Potassium fluoride(KF) has the composition of one fluorine and one potassium atom. What is the molecular geometry of potassium fluoride?. Drawing and predicting the KF molecular geometry is very easy by following the given method. Here in this post, we described step by step to construct KF molecular geometry. Fluorine and potassium come from the 17th and 1st family groups in the periodic table. Fluorine and potassium have seven and one valence electrons respectively.
Key Points To Consider When drawing The KF Molecular Geometry
A three-step approach for drawing the KF molecular can be used. The first step is to sketch the molecular geometry of the KF molecule, to calculate the lone pairs of the electron in the central fluorine atom; the second step is to calculate the KF hybridization, and the third step is to give perfect notation for the KF molecular geometry.
The KF molecular geometry is a diagram that illustrates the number of valence electrons and bond electron pairs in the KF molecule in a specific geometric manner. The geometry of the KF 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 KF 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 one K-F single bonds (dipole moment properties of the KF molecular geometry). One potassium-fluorine single bonds in the potassium fluoride(KF), for example, are polarised toward the more electronegative value fluorine atom, and because (K-F) single bonds have the same size and polarity, their sum is nonzero due to the KF molecule’s bond dipole moment due to pulling the electron cloud to the two side of linear geometry, and the KF molecule is classified as a polar molecule.
The molecule of potassium fluoride(with linear shape KF molecular geometry) is tilted at 180 degrees bond angle of K-F. It has a difference in electronegativity values between fluorine and potassium atoms, with fluorine’s pull the electron cloud being greater than potassium’s. But bond polarity of K-F is not canceled to each other in the linear geometry. As a result, it has a nonzero permanent dipole moment in its molecular structure. The KF molecule has a nonzero dipole moment due to an unequal charge distribution of negative and positive charges in the linear geometry.
Overview: KF electron and molecular geometry
According to the VSEPR theory, the KF molecule ion possesses linear molecular geometry. Because the center atom, fluorine, has one K-F single bond with the one potassium atom surrounding it. The K-F bond angle is 180 degrees in the linear KF molecular geometry. The KF molecule has a linear geometry shape because it contains one potassium atom in the linear and four corners with four lone pairs of electrons.
There is one K-F single bond at the KF molecular geometry. After linking the one potassium atom and four lone pairs of electrons on the fluorine atom (as fluoride ion) in the linear form, it maintains the linear-shaped structure. In the KF molecular geometry, the K-F single bond has stayed in the one terminal and four lone pairs of electrons on the fluorine atom of the linear molecule.
The center fluorine atom of KF has four lone pairs of electrons, resulting in linear KF electron geometry. However, the molecular geometry of KF looks linear-shaped and has four lone pairs of electrons on the fluorine of the KF geometry. It’s the KF molecule’s slight asymmetrical geometry. As a result, the KF molecule is more polar.
How to find KF hybridization and molecular geometry
Calculating lone pairs of electrons on fluorine in the KF geometry:
- Determine the number of lone pairs of electrons in the core fluorine atom of the Lewis structure. Because the lone pairs of electrons on the fluorine atom are mostly responsible for the molecule geometry planar, we need to calculate out how many there are on the central fluorine atom of the KF Lewis structure.
Use the formula below to find the lone pair on the fluorine atom of the KF molecule.
L.P(F) = V.E(F) – N.A(K-F)
Lone pair on the central fluorine atom in KF= L.P(F)
The core central fluorine atom’s valence electron in KF = V.E(F)
Number of K-F bond = N.A (K-F)calculation for fluorine atom lone pair in KF molecule.
For instance of KF, the central atom, fluorine, has seven electrons in its outermost valence shell, one K-F single bond connection. This gives a total of one connection.
As a result of this, L.P(F) = (8 –0)=8
The lone pair of electrons in the fluorine atom of the KF molecule is four.
Calculating lone pair of electrons on potassium in the KF geometry:
Finding lone pair of electrons for the terminal potassium atom is similar to the central fluorine atom. We use the following formula as given below
Use the formula below to find the lone pair on the sosium atom of the KF molecule.
L.P(K) = V.E(K) – N.A(K-F)
Lone pair on the terminal potassium atom in KF = L.P(K)
Terminal potassium atom’s valence electron in KF= V.E(K)
Number of K-F bonds = N.A ( K-F)calculation for potassium atom lone pair in KF molecule.
For instance of KF, their terminal atoms, potassium, have one electron in its outermost valence shell, one K-F single bond connection. This gives a total of one K-F single bond connection. But we are considering only one connection for the calculation.
As a result of this, L.P(K) = (0 –0)=0
The lone pair of electrons in the potassium atom of the KF molecule is zero. One potassium atom is connected with the central fluorine atom.
In the KF electron geometry structure, the lone pairs on the central fluorine atom are four, lone pairs of electrons in the potassium atom have zero. One potassium atom has no lone pairs of electrons.
It means there are four lone pairs of electrons in the core fluorine atom (as fluoride ion). Four lone pair of electrons on the central fluorine atom is responsible for the linear nature of KF molecular geometry. But in the structure potassium atom is polarised sidewise in their linear geometry.
The four lone pairs of electrons are placed at another side of the KF geometry. Because the potassium atom is a lower electronegative value as compared with other atoms in the KF molecule. One potassium atom is polarized towards the sidewise in the KF structure.
But in reality, the KF has four lone pairs of electrons in its structure. This makes the KF more asymmetrical in the structure of the molecule. Because there is electric repulsion between bond pairs and lone pairs.
But some sort of interaction is there between potassium empty hole and lone pairs of electrons of fluorine of another KF molecule. Here, potassium of one molecule acts as an acceptor and fluorine of another molecule as a donor. This is called potassium bonding between the two KF molecules. This is one of the main intermolecular forces in KF.
But in the central, fluorine atom has four lone pairs of electrons and these lone pair electrons are placed in the four corners of the tetrahedral.
Calculate the number of molecular hybridizations of the KF molecule
What is KF 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
KF molecule is made of one fluorine and a potassium atom. The potassium and fluorine atoms have s and p orbitals. But potassium atom has only s orbital in the ground state. Potassium comes as the fourth element in the periodic table. The fluorine atom also belongs to the halogen family group. But it falls as the first element in the periodic table.
When these atoms combine to form the KF molecule, its atomic orbitals are mixed and form unique molecular orbitals due to hybridization.
How do you find the KF molecule’s hybridization? We must now determine the molecular hybridization number of KF.
The formula of KF molecular hybridization is as follows:
No. Hyb of KF= N.A(K-F bond) + L.P(F)
No. Hy of KF = the number of hybridizations of KF
Number of K-F bonds = N.A (K-F bonds)
Lone pair on the central fluorine atom = L.P(F)Calculation for hybridization number for KF molecule
In the KF molecule, fluorine is a core central atom with one potassium atom connected to it. It has four lone pairs of electrons on fluorine (as a fluoride ion). The number of KF hybridizations (No. Hyb of KF) can then be estimated using the formula below.
No. Hyb of KF= 4+0=4
The KF molecule ion hybridization is four. The fluorine and potassium atoms have s and p orbitals. The sp3 hybridization of the KF molecule is formed when one s orbital and three p orbitals join together to form the KF molecular orbital.
Molecular Geometry Notation for KF Molecule :
Determine the form of KF molecular geometry using VSEPR theory. The AXN technique is commonly used when the VSEPR theory is used to calculate the shape of the KF molecule.
The AXN notation of KF molecule is as follows:
The central fluorine atom in the K molecule is denoted by the letter A.
The bound pairs (one K-F bonds) of electrons to the core fluorine atom are represented by X.
The lone pairs of electrons on the central fluorine atom are denoted by the letter N.Notation for KF molecular geometry
We know that fluorine is the core atom, with no electron pair bound (one ionic bond K-F) and four lone pairs of electrons. The general molecular geometry formula for KF is AN4.
According to the VSEPR theory, if the KF molecule ion has an AN4 generic formula, the molecular geometry and electron geometry will both be linear-shaped forms.
|Name of Molecule||Potassium fluoride|
|Chemical molecular formula||KF|
|Molecular geometry of KF||linear|
|Electron geometry of KF||linear|
|Hybridization of KF||sp3|
|Bond angle (K-F)||180º degree|
|Total Valence electron for KF||8|
|The formal charge of KF on fluorine||0|
In this post, we discussed the method to construct KF molecular geometry, the method to find the lone pairs of electrons in the central KF atom, KF hybridization, and KF molecular notation. Need to remember that, if you follow the above-said method, you can construct the KF molecular structure very easily.
What is KF Molecular geometry?
KF Molecular geometry is an electronic structural representation of molecules.
What is the molecular notation for KF molecule?
KF molecular notation is AX1N3.
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
- 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