Past papers
Link to A-Level Specification
Intervention Timetable
VIMA Dates
Topic 4 exam style questions
VIMAIII Content
Textbook Answers
Module 4 exam style Qs
Module 4 Exam Style Qs - mark scheme
Module 2 Exam style Qs - mark scheme
Link to 18.2 Concentration-Time Graph Lesson Resources
VIMAV Info
Content - everything you have covered in year 12 so far including practical skills.
- 2x papers - 90 mins long
- Paper 1 has multiple choice questions
- Paper 2 does not
- Paper 1 - Monday 27th June 2016 - 13.30 - Boothroyd Hall
- Paper 2 - Thursday 30th June 2016 - 9am - Boothroyd Hall
YEAR 12 CHEMISTRY HOMEWORK BLOG
Due 20th June 2016
Complete all graphs to find the order with respect to HCl by finding and then plotting the initial rate of reaction for at least 3 concentrations. To be handed in on Monday.
Due Wednesday 4th May 2016
Complete worksheet on dynamic equilibrium attached here.
Due 27th April 2016
Complete textbook questions on p159
Due 13th April 2016
1. Complete the worksheet on the Boltzmann Distribution given to you in class
2. Complete questions 1-15 on the attached document.
3. Complete the past exam questions given to you in class on Monday.
(Just a reminder... you have an intervention test on Wednesday!)
Due 9th March 2016
Complete summary questions on page 141.
Due 2nd March 2016
Answer ALL textbook questions pages 142-143.
Due 24th February 2016
Complete the June 2010 past paper attached here.
Due 10th February 2016
Copy out every definition 10 times each.
- Activation energy, Ea, is the minimum energy required for a reaction to take place.
- Enthalpy profile diagrams – a diagram that shows the relative enthalpies of the reactants and the products and the enthalpy change ΔH .
- Enthalpy – H - is the measure of the heat energy in a chemical system.
- Standard pressure – 100 kPa
- Standard temperature – 298K
- Standard Enthalpy change of Reaction - ΔrHϴ - the enthalpy change that accompanies the reaction in the molar quantities shown in a chemical equation, under standard conditions, with all their reactants and products in their standard states.
- Standard Enthalpy change of formation - ΔfHϴ - the enthalpy change that takes place when one mole of a compound is formed from elements, under standard conditions, with all their reactants and products in their standard states.
- Standard Enthalpy change of combustion - ΔcHϴ - the enthalpy change that takes place when one mole of a substance reacts completely with oxygen, under standard conditions, with all their reactants and products in their standard states.
- Standard Enthalpy change of neutralisation - ΔneutHϴ - is the energy change that accompanies the reaction of an acid by a base to form one mole of H2O (l), under standard conditions, with all their reactants and products in their standard states.
Due 25th January 2016
Complete the whole past paper attached here, ready to go through on monday as part of revision.
Due 20th January 2016
Complete the new style Kerboodle past paper questions attached here.
Due Wednesday 13th January 2016
1. Finish worksheet from lesson on 11/01 - attached here in case you need it.
2. Copy out the definitions below 10 times each.
3. Complete the past paper questions attached here on group 2 elements.
- Periodicity - is the repeating trend in properties of the elements across a period.
- First ionisation energy – the energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions.
- Second Ionisation Energy - is the energy required to remove one electron from each atom in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions.
- Metallic bonding – fixed lattice of cations (positive ions) surrounded by a sea of delocalised electrons to create a giant metallic lattice.
Due Wednesday 6th January 2016
Complete the past paper questions if not finished in class on Monday. Link to sheet if needed here.
Due Wednesday 16th December
Complete past paper questions attached here.
Due 9th December
Complete worksheet from class.
Due 2nd December 2015
Finish off the worksheet started in lesson as revision before VIMAII. (example questions relating to amount of substance).
Due Wednesday 25th November (a.k.a - THE DAY OF VIMAII)
Complete ALL of the worksheet attached, with past paper questions. These questions will be most similar to the actual questions you will be answering in your A-level exams, so this is one of the most important worksheets you will have completed to date. Make sure you put in as much effort as possible. We will go through this as revision for the first 30 minutes on Wednesday, then your VIMAII is 1.5hrs.
Due 18th November 2015 (set 11/11/2015)
Complete past paper questions attached below. This link may be helpful in understanding how/why molecules have different shapes: https://ch301.cm.utexas.edu/help/ch301/geometries.pdf
Re-cap on acids
Molecule shapes and bond angles
The worksheet from class on Monday also has to be completed if not done so in lesson. (Link to worksheet here if needed)
Due - Wednesday 11th November (Set 04/11/2015) - 2 pieces of h/wk
1. Page 67 in textbook - complete question 3 (if you want to push yourself, try 4 and 5 as well)
2. Copy out each definition 10 times each. (This is to help you learn the definitions word for word, so DO NOT write...
'Ionic
Ionic
Ionic' etc.
as it will not help you remember the definition and will be a waste of your time and not beneficial!
- Ionic bonding is the electrostatic attraction between positive and negative ions. It holds together cations and anions in ionic compounds.
- Covalent bonding – is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
- Dative covalent bond (or co-ordinate bond) is a covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only.
- Polar – with charges at different ends of the molecule caused by electronegative atoms
- Electronegative – a measure of the attraction of a bonded atom for the pair of electrons in a covalent bond.
- Salt – a product where the H+ ions in an acid are replaced by metal or ammonium ions.
- Base – a compound that neutralises an acid and acts as a proton acceptor.
- Acid – a species that donates/releases H+ ions in aqueous solution.
Due - 2nd November 2015
Get all your notes into a folder with dividers. (If you have TIZ for physics, you know what i am expecting!)
Due - Monday 19th October (Set 14/10/2015)
Complete past paper questions attached here. Can you also bring your test in (this counts as part of your homework - no test = 20 minutes) - we are going to keep these in your folders that stay here, along with the learning capability frameworks you just went through. Your re-take VIMA will be as soon as you get back after half term.
Due - Wednesday 14th October 2015 (Set 12/10/2015)
Fill in the front of your test paper, identifying your weak areas what what you will do to improve.
Due Wednesday 7th October 2015 (set 30/09/2015)
Complete past paper questions ready to mark on Wednesday morning. Link to worksheet here. All lesson resources and past worksheets and homeworks available from link at the top.
Due - Wednesday 30th September 2015 (set 23/09/2015)
Complete titration calculations worksheet, ready to mark on Wednesday morning.
(Link to worksheet here) If the class worksheet was not finished, this must also be completed for next lesson. Click on the Lesson Resources link at the top of the page to access the worksheet and class powerpoints.
Due - Wednesday 23rd September 2015 (Set 16/09/2015)
Complete these calculations on RAM (link to worksheet here); bring this in ready to mark on Wednesday morning.
Due - Wednesday 16th September 2015
Hand-write the following definitions 10 times each for next lesson:
Atomic (proton) number is the number of protons in the nucleus of an atom.
Mass number (nucleon) number is the number of particles (neutrons and protons) in the nucleus.
Relative Atomic Mass, Ar, is the weighted mean mass of an atom of an element compared with 1/12 of the mass of an atom of carbon-12.
Relative isotopic mass is the mass of an atom of an isotope compared with 1/12 of the mass of an atom of carbon-12.
Relative molecular mass, Mr, is the weighted mean mass of a molecule compared with 1/12 of the mass of an atom of carbon-12.
Relative formula mass, is the weighted mean mass of a formula unit compared with 1/12 of the mass of an atom of carbon-12.
