Q1.
Which of these atoms has the smallest number of neutrons?
 
A	3H		
B	4He		
C	5He		
D	4Li		
(Total 1 mark)
Q2.
Which one of the following lists the first ionisation energies (in kJ mol−1) of the elements Mg, Al, Si, P and S in this order?
 
A	577	786	1060	1000	1260	
B	736	577	786	1060	1000	
C	786	1060	1000	1260	1520	
D	1060	1000	1260	1520	418	
(Total 1 mark)
Q3.
Which one of the following is the electronic configuration of an element with a maximum oxidation state of +5?
A       1s2 2s2 2p5
B       1s2 2s2 2p6 3s2 3p1
C       1s2 2s2 2p6 3s2 3p3
D       1s2 2s2 2p6 3s2 3p6 3d7 4s2
(Total 1 mark)
Q4.
In which one of the following pairs is the first ionisation energy of element Y greater than that of element X?
 
 	electronic configuration
of element X	electronic configuration
of element Y	
A	1s1	ls2	
B	1s2 2s2	ls22s2 2p1	
C	1s2 2s22p3	ls22s22p4	
D	1s2 2s22p6	ls22s22p6 3s1	
(Total 1 mark)
Q5.
The successive ionisation energies for element X are shown in the following graph.
 
Which element is X?
 
A	Nitrogen		
B	Phosphorus		
C	Aluminium		
D	Boron		
(Total 1 mark)
Q6.
Which one of the following ionisations requires less energy than the first ionisation energy of oxygen?
A       S(g) → S+(g) + e−
B       O+(g) → O2+(g) + e−
C       N(g) → N+(g) + e−
D       F(g) → F+(g) + e−
(Total 1 mark)
Q7.
Which one of the following atoms has only two unpaired electrons in its ground (lowest energy) state?
A       helium
B       beryllium
C       nitrogen
D       oxygen
(Total 1 mark)
Q8.
Assuming that chlorine exists as two isotopes, and that hydrogen and carbon exist as one isotope each, how many molecular ion peaks will be shown in the mass spectrum of C4H6Cl4?
A       2
B       3
C       4
D       5
(Total 1 mark)
Q9.
Which one of the following does not have a pair of s electrons in its highest filled electron energy sub-level?
A       H−
B       Mg
C       P3+
D       Ar
(Total 1 mark)
Q10.
Ions of two isotopes of iron are
53Fe2+               56Fe2+
Which statement is correct?
 
A	The ions of both the isotopes have the electronic configuration 1s22s22p63s23p64s23d6		
B	The ions of both the isotopes contains 26 neutrons		
C	53Fe2+ has fewer protons than 56Fe2+		
D	After acceleration to the same kinetic energy 56Fe2+ will move more slowly than 53Fe2+		
(Total 1 mark)
Q11.
Bromine exists as two isotopes 79Br and 81Br, which are found in almost equal abundance.
Which of the statements is correct?
 
A	The first ionisation energy of 79Br is less than the first ionisation energy of 81Br		
B	The atomic radius of 79Br is less than the atomic radius of 81Br		
C	The mass spectrum of C3H7Br has two molecular ion peaks at 122 and 124		
D	79Br is more reactive than 81Br		
(Total 1 mark)
Q12.
Which of these elements has the highest second ionisation energy?
 
A	Na		
B	Mg		
C	Ne		
D	Ar		
(Total 1 mark)
Q13.
Which one of the following statements is correct?
A       The first ionisation energies of the elements in Period 3 show a general decrease from sodium to chlorine.
B       The electronegativities of Group 2 elements decrease from magnesium to barium.
C       The strength of the intermolecular forces increases from hydrogen fluoride to hydrogen chloride.
D       The ability of a halide ion to act as a reducing agent decreases from fluoride to iodide.
(Total 1 mark)
Q14.
Which is the correct classification for the element yttrium (Y)?
 
A	s block		
B	p block		
C	d block		
D	f block		
(Total 1 mark)
Q15.
Which of the following is a correct statement about the trend in atomic radius across Period 3 of the Periodic Table?
 
A	radius increases because the atoms have more electrons		
B	radius decreases because nuclear charge increases		
C	radius increases because shielding (screening) increases		
D	radius decreases because shielding (screening) decreases		
(Total 1 mark)
Q16.
Chlorine has two isotopes, 35Cl and 37Cl. The number of molecular ion peaks in the mass spectrum of a sample of Cl2 is
A       2
B       3
C       4
D       5
(Total 1 mark)
Q17.
Photochromic glass contains silver ions and copper ions. A simplified version of a redox equilibrium is shown below. In bright sunlight the high energy u.v. light causes silver atoms to form and the glass darkens. When the intensity of the light is reduced the reaction is reversed and the glass lightens.
Cu+(s) + Ag+(s)  Cu2+(s) + Ag(s)
clear glass          dark glass
Which one of the following is a correct electron arrangement?
A       Cu+ is [Ar]3d94s1
B       Cu is [Ar]3d104s2
C       Cu2+ is [Ar]3d84s1
D       Cu+ is [Ar]3d10
(Total 1 mark)
Q18.
The mass spectrum of the isotopes of element X is shown in the diagram.
 
m / z
(a)     Define the term relative atomic mass.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(b)     Use data from the diagram to calculate the relative atomic mass of X.
Give your answer to one decimal place.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(3)
(c)     Identify the ion responsible for the peak at 72
___________________________________________________________________
(1)
(d)     Identify which one of the isotopes of X is deflected the most in the magnetic field of a mass spectrometer. Give a reason for your answer.
Isotope ____________________________________________________________
Reason ____________________________________________________________
(2)
(e)     In a mass spectrometer, the relative abundance of each isotope is proportional to the current generated by that isotope at the detector.
Explain how this current is generated.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(f)     X and Zn are different elements.
Explain why the chemical properties of 70X and 70Zn are different.
___________________________________________________________________
___________________________________________________________________
(1)
Q19.
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.
___________________________________________________________________
(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
___________________________________________________________________
(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.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(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 _________________________________________________________
___________________________________________________________________
___________________________________________________________________
Q20.
(a)     Use your knowledge of electron configuration and ionisation energies to answer this question. The following diagram shows the second ionisation energies of some Period 3 elements.
 
(i)      Draw an ‘X’ on the diagram to show the second ionisation energy of sulfur.
(1)
(ii)     Write the full electron configuration of the Al2+ ion.
______________________________________________________________
(1)
(iii)    Write an equation to show the process that occurs when the second ionisation energy of aluminium is measured.
______________________________________________________________
(1)
(iv)    Give one reason why the second ionisation energy of silicon is lower than the second ionisation energy of aluminium.
______________________________________________________________
______________________________________________________________
______________________________________________________________
(1)
(b)     Predict the element in Period 3 that has the highest second ionisation energy.
Give a reason for your answer.
Element ____________________________________________________________
Reason ____________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(c)     The following table gives the successive ionisation energies of an element in Period 3.
 
 	First	Second	Third	Fourth	Fifth	Sixth	
Ionisation energy / kJ mol−1	786	1580	3230	4360	16100	19800	
Identify this element.
___________________________________________________________________
(1)
(d)     Explain why the ionisation energy of every element is endothermic.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(Extra space) ________________________________________________________
___________________________________________________________________
(1)
(Total 8 marks)
Q21.
(a)     Complete the following table.
 
Particle	Relative charge	Relative mass	
Proton	 	 	
Neutron	 	 	
Electron	 	 	
(3)
(b)     An atom of element Z has two more protons and two more neutrons than an atom of . Give the symbol, including mass number and atomic number, for this atom of Z.
___________________________________________________________________
(2)
(c)     Complete the electronic configurations for the sulphur atom, S, and the sulphide ion, S2–.
S       1s2 ___________________________________________________________
S2–     1s2 ___________________________________________________________
(2)
(d)     State the block in the Periodic Table in which sulphur is placed and explain your answer.
Block ______________________________________________________________
Explanation _________________________________________________________
(2)
(e)     Sodium sulphide, Na2S, is a high melting point solid which conducts electricity when molten. Carbon disulphide, CS2, is a liquid which does not conduct electricity.
(i)      Deduce the type of bonding present in Na2S and that present in CS2
Bonding in Na2S ________________________________________________
Bonding in CS2 _________________________________________________
(ii)     By reference to all the atoms involved explain, in terms of electrons, how Na2S is formed from its atoms.
______________________________________________________________
______________________________________________________________
(iii)     Draw a diagram, including all the outer electrons, to represent the bonding present in CS2

 
(iv)    When heated with steam, CS2 reacts to form hydrogen sulphide, H2S, and carbon dioxide.
Write an equation for this reaction.
______________________________________________________________
(7)
(Total 16 narks)
Q22.
(a)     (i)      Complete the electronic configuration of aluminium.
1s2 ___________________________________________________________
(ii)     State the block in the Periodic Table to which aluminium belongs.
______________________________________________________________
(2)
(b)     Describe the bonding in metals.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(c)     Explain why the melting point of magnesium is higher than that of sodium.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(3)
(d)     Explain how metals conduct electricity.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
Q23.
The mass spectrum of a sample of krypton taken from a meteorite is shown below.
 
(a)     Use this spectrum to calculate the relative atomic mass of this sample of krypton.
Give your answer to one decimal place.
Explain why the value you have calculated is slightly different from the relative atomic mass given in the Periodic Table.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
 (4)
(b)     State how krypton is ionised in the mass spectrometer.
Write an equation, including state symbols, to show the reaction that occurs when the first ionisation energy of Kr is measured.
Sometimes the mass spectrum of Kr has a very small peak with an m/z value of 42.
Explain the occurrence of this peak.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
 (5)
(Total 9 marks)
Q24.
This question is about Period 3 of the Periodic Table.
(a)     Deduce which of Na+ and Mg2+ is the smaller ion.
Explain your answer.
Smaller ion _________________________________________________________
Explanation _________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(b)     Write an equation to represent the process that occurs when the first ionisation energy for sodium is measured.
___________________________________________________________________
(1)
(c)     The first ionisation energies of some Period 3 elements are shown in the following graph.
 
Complete the graph by plotting the approximate first ionisation energy values for magnesium and sulfur.
Explain why the first ionisation energy of sulfur is different from that of phosphorus.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(4)
(Total 7 marks)
Q25.
The diagram below shows the values of the first ionisation energies of some of the elements in Period 3.
 
(a)     On the above diagram, use crosses to mark the approximate positions of the values of the first ionisation energies for the elements Na, P and S. Complete the diagram by joining the crosses.
(3)
(b)     Explain the general increase in the values of the first ionisation energies of the elements Na–Ar.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(3)
(c)     In terms of the electron sub-levels involved, explain the position of aluminium and the position of sulphur in the diagram.
Explanation for aluminium ______________________________________________
___________________________________________________________________
___________________________________________________________________
Explanation for sulphur ________________________________________________
___________________________________________________________________
___________________________________________________________________
(4)
(Total 10 marks)
Q26.
(a)     State the meaning of the term electronegativity.
___________________________________________________________________
___________________________________________________________________
(2)
(b)     State and explain the trend in electronegativity values across Period 3 from sodium to chlorine.
Trend ______________________________________________________________
Explanation _________________________________________________________
(3)
(c)     What is meant by the term first ionisation energy?
___________________________________________________________________
___________________________________________________________________
(2)
(d)     The diagram below shows the variation in first ionisation energy across Period 3.

(i)      What is the maximum number of electrons that can be accommodated in an s sub-level?
______________________________________________________________
______________________________________________________________
(ii)     What evidence from the diagram supports your answer to part (d)(i)?
______________________________________________________________
______________________________________________________________
(iii)     What evidence from the diagram supports the fact that the 3p sub-level is higher in energy than the 3s?
______________________________________________________________
______________________________________________________________
(iv)    What evidence from the diagram supports the fact that no more than three unpaired electrons can be accommodated in the 3p sub-level?
______________________________________________________________
______________________________________________________________
______________________________________________________________
(5)
(Total 12 marks)
Q27.
(a)     Explain why the atomic radii of the elements decrease across Period 3 from sodium to chlorine.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(b)     Explain why the melting point of sulfur (S8) is greater than that of phosphorus (P4).
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(c)     Explain why sodium oxide forms an alkaline solution when it reacts with water.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(d)     Write an ionic equation for the reaction of phosphorus(V) oxide with an excess of sodium hydroxide solution.
___________________________________________________________________
(1)
(Total 7 marks)
Q28.
(a)    State the meaning of the term mass number of an isotope.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(1)
(b)     Give the symbol of the element that has an isotope with a mass number of 68 and has 38 neutrons in its nucleus.
___________________________________________________________________
(1)
(c)     The following shows a simplified diagram of a mass spectrometer.

(i)      State what happens to the sample in the parts labelled P and Q.
P ____________________________________________________________
Q ____________________________________________________________
(2)
(ii)     In a mass spectrometer, the isotopes of an element are separated.
Two measurements for each isotope are recorded on the mass spectrum.
State the two measurements that are recorded for each isotope.
Measurement 1 _________________________________________________
Measurement 2 _________________________________________________
(2)
(d)     A sample of element R contains isotopes with mass numbers of 206, 207 and 208 in a 1:1:2 ratio of abundance.
(i)      Calculate the relative atomic mass of R. Give your answer to one decimal place.
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
(3)
(ii)     Identify R.
______________________________________________________________
(1)

(iii)    All the isotopes of R react in the same way with concentrated nitric acid.
State why isotopes of an element have the same chemical properties.
______________________________________________________________
______________________________________________________________
 (1)
(Total 11 marks)
Q29.
This question is about electron configuration.
(a)     Give the full electron configuration of an Al atom and of a Cr3+ ion.
Al atom ____________________________________________________________
Cr3+ ion ____________________________________________________________
(2)
(b)     Deduce the formula of the ion that has a charge of 2+ with the same electron configuration as krypton.
___________________________________________________________________
(1)
(c)     Deduce the formula of the compound that contains 2+ ions and 3− ions that both have the same electron configuration as argon.
___________________________________________________________________
(1)
(Total 4 marks)
Q30.
The manufacturer supplying concentrated ethanoic acid for the production of vinegar also supplied other acids. The label had come off a batch of one of these other acids. 
A sample of this unknown acid was analysed and found to contain 54.5% of carbon and 9.10% of hydrogen by mass, the remainder being oxygen.
(a)     Use these data to calculate the empirical formula of the unknown acid. 
Show your working.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(3)

(b)     A sample of the unknown acid was analysed in a mass spectrometer. The mass spectrum obtained is shown below.
 
Use the mass spectrum to determine the Mr of the unknown acid.
___________________________________________________________________
(1)
(c)     Use your answers from parts (a) and (b) to determine the molecular formula of the unknown acid. 
(If you could not answer part (b), you should assume that the Mr of the acid is 132.0 but this is not the correct value.)
Show your working.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(Total 6 marks)
Q31.
This question is about the first ionisation energies of some elements in the Periodic Table.
(a)     Write an equation, including state symbols, to show the reaction that occurs when the first ionisation energy of lithium is measured.
___________________________________________________________________
(1)
(b)     State and explain the general trend in first ionisation energies for the Period 3 elements aluminium to argon.
Trend _____________________________________________________________
Explanation _________________________________________________________
___________________________________________________________________
___________________________________________________________________
 (3)

(c)     There is a similar general trend in first ionisation energies for the Period 4 elements gallium to krypton.
State how selenium deviates from this general trend and explain your answer.
How selenium deviates from this trend ____________________________________
Explanation _________________________________________________________
___________________________________________________________________
___________________________________________________________________
 (3)
(d)     Suggest why the first ionisation energy of krypton is lower than the first ionisation energy of argon.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(1)
(e)     The table below gives the successive ionisation energies of an element.
 
 	First	Second	Third	Fourth	Fifth	
Ionisation energy / kJ mol–1	590	1150	4940	6480	8120	
						
Deduce the group in the Periodic Table that contains this element.
___________________________________________________________________
(1)
(f)      Identify the element that has a 5+ ion with an electron configuration of
1s2 2s2 2p6 3s2 3p6 3d10
___________________________________________________________________
(1)
(Total 10 marks)
Q32.
(a)    Table 1 shows some data about fundamental particles in an atom.
Table 1	
Particle	proton	neutron	electron	
Mass / g	1.6725 × 10–24	1.6748 × 10–24	0.0009 × 10–24	
(i)      An atom of hydrogen can be represented as 1H
Use data from Table 1 to calculate the mass of this hydrogen atom.
______________________________________________________________
(1)

(ii)     Which one of the following is a fundamental particle that would not be deflected by an electric field?
A     electron
B     neutron
C     proton
Write the correct letter, A, B or C, in the box.
 
(1)
(b)     A naturally occurring sample of the element boron has a relative atomic mass of 10.8.
In this sample, boron exists as two isotopes, 10B and 11B
(i)      Calculate the percentage abundance of 10B in this naturally occurring sample of boron.
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
(2)
(ii)     State, in terms of fundamental particles, why the isotopes 10B and 11B have similar chemical reactions.
______________________________________________________________
______________________________________________________________
______________________________________________________________
(1)
(c)    Complete Table 2 by suggesting a value for the third ionisation energy of boron.
Table 2	
 	First	Second	Third	Fourth	Fifth	
Ionisation energy / kJ mol–1	799	2420	 	25 000	32 800	
(1)
(d)     Write an equation to show the process that occurs when the second ionisation energy of boron is measured. Include state symbols in your equation.
___________________________________________________________________
(1)
(e)     Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron.
___________________________________________________________________
Q33.
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.
______________________________________________________________
______________________________________________________________
______________________________________________________________
(2)
(ii)     Write an equation, including state symbols, to show the reaction that occurs when the second ionisation energy of magnesium is measured.
 
______________________________________________________________
(1)
(iii)     Explain why the second ionisation energy of magnesium is greater than the first ionisation energy of magnesium.
______________________________________________________________
______________________________________________________________
______________________________________________________________
(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 _________________________________________________________
___________________________________________________________________
___________________________________________________________________
(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 _______________________________________
___________________________________________________________________
Explanation _________________________________________________________
___________________________________________________________________
___________________________________________________________________
(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.
___________________________________________________________________
(1)
(Total 13 marks)
Q34.
(a)     P and Q are oxides of Period 3 elements.
Oxide P is a solid with a high melting point. It does not conduct electricity when solid but does conduct when molten or when dissolved in water. Oxide P reacts with water forming a solution with a high pH.
Oxide Q is a colourless gas at room temperature. It dissolves in water to give a solution with a low pH.
(i)      Identify P. State the type of bonding present in P and explain its electrical conductivity. Write an equation for the reaction of P with water.
(ii)     Identify Q. State the type of bonding present in Q and explain why it is a gas at room temperature. Write an equation for the reaction of Q with water.
(9)
(b)     R is a hydroxide of a Period 3 element. It is insoluble in water but dissolves in both aqueous sodium hydroxide and aqueous sulphuric acid.
(i)      Give the name used to describe this behaviour of the hydroxide.
(ii)     Write equations for the reactions occurring.
(iii)     Suggest why R is insoluble in water.
(6)
(Total 15 marks)
Q35.
(a)     Explain why certain elements in the Periodic Table are classified as p-block elements. Illustrate your answer with an example of a p-block element and give its electronic configuration.
(3)
(b)     Explain the meaning of the term periodicity as applied to the properties of rows of elements in the Periodic Table. Describe and explain the trends in atomic radius, in electronegativity and in conductivity for the elements sodium to argon.
(13)
(Total 16 marks)

Mark schemes
Q1.
D
[1]
Q2.
B
[1]
Q3.
C
[1]
Q4.
A
[1]
Q5.
C
[1]
Q6.
A
[1]
Q7.
D
[1]
Q8.
D
[1]
Q9.
D
[1]
Q10.
D
[1]
Q11.
C
[1]
Q12.
A
[1]
Q13.
B
[1]
Q14.
C
[1]
Q15.
B
[1]
Q16.
B
[1]
Q17.
D
[1]
Q18.
(a)    Average / mean mass of 1 atom (of an element)
1/12 mass of one atom of 12C
If moles and atoms mixed, max = 1
1
Mark top and bottom line independently.
All key terms must be present for each mark.
1
OR
Average / mean mass of atoms of an element
1/12 mass of one atom of 12C
OR
Average / mean mass of atoms of an element ×12
mass of one atom of 12C
OR
(Average) mass of one mole of atoms
1/12 mass of one mole of 12C
OR
(Weighted) average mass of all the isotopes
1/12 mass of one atom of 12C
OR
Average mass of an atom / isotope (compared to C−12) on a scale in which an atom of C−12 has a mass of 12
This expression = 2 marks.
(b)      
1
1
= 72.4
72.4 only
1
(c)     (72)Ge+ or germanium+
Must show ‘+’ sign.
Penalise wrong mass number
1
(d)     70
If M1 incorrect or blank CE = 0/2
Ignore symbols and charge even if wrong.
1
Lowest mass / lowest m/z
Accept lightest.
Accept fewest neutrons.
1
(e)     Electron(s) transferred / flow (at the detector)
M1 must refer to electron flow at the detector.
If M1 incorrect CE = 0/2
1
(From detector / plate) to the (+) ion
Do not allow from a charged plate.
1
(f)     They do not have the same electron configuration / they have different number of electrons (in the outer shell)
Ignore electrons determine the properties of an atom.
Ignore they are different elements or different number of protons.
1
[11]
Q19.
(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]
Q20.
(a)     (i)      Higher than P
1
(ii)     1s2 2s2 2p6 3s1
Allow any order
1
(iii)    Al+(g) + e (−)   Al2+(g) + 2e(−)
OR
Al+(g)   Al2+(g) + e(−)
OR
Al+(g) − e(−)   Al2+(g)
1
(iv)    Electron in Si (removed from) (3)p orbital / electron (removed) from higher energy orbital or sub-shell / electron in silicon is more shielded
Accept converse arguments relating to Al
Penalise incorrect p-orbital
1
(b)     Sodium / Na
Allow Na+
1
Electron (removed) from the 2nd shell / 2p (orbital)
M2 is dependent on M1
Allow electron from shell nearer the nucleus (so more attraction)
1
(c)     Silicon / Si
Not SI
1
(d)     Heat or energy needed to overcome the attraction between the (negative) electron and the (positive) nucleus or protons
Not breaking bonds
QoL
Or words to that effect eg electron promoted to higher energy level (infinity) so energy must be supplied
1
[8]
Q21.
(a)     
Particle	Relative charge	Relative mass	 	
Proton	+1 or 1+	1	(1)	
Neutron	0
or no charge/neutral/zero	1 (not – 1)	(1)	
Electron	–1 or 1–	1/1800 to 1/2000	(1)	
or negligible
or zero
or 5.0 × 10– 4 to 5.6 × 10– 4
if ‘g’ in mass column - wrong
penalise once
3
(b)      (1)(1)
Allow numbers before or after Ar
2
(c)     S: 1s2 2s2 2p6 3s2 3p4 (1)
Allow upper case letters
S2–: 1s2 2s2 2p6 3s2 3p6 (1)
If use subscript penalise once
2
(d)     Block: p (1)
Explanation: Highest energy or outer orbital is (3) p
OR outer electron, valency electron in (3) p
NOT 2p etc.
2
(e)     (i)      Bonding in Na2S: ionic (1)
Bonding in CS2:  covalent (1)
ignore other words such as dative / polar / co-ordinate
(ii)     Clear indication of electron transfer from Na to S (1)
1 e– from each (of 2) Na atoms or 2 e– from 2 Na atoms (1)
QoL correct English
(iii)     
 
Correct covalent bonds (1)
All correct including lone pairs (1)
Allow all •s or all ×s
M2 tied to M1
NOT separate e–s in S•- 2 l p
(iv)    CS2 + 2H2O → CO2 + 2H2S (1)
Ignore state symbols even if wrong
7
[16]
Q22.
(a)     (i)      1s2 2s2 2p6 3s2 3p1 (1)
Allow subscripted electron numbers
(ii)     p (block) (1)
Allow upper or lower case ‘s’ and ‘p’ in (a)(i) and (a)(ii)
2
(b)     Lattice of metal / +ve ions/ cations / atoms (1)
Not +ve nuclei/centres
Accept regular array/close packed/tightly packed/uniformly arranged
          (Surrounded by) delocalised electrons (1)
Note: Description as a ‘giant ionic lattice’ = CE
2
(c)     Greater nuclear or ionic charge or more protons (1)
          Smaller atoms / ions (1)
Accept greater charge density for either M1 or M2
          More delocalised electrons / e– in sea of e– / free e– (1)
          Stronger attraction between ions and delocalised / free electrons etc. (1)
Max 3
Note: ‘intermolecular attraction/ forces’ or covalent molecules = CE
Accept stronger ‘electrostatic attraction’ if phrase prescribed elsewhere
Ignore references to m/z values
If Mg or Na compared to Al, rather than to each other, then: Max 2
Treat description that is effectively one for Ionisation Energy as a ‘contradiction’
3
(d)     (Delocalised) electrons (1)
          Move / flow in a given direction (idea of moving non-randomly)
or under the influence applied pd   QoL mark   (1)
Allow ‘flow through metal’
Not: ‘Carry the charge’; ‘along the layers’; ‘move through the metal’
2
[9]
Q23.
(a)               
M1 for the top line
M2 is for division by 17
1
= 84.0
Not 84
No consequential marking from M1 or M2
Ignore units
1
The Ar in the Periodic table takes account of the other isotopes /
different amounts of isotopes (or words to that effect regarding isotopes)
Award independently
Comparison implied
Isotope(s) alone, M4 = 0
1
(b)     (Beam of electrons from) an electron gun / high speed / high energy electrons
1
Knocks out electron(s) (to form a positive ion)
1
Kr(g) + e– → Kr+(g) + 2e(–)
State symbols must clearly be (g)
1
OR
Kr(g) → Kr+(g) + e(–) / Kr(g) – e(–) → Kr+(g)
The 84Kr isotope
One mark for identifying the 84 isotope
1
Has 2 electrons knocked out / gets a 2+ charge
One mark for the idea of losing 2 electrons (from this isotope)
1
[9]
Q24.
(a)     Mg(2+) or Magnesium
Na+ CE=0
1
Because Mg2+ has more protons
AND
With the same shielding/screening/electron arrangement/number of electrons (or isoelectronic)
Allow larger/stronger nuclear charge
Ignore atomic radius
1
(b)     Na(g) → Na+(g) + e−
1 for correct species and gas phase
Allow e without charge
Allow Na(g) – e− → Na+(g)
Na(g) + e− → Na+(g) + 2e−
1
(c)     Mg between 600-800
1
S between 800-1040
If S not lower than P on graph then M1 only
If no plots on graph must state S below P to access M3 & M4
1
e− paired in (3)p orbital in S (owtte)
Allow (3)p subshell/sublevel provided pair mentioned
1
Paired e− repel (so less energy needed to remove)
1
[7]
Q25.
(a)     
 
1
(b)     Increased nuclear charge / proton number (1)
NOT increased atomic number
Electrons enter same shell / energy level OR atoms get smaller
OR same shielding (1)
          Stronger attraction between nucleus and (outer) electrons (1)
Q of L
3
(c)     Explanation for aluminium: (third) electron in (3)p sub-shell (1)
Sub-shell further away from nucleus OR of higher energy (1)
OR extra shielding from (3)s
Explanation for sulphur: Pair of electrons in (3)p orbital (1)
Repulsion between electrons (1)
tied to reference to e– pair in M3
Penalise ‘2p’ once only
4
[10]
Q26.
(a)     Ability (or power) of an atom to attract electron density
(or electrons or ‑ve charge) (1)
in a covalent bond (1)
or shared pair
If remove an electron lose first mark
2
(b)     Trend: increases (1)
Explanation: nuclear charge (number of protons) increases (1)
electrons in same shell (1)
OR similar shielding
OR atoms similar size or smaller
OR 1 mol of e-
3
(c)     Heat / enthalpy / energy for removal of one electron (1)
from a gaseous atom (1)
can score in an equation
must have first mark to score the second
2
(d)     (i)      2 (1)
(ii)     Two elements (or Na / Mg) before the drop (in energy) to Al (1)
(iii)     ionisation energy of Al < that for Mg (1)
(iv)    fall in energy from P to S (1)
or discontinuity in trend
From Al to P there are 3 additional electrons (1)
or three elements
For second mark idea of block of 3 elements
5
[12]
Q27.
(a)     The number of protons increases (across the period) / nuclear charge increases
1
Therefore, the attraction between the nucleus and electrons increases
Can only score M2 if M1 is correct
1
(b)     S8 molecules are bigger than P4 molecules
Allow sulfur molecules have bigger surface area and sulfur molecules have bigger Mr
1
Therefore, van der Waals / dispersion / London forces between molecules are stronger in sulfur
1
(c)     Sodium oxide contains O2– ions
1
These O2– ions react with water forming OH– ions
O2– + H2O   2OH– scores M1 and M2
1
(d)     P4O10 + 12OH–     4PO43- + 6H2O
1
[7]
Q28.
(a)    (Total number of) protons and neutrons (in nucleus of atom)
(number of) nucleons
1
(b)     Zn
Do not allow Zn−1 or Zn+1 or ZN
Ignore numbers
1
(c)    (i)      P = ionise (sample)
Allow removing an electron / forms (+) ions
1
Q = accelerate (sample)
Allow speeds (ions) up
Penalise molecules / atoms
1
(ii)     m / z
Allow mass / charge
1
(relative) abundance / (relative) intensity
QoL
Allow M1 + M2 in any order
1
(d)    (i)       
M1 = topline
1
M2 = ÷ 4
1
= 207.3
Only
207.3 = 3 marks
1
(ii)     Lead / Pb
Not PB
1
(iii)    Same number of electrons (in outer shell) / same electronic configuration
Ignore electrons determine chemical properties
Ignore reference to p and n if correct
Penalise if incorrect
1
[11]
Q29.
(a)     1s22s22p63s23p1
1
1s22s22p63s23p63d3
1
If noble gas core used correctly in both then scores 1
Allow subscripts and capitals
Ignore 4s0
(b)     Sr2+
Ignore name and correct proton/mass number
Allow Sr+2
1
(c)     Ca3P2
Allow reversed or ionic formula
Ignore name
1
[4]
Q30.
(a)      Percentage of oxygen is 36.4%
% of oxygen stated or shown in calculation.
1
Correct calculation of ratios (C 4.54, H 9.10, O 2.28)
Mark is for correct method, dividing % by Ar
1
Empirical formula C2H4O
Allow consequential answer from wrong percentage of oxygen (max 2 marks).
1
(b)     88
Accept 88.0
Do not penalise correct answer in g.
1
(c)     Ratio MF / EF of 2 (88 / 44.0 = 2)
If use 132 / 44 = 3, molecular formula C6H12O3 scores 2 marks.
1
Molecular formula is C4H8O2
Accept consequential answers from (a) and (b)
1
[6]
Q31.
(a)     Li(g) → Li+(g) + e-(g)
Li(g) - e-(g) → Li+(g)
Li(g) + e-(g) → Li+(g) + 2e-
One mark for balanced equation with state symbols
Charge and state on electron need not be shown
1
(b)     Increases
If trend wrong then CE = 0/3 for (b). If blank mark on.
1
Increasing nuclear charge / increasing no of protons
Ignore effective with regard to nuclear charge
1
Same or similar shielding / same no of shells / electron
(taken) from same (sub)shell / electron closer to the
nucleus / smaller atomic radius
1
(c)     Lower
If not lower then CE = 0/3
1
Paired electrons in a (4) p orbital
If incorrect p orbital then M2 = 0
1
(Paired electrons) repel
If shared pair of electrons M2 + M3 = 0
1
(d)     Kr is a bigger atom / has more shells / more shielding
in Kr / electron removed further from nucleus/ electron
removed from a higher (principal or main) energy level
CE if molecule mentioned
Must be comparative answer
QWC
1
(e)     2 / two / II
1
(f)      Arsenic / As
1
[10]
Q32.
(a)     (i)      1.6734 × 10−24 (g)
Only.
1.6734 × 10−27 kg
Not 1.67 × 10−24 (g).
1
(ii)     B
1
(b)    (i)       = 10.8
OR ratio 10:11 = 1:4 OR 20:80 etc
Allow idea that there are 5 × 0.2 divisions between 10 and 11.
1
abundance of 10B is 20(%)
OR
 = 10.8
10x + 1100 − 11x = 1080
∴ x = 1100 − 1080 = 20%
Correct answer scores M1 and M2.
1
(ii)     Same number of electrons (in outer shell or orbital)
Ignore electrons determine chemical properties.
Same electronic configuration / arrangement
Ignore protons unless wrong.
1
(c)     Range between 3500 and 10 000 kJ mol−1
1
(d)     B+(g)  B2+(g) + e(−)
B+(g) − e(−)  B2+(g)
B+(g) + e(−)  B2+(g) + 2e(−)
Ignore state symbol on electron even if wrong.
1
(e)     Electron being removed from a positive ion (therefore needs more energy) / electron being removed is closer to the nucleus
Must imply removal of an electron.
Allow electron removed from a + particle / species or from a 2+ ion.
Not electron removed from a higher / lower energy level / shell.
Not electron removed from a higher energy sub-level / orbital.
Ignore electron removed from a lower energy sub-level / orbital.
Ignore ‘more protons than electrons’.
Not ‘greater nuclear charge’.
Ignore ‘greater effective nuclear charge’.
Ignore shielding.
1
[8]
Q33.
(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]
Q34.
(a)     (i)      Deductions:
         Ionic (1)
Ions not free to move in the solid state (1)
Ions free to move when molten or in aqueous solution (1)
Identity of P: Na2O or sodium oxide (1)
N.B. If a formula given this must be correct
         Equation: Na2O + H2O → 2 NaOH (1)
5
(ii)     Deductions:
         Covalent
Intermolecular forces are weak or van der Waals forces,
or dipole-dipole
N.B. Any answer including a reference to hydrogen bonding is incorrect
         Identity of Q: SO2 or sulphur dioxide (1)
         Equation: SO2 + H2O → H2 SO3(1)
NB Allow max one for SO3
4
(b)     (i)      Amphoteric (1)
(ii)     Equation with NaOH
         Al(OH)3 + NaOH → NaAl(OH)4
OR Al(OH)3(H2O)3 + OH– → [Al(OH)4(H2O)2]– + H2O
OR Al(OH)3 + OH– → [Al(OH)4]–
R identified as Al(OH)3 or Al(OH)3(H2O)3 (1)
A balanced equation (1)
N.B. Allow equation with six co-ordinate Aluminium and up to six OH– ligands
N.B. Allow equation mark if M(OH)3 given in a balanced equation
         Equation with H2SO4
2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2O
OR Al(OH)3(H2O)3 + H+ → [Al(OH)2(H2O)4+ + H2O
NB Allow equations with six co-ordinate Aluminium and up to six H2O ligands NB Allow equation mark if M(OH)3 given in a balanced equation
Correct Al species as product (1)
A balanced equation (1)
(iii)     Large lattice energy
or strong covalent bonds
or ΔHsoln is very positive
or ΔG is positive
or sum of hydration energies less than covalent bond energies (1)
6
[15]
Q35.
(a)     Elements in the p block have their outer electron(s) in
p orbital(s) or levels or sub-shells (1)
example of element (1)
correct electronic configuration (1)
3
(b)     Pattern in the change in the properties of a row of elements (1)
OR Trend in the properties of elements across a period
          Repeated in the next row (1)
OR element underneath (or in same group) has similar properties
          atomic radius
decreases across the row (1)
CE if trend is wrong
number of protons increases (1) (or nuclear charge increases)
more attraction for electrons in the same shell (1)
electronegativity
increases across the row (1)
number of protons increases (1) (or nuclear charge)
atomic radius decreases (1) (or shielding remains the same or electrons
in the same shell) more attraction for bonding or shared electrons (1)
          conductivity
decreases row (1)
OR significant drop from Al to Si
          Na–Al metals (1)
OR metallic bonding or description of metallic bonding
          Two of Si - Ar non metals (1)
OR molecular or covalent
EITHER electrons free to move (or delocalised) in metals
OR electrons unable to move in non-metals (1)
13
[16]