Chlorine monofluoride is a volatile interhalogen compound with the chemical formula ClF. It is a colorless gas at room temperature and is stable even at high temperatures.
Chlorine Trifluoride
dsp^3
or
sp^3d^1
the f-p-f bond angle is 120the cl -p-cl bond angle is 180and the f - p - cl bond angle is 90
P-S , H-F, P-Cl
F-F Cl-Cl or any other halogen-halogen ;halogen- alkaline metal Na-Cl
Br I N Cl H O F
F
the f-p-f bond angle is 120the cl -p-cl bond angle is 180and the f - p - cl bond angle is 90
P-S , H-F, P-Cl
F is the stronger base because it is bigger than Cl
F-F Cl-Cl or any other halogen-halogen ;halogen- alkaline metal Na-Cl
Br I N Cl H O F
F
Total electrons --> 7+42-1=48 Cl as a central atom One lone pair on Cl (on the side) 4 F's up and down and the other two on the opposite side of lone pair. F I :- Cl - F - F I F This is the best I can do with plain text.
yeet
As-F bonds should be more polar, because fluorine is the most electronegative of all elements.
Cl and F
bond energy (in kJ/mol) F-F:158 Cl-Cl: 244 Hence, in order of decreasing bond strength: Cl-Cl => => (F-F) => Fluorine is an anomaly. Bond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker. Fluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond. I hope that answers your question.
CCl2F2 has a tetrahedral molecular geometry, since the central atom (C) has four bonds around it, 2 with Cl, and 2 with F.