States of Matter

1. States of Matter Diffusion Define diffusion __________________________________________ _______________________ ________________________________ The smoke forms nearer to the ammonia end – why?.___________________________________- Pressure Define pressure __________________________________________ _______________________ ________________________________ State 4 ways to increase pressure ________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ 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 _______________________ _______________________ _______________________ Separation techniques – draw a labelled diagram for the following and give an example of each filtering Chromatography Distillation Fractional distillation Crystallisation Purity testing Define Solvent _________________________________________ Define Solute _________________________________________ Define insoluble _________________________________________ Define dissolve_________________________________________ Define solution_________________________________________

2. Metallic/Ionic/Covalent Bonding Chemical reactions • 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 Covalent Bonding – Draw on the electrons to show bonding Ionic Bonding – Draw the ions for the following Hydrogen Chlorine Water Oxygen Methane (CH4) Carbon dioxide (CO2)

3. Name the 3 parts of the atom. a__________________ b__________________ c__________________ • 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 __________. 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+ compound Cl- 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 _______. • 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. Complete the electron arrangement of a boron atom Complete the electron arrangement of a boron ion

4. Periodic Table Label Nucleon number and Proton number (LHS) Protons neutrons Electrons (RHS) Name the 3 parts of the atom. a__________________ b__________________ c__________________ • 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 ________________. Halogens Give two examples of halogens ______________________________________ Describe what they look like _______________________________________ Why does reactivity decreasedown the group? _______________________________________ _____________________________________ Transition metals What are their physical properties? _________________________ _________________________ What are their chemical properties? _________________________ _________________________ What are their uses? __________________________________________________ Alkali Metals What do they look like? ______________________________________ Why are they stored under oil? _______________________________________ Why does reactivity increasedown the group? _______________________________________ _______________________________________ Write the equation for sodium with water produces sodium hydroxide and hydrogen ______________________________________

5. Moles Gas Calculations What volume does 0.25moles of a gas occupy at rtp? 1 mole occupies 24 dm3 so 0.25 moles occupies 0.25 x 24 dm3 = 6 dm3 So 0.25 moles of any gas occupies 6dm3 at rtp. Q 3 What volume of nitrogen reacts with 10 kg of hydrogen to form ammonia? N2(g) + 3 H2(g) ® 2 NH3(g) Q4 What volume of oxygen reacts with 510 g of ammonia? 4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g) Avagadro’s constant is 6.02x1023 Atom calculations How many atoms of carbon are in a 10 g diamond Moles = mass/RMM = 10/12= 0.833 moles 1 moles = 6.02x1023 0.833 x 6.02x1023 = 5.02x1023 Q1 What mass of silicon contains 1.25x1022 silicon atoms Q2 What mass of titanium contains 1.204x1024 atoms • Concentrations • Solution A contains 2.5g copper sulphate in 1dm3 of water • Solution B contains 125g copper sulphate in 0.5dm3 water • Change the mass to moles. • Mr of copper sulphate is 250 • Solution A : 2.5g = 0.01 moles 1dm3 there are 0.01 moles/dm3 • Solution B : 125g in 0.5dm3, which is 250g in 1dm3 =1 moles/dm3 = 1M • Q5 What is the concentration of a solution containing. • 4 moles in 2 dm3 of solution • 0.3 moles in 200cm3 of solution • Q6 The Mr of sodium hydroxide is 40. How many grams of sodium hydroxide are in • 500cm3 of a molar solution • 25cm3 of a 0.5M solution What mass of aluminium oxide is produced when 135 g of aluminium is burned in oxygen? 2 Al + 3 O2 Al2O3 What mass of iodine is produced when 7.1 g of chlorine reacts with excess potassium iodide? Cl2 + 2 KI  2 KCl + I2 For each of the following compounds the Mr and the empirical formula is shown. Work out the molecular formula of each compound. empirical formula = CH3 Mr = 30 empirical formula = NH3 Mr = 17 empirical formula = CH2 Mr = 98 empirical formula = CH Mr = 78 Calculate the percentage of the elements shown in the following compounds:  C in CO N in (NH4)2SO4  O in Al(OH)3 O in Na2CO3.10H2O

6. Acids and Bases Zinc reacts with oxygen. Zinc oxide is made. What are the reactants?________ ________ What is the product?_____________ Complete the word equation for this reaction ___________+ ____________ __________ ________ 2Zn + O2 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 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 + ___________ ____________ • Acids have pHs of _____ to _____ • Bases (soluble alkalis) have pHs of _______ to ______. • Neutral is pH _______ • Indicators are used to…. • 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

7. Organic Chemistry Cracking Difference between alkanes and alkenes __________________________________________________ __________________________________________________ What can you use to test if something is an alkane or alkene? __________________________________________________ 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 ________________________________________________________ Two ways to make alcohol __________________________________________________ __________________________________________________ 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.

8. Polymers Match up the following 5 uses of plastics ____________________________________________________________________________________________________ 5 properties of plastics _____________________________________________________________________________________________________________________________ How can plastics be disposed of __________________________________________________

9. Define Rate of Reaction _______________________________________ Rates of Reaction What FOUR things cause a reaction to increase? Explain using particle theory! 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) ____________________________________________________________________________________________________________________________________________________________________________________________________________________________

10. Behaviour of Metals 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? ___________________ ______________________ Why does aluminium not rust? ______________________________ _______________________________________________________ Explain 2 ways you can protect iron from rusting? _______________________________________________________ _______________________________________________________ ______________________________________________________ Iron reduces copper oxide (OIL RIG) Equation Fe (s) + CuO (s)  FeO (s) + Cu(s) 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)

11. This reaction takes place in the blast furnace: Fe2O3(s) + 3CO ( g) 2Fe (l) + 3CO2( g) The word equation for the reaction is: …………………………………………………………………………………………… It is a redox reaction, because …………………………………………………………………………………………… The reducing agent in this reaction is ……………………………….... REDOX OILRIG stands for O_________ I__ L_______ o __ e_________ R__________ I__ G_______ o__ e_________ Which is being oxidised and which is being reduced? • a) Mg + 2HCl → MgCl2 + H2 • b) 2CO + O2 → 2 CO2 • c) 3H2 + N2 → 2NH3 • d) 4Na + O2 → 2Na2O Work out the oxidation states : 2Mg + O2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 Cu2O ___________ • Fe in FeCl2___________ • Fe in FeCl3 ___________

12. Electrolysis 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. 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 ___________________________ Match the keyword negative ions liquid which conducts electricity positive electrode Positive ions Negative electrode Anode Cathode Anions Cations Electrolyte

13. USES of METALS 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 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 ______________ _______________________________________________________ Ores What is haematite ? ______________________ What is bauxite? _________________________ Extracting zinc How do you extract zinc from zinc blende? _______________________________________ _______________________________________ _______________________________________ 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. _________________________________________________________________________________

14. 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 releasedExothermic/endothermic Burning a fuel in air Exothermic/endothermic Increasing Pressure Increasing Concentration Increasing temperature

15. Seperation of air AIR and WATER You can separate gases from air by fractional distillation. ________________________________________________________ ________________________________________________________ 2 uses of oxygen _______________________________________ 2 uses of nitrogen _______________________________________ 2 uses of noble gases _______________________________________ What is the equation for respiration _______________________________________________________ What is the equation for combustion _______________________________________________________ What is the equation for photosynthesis _______________________________________________________ What is thermal decomposition? _______________________________________________________ Water treatment Add the labels chlorination (kill bacteria) coagulant sand filters and charcoal add air Define solution_________________________________ Define solvent _________________________________ Define soluble_________________________________ 2 tests for water? ________________________________________________________ ________________________________________________________ What is the composition of air? Complete the pie chart for oxygen, nitrogen, carbon dioxide and other gases Name 4 pollutants in air _______________________________ _____________________________________________________________ Rusting What 2 conditions are needed for rusting? _______________________ Write and equation __________________________________________ How can you stop rusting _____________________________________ __________________________________________________________ __________________________________________________________

16. Non-Metals Y11 Thermal decomposition Define Thermal decomposition ______________________________ 2 Uses of Calcium oxide ____________________________________ What is the equation for calcium oxide when it reacts with water? ________________________________________________________ Making fertilisers Element What it is used for? Nitrogen _______________________________________ Phosphorous _______________________________________ Potassium _______________________________________ Limestone Formula of Limestone? ___________________________________ 2 uses of limestone _____________________________________ Formula of Lime _______________________________________ 2 uses of lime ________________________________________ Formula of Slaked Lime ___________________________________ 2 uses of Slaked Lime ____________________________________ Equations for making fertilisers 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? _______________________ _____________________________________________________

17. In the Lab