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Chapter 11: Problem 10

What is the hybridization of bromine in each of the following: (a) \(\mathrm{BrF}_{3} ;\) (b) \(\mathrm{BrO}_{2}^{-} ;\) (c) \(\mathrm{BrF}_{5} ?\)

Short Answer

Expert verified
(a) sp3d; (b) sp3d; (c) sp3d2

Step by step solution

01

Determine Valence Electrons for Bromine

Bromine (Br) is in Group 17 of the periodic table, so it has 7 valence electrons.
02

Calculate Total Electron Pairs

Determine the total number of electron pairs around bromine for each compound or ion. This includes bonding pairs and lone pairs.
03

Analyze \(\text{BrF}_{3}\)

Bromine has 7 valence electrons. It forms three single bonds with fluorine atoms, using 3 pairs. The remaining 2 pairs are lone pairs. Total electron pairs around bromine are 5 (3 bonding + 2 lone pairs). Thus, the hybridization is \(\text{sp}^{3}\text{d}\).
04

Analyze \(\text{BrO}_{2}^{-}\)

First, add the extra electron due to the negative charge, so bromine has 8 electrons now. Bromine forms two single bonds with oxygen. This uses 2 pairs. The remaining 3 pairs are lone pairs. Total electron pairs around bromine are 5 (2 bonding + 3 lone pairs). Therefore, the hybridization is \(\text{sp}^{3}\text{d}\).
05

Analyze \(\text{BrF}_{5}\)

Bromine has 7 valence electrons and forms five single bonds with fluorine atoms, using 5 pairs. The remaining 1 pair is a lone pair. Total electron pairs around bromine are 6 (5 bonding + 1 lone pair). Thus, the hybridization is \(\text{sp}^{3}\text{d}^{2}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Valence Electrons
Valence electrons are the electrons located in the outermost shell of an atom. These electrons play a crucial role in chemical bonding and reactions.
For bromine (Br), which belongs to Group 17 of the periodic table, there are 7 valence electrons.
Valence electrons determine how atoms interact with each other, as they can be shared or transferred to form bonds.
Bonding Pairs
Bonding pairs refer to pairs of electrons that are shared between two atoms, forming a covalent bond.
In \(\text{BrF}_{3}\), bromine forms three single bonds with fluorine atoms, which means there are three bonding pairs.
Bonding pairs are critical in determining the geometry and hybridization of molecules.
Lone Pairs
Lone pairs are pairs of valence electrons that are not involved in bonding and remain on a single atom.
For example, in \(\text{BrF}_{3}\), besides three bonding pairs, there are two lone pairs on bromine.
Lone pairs can influence the shape and hybridization of molecules by repelling bonding pairs.
Electron Pairs
Electron pairs encompass both bonding pairs and lone pairs.
To determine the hybridization of an atom, total electron pairs around the atom are considered.
In \(\text{BrO}_{2}^{-} \), bromine has a total of 5 electron pairs (2 bonding + 3 lone pairs). This leads to an \(\text{sp}^{3}\text{d}\) hybridization.
Hybridization in Bromine Compounds
Hybridization involves mixing atomic orbitals to form new hybrid orbitals that can accommodate electron pairs.
In bromine compounds:
* \(\text{BrF}_{3} \) has hybridization \(\text{sp}^{3}\text{d}\) due to 5 electron pairs
* \(\text{BrO}_{2}^{-}\) also has \(\text{sp}^{3}\text{d}\) hybridization with 5 electron pairs.
* \(\text{BrF}_{5}\) has \(\text{sp}^{3}\text{d}^{2}\) hybridization owing to 6 electron pairs.
Hybridization is essential for understanding the geometry and bonding in molecules.

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Most popular questions from this chapter

Give the number and type of hybrid orbital that forms when each set of atomic orbitals mixes: (a) two \(d\), one \(s\), and three \(p\) (b) three \(p\) and one \(s\)

Linoleic acid is an essential fatty acid found in many vegetable oils, such as soy, peanut, and cottonseed. A key structural feature of the molecule is the cis orientation around its two double bonds, where \(\mathrm{R}_{1}\) and \(\mathrm{R}_{2}\) represent two different groups that form the rest of the molecule. (a) How many different compounds are possible, changing only the cis-trans arrangements around these two double bonds? (b) How many are possible for a similar compound with three double bonds?

Methyl isocyanate, \(\mathrm{CH}_{3}-\ddot{\mathrm{N}}=\mathrm{C}=\ddot{\mathrm{O}}:,\) is an intermediate in the manufacture of many pesticides. In \(1984,\) a leak from a manufacturing plant resulted in the death of more than 2000 people in Bhopal, India. What are the hybridizations of the \(\mathrm{N}\) atom and the two \(\mathrm{C}\) atoms in methyl isocyanate? Sketch the molecular shape.

How many hybrid orbitals form when four atomic orbitals of a central atom mix? Explain.

2-Butene \(\left(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CHCH}_{3}\right)\) is a starting material in the manufacture of lubricating oils and many other compounds. Draw two different structures for 2 -butene, indicating the \(\sigma\) and \(\pi\) bonds in each.
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