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Ch.8 - Basic Concepts of Chemical Bonding
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.8 - Basic Concepts of Chemical BondingProblem 91b
Chapter 8, Problem 91b

The hypochlorite ion, ClO-, is the active ingredient in bleach. The perchlorate ion, ClO4-, is a main component of rocket propellants. Draw Lewis structures for both ions. (b) What is the formal charge of Cl in the perchlorate ion, assuming the Cl—O bonds are all single bonds?

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1
Step 1: For the hypochlorite ion (ClO^-), start by counting the total number of valence electrons. Chlorine has 7 valence electrons, oxygen has 6, and the negative charge adds 1 more electron, totaling 14 electrons.
Step 2: Draw the skeletal structure for ClO^-. Place Cl and O next to each other and connect them with a single bond. Distribute the remaining electrons to satisfy the octet rule, starting with the more electronegative atom, oxygen.
Step 3: For the perchlorate ion (ClO4^-), count the total number of valence electrons. Chlorine has 7 valence electrons, each oxygen has 6, and the negative charge adds 1 more electron, totaling 32 electrons.
Step 4: Draw the skeletal structure for ClO4^-. Place Cl in the center and connect it to four O atoms with single bonds. Distribute the remaining electrons to satisfy the octet rule for each oxygen atom.
Step 5: To find the formal charge of Cl in ClO4^-, use the formula: Formal Charge = (Valence electrons of Cl) - (Non-bonding electrons on Cl) - (Bonding electrons/2). Assume all Cl—O bonds are single bonds.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for understanding molecular geometry and reactivity. In the case of ions like ClO- and ClO4-, drawing the Lewis structure allows us to see how the chlorine and oxygen atoms are bonded and the distribution of electrons.
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Formal Charge

Formal charge is a concept used to determine the charge of an atom in a molecule or ion, calculated by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the Lewis structure. It helps assess the stability of a molecule and the distribution of charge. For the perchlorate ion, calculating the formal charge of chlorine involves considering its valence electrons and the bonds it forms with oxygen.
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Ionic and Covalent Bonds

Ionic and covalent bonds are two primary types of chemical bonds. Ionic bonds occur when electrons are transferred from one atom to another, resulting in charged ions, while covalent bonds involve the sharing of electrons between atoms. In the context of the hypochlorite and perchlorate ions, understanding these bonding types is essential for analyzing their structures and properties, particularly when considering the nature of the Cl—O bonds.
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Related Practice
Textbook Question

Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in O3 (b) phosphorus in PF6- (c) nitrogen in NO2 (d) iodine in ICl3 (e) chlorine in HClO4 (hydrogen is bonded to O).

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Textbook Question

Although I3- is a known ion, F3- is not. (b) One of your classmates says that F3- does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong.

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Textbook Question

The following three Lewis structures can be drawn for N2O:

(b) The N—N bond length in N2O is 1.12 Å, slightly longer than a typical N≡N bond; and the N—O bond length is 1.19 Å, slightly shorter than a typical N═O bond (see Table 8.4). Based on these data, which resonance structure best represents N2O?

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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. (c) Based on electronegativity differences, predict the identity of the polyatomic anion. Draw a Lewis structure for this ion.

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Textbook Question

The hypochlorite ion, ClO-, is the active ingredient in bleach. The perchlorate ion, ClO4-, is a main component of rocket propellants. Draw Lewis structures for both ions. (c) What is the oxidation number of Cl in the hypochlorite ion? (d) What is the oxidation number of Cl in the perchlorate ion, assuming the Cl—O bonds are all single bonds?

Textbook Question

The following three Lewis structures can be drawn for N2O:

(a) Using formal charges, which of these three resonance forms is likely to be the most important?

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