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Assessment formats: do they make a difference?
Eleni Danili and Norman Reid
Appendix 1
Test 1: Atomic Structure-Classification of Matter
Section 1. Each question has only ONE correct answer. Tick the answer that you think is correct.
1. What would be the volume in litres of 240g of oil if the density of the oil were 0.8 g/mL? ! 300L ! 0.3L ! 192L ! 0.19L
Discrimination index: 0.
2. Which one of the following represents correctly the electrical charges of the three basic particles, which make up atoms? proton neutron electron ! +1 0 + ! +1 0 - ! 0 0 + ! +1 +1 -
Discrimination index: 0.
3. An atom of element X contains 13 protons and 14 neutrons. Which of the following correctly represents this?
!
14 13 X
!
27 14 X
!
27 13 X
!
13 27 X
Discrimination index: 0.
4. The two isotopes of carbon
12 6 C^ and
14 6 C^ , differ from each other in: ! mass number ! atomic number ! chemical properties ! number of electrons
Discrimination index: 0.
5. The atomic number of potassium is 19 and its relative atomic mass is 39. Which one of the following represents correctly the atomic particles found in the K +^ ion: ! 19 protons 20 neutrons 19 electrons ! 19 protons 20 neutrons 18 electrons
! 20 protons 19 neutrons 20 electrons ! 20 protons 19 neutrons 18 electron
Discrimination index: 0.
6. When a magnet is passed over a sample of powdered metal, some of the sample is attracted to the magnet and some is not. The powdered metal sample is: ! a single element ! pure substance ! homogeneous mixture ! heterogeneous mixture
Discrimination index: 0.
7. Which one of the following is usually described as a ‘physical change’?
! the burning of magnesium in air ! the rusting of iron ! the evaporation of alcohol ! the rotting of an apple
Discrimination index: 0.
8. Which of the following involves at least one ‘chemical change’? ! the burning of wood ! converting water to steam in an electric kettle ! producing salt from sea water by evaporation ! sublimation of iodine
Discrimination index: 0.
9. Which of the following is a pure substance?
! air ! milk ! carbon dioxide ! rain
Discrimination index: 0.
10. The solubility of AgCl in water is:
! the minimum mass of water which can dissolve in a given mass of AgCl at fixed temperature ! the maximum mass of AgCl which can be dissolved in water at a fixed temperature ! the mass of AgCl can be dissolved in a given mass of water at a fixed temperature ! the maximum mass of Ag Cl can be dissolved in given mass of water at a fixed temperature
Discrimination index: 0.
11. The solubility of a gas in a liquid
! increases as the temperature of the solution is increased. ! increases as pressure of the gas at the surface is increased. ! increases as the volume of the solution is increased. ! decreases as pressure of the gas at the surface is increased.
(iii) The mass of crystals that would form if a solution containing 60g of potassium nitrate in 100g of water were cooled from 60 ˚C to 20 ˚C.
Appendix 2
Test 2: Periodic Table - Chemical bonds
Section 1
1. You are given the following elements with atomic numbers: 7, 12, 18, 38, 54. Which of them have similar properties? Explain your answer:
2. Two elements, X and Y, each forms a compound with chlorine. The chloride of X is a solid whose solution in water has a high conductivity. The chloride of Y is a liquid, which does not conduct electricity. (a) To which main group of the periodic table is X likely to belong? (b) Explain your answer. (c) To which main group of the periodic table is Y likely to belong? (d) Explain your answer. 3. What do the following have in common? (^) 10Ne, (^) 9F-^ , (^) 12Mg2+
Section 2
4. Each box in the grid below refers to an element. Look at the boxes and answer the questions that follow. (Boxes may be used as many times as you wish)
A The element with electron arrangement: 2.8.
B
Sodium
C
Ar
D
Magnesium
E
The element which is a brown liquid at room temperature
F
The elements which has 1 electron in each atom G The element of atomic number 19
H
Chlorine
L
Nitrogen
Select the box (es) which contain:
(a) Elements in the same group of the periodic table. (b) Elements that are gases in room temperature. (c) Atoms of which element (or elements) form ions with the same electron arrangement as argon atoms.
(d) Two elements that will combine to form an ionic compound with the formula X 3 Y 2. (e) Elements that form a covalent compound with the element that is in the box F.
Appendix 3
Test 3: Mole
Section 1
1. We have two balloons which when they are empty are identical in weight. The first is filled with 1 mol of oxygen (O 2 ). The second is filled with 2 mol of methane (CH 4 ). (Relative atomic mass: O =16, C = 12, H=1)
(a) Work out the formula mass of each substance and find out which balloon now weighs more: (b) Which balloon has the bigger volume under STP condition? Explain your answer.
Section 2
2. Look at the boxes and answer the following questions. Each question may have more than one answer. (Boxes may be used as many times as you wish). (Ar = 40, N = 14, C = 12, O = 16)
A. B. C. 2NA 56g 22.4l molecules (STP conditions) D. E. F. 44g 2mol NA molecules G. H. I. 44.8l 28g 22g (STP conditions)
(a) Pick the box (es) which contain mass of 1mole of CO 2. (b) Pick the box(es) which contain the same amount of N 2 as the one that is in the box B.
Discrimination index: 0.
- Which compound would produce an acidic solution when dissolved in water? ! Potassium oxide ! Sodium oxide ! Sulphur dioxide ! Sodium bromide
Discrimination index: 0.
- Which pair of chemical could you use to make lead sulphate? (Use information given at the end of the test for the solubility of some compounds) ! Lead nitrate and barium sulphate ! Lead nitrate and sodium sulphate ! Lead phosphate and sodium sulphate ! Lead phosphate and barium sulphate
Discrimination index: 0.
The reaction between copper oxide and nitric acid is given below CuO + HNO 3! Cu(NO 3 ) 2 + H 2 O
The correct balanced equation is: ! CuO + H 2 NO 3! Cu(NO 3 ) 2 + H 2 O ! CuO + 2HNO 3! Cu(NO 3 ) 2 + H 2 O ! CuO + HNO 3! Cu(NO 3 ) 2 + H 2 O ! 2CuO + 2HNO 3! Cu(NO 3 ) 2 + H 2 O
Discrimination index: 0.
- Which is the balanced equation for the reaction of barium chloride solution with zinc sulphate solution? ! BaCl 2 + ZnSO 4! BaSO 4 + ZnCl 2 ! 2BaCl + ZnSO 4! Ba 2 SO 4 + 2ZnCl ! BaCl 2 + Zn 2 SO 4! BaSO 4 + 2ZnCl ! 2BaCl 2 + Zn 2 SO 4! Ba 2 SO 4 + 2ZnCl (^2)
Discrimination index: 0.
- When sodium reacts with water the products made are:
! a salt and hydrogen ! an alkaline solution and hydrogen ! an alkaline oxide and hydrogen ! an acid and hydrogen
Discrimination index: 0.
- Which of the following metals will react with the given solutions?
! Cu and Fe(NO 3 ) (^2) ! Fe and Cu(NO 3 ) (^2) ! Zn and MgCl 2 ! Ag and HCl
Discrimination index: –0.
- CaCl 2 dissolves in water. Which of the following statements is correct:
! The number of cations and anions are the same ! The number of cations are double of the number of anions ! The number of anions are double of the number of cations ! There are no anions and cations because it has a pH= 7
Discrimination index: 0.
Section 2
- Look at the boxes and answer the following questions. Each question may have more than one answer. (You may use the box as many times as you wish)
A
Contains same number of hydrogen ions, H+(aq), and hydroxide ions, OH-
B
It reacts with calcium carbonate and gives carbon dioxide gas
C
It turns universal indicator blue
D
It turns universal indicator red
E
It reacts with hydrochloric acid and gives a salt
F
It forms compounds called chlorides
G
It conducts electricity
H
It contains many hydroxide ions
I
It has a pH less than 7
Select the box(es) which contain statements which are true about: (a) Hydrochloric acid solution (b) Sodium hydroxide solution (c) Sodium chloride solution
- Look at the boxes and answer the following questions. Each question may have more than one answer. (You may use the box as many times as you wish)
A
Sodium Oxide Na (^) 2O
B
Lead Nitrate Pb(NO 3 ) (^2)
C
Phosphorus Trioxide P (^) 2O (^3) D Barium Iodide BaI (^2)
E
Calcium Oxide CaO
F
Sodium Nitrate Na(NO (^) 3) (^2) G Sulphur Dioxide SO (^2)
H
Magnesium Sulphate MgSO (^4)
L
Nitrogen Dioxide NO (^2)
! Doubled ! Not changed ! Quadrupled ! Halved
- In a beaker, A, we have dissolved 0.2mole of NaCl in 200ml of water. In another beaker, B, we have dissolved 0.4mol of NaCl in 400ml water. Which of the following statements is correct: ! The solution in the beaker A has smaller concentration than the solution in beaker B ! The solution in the beaker A has the same concentration as the solution in the beaker B ! The solution in the beaker B has smaller concentration than the beaker A ! The solution in the beaker B has double concentration of the solution in the beaker A.
- You want to prepare 4l of a solution of potassium hydroxide with concentration 0.1mol/l. For this purpose you will use: ! 0.1moles KOH ! 1 moles KOH ! 0.4moles KOH ! 4 moles KOH
- One pupil has mixed together two solutions of Na 2 CO 3 with concentrations of 0.1 mol/l and 0.5mol/l respectively. The possible concentration of the new solution is: ! 0.01mol/l ! 0.6mol/l ! 0.1mol/l ! 0.3mol/l
- You prepared a NaCl solution by adding 1mole (58.44g) of NaCl to a 1-litre volumetric flask and then added water to dissolve it. When you have finished, the final volume in your flask looked like figure 1
The solution you prepared is
! Greater than 1mol/l because you added more solvent than necessary ! Less than 1mol/l because you added more solvent than necessary ! Less than 1mol/l because you added less solvent than necessary ! 1mol/l because the amount of solute, not solvent determines the concentration
Section 2
- Each box in the grid below represents beakers with aqueous solution of NaOH. Look at the boxes and answer the following questions. Each question may have more than one answer. (Boxes my be used as many times as you wish)
A B C
D E F
500 ml (^) 250 ml 250 ml
500 ml (^) 250 ml 500 ml
(a) Which solution is most concentrated? (b) Which solution is least concentrated? (c) When solutions B and E are combined, the resulting solution has the same concentration as solution: (d) Which solutions have the same concentration? (e) If you evaporate half of the water from solution D, the resulting solution will have the same concentration as solution:
Section 3
- The concentration of the acid in a bottle is shown on the label as 0.5M (a) Explain what this means. (b) How many moles of sulphuric acid would you need to use to make 2 litre of a solution with the same concentration as in the bottle above? (c) If you add water to the 2 litre solution until the final volume is 4litre, what is the new concentration of the solution:
