Skip to main content
Ch.1 - Structure and Bonding
Wade - Organic Chemistry 9th Edition
Wade9th EditionOrganic ChemistryISBN: 9780135213728당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Wade 9th EditionCh.1 - Structure and Bonding문제 40d,e,f
1장, 문제 40d,e,f

For each of the following structures,
1. Draw a Lewis structure; fill in any nonbonding electrons.
2. Calculate the formal charge on each atom other than hydrogen
d. [(CH3)3O]+
e. CH3NC
f. (CH3)4NBr

검증된 단계별 안내
1
Step 1: For each molecule, start by identifying the total number of valence electrons. For example, in [(CH3)3O]+, calculate the valence electrons for carbon, hydrogen, and oxygen, and adjust for the positive charge.
Step 2: Draw the skeletal structure of the molecule. For [(CH3)3O]+, place the oxygen atom in the center with three CH3 groups attached to it. For CH3NC, connect the carbon atoms in a chain with nitrogen at the end. For (CH3)4NBr, place nitrogen in the center with four CH3 groups and a bromine ion nearby.
Step 3: Distribute the valence electrons around the atoms to satisfy the octet rule, starting with the outer atoms. Remember to account for the positive charge in [(CH3)3O]+ by removing one electron from the total count.
Step 4: Calculate the formal charge for each atom using the formula: Formal Charge = (Valence electrons) - (Nonbonding electrons) - 0.5*(Bonding electrons). Apply this to each atom in the structures, excluding hydrogen.
Step 5: Adjust the structure if necessary to minimize formal charges, ensuring that the most electronegative atoms carry negative charges if possible. Verify that the total charge of the molecule matches the given charge.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
9m
도움이 되었나요?

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of atoms, the distribution of electrons, and the connectivity within a molecule. To draw a Lewis structure, count the total valence electrons, arrange the atoms, and distribute the electrons to satisfy the octet rule for each atom.
추천 영상:
04:12
Drawing the Lewis Structure for N2H4.

Formal Charge Calculation

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated using the formula: Formal Charge = (Valence Electrons) - (Nonbonding Electrons) - (Bonding Electrons/2). It helps in determining the most stable Lewis structure by ensuring that the sum of formal charges in a molecule equals the overall charge of the molecule. Atoms in a molecule are ideally assigned formal charges as close to zero as possible.
추천 영상:
01:34
Calculating formal and net charge.

Nonbonding Electrons

Nonbonding electrons, also known as lone pairs, are valence electrons that are not shared with another atom in a covalent bond. They are important in determining the shape and reactivity of molecules, as they occupy space and can influence molecular geometry according to VSEPR theory. In Lewis structures, nonbonding electrons are represented as pairs of dots around the atom.
추천 영상:
03:54
The 18 and 16 Electron Rule
관련 실천
교과서 질문

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

a.

b.

c.

d.

794
views
교과서 질문

1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.

2. In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.

a. C—Cl

b. C—H

c. C—Li

d. C—N

e. C—O

1179
views
교과서 질문

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

e.

f.

g.

h.

1564
views
1
rank
교과서 질문

Give the molecular formula of each compound shown

(g)

(h)

1079
views
교과서 질문

Give the molecular formula of each compound shown

(d)

(e)

(f)

1064
views
교과서 질문

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

i.

j.

k.

l.

970
views