Year 13 Organic Summer questions	

	Name:	
________________________	

Class:	
________________________	

Date:	
________________________	

 	
Time:	76 minutes	
Marks:	73 marks	
Comments:		

Q1.
This question is about compounds of the elements in Period 3.
(a)     Phosphorus burns in air to form phosphorus(V) oxide.
Write an equation for this reaction.
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(1)
(b)     Sulfur forms two oxides, SO2 and SO3
Both oxides react with water to form acidic solutions.
State the formula of each acid formed and the approximate pH of a 0.1 mol dm–3 solution of each acid.
Formula of acid formed by SO2 __________________________________________
pH _____________________________________________
Formula of acid formed by SO3 __________________________________________
pH _____________________________________________
(2)
(c)     Aluminium oxide can act as an acid and can act as a base.
Write an equation to show aluminium oxide acting as an acid.
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(1)
(d)     Silicon reacts with oxygen to form SiO2 and with chlorine to form SiCl4
The table shows the melting points of SiO2 and SiCl4
 
Compound	Melting point / °C	
SiO2	1710	
SiCl4	–69	
Explain, in terms of structure and bonding, why SiO2 has a very high melting point but SiCl4 has a very low melting point.
SiO2 _______________________________________________________________
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SiCl4 ______________________________________________________________
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(4)
(Total 8 marks)
Q2.
Which statement about sulfur dioxide is correct?
 
A	It is an ionic compound.	 	
B	It is insoluble in water.	 	
C	It reacts with calcium hydroxide solution.	 	
D	It reacts with hydrochloric acid.	 	
(Total 1 mark)
Q3.
Which element could be sulfur?
 
 	Melting point of element	Solution of oxide	 	
A	high	acidic	 	
B	high	alkaline	 	
C	low	acidic	 	
D	low	alkaline	 	
(Total 1 mark)
Q4.
Which of these atoms has the largest atomic radius?
 
A	Ar		
B	Cl		
C	Mg		
D	Na		
(Total 1 mark)
Q5.
Which of these atoms has the highest electronegativity?
 
A	Na		
B	Mg		
C	Cl		
D	Ar		
(Total 1 mark)
Q6.
A propanedioate ion can act as a bidentate ligand.
The skeletal formula of a propanedioate ion is shown.

(a)     Give the meaning of the term bidentate ligand.
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(1)
(b)     Ni2+ ions form a complex ion Z that contains two propanedioate ligands and two water ligands.
Z exists as three stereoisomers. One of these stereoisomers is shown. The charge has not been shown.

Complete the diagrams of the other two stereoisomers of Z.
You do not need to include any charges on your diagrams.
For each stereoisomer, place one or more ticks in the boxes to identify the type or types of isomer shown.
 
 	cis	 	
	trans	 	
	optical	 	
 
 	cis	 	
	trans	 	
	optical	 	
(4)
(Total 5 marks)
Q7.
A solution containing EDTA4− ions is added to a solution containing [CuCl4]2− ions.
The EDTA4− ions replace the Cl− ligands in the copper complex to form [CuEDTA]2− ions.
Why does this reaction occur?
 
A	EDTA4− is more highly charged than Cl−	 	
B	EDTA4− is larger than Cl−	 	
C	The enthalpy change is positive.	 	
D	The entropy change is positive.	 	
(Total 1 mark)
Q8.
Which of the following is not able to act as a ligand?
 
A	Cl−	 	
B	CH3CH2CH3	 	
C	H2O	 	
D	H2NCH2CH2NH2	 	
(Total 1 mark)
Q9.
(a)     Explain how the electron pair repulsion theory can be used to deduce the shape of, and the bond angle in, PF3
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(6)
(b)     State the full electron configuration of a cobalt(II) ion.
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(1)
(c)     Suggest one reason why electron pair repulsion theory cannot be used to predict the shape of the [CoCl4]2− ion.
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(1)
(d)     Predict the shape of, and the bond angle in, the complex rhodium ion [RhCl4]2−.
Shape _____________________________________________________________
Bond angle _________________________________________________________
(2)
(Total 10 marks)
Q10.
This diagram represents the energy change that occurs when a d electron in a transition metal ion is excited by visible light.
 
(a)     Give the equation that relates the energy change ΔE to the Planck constant h and the frequency of the visible light v.
Use this equation and the information in the diagram to calculate a value for the frequency of the visible light, and state the units.
The Planck constant h = 6.63 × 10−34 J s.
Equation ___________________________________________________________
Calculation _________________________________________________________
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(2)
(b)     Explain why this electron transition causes a solution containing the transition metal ion to be coloured.
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(2)
(c)     The energy change shown in the diagram represents the energy of red light and leads to a solution that appears blue.
Blue light has a higher frequency than red light.
Suggest whether the energy change ΔE will be bigger, smaller or the same for a transition metal ion that forms a red solution. Explain your answer.
Energy change ______________________________________________________
Explanation _________________________________________________________
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(2)
(d)     State three different features of transition metal complexes that cause a change in the value of ΔE, the energy change between the ground state and the excited state of the d electrons.
Feature 1 ___________________________________________________________
Feature 2 ___________________________________________________________
Feature 3 ___________________________________________________________
(3)
(Total 9 marks)
Q11.
Ionisation energies provide evidence for the arrangement of electrons in atoms.
(a)     Complete the electron configuration of the Mg+ ion.
1s2 _______________________________________________________________
(1)
(b)     (i)      State the meaning of the term first ionisation energy.
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(2)
(ii)     Write an equation, including state symbols, to show the reaction that occurs when the second ionisation energy of magnesium is measured.
 
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(1)
(iii)     Explain why the second ionisation energy of magnesium is greater than the first ionisation energy of magnesium.
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(1)
(iv)    Use your understanding of electron arrangement to complete the table by suggesting a value for the third ionisation energy of magnesium.
 
 	First	Second	Third	Fourth	Fifth	
Ionisation energies of magnesium / kJ mol–1	736	1450	 	10 500	13 629	
						
(1)
(c)     State and explain the general trend in the first ionisation energies of the Period 3 elements sodium to chlorine.
Trend ______________________________________________________________
Explanation _________________________________________________________
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(3)
(d)     State how the element sulfur deviates from the general trend in first ionisation energies across Period 3. Explain your answer.
How sulfur deviates from the trend _______________________________________
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Explanation _________________________________________________________
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(3)
(e)     A general trend exists in the first ionisation energies of the Period 2 elements lithium to fluorine. Identify one element which deviates from this general trend.
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(1)
(Total 13 marks)
Q12.
Sodium, aluminium and silicon are solid elements with a silver colour. These elements react with oxygen to form oxides with high melting points. Aluminium is a reactive metal, but it resists corrosion in water because it has a surface coating of aluminium oxide.
(a)     In terms of its structure and bonding, explain why silicon dioxide has a high melting point.
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(3)
(b)     State the type of bonding in aluminium oxide.
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(1)
(c)     Write an equation for the reaction of aluminium with oxygen.
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(1)
(d)     Suggest one property of the aluminium oxide coating that causes aluminium to resist corrosion in water.
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(1)
(e)     Sodium metal is not resistant to corrosion in water, despite having a surface coating of sodium oxide. Write an equation to show how sodium oxide reacts with water.
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(1)
(f)      Aluminium oxide is amphoteric. It reacts with acids and alkalis.
(i)      Write an equation for the reaction between aluminium oxide and hydrochloric acid.
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(1)
(ii)     Write an equation for the reaction between aluminium oxide and an excess of aqueous sodium hydroxide.
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(1)
(g)     Silicon dioxide does not react with hydrochloric acid but it does react with sodium hydroxide. State one property of silicon dioxide that can be deduced from this information and write an equation for its reaction with sodium hydroxide.
Property ___________________________________________________________
Equation ___________________________________________________________
(2)
(Total 11 marks)
Q13.
The following diagram shows the first ionisation energies of some Period 3 elements.
 
(a)     Draw a cross on the diagram to show the first ionisation energy of aluminium.
(1)
(b)     Write an equation to show the process that occurs when the first ionisation energy of aluminium is measured.
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(2)
(c)     State which of the first, second or third ionisations of aluminium would produce an ion with the electron configuration 1s2 2s2 2p6 3s1
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(1)
(d)     Explain why the value of the first ionisation energy of sulfur is less than the value of the first ionisation energy of phosphorus.
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(2)
(e)     Identify the element in Period 2 that has the highest first ionisation energy and give its electron configuration.
Element ____________________________________________________________
Electron configuration _________________________________________________
(2)
(f)      State the trend in first ionisation energies in Group 2 from beryllium to barium.
Explain your answer in terms of a suitable model of atomic structure.
Trend ______________________________________________________________
Explanation _________________________________________________________
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(3)
(Total 11 marks)

Mark schemes
Q1.
(a)  P4 + 5O2 ⟶ P4O10
allow multiples or fractions
ignore state symbol
allow
4P + 5O2 ⟶ P4O10
reject any formula for phosphorous that is not P or P4
1
(b)  Formulae:
H2SO3 AND H2SO4
If no mark awarded then award 1 mark for correct formula and pH for one oxide
1
pH values
SO2 any in range 2 to 5
AND
SO3 any in range 0 to 1
1
(c)  Al2O3 + 2NaOH + 3H2O ⟶ 2NaAl(OH)4
ignore state symbols
Allow any of:
Al2O3 + 2OH− + 3H2O ⟶ 2Al(OH)4−
Al2O3 + 6OH− + 3H2O ⟶ 2Al(OH)63−
Al2O3 + 6NaOH + 3H2O ⟶ 2Na3Al(OH)6
Reject reactions with carbonates and hydrogen carbonates
1
(d)  M1 SiO2 giant (lattice) and covalent
Allow “macromolecular” for “giant lattice” and “giant covalent” for M1
1
M2 strong (covalent) bonds (between atoms) / require lots of energy to overcome − break
If SiO2 is not covalent, lose M2
1
M3 SiCl4 (simple) molecular
1
M4 weak forces between molecules / weak van der Waal’s forces / weak intermolecular forces
and
require little energy to overcome
if breaking covalent bonds in SiCl4 then do not award M4
1
If SiO2 stated as not covalent, do not award M1 or M2
If SiCl4 stated as not covalent, do not award M3 or M4
[8]
Q2.
C
[1]
Q3.
C
[1]
Q4.
D
[1]
Q5.
C
[1]
Q6.
(a)  M1 donates an electron pair (to a metal atom/ion) from two different atoms
1
(b)
 
1
 
cis	 	
trans	✓	
optical	 	
1
 
1
 
cis	✓	
trans	 	
optical	✓	
1
[5]
Q7.
D
[1]
Q8.
B
[1]
Q9.
(a)     This question is marked using levels of response. Refer to the Mark Scheme Instructions for Examiners for guidance on how to mark this question.
All stages are covered and the explanation of each stage is generally correct and virtually complete.
Answer is communicated coherently and shows a logical progression from stage 1 to stage 2 then stage 3.
Level 3
5 – 6 marks
All stages are covered but the explanation of each stage may be incomplete or may contain inaccuracies OR two stages are covered and the explanations are generally correct and virtually complete.
Answer is mainly coherent and shows progression from stage 1 to stage 3.
Level 2
3 – 4 marks
Two stages are covered but the explanation of each stage may be incomplete or may contain inaccuracies, OR only one stage is covered but the explanation is generally correct and virtually complete
Answer includes isolated statements but these are not presented in a logical order or show confused reasoning.
Level 1
1 – 2 marks
Insufficient correct chemistry to gain a mark.
Level 0
0 marks
Indicative chemistry content
Stage 1: Electrons round P
•        P has 5 electrons in the outside shell
•        With 3 electrons from 3 fluorine, there are a total of 8 electrons in outside shell
•        so 3 bond pairs, 1 non-bond pair
Stage 2: Electron pair repulsion theory
•        Electron pairs repel as far as possible
•        Lone pair repels more than bonding pairs
Stage 3: Conclusions
•        Therefore, tetrahedral / trigonal pyramidal shape
•        With angle of 109(.5)° decreased to 107°
6
(b)     1s22s22p63s23p63d7
Allow correct numbers that are not superscripted
1
(c)     Too many electrons in d sub-shell / orbitals
1
(d)     Tetrahedral (shape)
1
109.5°
Allow 109°
1
[10]
Q10.
(a)     ΔE = hv
Allow = hf
1
v = ΔE / h = 2.84 × 10−19 / 6.63 × 10−34 = 4.28 × 1014 s−1 / Hz
Allow 4.3 × 1014 s−1 / Hz
Answer must be in the range:
4.28 − 4.30 × 1014
1
(b)     (One colour of) light is absorbed (to excite the electron)
If light emitted, CE = 0
1
The remaining colour / frequency / wavelength / energy is transmitted (through the solution)
Allow light reflected is the colour that we see.
1
(c)     Bigger
1
Blue light would be absorbed
OR light that has greater energy than red light would be absorbed
OR higher frequency (of light absorbed / blue light) leads to higher ΔE
Can only score M2 if M1 is correct.
1
(d)     Any three from:
•         (Identity of the) metal
•         Charge (on the metal) / oxidation state / charge on complex
•         (Identity of the) ligands
•         Co-ordination number / number of ligands
•         Shape
3 max
[9]
Q11.
(a)     2s22p63s1
1s2 can be rewritten
Allow 2s22px22py22pz23s1
Allow subscripts and capitals
1
(b)     (i)      Energy/enthalpy (needed) to remove one mole of electrons
from one mole of atoms/compounds/molecules/elements
1
OR
Energy to form one mole of positive ions from one mole of atoms
OR
Energy/enthalpy to remove one electron from one atom
In the gaseous state (to form 1 mol of gaseous ions)
Energy given out loses M1
M2 is dependent on a reasonable attempt at M1
Energy needed for this change
X(g) → X+(g) + e(–) = 2 marks
This equation alone scores one mark
1
(ii)     Mg+(g) → Mg2+(g) + e(–)
Mg+(g) + e(–) → Mg2+(g) + 2e(–)
Mg+(g) – e(–) → Mg2+(g)
Do not penalise MG
Not equation with X
1
(iii)     Electron being removed from a positive ion (therefore need more
energy)/electron being removed is closer to the nucleus/Mg+
smaller (than Mg)/Mg+ more positive than Mg
Allow from a + particle/species
Not electron from a higher energy level/or higher sub-level
More protons = 0
1
(iv)    Range from 5000 to 9000 kJ mol–1
1
(c)     Increase
If decrease CE = 0/3
If blank mark on
1
Bigger nuclear charge (from Na to Cl)/more protons
QWC
1
electron (taken) from same (sub)shell/similar or same shielding/
electron closer to the nucleus/smaller atomic radius
If no shielding = 0
Smaller ionic radius = 0
1
(d)     Lower
If not lower CE = 0/3
If blank mark on
Allow does not increase
1
Two/pair of electrons in (3)p orbital or implied
Not 2p
1
repel (each other)
M3 dependent upon a reasonable attempt at M2
1
(e)     Boron/B or oxygen/O/O2
1
[13]
Q12.
(a)     Macromolecular
Or giant molecule
Or giant covalent (also gains M2)
Do not allow giant atomic
Ionic/metallic CE=0 for all 3 marks
1
Covalent bonding (between atoms)
Do NOT allow if between molecules
1
Many/strong bonds to be broken (or lots of energy required)
Lose both bonding marks if contradiction e.g. mention of intermolecular forces
Note: ‘covalent bonds between molecules’ loses M2 but not M3
1
(b)     Al2O3 ionic
Allow ionic + covalent/ionic with covalent character
1
(c)     2Al + 3/2O2 → Al2O3
Allow multiples
Ignore state symbols
1
(d)     Insoluble/impermeable/non-porous
Or does not react/inert
Do not allow thick layer
Must imply property of Al2O3 not Al
1
(e)     Na2O + H2O → 2NaOH
Or Na2O + H2O → 2Na+ + 2OH–
1
(f)      (i)      Al2O3 + 6HCl → 2AlCl3 + 3H2O
Ionic equations with Al2O3 possible
e.g. Al2O3 + 6H+ → 2Al3+ + 3H2O
Do not allow formation of Al2Cl6
1
(ii)     Al2O3 + 2NaOH + 3H2O → 2NaAl(OH)4
Other equations with Al2O3 are possible e.g.
Al2O3 + 2OH– + 3H2O → 2[Al(OH)4]–
Al2O3 + 2OH– + 7H2O → 2[Al(H2O)2(OH)4]–
1
(g)     SiO2 acidic/Lewis acid/electron pair acceptor
1
SiO2 + 2NaOH → Na2SiO3 + H2O
Allow SiO2 not amphoteric
Do NOT allow BL acid
Other equations with SiO2 are possible e.g. 
SiO2 + 2OH– → SiO32– + H2O 
SiO2 + 2OH– + 2H2O → Si(OH)62–
1
[11]
Q13.
(a)     Cross between the Na cross and the Mg cross
1
(b)     Al(g) → Al+(g) + e–
Al(g) – e– → Al+(g)
Al(g) + e– → Al+(g) + 2e–
One mark for state symbols consequential on getting equation correct.
Electron does not have to have the – sign on it
Ignore (g) if put as state symbol with e– but penalise state symbol mark if other state symbols on e–
2
(c)     2nd/second/2/II
Only
1
(d)     Paired electrons in (3)p orbital
Penalise wrong number
If paired electrons repel allow M2
1
repel
1
(e)     Neon/Ne
No consequential marking from wrong element
1
1s22s22p6/[He}2s22p6
Allow capital s and p
Allow subscript numbers
1
(f)      Decreases
CE if wrong
1
Atomic radius increases/electron removed further from nucleus
or nuclear charge/electron in higher energy level/Atoms
get larger/more shells
Accept more repulsion between more electrons for M2
Mark is for distance from nucleus
Must be comparative answers from M2 and M3
CE M2 and M3 if mention molecules
Not more sub-shells
1
As group is descended more shielding
1
[11]