AGNuke said:You can take Lone Pair-Bond pair repulsions, Interaction of H and F (due to their size difference), F F interactions, and probably C-H C-F Bond interaction.
AGNuke said:Two C-F bonds will repel each other, thus they will try to maximize their angle, but their repulsion with lone pair is even greater, hence they will be forced to elongate themselves in order to face minimal repulsion from each other and the lone pair.
Try to work on this.
AGNuke said:Might be. But you should check around the internet for factual data before putting your vote in my "theory".
See, I am assuming that you are preparing for college entrance exam (JEE).
A C-F bond length refers to the distance between the carbon atom and the fluorine atom in a molecule. It is a measure of the strength and stability of the bond between these two atoms.
C-F bond length is typically determined using spectroscopic techniques, such as infrared or nuclear magnetic resonance (NMR) spectroscopy. These methods allow scientists to measure the distance between the carbon and fluorine atoms in a molecule.
The main factors that affect C-F bond length are the electronegativity of the atoms involved and the presence of any nearby functional groups. As fluorine is highly electronegative, it tends to pull electrons towards itself, resulting in a shorter bond length.
The C-F bond is one of the strongest bonds in organic chemistry, making molecules containing this bond highly stable. This also makes them resistant to chemical reactions, which can be useful in certain applications, such as in pharmaceuticals.
Yes, there is a general trend of decreasing C-F bond length as you move down a group in the periodic table. This is due to the increasing atomic size and decreasing electronegativity of the atoms involved.