The iodine solid chemical formula is I2. Drawing I2 Lewis Structure is very easy to by using the following method. Here in this post, we described step by step method to construct I2 Lewis Structure. The diatomic iodine molecule elements come as members of the halogen family group from the periodic table. The valence electrons in the iodine atom are seven. iodine solid is used to make chemical corrosive reagents for organic chemical reactions as an iodinating agent in organic chemistry. It is used as a disinfectant.
Key Points To Consider When Drawing The I2 Electron Dot Structure
A three-step approach for drawing the I2 Lewis structure can be used. The first step is to sketch the Lewis structure of the I2 molecule, to add valence electrons around the two iodine atoms, and the final step is to combine the two iodine diatomic atoms to get the I2 Lewis Structure.
The I2 Lewis structure is a diagram that illustrates the number of valence electrons and bond electron pairs in the I2 molecule. The geometry of the I2 molecule can then be predicted using the Valence Shell Electron Pair Repulsion Theory (VSEPR Theory), which states that molecules will choose the I2 geometrical shape in which the electrons have from one another.
Finally, you must add their bond polarities to compute the strength of the one I-I single bonds (dipole moment properties of the I2 molecule). The iodine-iodine bonds in iodine molecule(I2), for example, are polarised equally the more electronegative iodine in I2 molecule, and because both bonds have the same size and are located around one iodine terminal of the two tetrahedral or linear structure with three lone pairs (in total six electrons) on the iodine atoms, their sum of dipole moment is zero due to the I2 molecule’s bond dipole moment and two iodine atoms canceled the polarity. Because I-I bonds polarity is canceled in the I2 molecule due to the presence of two equal sharing in the linear geometry. The iodine(I2) molecule is classified as a nonpolar molecule.
The molecule of diatomic iodine(with tetrahedral or linear-shaped molecular geometry) is tilted, the bond angles between iodine and iodine are 180 degrees. It has no difference in electronegativity values between iodine and other iodine atoms, with both iodine’s pull being equal in the I2 molecule. But they canceled each other due to the symmetrical linear structure with three lone pairs in the molecular geometry of the I2 molecule.
As a result, it has the zero dipole moment. The I2 molecule has a zero dipole moment due to an equal charge distribution of negative charges on both iodine terminals. But both iodine atoms fall on the halogen family groups in the periodic table. The iodine atom is a more electronegative value than iodine atom in the halogen family group. The I2 molecule has the net dipole moment of 0D value in the ground state energy level.
I2 molecule has one I-I single bond. Its dipole moment in the ground state is totally different as compared with the excited state. If it absorbs light may be from visible or UV light. It undergoes pi to pi star and n to pi star transition from ground state energy level to excited state energy level. In the excited state energy level, the I2 molecule shows a definite dipole moment. But it is very dynamic in nature.
Molecules can be classified as polar or nonpolar. The molecule polar behaves in a different manner as compared to nonpolar.
Overview: I2 Lewis Structure
The terminal atom is iodine, which is bordered on two terminals with iodine atoms( in tetrahedral or linear geometry), and three lone pairs on the two iodine atoms in the tetrahedral or linear molecular geometry. iodine has seven outermost valence electrons, indicating that it possesses seven electrons in its outermost shell. To complete the octet of the two iodine atoms requires one valence electron on each of their outermost shell.
One iodine atom establishes covalent connections with the other terminal iodine atom as a result, leaving each iodine atom with three lone pairs. There are three lone pairs of electrons on the iodine terminal atom that resists the bond pairs of the I-I bond. According to VSEPR theory, the I-I bond pairs polarity lead the I2 molecule to take on the linear or tetrahedral geometry structure.
The I2 molecule’s one I-I bond is arranged in symmetrical polarity order around the linear or tetrahedral molecular geometry, giving rise to the I2 molecular shape. The bond order of the I2 molecule is one. The I2 molecule has a tetrahedral or linear molecular geometry because there is an electrical repulsion between the lone pairs of electrons in iodine and one single bond pair(I-I) of the I2 molecule.
Lewis structure of I2 has dot electron representative structure. Valence electrons of atoms undergo orbitals mixing in the chemical reactions, giving new types of molecular species of I2. The molecule is nothing but a bundle of valence electrons from the atoms. But it is converted to bond pairs and lone pairs in the molecular structure.
Electronegative value Difference Calculation of I2 Molecule:
iodine and iodine Electronegative difference in I2 molecule:
The iodine atom has an electronegativity of 2.66 in the I2 molecule. The difference in electronegativity of iodine and iodine can be estimated using the method below.
The electronegative value difference between iodine and iodine in I2 molecule
Electronegativity value of iodine= 2.66
Electronegativity value of iodine= 2.66
Difference of electronegativity value between iodine and iodine in I2 molecule = 2.66 – 2.66= 0.00
The electronegativity difference between I-I bond calculation of I2 molecule
The electronegative difference between iodine and iodine is less than 0.5. This indicated the bond polarity moves near to nonpolar nature. I-I bond polarity in the I2 molecule is nonpolar.
Because of this difference in electronegativity of iodine and iodine atoms, the I2 molecule’s I-I bond becomes nonpolar. The total net dipole moment of the I2 molecule is zero due to the cancellation of the bond dipole moment in the linear or tetrahedral geometry due to the presence of three lone pairs of electrons. The electronegativity of an atom is the strength with which it may attract bound electron pairs to its side. The polarity and Lewis structure of HI are discussed in our previous post.
As a result, the I-I bond’s dipole moment is higher due to the polarization of the bonds and three lone pairs of electrons on iodine, and all I-I bonds’ dipoles are arranged in the symmetrical I2 molecular geometry. The I2 molecule has a zero net dipole moment.
The electron dot structure of the I2 molecule is also known as the I2 Lewis structure. It determines the number of outermost valence electrons as well as the electrons engaged in the I2 molecule’s bond formation. The outermost valence electrons of the I2 molecule must be understood while constructing the Lewis structure of the molecule.
The iodine atom is the terminal element in I2 molecular geometry, with seven electrons in its outermost valence electron shell.
The I2 has a total of 14 valence electrons as a result of the foregoing above-said reasoning. With the terminal iodine atom, the other terminal with one iodine atom forms covalent bond, leaving the iodine atom with three lone pairs(12 electron total) in the middle of linear or tetrahedral geometry.
Because three lone pairs on the terminal iodine atoms create interaction with I-I bond pairs(but it is negligible in the ground state of the I2 molecule). The bond angle of the I-I bond in the linear or tetrahedral molecular geometry is approximately 180 degrees. This angle is greater than the CH4 molecule bond angle. The I-I bond length is longer than the F-F bond length.
To sketch the I2 Lewis structure by following these instructions:
Step-1: I2 Lewis dot Structure by counting valence electrons on the iodine atom
To calculate the valence electron of each atom in I2, look for its periodic group from the periodic table. The halogen group families, which is the 17th in the periodic table, are made up of two iodine atoms. In their outermost shells, iodine and iodine have seven and seven valence electrons respectively.
Calculate the total number of valence electrons in the I2 molecule’s outermost valence shell. The first step is to determine how many electrons are in the I2 Lewis structure’s outermost valence shell. An electron in an atom’s outermost shell is known as a valence electron. It is represented by dots in the I2 Lewis diagram. The I2 molecule’s core iodine atom can be represented as follows:
Total outermost valence shell electron of iodine atom in I2= 7
Total outermost valence shell electron of iodine atom in I2= 7
The I2 molecule has one terminal iodine and other terminal iodine atoms. Then the total outermost valence shell electrons can be calculated as follows
∴ Total outermost valence shell electrons available for I2 Lewis structure( dot structure) = 7+7= 14 valence electrons in I2.
calculation of total valence electron of I2 molecule
Choose the atom with the least electronegative value atom and insert it in both terminals of the molecular geometry of I2. We’ll choose the least electronegative value atom in the I2 molecule to place in the terminal of the I2 Lewis structure diagram in this phase.
The first step is to put seven valence electrons around the iodine atom as given in the figure.
Step-2: Lewis dot Structure for I2 generated from step-1
Connect the two terminal atoms of the I2 molecule with one single I-I bond. In this stage, use one iodine atom on the outside of the I2 molecule to the other terminal iodine atom in the molecular geometry.
Count how many electrons from the outermost valence shell have been used in the I2 structure so far. I-I single bond carries two electrons because the iodine atom is connected to another iodine atom by I-I single bonds. Bond pairings of I-I are what they’re called.
So, out of the total of 14 valence electrons available for the I2 Lewis structure, we used four electrons for the I2 molecule’s one I-I single bond. The I2 molecule has three lone pairs of electrons in the two-terminal iodine atoms.
Place the valence electrons in the I-I bond pair starting with the one terminal iodine, another iodine atom in the I2 molecule. In the I2 Lewis structure diagram, we always begin by introducing valence electrons from the terminal iodine atom(in step1). As a result, wrap around the terminal iodine atom’s bond pair valence electrons first (see figure for step1).
The iodine atom in the molecule gets only 14 electrons around its molecular structure. This central iodine atom is octet stable. But it has three lone pairs. iodine (I2) is a brownish color solid. iodine is very corrosive in nature. It is one of the very reactive chemical reagents with carbohydrate.
iodine requires 8 electrons in its outermost valence shell to complete the molecular octet stability, two electrons bond pairs in one I-I single bond, and three lone pairs in the terminal iodine atom. iodine already shares 8 electrons to the one I-I single bonds.
We’ve positioned 8 electrons around the one-terminal iodine atoms(step-1), which is represented by a dot, in the I2 molecular structure above. The iodine atom completes its molecular octet stability in the I2 molecule because it possesses 2 electrons in its (one I-I single bonds) bond pairs with one iodine in the outermost valence shell.
Count how many outermost valence shell electrons have been used so far using the I2 Lewis structure. One electron bond pairs are shown as dots in the I2 chemical structure, whereas one single bond contains two electrons. The outermost valence shell electrons of the I2 molecule(bond pairs) are 2 as a result of the calculation. The total valence electron in a iodine atom is 8.
So far, we’ve used 8 of the I2 Lewis structure’s total 14 outermost valence shell electrons. Three lone pairs of electrons on each iodine atom in the linear or tetrahedral geometry of the I2 molecule.
Complete the terminal I2 atom stability and, if necessary, apply a covalent bond. The terminal iodine atom undergoes octet stability(due to one single bond pair of electrons).
The core atom in the I2 Lewis structure is iodine, which is bonded to the one terminal iodine atom by single bonds (one I-I). With the help of one single bond, it already shares 8 electrons. As a result, the iodine follows the octet rule and has 8 electrons surrounding it on the one terminal of the I2 molecule’s linear or tetrahedral geometry.
How to calculate the formal charge on iodine and other iodine atoms in I2 Lewis Structure?
Calculating formal charge on the iodine of I2 molecule:
The formal charge on the I2 molecule’s iodine central atom often corresponds to the actual charge on that iodine terminal atom. In the following computation, the formal charge will be calculated on the terminal iodine atom of the I2 Lewis dot structure.
To calculate the formal charge on the terminal iodine atom of the I2 molecule by using the following formula:
The formal charge on the iodine atom of I2 molecule= (V. E(I)– L.E(I) – 1/2(B.E))
V.E (I) = Valence electron in a iodine atom of I2 molecule
L.E(I) = Lone pairs of an electron in the iodine atom of the I2 molecule.
B.E = Bond pair electron in F atom of I2 molecule
calculation of formal charge on iodine atom in I2 molecule
The iodine terminal atom (one single bond connected to one iodine atom) of the I2 molecule has seven valence electrons, three lone pairs of electrons(six electrons), and 2 bonding pairing valence electrons. Put these values for the iodine atom in the formula above.
Formal charge on iodine atom of I2 molecule = (7- 6-(2/2)) =0
In the Lewis structure of I2, the formal charge on the terminal iodine atom is zero.
In this post, we discussed the method to construct the I2 Lewis structure. First, the valence electrons are placed around the two iodine atoms. Finally, when we combined the first and second steps. It gives I2 Lewis structure. Need to remember that, if you follow the above-said method, you can construct molecular dot structure very easily.
What is the I2 Lewis structure?
I2 Lewis structure is dot representation
What is the formal charge on the I2 Lewis structure?
Zero charges on the I2 molecular structure
The polarity of the molecules
The polarity of the molecules are listed as follows
- Polarity of BeI2
- Polarity of SF4
- Polarity of CH2I2
- 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 SI2
- 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