Textbook Question
Consider the collection of nonmetallic elements: B, As, O, and I. (d) Which element would likely to participate in two covalent bonds?
Ch.8 - Basic Concepts of Chemical Bonding
Chapter 8, Problem 87a
(a) Using the electronegativities of Br and Cl, estimate the partial charges on the atoms in the Br¬Cl molecule.
Verified step by step guidance1
First, understand the concept of electronegativity: Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The higher the electronegativity, the more an atom attracts electrons.
Identify the electronegativities of bromine (Br) and chlorine (Cl) from a reliable source, such as a chemistry textbook or database. Typically, chlorine has a higher electronegativity than bromine.
Determine the difference in electronegativity between the two atoms. This difference will help you understand how the electrons are distributed in the Br-Cl bond.
Use the electronegativity difference to estimate the partial charges: The atom with the higher electronegativity (Cl) will have a partial negative charge (δ-), while the atom with the lower electronegativity (Br) will have a partial positive charge (δ+).
Express the partial charges in the Br-Cl molecule using the symbols δ+ and δ-. This notation indicates the direction of electron density shift due to the difference in electronegativity.
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Related Practice
Textbook Question
The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of 1.24 D, and the Cl — O bond length is 160 pm. (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the ClO molecule?
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Textbook Question
The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of 1.24 D, and the Cl—O bond length is 160 pm. (c) Using formal charges as a guide, propose the dominant Lewis structure for the molecule. (g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of 1.24 D, and the Cl—O bond length is 160 pm. (d) The anion ClO exists. What is the formal charge on the Cl for the best Lewis structure for ClO-?
Textbook Question
(b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule.
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Textbook Question
(c) The measured dipole moment of BrCl is 0.57 D. If you assume the bond length in BrCl is the sum of the atomic radii, what are the partial charges on the atoms in BrCl using the experimental dipole moment?
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Textbook Question
A major challenge in implementing the 'hydrogen economy' is finding a safe, lightweight, and compact way of storing hydrogen for use as a fuel. The hydrides of light metals are attractive for hydrogen storage because they can store a high weight percentage of hydrogen in a small volume. For example, NaAlH4 can release 5.6% of its mass as H2 upon decomposing to NaH(s), Al(s), and H2(g). NaAlH4 possesses both covalent bonds, which hold polyatomic anions together, and ionic bonds. (b) Which element in NaAlH4 is the most electronegative? Which one is the least electronegative? Which element in NaAlH4 is the least electronegative?
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