Question

1. chemical name: bromine difluoride anion formula: brf₂⁻ 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, each Fluorine (F) has 7 valence electrons, and there is an extra electron due to the negative charge. So the total number of valence electrons is \(7 + 2\times7+ 1=22\).

Step2: Draw Lewis structure

Place Br in the center. Connect Br to two F atoms with single bonds. Then distribute the remaining electrons as lone - pairs. Br has 3 lone - pairs and each F has 3 lone - pairs.

Step3: Calculate electron - domain geometry

The number of electron domains around the central Br atom is \(2\) (bonding pairs) \(+ 3\) (lone - pairs) \(= 5\). So the standard electron geometry is trigonal bipyramidal.

Step4: Determine molecular geometry

With 2 bonding pairs and 3 lone - pairs, the molecular geometry is linear.

Step5: Find hybridization

For 5 electron domains around the central atom, the hybridization of the central Br atom is \(sp^{3}d\).

Step6: Determine polarity

Since the molecular geometry is linear and the bond dipoles cancel out (symmetrical arrangement), and it is an ion (\(BrF_{2}^{-}\)), it is an ion.

Answer:

Lewis electron - dot structure: Br is in the center with single bonds to two F atoms. Br has 3 lone - pairs and each F has 3 lone - pairs.
Perspective drawing with bond angles: Linear, bond angle \(180^{\circ}\)
Standard electron geometry: Trigonal bipyramidal
Molecular geometry: Linear
Hybridization of central atom: \(sp^{3}d\)
Is the molecule polar, non - polar, or ion? Ion