IGCSE-G1chemistry 提纲

G1化学提纲思维导图，中英结合，梳理了相关化学单元的重要知识点，结构清晰，层次分明，有助于学习者进行知识的整合与复习。

chemistry unit1-6/11-15

• Unit 11Acids and bases
  • An acid is a proton donor . (从反应物到产物失去一个 H+) A base is a proton acceptor. (从反应物到产物得到一个 H+)
  • 1.The ions produced by acid and base
    • Acid produce hydrogen ions, H+, when dissolved in water 例 HCl, H2SO4, HNO3, H3PO4
    • Base: a compound that can react with an acid to form a salt. Bases can be metal oxides, hydroxides or carbonates and ammonia. 例CaO, Cu(OH)2, Na2CO3, NH3
    • Alkali is a base that is soluble in water. Alkali produce hydroxide ions, OH-, when dissolved in water 例 NaOH ，Ca(OH)2,NH3·H2O
  • 2. The pH of acid and base
    • The lower the pH, the more acidic the solution is. The higher the pH, the more alkaline the solution is.
  • Properties of acids
    • Turn blue litmus red. Turn methyl orange red (pH≤3.1). React with metals to produce hydrogen gas and the salt of the metal. -Mg(s) + H2SO4(aq) → MgSO4(aq) + H2(g) React with metal oxides to form a salt and water. -CuO(s) + 2HCl(aq) → CuCl2(aq) + H2O(l) React with metal hydroxides or aqueous ammonia to form a salt (and water). -HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)H2SO4(aq) + 2NH3(aq) → (NH4)2SO4(aq) React with carbonate/hydrogencarbonate to form a salt, water and carbon dioxide. -2HCl(aq) + Na2CO3(aq) → 2NaCl (aq) + H2O(l) + CO2(g)HCl(aq) + NaHCO3(aq) → 2NaCl (aq) + H2O(l) + CO2(g)
  • Properties of bases
    • Turn red litmus blue. Turn methyl orange yellow. Turn thylmolphthalein blue 1.React with acids (neutralization reaction). 2.React with ammonium salt to form a metal salt, ammonia and water. 3.(NH4)2SO4(aq) + 2KOH →K2SO4(aq) + 2NH3(g) + 2H2O (l) 4.Control the acidity of soil
  • Neutralisation reaction 中和反应 Neutralisation reaction: The reaction of an acid with a base to form a salt and water
  • Strong and weake acid/base
    • Strong acids/bases are completely ionized. Weak acids/bases are partially ionized.
    • Strong acid has a lower pH, greater electrical conductivity, faster rate of reaction (with metal carbonate/ Ca/ Zn/Mg) than weak acid. Strong base has a larger pH, greater electrical conductivity, faster rate of reaction (with acid) than weak base. pH : Strong acid: 1-3 weak acid: 4-7 strong base : 11-14 weak base: 8-10
  • types of oxide
• Unit 12-Making salts
  • Definite of Salt
    • A salt is produced when an acid reacts with a base. It is obtained when the hydrogen ions of acid are replaced with metal ions.
  • The solubility rules
  • test for gases, cations, anions
  • three methods of making salts
    • filtration: making soluble salts from insoluble reactant (从不溶的反应物中制可溶盐: 加过量不溶的反应物，过滤，结晶)
    • titration 滴定: making soluble salts from soluble reactants (need to se the indicator )从可溶的反应物中制可溶盐，用滴定
    • precipitation 沉淀法: making insoluble salts from soluble reactant 制不溶盐用沉淀法
• Unit 13 The Periodic Table
  • 元素周期表Periodic Table
    • Elements in the periodic table are arranged in order of their proton number. Group number = number of outer shell electrons; period number = number of electron shell Elements in the same group have similar chemical properties, because they have same number of outer shell electrons.
  • Group I metal: alkali metal
    • ☆ Physical properties（三低：低熔沸点、低密度、低硬度）
      • ① Group I metals are soft metal, have low m.p, b.p and low density. ② The m.p and b.p decrease down the group. ③ The alkali metals get softer down the group. ④ The density increase down the group
    • ☆ Chemical reactivity increases down the group.
      • Alkali metals can react with water to form metal hydroxide and hydrogen. 2Na + 2H2O—> 2NaOH + H2 Observation: Solid disappear/ melt/ move around, bubble, flame
  • Group VII elements: halogen
    • Group VII elements are diatomic molecules.
    • ☆ Physical properties
      • ① The m.p and b.p increase down the group. ② The state change from gas to liquid to solid down the group. ③ The colour gets darker down the group. ④ The density increase down the group.
    • ☆ The reactivity of halogens decreases down the group.
      • The more reactive halogen displaces the less reactive halogen from a its halide. Cl2 + 2NaBr —>Br2+ 2NaCl (活性强的非金属单质可以换出活性弱的)
  • Transition metal
    • ☆ Physical properties (三高: 高熔沸点、高密度、高硬度)
      • ① High melting and boiling points ② High density ③ Stronger and harder than Group I metals ④ Form colored compounds 所有金属共有的性质： 1、Malleable and ductile 2、conduct electricity
    • ☆Chemical properties
      • 1.They have variable oxidation states 2.Form complex ions 3.Elements and compounds of transition metals act as catalyst 4. are less reactive than metals from other groups
    • Noble gases in Group VIII or 0
      • eg. Helium for filling balloons (unreactive and low density). Argon used in lamps (unreactive).
      • Noble gases are unreactive monoatomic/ single atoms, because their outer electron shell are full. Noble gases provide an inert atmosphere
• unit14-Metals and reactivity
  • physical properties of metals
    • Structure of metal: a lattice of positive ions in a “sea of delocalized electrons” .
    • physical properties of metals: conductor of electricity and heat, malleable, ductile, shiny
    • Properties ① High m.p. & b.p.: The attractive force between metal ions and delocalised electrons is strong, which need a lot of energy to break. ② Good conductivity: the delocalised electrons are free to move. ③ Malleable and ductile: Metal ions are arranged in layers. When a force is applied, the layers can slide over each other.
  • The metal reactivity series (金属活性顺序)
    • K Na Ca Mg Al ( C ) Zn Fe Sn Pb (H) Cu Ag Au（从左往右降低）
    • Displacement reaction: （置换反应：活泼的金属/非金属单质换出不活泼的金属/非金属单质） The more reactive metal (carbon) can displace the less reactive metal from oxide and the solution of its salts.
  • Explain to the reactivity order
    • 1. Reason for reactivity series: A more reactive metal loses its outer shell electron (to form positive ion) more easily than a less reactive metal.（金属越活泼，说明其失去外层电子的能力强即越 容易失去外层电子）
    • Experiments to test reactivity order: 1) The more reactive metal reacts with water/ acids more violently. 2) React metals with different solutions of metal ions/oxides.
  • Unreactivity of aluminium
    • Aluminium form tough unreactive oxide layer which adheres to the metal. 4Al(s) + 3O2→ 2Al2O3(s)
    • The metals above carbon only can be extracted by electrolysis of their molten compound. Metals below carbon can be reduced by carbon
• unit15-more about metal
  • extracting iron
    • Raw materials: iron ore/ hematite, coke, limestone and air
    • 1.Coke burning: C (s) + O2(g)—>CO2 (g) (provide heat) 2.Carbon monoxide formed: CO2 (g)＋C (s）—> 2CO(g) (produce reducing agent) 3.Iron(III) oxide is reduced: Fe2O3(s) + 3CO (g)—>2Fe (l) + 3CO2 (g) Fe2O3(s) + 3C (s)—>2Fe (l) + 3CO(g） 4.Limestone decomposes: CaCO3—>CaO + CO2 5.Slag formation: SiO2(s) + CaO(s)—> CaSiO3(l) (slag is run off on the surface of the melton iron )
  • the rusting of iron
    • Methods
      • 1．Paint （汽车喷漆） 2. plastic coating （铁丝外层裹塑料） 3. metal plating （重点考察） 4. oiling
    • Sacrificial protection（牺牲保护法 — 替死鬼法
      • galvanising: (特指由)using a more reactive metal to protect a less reactive metal from corrosion —(zinc acts as a barrier which prevents water and air / oxygen form touching the iron.) 例Zn protect Fe: Zn is more reactive than Fe, Zn loses electrons more readily than Fe, so Zn corrodes before the Fe.
  • alloys
    • the similarity between alloy and metal
      • Good electrical conductor Godd heat conductor Malleable and ductile
    • the difference between alloy and metal
      • Alloy have lower melting than pure metal （impurity） Alloy harder and stronger than pure metal reason:different size of atoms make the structure less regular the layers can not slide very easily
  • use of metals
• unit6-chemical calculation
  • Calculations
    • Relative molecular mass (Mr): the sum of the relative atomic mass. eg. Mr (CO2)=12+16×2=4
    • Mole: Mole The amount of substance with the Avogadro constant of particles.
    • Avogadro constant Avogadro constant is the number of atoms, ions, or molecules in one mole. Avogadro constant = 6. 02/6.0 ×1023
    • Molar gas volume 简称 Vm: the volume of one mole of any gas (at definite temperature and pressure). At r.t.p. (room temperature and pressure, 20℃, 1 atm), Vm = 24 dm3/mol. 计算的时候特别需 注意体积的单位为 dm3 .
  • Calculate the mole
    • n(Number of mole) = m(real mass)／M(molar mass) = V(real volume)／Vm(molar volume) = = c (concentration) × V(volume of solution) 该公式适用于处于溶液中的物质。
      • M 通常用 Mr 代替（适用于任何已知质量的物质）
      • Vm 通常用 24 dm3 代替（适用于 RTP(room temperature and preesure)处于气态的物质））
  • Percentage
    • Percentage by mass
• unit5-Formula,equations
  • Type of equation.
  • Name of ionic compound离子化合物
  • Name of COVALENT compound共价化合物
• Unit 4 Structure and bonding
  • Metal atoms loss outer shell electrons to form positive ions
  • Ionic bonding -The attractive force between positive and negative ions.
  • Covalent bond: a shared electron pair(s) between two (non-metal) atoms
  • Metallic bonding -Definition of metallic bond- the attractive force between positive ions and delocalized. electrons
    • Structure of metal: a lattice of positive ions in a “sea of delocalized electrons” . Properties ① High m.p. & b.p.: The attractive force between metal ions and delocalised electrons is strong, which need a lot of energy to break. ② Good conductivity: the delocalised electrons are free to move. ③ Malleable and ductile: Metal ions are arranged in layers. When a force is applied, the layers can slide over each other.
  • 7. Giant covalent structure/ macromolecules
    •  Graphite structure: Each carbon atom forms 3 covalent bonds with others and are arranged in layers. The force between the layers is weak intermolecular force. Properties: ①soft, reason: weak intermolecular forces between layers, layers can slide over each other. ②high m.p. & b.p. , reason: each carbon atom is bonded to 3 other atoms, the covalent bonds between atoms is strong, which needs a lot of energy to break. ③conduct electricity, reason: the delocalised electron can move freely. Uses: electrode (conductor), lubricant (soft), pencil ‘lead’ (soft)
    •  Diamond structure: tetrahedral, each carbon atom forms 4 covalent bonds with others and they form giant covalent structure. Properties: ① hard, each carbon atom forms 4 covalent bonds with others and they form giant covalent structure. ② high m.p. & b.p., reason: carbon atoms are arranged tetrahedrally/ Each carbon atom is bonded to 4 other atoms. the covalent bonds between atoms are strong, which needs a lot of energy to break ③ can’t conduct electricity, reason: have no moving charged particles/ion/ electron Uses: cutting and drilling (hard) , jewellery (shiny)
    •  Silicon dioxide/ silicon(IV) oxide structure: • Similar to diamond, tetrahedrally arranged • Each silicon atom is bonded to four oxygen atoms. • Each oxygen atom is bonded to two silicon atoms. Properties: ① hard, ② high m.p. & b.p., ③ can’t conduct electricity (reason is similar to diamond).
• Unit 3 Atoms, elements and compounds
  • structure of atom
    • proton number（质子数）: the number of protons in the nucleus of an atom. nucleon number（核子数）: the number of protons plus neutrons in the nucleus of an atom.
  • the symbol of element
    • Atomic number = proton number 原子序数等于质子数 Mass number = nucleon number = proton number + neutron number In atoms, electron number = proton number In negative ions, electron number ＞ proton number 所带负电荷=电子数-质子数 In postive ions, electron number < proton number 所带正电荷=质子数-电子数
  • 6. element , compound and mixture
    • Alloy is as a mixture of a metal with other elements.
    • Element -is a substance made up of one type of atom is called an element.
    • A compound is a substance made up of two were more types of atoms join together be chemical bonding.
    • Mixture contains two or more elements or compounds that are not chemically bonded together. eg. air, sea water, solution
• Unit 2 seperating substance
  • Chromatography （纸色谱法）
    • =Value
    • Chromatogram(色谱图)
  • Methods of unification
    • Filtration-Separate an Insoluble of salt from a liquid.
    • Crystallization-Obtain a soluble crystalline solid from a solution.
    • Fractional distillation-Separate and mixture of liquids with different boiling point.
      • Example: separate mixture of ethanol and water • Ethanol has lower boiling point than water • When heating, ethanol evaporates more easily than water. • Water vapour condenses back into the flask by fractionating column. • Ethanol vapour goes to ethanol liquid in condenser and is collected first
• Unit 1 Particles theory
  • particles
    • ☆An atom is the smallest particle that cannot be broken down by chemical means
    • ☆A molecule is a particle of two or more atoms joined together.
    • An ion is an atom a group of atoms that carries an electrical charge.
  • state of the matter
    • solid
      • Fixed Arrangement,Only vibrate,Close together,Definite shape.
    • liquid
      • Random arrangement,Slide pass each other,Close together , shape of its container.
    • Gas
      • Random arrangement, move randomly,take the shape of its container.
  • particularly
    • diffusion
      • The random and constant movement of different particles so they get mixed up is called diffusion. 
    • -Changing of state
    • solvent,solutes,and solutions
      • Sarurated solution （饱和溶液）contains the maxium concentration of a solute dissolved in a solvent at a specified temperature. 