Oxygen is a non-metal element and is found naturally as a molecule. Each molecule is made up of two oxygen atoms that are strongly joined together. Oxygen has low melting and boiling points, so it is in a gas state at room temperature.

The American Heritage Dictionary of the English Language identifies room temperature as around 20–22 °C (68–72 °F), while the Oxford English Dictionary states that it is “conventionally taken as about 20 °C (68 °F)”.

gas

* Oxygen Difluoride will react slowly with WATER to form corrosive Hydrogen Fluoride gas.

OF2 Molecular Geometry As only atoms are bonded with the central atom, it has a molecular geometry similar to AX2 that corresponds to linear geometry. Although the electron geometry of OF2 is tetrahedral, its molecular geometry is linear.

According to VSEPR (Valence shell electron pair repulsion theory), the molecular geometry of OF2 is bent and its electron geometry is tetrahedral because the presence of two lone pairs on the central atom creates repulsion between bond pairs that make its shape look bent.

Oxygen difluoride, OF2 , is a polar molecule because it has a bent molecular geometry. This molecular geometry ensures that the dipole moments associated with the oxygen – fluoride bonds do not cancel each other out to produce a nonpolar molecule.

I found this equation on the internet for the hydrolysis of OF2: OF2+H2O⟶HF+O2. So, according to me, HF must make generate an acidic instead of neutral solution. But in JD Lee, it is stated that it is a neutral solution.

Oxygen difluoride | OF2 – PubChem.

English: Difluorine monoxide. Fluorine (di-)oxide.

This clearly indicates that oxygen is small in size and does not possess vacant orbitals to accommodate extra electrons. It can only accept two more electrons.

OF₄ can not exist theoretically. It’s electronic configuration is, 2, 8, 6. Valence = 8 – 6 = 2. So, Oxygen may exhibit a valency of 2 at maximum.

This molecule is octahedral in shape. Hydrogen is a very weak oxidizing agent as compared to fluorine this means that hydrogen is not able to oxidise sulphur to its maximum oxidation state. Hence, SH6 does not exist.

Answer. correct answer is OF4 as oxygen is restricted to s and p orbital only which contain maximum 8 electron. Since oxygen(atomic no. 8) has already 6 electron,so it make covalent bond with 2 fluorine atom which completes 8 electron.

Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams. Oxygen atom generally has -2 oxidation state (OS) But O has -1OS (in peroxides and peracids), +1OS in OF4,OS of O is +4 which is not possible.

(A) sf4 (b) of2 (c) of4 (d) o2f2. Reason : Oxygen has two unpaired electrons in its outer most configuration that is why it can make only two covalent bonds , at the same time it can not shift its electrons in nexr orbitals also as it does not have vacant d-orbitals .

But the compound OF4 is not possible to be formed theoretically as the valence electrons in the Oxygen atom is 6 and that is why if four fluorine atoms are associated, the octet configuration will be lost and that is why a stable compound will not be produced.

NO2+​ has sp hybridization because of 2 bond pairs and zero lone pairs and hence, the molecule will be linear.

Explanation: C2 of 2-butanol , and 2-bromobutane have 4 different groups attached, and the compounds are, therefore, capable of supporting optical isomerism, viz.

SF4 is unsymmetrical because of the presence of a lone pair of electrons. Due to which it is a polar molecule.

Is SO3 polar or nonpolar? SO3 is nonpolar and this is because of the trigonal planar shape of sulfur trioxide.

Bond Order =21(10−8)=1. Was this answer helpful?

Tetrahedral Geometry Molecules of methane, CH4, ammonia, NH3, and water, H2O, all have four electron groups around their central atom, so they all have a tetrahedral shape and bond angles of about 109.5°.

valence shell electron pair repulsion

1: Carbon: Always Tetravalent and Often Tetrahedral. Atoms combine in many different ways. As in all its compounds and its elemental forms, carbon is tetravalent, which means that it always forms four bonds. …

CF4 is tetrahedral, so you can consider it to bekind of spherically balanced. Since the four F atoms havethe same electronegativity values, there is no bias in electrondistribution toward any one. Therefore, electron/chargedistribution is symmetrical, which also means that themolecule is nonpolar.