Although I 3 - is a known ion, F 3 - is not. (c) Another classmate says F 3 - does not exist because it would violate the octet rule. Is this classmate possibly correct?

Hello. Everyone in this video. We're going to go ahead and evaluate these three oxygen species and trying to see if they violate the octet rule. So for eight we have hydroxide. Hydroxide is a very known um ion and the O H ion is going to be something that is definitely going to follow the octet rule. All right now the hydroxyl oh H with this little dot here, that's going to be a radical and all radicals do not obey the octet rule. And here we do have what looks to be an ion. However, there's a little dot again and that indicates that we have an ionic radical and like a radical. This also does not obey the octet rule. So based on these evaluations here, it means the only one that obeys the octet rule is going to be a our ion. I'm going to highlight this answer and a is going to be the final answer for our problem because it's the only one that will obey the octet rule.

Ch.8 - Basic Concepts of Chemical Bonding

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 89c

Chapter 8, Problem 89c

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?

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Understand the octet rule: Atoms tend to form compounds in ways that give them eight valence electrons, achieving a noble gas configuration.

Consider the electron configuration of fluorine: Fluorine has 7 valence electrons and needs 1 more to complete its octet.

Analyze the formation of I3-: In I3-, iodine can expand its octet because it has d orbitals available, allowing it to accommodate more than 8 electrons.

Evaluate the possibility of F3-: Fluorine, being in the second period, does not have d orbitals and cannot expand its octet beyond 8 electrons.

Conclude that F3- would violate the octet rule because fluorine cannot accommodate more than 8 electrons, supporting the classmate's statement.

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Key Concepts

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

Octet Rule

The octet rule is a chemical guideline that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict the formation of stable molecules and ions. In the case of F3-, the classmate's assertion is based on the idea that fluorine, which has seven valence electrons, cannot accommodate more than eight electrons without violating this rule.

Ionic and Molecular Species

Ionic species are formed when atoms transfer electrons, resulting in charged ions, while molecular species are formed through covalent bonding, where atoms share electrons. I3- is a known polyatomic ion consisting of three iodine atoms, while F3- would imply a hypothetical ion with three fluorine atoms. Understanding the nature of these species is crucial in evaluating the stability and existence of such ions.

Electron Configuration and Stability

Electron configuration refers to the distribution of electrons in an atom's orbitals, which influences its chemical properties and reactivity. Stability in ions and molecules often arises from achieving a full valence shell. In the case of F3-, the proposed configuration would lead to an unstable arrangement, as fluorine atoms would struggle to maintain a stable electron configuration while sharing or gaining additional electrons.

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Related Practice

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.

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. (d) What is the formal charge on hydrogen in the polyatomic ion?

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.

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 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?

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?

Verified video answer for a similar problem:

Key Concepts

Octet Rule

Ionic and Molecular Species

Electron Configuration and Stability

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?