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a)
The successive ionisation energies of vanadium are shown.
State the sub-levels from which each of the first four electrons are lost
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b)
Outline why there is an increase in ionisation energy from electron 3 to electron 5.
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c)
Explain why there is a large increase in the ionisation energy between electrons 5 and 6.
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d)
The first six ionisation energies, in kJ mol-1 , of an element are shown below
IE 1
IE 2
IE 3
IE 4
IE 5
IE 6
578
1816
2744
11576
14829
18375
Explain the large increase in ionisation energy from
IE 3 to
IE 4
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a)
When chromium(III) sulfate dissolves in water, a green solution containing the [Cr(H 2 O) 6 ] 3+ ion forms.
i)
State the bond angles found in this complex ion.
[1]
ii)
Explain why the chromium(III) complex ion is coloured.
[3]
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b)
Vanadium(V) oxide is the catalyst used in the Contact process as shown by the reactions:
SO 2 (g) + V 2 O 5 (s) → SO 3 (g) + V 2 O 4 (s)
V 2 O 4 (s) + ½O 2 (g) → V 2 O 5 (s)
i) Explain, using the equations, why V 2 O 5 is a catalyst.
[1]
ii) Explain why V 2 O 5 can act as a catalyst in this reaction.
[1]
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c)
Excess ammonia is added to a solution of Cu2+ ions resulting in the substitution of 4 ligands.
Using section 15 of the data booklet, explain why this reaction results in a shift in the wavelength of light absorbed by the Cu2+ complex.
[1]
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a)
Ibuprofen is a common non-steroidal anti-inflammatory drug (NSAID). It contains a benzene ring and a carboxylic acid at the end of one of the branches.
Deduce the number of resonance structures possible in the deprotonated form of ibuprofen.
[1]
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b)
Deduce the number of:
i)
Sigma (σ) bonds in ibuprofen
[1]
ii)
Pi (π) electrons in ibuprofen
[1]
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c)
The ibuprofen molecule contains both sp3 and sp2 hybridised orbitals.
i)
Identify how many sp3 hybrid orbitals are present.
[1]
ii)
Identify how many sp2 hybrid orbitals are present.
[1]
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d)
Explain why the benzene ring is a regular, planar hexagon.
[3]
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a)
State the formula for calculating the standard enthalpy change of reaction, ΔH r , using bond energies.
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b)
Use section 11 of the data booklet to calculate the enthalpy change, in kJ mol-1 , for the following reaction.
Cl2 + H2 → 2HCl
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c)
State whether the energy change for the reaction in part (b) is endothermic or exothermic.
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d)
Using section 11 of the data booklet, calculate the enthalpy change of reaction, ΔHr , in kJ mol-1 for the following reaction.
CH4 + Cl2 → CH3 Cl + HCl
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a)
A student measured the energy change when 1.35 g of zinc was added to 50 cm
3 of 0.5 mol dm
-3 copper sulfate, CuSO
4 (aq), solution. The initial temperature of 21
o C was recorded before the addition of the zinc and a temperature reading was taken every 30 seconds.
Use the graph to determine the overall temperature change for the reaction
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b)
Calculate the enthalpy change for the reaction in kJ mol-1 .
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c)
Calculate the percentage error between your value for the enthalpy change of reaction and the literature value of -217 kJ mol-1 . Give your answer to two significant figures.
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d)
Explain why your calculated value for the enthalpy change of reaction is different from the literature value of -271 kJ mol-1 .
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a)
Define the term nucleophile .
[2]
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b)
Explain why the hydroxide ion, OH- , is a stronger nucleophile than water.
[2]
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c)
State the two ways a nucleophilic substitution reaction can occur.
[1]
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d)
State the the name of the mechanism occurring in the image below which will form ethanol in one step.
[1]
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a)
Ethane-1,2-diol, C2 H6 O2 , can be distinguished from ethanedioic acid,C2 H2 O4 , by a number of analytic techniques including MS, IR and NMR
The MS of these molecules is shown below.
Which spectrum belongs to each molecule? Justify your answer.
Spectrum A
Spectrum B
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b)
The IR spectra of ethane-1,2-diol, C2 H6 O2 , and ethanedioic acid dihydrate,C2 H2 O4 .2H2 O, are shown in spectrum C and D . Use Section 26 of the Data Booklet to answer this question.
Spectrum C Spectrum D
Which spectrum belongs to each molecule? Justify your answer.
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c)
The 1 H NMR spectrum of ethane-1,2-diol is shown in spectrum E . Explain the significance of the spectrum.
Spectrum E
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d)
Suggest two modifications to the procedure which would make the result more reliable.
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