교과서 질문
What is the most common oxidation state for each of the
group 3A elements?
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
22장, 문제 86a
(a) Describe what is meant by an electron-deficient molecule.
검증된 단계별 안내1
An electron-deficient molecule is a term used in molecular chemistry to describe a molecule that has fewer than eight electrons around an atom in the molecule. This is in contrast to the 'octet rule' which states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas.
The term 'electron-deficient' is often used to describe molecules that cannot form a complete set of bonds using only the electrons from their valence shells. This can occur in molecules with elements from the second period of the periodic table (such as boron, beryllium) which have fewer than four valence electrons.
Electron-deficient molecules are often reactive, as they tend to accept electrons from other atoms or molecules to achieve a stable electron configuration. This makes them good Lewis acids, or electron pair acceptors.
In some cases, electron-deficient molecules can form stable structures by sharing electrons between more than two atoms, resulting in what's known as 'electron-deficient bonding' or '3-center 2-electron bonds'. An example of this is the boron hydrides (boranes).
Understanding the concept of electron-deficient molecules is important in chemistry as it helps predict the reactivity and bonding behavior of molecules.
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주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Electron Deficiency
Electron deficiency refers to a situation where a molecule has fewer electrons than required to achieve a stable electron configuration, typically resembling that of a noble gas. This often occurs in molecules with incomplete octets, leading to a tendency to accept electrons from other species, making them reactive and often acting as Lewis acids.
추천 영상:
가이드 코스
04:44
Electron Geometry
Lewis Acids and Bases
In the Lewis theory, acids are defined as electron pair acceptors, while bases are electron pair donors. Electron-deficient molecules often function as Lewis acids because they can accept electron pairs to complete their octet, facilitating various chemical reactions, including coordination and complex formation.
추천 영상:
가이드 코스
05:04Lewis Acids and Bases
Stability and Reactivity
The stability of a molecule is closely tied to its electron configuration. Electron-deficient molecules are generally less stable and more reactive due to their incomplete valence shells. This reactivity can lead to the formation of new bonds as these molecules seek to achieve a more stable electronic state through interactions with electron-rich species.
추천 영상:
가이드 코스
03:13Intepreting the Band of Stability