Final answer:
Bromine pentafluoride has a Lewis dot structure with a central bromine atom bonded to five fluorines and one lone pair on bromine. It has a square pyramidal geometry, zero formal charge on bromine, +5 and -1 oxidation states for bromine and fluorine respectively, bond angles of roughly 90° and 180°, contains polar bonds, and is an overall polar molecule due to its geometry.
Step-by-step explanation:
Properties of Bromine Pentafluoride (BrF5)
Bromine pentafluoride (BrF5) is an interhalogen compound with several interesting properties. Each aspect of this compound reveals more about its chemical characteristics.
a) Lewis dot structure for bromine pentafluoride
The Lewis dot structure of BrF5 shows a central bromine atom with five fluorine atoms bonded to it. Each fluorine has three lone pairs, while the bromine has one lone pair.
b) Formal charge on bromine
The formal charge is zero, as bromine shares one electron with each fluorine and has one lone pair.
c) Oxidation states for Bromine and Fluorine
Bromine in BrF5 has an oxidation state of +5, while each fluorine has an oxidation state of -1.
d) Bond angle in bromine pentafluoride
Since the geometry of BrF5 is a square pyramidal, the bond angles are approximately 90 degrees and 180 degrees.
e) Geometry of bromine pentafluoride
The geometry of BrF5 is square pyramidal, which is due to five groups around the central bromine atom: three bonding pairs and two lone pairs directed towards the vertices of a trigonal bipyramid.
f) Type of bonds in the molecule
This molecule contains polar bonds due to the difference in electronegativity between bromine and fluorine atoms.
g) Polarity of the molecule
The molecule overall is polar because of the asymmetrical distribution of polar bonds and the presence of a lone pair on the central atom which distorts the symmetry.