BrF is polar, its dipole moment is known, 1.4D . Dipole -dipole will be the strongest intermolecular force. Dispersion forces will also be present. The argument runs -
Dispersion forces are caused by the total number of electrons, compare BrF (number of electrons 44 with noble gases say Xenon, 54 electrons)
BrF decomposes around 200C , its boiling point which is considerably higher than the bp of xenon (-108 oC). Indicating factors other than disperison forces are at play causing the bp to be so high.
Br +3, balanced by 3 fluorines each with -1.
The atoms in the reacts are always present in the products. There is one mole of bromine per molecule and .196 moles of the molecule. Thus, there will be .196 mols of bromine present after the reaction.
well BrF3 will auto dissociate to give BrF4- + BrF2+ ...the KF will give a F- to the BrF3 obviously this giving is really due the higher electronegativity of the fluorine thus their will be an increase in the amounts of BrF4- in solution .Using the solvent-system definition of an acid or base.Any specie (molecule ,ion)which increases the anionic or negatively charged amounts of species in solution is a base.So KF definitely behaves as a base. You can use this same reasoning for SnF4 and try and figure that one out on your own.good luck .
Geometric isomers, also known as cis-trans isomers, occur when the spatial arrangement of atoms differs due to restricted rotation around a double bond or ring. In the case of BrF3, there are no geometric isomers because the molecule has a T-shaped molecular geometry with three fluorine atoms and one bromine atom located at the equatorial positions, resulting in a symmetrical structure. Therefore, BrF3 does not exhibit geometric isomerism.
a) XeOF4: square planar b) SF4: see-saw c) FOF: linear d) BrF3: T-shaped e) XeF2: linear
The chemical formula for bromine trifluoride is BrF3.
Br +3, balanced by 3 fluorines each with -1.
BrF3
Formula: BrF3
It is hard to say, because BrF is readily disproportioning into Br2,(l) and BrF3,(l) according to:3 BrF → BrF3 + Br2Bromine trifluoride, BrF3, is boiling at 125.72 °CCompared with Chlorine fluoride: this, ClF, is an (also) unstable brownish yellow gas (with boiling point 5°C)
The steric number of the central bromine atom in BrF3 is 5. This is because BrF3 has 3 bonded fluorine atoms and 2 lone pairs on the bromine atom, giving a total of 5 electron domains around the central atom.
The atoms in the reacts are always present in the products. There is one mole of bromine per molecule and .196 moles of the molecule. Thus, there will be .196 mols of bromine present after the reaction.
Out of SiCl4, BrF5, AsF5, BrF3, only SiCl4 has sp3 hybridization on the central atom, which is silicon. SiCl4 has four regions of electron density around the central silicon atom, leading to sp3 hybridization. The other compounds have different geometries and hybridizations: BrF5 and AsF5 have sp3d2 hybridization, while BrF3 has sp3d hybridization.
The preferred geometry of molecule BrF3 or bromine trifluoride is a planar "T-shaped" molecule. This is due to the two lone pairs of electrons on bromine, which cause a repulsion from the fluorine atoms.
well BrF3 will auto dissociate to give BrF4- + BrF2+ ...the KF will give a F- to the BrF3 obviously this giving is really due the higher electronegativity of the fluorine thus their will be an increase in the amounts of BrF4- in solution .Using the solvent-system definition of an acid or base.Any specie (molecule ,ion)which increases the anionic or negatively charged amounts of species in solution is a base.So KF definitely behaves as a base. You can use this same reasoning for SnF4 and try and figure that one out on your own.good luck .
Geometric isomers, also known as cis-trans isomers, occur when the spatial arrangement of atoms differs due to restricted rotation around a double bond or ring. In the case of BrF3, there are no geometric isomers because the molecule has a T-shaped molecular geometry with three fluorine atoms and one bromine atom located at the equatorial positions, resulting in a symmetrical structure. Therefore, BrF3 does not exhibit geometric isomerism.
a) XeOF4: square planar b) SF4: see-saw c) FOF: linear d) BrF3: T-shaped e) XeF2: linear