GCSE · Chemistry · AQA · Spec 8462

Graphite

Graphite is made only of carbon, yet it conducts electricity and feels soft — both properties come from the way its atoms are arranged.

Relationship matrix

Tap any cell to reveal it. Tap a column header to read one property down every item.

Structure / bonding factProperty it explains
Inside each layercarbon network
Between layersno covalent bonds
Delocalised electronsone per carbon

Each cell hides a short answer and the reason behind it. Predict before you tap.

Which feature matters?

Look for the feature graphite shares with metals.

Which feature best explains why graphite can conduct electricity?

Why is graphite soft and slippery?

?

Reason it through

How do graphite's layers lead to its soft, slippery property?

Link 1 of 4

First link · your turn

How are carbon atoms arranged in graphite?

2
Locked — reveal the link above first
3
Locked — reveal the link above first
4
Locked — reveal the link above first

From carbon atom to graphite properties

13 bonds234

Stage 1 of 4: 3 bonds. paused

3 bonds · 1/4Scrub from bonding to properties.

Each carbon bonds to three others.

Follow the structure-to-property chain from one carbon atom outward.

CHEMISTRY

See how flat carbon layers and delocalised electrons give graphite its unusual properties.

What you need to know

  • Each carbon atom in graphite forms three covalent bonds with three other carbon atoms.
  • The atoms form layers of hexagonal rings with no covalent bonds between neighbouring layers.
  • One electron from each carbon atom is delocalised.
  • Delocalised electrons explain conduction; sliding layers explain why graphite is soft and slippery.

The big picture

Graphite is built from layers of carbon atoms. Its delocalised electrons explain electrical conduction, while the lack of covalent bonds between layers explains why those layers can slide.

Key points

1Each carbon atom in graphite forms three covalent bonds with three other carbon atoms.
2The carbon atoms form layers of hexagonal rings.
3There are no covalent bonds between neighbouring layers.
4One electron from each carbon atom is delocalised.
5Delocalised electrons can move and carry charge, so graphite conducts electricity.
6The layers can slide over one another, so graphite is soft and slippery.
7Graphite is similar to metals because both have delocalised electrons.

Worked example

Problem

Explain why graphite conducts electricity and is soft.

🧠

Memory hook

Three bonds make the layer; one electron roams; layers slide.

★ Exam tip

For a structure–property explanation, name the structural feature and then state how that feature causes the property. Do not stop at 'graphite has layers'.

⚠ Watch out

Do not say the delocalised electrons move between the layers to make them slide. Delocalised electrons explain conduction; the lack of covalent bonds between layers explains sliding.

✓

Check yourself

Without looking: which graphite feature explains conduction, and which feature explains softness?

Flashcards

(20)
How many covalent bonds does each carbon form in graphite?
Three.
How many other carbon atoms is each carbon bonded to in graphite?
Three.
What shape do carbon atoms form within graphite layers?
Hexagonal rings.
How is graphite organised overall?
As layers of hexagonal carbon rings.
Are there covalent bonds between graphite layers?
No.
How many electrons from each carbon atom are delocalised?
One.
What does 'delocalised electron' mean here?
An electron that is not confined to one covalent bond and can move through the structure.
Which graphite feature explains electrical conduction?
Its mobile delocalised electrons.
Why can delocalised electrons make graphite conduct?
They can move through the structure and carry electrical charge.
Which graphite feature explains softness?
Its layered structure with no covalent bonds between layers.
Why can graphite layers slide?
There are no covalent bonds locking neighbouring layers together.
What property results from the layers sliding?
Graphite is soft and slippery.
What similarity does graphite have with metals?
Both contain delocalised electrons.
Complete the chain: no covalent bonds between layers → ?
Layers can slide → graphite is soft and slippery.
Complete the chain: one delocalised electron per carbon → ?
Electrons can move → graphite conducts electricity.
What type of bonding holds carbon atoms together within a graphite layer?
Covalent bonding.
Do the delocalised electrons explain graphite's softness?
No. They explain electrical conduction.
Do weak or absent covalent bonds within a layer explain softness?
No. The key point is that there are no covalent bonds between the layers.
What must a good graphite property explanation include?
The property, the relevant structure/bonding feature, and the causal link between them.
Give the two main properties explained in this lesson.
Electrical conduction and softness/slipperiness.

Tap any card to flip it, or use Study as deck to go through them one at a time. In the full lesson these run as a spaced-repetition deck — you rate each card Hard, Good or Easy and the tricky ones keep coming back until they stick.

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