Pentafluoro Iodine or Iodine pentafluoride(IF5) has the composition of one Iodine and five fluorine atoms. What is the molecular geometry of Iodine pentafluoride?. Drawing and predicting the IF5 molecular geometry is very easy by following the given method. Here in this post, we described step by step to construct IF5 molecular geometry. Iodine and fluorine come from the 17th family group in the periodic table. Iodine or fluorine has seven valence electrons.
Key Points To Consider When drawing The IF5 Molecular Geometry
A three-step approach for drawing the IF5 molecular can be used. The first step is to sketch the molecular geometry of the IF5 molecule, to calculate the lone pairs of the electron in the central Iodineatom; the second step is to calculate the IF5 hybridization, and the third step is to give perfect notation for the IF5 molecular geometry.
The IF5 molecular geometry is a diagram that illustrates the number of valence electrons and bond electron pairs in the IF5 molecule in a specific geometric manner. The geometry of the IF5 molecule ion can then be predicted using the Valence Shell Electron Pair Repulsion Theory (VSEPR Theory) and molecular hybridization theory, which states that molecules will choose the IF5 geometrical shape in which the electrons have from one another in the specific molecular structure.
Finally, you must add their bond polarities characteristics to compute the strength of the five I-F bonds (dipole moment properties of the IF5 molecular geometry). Five Iodine-fluorine bonds in the Iodine pentafluoride(IF5), for example, are polarised toward the more electronegative value fluorine atoms, and because all five (I-F) bonds have the same size and polarity, their sum is nonzero due to the IF5 molecule’s bond dipole moment due to pulling the electron cloud to the downside in the square pyramidal geometry, and the IF5 molecule is classified as a polar molecule.
The molecule of Iodine pentafluoride(with square pyramidal shape IF5 molecular geometry) is tilted at 82 degrees bond angle of I-F. It has a difference in electronegativity values between Iodine and fluorine atoms, with fluorine’s pull the electron cloud being greater than Iodine’s. But bond polarity of I-F is not canceled to each other in the square pyramidal geometry. As a result, it has a permanent dipole moment in its molecular structure. The IF5 molecule has a dipole moment due to an unequal charge distribution of negative and positive charges.
Overview: IF5 electron and molecular geometry
According to the VSEPR theory, the IF5 molecule ion possesses square pyramidal molecular geometry. Because the center atom, Iodine, has five I-F bonds with the five fluorine atoms surrounding it. The I-F bond angle is 82 degrees in the square pyramidal IF5 molecular geometry. The IF5 molecule has a square planar geometry shape because it contains four fluorine atoms in the plan and one fluorine lies out of the plan.
There are five I-F bonds at the IF5 molecular geometry. After linking the five fluorine atoms and one lone pair of electrons in the square pyramidal form, it maintains the square bipyramidal-shaped structure. In the IF5 molecular geometry, the I-F bonds have stayed in the five terminals and one lone pair of electrons on the Iodine atom of the square pyramidal molecule.
The center Iodine atom of IF5 has one lone pair of electrons, resulting in square pyramidal IF5 electron geometry. However, the molecular geometry of IF5 looks square pyramidal-shaped and one lone pair of electrons on the Iodine of the IF5 geometry. It’s the IF5molecule’s asymmetrical geometry. As a result, the IF5 molecule is polar.
How to find IF5 hybridization and molecular geometry
Calculating lone pairs of electrons on Iodine in the IF5 geometry:
- Determine the number of lone pairs of electrons in the core atom of the IF5 Lewis structure. Because the lone pairs of electrons on the Iodine atom are mostly responsible for the IF5 molecule geometry distortion, we need to calculate out how many there are on the central Iodine atom of the IF5 Lewis structure.
Use the formula below to find the lone pair on the Iodine atom of the IF5 molecule.
L.P(I) = V.E(I) – N.A(I-F)/2
Lone pair on the central Iodine atom in IF5= L.P(I)
The core central Iodine atom’s valence electron in IF5 = V.E(I)
Number of I-F bonds = N.A (I-F)calculation for Iodine atom lone pair in IF5 molecule.
For instance of IF5, the central atom, Iodine, has seven electrons in its outermost valence shell, five I-F bond connections. This gives a total of five connections.
As a result of this, L.P(I) = (7 –5)/2=1
The lone pairs of electrons in the Iodine atom of the IF5 molecule are one.
Calculating lone pairs of electrons on fluorine in the IF5 geometry:
Finding lone pairs of electrons for the terminal atom is not similar to the central Iodine atom. We use the following formula as given below
Use the formula below to find the lone pair on the fluorine atom of the IF5 molecule.
L.P(F) = V.E(F) – N.A(I-F)
Lone pair on the terminal fluorine atom in IF5 = L.P(F)
Terminal fluorine atom’s valence electron in IF5 = V.E(F)
Number of I-F bonds = N.A ( I-F)calculation for fluorine atom lone pair in IF5 molecule.
For instance of IF5, five terminal atoms, fluorine, have seven electrons in its outermost valence shell, one I-F bond connection. This gives a total of five IF bond connections. But we are considering only one connection for the calculation.
As a result of this, L.P(F) = (7 –1)=6
The lone pairs of electrons in the fluorine atom of the IF5 molecule are six. Five fluorine atoms are connected with the central Iodine atom.
In the IF5 electron geometry structure, the lone pair on the central Iodine atom is one, lone pairs of electrons in the fluorine atom have six. Five fluorine atoms have 30 lone pairs of electrons.
It means there are one lone pair of electrons in the core Iodine atom. One lone pair of electrons on the central Iodine atom is responsible for the square pyramidal nature of IF5 molecular geometry. But in the structure fluorine atoms are polarised sidewise in their geometry.
The one lone pair of electrons are placed at another side of the IF5 geometry. Because the Iodine atom is a lower electronegative value as compared with other atoms in the IF5 molecule. Five fluorine atoms are polarized towards the sidewise in the IF5 structure.
But in reality, the IF5 has one lone pair of electrons in its structure. This makes the IF5 more irregular structure of the molecule. Because there is electric repulsion between bond pairs and lone pairs. But some sort of interaction is there between fluorine lone pairs and bond pairs. But it is negligible.
Calculate the number of molecular hybridizations of the IF5 molecule
What is IF5 hybridization? This is a very fundamental question in the field of molecular chemistry. All the molecules are made of atoms. In chemistry, atoms are the fundamental particles. There are four different types of orbitals in chemistry. They are named s, p, d, and f orbitals.
The entire periodic table arrangement is based on these orbital theories. Atoms in the periodic table are classified as follows:
s- block elements
p- block elements
f-block elementsAtoms are classified in the periodic table
IF5 molecule is made of one Iodine, five fluorine atoms. The fluorine and Iodine atoms have s and p orbitals. Fluorine comes as the first element from the halogen family in the periodic table. The Iodine atom also belongs to the same family group. But it falls as the fourth element in the periodic table.
When these atoms combine to form the IF5 molecule, its atomic orbitals are mixed and form unique molecular orbitals due to hybridization.
How do you find the IF5 molecule’s hybridization? We must now determine the molecular hybridization number of IF5.
The formula of IF5 molecular hybridization is as follows:
No. Hyb of IF5= N.A(I-F bonds) + L.P(Br)
No. Hy of IF5 = the number of hybridizations of IF5
Number of I-F bonds = N.A (I-F bonds)
Lone pair on the central Iodine atom = L.P(I)Calculation for hybridization number for IF5 molecule
In the IF5 molecule, Iodine is a core central atom with five fluorine atoms connected to it. It has one lone pair of electrons on Iodine. The number of IF5 hybridizations (No. Hyb of IF5) can then be estimated using the formula below.
No. Hyb of IF5= 5+1=6
The IF5 molecule ion hybridization is six. The Iodine and fluorine atoms have s,p, and d orbitals. The sp3d2 hybridization of the IF5 molecule is formed when one S orbital, three p orbitals, and two d orbitals join together to form the IF5 molecular orbital.
Molecular Geometry Notation for IF5 Molecule :
Determine the form of IF5 molecular geometry using VSEPR theory. The AXN technique is commonly used when the VSEPR theory is used to calculate the shape of the IF5 molecule.
The AXN notation of IF5 molecule is as follows:
The central Iodine atom in the IF5 molecule is denoted by the letter A.
The bound pairs (five I-F bonds) of electrons to the core Iodine atom are represented by X.
The lone pairs of electrons on the central Iodine atom are denoted by the letter N.Notation for IF5 molecular geometry
We know that Iodine is the core atom, with five electron pairs bound (five I-F) and one lone pair of electrons. The general molecular geometry formula for IF5 is AX5N1.
According to the VSEPR theory, if the IF5 molecule ion has an AX5N1 generic formula, the molecular geometry and electron geometry will both square pyramidal forms.
|Name of Molecule
|Chemical molecular formula
|Molecular geometry of IF5
|Electron geometry of IF5
|Hybridization of IF5
|Bond angle (I-F)
|Total Valence electron for IF5
|The formal charge of IF5 on Iodine
In this post, we discussed the method to construct IF5 molecular geometry, the method to find the lone pairs of electrons in the central Iodine atom, IF5 hybridization, and IF5 molecular notation. Need to remember that, if you follow the above-said method, you can construct the IF5 molecular structure very easily.
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 CS2
- 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
- BeCl2 Lewis Structure and BeCl2 Molecular geometry
- SF4 Lewis Structure and SF4 Molecular geometry
- CH2Cl2 Lewis Structure and CH2Cl2 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
- SCl2 Lewis structure and SCl2 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
- 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 SCl4 Molecular 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
- ClF5 Lewis structure and ClF5 Molecular Geometry