What are periodic trends in the context of the Periodic Table?

Periodic trends refer to patterns observed in the properties of elements as you move across periods or down groups in the Periodic Table. These trends include variations in atomic radius, ionization energy, electronegativity, and electron affinity. Understanding these trends helps predict the behavior of elements in chemical reactions, which is essential for Cambridge IGCSE Coordinated Science.

How does atomic radius change across a period and down a group?

As you move across a period from left to right in the Periodic Table, the atomic radius generally decreases. This is because the number of protons increases, pulling the electron cloud closer to the nucleus. Conversely, as you move down a group, the atomic radius increases due to the addition of electron shells, which outweighs the increased nuclear charge. This concept is crucial for students studying Periodic Trends in Cambridge IGCSE Coordinated Science.

Why does ionization energy increase across a period?

Ionization energy tends to increase across a period because the effective nuclear charge increases as more protons are added to the nucleus. This stronger attraction makes it more difficult to remove an electron. Understanding this trend is important for Cambridge IGCSE students as it explains the reactivity of elements and their ability to form compounds.

What is the trend in electronegativity across the Periodic Table?

Electronegativity generally increases across a period from left to right and decreases down a group. This is because atoms with more protons and a smaller atomic radius can attract electrons more strongly. This trend is significant in predicting how elements will bond and interact, a key concept in the Cambridge IGCSE Coordinated Science curriculum.

How does electron affinity change across periods and groups?

Electron affinity generally becomes more negative across a period, indicating a stronger attraction for additional electrons. However, it becomes less negative down a group as the added electron would be further from the nucleus. This trend helps explain the chemical behavior of elements and is an important aspect of Periodic Trends in the Cambridge IGCSE Coordinated Science syllabus.

Why is "Saying Group I reactivity decreases down the group (like Group VII)" a common mistake in Periodic Trends?

Why it happens: Students apply the same reactivity trend to both groups without considering whether the reaction involves gaining or losing electrons. How to avoid it: Group I: reactivity INCREASES down (easier to LOSE outer electron). Group VII: reactivity DECREASES down (harder to GAIN electron). Always state whether electrons are lost or gained. Source: 0654 Examiner Report 2023

Why is "Saying 'shielding increases because there are more shells' without explaining the mechanism" a common mistake in Periodic Trends?

Why it happens: Students state the trend without linking it to the mechanism. How to avoid it: Explain: inner electrons repel the nuclear attraction on outer electrons → reduced effective nuclear charge on outer electrons → weaker attraction.

Why is "Saying atomic radius increases across a period because more electrons are added" a common mistake in Periodic Trends?

Why it happens: Students see more electrons and assume a larger atom, ignoring the stronger nuclear charge. How to avoid it: More electrons across a period are all in the SAME shell; the increasing nuclear charge pulls them all closer → SMALLER radius across a period.

The Periodic TableCambridge IGCSE Coordinated Sciences 0654

Periodic Trends

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Periodic Trends — Cambridge IGCSE Coordinated Science 0654

Properties change in regular patterns across periods and down groups. Cambridge tests trends in reactivity, atomic radius, ionisation energy, melting point, and metallic/non-metallic character.

What you’ll learn

Mapped to the Cambridge IGCSE 0654 syllabus (2025-2027).

C9.4 — Describe and explain trends in atomic radius, ionisation energy, and reactivity across periods and down groups.

Trends in the Periodic Table

Atomic size, ionisation energy, and reactivity all follow predictable patterns explained by electron shell structure and nuclear charge.

Atomic radius:

Across a period (→): DECREASES. Same number of shells but increasing nuclear charge pulls electrons closer.
Down a group (↓): INCREASES. More electron shells added → greater distance from nucleus.

Ionisation energy (energy to remove 1 outer electron from gaseous atom):

Across a period (→): INCREASES. More protons pulling same shells → harder to remove electron.
Down a group (↓): DECREASES. Outer electron is further from nucleus + more shielding by inner shells → easier to remove.

Reactivity of metals (Group I):

Reactivity INCREASES down the group.
Outer electron in a larger shell (further from nucleus, more shielded) → easier to lose.
Li < Na < K < Rb < Cs (reactivity order — K reacts vigorously with water, Na moderately, Li slowly)

Reactivity of non-metals (Group VII):

Reactivity DECREASES down the group.
Harder to attract and gain an electron when the outer shell is further from the nucleus.
F > Cl > Br > I (reactivity order — F most reactive halogen)

Metallic to non-metallic character across Period 3: Na (metal) → Mg (metal) → Al (metal) → Si (metalloid) → P (non-metal) → S (non-metal) → Cl (non-metal) → Ar (noble gas)

Across period: atomic radius ↓, ionisation energy ↑, non-metallic character ↑.
Down group: atomic radius ↑, ionisation energy ↓.
Group I: reactivity ↑ down. Group VII: reactivity ↓ down.

How it’s examined

Paper 4: 'Explain why potassium is more reactive than sodium' (3 marks — outer electron in shell further from nucleus, more shielding, less energy needed to remove it). 'State the trend in ionisation energy across Period 3' (1 mark — increases from left to right). MCQ tests which element is more reactive in displacement reactions.

Sources: Cambridge IGCSE Coordinated Sciences 0654 syllabus 2025-2027 (C9); 0654 Examiner Reports 2022-2024. Last reviewed 2026-05-14.

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Step-by-step worked examples — Periodic Trends

Step-by-step solutions to past-paper-style questions on periodic trends, written exactly the way a tutor would explain them at the board.

1Atomic radius trend across Period 3
Extended
Question
Explain why atomic radius decreases from sodium to argon across Period 3.
Step-by-step solution
1. Step 1
  Going from Na (Z=11) to Ar (Z=18), the atomic number (and therefore number of protons) increases from 11 to 18.
2. Step 2
  All elements in Period 3 have the same number of electron shells (3 shells); the outer electrons are all in the 3rd shell.
3. Step 3
  As nuclear charge increases (more protons), the nucleus attracts the outer electrons more strongly; the outer shell is pulled closer to the nucleus.
4. Step 4
  Radius decreases from Na to Ar across Period 3.
Answer
Number of protons increases (11 → 18); same number of shells (3); stronger nuclear attraction pulls outer electrons closer → atomic radius decreases across Period 3.
Examiner tip
Key phrases: 'increasing nuclear charge', 'same number of shells (shielding constant)', 'stronger attraction on outer electrons'.
2Ionisation energy trend down Group I
Extended
Question
Explain why ionisation energy decreases down Group I (from Li to Cs).
Step-by-step solution
1. Step 1
  Going down Group I, each element has one more electron shell than the element above.
2. Step 2
  The outer (valence) electron is in a shell further from the nucleus and is more shielded by inner shells from the nuclear charge.
3. Step 3
  The effective nuclear attraction on the outer electron decreases; it requires less energy to remove the outer electron.
4. Step 4
  Therefore, ionisation energy decreases down Group I.
Answer
More shells → outer electron further from nucleus → greater shielding → weaker nuclear attraction → less energy to remove outer electron → lower ionisation energy.
3Reactivity trend down Group VII
Extended
Question
State the trend in reactivity going down Group VII and explain the trend in terms of atomic structure.
Step-by-step solution
1. Step 1
  Reactivity DECREASES going down Group VII (F > Cl > Br > I).
2. Step 2
  Halogens react by gaining one electron to complete their outer shell.
3. Step 3
  Going down the group, the outer shell is further from the nucleus and more shielded by inner electrons.
4. Step 4
  It becomes harder for the nucleus to attract an incoming electron to the outer shell → decreasing reactivity.
Answer
Reactivity decreases down Group VII; the outer shell is further from the nucleus and more shielded → weaker attraction for an extra electron → less reactive.
Examiner tip
Contrast with Group I (reactivity increases down): metals react by losing electrons; easier to lose further from nucleus. Halogens react by gaining electrons; harder to attract further from nucleus.

Key Definitions and Keywords — Periodic Trends

Definitions to memorise and the exact keywords mark schemes credit for periodic trends answers — sharpened from recent examiner reports for the 2026 0654 sitting.

First ionisation energy
Examiner keyword
The energy required to remove one mole of electrons from one mole of atoms in the gaseous state to form one mole of positive ions: $X(g) \rightarrow X^+(g) + e^-$ . Increases across a period; decreases down a group.
Atomic radius
Examiner keyword
A measure of the size of an atom; decreases across a period (increasing nuclear charge) and increases down a group (additional electron shells).
Electron shielding
Examiner keyword
The reduction in the effective nuclear attraction on outer electrons caused by inner shell electrons. Greater shielding → weaker effective nuclear charge on outer electrons.
Nuclear charge
Examiner keyword
The positive charge of the nucleus, equal to the number of protons (atomic number). Increasing nuclear charge across a period increases attraction on outer electrons.
Metallic character
The tendency of an element to lose electrons and form positive ions; decreases across a period (left to right) and increases down a group.

Common Mistakes and Misconceptions — Periodic Trends

The traps other students keep falling into on periodic trends questions — taken from recent Cambridge IGCSE 0654 examiner reports and mark schemes — and how to avoid them.

✕Saying Group I reactivity decreases down the group (like Group VII)
0654 Examiner Report 2023
Why it happens
Students apply the same reactivity trend to both groups without considering whether the reaction involves gaining or losing electrons.
How to avoid it
Group I: reactivity INCREASES down (easier to LOSE outer electron). Group VII: reactivity DECREASES down (harder to GAIN electron). Always state whether electrons are lost or gained.
✕Saying 'shielding increases because there are more shells' without explaining the mechanism
Why it happens
Students state the trend without linking it to the mechanism.
How to avoid it
Explain: inner electrons repel the nuclear attraction on outer electrons → reduced effective nuclear charge on outer electrons → weaker attraction.
✕Saying atomic radius increases across a period because more electrons are added
Why it happens
Students see more electrons and assume a larger atom, ignoring the stronger nuclear charge.
How to avoid it
More electrons across a period are all in the SAME shell; the increasing nuclear charge pulls them all closer → SMALLER radius across a period.

Practice questions

Exam-style questions with step-by-step worked solutions. Try one before checking the method.

Past paper style quiz

Get a report showing which sub-topics you've nailed and which ones still need work.

Periodic Trends — frequently asked questions

The things students keep getting wrong in this sub-topic, answered.

The Periodic TableCambridge IGCSE Coordinated Sciences 0654

Periodic Trends

Work through the notes, try the practice questions, then take the quiz. The report tells you exactly what to revise next.

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Short Study Notes — Periodic Trends

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Periodic Trends — Cambridge IGCSE Coordinated Science 0654

Properties change in regular patterns across periods and down groups. Cambridge tests trends in reactivity, atomic radius, ionisation energy, melting point, and metallic/non-metallic character.

What you’ll learn

Mapped to the Cambridge IGCSE 0654 syllabus (2025-2027).

C9.4 — Describe and explain trends in atomic radius, ionisation energy, and reactivity across periods and down groups.

Trends in the Periodic Table

Atomic size, ionisation energy, and reactivity all follow predictable patterns explained by electron shell structure and nuclear charge.

Atomic radius:

Across a period (→): DECREASES. Same number of shells but increasing nuclear charge pulls electrons closer.
Down a group (↓): INCREASES. More electron shells added → greater distance from nucleus.

Ionisation energy (energy to remove 1 outer electron from gaseous atom):

Across a period (→): INCREASES. More protons pulling same shells → harder to remove electron.
Down a group (↓): DECREASES. Outer electron is further from nucleus + more shielding by inner shells → easier to remove.

Reactivity of metals (Group I):

Reactivity INCREASES down the group.
Outer electron in a larger shell (further from nucleus, more shielded) → easier to lose.
Li < Na < K < Rb < Cs (reactivity order — K reacts vigorously with water, Na moderately, Li slowly)

Reactivity of non-metals (Group VII):

Reactivity DECREASES down the group.
Harder to attract and gain an electron when the outer shell is further from the nucleus.
F > Cl > Br > I (reactivity order — F most reactive halogen)

Metallic to non-metallic character across Period 3: Na (metal) → Mg (metal) → Al (metal) → Si (metalloid) → P (non-metal) → S (non-metal) → Cl (non-metal) → Ar (noble gas)

Across period: atomic radius ↓, ionisation energy ↑, non-metallic character ↑.
Down group: atomic radius ↑, ionisation energy ↓.
Group I: reactivity ↑ down. Group VII: reactivity ↓ down.

How it’s examined

Sources: Cambridge IGCSE Coordinated Sciences 0654 syllabus 2025-2027 (C9); 0654 Examiner Reports 2022-2024. Last reviewed 2026-05-14.

Master this Topic

Worked examples, formulae, definitions and the mistakes examiners flag — everything you need to push from a pass to an A*.

Take this whole topic with you

Download a branded revision sheet — worked examples, formulae, definitions and common mistakes for Periodic Trends, ready to print or save as PDF.

Step-by-step worked examples — Periodic Trends

Step-by-step solutions to past-paper-style questions on periodic trends, written exactly the way a tutor would explain them at the board.

1Atomic radius trend across Period 3
Extended
Question
Explain why atomic radius decreases from sodium to argon across Period 3.
Step-by-step solution
1. Step 1
  Going from Na (Z=11) to Ar (Z=18), the atomic number (and therefore number of protons) increases from 11 to 18.
2. Step 2
  All elements in Period 3 have the same number of electron shells (3 shells); the outer electrons are all in the 3rd shell.
3. Step 3
  As nuclear charge increases (more protons), the nucleus attracts the outer electrons more strongly; the outer shell is pulled closer to the nucleus.
4. Step 4
  Radius decreases from Na to Ar across Period 3.
Answer
Number of protons increases (11 → 18); same number of shells (3); stronger nuclear attraction pulls outer electrons closer → atomic radius decreases across Period 3.
Examiner tip
Key phrases: 'increasing nuclear charge', 'same number of shells (shielding constant)', 'stronger attraction on outer electrons'.
2Ionisation energy trend down Group I
Extended
Question
Explain why ionisation energy decreases down Group I (from Li to Cs).
Step-by-step solution
1. Step 1
  Going down Group I, each element has one more electron shell than the element above.
2. Step 2
  The outer (valence) electron is in a shell further from the nucleus and is more shielded by inner shells from the nuclear charge.
3. Step 3
  The effective nuclear attraction on the outer electron decreases; it requires less energy to remove the outer electron.
4. Step 4
  Therefore, ionisation energy decreases down Group I.
Answer
More shells → outer electron further from nucleus → greater shielding → weaker nuclear attraction → less energy to remove outer electron → lower ionisation energy.
3Reactivity trend down Group VII
Extended
Question
State the trend in reactivity going down Group VII and explain the trend in terms of atomic structure.
Step-by-step solution
1. Step 1
  Reactivity DECREASES going down Group VII (F > Cl > Br > I).
2. Step 2
  Halogens react by gaining one electron to complete their outer shell.
3. Step 3
  Going down the group, the outer shell is further from the nucleus and more shielded by inner electrons.
4. Step 4
  It becomes harder for the nucleus to attract an incoming electron to the outer shell → decreasing reactivity.
Answer
Reactivity decreases down Group VII; the outer shell is further from the nucleus and more shielded → weaker attraction for an extra electron → less reactive.
Examiner tip
Contrast with Group I (reactivity increases down): metals react by losing electrons; easier to lose further from nucleus. Halogens react by gaining electrons; harder to attract further from nucleus.

Key Definitions and Keywords — Periodic Trends

Definitions to memorise and the exact keywords mark schemes credit for periodic trends answers — sharpened from recent examiner reports for the 2026 0654 sitting.

First ionisation energy
Examiner keyword
The energy required to remove one mole of electrons from one mole of atoms in the gaseous state to form one mole of positive ions: $X(g) \rightarrow X^+(g) + e^-$ . Increases across a period; decreases down a group.
Atomic radius
Examiner keyword
A measure of the size of an atom; decreases across a period (increasing nuclear charge) and increases down a group (additional electron shells).
Electron shielding
Examiner keyword
The reduction in the effective nuclear attraction on outer electrons caused by inner shell electrons. Greater shielding → weaker effective nuclear charge on outer electrons.
Nuclear charge
Examiner keyword
The positive charge of the nucleus, equal to the number of protons (atomic number). Increasing nuclear charge across a period increases attraction on outer electrons.
Metallic character
The tendency of an element to lose electrons and form positive ions; decreases across a period (left to right) and increases down a group.

Common Mistakes and Misconceptions — Periodic Trends

The traps other students keep falling into on periodic trends questions — taken from recent Cambridge IGCSE 0654 examiner reports and mark schemes — and how to avoid them.

✕Saying Group I reactivity decreases down the group (like Group VII)
0654 Examiner Report 2023
Why it happens
Students apply the same reactivity trend to both groups without considering whether the reaction involves gaining or losing electrons.
How to avoid it
Group I: reactivity INCREASES down (easier to LOSE outer electron). Group VII: reactivity DECREASES down (harder to GAIN electron). Always state whether electrons are lost or gained.
✕Saying 'shielding increases because there are more shells' without explaining the mechanism
Why it happens
Students state the trend without linking it to the mechanism.
How to avoid it
Explain: inner electrons repel the nuclear attraction on outer electrons → reduced effective nuclear charge on outer electrons → weaker attraction.
✕Saying atomic radius increases across a period because more electrons are added
Why it happens
Students see more electrons and assume a larger atom, ignoring the stronger nuclear charge.
How to avoid it
More electrons across a period are all in the SAME shell; the increasing nuclear charge pulls them all closer → SMALLER radius across a period.

Practice questions

Exam-style questions with step-by-step worked solutions. Try one before checking the method.

Past paper style quiz

Get a report showing which sub-topics you've nailed and which ones still need work.

Periodic Trends — frequently asked questions

The things students keep getting wrong in this sub-topic, answered.

Periodic Trends

Short Study Notes in the form of Slides

Short Study Notes — Periodic Trends

Detailed Notes

What you’ll learn

How it’s examined

1Atomic radius trend across Period 3

2Ionisation energy trend down Group I

3Reactivity trend down Group VII

First ionisation energy

Atomic radius

Electron shielding

Nuclear charge

Metallic character

✕Saying Group I reactivity decreases down the group (like Group VII)

✕Saying 'shielding increases because there are more shells' without explaining the mechanism

✕Saying atomic radius increases across a period because more electrons are added

Practice questions

Past paper style quiz

Assess your understanding

Periodic Trends — frequently asked questions

Periodic Trends

Short Study Notes in the form of Slides

Short Study Notes — Periodic Trends

Detailed Notes

What you’ll learn

How it’s examined

1Atomic radius trend across Period 3

2Ionisation energy trend down Group I

3Reactivity trend down Group VII

First ionisation energy

Atomic radius

Electron shielding

Nuclear charge

Metallic character

✕Saying Group I reactivity decreases down the group (like Group VII)

✕Saying 'shielding increases because there are more shells' without explaining the mechanism

✕Saying atomic radius increases across a period because more electrons are added

Practice questions

Past paper style quiz

Assess your understanding

Periodic Trends — frequently asked questions