Review Chemistry Paper 1

Transcription

1 Atomic Structure Topic Define an atom and element. Use scientific conventions to identify chemical symbols Identify elements by chemical symbols Define compound Use chemical formulae to show different elements and number of atoms present in a compound Write word and symbol equations for chemical reactions Define the terms reactant and product Understand that mass of product is equal to mass of reactants Know that mixtures consist of two or more elements/compounds that are not chemically combined Components of mixtures retain their properties e.g. mixture of Iron & Sulphur; Fe is still magnetic, S is still yellow. Know physical methods to separate mixtures; filtration, crystallisation, simple distillation, fractional distillation & chromatography. Understand the Plum pudding model of the atom Understand that the nuclear model is now accepted Know the mass & charges of Protons, Neutrons & Electrons Understand the terms atomic number and mass number Describe isotope Work out the electronic configuration of the first 20 elements Know the key stages in the development of the Periodic table (Newlands & Mendeleev) Understand the properties of Group 0 elements, noble gases Understand the properties of Group 1 elements, alkali metals Understand the properties of Group 7 elements, halogens Quantitative Chemistry topic Conservation of mass and the quantitative interpretation of chemical equations Explain the meaning of the law of conservation. Write simple word equations. Write simple symbol equations. Balance symbol equations and add state symbols. Balance complex equations (HT) Recall the definition of relative atomic mass. Find the relative atomic mass from the Periodic Table. Define the relative molecular mass. Calculate the relative formula mass. Use measurements of mass before and after an experiment to explain what has happened to the mass during the experiment and why it has happened.

2 Quantitative Chemistry Topic Continued Use of amount of substance in relation to masses of pure substances (higher tier unless stated) Define one mole in terms of Mr and Ar Calculate the number of moles in a substance using the relative formula mass. Balance chemical equations and use these to calculate the masses of substances present. Use the masses of substances present in a reaction to write a balanced equation. Define the term limiting reactant. Link the limiting reactant to the number of moles. Link the limiting reactant to the masses in grams. Explain the meaning of concentration and the unit grams per dm 3 (FT) Be able to convert cm 3 into dm 3 (FT) Use the equation to calculate the concentration of a solution. C = m / v (FT) Rearrange the equation to make mass the subject. C = m / v Exothermic and endothermic reactions Define the term: exothermic, endothermic Chemical Energy Changes Topic Write the required practical with all variables and analyse the data and know the method investigating the variables that affect temperature changes in reacting solutions Define the term activation energy. Draw reaction profiles for exothermic and endothermic. Explain what the diagrams display. Calculate the energy transferred in chemical reactions Describe how to how to calculate the energy transferred in a chemical reaction. Explain why a chemical reaction is classed as being exothermic or endothermic in relation to the energy involved in breaking and making bonds. Use the collision theory to explain rate of reaction Explain the use of a catalyst and the effects on the rate of reaction Explain reversible reaction Define equilibrium The energy change of reactions (HT) Explain the use of energy to break reactant bonds Explain energy released when bonds break Calculate bond energies Explain the differences between sum of energy needed to break bonds and make bonds Exothermic reaction bond energies Calculate energy transferred in chemical reactions using bond energies

3 Chemical Change topic Reactivity of metals Metal oxides Write a word equation to show what happens when a metal reacts with oxygen Define the term oxidation Define the term reduction Reactivity series State what type of ions metals make when they form ionic bonds Predict the products of a displacement reaction when given a reactivity series. Extraction of metals and reduction Explain why metals like gold can be found in the Earth on their own Describe how metals less reactive than Carbon can be separated from their ore Define the term oxidation in terms of electron transfer (Higher only) Define the term reduction in terms of electron transfer Higher only) Reactions of acids with metals/making salts State the ions all acids have State the ions all alkalis have Recall the colours of the Universal Indicator scale and what they represent. Write a word equation for the reaction of an acid with an alkali and name this type of reaction Write a word equation for the reaction of an acid with a base and name this type of reaction Write a word equation for the reaction of an acid with a metal carbonate Describe the difference between an acid and a base Write a method for making a soluble salt from an insoluble base. Include the equipment you would use. Define the term strong acid using the term ionisation (Higher only) Define the term weak acid using the term ionisation (Higher only) Electrolysis Define the terms electrolysis, electrolyte, anode and cathode Describe what happens at the anode when lead bromide is electrolysed Describe what happens at the cathode when lead bromide is electrolysed Explain why electrolytes have to be liquids and not solids Write half equations to show what happens at the anode and the cathode during the electrolysis of lead bromide (Higher Only) Describe how electrolysis can be used to separate Aluminium from its ore. Explain why cryolite is use d in the process of separating Aluminium from its ore. Write half equations to show what happens at the anode and the cathode during the electrolysis of Aluminium ore (Higher Only) Write a method for the electrolysis of sodium chloride solution (an aqueous solution) Include equipment you would use and the results you would see. Explain why you get Hydrogen gas at the negative electrode when you electrolyse an aqueous solution.

4 Structures & Bonding Topic Explain why simple molecules have low melting and boiling points and link to RT state Understand that the intermolecular forces are overcome when a simple molecular substance melts or boils NOT the covalent bond! Explain why simple molecules do not conduct electricity. Explain why ionic compounds have high melting and boiling points. Explain how ionic compounds conduct electricity when molten or dissolved in water. Explain why giant covalent structures like diamond/graphite/silica have very high melting points. Explain why the bonding in diamond allows it to be very hard. Explain why the bonding in graphite allows it to be soft and slippery. Explain how delocalised electrons allow graphite to conduct heat and electricity. Describe the uses of fullerenes including graphene sheets and nanotubes Recognise carbon structures from diagrams and descriptions. Explain why the structure of metals allow them to conduct heat and electricity and to be shaped and bent State what an alloy is and explain why alloys are harder than pure metals (different sizes atoms) Describe how properties of polymers (thermosetting/softening) depend on what they are made from and the conditions they were made under Draw diagrams to model particles in the 3 states of matter Use particle theory to explain melting, boiling, freezing and condensing Describe how materials might change at the melting and boiling points Use ideas about types of bonding, forces and energy to explain and compare melting and boiling points Predict the state of a material given data about melting and boiling points HT Explain the limitations of particle diagrams to show states and how they change in that they show no forces and all are shown as solid inelastic spheres Include and interpret state symbols in chemical equations for all the reactions I have studied

5 Structures & Bonding Topic part 2 Work out the charge on ions in groups 1&2 and 6&7 from the periodic table Write formula for ionic compounds Draw using dot and cross diagrams the electronic structure of ions in the above groups and compound they make eg NaCl, MgCl 2 Represent covalent bonds as dot and cross diagrams in molecules like water, ammonia, hydrogen chloride, methane, oxygen, chlorine, nitrogen AND giant structures like diamond and SiO 2 Represent covalent bonds as single lines in molecules like water, ammonia, hydrogen chloride, methane, oxygen, chlorine, nitrogen AND giant structures like diamond and SiO 2 Draw a diagram to represent bonding in metals. Define the term compound Describe how ions are formed in ionic bonding Explain why ionic compounds can form giant ionic structures Recognise the type of bonding/structure from a diagram Explain why covalent compounds are often simple molecules Work out empirical and molecular formulae from diagrams/models Describe limitations of 2D and 3D models Describe and explain the properties of giant covalent structures like diamond and SiO 2 Explain how delocalised electrons occur in metals