📚 Year 10 Edexcel Chemistry: Syllabus Overview | Year 10 Edexcel 化学：课程大纲全面解析
Year 10 Edexcel Chemistry lays the foundation for understanding the material world at the atomic and molecular level. This stage covers core principles from states of matter and atomic structure to chemical bonding, quantitative chemistry, and the periodic table. As the first year of the two-year International GCSE (9-1) course, it builds essential practical skills and theoretical knowledge, preparing students for the deeper demands of Year 11 and final examinations. In this comprehensive guide, we walk through every major topic, highlight key equations, and explain the practical investigations that define the syllabus.
Year 10 Edexcel 化学课程为在原子和分子层面理解物质世界奠定基础。这一阶段涵盖从物质状态、原子结构到化学键、定量化学和元素周期表的核心原理。作为两年制 International GCSE (9-1) 课程的第一年，它培养了基本的实验技能与理论知识，为学生应对 Year 11 的更高要求及最终考试做好准备。在本全面解析中，我们将逐一梳理每个重要主题，突出关键方程式，并解释定义该教学大纲的实践探究活动。
1. States of Matter and Changes of State | 物质状态与状态变化
Matter exists in three main states: solid, liquid, and gas. The arrangement, movement, and energy of particles determine the properties of each state. Solids have a fixed shape and volume because particles are closely packed in a regular pattern and vibrate in fixed positions. Liquids have a fixed volume but take the shape of their container; particles are close together but can move past each other. Gases have no fixed shape or volume; particles are far apart, move rapidly, and fill the available space completely.
物质以三种主要状态存在：固态、液态和气态。粒子的排列方式、运动及能量决定了每种状态的性质。固体有固定的形状和体积，因为粒子紧密地呈规则排列，并在固定位置上振动。液体有固定的体积，但会呈现容器的形状；粒子彼此靠近但能相互滑动。气体没有固定的形状或体积；粒子相距甚远，快速运动，并完全充满可用空间。
The interconversions between states—melting, freezing, boiling, condensing, sublimation, and deposition—are physical changes. Heating or cooling changes the kinetic energy of particles, breaking or forming intermolecular forces without altering the chemical identity of the substance. The flat sections on a heating or cooling curve represent changes of state where temperature remains constant because energy is used to overcome attractive forces rather than to raise temperature.
状态之间的相互转化——熔化、凝固、沸腾、凝结、升华和凝华——都是物理变化。加热或冷却会改变粒子的动能，破坏或形成分子间作用力，而不会改变物质的化学身份。加热或冷却曲线上的平台段代表状态变化，此时温度保持恒定，因为能量被用于克服吸引作用力，而不是用来升高温度。
- Melting point: temperature at which solid becomes liquid. | 熔点：固体变为液体的温度。
- Boiling point: temperature at which liquid becomes gas throughout. | 沸点：整个液体变为气体的温度。
- Diffusion experiments with ammonia and hydrogen chloride illustrate particle motion in gases. | 氨气与氯化氢的扩散实验说明了气体中的粒子运动。
2. Elements, Compounds, and Mixtures | 元素、化合物与混合物
An element is a substance that cannot be broken down into simpler substances by chemical means. Elements are made up of only one type of atom and are listed on the Periodic Table. A compound contains two or more different elements chemically combined in fixed proportions; its properties are different from those of its constituent elements. A mixture consists of two or more elements or compounds that are not chemically combined; each component retains its own properties and can be separated by physical techniques such as filtration, distillation, or chromatography.
元素是无法通过化学方法分解为更简单物质的物质。元素只由一种原子组成，并被列入元素周期表。化合物包含两种或多种以固定比例化学结合的不同元素；化合物的性质与其组成元素的性质不同。混合物由两种或多种没有发生化学结合的元素或化合物组成；每种成分保持自身的性质，并可通过过滤、蒸馏或色谱等物理技术进行分离。
Simple diagrams help distinguish these categories: elements show identical atoms, compounds show molecules with two or more atom types bonded together, and mixtures show different atoms or molecules intermingled. The purity of a substance can be assessed by its boiling point; a pure substance boils at a sharp, specific temperature, while a mixture boils over a range of temperatures.
简单的示意图有助于区分这些类别：元素显示相同的原子，化合物显示由两种或多种原子键合而成的分子，混合物则显示不同的原子或分子混杂在一起。物质的纯度可以通过其沸点来评估；纯物质在一个清晰、特定的温度下沸腾，而混合物则在一个温度范围内沸腾。
Key separation methods covered in Year 10 include simple distillation (to separate a solvent from a solution), fractional distillation (to separate liquids with different boiling points), filtration (to separate an insoluble solid from a liquid), and paper chromatography (to separate dissolved substances based on their solubility).
Year 10 涉及的关键分离方法包括简单蒸馏（从溶液中分离溶剂）、分馏（分离沸点不同的液体）、过滤（从液体中分离不溶性固体）以及纸色谱（根据溶解性分离溶解的物质）。
3. Atomic Structure and the Periodic Table | 原子结构与元素周期表
Atoms consist of a small, dense nucleus containing protons and neutrons, surrounded by electrons in energy levels (shells). The relative mass of a proton is 1, a neutron is 1, and an electron is 1/1836. The relative charge of a proton is +1, neutron is 0, and electron is -1. Atomic number (Z) is the number of protons in the nucleus and defines the element. Mass number (A) is the total number of protons and neutrons. In a neutral atom, the number of electrons equals the number of protons.
原子由一个微小而致密的原子核（含质子和中子）以及位于能级（电子层）中的电子组成。质子的相对质量为 1，中子为 1，电子为 1/1836。质子的相对电荷为 +1，中子为 0，电子为 -1。原子序数（Z）是原子核中的质子数，它定义了元素。质量数（A）是质子与中子的总数。在中性原子中，电子数等于质子数。
Electrons occupy specific energy levels (shells) around the nucleus. The first shell holds up to 2 electrons, and the second and third shells each hold up to 8 electrons. The electronic configuration determines an element's chemical properties and its position in the Periodic Table. For example, sodium (atomic number 11) has the configuration 2,8,1.
电子占据原子核周围特定的能级（电子层）。第一层最多容纳 2 个电子，第二层和第三层各最多容纳 8 个电子。电子排布决定了一种元素的化学性质及其在元素周期表中的位置。例如，钠（原子序数 11）的电子排布为 2、8、1。
Isotopes are atoms of the same element with the same atomic number but different mass numbers due to differing numbers of neutrons. They have identical chemical properties because electron configurations are the same. The relative atomic mass (Aᵣ) of an element is the weighted average mass of its isotopes relative to 1/12th the mass of a carbon-12 atom.
同位素是同一元素中原子序数相同但中子数不同因而质量数不同的原子。它们具有相同的化学性质，因为电子排布相同。元素的相对原子质量（Aᵣ）是其同位素相对于碳-12 原子质量 1/12 的加权平均质量。
The Periodic Table arranges elements in order of increasing atomic number. Groups (vertical columns) contain elements with the same number of electrons in the outer shell, leading to similar chemical properties. Periods (horizontal rows) correspond to the number of occupied electron shells. Students must be able to deduce the electronic configuration of the first 20 elements and identify the group and period of an element from its configuration.
元素周期表按照原子序数递增的顺序排列元素。族（纵列）包含最外层电子数相同的元素，因此化学性质相似。周期（横行）对应已占据的电子层数。学生必须能够推断前 20 号元素的电子排布，并根据排布确定元素所在的族和周期。
4. Ionic Bonding | 离子键
Ionic bonding occurs between metals and non-metals. Metal atoms lose electrons to form positively charged ions (cations), while non-metal atoms gain electrons to form negatively charged ions (anions). The strong electrostatic forces of attraction between oppositely charged ions hold the giant ionic lattice together. This transfer of electrons allows both types of atoms to achieve full outer electron shells, typically the stable electronic structure of a noble gas.
离子键发生在金属与非金属之间。金属原子失去电子，形成带正电的离子（阳离子）；而非金属原子获得电子，形成带负电的离子（阴离子）。带相反电荷的离子之间强大的静电吸引力将巨型离子晶格结合在一起。这种电子转移使两种原子都能达到满的最外层电子结构，通常就是惰性气体的稳定电子结构。
The formula of an ionic compound shows the simplest ratio of ions that balances the total positive and negative charges. For example, in sodium chloride (NaCl), each Na⁺ ion pairs with one Cl⁻ ion. In magnesium oxide (MgO), Mg²⁺ balances O²⁻. For magnesium chloride (MgCl₂), one Mg²⁺ ion requires two Cl⁻ ions. Dot-and-cross diagrams are used to illustrate the transfer of electrons from metal to non-metal.
离子化合物的化学式表示了能平衡总正负电荷的离子最简整数比。例如，在氯化钠 (NaCl) 中，每个 Na⁺ 离子与一个 Cl⁻ 离子配对。在氧化镁 (MgO) 中，Mg²⁺ 与 O²⁻ 平衡。对于氯化镁 (MgCl₂)，一个 Mg²⁺ 离子需要两个 Cl⁻ 离子。用点叉图来表示电子从金属到非金属的转移过程。
Ionic compounds have high melting and boiling points because a large amount of energy is needed to overcome the strong electrostatic forces throughout the giant lattice. They do not conduct electricity when solid because the ions are fixed in position. However, when molten or dissolved in water, the ions become free to move and can carry charge, so the compound conducts electricity.
离子化合物具有较高的熔点和沸点，因为需要大量的能量来克服遍布整个巨型晶格的强静电吸引力。它们在固态时不导电，因为离子被固定在位置上。然而，当熔融或溶于水时，离子可以自由移动并携带电荷，因此该化合物能够导电。
5. Covalent Bonding and Simple Molecular Substances | 共价键与简单分子物质
e nuclei of the two atoms. By sharing electrons, atoms can achieve full outer shells. Covalent bonds can be single, double, or triple bonds, as seen in H₂ (H-H), O₂ (O=O), and N₂ (N≡ s diagrams and displayed formulae are essential tools for representing covalent compounds.
共价键发生在非金属原子之间。共价键是共用电子对与两个原子的原子核之间的强静电吸引力。通过共享电子，原子可以获得满的最外层。共价键可以是单键、双键或三键，例如 H₂ (H-H)、O₂ (O=O) 和 N₂ (N≡N)。点叉图和结构式是表示共价化合物的重要工具。
Simple molecular substances consist of small molecules held together by weak intermolecular forces. Examples include water (H₂O), carbon dioxide (CO₂), methane (CH₄), and chlorine (Cl₂). Because the intermolecular forces are weak, simple molecular substances have low melting and boiling points. They do not conduct electricity because there are no free ions or electrons; the molecules are neutral.
简单分子物质由通过弱分子间作用力结合在一起的小分子组成。例如水 (H₂O)、二氧化碳 (CO₂)、甲烷 (CH₄) 和氯气 (Cl₂)。由于分子间作用力很弱，简单分子物质的熔点和沸点较低。它们不导电，因为没有自由移动的离子或电子；分子是电中性的。
Students must be able to predict the type of bonding in a substance based on the elements present and explain physical properties in terms of structure and bonding. The syllabus also expects familiarity with giant covalent structures (introduced in Year 10 and expanded in Year 11), such as diamond, graphite, and silicon dioxide, which have high melting points due to strong covalent bonds throughout the structure.
学生必须能够根据所含元素预测物质中的键合类型，并从结构和键合的角度解释物理性质。教学大纲还要求学生了解巨型共价结构（在 Year 10 引入并在 Year 11 扩展），如金刚石、石墨和二氧化硅，它们由于整个结构中存在强共价键而具有很高的熔点。
6. Metallic Bonding | 金属键
Metallic bonding occurs in metals and alloys. It is described as the electrostatic attraction between a lattice of positive metal ions and a ‘sea’ of delocalised electrons. These delocalised electrons are free to move throughout the metal structure. This model explains why metals are good conductors of heat and electricity, are malleable and ductile, and have high melting points (though some, like mercury, are liquid at room temperature).
金属键存在于金属和合金中。它被描述为金属阳离子的晶格与“海”离域电子之间的静电吸引力。这些离域电子可以在整个金属结构中自由移动。这个模型解释了为什么金属是热和电的良导体，具有延展性和可锻性，并且通常具有高熔点（尽管有些金属，如汞，在室温下为液态）。
The strength of metallic bonding depends on the charge of the metal ion and the number of delocalised electrons per atom. Magnesium (Mg²⁺) forms stronger metallic bonds than sodium (Na⁺) because it has a higher charge and contributes more delocalised electrons. Alloys are mixtures of metals (or metals with non-metals) designed to disrupt the regular lattice, preventing layers from sliding easily and thus making the material harder and stronger.
金属键的强度取决于金属离子的电荷以及每个原子提供的离域电子数。镁 (Mg²⁺) 形成的金属键比钠 (Na⁺) 强，因为它的电荷更高且贡献了更多的离域电子。合金是金属（或金属与非金属）的混合物，旨在扰乱规则的晶格，阻止原子层轻易滑动，从而使材料更硬更强。
7. Chemical Formulae, Equations, and Calculations | 化学式、方程式与计算
nts and products, with the same number of each type of atom on both sides. State symbols (s), (l), (g), and (aq) indicate solid, liquid, gas, and aqueous solution respectively. For example: 2Mg(s) + O₂(g) → 2MgO(s).
定量化学从书写配平的化学方程式开始。一个配平的方程式显示了反应物和生成物正确的化学计量比，两侧每种原子的数量相等。状态符号 (s)、(l)、(g) 和 (aq) 分别表示固态、液态、气态和水溶液。例如：2Mg(s) + O₂(g) → 2MgO(s)。
e sum of the relative atomic masses of the atoms in its formula. The mole concept is central: one mole of any substance contains 6.02 × 10²³ particles (Avogadro's constant) and has a mass in grams equal to its relative formula mass.
Year 10 引入的关键计算包括相对式量 (Mᵣ)、摩尔和浓度。化合物的相对式量是其化学式中各原子相对原子质量的总和。摩尔概念是核心：1 摩尔任何物质含有 6.02 × 10²³ 个粒子（阿伏伽德罗常数），并且其以克为单位的质量等于它的相对式量。
The mole triangle links mass, moles, and Mᵣ:
Number of moles = Mass (g) ÷ Mᵣ
This equation is used to convert between mass and moles. Concentration is expressed in g/dm³ or mol/dm³:
Concentration (g/dm³) = Mass of solute (g) ÷ Volume of solution (dm³)
Concentration (mol/dm³) = Number of moles ÷ Volume (dm³)
Students must be able to calculate reacting masses using balanced equations and mole ratios, and determine the limiting reactant in a reaction.
摩尔三角将质量、摩尔和 Mᵣ 联系起来：
摩尔数 = 质量 (g) ÷ Mᵣ
该等式用于在质量和摩尔之间进行转换。浓度以 g/dm³ 或 mol/dm³ 表示：
浓度 (g/dm³) = 溶质质量 (g) ÷ 溶液体积 (dm³)
浓度 (mol/dm³) = 摩尔数 ÷ 体积 (dm³)
学生必须能够运用配平的方程式和摩尔比计算反应质量，并确定反应中的限量反应物。
8. Group 1 and Group 7 Elements | 第 1 族与第 7 族元素
Group 1 elements (alkali metals): lithium, sodium, potassium, rubidium, caesium. They have one electron in their outer shell, which they lose readily to form +1 ions. Reactivity increases down the group because the outer electron is further from the nucleus and more shielded, so it is more easily lost. They react vigorously with water to produce metal hydroxides (alkaline solutions) and hydrogen gas. The general equation is:
2M(s) + 2H₂O(l) → 2MOH(aq) + H₂(g)
Observations include fizzing, moving on the water surface, and for potassium, a lilac flame.
第 1 族元素（碱金属）：锂、钠、钾、铷、铯。它们的最外层只有一个电子，容易失去形成 +1 价离子。反应性沿族向下增强，因为最外层电子离原子核更远，且屏蔽效应更强，因此更容易失去。它们与水剧烈反应，生成金属氢氧化物（碱性溶液）和氢气。通用方程式为：
2M(s) + 2H₂O(l) → 2MOH(aq) + H₂(g)
观察到的现象包括嘶嘶声、在水面上四处游动，钾还会产生淡紫色火焰。
ons. Reactivity decreases down the group because the outer shell is further from the nucleus, making it harder to attract an extra electron. Halogens are diatomic molecules (F₂, Cl₂, Br₂, I₂). A more reactive halogen can displace a less reactive halogen from an aqueous solution of its halide salt. For example: Cl₂(aq) + 2NaBr(aq) → 2NaCl(aq) + Br₂(aq).
第 7 族元素（卤素）：氟、氯、溴、碘。它们的最外层有 7 个电子，获得一个电子形成 -1 价离子。反应性沿族向下减弱，因为最外层离原子核更远，使吸引额外电子变得更困难。卤素是双原子分子 (F₂、Cl₂、Br₂、I₂)。活泼性更强的卤素可以将活泼性较弱的卤素从其卤化物盐的水溶液中置换出来。例如：Cl₂(aq) + 2NaBr(aq) → 2NaCl(aq) + Br₂(aq)。
Physical trends: as you go down the group, melting and boiling points increase due to stronger intermolecular forces. Colour intensifies from pale yellow (fluorine) through green-yellow (chlorine) to red-brown (bromine) and purple-black (iodine). The state changes from gas to liquid to solid.
物理趋势：沿族向下，熔点和沸点由于分子间作用力增强而升高。颜色从淡黄（氟）经过黄绿（氯）到红褐（溴）和紫黑（碘）加深。状态由气态变为液态再到固态。
9. Acids, Bases, and Salts | 酸、碱与盐
and nitric acid (HNO₃). A base is a substance that neutralises acids; soluble bases are called alkalis and release hydroxide ions (OH⁻) in water. The pH scale (0-14) measures acidity or alkalinity: pH < 7 is acidic, pH = 7 is neutral, pH > 7 is alkaline. Universal indicator and pH meters are used to determine pH.
酸是在水溶液中释放氢离子 (H⁺) 的物质。常见的酸包括盐酸 (HCl)、硫酸 (H₂SO₄) 和硝酸 (HNO₃)。碱是能中和酸的物质；可溶的碱被称为碱类，在水中释放氢氧根离子 (OH⁻)。pH 标度 (0-14) 用于衡量酸碱性：pH < 7 呈酸性，pH = 7 呈中性，pH > 7 呈碱性。通用指示剂和 pH 计用于测定 pH 值。
xide or metal hydroxide reacts with an acid, a salt and water are formed. When a metal carbonate reacts with an acid, a salt, water, and carbon dioxide are formed. The type of salt produced depends on the acid used: hydrochloric acid gives chlorides, sulfuric acid gives sulfates, nitric acid gives nitrates.
中和反应：酸 + 碱 → 盐 + 水。用离子来解释就是：H⁺ + OH⁻ → H₂O。当金属氧化物或金属氢氧化物与酸反应时，生成盐和水。当金属碳酸盐与酸反应时，生成盐、水和二氧化碳。产生的盐的类型取决于所用的酸：盐酸生成氯化物，硫酸生成硫酸盐，硝酸生成硝酸盐。
Method for preparing a pure, dry sample of a soluble salt involves reacting an acid with an insoluble base (e.g., copper oxide) or a suitable carbonate, filtering off the excess solid, and gently heating the filtrate to evaporate water until crystallisation point. Crystals then form upon cooling.
制备纯净干燥的可溶性盐样品的方法包括：使酸与不溶性碱（如氧化铜）或合适的碳酸盐反应，滤去过量的固体，然后缓慢加热滤液蒸发水分至结晶点。冷却后晶体析出。
10. Electrolysis | 电解
Electrolysis is the decomposition of an ionic compound into its elements using direct current. It requires a molten or dissolved ionic compound (electrolyte), two electrodes connected to a power supply, and a complete circuit. The positive electrode is the anode, attracting anions; the negative electrode is the cathode, attracting cations. During electrolysis, cations are reduced (gain electrons) at the cathode, and anions are oxidised (lose electrons) at the anode.
电解是利用直流电将离子化合物分解为其组成元素的过程。它需要有熔融或溶解的离子化合物（电解质）、与电源连接的两个电极，以及一个完整的电路。正极是阳极，吸引阴离子；负极是阴极，吸引阳离子。在电解过程中，阳离子在阴极被还原（获得电子），阴离子在阳极被氧化（失去电子）。
In the electrolysis of molten lead(II) bromide (PbBr₂), lead metal forms at the cathode, and bromine gas forms at the anode. The half-equations are:
Cathode: Pb²⁺ + 2e⁻ → Pb
Anode: 2Br⁻ → Br₂ + 2e⁻
In aqueous solutions, the presence of water complicates the products. At the cathode, the less reactive element is discharged (either the metal ion or hydrogen from water). At the anode, a halide ion (if present) is discharged; otherwise, oxygen from water is discharged.
在电解熔融溴化铅 (PbBr₂) 时，铅金属在阴极生成，溴气在阳极生成。其半方程式为：
阴极：Pb²⁺ + 2e⁻ → Pb
阳极：2Br⁻ → Br₂ + 2e⁻
在水溶液中，水的存在使产物变得复杂。在阴极，较不活泼的元素被析出（可以是金属离子或来自水的氢气）。在阳极，如果存在卤素离子，则卤素离子被析出；否则，来自水的氧气被析出。
Electrolysis has important industrial applications, including the extraction of reactive metals like aluminium from their ores, and the purification of copper. In Year 10, students often investigate the electrolysis of copper(II) sulfate solution with inert graphite electrodes, observing a pink-brown coating of copper on the cathode and bubbles of oxygen at the anode.
电解具有重要的工业应用，包括从矿石中提取铝等活泼金属，以及精炼铜。在 Year 10，学生经常会研究用惰性石墨电极电解硫酸铜溶液，观察阴极上红棕色的铜镀层以及阳极上的氧气气泡。
11. Energetics – Exothermic and Endothermic Reactions | 能量学 – 放热反应与吸热反应
Chemical reactions involve energy changes. Exothermic reactions transfer energy to the surroundings, usually causing a temperature rise. Examples include combustion, neutralisation, and respiration. Endothermic reactions absorb energy from the surroundings, causing a temperature decrease. Examples include thermal decomposition of carbonates and photosynthesis.
化学反应涉及能量变化。放热反应将能量传递给周围环境，通常导致温度升高。例子包括燃烧、中和反应和呼吸作用。吸热反应从周围环境吸收能量，导致温度降低。例子包括碳酸盐的热分解和光合作用。
On an energy level diagram, exothermic reactions show products at a lower energy level than reactants, with the difference given as ΔH negative. Endothermic reactions show products higher than reactants, with ΔH positive. The activation energy (Eₐ) is the minimum energy required for a reaction to occur, shown as the peak in the diagram. Simple calorimetry experiments allow students to measure temperature changes when a solid dissolves or during a neutralisation reaction, using a polystyrene cup to reduce heat loss.
在能级图中，放热反应显示生成物的能量水平低于反应物，其差值表示为 ΔH 负值。吸热反应显示生成物高于反应物，ΔH 为正值。活化能 (Eₐ) 是反应发生所需的最低能量，在图中表现为峰值。简单的量热实验允许学生测量固体溶解或中和反应过程中的温度变化，通常使用聚苯乙烯杯以减少热量散失。
12. Rates of Reaction (Introduction) | 反应速率（引言）
The rate of a chemical reaction is a measure of how quickly reactants are converted into products. It can be monitored by measuring the volume of gas evolved, the change in mass (if gas escapes to the atmosphere), the formation of a precipitate (often by observing a cross through a solution until it disappears), or colour change. The rate at any point is the gradient of a tangent to the curve on a concentration–time or volume–time graph.
化学反应速率是衡量反应物转化为生成物快慢的量度。可以通过测量产生气体的体积、质量的变化（如果气体逸散到空气中）、沉淀的形成（通常通过观察溶液下的十字标记直到消失）或颜色变化来监测。任意一点的速率是浓度-时间或体积-时间曲线图上切线的斜率。
Factors affecting the rate of reaction include temperature, concentration (of solutions), surface area (of solids), pressure (of gases), and the presence of a catalyst. Increasing temperature increases the kinetic energy of particles, leading to more frequent collisions and a greater proportion of collisions with energy greater than the activation energy. Increasing concentration, pressure, or surface area increases the frequency of collisions. Catalysts provide an alternative reaction pathway with a lower activation energy, speeding up the reaction without being used up.
影响反应速率的因素包括温度、浓度（对溶液）、表面积（对固体）、压强（对气体）以及是否存在催化剂。升高温度会增加粒子的动能，导致碰撞更频繁，且更大比例的碰撞其能量超过活化能。增加浓度、压强或表面积会增加碰撞的频率。催化剂提供了另一条活化能较低的反应途径，从而加快反应速率，而自身不被消耗。
Collision theory is fundamental: for a reaction to occur, particles must collide with sufficient energy (at least the activation energy) and with the correct orientation. Year 10 practicals often include measuring gas volume from the reaction of marble chips (calcium carbonate) with hydrochloric acid, varying the concentration of the acid or the size of the marble chips to explore the effect on rate.
碰撞理论是基础：要使反应发生，粒子必须以足够的能量（至少为活化能）且以正确的取向发生碰撞。Year 10 的实践通常包括测量大理石碎片（碳酸钙）与盐酸反应产生的气体体积，改变酸的浓度或大理石碎片的大小，以探究对反应速率的影响。
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