📚 IB Chemistry: Cambridge Core Principles | IB 化学：剑桥核心原理
The IB Chemistry course, built upon the Cambridge curriculum's rigorous foundation, aims to develop a deep understanding of chemical principles through inquiry and experimentation. This article distils the core principles that form the backbone of both Standard Level (SL) and Higher Level (HL) syllabi, providing a concise yet comprehensive bilingual revision guide for students seeking to master key topics such as atomic structure, bonding, energetics, kinetics, equilibrium, acids and bases, redox reactions, and organic chemistry. Each section presents essential concepts in paired English-Chinese paragraphs, aligning with the assessment objectives of knowledge, application, and analysis.
IB 化学课程以剑桥课程的严谨体系为基础，旨在通过探究和实验培养学生对化学原理的深刻理解。本文提炼了构成标准水平 (SL) 和高级水平 (HL) 大纲支柱的核心原理，为希望掌握关键主题——如原子结构、化学键、能量学、动力学、平衡、酸和碱、氧化还原反应以及有机化学——的学生提供一份简洁而全面的中英双语复习指南。每一部分都以英中对照段落呈现核心概念，紧密贴合知识、应用和分析的评估目标。
1. Stoichiometric Relationships | 化学计量关系
f substance that contains exactly 6.02 × 10²³ elementary entities (Avogadro constant). Using molar mass (g mol⁻¹) and the ideal gas equation PV = nRT, one can interconvert between mass, volume of gases, and number of particles.
化学计量学是对化学反应中反应物和产物的定量研究。摩尔是基本单位，定义为恰好包含 6.02×10²³ 个基本微粒（阿伏伽德罗常数）的物质的量。利用摩尔质量（g mol⁻¹）和理想气体方程 PV = nRT，可以在质量、气体体积和粒子数之间进行换算。
The empirical formula is the simplest whole-number ratio of atoms in a compound, while the molecular formula gives the actual number of each atom. Percentage yield and atom economy are key indicators of reaction efficiency: percentage yield compares actual to theoretical yield, and atom economy assesses the proportion of reactant atoms incorporated into the desired product.
实验式是化合物中原子的最简整数比，而分子式则给出了每种原子的实际数目。百分产率和原子经济性是衡量反应效率的关键指标：百分产率是实际产量与理论产量的比值，原子经济性则评估反应物原子并入目标产物的比例。
Limiting reactant calculations determine which reactant is completely consumed first, thereby controlling the maximum amount of product formed. Solution stoichiometry uses concentration (mol dm⁻³) and volume to relate moles of solute, crucial for titrations.
限量反应物计算可确定哪种反应物首先被完全消耗，从而控制产物的最大生成量。溶液计量学利用浓度（mol dm⁻³）和体积来关联溶质的摩尔数，这对于滴定实验至关重要。
2. Atomic Structure | 原子结构
Atoms consist of a dense, positively charged nucleus containing protons and neutrons, surrounded by a cloud of electrons in quantified energy levels. The atomic number (Z) defines the element, while the mass number (A) is the sum of protons and neutrons. Isotopes are atoms of the same element with different neutron numbers, exhibiting similar chemical properties but varying physical properties.
原子由一个致密带正电的、包含质子和中子的原子核以及环绕在量化能级上的电子云组成。原子序数 (Z) 定义了元素，而质量数 (A) 是质子数与中子数之和。同位素是同一元素中中子数不同的原子，它们化学性质相似但物理性质有别。
Electrons occupy sub-levels (s, p, d, f) within main energy levels. The electron configuration follows the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. For HL, the anomalies in transition metal configurations and the concept of orbital shapes (spherical s, dumbbell p) are explored. The successive ionization energies provide evidence for shell structure and electron shielding.
电子占据主能级内的亚层（s, p, d, f）。电子排布遵循构造原理、洪特规则和泡利不相容原理。对于 HL 内容，还需探讨过渡金属排布的异常及轨道形状（球形 s、哑铃型 p）。逐级电离能的数据为电子层结构和屏蔽效应提供了证据。
Emission spectra arise when excited electrons fall back to lower energy levels, emitting photons of specific wavelengths. The hydrogen emission spectrum converges at high energy, leading to the calculation of the ionization energy using the Rydberg formula.
激发态电子跃迁回较低能级时会发射特定波长的光子，形成发射光谱。氢原子发射光谱在高能端收敛，可利用里德伯公式计算电离能。
3. Periodicity | 元素周期律
The periodic table arranges elements by increasing atomic number, revealing recurring patterns in physical and chemical properties. Groups 1 (alkali metals) and 17 (halogens) show clear trends: reactivity increases down Group 1 but decreases down Group 17 due to changes in atomic radius and electron affinity. Oxides change from basic to acidic across a period.
元素周期表按原子序数递增排列，揭示了物理和化学性质的周期性规律。第1族（碱金属）和第17族（卤素）表现出清晰的递变趋势：由于原子半径和电子亲和能的变化，第1族反应性从上到下增强，而第17族则减弱。氧化物从左至右从碱性变为酸性。
Atomic radius decreases across a period due to increased nuclear charge pulling electrons closer, but increases down a group as extra electron shells are added. The first ionization energy generally increases across a period and decreases down a group, with minor dips between Groups 2 and 13, and 15 and 16, explained by orbital filling and electron-electron repulsion.
由于核电荷增加吸引电子更紧密，原子半径在同周期内从左到右减小，而从上到下因新增电子层而增大。第一电离能从左到右总体升高，从上到下降低；在第2和第13族之间、第15和第16族之间出现小幅下降，可用轨道填充和电子间排斥解释。
Melting points for Period 3 elements reflect structure: giant metallic (Na, Mg, Al) with rising trend, giant covalent (Si) very high, and simple molecular (P₄, S₈, Cl₂, Ar) with low melting points influenced by intermolecular forces.
第三周期元素的熔点反映了结构差异：巨型金属晶体（Na, Mg, Al）熔点递升，巨型共价晶体（Si）熔点极高，简单分子晶体（P₄、S₈、Cl₂、Ar）受分子间作用力影响熔点较低。
4. Chemical Bonding and Structure | 化学键与结构
Ionic bonding involves the electrostatic attraction between oppositely charged ions formed by electron transfer. It typically occurs between metals and non-metals with large electronegativity differences, yielding lattice structures with high melting points and brittleness. Formula units represent the simplest ion ratio.
离子键是由电子转移形成的带相反电荷的离子之间的静电吸引力。通常发生在电负性差大的金属与非金属之间，形成具有高熔点和脆性的晶格结构。化学式单元表示最简离子比。
Covalent bonding results from the sharing of electron pairs between atoms with small electronegativity differences. The VSEPR theory predicts molecular shapes based on electron-pair repulsion: linear (e.g., BeCl₂), bent (H₂O), trigonal planar (BF₃), tetrahedral (CH₄), and octahedral (SF₆). Bond polarity arises from unequal sharing, leading to dipole moments.
共价键由电负性差小的原子之间共享电子对形成。价层电子对互斥理论 (VSEPR) 基于电子对排斥预测分子形状：直线形（如 BeCl₂）、角形（H₂O）、平面三角形（BF₃）、四面体形（CH₄）和八面体形（SF₆）。键的极性源于共享不均，产生偶极矩。
Metallic bonding is described by a lattice of cations immersed in a sea of delocalized electrons, explaining conductivity, malleability, and high melting points. Giant covalent structures (diamond, graphite, SiO₂) display extreme hardness and high sublimation points. Intermolecular forces—London dispersion forces, dipole-dipole interactions, and hydrogen bonding—govern bulk properties of covalent molecules.
金属键被描述为沉浸在离域电子“海洋”中的阳离子晶格，这解释了导电性、延展性和高熔点。巨型共价结构（金刚石、石墨、SiO₂）表现出极高的硬度和升华点。分子间作用力——伦敦色散力、偶极-偶极相互作用和氢键——支配共价分子的宏观性质。
5. Energetics / Thermochemistry | 能量学/热化学
c reactions absorb energy (ΔH > 0). Standard enthalpy changes are measured under standard conditions (100 kPa, 298 K). Calorimetry using q = mcΔT allows experimental determination of enthalpy changes.
化学反应涉及能量变化，主要以热（焓，ΔH）的形式表现。放热反应释放能量（ΔH < 0），吸热反应吸收能量（ΔH > 0）。标准焓变在标准条件（100 kPa，298 K）下测量。使用 q = mcΔT 的量热法可以实验测定焓变。
Hess's law states that the total enthalpy change for a reaction is independent of the route taken. This allows the calculation of unknown enthalpy changes using formation enthalpies or combustion data. Bond enthalpies can be used to estimate ΔH, though the values are average and neglect molecular environment.
赫斯定律指出，一个反应的总焓变与途径无关。这允许利用生成焓或燃烧热数据计算未知的焓变。键焓可用于估算 ΔH，但键焓是平均值且忽略了分子环境的影响。
Standard enthalpy of formation (ΔH°f) of a compound is the enthalpy change when one mole of the compound is formed from its elements in their standard states. Born-Haber cycles relate lattice enthalpy, ionization energies, and electron affinities for ionic compounds, essential for understanding stability.
化合物的标准生成焓 (ΔH°f) 是指在标准状态下由元素生成一摩尔该化合物时的焓变。玻恩-哈伯循环将离子化合物的晶格焓、电离能和电子亲和能联系起来，这对于理解稳定性至关重要。
6. Chemical Kinetics | 化学动力学
Chemical kinetics studies the rate of reaction and the factors affecting it. Rate is defined as the change in concentration of a reactant or product per unit time. The collision theory states that for a reaction to occur, particles must collide with sufficient energy (activation energy, Eₐ) and correct orientation.
化学动力学研究反应速率及其影响因素。速率定义为反应物或产物浓度在单位时间内的变化。碰撞理论指出，反应发生需要粒子以足够的能量（活化能，Eₐ）和正确的取向发生碰撞。
Boltzmann distribution curve illustrates that raising temperature not only increases the average kinetic energy but also significantly enlarges the fraction of molecules with energy ≥ Eₐ.
影响速率的因素包括浓度（或气体压强）、温度、表面积和催化剂的存在。麦克斯韦-玻尔兹曼分布曲线表明，升高温度不仅增加平均动能，还显著增大了能量 ≥ Eₐ 的分子比例。
e rate equations (rate = k[A]ᵐ[B]ⁿ), determination of order from experimental data, and the Arrhenius equation linking rate constant k to temperature and Eₐ.
催化剂通过提供较低活化能的替代路径来提高速率，自身不被消耗。HL 专题包括速率方程（rate = k[A]ᵐ[B]ⁿ）、从实验数据确定反应级数，以及将速率常数 k 与温度和 Eₐ 联系起来的阿伦尼乌斯方程。
7. Chemical Equilibrium | 化学平衡
Many reactions are reversible; at equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant. The equilibrium constant (Kc) expresses the ratio of product to reactant concentrations raised to their stoichiometric coefficients.
许多反应是可逆的；达到平衡时，正逆反应速率相等，反应物和产物的浓度保持恒定。平衡常数 (Kc) 表示产物浓度与反应物浓度的比值，各浓度以化学计量系数为指数。
Le Chatelier' t the imposed change. For gaseous equilibria, the partial pressure constant Kp is used, and the relationship Kp = Kc(RT)^Δn links the two constants.
勒夏特列原理预测，当平衡体系受到浓度、温度或压强变化的影响时，会向削弱该变化的方向移动。对于气体平衡，采用分压常数 Kp，并通过 Kp = Kc(RT)^Δn 关联这两个常数。
The magnitude of K indicates the extent of reaction: K ≫ 1 favours products, K ≪ 1 favours reactants. For the Haber process (N₂ + 3H₂ ⇌ erature and high pressure optimise yield, but compromise must be made for kinetic reasons.
K 值的大小指示反应进行的程度：K ≫ 1 倾向于产物，K ≪ 1 倾向于反应物。对于哈伯法（N₂ + 3H₂ ⇌ 2NH₃，ΔH = -92 kJ mol⁻¹），低温和高压可提高产率，但出于动力学原因需做出权衡。
8. Acids and Bases | 酸和碱
Arrhenius acids produce H⁺ in water, and bases produce OH⁻. Bronsted-Lowry theory extends this: an acid is a proton donor, a base is a proton acceptor. Conjugate acid-base pairs differ by one proton. Strong acids (HCl, H₂SO₄, HNO₃) fully dissociate, while weak acids (CH₃COOH, H₂CO₃) partially dissociate.
根据阿伦尼乌斯理论，酸在水中产生 H⁺，碱产生 OH⁻。布朗斯特-劳里理论扩展了这一概念：酸是质子的给予体，碱是质子的接受体。共轭酸碱对之间相差一个质子。强酸（HCl、H₂SO₄、HNO₃）完全解离，弱酸（CH₃COOH、H₂CO₃）部分解离。
ion constant Kₐ = [H⁺][A⁻]/[HA] governs equilibrium. pKₐ = -log Kₐ; lower pKₐ signals stronger acid. Buffer solutions resist pH change and consist of a weak acid and its conjugate base.
pH 标度 pH = -log[H⁺] 量度酸碱度。对于强一元酸，[H⁺] 等于酸浓度。对于弱酸，酸解离常数 Kₐ = [H⁺][A⁻]/[HA] 决定平衡。pKₐ = -log Kₐ；pKₐ 越小酸性越强。缓冲溶液能抵抗 pH 变化，由弱酸及其共轭碱组成。
tinct colours; they change at a pH range around their pKₐ. The Henderson-Hasselbalch equation pH = pKₐ + log([A⁻]/[HA]) is used to design buffers.
滴定曲线描绘 pH 对加入滴定剂体积的关系，揭示等当点和缓冲区域。指示剂是具有不同颜色的弱酸，在接近其 pKₐ 的 pH 范围内变色。亨德森-哈塞尔巴尔赫方程 pH = pKₐ + log([A⁻]/[HA]) 用于设计缓冲溶液。
9. Redox Processes | 氧化还原过程
Oxidation is the loss of electrons, reduction is the gain of electrons (OIL RIG). Oxidation states are assigned to atoms using rules, helping to identify which species is oxidized and which is reduced. Redox reactions are balanced using half-equations, combining them to cancel electrons.
氧化是失去电子，还原是得到电子（OIL RIG）。利用规则为原子分配氧化数，有助于识别哪种物质被氧化、哪种被还原。氧化还原反应通过半反应式配平，组合时使电子抵消。
ctrode with higher reduction potential undergoes reduction (cathode), and the other oxidation (anode). The standard cell potential E°cell = E°cathode - E°anode, and ΔG° = -nFE°cell measures spontaneity.
电化学电池将化学能转化为电能。伏打电池由两个通过盐桥连接的半电池组成；具有更高还原电位的电极发生还原（阴极），另一个发生氧化（阳极）。标准电池电势 E°cell = E°cathode - E°anode，ΔG° = -nFE°cell 衡量反应的自发性。
Electrolysis is the non-spontaneous process driven by an external power source. Faraday' e produced. Products of aqueous electrolysis depend on the relative reduction potentials of ions and water.
电解是依赖外部电源驱动的非自发过程。法拉第定律将电量（Q = It）与产物的物质的量联系起来。水溶液电解的产物取决于离子与水的相对还原电位。
10. Organic Chemistry | 有机化学
ds. Functional groups dictate chemical behaviour: alkanes (C-C), alkenes (C=C), alkynes (C≡ es. Homologous series show a gradation in physical properties and common general formulas.
有机化学以碳化合物为中心。官能团决定化学行为：烷烃 (C-C)、烯烃 (C=C)、炔烃 (C≡C)、醇 (-OH)、卤代烷 (-X)、醛、酮、羧酸和胺。同系列在物理性质上呈现递变，并具有通式。
Alkanes undergo free-radical substitution (for example, chlorination of methane under UV light). Alkenes undergo electrophilic addition (e.g., bromination, hydration), following Markovnikov's rule where applicable. Alcohols can be oxidized to aldehydes, ketones, or carboxylic acids; dehydration yields alkenes.
烷烃发生自由基取代反应（如甲烷在紫外光下的氯化）。烯烃发生亲电加成反应（如溴化、水合），并在适用时遵循马氏规则。醇可氧化为醛、酮或羧酸；脱水反应生成烯烃。
Structural isomerism (chain, position, functional group) and stereoisomerism (geometric E/Z, optical) are central. Optical isomers contain a chiral carbon (four different groups) and rotate plane-polarized light. Condensation polymerisation forms polyesters and polyamides, with emphasis on linkages.
构造异构（碳链、位置、官能团）和立体异构（几何 E/Z、光学）是核心内容。光学异构体含有手性碳（四个不同基团）并能旋转平面偏振光。缩合聚合生成聚酯和聚酰胺，重点在于连接基团。
Published by TutorHao | Chemistry Revision Series | aleveler.com
更多咨询请联系16621398022（同微信）
或截图后用「扫一扫 → 相册」选择本图