CF 4 has a Tetrahedral molecular structure and shape with bond angles of 109.5 °. The hybridization of the CF 4 is given by sp 3. In its most stable state, the Carbon atom forms covalent atoms with the Fluorine atoms. CF 4 comprises a Carbon atom surrounded by four Fluorine atoms. Let’s quickly summarize the salient features of Carbon Tetrafluoride Since there are no lone pairs, the electron geometry is Tetrahedral as well. Therefore, the molecular geometry of CF 4 is Tetrahedral. F ormula Shape Bond Angle ( Theoretical ) AX 2 Linear 180 AX 3 Trigonal Planar 120 AX 4 Tetrahedral 109.5 AX 5 Trigonal Bipyrimidal 120, 90 AX 6 Octahedral 90 AX 2 N Bent 120 AX 2 N 2 Bent 109.5 From the A-X-N table below, we can determine the molecular geometry. We can ignore ‘N’ since there are no lone pairs. Therefore, that would give us AX 4 for the CF 4 molecule. ‘N’ represents the number of lone pairs attached to the central atom. In this case, there are four Fluorine atoms bonded to the central Carbon atom. ‘X’ represents the number of atoms bonded to the central atom. This can also be determined by using the steric number or the A-X-N method. This results in a Tetrahedral molecular geometry, as shown. As such, the bond angle of CF 4 is 109.5 °. CF 4 Bond AnglesĪccording to the VSEPR theory, the Fluorine atoms all repel each other forming a tetrahedral shape. Pi-bonds are absent, making the structure remarkably stable.Īs such, the hybridization of the central Carbon atom is sp 3. Sigma bonds are formed between Carbon and Fluorine. To know more about the hybridization of CF 4 in detail, we look into the nature of the C-F bond. This is especially true for non-polymeric arrangements. The number of electron domains is an easy way to determine the hybridization of a molecule. This structure gives rise to four electron domains. There are four covalent bonds present between Carbon and Fluorine. To determine the hybridization, we take a quick look at the Lewis structure of the CF 4 molecule shown above. The Carbon Tetrafluoride molecule comprises four Fluorine atoms, all pulled together by the central Carbon atom. The Lewis Structure is stable due to all of the outermost shells being filled for each element. There is no need to check for formal charges as the octet rule is fulfilled for all of the atoms as shown. From the figure below, it is seen that the central Carbon atom forms four covalent bonds. 
We then begin drawing up the Lewis structure by forming C-F bonds using the available valence electrons. The Fluorine atoms in CF 4 are then placed around the central Carbon atom.
This arrangement lets it form covalent bonds with the surrounding Fluorine atoms. CF 4 Lewis StructureĬarbon acts as the central atom in the structure. Therefore, the total number of valence electrons in CF 4 is given by:Īs a result there are 32 valence electrons for CF4.
Therefore, the four Fluorine atoms present contribute: 7 x 4 = 28 Valence Electrons. Therefore, a single carbon atom contributes: 4 x 1 = 4 Valence Electrons.įluorine is in group 17 of the periodic table with the electronic configuration 2s 2 2p 5. This, in turn, makes these electrons readily available upon excitation.Ĭarbon Tetrafluoride comprises four Fluorine atoms and a single Carbon atom.Ĭarbon is in group 4 of the periodic table with the electronic configuration 2s 2 2p 2. They are present in the atom’s outermost shell, where the force of attraction from the nucleus is relatively less. Valence electrons are those electrons that are available for exchanges and bond formation. CF4 Molecular Geometry and Shape CF 4 Valence Electrons.
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