To understand molecular geometry, polarity, and other properties of a compound, one must first understand certain fundamental properties of the compound and its Lewis structure. Sulfur Tetrafluoride has the molecular formula SF4. Is SF4 polar or nonpolar? It’s a colourless, corrosive gas that’s used to make a variety of organofluorine compounds. SF4 is a toxic compound that is commonly used in chemical and industrial applications.
Sulfur Tetraflouride is the name of the molecule ( SF4). SF4 (sp3) has 34 Valence Electrons in its molecule orbital hybridization. The bond angles between sulphur and flourine are 102 and 173 degrees, respectively. SF4 has a trigonal bipyramidal molecular geometry. The lone pairs in sulfur, on the other hand, were not included in the plan of the molecular geometry.
Is SF4 is polar or nonpolar? before answer this question, we need to understand the molecular geometry and Lewis structure of SF4.
SF4 Molecular Geometry (Theory)
Using the molecular formula or the Valence shell electron pair repulsion theory (VSEPR) model, it is simple to consider the molecular geometry of a given molecule. A molecular formula can be used to determine the precise number and type of atoms in a compound. The compound contains one sulfur atom and four fluorine atoms, making it identical to the chemical formula of AX4E.
In the above figure, It is the molecular geometry of SF4. Yellow colour ball is sulfur atom and remaining four grey colour balls are fluorine atom. Mulliken charge distribution of SF4 is given in the figure. -0.487 e is distributed equally in all fluorine atom and 1.949 e is in the sulfur atom.
Trigonal bipyramidal molecular geometry is found in molecules with the molecular formula AX4E (E is lone pairs of electrons). The equatorial positions of two fluorine atoms forming bonds with the sulfur atom are seen, while the axial positions of the other two are shown. Since the central atom has one lone pair, it repels the connecting pair of electrons, slightly altering the form and giving it the appearance of a see-saw.
SF4 showed Trigonal bipyramidal structure with five number of electron pairs. SF4 has 4 number of bonding pairs and 1 non bonding pairs of electron. The molecular shape of SF4 is disphenoidal. Bond length of S-F bond in axial and equatorial are 164.6 and 154.5, respectively. Bond angle of F-S-F in axial to axial and equatorial are 167.0 and 101.6, respectively.
To maximise the molecule’s stability, the electrons adopt this pattern of structure, which follows the VSEPR law, to minimise the repulsion forces between the lone pairs of electrons.
SF4 Lewis Structure (Dot formula)
The Lewis arrangement is a visual representation of the molecule’s bonds and valence electrons. Lines represent bonds formed between two atoms, while circles represent valence electrons that do not form any bonds.
Bonding pairs of electrons are those that assist in the formation of bonds, while nonbonding pairs of electrons, also known as lone pairs, are those that do not participate or form any bonds.
And before we can draw the Lewis structure of SF4, we need to know how many valence electrons there are in the molecule.
And we need to know how many valence electrons there are in SF4 before we can draw the Lewis structure. It should obey the octet rule. Which is the basic for Lewis structure.
This complex contains one sulphur atom and four fluorine atoms, as can be seen. To determine the overall valence electrons of this compound, we must first determine the valence electrons of both atoms separately.
Valence electrons of Sulfur atom: 6
Valence electrons of four Fluorine atoms: 4* (7) =28
( as there are four fluorine atoms in SF4 molecule, we have to consider valence electrons of all four fluorine atoms)
Total number of valence electrons in SF4 molecule = number of valence electrons in sulfur atom + number of valence electrons in four fluorine atoms
= 6 + 28
= 34 valence electrons in SF4 molecule
Now that we know how many valence electrons there are in the molecule, we can better understand how the atoms form bonds and how the molecule is put together.
Octet Rule definition for SF4
Octet Rule definition:
In most of their molecular compounds, the representative elements or atoms to achieve noble gas configurations.Octet Rule
The above statement is usually called the octet rule for molecular compounds, because the noble gas configurations in the periodic table have 8 e in their outermost shells (except for He, which has 2 e). This is the stable configuration of an atom.
For the time being, we’ll limit our conversation to compounds containing the representative elements. We can’t write Lewis formulas with only the octet rule law. We also have to figure out how many of the available valence electrons are bonding electrons (shared) and how many are unshared electrons (associated with just one atom) across the bonded atoms.
A lone pair is a pair of unshared electrons in the same orbital. In this case, a simple mathematical relationship is useful:
S = N-A
The cumulative number of electrons exchanged by the molecule or polyatomic ion is denoted by the letter S.
N is the cumulative number of valence shell electrons needed by all atoms in the molecule or ion in order to obtain noble gas configurations (N = 8 X number of atoms that
are not H, plus 2 X number of H atoms).
A is the total number of electrons required in all of the (representative) atoms’ valence shells. The estimate of their periodic group numbers equals this. If required, we must change A for ionic charges. Negative charges are represented by adding electrons, and positive charges are represented by subtracting electrons.
Octet rule Calculation for SF4
By using the following step wise procedure as follows. The calculation of S = N – A in step 2 shows only 6 e shared, but a minimum of 8 e are required to bond four F atoms to the central S atom.
The SF4 molecule skeleton is
N = 1 x 8 (S atom) + 4 X 8 (F atoms) = 40 e needed
A = 1 X 6 (S atom) + 4 X 7 (F atoms) = 34 e available
S = N – A = 40 – 34 = 6 e shared. Four F atoms are bonded to the central S atom in SF4 molecule. This requires a minimum of 8 e (octet rule law), but only 6 e have been calculated in step 2.
Now SF4 molecules have satisfied the octet rule, but we have used only 32 of the 34 e available. SF4 molecule placed the other two electrons on the central S atom.
Since sulphur is the least electronegative atom in this molecule, it would be the central atom, with four fluorine atoms forming bonds on its sides. Per fluorine atom can form a bond with the central atom, resulting in four bonds in the molecule configuration, using four fluorine valence electrons and four sulphur atom electrons. Our focused question is, “is SF4 polar or nonpolar?.”
As a result, eight valence electrons are still used, bringing the total number of valence electrons down to 24 from 34. The central fluorine atom has two valence electrons, while the other fluorine atoms all have six.
To show bonds, draw lines between S and F, and use dots to show lone pairs of electrons. Each fluorine atom would have three pairs of six valence electrons (shown as dots), as well as one sulphur bond. The core atom, on the other hand, would have two valence electrons as well as four bonds.
Is SF4 polar or nonpolar molecule?
Knowing the Lewis structure and molecular geometry of a substance makes depicting the molecule’s polarity much simpler. The asymmetric distribution of electrons on the central atom is caused by one lone pair on the central sulphur atom and four bonding pairs of electrons.
Two fluorine atoms can cancel each other’s dipole moment due to the see-saw shape of the molecule, but the other two can’t due to the electron structure. The charge distribution is uneven since fluorine atoms are more electronegative than sulphur atoms. As a consequence, the dipole moment is not cancelled, resulting in polarity. As a result, SF4 is polar.
sulfur in the SF4 molecule in +4 state is converted to the +6 state, when SF4 molecule reacts with fluorine to form SF6 molecule. This is one of the best examples of oxidation and reduction reaction.
SF4(g) + F2(g) —–> SF6(g)
SF4 Hybridization in the molecular orbitals
Let’s start by looking at the electron density regions for the central atom to figure out how the SF4 molecule is hybridised.
With four bonding pairs of electrons and one lone pair, sulphur has a total of five electron density regions. As a result, the sulphur atom has five hybridised orbitals: one 3s, three 3p, and one 3d orbital. The sp3d hybridization is caused by the alignment of electrons around the atom and hybridised orbitals. The steric number can also be used to determine hybridization.
Thus, the steric strain in SF4 molecule is five due to lone pairs of electron also.SF4 molecule exhibit SP3 hybrization vert similar like methane molecule. But it has lone pair of electron, it induces polarity in the molecule.
SF4 Bond angles and shape in molecular geometry
The central sulphur atom has one lone pair of electrons and forms four bonds with the surrounding fluorine atoms. Fluorine atoms in the equatorial positions have bond angles of 102 degrees, whereas those in the axial positions have bond angles of 173 degrees, which vary from the trigonal bipyramidal molecular geometry that results in a see-saw pattern.
Because of the lone pair on the central atom, the bond angles for equatorial fluorine atoms change from 120 degrees to 102 degrees, and 173 degrees instead of 180 degrees for axial fluorine atoms.
Conclusion on SF4 molecule
To summarise all of the properties, Sulfur Tetrafluoride has 34 valence electrons, of which four covalent bonds and one lone pair of electrons are formed on the central atom in its Lewis structure. On each fluorine atom, there are three lone pairs. It has the formula AX4E for its molecular geometry. It has sp3 hybridazation and having polarity.
Some related post on polar or nonpolar:
FAQ on “Is SF4 polar or nonpolar?”
Is sf4 polar or nonpolar molecule
SF4 (sulphur tetrafluoride) is a polar compound with trigonal bipyramidal structure.
How to determine if a molecule is polar or nonpolar?
Polarity in molecules. Lewis structures are commonly used to decide whether a molecule is polar or nonpolar. Nonpolar materials will be symmetric, which means that all of the sides surrounding the central atom will be equal – bonded to the same element with no unshared electron pairs.
what is the molecular geometry of sf4?
Molecular Structure of SF4 is
The polarity of the molecules
The polarity of the molecules are listed as follows
- Polarity of BeCl2
- Polarity of SF4
- Polarity of CH2Cl2
- Polarity of NH3
- Polarity of XeF4
- Polarity of BF3
- Polarity of NH4+
- Polarity of CHCl3
- Polarity of BrF3
- Polarity of BrF5
- Polarity of SO3
- Polarity of SCl2
- Polarity of PCl3
- Polarity of H2S
- Polarity of NO2+
- Polarity of HBr
- Polarity of HCl
- Polarity of CH3F
- Polarity of SO2
- Polarity of CH4
Lewis Structure and Molecular Geometry
Lewis structure and molecular geometry of molecules are listed below
- CH4 Lewis structure and CH4 Molecular geometry
- BeI2 Lewis Structure and BeI2 Molecular geometry
- SF4 Lewis Structure and SF4 Molecular geometry
- CH2I2 Lewis Structure and CH2I2 Molecular geometry
- NH3 Lewis Structure and NH3 Molecular geometry
- XeF4 Lewis Structure and XeF4 Molecular geometry
- BF3 Lewis Structure and BF3 Molecular geometry
- NH4+ Lewis Structure and NH4+ Molecular geometry
- CHCl3 Lewis Structure and CHCl3 Molecular geometry
- BrF3 Lewis Structure and BrF3 Molecular geometry
- BrF5 Lewis Structure and BrF5 Molecular geometry
- SO3 Lewis Structure and SO3 Molecular geometry
- SI2 Lewis structure and SI2 Molecular Geometry
- PCl3 Lewis structure and PCl3 Molecular Geometry
- H2S Lewis structure and H2S Molecular Geometry
- NO2+ Lewis structure and NO2+ Molecular Geometry
- HBr Lewis structure and HBr Molecular Geometry
- CS2 Lewis structure and CS2 Molecular Geometry
- CH3F Lewis structure and CH3F Molecular Geometry
- SO2 Lewis structure and SO2 Molecular Geometry
- HCl Lewis structure and HCl Molecular Geometry
- HF Lewis structure and HF Molecular Geometry
- HI Lewis structure and HI Molecular Geometry
- CO2 Lewis structure and CO2 Molecular Geometry
- SF2 Lewis structure and SF2 Molecular Geometry
- SBr2 Lewis structure and SBr2 Molecular Geometry
- SCl2 Lewis structure and SCl2 Molecular Geometry
- PF3 Lewis structure and PF3 Molecular Geometry
- PBr3 Lewis structure and PBr3 Molecular Geometry
- CH3Cl Lewis structure and CH3Cl Molecular Geometry
- CH3Br Lewis structure and CH3Br Molecular Geometry
- CH3I Lewis structure and CH3I Molecular Geometry
- SCl4 Lewis structure and SCl4Molecular Geometry
- SBr4 Lewis structure and SBr4 Molecular Geometry
- CH2F2 Lewis structure and CH2F2 Molecular Geometry
- CH2Br2 Lewis structure and CH2Br2 Molecular Geometry
- XeCl4 Lewis structure and XeCl4 Molecular Geometry
- BCl3 Lewis structure and BCl3 Molecular Geometry
- BBr3 Lewis structure and BBr3 Molecular Geometry
- CHF3 Lewis structure and CHF3 Molecular Geometry
- CHBr3 Lewis structure and CHBr3 Molecular Geometry
- ClF3 Lewis structure and ClF3 Molecular Geometry
- IF3 Lewis structure and IF3 Molecular Geometry
- ICl3 Lewis structure and ICl3 Molecular Geometry
- IBr3 Lewis structure and IBr3 Molecular Geometry
- ClF5 Lewis structure and ClF5 Molecular Geometry
- IF5 Lewis structure and IF5 Molecular Geometry
- PH3 Lewis structure and PH3 Molecular Geometry
- AsH3 Lewis structure and AsH3 Molecular Geometry
- AsCl3 Lewis structure and AsCl3 Molecular Geometry
- AsF3 Lewis structure and AsF3 Molecular Geometry
- NCl3 Lewis structure and NCl3 Molecular Geometry
- NF3 Lewis structure and NF3 Molecular Geometry
- NBr3 Lewis structure and NBr3 Molecular Geometry
- AlCl3 Lewis structure and AlCl3 Molecular Geometry
- AlF3 Lewis structure and AlF3 Molecular Geometry
- AlBr3 Lewis structure and AlBr3 Molecular Geometry
- CCl4 Lewis structure and CCl4 Molecular Geometry