Therefore, from the above figure, it is observed that all 20 valence electrons have been placed systematically. This means that the remaining valence electrons will now be placed on the Fluorine atoms instead. The octet and duplet requirements for the Carbon and Hydrogen atoms have been fulfilled.
Where do the remaining valence electrons go? Do they go on the Hydrogen atoms? Well, to determine this observe the figure. This means that eight valence electrons have been used. It can be observed that there are eight dots on the structure so far. Two valence electrons are placed in between atoms to form covalent bonds. The arrangement would look something like this: With four valence electrons, it can facilitate chemical bonding with the four other atoms present. Now, we can assemble the Lewis structure for CH2F2.Ĭarbon as the central atom here makes sense. We know the number of valence electrons available for placement from the previous section. It also shows the chemical bonds present and gives much-needed insight into molecular geometry and chemical polarity, among other things. The Lewis structure represents the assembly of individual atoms and electrons within that compound. Therefore, the total number of valence electrons in CF4 is given by:Ĥ + 2 + 14 = 20 Valence Electrons CH2F2 Lewis Structure Therefore, the two Fluorine atoms present contribute: 7 x 2 = 14 Valence Electrons. Fluorine is in group 17 of the periodic table with the electronic configuration 2s22p5. Therefore, the two Hydrogen atoms contribute 1 x 2 = 2 valence electrons.įinally, we have two Fluorine atoms. Hydrogen has an electronic configuration of 1s1. Therefore, a single carbon atom contributes: 4 x 1 = 4 Valence Electrons. Carbon is in group 4 of the periodic table with the electronic configuration 2s22p2. Let’s take a look at how many valence electrons are available to us to assemble the CH2F2 Lewis structure:įirst, we have Carbon. They can break to take part in bond formation and electron exchanges. Valence electrons, as we know, are electrons that are in the outermost shells of atoms. This depends on each element’s position in the periodic table and, therefore, its electronic configuration. Each constituent atom in Difluoromethane contributes a set amount of valence electrons. To assemble the Lewis structure of Difluoromethane, we must first calculate the number of valence electrons available. Concluding Remarks CH2F2 Valence Electrons.of valence electrons 4 + (1 x 2) + (7 x 2) = 20 valence electrons Hybridization of the central atom sp3 Bond Angles 109.5° Molecular Geometry of CH2F2 Tetrahedral Molecular Geometry Let us look at some of the properties of Difluoromethane below: Name of the molecule Difluoromethane (CH2F2) No. The Lewis structure of Difluoromethane will help us understand its structure and atomic constitution. This is still relatively less than other refrigerants like R410A or R417A.Īlternatives to HFCs are being tested, and the United States has begun phasing out the use of Difluoromethane over 15 years. It has an ODP (Ozone Damaging Potential) of 0 and is 675 times more likely to cause Global Warming than Carbon Dioxide. Difluoromethane has found wide use in Asia and other developing regions.
As such, hydrofluorocarbons or HFCs are preferred. CFCs and other aerosols have been ruled as damaging to the ozone layer. Owing to its thermodynamic properties, Difluoromethane is used as a refrigerant. Dichloromethane reacts with Hydrogen Fluoride (HF) in three phases under different conditions. It also has exceptional thermal stability and is generally insoluble in water.ĬH2F2 is industrially manufactured via the fluorination of Dichloromethane (CH2Cl2). It is a colorless and odorless gas that is also mildly inflammable. Here, two Fluorine atoms take the place of Hydrogen atoms in Methane (CH4) to form CH2F2. Being a refrigerant, Difluoromethane is also known as HFC-32 or, more commonly, R-32. The chemical formula CH2F2 represents Difluoromethane.
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