Giant Structures

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Notes

Introduction to Giant Structures

**Giant covalent structures** contain billions of non-metal atoms joined by **strong covalent bonds** in a giant lattice.
Diamond and graphite are **allotropes of carbon** – same element, different bonding arrangements.
Giant structures have very high melting points due to many strong bonds.
Silicon(IV) oxide (SiO₂) is also a giant covalent compound.

Diamond – Structure & Properties

Each carbon atom bonds to **four others** in a **tetrahedral** arrangement.
All bonds are **identical, very strong covalent bonds**; no intermolecular forces.
**Does not conduct electricity** – all outer electrons are used in bonds.
**Extremely hard** and dense – used in cutting tools and drills.
**Very high melting point** – many strong bonds need lots of energy to break.
Hard but **brittle** (can be smashed with a hammer).

Graphite – Structure & Properties

Each carbon atom bonds to **three others**, forming **layers of hexagons**.
One **delocalised electron** per carbon atom is free to move between layers.
**Conducts electricity** – delocalised electrons carry charge.
**High melting point** – strong covalent bonds within layers.
**Slippery** – layers held by **weak intermolecular forces** can slide over each other.
Used as a **lubricant**, in **pencils**, and as **electrodes** (unreactive, conducts).

Silicon(IV) Oxide (SiO₂)

**Giant covalent structure** – each Si bonds to **4 O** atoms, each O bonds to **2 Si** atoms.
Forms a **tetrahedral** arrangement similar to diamond.
**Very hard**, **high melting point**, **insoluble in water**, **does not conduct electricity**.
Occurs naturally as **sand** and **quartz**.
Used to make **sandpaper** and to **line furnaces** (cheap, heat-resistant).

Metallic Bonding

Metals consist of a **giant lattice** of **positive metal ions** surrounded by a **‘sea of delocalised electrons’**.
The **metallic bond** is the electrostatic attraction between positive ions and delocalised electrons.
**High melting/boiling points** – strong metallic bonds require lots of energy to break.
**Good conductors of heat and electricity** – delocalised electrons move freely.
**Malleable** and **ductile** – layers of ions can slide over each other without breaking bonds.

Diamond (tetrahedral), graphite (layered), and metallic bonding (positive ions in sea of electrons).

Practice questions

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1.Which statement about carbon allotropes is correct?
Easy
- ADiamond contains carbon atoms bonded to three other carbon atoms.
- BGraphite is a good conductor of electricity because of the presence of mobile ions.
- CDiamond is used as a lubricant because of the weak intermolecular forces between its layers.
- DGraphite is a good conductor of electricity because it contains delocalised electrons.
2.Which row describes how graphite can be used in electrolysis?
Easy
- ADelocalised electrons – conducts electricity
- BDelocalised electrons – acts as an insulator
- CLow melting point – acts as an insulator
- DLow melting point – conducts electricity
3.Which statement correctly describes the bonding in metals?
Easy
- AA lattice of negative ions in a 'sea of electrons'.
- BA lattice of positive ions in a 'sea of electrons'.
- CA lattice of neutral atoms with delocalised electrons.
- DA lattice of negative ions with delocalised electrons.
4.Which row provides a correct description of the properties of metals?
Easy
- Amelting point high, boiling point low, conducts electricity yes
- Bmelting point low, boiling point high, conducts electricity yes
- Cmelting point low, boiling point low, conducts electricity no
- Dmelting point high, boiling point high, conducts electricity yes
5.What other property does graphite have that makes it useful for electrodes?
Easy
- AGraphite is an unreactive substance and doesn’t react with the electrolyte.
- BGraphite is soft and easy to shape into electrodes.
- CGraphite has a low melting point due to the weak forces in between the layers.
- DGraphite dissolves readily in water.
6.Which of the following statements about graphite and diamond are incorrect? 1 They are allotropes of carbon. 2 They both conduct electricity. 3 They form different numbers of bonds within their structures. 4 They have different uses.
Medium
- A2 and 3
- B2 only
- C1, 3 and 4
- D2 and 4
7.Which statement correctly describes the structure of macromolecules?
Medium
- AGiant molecular crystal which is held together by weak intermolecular forces.
- BGiant molecular crystal which is held together by strong ionic bonds.
- CGiant molecular crystal which is held together by weak metallic bonds.
- DGiant molecular crystal which is held together by strong covalent bonds.
8.Which statement about graphite and diamond is not correct?
Medium
- AGraphite is a good lubricant due to the weak forces in between the layers.
- BDiamond is used as a drill tip because it is an extremely hard substance.
- CGraphite has a low melting point due to the weak forces in between the layers.
- DDiamond is an allotrope of carbon.

More questions

9.The following statements describe the structure and properties of silicon(IV) oxide. 1. Giant covalent structure held together by many strong covalent bonds. 2. It is a very hard substance. Which of the following is correct for statements 1 and 2?
Medium
- AStatement 2 is correct but statement 1 is incorrect.
- BBoth statements are incorrect.
- CBoth are correct and statement 1 explains statement 2.
- DBoth are correct and statement 2 explains statement 1.
10.Statements 1, 2 and 3 are about diamond and graphite. 1. They have atoms that form three equally strong bonds 2. They are both formed from the same element 3. They each conduct electricity Which statement(s) is / are correct?
Medium
- A1 only
- B2 only
- C1 and 3
- D1 and 2
11.Silicon(IV) oxide and phosphorus(V) oxide are oxides of elements in Period 3 of the Periodic Table. Which row describes the correct properties of these two oxides?
Medium
- Anature acidic, type of bonding covalent, melting point of SiO2 high, melting point of P4O10 low
- Bnature acidic, type of bonding covalent, melting point of SiO2 low, melting point of P4O10 low
- Cnature basic, type of bonding ionic, melting point of SiO2 high, melting point of P4O10 low
- Dnature basic, type of bonding ionic, melting point of SiO2 low, melting point of P4O10 low
12.Which statement correctly describes the arrangement of atoms in silicon dioxide?
Hard
- AEach silicon atom is bonded to two oxygen atoms and each oxygen atom is bonded to one silicon atom.
- BEach silicon atom is bonded to four oxygen atoms and each oxygen atom is bonded to two silicon atoms.
- CEach silicon atom is bonded to four oxygen atoms and each oxygen atom is bonded to four silicon atoms.
- DEach silicon atom is bonded to two oxygen atoms and each oxygen atom is bonded to four silicon atoms.
13.Which of the following statements about silicon(IV) dioxide and diamond are correct? 1 Silicon(IV) dioxide forms a giant ionic lattice structure. 2 They are both compounds. 3 They both have very high melting points. 4 There are strong covalent bonds in silicon(IV) dioxide.
Hard
- A1 and 3
- B1 only
- C1, 2 and 4
- D3 and 4
14.Which row correctly describes the use of graphite and silicon(IV) dioxide?
Hard
- Agraphite: electrodes, silicon(IV) dioxide: production of plastics
- Bgraphite: electrolyte, silicon(IV) dioxide: production of glass
- Cgraphite: electrolyte, silicon(IV) dioxide: production of plastics
- Dgraphite: electrodes, silicon(IV) dioxide: production of glass
15.Which row provides a correct description of the structure and properties of silicon(IV) oxide? (✓ = yes, × = no)
Hard
- Aforms an acidic oxide: ✓, has a giant structure: ✓, conducts electricity: ×
- Bforms an acidic oxide: ✓, has a giant structure: ×, conducts electricity: ✓
- Cforms an acidic oxide: ×, has a giant structure: ✓, conducts electricity: ×
- Dforms an acidic oxide: ×, has a giant structure: ×, conducts electricity: ✓
16.Metallic bonds are very strong and give metals their properties. Which of the following definitions is correct for a metallic bond?
Hard
- AA metallic bond is formed by the electrostatic attraction that occurs due to electron transfer between metal atoms.
- BA metallic bond is formed by the electrostatic attraction between the positive ions and the delocalised electrons.
- CA metallic bond is formed by the electrostatic attraction that occurs due to the uneven sharing of electrons between metal atoms.
- DA metallic bond is formed by the intermolecular forces between the positive metal ions and the delocalised electrons.
17.Metals are malleable and ductile and can be hammered and pulled into useful shapes. Which statement correctly explains these properties?
Hard
- ALayers of atoms in the metal lattice are rigid and held strongly together so they cannot move.
- BLayers of atoms in a metal can slide over one another and break the attractive forces that hold them together.
- CLayers of atoms in a metal can slide over one another and new attractive forces are formed between the metal ions and the delocalised electrons.
- DLayers of atoms in a metal cannot slide over one another and the attractive forces between the metal ions and the delocalised electrons are unbreakable.
18.Which of the following is an allotrope of carbon?
Easy
- ASilicon dioxide
- BGraphite
- CSodium chloride
- DCarbon dioxide
19.Why does diamond have a very high melting point?
Easy
- AIt has weak intermolecular forces between layers.
- BIt has strong covalent bonds throughout the structure.
- CIt has delocalised electrons that require much energy to move.
- DIt has ionic bonds between carbon atoms.
20.Which property allows graphite to be used as a lubricant?
Medium
- AIt has delocalised electrons.
- BIt has a high melting point.
- CThe layers can slide over each other due to weak forces between them.
- DIt is hard and dense.
21.In metallic bonding, the delocalised electrons are responsible for which property?
Medium
- AHigh melting point only
- BElectrical conductivity only
- CBoth electrical conductivity and malleability
- DNeither electrical conductivity nor malleability
22.Which statement best explains why silicon(IV) oxide is hard and has a high melting point?
Hard
- AIt has a giant ionic lattice with strong electrostatic forces.
- BIt has a giant covalent structure with many strong covalent bonds.
- CIt has simple molecules held by strong intermolecular forces.
- DIt has a metallic lattice with delocalised electrons.
23.Which of the following substances does NOT conduct electricity in any state?
Hard
- AGraphite (solid)
- BCopper (solid)
- CSilicon(IV) oxide (solid)
- DMolten sodium chloride
24.The structures of two solids X and Y are shown below. X has layers of hexagonal rings with weak forces between layers, and Y has a tetrahedral arrangement with each atom bonded to four others. What are the correct uses of these structures?
Medium
- AX: industrial lubricant; Y: glass cutter
- BX: industrial lubricant; Y: industrial lubricant
- CX: glass cutter; Y: industrial lubricant
- DX: glass cutter; Y: glass cutter
25.Graphite is used to produce electrodes due to its ability to conduct electricity. What other property does graphite have that makes it useful for this application?
Medium
- AGraphite is unreactive and does not react with the electrolyte.
- BGraphite is soft and easy to shape into electrodes.
- CGraphite has a low melting point due to weak forces between layers.
- DGraphite dissolves readily in water.
26.Silicon(IV) oxide and phosphorus(V) oxide are oxides of elements in Period 3. Which row describes the correct properties of these two oxides?
Hard
- Anature: acidic, bonding: covalent, melting point SiO2: high, melting point P4O10: low
- Bnature: acidic, bonding: covalent, melting point SiO2: low, melting point P4O10: low
- Cnature: basic, bonding: ionic, melting point SiO2: high, melting point P4O10: low
- Dnature: basic, bonding: ionic, melting point SiO2: low, melting point P4O10: low
27.In an experiment, a student tests the electrical conductivity of four solids. Which solid is most likely to conduct electricity as a solid?
Medium
- ADiamond
- BSilicon(IV) oxide
- CGraphite
- DSodium chloride
28.A student is given a sample of a white solid. It is very hard, has a very high melting point, and does not conduct electricity in any state. What is the most likely identity of the solid?
Hard
- AGraphite
- BSilicon(IV) oxide
- CCopper
- DSodium chloride
29.Which property of graphite is correctly explained by its structure?
Medium
- AIt is hard because of strong covalent bonds between layers.
- BIt conducts electricity because of delocalised electrons between layers.
- CIt has a low melting point because of weak covalent bonds within layers.
- DIt is slippery because of strong covalent bonds between layers.
30.Which statement about diamond is correct?
Easy
- ADiamond contains carbon atoms bonded to three other carbon atoms.
- BDiamond is a good conductor of electricity.
- CDiamond is used as a lubricant because of weak forces between layers.
- DDiamond is an allotrope of carbon.
31.Which row correctly describes the structure and bonding in silicon(IV) oxide?
Medium
- AGiant ionic lattice, strong electrostatic forces
- BGiant covalent lattice, strong covalent bonds
- CGiant metallic lattice, delocalised electrons
- DSimple molecular, weak intermolecular forces
32.A student is asked to design an experiment to compare the hardness of diamond and silicon(IV) oxide. Which method would be most appropriate?
Hard
- AMeasure the electrical conductivity of each substance.
- BTry to scratch each substance with a steel nail.
- CHeat each substance and record the temperature at which it melts.
- DAdd each substance to water and check for solubility.
33.Which statement explains why metals are malleable?
Medium
- AThe layers of atoms can slide over each other because the metallic bonds are weak.
- BThe layers of positive ions can slide over each other and new metallic bonds form.
- CThe atoms are held together by strong covalent bonds that break easily.
- DThe delocalised electrons prevent the layers from moving.
34.Which substance has a giant covalent structure?
Easy
- ASodium chloride
- BGraphite
- CCopper
- DIce
35.A student measures the electrical conductivity of a substance in solid and molten states. The results show it does not conduct when solid but conducts when molten. What type of structure does the substance most likely have?
Hard
- AGiant covalent
- BGiant ionic
- CGiant metallic
- DSimple molecular
36.Which row correctly describes the uses of graphite and silicon(IV) oxide?
Medium
- AGraphite: electrodes; Silicon(IV) oxide: production of glass
- BGraphite: production of glass; Silicon(IV) oxide: electrodes
- CGraphite: lubricant; Silicon(IV) oxide: production of plastics
- DGraphite: cutting tools; Silicon(IV) oxide: lubricant
37.In an experiment to test the hardness of two solids, a student tries to scratch each with a piece of quartz. Solid A is scratched, solid B is not. What can be concluded?
Hard
- ASolid A is harder than quartz.
- BSolid B is harder than quartz.
- CBoth solids are harder than quartz.
- DQuartz is harder than both solids.
38.Which property of graphite allows it to be used as a lubricant?
Easy
- AIt has a high melting point.
- BIt conducts electricity.
- CIt has weak forces between layers.
- DIt is hard.
39.Which statement correctly describes the structure of diamond?
Easy
- AEach carbon atom is bonded to three other carbon atoms, forming layers of hexagons.
- BEach carbon atom is bonded to four other carbon atoms, forming a tetrahedral structure.
- CEach carbon atom is bonded to two other carbon atoms, forming chains.
- DEach carbon atom is bonded to four other carbon atoms, forming layers of hexagons.
40.What is the main reason graphite can conduct electricity?
Easy
- AIt has strong covalent bonds within layers.
- BIt has weak forces between layers.
- CIt contains delocalised electrons.
- DIt is an allotrope of carbon.

Slides

Giant Covalent Structures

Giant covalent structures contain billions of non-metal atoms joined by covalent bonds in a lattice.
Diamond and graphite are allotropes of carbon with giant covalent structures.
Silicon(IV) oxide (SiO₂) is another example, found as sand and quartz.

Structure of Diamond

Each carbon atom bonds to four others, forming a tetrahedral structure.
All covalent bonds are identical, very strong, and there are no intermolecular forces.

How many carbon atoms does each carbon atom bond to in diamond?

Structure of Graphite

Each carbon atom bonds to three others, forming layers of hexagons.
One electron per carbon atom becomes delocalised, free to move between layers.
Strong covalent bonds within layers, but weak intermolecular forces between layers.

Why does graphite conduct electricity?

It has free ions
It has delocalised electrons
It has weak intermolecular forces
It has a high melting point

Which of these are properties of graphite?

Conducts electricity
Very hard
Slippery / lubricant
High melting point

Properties and Uses of Diamond

Diamond does not conduct electricity (all electrons held in bonds).
It has a very high melting point due to strong covalent bonds.
It is extremely hard and dense, used in cutting tools and drills.

Why is diamond used in drill tips?

It conducts electricity
It is very hard
It has a low melting point
It is slippery

Silicon(IV) Oxide (SiO₂)

Each silicon atom bonds to four oxygen atoms; each oxygen bonds to two silicon atoms.
It has a giant covalent structure similar to diamond.
It is very hard, has a high melting point, does not conduct electricity, and is insoluble in water.

Silicon(IV) oxide has a ____ covalent structure and does not conduct ____.

Metallic Bonding

Metals consist of a lattice of positive metal ions surrounded by a 'sea' of delocalised electrons.
The metallic bond is the electrostatic attraction between positive ions and delocalised electrons.
This bonding occurs in metals and alloys.

What is the metallic bond?

Attraction between positive ions and delocalised electrons
Attraction between positive and negative ions
Covalent bonds between metal atoms
Intermolecular forces between metal atoms

Properties of Metals

High melting and boiling points due to strong metallic bonds.
Good conductors of heat and electricity because delocalised electrons carry charge.
Malleable and ductile because layers of ions can slide over each other.

Which of these are properties of metals?

High melting point
Conduct electricity when solid
Brittle
Malleable

Why are metals malleable?

Strong covalent bonds break easily
Layers of ions slide over each other
Delocalised electrons hold layers rigid
Metallic bonds are weak

In metallic bonding, the outer electrons become ____ and form a '____ of electrons'.

Comparing Giant Structures

Diamond: each C bonded to 4 others, very hard, no conductivity.
Graphite: each C bonded to 3 others, layers, conducts electricity, slippery.
SiO₂: each Si bonded to 4 O, hard, no conductivity.
Metals: positive ions in sea of electrons, conduct, malleable.

Which of the following does NOT conduct electricity?

Graphite
Copper
Diamond
Iron

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