Question

1. chemical name: bromine tetrafluoride anion formula: brf4- lewis electron - dot structure: perspective drawing with bond angles: standard electron geometry: molecular geometry: hybridization of central atom: is the molecule polar, nonpolar, or ion?

Explanation:

Step1: Determine valence - electrons

Bromine (Br) has 7 valence electrons and each fluorine (F) has 7 valence electrons. Since it is an anion with a - 1 charge, the total number of valence electrons is \(7 + 4\times7+1=36\).

Step2: Draw Lewis - structure

Place Br in the center and surround it with 4 F atoms. Connect each F to Br with a single bond (using 8 electrons). Then distribute the remaining 28 electrons as lone - pairs. Each F gets 3 lone - pairs and Br gets 2 lone - pairs.

Step3: Determine electron - geometry

The central atom Br has 6 electron - groups (4 bonding pairs and 2 lone - pairs). According to VSEPR theory, the electron - geometry is octahedral.

Step4: Determine molecular geometry

With 4 bonding pairs and 2 lone - pairs, the molecular geometry is square planar.

Step5: Determine hybridization

The central atom Br has 6 electron - groups, so the hybridization is \(sp^{3}d^{2}\).

Step6: Determine polarity

The molecule is square planar. The bond dipoles of the Br - F bonds cancel out due to the symmetrical nature of the square planar geometry. But since it is an anion (\(BrF_{4}^{-}\)), it is an ion.

Answer:

Lewis electron - dot structure: Br is in the center with 4 single bonds to F atoms and 2 lone - pairs on Br, and 3 lone - pairs on each F.
Perspective drawing with bond angles: Square planar with bond angles of 90°.
Standard electron geometry: Octahedral
Molecular geometry: Square planar
Hybridization of central atom: \(sp^{3}d^{2}\)
Is the molecule polar, non - polar, or ion? Ion