OSF4 Lewis Structure & Characteristics: 17 Complete Facts

OSF4 Lewis structure stands for the sketch of shape of the compound named Thionyl Tetrafluoride. Let us define the Lewis structure of the compound below.

OSF4 Lewis structure is the electronic structure that indicates the number if electrons involve the bonding between Oxygen, Sulphur and Fluorine atoms. In this structure the electrons are symbolised by few dots.  The drawing of this structure refers several facts about its internal formation.

OSF4 Lewis structure develops knowledge regarding distinguishable characteristics of OSF4. Those characteristics and facts would be described throughout this article.

How to draw OSF4 Lewis structure?

Drawing the Lewis structure of OSF4 would be conducted through five easy steps. Those steps are described below:

Step 1: Identification of valence electrons number

Identifying the number of valence electron in the compound can be obtained by calculating the number of valence electrons in the individual atoms of the compound. This step fundamentally provides knowledge regarding the lack of electrons in the valence shell that creates urge of forming bonds.

Step 2: Finding centre atom

Based on the electronegativity of atoms centre atom is chosen in a compound. Least electronegative atom gets the place in centre. In OSF4, both O and S participate in bonding with a single atom so they both have chance to be in centre position. S gets the centre position in OSF4.

Step 3: Forming bond between the elements

After obtaining the lack or extensity of electrons in the last energy level of atoms, the formation of bonds takes place in the compounds. Putting two dots between two different elements one bond is represented in the Lewis structure. To make double bond among S and O four dots are put between them.

Step 4: Putting lone pairs around elements

Lone pairs present in each electron after making bonds are highlighted by the dots of electrons in Lewis structure. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, this step is important to calculate the total number of lone pairs in OSF4 to recognise the internal effect works in it.

Step 5: Calculation of formal charges

Formal charge calculation is the last step of making the electronic skeleton of the compound. Formal charge calculation makes it complete by denoting the presence of zero charge that is neutral state in OSF4.

OSF4 Lewis structure resonance

Resonance takes place in presence of extra electron in structure and in presence of pi bonds. Let us find effect of resonance in OSF4.

OSF4 Lewis structure resonance is irrelevant as O and S atoms have no urge to break the π bond and create extra valence electron in Sulphur. It becomes unstable after undergoing resonance. Stability is the most important factor for any compound so OSF4 has no intention to make any resonating structure.

OSF4 Lewis structure shape

Shape is neatly determined by Lewis structure of compound by displaying electronic arrangement and bonds in it. Let us examine the shape of OSF4 below.

OSF4 Lewis structure shape is Trigonal bypyramidal. The compound does not possess exactly the Trigonal bypyramidal shape but it can be described as distorted Trigonal bypyramidal. An equator position is found in the compound that is significantly held by Oxygen atom of OSF4.

The bond length of different atoms in OSF4 is different.  Generally, the length of equator bond in Trigonal bypyramidal compounds is found to be shortest. Therefore, O-S bond in the compound is shortest with 1.409Å. Even after having similar type of F atoms axial S-F bond and equator S-F bonds lengths differ and given distorted shape of OSF4.

OSF4 Lewis structure formal charge

Formal charge is a factor that can help to define the ionic nature of the compound by displaying the presence of ions in it. Let us identify if OSF4 has any ions or not.

OSF4 Lewis structure formal charge is calculated below with the help of the formula: Formal charge = number of valence electrons – number of nonbonding electrons – number of electron shared (number of bonding electrons/2)

The table is reflecting the calculation with well-organised value of each factor:

Elements and
the number of
their valence electrons
Number of
Number of
electron shared
Formal charge
S = 606/2 = 3(6-0-3) = 3
O = 642/2 = 1(6-4-1) = 1
F1 = 76½ = 0.5(7-6-0.5) = 0.5
F2 = 76½ = 0.5(7-6-0.5) = 0.5
F3 = 76½ = 0.5(7-6-0.5) = 0.5
F4 = 76½ = 0.5(7-6-0.5) = 0.5
OSF4 = 40(3-1-0.5-0.5-0.5-0.5)
= 0
OSF4 Lewis structure Formal charge calculation

OSF4 Lewis structure angle

Angle between the bonds in OSF4  can also be obtained by keenly examining the Lewis structure that exhibits facts about bind formation. Let us find bond angle of OSF4.

OSF4 Lewis structure bond angle should be 120o as per its shape. The distorted shape of compound highlights the fact that the type of bonds formed by element with Sulphur is different which makes the compound deviated from its ideal bond angle.  The compound shows various bond angles nearer to the ideal one.

The bond angle between equatorial Fluorine atoms in OSF4 is estimated as 112.8°. The bond angle between equatorial and axial Fluorine atoms is 85.7° whereas the bond angle between equatorial Fluorine and Oxygen is 123.6°. Besides, Oxygen and Axial Fluorine atoms create bonds with 97.7° estimated bond angle.

OSF4 Lewis structure octet rule

Octet rule enhance the knowledge regarding urge of electrons and formation of bonds among the periodic elements. Let us signify the rule for OSF4 below.

OSF4 Lewis structure octet rule says, all the elements here significantly collect 8 electrons in its valence shell. According to the rule, if an element can gain 8 electrons in the last energy level and adopt similar electronic configuration as the nearest noble gas, it can be as stable as noble gas.

By maintaining octet rule Oxygen and Fluorine atoms shares 2 and 1 electrons with S respectively. S also gets satisfaction with 10 electrons with expanded octet.  This electron sharing process meets the electronic needs of each atom and stabilises their configurations.

OSF4 Lewis structure lone pairs

The number of lone pairs in a compound is significantly identified from the Lewis structure. Let us count the lone pairs in OSF4 through this section.

OSF4 Lewis structure has total 14 lone pairs. S in the compound does not have any lone pairs as its all electrons participate in bonding. O atom shares two electrons with Sulphur so the remaining number of lone pairs in oxygen is 2. Each F gives one electron to Sulphur and hold 3 lone pairs.

VSEPR theory is an interesting one that significantly denotes the number of lone pairs in the compounds. This theory helps to identify any repulsive factors that work in the compound due to the presence of lone pairs. Moreover the ,one of lone pairs are counted to calculate the steric number of OSF4 to signify its hybridisation structure.

OSF4 valence electrons

Valence electrons are the most important feature in the formation of bond among elements. Let us calculate the number of valence electrons in OSF4 below:

The total number of valence electron in OSF4 is 40.

  • The number of valence electrons in Sulphur = 6
  • The number of valence electrons in Oxygen = 6
  • The number of valence electrons in each Fluorine atom = 7
  • The number of valence electrons in four Fluorine atom = (7*4) = 28
  • The total number of valence electron in OSF4 = (6+6+28) = 40

The above calculation significantly incorporates the idea about deficiency in atoms to fill their octet state. Valence electrons are the responsible for making bonds between two elements and forming bonds in accordance with their compatibility. 

OSF4 hybridization

Fact of hybridisation stands to the next door of lone pair calculation as lone pairs play a huge role in finding hybridisation state. Let us find the hybridisation of OSF4 here.

OSF4 Lewis structure is Sp3d hybridised. It means the central atom of the compound is sp3d hybridised by having zero lone pairs in the structure. Hybridisation is the conjugated state of orbitals in compound that is formed after the elements share electrons with each other.

osf4 lewis structure
OSF4 Lewis structure hybridisation from Wikipedia

Steric number of OSF4 is another supportive factor that indulges proof about the formation of sp3d hybridisation. The addition of bonded electrons and the number of lone pairs of central atom gives steric number. The stearic number of OSF4 is 5 and according to VSEPR theory 5 steric number denotes sp3d hybridisation.

Is OSF4 solid?

The strong interaction force between the participative elements in a compound forms solid state of compounds. Let is identify the state of OSF4 in chemistry.

OSF4 is not solid, it is a gaseous compound in room temperature as its internal structure is made of Fluorine gas. The internal bond strength is quite loose and less intact which makes it gaseous.  By rising pressure and lowering temperature this compound can be converted into liquid.

Is OSF4 soluble in water?

Water solubility depends on the internal bond strength of the compound. As a gaseous substance how OSF4 reacts with water would be described in this section.

OSF4 gas is highly soluble in water. This gaseous compound is noticed to be hygroscopic and huge attraction to the polar substance like water. It is due to its lose internal bonding. The length of bonds are also different in OSF4 and the compound undergoes in reaction with H2O to give out Hydrofluoric acid.

Is OSF4 polar or nonpolar?

Polarity depends on the structural format created by the periodic element to make a compound.  Let us evaluate the fact below for OSF4.

OSF4 is a Polar compound. It is purely polar by nature and possesses a specific amount of dipole moment. As polarity depends on structure, it can be said that the polarity of OSF4 is also an effect of its structure. There is a significant reason to call its polar anyway.

Why OSF4 is polar?

OSF4 is polar as it has asymmetric Trigonal bypyramidal structure. Therefore, the distribution of charge also differs in case of internal bonding. Asymmetric charge distribution is the key factor, which plays significant role to make the compound polar.

Is OSF4 molecular compound?

Molecular compound refer to the neutral formation by participation of different molecules or atoms in bonding. Let us signify if OSf4 is molecular or not.

OSF4 is molecular compound by its neutral structure. A specific shape, particular bond angle and well-defined molecular geometry proof its molecular presence in the chemistry. The happy elements in Thionyl tetrafluoride do not hold any negative or positive charges in it that makes it pure molecular compound.

Is OSF4 acid or base?

Acidity and basicity of the compounds can be determined by the structural formulation. Let us describe the facts for OSF4 to answer this question below.

OSF4 is neutral compound that can be considered as more acid than a base. It is due to the weak bond strength of elements. A distorted structure of OSF4 makes its bonds weak and easily dissociable. It has huge tendency to break its bond and release free energy,

Is OSF4 electrolyte?

Electrolytes are those who carry free electrons or charges in the internal geometry.  This fact can also be apparently measured for OSF4 in this study.

OSF4 is not an electrolyte. It means the compound does not have the capability of carrying charges in molten state. This gaseous substance can break its bond and gives out energy or electron. Its conjugate acid or base can be considered as strong electrolytes.

Is OSF4 salt?

Salts are defined as the composition of positive charged ion and negative ions ion one single compound. Let us find the characteristic in depth for OSF4

OSF4 is not a salt. The compound is not capable of meeting the criterion of a salt. All the characteristics of a salt are opposed by the exceptional structure of OSF4. The proportion of opposite charges is not equivalent to make the compound salt in proper way.

Is OSF4 Ionic or Covalent?

Ionic bonds refer to the formation of bonds by electron transfer whereas covalent bonds are formed by sharing valence electrons. Let us find which process is happened in OSF4.

OSF4 is a covalent compound. The compound is formed with covalent bond by filling the needs of electrons to get ultimate stability in the periodic table. Covalent nature of OSF4 refers to the fact that the elements follow electron-sharing method to generate bonds between each other. 

Why OSF4 is covalent?

OSF4 is covalent as the elements share valence electrons with each other. The bonds are formed by the participation of valence electron by the electronic reaction. As the elements help to satisfy each other’s octet state with partial cooperation, the compound formed by them is called covalent.


This article has stated that OSF4 Lewis structure is holding Trigonal bypyramidal shape. In accordance with the VSEPR table, the steric number of OSF4 is 5 and it refers to sp3d hybridisation. Moreover, the bond angles of the compound differ for different position of Fluorine atoms and this fact makes the compound exceptional in chemistry. 

Scroll to Top