Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경

Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

문제 87a

8장, 문제 87a

(a) Using the electronegativities of Br and Cl, estimate the partial charges on the atoms in the Br¬Cl molecule.

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Identify the electronegativities of bromine (Br) and chlorine (Cl) from the periodic table or a reliable source. Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond.

Compare the electronegativities of Br and Cl. The atom with the higher electronegativity will attract the shared electrons more strongly, resulting in a partial negative charge (δ-), while the other atom will have a partial positive charge (δ+).

Calculate the difference in electronegativity between Cl and Br. This difference will help determine the extent of the partial charges. A larger difference indicates a more polar bond.

Assign the partial charges based on the electronegativity difference. The atom with the higher electronegativity (Cl) will have a partial negative charge, while the atom with the lower electronegativity (Br) will have a partial positive charge.

Express the partial charges using the delta notation: Cl will have a δ- and Br will have a δ+. This notation indicates the direction of the dipole moment in the Br-Cl molecule.

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Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It is a key factor in determining the polarity of a molecule. In the case of the Br-Cl bond, comparing the electronegativities of bromine and chlorine helps predict how the electron density is distributed between the two atoms, leading to the development of partial charges.

Partial Charges

Partial charges occur in polar covalent bonds where electrons are not shared equally between atoms. When one atom is more electronegative, it pulls the shared electrons closer, resulting in a slight negative charge (δ-) on that atom and a slight positive charge (δ+) on the less electronegative atom. In the Br-Cl molecule, the difference in electronegativity will create these partial charges, indicating the molecule's polarity.

Polarity of Molecules

Polarity refers to the distribution of electrical charge over the atoms in a molecule. A molecule is polar if it has a net dipole moment due to the arrangement of its bonds and the electronegativities of its constituent atoms. Understanding the polarity of the Br-Cl molecule is essential for predicting its behavior in different chemical environments, such as solubility and reactivity.

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교과서 질문

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^-?

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교과서 질문

(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?

Consider the collection of nonmetallic elements: B, As, O, and I. (d) Which element would likely to participate in two covalent bonds?

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교과서 질문

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?

987

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교과서 질문

(b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule.

881

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교과서 질문

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?

365

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