How to draw CHF3 Lewis Structure? - Science Education and Tutorials

Drawing CHF3 Lewis Structure is very easy to by using the following method. Here in this post, we described step by step method to construct CHF3 Lewis Structure. The carbon element comes as the first member of the carbon family group from the periodic table. The valence electrons carbon is four. The branch of carbon chemistry is called organic chemistry.

Table of Contents

Key Points To Consider When Drawing The CHF3 Electron Dot Structure

A three-step approach for drawing the CHF3 Lewis structure can be used. The first step is to sketch the Lewis structure of the CHF3 molecule, to add valence electrons around the carbon atom; the second step is to add valence electrons to the three fluorine and one hydrogen atoms, and the final step is to combine the step1 and step2 to get the CHF3 Lewis Structure.

The CHF3 Lewis structure is a diagram that illustrates the number of valence electrons and bond electron pairs in the CHF3 molecule. The geometry of the CHF3 molecule can then be predicted using the Valence Shell Electron Pair Repulsion Theory (VSEPR Theory), which states that molecules will choose the CHF3 geometrical shape in which the electrons have from one another.

Finally, you must add their bond polarities to compute the strength of the C-H bond and three C-F bond(dipole moment properties of the CHF3 molecule). The carbon-hydrogen and carbon-fluorine bonds in trifluoromethane or fluoroform(CHF3), for example, are polarised toward the more electronegative fluorine in CHF3 molecule, and because both bonds have the same size and located around three fluorine and one hydrogen terminals of the tetrahedral with no lone pairs on the carbon atom, their sum of dipole moment is nonzero due to the CHF3 molecule’s bond dipole moment and more electron polarity to the fluorine atom. Because each three C-F and one C-H bonds polarity not canceled each other in the CHF3 molecule. The trifluoromethane or fluoroform(CHF3) molecule is classified as a polar molecule.

The molecule of trifluoromethane (with tetrahedral molecular geometry) is tilted, the bond angles between carbon, fluorine, and hydrogen are 109.5 degrees. It has a difference in electronegativity values between carbon, fluorine, and hydrogen atoms, with central carbon’s pull being less than terminal fluorine’s in the CHF3 molecule. But they canceled each other due to the symmetrical molecular geometry of the CHF3 molecule. As a result, it has the nonzero dipole moment. The CHF3 molecule has a nonzero dipole moment due to an unequal charge distribution of negative and positive charges. The net dipole moment of the CHF3 molecule is 1.61 D.

Molecules can be classified as polar or nonpolar. The molecule polar behaves in a different manner as compared to nonpolar.

Overview: CHF3 Lewis Structure

The central atom is carbon, which is bordered on four terminals with three fluorine and one hydrogen atoms( in tetrahedral geometry), and a no lone pair on the central in the tetrahedral geometry. Carbon has four outermost valence electrons, indicating that it possesses four electrons in its outermost shell, whereas hydrogen only has one valence electron in its outermost shell. The fluorine atom has seven valence electrons. To complete the octet of the carbon atom, a carbon central atom requires four valence electrons.

Three fluorine and one hydrogen atoms establish covalent connections with the central carbon atom as a result, leaving the carbon atom with no lone pair. There is a no lone pair electron on the carbon central atom that resists the bond pairs of the three C-F and C-H. According to VSEPR theory, the C-F bond pairs polarity lead the CHF3 molecule to take on the tetrahedral molecular geometry shape.

The CHF3 molecule’s C-H and C-F bonds are arranged in unsymmetrical polarity order around the tetrahedral molecular geometry, giving rise to the CHF3 molecular shape. The CHF3 molecule has a tetrahedral molecular geometry because there is no electrical repulsion between the lone pairs of electrons in fluorine and four bond pairs(C-H and three C-F) of the CHF3 molecule.

Lewis structure of CHF3 has dot electron representative structure. Valence electrons of atoms undergo chemical reactions, gives new types of molecular species. 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 Difference Calculation of CHF3 Molecule:

Carbon and Hydrogen Electronegative difference in CHF3:

The carbon atom has an electronegativity of 2.6, while hydrogen has an electronegativity of 2.20 in the CHF3 molecule. The difference in electronegativity of carbon and hydrogen can be estimated using the method below.

The electronegative value difference between carbon and hydrogen
Electronegativity value of carbon = 2.6
Electronegativity value of hydrogen= 2.20
Difference of electronegativity value between carbon and hydrogen= 2.6 – 2.20=0.4
Electronegativity difference between C-H bond calculation of CHF3 molecule

The electronegative difference between carbon and hydrogen is less than 0.5. This indicated the bond polarity moves near to nonpolar nature. C-H bond polarity in CHF3 molecule is nonpolar.

Carbon and fluorine Electronegative difference in CHF3:

The carbon atom has an electronegativity of 2.6, while fluorine has an electronegativity of 3.98 in the CHF3 molecule. The difference in electronegativity of carbon and fluorine can be estimated using the method below.

The electronegative value difference between carbon and fluorine
Electronegativity value of carbon = 2.6
Electronegativity value of fluorine= 3.98
Difference of electronegativity value between carbon and hydrogen= 3.98 – 2.6=1.38
Electronegativity difference between C-F bond calculation of CHF3 molecule

Due to the difference in electronegativity value of greater than 0.5, the C-F bond of the CHF3 molecule becomes polar. Because of this difference in electronegativity, the CHF3 molecule’s C-F bond becomes polar. The total net dipole moment of the CHF3 molecule is nonzero due to the no cancellation of the bond dipole moment in the tetrahedral geometry. The electronegativity of an atom is the strength with which it may attract bound electron pairs to its side. The polarity of CHF3 is discussed in our previous post.

As a result, the C-F bond’s dipole moment is high due to the polarization of the bonds and lone pairs of electrons on fluorine, and all C-H and C-F bonds’ dipoles are arranged in the asymmetrical CHF3 molecular geometry. The CHF3 molecule’s total dipole moment is predicted to be 1.61 D.

The electron dot structure of the CHF3 molecule is also known as the CHF3 Lewis structure. It determines the number of outermost valence electrons as well as the electrons engaged in the CHF3 molecule’s bond formation. The outermost valence electrons of the CHF3 molecule must be understood while considering the Lewis structure of the molecule.

The carbon atom is the middle element in CHF3 molecular geometry, with four electrons in its outermost valence electron shell, whereas the hydrogen atom has one electron in its outermost valence electron shell. The fluorine atom has seven valence electrons.

The CHF3 has a total of 26 valence electrons as a result of the foregoing above said reasoning. With the core central carbon atom, the four terminal with three fluorine and one hydrogen atoms forms covalent bonds, leaving the carbon atom with a no lone pair in the middle of tetrahedral geometry.

Because lone pair on the terminal fluorine atom creates interaction with C-F bond pairs(but it is negligible). The bond angle of the F-C-H bond in the tetrahedral molecular geometry is approximately 109.5 degrees. This angle is similar to that of the CH4 molecule bond angle. The C-H bond length is 109 pm(picometer). The C-F bond length of CHF3 is shorter than C-Cl bond length of CHCl3.

To sketch the CHF3 Lewis structure by following these instructions:

Step-1: CHF3 Lewis dot Structure by counting valence electrons on the carbon atom

To calculate the valence electron of each atom in CHF3, look for its periodic group from the periodic table. The carbon, halogen, and hydrogen families, which are the 14th,17th, and 1st groups in the periodic table, are both made up of carbon, fluorine, and hydrogen atoms. In their outermost shells, carbon, fluorine, and hydrogen have four, seven, and one valence electrons, respectively.

Calculate the total number of valence electrons in the CHF3 molecule’s outermost valence shell. The first step is to determine how many electrons are in the CHF3 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 CHF3 Lewis diagram. The CHF3 molecule’s core carbon atom can be represented as follows:

Total outermost valence shell electron of carbon atom in CHF3= 4
Total outermost valence shell electron of fluorine atom in CHF3= 7
Total outermost valence shell electron of the hydrogen atom in CHF3= 1
The CHF3 molecule has one central carbon, three fluorine, and one hydrogen atoms. Then the total outermost valence shell electrons can be calculated as follows
∴ Total outermost valence shell electrons available for CHF3 Lewis structure( dot structure) = 4+3*7+1*1=26 valence electrons in CHF3.
calculation of total valence electron of CHF3 molecule

Choose the atom with the least electronegative value atom and insert it in the center of the molecular geometry of CHF3. We’ll choose the least electronegative value atom in the CHF3 molecule to place in the center of the CHF3 Lewis structure diagram in this phase. The electronegativity value in periodic groups grows from left to right in the periodic table and drops from top to bottom.

The first step is to put four valence electrons around the carbon atom as given in the figure.

Step-2: Lewis Structure of CHF3 for counting valence electrons around the terminal hydrogen and fluorine atoms

As a result, carbon is the first atom in the periodic table’s carbon family group. Hydrogen is the first member of the hydrogen family. The electronegative value of the fluorine atom is higher than that of the hydrogen and carbon atoms in the CHF3 molecule. Furthermore, carbon has a four electrons limit since hydrogen is the less electronegative element in the CHF3 molecule.

In the CHF3 Lewis structure diagram, the carbon atom can be the center atom of the molecule. As a result, central carbon in the CHF3 Lewis structure, with all three fluorine and one hydrogen atoms arranged in the tetrahedral geometry.

Add valence electrons around the fluorine and hydrogen atom, as given in the figure.

Step-3: Lewis dot Structure for CHF3 generated from step-1 and step-2

Connect the exterior and core central atom of the CHF3 molecule with three single C-F and one C-H bond. In this stage, use three fluorine and one hydrogen atom on the outside of the CHF3 molecule to the central carbon atom in the middle.

Count how many electrons from the outermost valence shell have been used in the CHF3 structure so far. Each C-H and C-F bonds carries two electrons because each carbon atom is connected to three fluorine and one hydrogen atoms by three C-F and one C-H bonds. Bond pairings of C-H and C-F are what they’re called.

So, out of the total of 26 valence electrons available for the CHF3 Lewis structure, we used 8 for the CHF3 molecule’s three C-F and one C-H bond. The CHF3 molecule has no lone pairs of electrons in the central carbon atom.

Place the valence electrons in the C-H and C-F bond pairs starting with the core carbon, three fluorine, and one hydrogen in the CHF3 molecule. In the CHF3 Lewis structure diagram, we always begin by introducing valence electrons from the central carbon atom(in step1). As a result, wrap around the central carbon atom’s bond pair valence electrons first (see figure for step1).

The carbon atom in the molecule gets only eight electrons around its molecular structure. This central carbon atom is octet stable. But it has no lone pairs. Methane(CH4) is the gaseous form in nature. when methane acted as a fuel, it is used as domestic fuel. But chloroform is a colorless liquid and not miscible with water.

Carbon requires 8 electrons in its outermost valence shell to complete the molecular stability, 8 electrons bond pairs in C-F and C-H bonds. Then lone pairs of electrons on the fluorine atoms of the CHF3 molecule is placed in a tetrahedral geometry. Fluorine already shares eight electrons to the three C-F and one C-H bonds. Then place the valence electron in the hydrogen and fluorine atoms, it placed around one and seven electrons on each atom(step-2). 18 valence electrons placed around fluorine atoms as lone pairs of electrons.

We’ve positioned no electrons around the terminal hydrogen atoms(step-3), which is represented by a dot, in the CHF3 molecular structure above. The carbon atom completes its molecular stability in the CHF3 molecule because it possesses 8 electrons in its (three C-F and one C-H) bond pairs with three fluorine and one hydrogen in the outermost valence shell.

Count how many outermost valence shell electrons have been used so far using the CHF3 Lewis structure. Four electron bond pairs are shown as dots in the CHF3 chemical structure, whereas four single bonds each contain two electrons. The outermost valence shell electrons of the CHF3 molecule(bond pairs) are eight as a result of the calculation.

So far, we’ve used 26 of the CHF3 Lewis structure’s total 26 outermost valence shell electrons. No lone pair of electrons on the carbon atom in the tetrahedral geometry of the CH4 molecule.

Complete the middle carbon atom stability and, if necessary, apply a covalent bond. The central carbon atom undergoes octet stability(due to resonance structure with charge and bond pairs).

The core atom in the CHF3 Lewis structure is carbon, which is bonded to the three fluorine and one hydrogen atom by single bonds (C-H and C-F). With the help of three and one single bond, it already shares eight electrons. As a result, the carbon follows the octet rule and has 8 electrons surrounding it on the four terminals of the CHF3 molecule’s tetrahedral geometry.

How to calculate the formal charge on a carbon, fluorine, and hydrogen atoms in CHF3 Lewis Structure?

Calculating formal charge on the carbon of CHF3 molecule:

The formal charge on the CHF3 molecule’s carbon central atom often corresponds to the actual charge on that carbon central atom. In the following computation, the formal charge will be calculated on the central carbon atom of the CHF3 Lewis dot structure.

To calculate the formal charge on the central carbon atom of the CHF3 molecule by using the following formula:
The formal charge on the carbon atom of CHF3 molecule= (V. E(C)– L.E(C) – 1/2(B.E))
V.E (C) = Valence electron in a carbon atom of CHF3 molecule
L.E(C) = Lone pairs of an electron in the carbon atom of the CHF3 molecule.
B.E = Bond pair electron in C atom of CHF3 molecule
calculation of formal charge on carbon atom in CHF3 molecule

The carbon core atom (four single bonds connected to three fluorine and one hydrogen atoms ) of the CHF3 molecule has four valence electrons, no lone pairs of electrons(zero electrons), and eight bonding pairing valence electrons. Put these values for the carbon atom in the formula above.

Formal charge on carbon atom of CHF3 molecule = (4- 0-(8/2)) =0

In the Lewis structure of CHF3, the formal charge on the central carbon atom is zero.

Calculating formal charge on the hydrogen of CHF3 molecule:

The formal charge on the CHF3 molecule’s hydrogen terminal atom often corresponds to the actual charge on that hydrogen terminal atom. In the following computation, the formal charge will be calculated on the terminal hydrogen atom of the CHF3 Lewis dot structure.

To calculate the formal charge on the terminal hydrogen atom of the CHF3 molecule by using the following formula:
The formal charge on the hydrogen atom of CHF3 molecule= (V. E(H)– L.E(H) – 1/2(B.E))
V.E (H) = Valence electron in a hydrogen atom of CHF3 molecule
L.E(H) = Lone pairs of an electron in the hydrogen atom of the CHF3 molecule.
B.E = Bond pair electron in H atom of CHF3 molecule
calculation of formal charge on hydrogen atom in CHF3 molecule

The hydrogen terminal atom of the CHF3 molecule has one valence electron, no lone pairs of electrons(zero electrons), and two bonding pairing valence electrons. Put these values for the hydrogen atom in the formula above.

Formal charge on hydrogen atom of CHF3 molecule = (1- 0-(2/2)) =0

In the Lewis structure of CHF3, the formal charge on the terminal hydrogen atom is zero.

Calculating formal charge on the fluorine of CHF3 molecule:

The formal charge on the CHF3 molecule’s fluorine terminal atom often corresponds to the actual charge on that fluorine terminal atom. In the following computation, the formal charge will be calculated on the terminal fluorine atom of the CHF3 Lewis dot structure.

To calculate the formal charge on the terminal fluorine atom of the CHF3 molecule by using the following formula:
The formal charge on the fluorine atom of CHF3 molecule= (V. E(F)– L.E(F) – 1/2(B.E))
V.E (F) = Valence electron in a fluorine atom of CHF3 molecule
L.E(F) = Lone pairs of an electron in the fluorine atom of the CHF3 molecule.
B.E = Bond pair electron in Cl atom of CHF3 molecule
calculation of formal charge on fluorine atom in CHF3 molecule

The fluorine terminal atom of the CHF3 molecule has seven valence electrons, three lone pairs of electrons(six electrons), and two bonding pairing valence electrons. Put these values for the fluorine atom in the formula above.

Formal charge on fluorine atom of CHF3 molecule = (7- 6-(2/2)) =0

In the Lewis structure of CHF3, the formal charge on the terminal fluorine atom is zero.

Summary:

In this post, we discussed the method to construct the CHF3 Lewis structure. First, the valence electrons are placed around the carbon atom. Second, place the valence electron on the hydrogen and fluorine atoms. Finally, when we combined the first and second steps. It gives CHF3 Lewis structure. Need to remember that, if you follow above said method, you can construct molecular dot structure very easily.