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 54b

8장, 문제 54b

Consider the formate ion, HCO₂^-, which is the anion formed when formic acid loses an H⁺ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?

검증된 단계별 안내

insert step 1> Identify the central atom in the formate ion, HCO_2^-. In this case, the central atom is carbon (C).

insert step 2> Draw the Lewis structure for the formate ion. Start by arranging the atoms with carbon in the center, hydrogen (H) and two oxygen (O) atoms bonded to it.

insert step 3> Count the total number of valence electrons available. Carbon has 4, each oxygen has 6, and hydrogen has 1. The negative charge adds an extra electron, making a total of 18 valence electrons.

insert step 4> Distribute the electrons to satisfy the octet rule for each atom, starting with the outer atoms (oxygen) and then the central atom (carbon).

insert step 5> Determine if resonance structures are needed by checking if there are multiple ways to arrange the electrons while maintaining the same arrangement of atoms. In the case of the formate ion, consider if the double bond can be placed between carbon and either oxygen atom, indicating resonance.

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주요 개념

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Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In molecules where multiple valid Lewis structures can be drawn, resonance helps to represent the actual distribution of electrons more accurately. The true structure is a hybrid of these resonance forms, which can affect the stability and reactivity of the molecule.

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 provide a visual way to understand how atoms are connected and the arrangement of electrons. For the formate ion, drawing the Lewis structure helps to identify the presence of resonance by showing how electrons can be distributed differently among the atoms.

Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule and to assess the stability of different resonance structures. It is calculated by taking the number of valence electrons in an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. A lower formal charge on atoms typically indicates a more stable structure, guiding the selection of the most significant resonance forms.

관련 실천

교과서 질문

Consider the formate ion, HCO₂^-, which is the anion formed when formic acid loses an H⁺ ion. The H and the two O atoms are bonded to the central C atom. (c) Would you predict that the C—O bond lengths in the formate ion would be longer or shorter relative to those in CO₂?

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교과서 질문

Predict the ordering, from shortest to longest, of the bond lengths in CO, CO₂, and CO₃^2- .

845

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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.

573

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교과서 질문

Based on Lewis structures, predict the ordering, from shortest to longest, of N¬O bond lengths in NO+, NO2-, and NO3-.

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

622

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