📚 Alkanes in A-Level Edexcel Chemistry: Key Exam Concepts | A-Level Edexcel 化学:烷烃 考点精讲
Alkanes form the foundation of organic chemistry in the Edexcel A-Level syllabus. A solid grasp of their structure, nomenclature, physical trends, combustion, and free-radical substitution mechanism is essential for high marks. This revision guide distils every key point, linking concepts to typical exam questions.
烷烃是 Edexcel A-Level 有机化学的基石。透彻掌握它们的结构、命名、物理性质规律、燃烧及自由基取代机理是取得高分的必要条件。本篇精讲提炼每一个考点,并将概念与典型考题紧密挂钩。
1. Introduction and General Formula | 烷烃通式与简介
Alkanes are saturated hydrocarbons containing only carbon–carbon single bonds. Their general formula is CₙH₂ₙ₊₂, where n is the number of carbon atoms. Each carbon atom is sp³ hybridised, giving a tetrahedral geometry with bond angles of approximately 109.5°. All bonds are sigma (σ) bonds, formed by end-on overlap of orbitals, which allows free rotation about the C–C axis.
烷烃是只含碳-碳单键的饱和烃。通式为 CₙH₂ₙ₊₂,其中 n 为碳原子数。每个碳原子采取 sp³ 杂化,呈四面体构型,键角约 109.5°。全部键均为 σ 键,由轨道端对端重叠形成,这使得 C–C 键可以自由旋转。
The high bond enthalpy of the C–C and C–H σ bonds makes alkanes relatively unreactive, except towards combustion and free-radical substitution. This low reactivity is a frequently examined concept.
C–C 和 C–H σ 键较高的键焓使得烷烃相对惰性,只对燃烧和自由基取代反应较为敏感。这种低反应性是常考的概念。
2. Nomenclature and Structural Isomerism | 命名与结构异构
IUPAC names for straight‑chain alkanes are based on the number of carbons: methane (1), ethane (2), propane (3), butane (4), pentane (5), hexane (6), heptane (7), octane (8), nonane (9), decane (10). Branched alkanes are named by identifying the longest continuous carbon chain, numbering to give the lowest locants to substituents, and listing alkyl groups alphabetically (e.g. 2,2‑dimethylbutane).
直链烷烃的 IUPAC 名称取决于碳原子数:甲烷(1)、乙烷(2)、丙烷(3)、丁烷(4)、戊烷(5)、己烷(6)、庚烷(7)、辛烷(8)、壬烷(9)、癸烷(10)。支链烷烃命名时,找出最长碳链,编号使取代基位次最小,并按字母顺序列出烷基(如 2,2‑二甲基丁烷)。
Structural isomerism starts at C₄H₁₀: butane and 2‑methylpropane (isobutane). As carbon number increases, the number of possible isomers rises rapidly. Pentane has three isomers, hexane has five. Examiners often ask students to draw and name all constitutional isomers for a given formula, stressing chain isomerism.
结构异构从 C₄H₁₀ 开始:丁烷和 2‑甲基丙烷(异丁烷)。随着碳数增加,可能的异构体数目急剧增多。戊烷有 3 种异构体,己烷有 5 种。考官常要求给出某分子式的全部构造异构体,并写出名称,侧重碳链异构。
3. Physical Properties and Trends | 物理性质及变化规律
Alkanes are non‑polar, so the only intermolecular forces are instantaneous dipole‑induced dipole (London dispersion) forces. Boiling point increases with chain length because more electrons create stronger temporary dipoles. For isomers, branching lowers the boiling point: a more branched molecule has a smaller surface area, so London forces are weaker. This is a classic exam explanation.
烷烃为非极性分子,分子间仅存在瞬时偶极‑诱导偶极力(伦敦色散力)。随碳链增长,电子数目增多,瞬时偶极增强,沸点升高。对于异构体,支链会使沸点降低:支链越多,分子表面积越小,伦敦力越弱。这是经典的考试解释。
All alkanes are insoluble in water, as they cannot form hydrogen bonds, and their density is less than that of water. The table below summarises boiling points of isomeric pentanes.
所有烷烃都不溶于水(无法形成氢键),且密度均小于水。下表归纳了戊烷异构体的沸点。
| Isomer (isomer) | Boiling point / °C (沸点/℃) |
|---|---|
| Pentane CH₃(CH₂)₃CH₃ | 36 |
| 2‑Methylbutane CH₃CH(CH₃)CH₂CH₃ | 28 |
| 2,2‑Dimethylpropane C(CH₃)₄ | 9.5 |
4. Combustion Reactions | 燃烧反应
Alkanes burn readily in excess oxygen to give carbon dioxide and water. The complete combustion of methane is:
烷烃在过量氧气中容易燃烧,生成二氧化碳和水。甲烷的完全燃烧为:
CH₄ + 2O₂ → CO₂ + 2H₂O
For any alkane CₙH₂ₙ₊₂, the general equation is CₙH₂ₙ₊₂ + (1.5n+0.5)O₂ → nCO₂ + (n+1)H₂O. Combustion is highly exothermic, making alkanes important fuels.
对于任意烷烃 CₙH₂ₙ₊₂,完全燃烧的通式为 CₙH₂ₙ₊₂ + (1.5n+0.5)O₂ → nCO₂ + (n+1)H₂O。反应大量放热,因此烷烃是重要的燃料。
In limited oxygen, incomplete combustion produces carbon monoxide (CO) and/or carbon (soot). CO is a toxic gas that binds to haemoglobin. Unburnt hydrocarbons also contribute to photochemical smog. Edexcel often asks for balanced equations of incomplete combustion and the associated hazards.
在氧气不足时,不完全燃烧生成一氧化碳(CO)和/或碳(炭黑)。CO 是有毒气体,能与血红蛋白结合。未燃烧的烃类还会加剧光化学烟雾。Edexcel 常要求书写不完全燃烧的配平方程式,并说明其危害。
5. Free Radical Substitution: An Overview | 自由基取代反应概述
When alkanes react with halogens (Cl₂, Br₂) in the presence of ultraviolet light, a hydrogen atom is replaced by a halogen atom. The overall reaction for methane and chlorine is:
烷烃与卤素(Cl₂、Br₂)在紫外光照射下反应,其中一个氢原子被卤原子取代。甲烷与氯气的总反应为:
CH₄ + Cl₂ → CH₃Cl + HCl
This is a free‑radical chain reaction, proceeding via a mechanism that involves three stages: initiation, propagation, and termination. The C–H bond breaks homolytically – each atom takes one electron, forming radicals.
该反应属于自由基链式反应,通过引发、传递和终止三个阶段进行。C–H 键发生均裂——每个原子各带走一个电子,形成自由基。
Key conditions: ultraviolet light (or strong heating) to provide the energy for homolytic fission of the Cl–Cl bond. In the absence of UV light, the reaction is very slow. This is a common question: ‘Why is UV light needed?’
关键条件:紫外光(或强加热)提供能量使 Cl–Cl 键均裂。无紫外光时反应极慢。常考问题:“为什么需要紫外光?”
6. Stepwise Mechanism of Free Radical Substitution | 自由基取代的分步机理
Initiation: The Cl–Cl bond breaks homolytically, producing two chlorine radicals. This step requires UV light.
引发: Cl–Cl 键均裂,生成两个氯自由基。该步骤需要紫外光。
Cl₂ → 2Cl·
Propagation: A chlorine radical abstracts a hydrogen atom from methane, forming HCl and a methyl radical (·CH₃). The methyl radical then attacks a Cl₂ molecule, producing chloromethane and regenerating a Cl· radical. These two steps repeat, sustaining the chain.
传递: 一个氯自由基夺取甲烷的一个氢原子,生成 HCl 和甲基自由基(·CH₃)。该甲基自由基随后攻击一个 Cl₂ 分子,生成氯甲烷并再生一个 Cl· 自由基。这两步循环重复,维持链反应。
Step 1: CH₄ + Cl· → ·CH₃ + HCl
第1步: CH₄ + Cl· → ·CH₃ + HCl
Step 2: ·CH₃ + Cl₂ → CH₃Cl + Cl·
第2步: ·CH₃ + Cl₂ → CH₃Cl + Cl·
Termination: Any two radicals can combine to form a stable molecule, removing radicals and stopping the chain. Examples:
终止: 任意两个自由基结合形成稳定分子,消耗自由基,使链终止。例如:
Cl· + Cl· → Cl₂
·CH₃ + ·CH₃ → C₂H₆
Cl· + ·CH₃ → CH₃Cl
Writing the full mechanism with curly arrows showing movement of single electrons is a must‑master skill. For Edexcel, always show homolytic fission with a fish‑hook arrow.
正确写出完整机理(包括用弯箭头表示单电子移动)是必须掌握的技能。对 Edexcel 而言,务必将均裂用半箭头(鱼钩箭头)表示。
7. Limitations of Free Radical Substitution | 自由基取代的局限性
Once chloromethane is formed, it can undergo further substitution with chlorine radicals, giving a mixture of CH₂Cl₂, CHCl₃, and CCl₄. Because the reaction is a random radical process, the product is always a mixture. Separation is difficult, so free‑radical substitution is not a good method for preparing a single pure halogenoalkane.
一旦生成氯甲烷,它可继续与氯自由基发生取代反应,得到 CH₂Cl₂、CHCl₃ 和 CCl₄ 的混合物。由于反应是随机的自由基过程,产物总是混合物。分离困难,因此自由基取代不适合制备单一纯卤代烷。
Exam questions often highlight this limitation and ask why a mixture is obtained, or why the method is unsuitable for synthesis. They may also ask for all possible organic products when ethane reacts with Cl₂.
试题常突出这一局限性,问为何得到混合物,或为何该方法不适用于合成。也可能要求写出乙烷与 Cl₂ 反应时所有可能的有机产物。
8. Cracking and Reforming | 裂解与重整
Thermal cracking takes place at high temperature (700–1200 K) and high pressure. It produces a high proportion of alkenes, which are valuable feedstocks for polymers. The process involves homolytic fission of C–C bonds, generating radicals that rearrange to form shorter‑chain alkanes and alkenes.
热裂解在高温(700–1200 K)和高压下进行,产生较高比例的烯烃,后者是聚合物的宝贵原料。过程中 C–C 键均裂生成自由基,自由基重排后得到短链烷烃和烯烃。
Catalytic cracking uses a zeolite catalyst at moderate temperatures (~720 K) and slight pressure. It yields branched alkanes, cycloalkanes, and aromatic compounds, suitable for motor fuels. The branched products have higher octane numbers and burn more smoothly in petrol engines.
催化裂解使用沸石催化剂,在中等温度(约 720 K)和轻微压力下进行,得到支链烷烃、环烷烃和芳香烃,适合用作车用燃料。支链产物辛烷值更高,在汽油机中燃烧更平稳。
Reforming converts straight‑chain alkanes into branched or cyclic alkanes using a platinum catalyst, again to improve octane rating. Both cracking and reforming are key industrial processes that feature in applied chemistry questions.
重整以铂为催化剂,将直链烷烃转化为支链或环状烷烃,同样是为了提高辛烷值。裂解与重整均是重要的工业过程,常出现在应用化学题型中。
9. Environmental Concerns and Catalytic Converters | 环境问题与催化转化器
Burning alkane fuels produces CO₂, a greenhouse gas, and often CO, unburnt hydrocarbons, and NOx (from N₂ + O₂ at high engine temperatures). NOx contributes to acid rain and photochemical smog. Catalytic converters in car exhausts use platinum, palladium, and rhodium to catalyse reactions that reduce these pollutants.
烷烃燃料燃烧产生温室气体 CO₂,且常伴有 CO、未燃烃和 NOx(由发动机高温下 N₂ + O₂ 生成)。NOx 导致酸雨和光化学烟雾。汽车尾气中的催化转化器利用铂、钯、铑催化反应,减少这些污染物。
Key catalytic converter reactions:
催化转化器的主要反应:
2CO + 2NO → 2CO₂ + N₂
2CO + O₂ → 2CO₂
CₙHₘ + (n+m/4)O₂ → nCO₂ + (m/2)H₂O
These catalytic processes require sufficient oxygen and are most efficient at high temperatures. Edexcel may ask for the role of the catalyst and why CO and NO are dangerous, linking back to haemoglobin binding and respiratory problems.
这些催化过程需要足够的氧气,且在高温下最有效。Edexcel 会问及催化剂的作用、CO 和 NO 为何危险,并能联系血红蛋白结合与呼吸问题。
10. Exam Tips and Key Points | 考试技巧与要点总结
Always write the free‑radical mechanism with clear single‑electron arrows. Label initiation, propagation, and termination. Show all radical intermediates and terminate with different radical combinations. Never forget to state ‘UV light’ or ‘△’ in the initiation step.
写自由基机理时,务必用清晰的单电子箭头。标明引发、传递和终止。写出所有自由基中间体,并以不同自由基结合结束。切勿忘记在引发步骤中注明“紫外光”或“加热”。
When explaining boiling point trends, link the number of electrons to the strength of London forces. For branched vs straight‑chain isomers, mention surface area and contact between molecules. Use examples like pentane isomers to back up your answer.
解释沸点规律时,要将电子数目与伦敦力的强弱联系起来。对比支链与直链异构体时,要提及分子表面积和接触程度。用戊烷异构体等实例支撑答案。
For incomplete combustion, balance the equation carefully; consider CO and C as possible products if O₂ is limited. For environmental questions, be prepared to write balanced equations for catalytic converters and name the pollutants.
处理不完全燃烧时,仔细配平方程式;若 O₂ 不足,需考虑生成 CO 和 C。在环境问题中,要能写出催化转化器的配平方程式并说出污染物名称。
Finally, practice drawing structural isomers and naming them confidently. A quick check: C₆H₁₄ has five chain isomers – can you name them all? Make sure you can, because this is a favourite exam task.
最后,多加练习画出结构异构体并自信地命名。快速自查:C₆H₁₄ 有五种碳链异构体——你能全部命名吗?确保能做到,因为这是颇受青睐的考试题型。
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