Arrangement of elements
8.1What the syllabus asks of you
- Describe the Periodic Table as an arrangement of elements in periods and groups and in order of increasing proton number / atomic number
- Describe the change from metallic to non-metallic character across a period
- Describe the relationship between group number and the charge of the ions formed from elements in that group
- Explain similarities in the chemical properties of elements in the same group of the Periodic Table in terms of their electronic configuration
- Explain how the position of an element in the Periodic Table can be used to predict its properties
- Identify trends in groups, given information about the elements
Read the notes first
Chapter 8: Arrangement of elements
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Every question on Arrangement of elements, untimed, marked as you go.
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33 questions
1May / June 2026 · Paper 12 · Q20Show mark scheme →
AIn all groups, the reactivity of the elements increases down the group.
BThe metallic character of the elements increases from left to right across a period.
CThe charge in the nucleus changes by the same amount from one element to the next down a group.
DThe charge in the nucleus changes by the same amount from one element to the next across a period.
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2Oct / Nov 2025 · Paper 11 · Q20Show mark scheme →
AThe compound formed between X and W has covalent bonds.
BW and Y are both gases at r.t.p. that contain covalent bonds.
CX and Y react together more vigorously than Z and Y at r.t.p.
DX and Z both have two outer-shell electrons.
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3May / June 2025 · Paper 11 · Q22Show mark scheme →
Achlorine
Bfluorine
Coxygen
Dsulfur
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4May / June 2025 · Paper 12 · Q22Show mark scheme →
AAcross a period, elements at the left-hand side of the Periodic Table are more metallic than those at the right-hand side.
BDown a group, elements at the top of the group lose electrons more readily than those at the bottom of the group.
CElements in the same group of the Periodic Table have the same number of completed shells of electrons.
DElements in the same period of the Periodic Table have the same number of electrons in the outer shell.
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5Oct / Nov 2024 · Paper 12 · Q25Show mark scheme →
Athe masses of their atoms
Bthe number of electrons in the outer shell
Cthe number of neutrons in the nucleus
Dthe number of protons in the nucleus
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6May / June 2024 · Paper 11 · Q26Also set in Oct / Nov 2017 Paper 11Show mark scheme →
AQ and R react together to form a covalent compound.
BQ forms positive ions.
CR has more outer shell electrons than Q.
DR is more metallic than Q.
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7May / June 2024 · Paper 12 · Q25Show mark scheme →
AA
BB
CC
DD
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8Oct / Nov 2023 · Paper 11 · Q23Show mark scheme →
Aboth 1 and 2
B1 only
C2 only
Dneither 1 nor 2
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9Oct / Nov 2023 · Paper 12 · Q23Show mark scheme →
AW and Z are in the same group.
BX is a metal.
CX and Y will form the compound X3Y.
DY is a non-metal.
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10May / June 2023 · Paper 11 · Q21Show mark scheme →
Agroup determined by: the number of electrons in the outer shell; period determined by: the number of occupied shells; elements in the Periodic Table are arranged by: increasing proton number
Bgroup determined by: the number of occupied shells; period determined by: the number of electrons in the outer shell; elements in the Periodic Table are arranged by: increasing mass number
Cgroup determined by: the number of electrons in the outer shell; period determined by: the number of occupied shells; elements in the Periodic Table are arranged by: increasing mass number
Dgroup determined by: the number of occupied shells; period determined by: the number of electrons in the outer shell; elements in the Periodic Table are arranged by: increasing proton number
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11May / June 2023 · Paper 12 · Q25Show mark scheme →
Aa metal / covalent
Ba metal / ionic
Ca non-metal / covalent
Da non-metal / ionic
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12May / June 2022 · Paper 11 · Q30Show mark scheme →
AI; basic
BII; acidic
CIV; amphoteric
DVI; acidic
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13May / June 2022 · Paper 12 · Q31Show mark scheme →
AA gallium atom has three more protons than a selenium atom.
BGallium is more likely to form negative ions than selenium.
CSelenium atoms have fewer valence electrons than gallium atoms.
DSelenium has more non-metallic character than gallium.
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14Oct / Nov 2021 · Paper 11 · Q28Show mark scheme →
AElements at the left-hand side of the Periodic Table are more metallic than those, in the same period, near the right-hand side.
BElements at the top of a group lose electrons more readily than those, in the same group, that are lower in the Periodic Table.
CElements in the same group of the Periodic Table have the same number of completed shells of electrons.
DElements in the same period of the Periodic Table have the same number of electrons in the outer shell.
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15Oct / Nov 2021 · Paper 12 · Q28Show mark scheme →
AThe element germanium, in Group IV, has less metallic character than gallium, in Group III.
BElements in Group V form ions with a charge of 5+.
CElements in the same group react in a similar way because they all contain the same number of electrons.
DTransition elements are given this name as they easily change from solids to liquids.
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16May / June 2021 · Paper 12 · Q26Also set in May / June 2021 Paper 11Show mark scheme →
A1 and 2
B1 and 3
C2 and 4
D3 and 4
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17May / June 2021 · Paper 12 · Q27Show mark scheme →
AA germanium atom has two more valence electrons than a selenium atom.
BGermanium forms a Ge3+ ion and selenium forms an Se3- ion.
CGermanium has more metallic character than selenium.
DGermanium has similar properties to tellurium, and selenium has similar properties to tin.
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18May / June 2020 · Paper 11 · Q23Show mark scheme →
ACa Ca
BCa Cl
CLi Ca
DLi Cl
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19May / June 2020 · Paper 11 · Q25Show mark scheme →
AAll noble gases are unreactive due to having eight electrons in their outer shells.
BThe Group VII element astatine, At2, is expected to be a black solid at room temperature.
CThe reactivity of the elements in both Group I and Group VII increases down the group.
DWhen aqueous chlorine is added to aqueous potassium bromide there is no change in colour.
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20Oct / Nov 2019 · Paper 11 · Q23Show mark scheme →
A1, 2 and 3
B1 and 2 only
C1 and 3 only
D2 and 3 only
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21Oct / Nov 2019 · Paper 12 · Q21Show mark scheme →
AWX and YZ
BWY2 and WZ
CWZ and XZ
DX2Z3 and YZ
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22May / June 2019 · Paper 11 · Q26Show mark scheme →
AII
BIII
CIV
DVI
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23Oct / Nov 2018 · Paper 11 · Q24Show mark scheme →
Aability to form anions
Bmetallic character
Cnumber of electron shells
Dreactivity with water
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24May / June 2018 · Paper 11 · Q26Show mark scheme →
AAn atom of potassium, K, has more protons than an atom of argon, Ar.
BElements in the same period have similar chemical properties.
CElements that are non-metals form only covalent bonds with other elements.
DOn descending Group I from lithium, Li, to caesium, Cs, the metals become less reactive.
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25May / June 2018 · Paper 12 · Q26Show mark scheme →
AAntimony has more metallic character and more valency electrons per atom than indium.
BAntimony has more metallic character; indium has more valency electrons per atom.
CIndium has more metallic character; antimony has more valency electrons per atom.
DIndium has more metallic character and more valency electrons per atom than antimony.
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26May / June 2018 · Paper 12 · Q27Also set in May / June 2018 Paper 11Show mark scheme →
AA
BB
CC
DD
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27Oct / Nov 2017 · Paper 12 · Q27Show mark scheme →
AThey conduct electricity when molten.
BThey form covalent compounds when bonded to non-metals.
CThey exist as diatomic molecules.
DWhen Group I elements combine with Group VII elements, ionic compounds form.
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28May / June 2017 · Paper 11 · Q24Show mark scheme →
AW X Y
BW Y X
CX W Y
DX Y W
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29May / June 2017 · Paper 12 · Q22Show mark scheme →
AGroup II
BGroup III
CGroup V
DGroup VIII
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30May / June 2017 · Paper 12 · Q24Show mark scheme →
Aargon
Bcalcium
Ccopper
Dpotassium
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31Oct / Nov 2016 · Paper 11 · Q25Show mark scheme →
A1 and 2
B1 and 3
C2 and 4
D3 and 4
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32Oct / Nov 2016 · Paper 12 · Q24Show mark scheme →
AA
BB
CC
DD
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33May / June 2016 · Paper 11 · Q26Show mark scheme →
AAll the elements in the same group of the Periodic Table have the same reactivity.
BAll the elements with four electrons in their outer shells are metals.
CAn element in Group II of the Periodic Table would form an ion with a 2– charge.
DElements in the same period of the Periodic Table have the same number of shells of electrons.
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