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Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis
Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Mullins 1st EditionCh. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis문제 44a
2장, 문제 44a

Based on the formal charge, determine how many lone pairs are on each indicated atom.
(a) Diagram showing a molecule with labeled atoms (a) OH group and (b) O atom, indicating formal charge and lone pairs.

검증된 단계별 안내
1
Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons). This formula will help us determine the number of lone pairs on the indicated atom.
Step 2: Identify the valence electrons for the indicated atom. Refer to the periodic table to determine the number of valence electrons for the atom in question.
Step 3: Count the bonding electrons around the indicated atom. These are the electrons shared in covalent bonds. Each bond contributes two electrons.
Step 4: Count the non-bonding electrons (lone pairs) around the indicated atom. These are the electrons not involved in bonding. Use the formal charge formula to solve for the number of non-bonding electrons.
Step 5: Divide the non-bonding electrons by two to determine the number of lone pairs on the indicated atom. Verify your result by ensuring the formal charge matches the given or expected value.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m

주요 개념

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

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated by taking the number of valence electrons in the free atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms.
추천 영상:
01:34
Calculating formal and net charge.

Lone Pairs

Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a specific atom. They play a crucial role in determining the geometry and reactivity of molecules, as they can influence the shape and polarity of the molecule.
추천 영상:
가이드 코스
2:56
Base Pairing Concept 1

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 representation of the arrangement of electrons, allowing for the determination of formal charges and the identification of lone pairs on specific atoms.
추천 영상:
04:12
Drawing the Lewis Structure for N2H4.
관련 실천
교과서 질문

Given the line-angle drawings shown, answer the following questions:

(i) How many carbons are in each molecule?

(ii) How many hydrogens are at the circled carbon?

(iii) Is the indicated (→) carbon or 1° , 2°, 3°, or 4°?

(c)

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교과서 질문

Draw the most stable chair conformation for the following trisubstituted cyclohexane.

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교과서 질문

Draw two different chair conformations for each of the following molecules. Make sure that your drawings clearly show the cis–trans stereochemistry.

(c)

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교과서 질문

Modify the following line-angle drawings to show all lone pairs.

(b)

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교과서 질문

Modify the following line-angle drawings to show all lone pairs.

(a)

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교과서 질문

For each pair of conformations you drew in Assessment 3.41, indicate which is most stable.

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