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 49

8장, 문제 49

Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.

검증된 단계별 안내

insert step 1> Understand the concept of formal charge: Formal charge is a theoretical charge assigned to atoms in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, regardless of relative electronegativity.

insert step 2> Analyze statement (a): Formal charge is not the same as oxidation number. Oxidation numbers consider the electronegativity of atoms, while formal charges do not.

insert step 3> Analyze statement (b): Minimizing formal charge is a key principle in drawing the best Lewis structure, as it often leads to the most stable arrangement of atoms.

insert step 4> Analyze statement (c): Formal charge does not take into account the different electronegativities of atoms; it assumes equal sharing of electrons.

insert step 5> Analyze statement (d) and (e): Formal charge is not specifically useful for ionic compounds or in calculating dipole moments, as these concepts involve different considerations.

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주요 개념

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Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of bonds, and the number of non-bonding electrons. It helps in determining the most stable Lewis structure by indicating how electrons are distributed among atoms. A formal charge of zero is often preferred for the most stable structures.

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 are essential for visualizing molecular geometry and electron distribution. The best Lewis structure is typically the one that minimizes formal charges across the molecule, leading to greater stability.

Oxidation Number

Oxidation number is a concept used to indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. It differs from formal charge, as oxidation numbers consider the electronegativity of atoms and the overall charge of the molecule, while formal charge is a more localized concept focused on individual atoms in a Lewis structure.

관련 실천

교과서 질문

Draw Lewis structures for the following: (f) NH₂OH

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교과서 질문

Draw Lewis structures for the following: (d) H₂SO₄ (H is bonded to O) (e) OF₂

Write Lewis structures for the following: (a) H2CO (both H atoms are bonded to C), (b) H2O2, (c) C2F6 (contains a C¬C bond), (d) AsO33 - , (e) H2SO3 (H is bonded to O), (f) NH2Cl.

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교과서 질문

For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) SO₂ Write a single Lewis structure that obeys the octet rule for SO₂ and assign the formal charges on all the atoms. (b) SO₃ Write a single Lewis structure that obeys the octet rule for SO₃ and assign the formal charges on all the atoms. (c) SO₃^2- Write a single Lewis structure that obeys the octet rule for SO₃^2- and assign the formal charges on all the atoms.

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교과서 질문

(b) With what allotrope of oxygen is it isoelectronic?

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