability and decreases the trend to react with any other molecule like the element of group 0. Noble gases accept very much less trend to take office in whatever reaction and known as inert molecule.

Allow's accept an example of carbon dioxide. In CO_two, carbon and oxygen have 4 and 6 valance electrons respectively. So, carbon needs four and oxygen needs vi more electrons to be octet filled upwards. Thus, carbon and oxygen share their respective valance electrons with each other and assist to have 8 electrons in their valance beat. To attain this goal, carbon forms double bond with each of the oxygen atom (O=C=O) and have a linear structure with a bond bending 180⁰.

In SF₆ sulfur does not obey octet dominion as it needs 12 more electron to take total filled valance crush electron configuration. But octet dominion is applicable for fluorine because it needs 1 more electron to have total eight electrons in its outer nigh shell.

Frequently Asked Questions (FAQ)

Is SF_{half dozen} reactive with water?

Answer: Sulfur atom is sterically hindered in SF_{half dozen} due to presence of six fluorine atoms. For this hindrance, sulfur tin non react with h2o, alkali hydroxides. Thus, SF_six is a kinetically inert molecule.

What are the intermolecular forces present in SF_six molecule?

Answer: The post-obit intermolecular forces are present in SF6.

London dispersion force
Dipole-dipole interaction force
Hydrogen bonding.

Is SF₆ reactive?

Answer: No, SF_six is basically an inert molecule with a lifetime 3200 years due to the huge steric hindrance on sulfur atom.