Using VSEPR theory there are 4 electron pairs around the central oxygen , 2 of which are bonding and 2 are lone pairs. These electron pairs repel one another pointing approximately to the corners of a tetrahedron, the bond angle F-O-F would be approx 109.5. Not exactly as the lone pair- bonding pair repulsions are stronger than bonding pair - bonding pair repulsion which would lead to a reduction in the angle. This is observed as the bond angle is known to be 1030
Based on it's electronegative difference the kind of bond present in the compound OF2 is a Polar covalent bond.
As I originally stated in my original answer, the bonds in a molecule of OF2 are covalent. The electronegativity difference between them, according to the Pauling values is 0.54, which indicates a slightly polar covalent bond, in which Fluorine has the higher electronegativity value.
Without the lone pairs of electrons, it would be F -- O -- F
OF2 is covalent.
OF2 = Bent structure
Based on it's electronegative difference the kind of bond present in the compound OF2 is a Polar covalent bond.
OF2(Oxygen Difluoride) has a V shape just like H2O. The F-O-F angle is 103 degrees.
As I originally stated in my original answer, the bonds in a molecule of OF2 are covalent. The electronegativity difference between them, according to the Pauling values is 0.54, which indicates a slightly polar covalent bond, in which Fluorine has the higher electronegativity value.
Without the lone pairs of electrons, it would be F -- O -- F
The bond between O and F would be a covalent bond (dative/coordinate), if in fact OF existed. More likely it would exist as OF2 (still covalent bonds).
OF2 is covalent.
OF2 = Bent structure
What is the name of OF2? The correct answer is oxygen difluoride.
of2
Formula: O2F2
yes. with 2 lone pairs, OF2 is a dipole interaction
Since the covalent bond between sulfur and oxygen is polar, dipole dipole attractions are present as intermolecular forces.