States of Matter 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 _______________________ _______________________ _______________________ Diffusion Define diffusion __________________________________________ _______________________ ________________________________ 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 filteringChromatography DistillationFractional distillation CrystallisationPurity testing Define Solvent _________________________________________ Define Solute _________________________________________ Define insoluble _________________________________________ Define dissolve_________________________________________ Define solution_________________________________________

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 Metallic/Ionic/Covalent Bonding Ionic Bonding – Draw the ions for the following Covalent Bonding – Draw on the electrons to show bonding Hydrogen Chlorine Water Oxygen Methane (CH 4 ) Carbon dioxide (CO 2 ) DiamondGraphite Use Bonding (diagram) Properties

Subatomic particle MassCharge +1 0 Match the pictures above with the words below and define the words Element Compound Mixture Name the 3 parts of the nucleus. a__________________ b__________________ c__________________ Complete the sentences with the following words. (some are red herrings!) Ionicelement sodiumelectron covalent chlorinechlorinesodiumNa+ 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 _______. ionLost/ gained? Number of electrons Mg 2+ lost2 Cl - Li + O 2- Fe 3+ Complete the electron arrangement of a boron atom Complete the electron arrangement of a boron ion 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 __________. 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.

Rates of Reaction y10 What FOUR things cause a reaction to increase? Explain using particle theory! 1.______________________________________________________ 2.______________________________________________________ 3.______________________________________________________ 4.______________________________________________________ Draw the apparatus to investigate the rate of reaction Define Rate of Reaction _______________________________________ Two reasons a reaction stops? _________________________________________ _____________________________________ What 2 things need to occur for a reaction to happen _______________________________________ _______________________________________ Describe the role of light in photochemical reactions and the effect on the rate (speed) ________________________________________ ________________________________________ ________________________________________ ________________________________________ ________________________________________ ____________________

Equilibrium & Breaking Bonds Define exothermic reaction _______________________ _______________________________________________ Define endothermic reaction ______________________ _________________________________________________ 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 airExothermic/endothermic HydrogenBiofuelNuclear fuel 2 pros 2 cons Draw a labeled energy profile for the combustion of methane (CH 4 ) Draw a labeled energy profile for the dehydration of CuSO 4.5H 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 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 ___________________________ Anode Cathode Anions Cations Electrolyte negative ions liquid which conducts electricity positive electrode Positive ions Negative electrode ChemicalUses Sodium chloride Chlorine Hydrogen Sodium hydroxide Electrolysis of Brine Ionic equation at cathode ___________________________ Ionic equation at anode ___________________________

Moles y10 Atom calculations How many atoms of carbon are in a 10 g diamond Moles = mass/RMM = 10/12= moles 1 moles = 6.02x x 6.02x10 23 = 5.02x10 23 Q1 What mass of silicon contains 1.25x10 22 silicon atoms Q2 What mass of titanium contains 1.204x10 24 atoms Avagadro’s constant is 6.02x10 23 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 KI  2 KCl + I 2 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) 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 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 = CHM 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