Textbook Question
Although I3- is a known ion, F3- is not. (c) Another classmate says F3- does not exist because it would violate the octet rule. Is this classmate possibly correct?
Ch.8 - Basic Concepts of Chemical Bonding
Chapter 8, Problem 91c,d
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?
Verified step by step guidance1
To draw the Lewis structure for the hypochlorite ion (ClO-), start by counting the total number of valence electrons. Chlorine (Cl) has 7 valence electrons, and oxygen (O) has 6 valence electrons. The negative charge adds one more electron, giving a total of 14 valence electrons.
Arrange the atoms with chlorine as the central atom and oxygen bonded to it. Place a single bond between Cl and O, which uses 2 electrons. Distribute the remaining electrons to satisfy the octet rule, starting with the outer atom (oxygen) and then the central atom (chlorine).
For the perchlorate ion (ClO4-), count the total valence electrons: chlorine has 7, each oxygen has 6, and the negative charge adds one more electron, totaling 32 valence electrons. Place chlorine in the center and arrange four oxygen atoms around it, each connected by a single bond.
Distribute the remaining electrons to complete the octets for each oxygen atom first, then the chlorine atom. Remember that the perchlorate ion can have resonance structures due to the possibility of multiple bonds between Cl and O.
To find the oxidation number of Cl in each ion, use the rule that oxidation numbers are assigned based on the assumption that all bonds are ionic. In ClO-, assign oxygen an oxidation number of -2, and solve for Cl. In ClO4-, assign each oxygen an oxidation number of -2, and solve for Cl, considering the overall charge of the ion.
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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 hypochlorite and perchlorate, drawing their Lewis structures allows us to identify the formal charges and the overall electron distribution.
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Oxidation Numbers
Oxidation numbers are a way to keep track of electron transfer in chemical reactions, indicating the degree of oxidation of an atom in a compound. They are assigned based on a set of rules, such as the oxidation number of oxygen is typically -2, and the sum of oxidation numbers in a neutral compound is zero. Understanding oxidation numbers is essential for determining the oxidation state of chlorine in the hypochlorite and perchlorate ions.
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Ionic Compounds and Bonding
Ionic compounds are formed when atoms transfer electrons, resulting in the formation of charged ions that attract each other due to electrostatic forces. In the context of hypochlorite and perchlorate ions, recognizing that chlorine is bonded to oxygen through ionic interactions helps in understanding the stability and reactivity of these ions. This knowledge is fundamental when analyzing their roles in various chemical processes, such as in bleach and rocket propellants.
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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).
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. (b) What is the formal charge 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?
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?