Draw Lewis structures for the following free radicals. a. The ethyl radical, CH3—ĊH2 b. The tert-butyl radical, (CH3)3C•

Ch.4 - The Study of Chemical Reactions

Wade9th EditionOrganic ChemistryISBN: 9780135213728당신이 사용하는 게 아니라요?교과서 변경

모든 교과서

Wade 9th Edition

Ch.4 - The Study of Chemical Reactions

문제 1

4장, 문제 1

Draw Lewis structures for the following free radicals.
a. The ethyl radical, CH₃—ĊH₂
b. The tert-butyl radical, (CH₃)₃C•

검증된 단계별 안내

Step 1: Understand that a free radical is a molecule that contains an unpaired electron. This unpaired electron is typically represented as a dot (•) in Lewis structures.

Step 2: For the ethyl radical (CH3—CH2•), start by drawing the Lewis structure for ethane (CH3—CH3). Ethane consists of two carbon atoms single-bonded to each other, with each carbon atom also bonded to three hydrogen atoms.

Step 3: To convert ethane to the ethyl radical, remove one hydrogen atom from the CH2 group, leaving an unpaired electron on the second carbon atom. The structure should now be CH3—CH2•, with the dot representing the unpaired electron on the second carbon.

Step 4: For the tert-butyl radical ((CH3)3C•), begin by drawing the Lewis structure for tert-butyl cation ((CH3)3C+). This involves a central carbon atom bonded to three methyl groups (CH3).

Step 5: To form the tert-butyl radical, replace the positive charge with an unpaired electron. The central carbon atom will have three single bonds to the methyl groups and one unpaired electron, represented as (CH3)3C•.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

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 electrons around atoms, which helps in understanding the molecule's geometry, reactivity, and properties. In the case of free radicals, the Lewis structure will show an unpaired electron, which is crucial for identifying the radical nature of the molecule.

Free Radicals

Free radicals are atoms or molecules that contain an unpaired electron, making them highly reactive. In organic chemistry, radicals are often intermediates in reactions and can be identified by a single dot representing the unpaired electron in their Lewis structures. Understanding free radicals is important for predicting reaction mechanisms and the stability of different radical species.

Hybridization and Molecular Geometry

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals, which influences the geometry and bonding properties of molecules. For example, the carbon atoms in ethyl and tert-butyl radicals are typically sp3 hybridized, leading to a tetrahedral geometry. Recognizing the hybridization helps in accurately drawing the Lewis structures and understanding the spatial arrangement of atoms and electrons in radicals.