_______________________

Name:
_
Classification
_______________________
Class:
_

_______________________
Date:
_

Time: 93 minutes

Marks: 90 marks

Comments:

Page 1 of 21
Q1.
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)

Q2.
Which element is in the f-block of the Periodic Table?

A Palladium

B Phosphorus

C Platinum

D Plutonium
(Total 1 mark)

Q3.
Which element is in the d-block of the Periodic Table?

A Selenium

B Antimony

C Tantalum

D Lead
(Total 1 mark)

Q4.
(a) Nickel is a metal with a high melting point.

(i) State the block in the Periodic Table that contains nickel.

______________________________________________________________
(1)

(ii) Explain, in terms of its structure and bonding, why nickel has a high melting
point.

Page 2 of 21
 ______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________
(2)

(iii) Draw a labelled diagram to show the arrangement of particles in a crystal of

nickel.
In your answer, include at least six particles of each type.

(2)

(iv) Explain why nickel is ductile (can be stretched into wires).

______________________________________________________________

______________________________________________________________

______________________________________________________________
(1)

(b) Nickel forms the compound nickel(II) chloride (NiCl2).

(i) Give the full electron configuration of the Ni2+ ion.

______________________________________________________________
(1)

(ii) Balance the following equation to show how anhydrous nickel(II) chloride can
be obtained from the hydrated salt using SOCl2
Identify one substance that could react with both gaseous products.

......NiCl2.6H2O(s) + ...... SOCl2(g) ......NiCl2(s) + ......SO2(g) + ......HCl(g)

Substance ____________________________________________________
(2)
(Total 9 marks)

Q5.
The element rubidium exists as the isotopes 85Rb and 87Rb

(a) State the number of protons and the number of neutrons in an atom of the isotope

Page 3 of 21
 85
Rb

Number of protons ___________________________________________________

Number of neutrons __________________________________________________

(2)

(b) (i) Explain how the gaseous atoms of rubidium are ionised in a mass
spectrometer

______________________________________________________________

______________________________________________________________

______________________________________________________________

______________________________________________________________
(2)

(ii) Write an equation, including state symbols, to show the process that occurs
when the first ionisation energy of rubidium is measured.

______________________________________________________________
(1)

(c) The table shows the first ionisation energies of rubidium and some other elements in
the same group.

Element sodium potassium rubidium

First ionisation
494 418 402
energy / kJ mol–1

State one reason why the first ionisation energy of rubidium is lower than the first
ionisation energy of sodium.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(1)

(d) (i) State the block of elements in the Periodic Table that contains rubidium.

______________________________________________________________
(1)

(ii) Deduce the full electron configuration of a rubidium atom.

______________________________________________________________
(1)

Page 4 of 21
 (e) A sample of rubidium contains the isotopes 85Rb and 87Rb only.
The isotope 85Rb has an abundance 2.5 times greater than that of 87Rb

Calculate the relative atomic mass of rubidium in this sample.

Give your answer to one decimal place.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(3)

(f) By reference to the relevant part of the mass spectrometer, explain how the
abundance of an isotope in a sample of rubidium is determined.

Name of relevant part _________________________________________________

Explanation _________________________________________________________

___________________________________________________________________

___________________________________________________________________
(2)

(g) Predict whether an atom of 88Sr will have an atomic radius that is larger than, smaller
than or the same as the atomic radius of 87Rb. Explain your answer.

Atomic radius of 88Sr compared to 87Rb ___________________________________

Explanation _________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(3)
(Total 16 marks)

Q6.
The elements phosphorus, sulfur, chlorine and argon are in the p block of the Periodic
Table.

(a) State why these elements are classified as p block elements.

___________________________________________________________________
(1)

(b) State the trend in atomic radius from phosphorus to chlorine and explain the trend.

Trend ______________________________________________________________

Explanation _________________________________________________________

Page 5 of 21
 ___________________________________________________________________

___________________________________________________________________
(3)

(c) In terms of structure and bonding, explain why sulfur has a higher melting point than
phosphorus.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(3)

(d) In terms of atomic structure, explain why the van der Waals’ forces in liquid argon
are very weak.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(2)
(Total 9 marks)

Q7.
(a) State the meaning of the term first ionisation energy of an atom.

___________________________________________________________________

___________________________________________________________________
(2)

(b) Complete the electron arrangement for the Mg2+ ion.

1s2 ________________________________________________________________
(1)

(c) Identify the block in the Periodic Table to which magnesium belongs.

___________________________________________________________________
(1)

(d) Write an equation to illustrate the process occurring when the second ionisation
energy of magnesium is measured.

___________________________________________________________________
(1)

(e) The Ne atom and the Mg2+ ion have the same number of electrons. Give two
reasons why the first ionisation energy of neon is lower than the third ionisation
energy of magnesium.

Page 6 of 21
 Reason 1 ___________________________________________________________

Reason 2 ___________________________________________________________
(2)

(f) There is a general trend in the first ionisation energies of the Period 3 elements, Na
– Ar

(i) State and explain this general trend.

Trend ________________________________________________________

Explanation ____________________________________________________

______________________________________________________________

______________________________________________________________

(ii) Explain why the first ionisation energy of sulphur is lower than would be
predicted from the general trend.

______________________________________________________________

______________________________________________________________

______________________________________________________________
(5)
(Total 12 marks)

Q8.
(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.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

Page 7 of 21
 ___________________________________________________________________
(3)

(d) Explain how metals conduct electricity.

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(2)
(Total 9 marks)

Q9.
(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 ________________________________________________

Page 8 of 21
 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)

Q10.
(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.

___________________________________________________________________

Page 9 of 21
___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________

___________________________________________________________________
(13)
(Total 16 marks)

Page 10 of 21
Mark schemes

Q1.
C
[1]

Q2.
D
[1]

Q3.
C
[1]

Q4.
(a) (i) d (block) OR D (block)
Ignore transition metals / series.
Do not allow any numbers in the answer.
1

(ii) Contains positive (metal) ions or protons or nuclei and delocalised /

mobile / free / sea of electrons
Ignore atoms.
1

Strong attraction between them or strong metallic bonds

Allow ‘needs a lot of energy to break / overcome’ instead of
‘strong’.
If strong attraction between incorrect particles, then CE = 0 /
2.
If molecules / intermolecular forces / covalent bonding / ionic
bonding mentioned then CE=0.
1

(iii)

M1 is for regular arrangement of atoms / ions (min 6 metal

particles).
M2 for + sign in each metal atom / ion.
Allow 2+ sign.
2

(iv) Layers / planes / sheets of atoms or ions can slide over one another
QoL.
1

(b) (i) 1s2 2s2 2p6 3s2 3p6 3d8 (4s0)

Page 11 of 21
 Only.
1

(ii) NiCl2.6H2O + 6 SOCl2 NiCl2 + 6 SO2 + 12 HCl

Allow multiples.
1

NaOH / NH3 / CaCO3 / CaO

Allow any name or formula of alkali or base.
Allow water.
1
[9]

Q5.
(a) 37
These answers only.
Allow answers in words.
1

48
Ignore any sum(s) shown to work out the answers.
1

(b) (i) Electron gun / high speed/high energy electrons

Not just electrons.
Not highly charged electrons.
1

Knock out electron(s)

Remove an electron.
1

(ii) Rb(g) → Rb+(g) + e(–)

OR
Rb(g) + e(–) → Rb+(g) + 2e(–)
OR
Rb(g) - e(–) → Rb+(g)
Ignore state symbols for electron.
1

(c) Rb is a bigger (atom) / e further from nucleus / electron lost from a higher
energy level/ More shielding in Rb / less attraction of nucleus in Rb for outer
electron / more shells
Answer should refer to Rb not Rb molecule
If converse stated it must be obvious it refers to Na
Answer should be comparative.
1

(d) (i) s / block s / group s

Only
1

(ii) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

Allow 3d10 before 4s2

Page 12 of 21
 Allow in any order.
1

(e) (85 × 2.5) + 87 ×1

3.5
M1 is for top line
1
1

= 85.6
Only
1

OR

(58 × 5) + 87 ×2
7
M185Rb 71.4% and 87Rb 28.6%
M2 divide by 100
1
1

85.6
M3 = 85.6
1

(f) Detector
Mark independently
Allow detection (plate).
1

Current / digital pulses / electrical signal related to abundance

Not electrical charge.
1

(g) Smaller
Chemical error if not smaller, CE = 0/3
If blank mark on.
1

Bigger nuclear charge / more protons in Sr

Not bigger nucleus.
1

Similar/same shielding
QWC
(Outer) electron entering same shell/sub shell/orbital/same
number of shells.
Do not allow incorrect orbital.
1
[16]

Q6.
(a) Outer electrons are in p orbitals
1

Page 13 of 21
 (b) decreases
1

Number of protons increases

1

Attracting outer electrons in the same shell (or similar shielding)

1

(c) Sulfur molecules (S8) are larger than phosphorus (P4)

1

Therefore van der Waals’ forces between molecules are stronger

1

Therefore more energy needed to loosen forces between molecules

1

(d) Argon particles are single atoms with electrons closer to nucleus
1

Cannot easily be polarised (or electron cloud not easily distorted)

1
[9]

Q7.
(a) enthalpy/energy change/required when an electron is removed/
knocked out / displaced/ to form a uni-positive ion
(ignore ‘minimum’ energy)
1

from a gaseous atom

(could get M2 from a correct equation here)
(accept ‘Enthalpy/energy change for the process...’
followed by an appropriate equation, for both marks)
(accept molar definitions)
1

(b) 1s2 2s22p6

(accept capitals and subscripts)

1

(c) ‘s’ block

(not a specific ‘s’ orbital – e.g. 2s)
1

(d) Mg+(g) → Mg2+(g) + e– or

Mg+(g) + e– → Mg2+(g) + 2e– or

Mg+(g) – e– → Mg2+(g)
1

(e) Mg2+ ion smaller than Ne atom / Mg2+ e– closer to nucleus

(Not ‘atomic’ radius fo Mg2+)
1

Page 14 of 21
 Mg2+ has more protons than Ne / higher nuclear charge or
e– is removed from a charged Mg2+ion / neutral neon atom
(accept converse arguments)
(If used ‘It’ or Mg/magnesium/Mg3+ etc. & 2 correct reasons,
allow (1))
1

(f) (i) trend: increases

(if ‘decreases’, CE = 0/3)
1

Expln: more protons / increased proton number /

increased nuclear charge
(NOT increased atomic number)
1

same shell / same shielding / smaller size

1

(ii) QoL reference to the e– pair in the 3p sub-level

(penalise if wrong shell, e.g. ‘2p’, quoted)
1

repulsion between the e–in this e–pair

(if not stated, ‘e– pair’ must be clearly implied)
(mark M4 and M5 separately)
1
[12]

Q8.
(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)

Page 15 of 21
 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]

Q9.
(a)
Particle Relative charge Relative mass

Proton +1 or 1+ 1 (1)

Neutron 0 1 (not – 1) (1)

or no
charge/neutral/zero

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)

Page 16 of 21
 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]

Q10.
(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)

Page 17 of 21
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]

Page 18 of 21
Examiner reports

Q3.
Usually well answered.

Q4.
This question was generally quite well answered. In part (a)(i), most students knew the
correct block in the Periodic Table although some seemed to think that the name
‘Transition Metals’ was enough to identify the d block. In part (a)(ii), the biggest issue was
the omission of ‘positive’ when describing ions and ‘delocalised’ when describing the
electrons involved in the bonding. The diagrams in part (a)(iii) generally scored highly but
some were untidy and failed to show a regular arrangement of ions. Surprisingly, many
students did not refer to layers of atoms / ions sliding in part (a)(iv) and therefore did not
score the mark. Answers to part (b)(i) were disappointing and showed that students could
not write the electron configuration of ions in the d block. Balancing the equation proved
difficult but a good number of students did this well and many students could suggest a
suitable substance in part (b)(ii).

Q5.
Part (a) was done very well. In part (b)(i), many students stated that a positive ion was
formed but failed to say how. The equation in part (b)(ii) was well done with only a few
omitting the state symbols. In part (c), a number of students failed to score the mark since
they referred to a rubidium molecule, showing a lack of understanding of the metals given.
In part (d)(ii) there were many students who filled the 4d rather than the 5s orbitals and
some gave an abbreviated electron structure even though the question asked for the full
electron structure. Many students found part (e) difficult although it was pleasing to see
some gain full marks. Part (f) was not well understood with many students confusing
charge and current. The answers to part (g) were generally good although a few students
did not give complete explanations and lost the last mark.

Q7.
Candidates tended to score a little better on this question than on question 3 but, overall,
the question was not well answered. Part (a) was generally well done, although
incomplete answers were quite common. The most common error was to omit reference
to gaseous atoms.

Parts (b) and (c) were often well answered; however, in part (d) incorrect ionic charges
and missing or incorrect state symbols were quite often seen.

Part (e) was poorly done. Many candidates referred to difference in the number of electron
shells present in the two species despite being told in the question that they had the same
number of electrons. Some candidates attributed the difference to a special stability
enjoyed by neon as a consequence of it having a full outer electron shell. Clearly, the
majority of candidates failed to appreciate the significance of the two species having the
same number of electrons. Many answers referred to ”It’, magnesium or Mg, rather than
correctly identifying the species being discussed.

In part (f), candidates are asked to demonstrate their understanding of a trend required in
the specification. While part (f)(i) was often competently dealt with, answers in part (f)(ii)
frequently lacked sufficient specific detail to be awarded credit. Often, candidates failed to
identify the electron pair from which from which the first electron would be removed, or to

Page 19 of 21
 explain the relatively low first ionisation energy of sulphur in terms of repulsion between
the electrons in this electron pair. Vague phrases such as ‘electron pairs repel’, or a
reference to a more stable half-filled shell being formed, earned no credit.

Q8.
Some good responses were seen but overall this question was not well answered
however most candidates managed to earn some marks. Part (a) was generally
satisfactorily answered with occasional errors in the electron configuration, and most
candidates correctly assigned aluminium to the p block of the Periodic Table. In part (b),
references to delocalised electrons were frequently seen, however mention of the
existence of a close-packed lattice of positive ions was much less common. Some good
answers were seen in part (c), although many responses were related to differences in
ionisation energy rather than to differences in melting point. There was also much
confusion over the type of attractive force present, with frequent references to ‘ionic
bonding’, ‘intermolecular forces’, and to ‘magnesium having a full s subshell’.

Only rarely was the higher melting point of magnesium attributed to a greater attraction
between the ionic lattice and the delocalised electrons that resulted from its higher ionic
charge and increased number/concentration of delocalised electrons. In part (d), most
candidates made mention of electrons but very few made reference to an electrical
current being a flow of electrons through a metal. The incorrect idea of passing the charge
from one electron to another was very common, as were vague references to electrons
being free to move in the metal.

Q9.
Many candidates answered this question quite well but full marks were not that common.
Most candidates correctly completed the table in part (a) but it was not unusual for either
the signs or the values of the relative charges to be omitted. In a few instances, the values
of the electron and the neutron were transposed. Success in part (b) was far from
universal. Errors such as 39.9 and 36 for the mass number were quite common, as was
the use of Z to represent the element. Part (c) was, in the main, successfully completed
but the odd d level was seen, as were configurations for the S2– ion showing 3p2 rather
than 3p6 electrons, or even a 2p8 arrangement. While part (d) was also generally well
done, some candidates were found to be unfamiliar with this part of the specification and
the suggestion that the element was found in block 6, because it contained 6 outer
electrons, was not uncommon. Some candidates incorrectly referred to the p-block or p-
shell, rather than using the correct terms sub-level or sub-shell. In part (e), a surprising
number of candidates identified incorrectly the bonding in Na2S as being covalent or
metallic, and the bonding in CS2 as being ionic, molecular or dative. For those candidates
who did recognise the ionic nature of the bonding in Na2S, their descriptions were often
vague and they did not express clearly the transfer of electrons which takes place, and the
numbers of electrons involved. Many answers could have equally well fitted the
description for the formation of a covalent bond. The diagram of the bonding in CS2 was
frequently flawed, with spare electrons being placed around carbon and extra lone pairs
on the sulphur atoms. Some candidates showed a single bond between the sulphur and
carbon atoms, whilst others only included a single sulphur atom. The equation was almost
invariably correct; although, in a few cases, the equation was not balanced.

Q10.
Marks awarded for this question were not as high as for question 5. There was some
evidence that candidates were short of time, particularly those who wrote irrelevant
information about the operation of the mass spectrometer in question 5. In part (a) the
example of a p-block element and its electronic configuration were more often correct than
was an explanation of why elements are classified as p-block. The meaning of the term

Page 20 of 21
periodicity was not understood well in part (b). Many candidates considered that
periodicity referred to trends down a Group. The remainder of part (b) discriminated
effectively between good and weak candidates. The latter sometimes stated trends in the
wrong direction and gave only partial explanations.

Page 21 of 21