States of Matter Y9 Diffusion Define diffusion Draw a particles (circles) diagram Heating and cooling curves Label the graph with the state at each point. Why does the temperature not change when something changes state The smoke forms nearer to the ammonia end why?. - Pressure Define pressure State 4 ways to increase pressure Separation techniques draw a labelled diagram for the following and give an example of each filtering Distillation Chromatography Fractional distillation Define Solvent Define Solute Define insoluble Define dissolve Define solution Crystallisation Purity testing
Chemical reactions Y9 Give 4 signs that a chemical reaction has taken place Element/compound or mixture Can contain any number of substances in a different ratio A/B/C/D Element/compound or mixture Contains one type of atom A/B/C/D Element/compound or mixture Contains more than one type of atom chemically bonded A/B/C/D lement/compound or mixture Metallic/Ionic/Covalent Bonding Ionic Bonding Draw the ions for the following Diamond Graphite Covalent Bonding Draw on the electrons to show bonding Hydrogen Chlorine Use Bonding (diagram) Oxygen Methane (CH 4 ) Water Properties Carbon dioxide (CO 2 )
Subatomic particle Mass Charge +1-1 Colour on the Periodic table non-metals unreactive gases alkali metals are found (very reactive) Atoms in the same group have similar properties because they have the same number of in the outer shell. The mass number is the total number of and. The atomic number is the number of. 0 Match the pictures above with the words below and define the words Element Compound Mixture Complete the sentences with the following words. (some are red herrings!) Ionic element sodium electron covalent chlorine chlorine sodium Na+ Na- Cl+ compoundcl- Sodium chloride NaCl is a. There are bonds between the two elements and. When these atoms bond one from the atom is donated to the atom. This results in 2 ions : and. Complete the electron arrangement of a boron atom Complete the electron arrangement of a boron ion Isotopes Isotopes are atoms of the same element with the same/different numbers of protons. Isotopes are atoms of the same element with the same/ different numbers of electrons. Isotopes are atoms of the same element with the same/ different numbers of neutrons. ion Lost/ gained? Mg 2+ lost 2 Cl - Li + O 2- Fe 3+ Number of electrons
Periodic Table y10 Subatomic particle Mass Charge +1-1 0 Label Nucleon number and Proton number (LHS) Protons neutrons Electrons (RHS) Colour on the Periodic table non-metals unreactive gases alkali metals are found (very reactive) Atoms in the same group have similar properties because they have the same number of in the outer shell. The nucleon number is the total number of and. The proton number is the number of which is equal to the number of. Alkali Metals What do they look like? Why are they stored under oil? Why does reactivity increase down the group? Write the equation for sodium with water produces sodium hydroxide and hydrogen Transition metals What are their physical properties? What are their chemical properties? What are their uses? Halogens Give two examples of halogens Describe what they look like Why does reactivity decrease down the group?
Rates of Reaction y10 What FOUR things cause a reaction to increase? Explain using particle theory! 1. 2. 3. 4. Define Rate of Reaction Two reasons a reaction stops? What 2 things need to occur for a reaction to happen Draw the apparatus to investigate the rate of reaction Describe the role of light in photochemical reactions and the effect on the rate (speed)
Equilibrium & Breaking Bonds Define exothermic reaction Define endothermic reaction Define equilibrium Define Dynamic Exothermic/endothermic? Amount of energy needed to break bonds less than amount of energy released. Exothermic/endothermic If the energy taken in to break bonds is more than the energy released Exothermic/endothermic Burning a fuel in air Exothermic/endothermic Hydrogen Biofuel Nuclear fuel 2 pros 2 cons Increasing Pressure Increasing Concentration Increasing temperature
REDOX y10 OILRIG stands for O I L o e R I G o e Rules Oxidation state of an element is 0 Ionic compounds oxidation state is its charge Hydrogen = +1 Oxygen = -2 Oxidation states in a compound = 0 This reaction takes place in the blast furnace: Fe 2 O 3 (s) + 3CO ( g) 2Fe (l) + 3CO 2 ( g) The word equation for the reaction is: It is a redox reaction, because The reducing agent in this reaction is... Which is being oxidised and which is being reduced? Work out the oxidation states : 2Mg + O 2 2MgO Mg = O = MgO Has the Mg been oxidised/reduced? Has the O been oxidised/reduced? What is the oxidation state of: Cu in CuO Cu in Cu 2 O Fe in FeCl 2 Fe in FeCl 3 a) Mg + 2HCl MgCl 2 + H 2 b) 2CO + O 2 2 CO 2 c) 3H 2 + N 2 2NH 3 d) 4Na + O 2 2Na 2 O
Electrolysis y10 What is a conductor? _ What is an insulator? Why are the only solids that conduct are metals and graphite Why do ionic substances only conduct when molten/dissolved Electrolysis Define electrolysis 4 uses of electrolysis RULES FOR ELECTROLYSIS At cathode (-), either a metal/hydrogen forms If a metal is more reactive than hydrogen its ions stay in solution and hydrogen bubbles off If the metal is less reactive than hydrogen the metal forms. At anode (+) a non-metal other than hydrogen forms. If it is a concentrated solution of a halide then halogens form. If the halide solution is dilute /no halide oxygen forms. Match the keyword Anode Cathode Anions Cations Electrolyte negative ions liquid which conducts electricity positive electrode Positive ions Negative electrode Chemical Sodium chloride Chlorine Hydrogen Sodium hydroxide Uses Electrolysis of Brine Ionic equation at cathode Ionic equation at anode Test for chlorine Electrolysis of copper with copper electrodes Ionic equation at cathode Ionic equation at anode Electrolysis of copper with inert electrodes Ionic equation at cathode Ionic equation at anode
Moles y10 Avagadro s constant is 6.02x10 23 Atom calculations How many atoms of carbon are in a 10 g diamond Moles = mass/rmm = 10/12= 0.833 moles 1 moles = 6.02x10 23 0.833 x 6.02x10 23 = 5.02x10 23 Q1 What mass of silicon contains 1.25x10 22 silicon atoms Gas Calculations What volume does 0.25moles of a gas occupy at rtp? 1 mole occupies 24 dm 3 so 0.25 moles occupies 0.25 x 24 dm 3 = 6 dm 3 So 0.25 moles of any gas occupies 6dm 3 at rtp. Q 3 What volume of nitrogen reacts with 10 kg of hydrogen to form ammonia? N 2(g) + 3 H 2(g) 2 NH 3(g) Q4 What volume of oxygen reacts with 510 g of ammonia? 4 NH 3(g) + 5 O 2(g) 4 NO (g) + 6 H 2 O (g) Q2 What mass of titanium contains 1.204x10 24 atoms What mass of aluminium oxide is produced when 135 g of aluminium is burned in oxygen? 2 Al + 3 O 2 Al 2 O 3 What mass of iodine is produced when 7.1 g of chlorine reacts with excess potassium iodide? Cl 2 + 2 KI 2 KCl + I 2 For each of the following compounds the M r and the empirical formula is shown. Work out the molecular formula of each compound. 1. empirical formula = CH 3 M r = 30 2. empirical formula = NH 3 M r = 17 3. empirical formula = CH 2 M r = 98 4. empirical formula = CH M r = 78 Calculate the percentage of the elements shown in the following compounds: C in CO N in (NH 4 ) 2 SO 4 O in Al(OH) 3 O in Na 2 CO 3.10H 2 O Concentrations Solution A contains 2.5g copper sulphate in 1dm 3 of water Solution B contains 125g copper sulphate in 0.5dm 3 water Change the mass to moles. Mr of copper sulphate is 250 Solution A : 2.5g = 0.01 moles 1dm 3 there are 0.01 moles/dm 3 Solution B : 125g in 0.5dm 3, which is 250g in 1dm 3 =1 moles/dm 3 = 1M Q5 What is the concentration of a solution containing. a) 4 moles in 2 dm 3 of solution b) 0.3 moles in 200cm 3 of solution Q6 The Mr of sodium hydroxide is 40. How many grams of sodium hydroxide are in a) 500cm 3 of a molar solution b) 25cm 3 of a 0.5M solution
Behaviour of Metals y10 Where are metals found in the periodic table? Name 5 properties of metals Chemical properties of metals Draw a picture of an alloy What is an alloy? Iron reduces copper oxide (OIL RIG) Equation Fe (s) + CuO (s) FeO (s) + Cu(s) Why does aluminium not rust? Explain 2 ways you can protect iron from rusting? Half equations Ionic equations Thermal Decomposition Reactions Oxide + carbon dioxide (except Na &K) Oxide + Water (except Na & K) Oxide + nitrogen dioxide + oxygen (except Na & K)
USES of METALS y10 Name two uses of aluminium? Two uses of copper? Two uses of zinc? Name the uses of mild steel Name the uses of stainless steel Name the uses of copper related to its properties Label the blast furnace Name an iron ore used in the blast furnace. Name two substances that are mixed with iron ore Name one of the gases leaving the blast furnace. Name two substances which react together to produce most of the energy required to heat the furnace to 1400 C What impurities are found and how are they removed. Extraction of metals from the ores Label on the right Which ones are extracted by electrolysis, which are found naturally and which are burnt with carbon and reduced Ores What is haematite? What is bauxite? Extracting zinc How do you extract zinc from zinc blende?
AIR and WATER Y11 What is the equation for respiration What is the equation for combustion What is the equation for photosynthesis Seperation of air You can separate gases from air by fractional distillation. 2 uses of oxygen 2 uses of nitrogen 2 uses of noble gases Water treatment Add the labels chlorination (kill bacteria) coagulant sand filters and charcoal add air What is thermal decomposition? What is the composition of air? Complete the pie chart for oxygen, nitrogen, carbon dioxide and other gases Name 4 pollutants in air Define solution Define solvent Define soluble 2 tests for water? Rusting What 2 conditions are needed for rusting? Write and equation How can you stop rusting
Non-Metals Y11 Making fertilisers Element What it is used for? Nitrogen Phosphorous Potassium Equations for making fertilisers Thermal decomposition Define Thermal decomposition 2 Uses of Calcium oxide What is the equation for calcium oxide when it reacts with water? Limestone Formula of Limestone? 2 uses of limestone Formula of Lime 2 uses of lime _ Formula of Slaked Lime 2 uses of Slaked Lime Ammonia + nitric acid + Sulphuric acid ammonium Ammonia + acid phosphate Potassium hydroxide + nitric acid potassium +water Ammonium chloride + calcium hydroxide calcium chloride + water + Haber Process What does the Haber process make? What is the equation? Where does the nitrogen come from? Where does the hydrogen come from? 3 conditions for the Haber Process?
Organic Chemistry Y11 Difference between alkanes and alkenes What can you use to test if something is an alkane or alkene? Two ways to make alcohol Cracking What is cracking? What conditions are needed for cracking? What is a hydrocarbon? Combustion What is combustion? _ Equation for Complete Combustion Equation for Incomplete Combustion Fractional Distillation The crude oil enters the column at the where it is extremely. Here the different fractions and evaporates. The higher they rise the they become. When they enough they will turn back to. The fractions can be collected at the of the column. Fractions with boiling points are found at the bottom. Ones with boiling points are found at the top.
Polymers Y11 Match up the following 5 uses of plastics 5 properties of plastics How can plastics be disposed of
Acids and Bases Y10 Zinc reacts with oxygen. Zinc oxide is made. What are the reactants? What is the product? Complete the word equation for this reaction + Reactions with Acids. Complete the equations Acid+ metal salt + hydrogen Hydrochloric acid + magnesium chloride + hydrogen acid + zinc zinc sulfate + Hydrogen Acid + metal oxide salt + water Acid + metal hydroxide salt + water Nitric acid + copper oxide- + water Sulphuric acid + zinc sulfate + water acid + sodium hydroxide sodium chloride + Acid+ metal carbonate salt + water + carbon dioxide Hydrochloric acid + sodium carbonate + water + Which gas What do you do? What happens? Gives a squeaky pop 2Zn + O 2 2ZnO How many Zinc and Oxygen atoms are on the left-hand side? Zn 0 How many Zinc and Oxygen atoms are on the right-hand side? Zn O Is this equation balanced? Yes/No ph 2 7 8 14 Colour with Universal indicator Purple Red Blue Green Acid Alkali, neutral? Strong Alkali Acids have phs of to Bases (soluble alkalis) have phs of to. Neutral is ph Indicators are used to. Oxygen Bubble through limewater Complete the equation for a neutralisation reaction: Acid+ Alkali + Tick which of the following are real uses of neutralisation reactions. Indigestion tablets (neutralising stomach acid) In cars (neutralising battery acid) On fish and chips (vinegar is an acid) In Gardening (Neutralising acidic soils) In Lakes (Neutralising lakes which have become acidic due to acid rain
In the Lab Y11 Metal Colour of flame Copper Lilac Ion tested Solution added colour Barium chloride + dilute hydrochloric acid Chloride (Cl ) A white precipitate Copper zinc Lithium Sodium Barium Brick-red Iron(III), (Fe 3+ (aq)) Iron(II) (Fe 2+ (aq)) Sodium hydroxide Sodium hydroxide with aluminium foil and heat Hydrochloric acid White precipitate in NaOH, which dissolves in excess Bubbles of carbon dioxide are given off. Colourless precipitate Iodide (I ) Barium chloride + dilute hydrochloric acid A white precipitate of barium sulfate is formed. Metal Colour of flame Carbon dioxide Damp litmus gets bleached Oxygen Hydrogen