📚 IB Chemistry for the IB Diploma: Core Topics and Exam Strategy | IB 化学文凭课程：核心主题与考试策略
The IB Diploma Programme chemistry course challenges students to combine conceptual understanding, practical investigation, and critical thinking. This article reviews the core topics, common pitfalls, and exam techniques that help you work toward a level 7.
IB 文凭课程化学要求学生将概念理解、实验探究和批判性思维结合起来。本文梳理核心主题、常见易错点及考试技巧，帮助你向 7 分目标迈进。
1. The IB Chemistry Syllabus at a Glance | IB 化学课程大纲一览
The syllabus is organised into core topics, additional higher level (AHL) material, and options. Standard level students cover 11 core topics, while higher level students also study 5 AHL topics in greater depth. Both levels complete a practical scheme of work and an individual investigation.
大纲分为核心主题、高级（AHL）内容和选修主题。标准水平学生覆盖 11 个核心主题，而高级水平学生还需深入学习 5 个 AHL 主题。两个水平都要求完成实验方案和一项个人探究。
Topics range from stoichiometry and atomic structure to energetics, equilibrium, redox and organic chemistry. The internal assessment contributes 20% of the final grade, so practical skills and data analysis are just as important as written papers.
主题涵盖化学计量、原子结构、能量学、平衡、氧化还原和有机化学等。内部评估占最终成绩的 20%，因此实验技能与数据分析与笔试同样重要。
2. Stoichiometric Relationships | 化学计量关系
Stoichiometry links the mole concept to balanced equations. One mole contains exactly 6.022 × 10²³ particles. Use molar mass to convert between mass and amount, and molar volume at STP to convert between gas volume and amount.
化学计量将摩尔概念与配平方程式联系起来。1 摩尔精确含有 6.022 × 10²³ 个粒子。利用摩尔质量在质量与物质的量之间转换，利用标准状况下的摩尔体积在气体体积与物质的量之间转换。
n = m / M
The limiting reagent determines the theoretical yield. Percentage yield compares the actual mass obtained with the theoretical mass. Always check that your equation is balanced and that units cancel correctly.
限制试剂决定理论产量。产率百分数将实际得到的质量与理论质量进行比较。务必检查方程式是否配平，以及单位是否正确约去。
3. Atomic Structure and Periodicity | 原子结构与周期性
Atoms consist of protons, neutrons and electrons. The number of protons defines the element, while isotopes differ in neutron number. Electron configuration follows the Aufbau principle, Hund’s rule and the Pauli exclusion principle.
原子由质子、中子和电子组成。质子数决定元素种类，同位素则因中子数不同而不同。电子排布遵循构造原理、洪特规则和泡利不相容原理。
Periodic trends such as atomic radius, ionisation energy and electronegativity arise from nuclear charge and shielding. Across a period, atomic radius generally decreases; down a group, it increases.
原子半径、电离能和电负性等周期趋势来源于核电荷与屏蔽效应。同一周期从左到右原子半径通常减小；同一族从上到下原子半径增大。
4. Chemical Bonding and Structure | 化学键与结构
Ionic, covalent and metallic bonding can be explained by electrostatic attractions and the sharing or delocalisation of electrons. Lewis structures, VSEPR theory and hybridisation help predict molecular shape and polarity.
离子键、共价键和金属键可以通过静电吸引以及电子的共用或离域来解释。路易斯结构、VSEPR 理论和杂化有助于预测分子形状与极性。
Intermolecular forces, including London dispersion forces, dipole-dipole interactions and hydrogen bonding, affect boiling points and solubility. Bond polarity alone does not always make a molecule polar; geometry matters.
分子间作用力，包括伦敦色散力、偶极-偶极相互作用和氢键，影响沸点和溶解度。仅键有极性并不一定使分子有极性；几何构型也很关键。
5. Energetics and Thermochemistry | 能量学与热化学
Enthalpy change (ΔH) measures heat transferred at constant pressure. Exothermic reactions release energy (ΔH < 0), while endothermic reactions absorb energy (ΔH > 0). Hess’s law allows enthalpy changes to be combined.
焓变（ΔH）衡量恒压条件下传递的热量。放热反应释放能量（ΔH < 0），吸热反应吸收能量（ΔH > 0）。盖斯定律允许对不同焓变进行加和。
q = mcΔT
Standard enthalpy changes of formation and combustion are common calculations. Bond enthalpies can estimate reaction enthalpy, but average bond enthalpies are less accurate for molecules with resonance or strong intermolecular forces.
标准生成焓和标准燃烧焓是常见计算。键焓可以估算反应焓，但对于存在共振或较强分子间作用力的分子，平均键焓的准确性较低。
6. Chemical Kinetics | 化学动力学
Rate of reaction depends on concentration, temperature, surface area and catalysts. The rate equation, rate = k[A]ᵐ[B]ⁿ, is determined experimentally, not from the stoichiometric coefficients.
反应速率取决于浓度、温度、表面积和催化剂。速率方程 rate = k[A]ᵐ[B]ⁿ 由实验确定，而不是来自化学计量数。
The rate constant k varies with temperature according to the Arrhenius equation. Activation energy is the minimum energy required for a collision to lead to reaction. Maxwell-Boltzmann distributions show why higher temperature increases rate.
速率常数 k 随温度变化，遵循阿伦尼乌斯方程。活化能是碰撞能引发反应所需的最低能量。麦克斯韦-玻尔兹曼分布说明为什么升高温度会加快反应速率。
7. Chemical Equilibrium | 化学平衡
At equilibrium, the forward and reverse rates are equal, and concentrations remain constant. The equilibrium constant Kc has a fixed value at a given temperature. If Kc is large, the equilibrium lies to the right.
平衡时，正逆反应速率相等，各物质浓度保持恒定。在给定温度下，平衡常数 Kc 有固定值。如果 Kc 很大，平衡位置偏向右侧。
Le Chatelier’s principle predicts the response to changes in concentration, pressure and temperature. Only temperature changes the value of Kc; catalysts speed up both directions equally.
勒夏特列原理可预测浓度、压强和温度变化时平衡的移动方向。只有温度会改变 Kc 的数值；催化剂同等程度地加快正逆反应。
8. Acids and Bases | 酸与碱
Brønsted-Lowry acids donate protons and bases accept protons. pH is defined as −log₁₀[H⁺]. Strong acids and bases dissociate fully, while weak ones establish an equilibrium described by Ka and Kb.
布朗斯特-劳里酸是质子给体，碱是质子受体。pH 定义为 −log₁₀[H⁺]。强酸和强碱完全电离，而弱酸和弱碱建立由 Ka 和 Kb 描述的平衡。
Buffer solutions resist pH change and consist of a weak acid and its conjugate base. Tit
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