Giant Structures

Học bằng cách chơi

Trả lời những câu hỏi này để kiếm năng lượng, rồi câu cá và khám phá. Không cần tài khoản.

Dành cho giáo viên: slide bài học, ghi chú ôn tập sẵn dùng cho Giant Structures (Co-ordinated Sciences (Double Award) [CIE], Chemistry) — dùng trong bài giảng của bạn, hoặc chạy chủ đề như một hoạt động lớp học tương tác để học sinh chơi như một trò chơi trực tiếp.

Ghi chú bài học

Giant Covalent Structures: Diamond & Graphite

Both diamond and graphite are allotropes of carbon with giant covalent structures.
Giant covalent structures contain billions of non-metal atoms joined by covalent bonds forming a giant lattice.
In diamond, each carbon atom bonds to four others in a tetrahedral arrangement.
In graphite, each carbon atom bonds to three others, forming layers of hexagons with one delocalised electron per atom.
Covalent bonds within graphite layers are very strong; layers are held by weak intermolecular forces.
Diamond has no free electrons – all outer electrons are in covalent bonds, so it does not conduct electricity.
Graphite conducts electricity because delocalised electrons can move between layers and carry charge.
Both have very high melting points due to strong covalent bonds requiring much energy to break.

Diamond — giant covalent structure

Properties & Uses of Diamond

Diamond is extremely hard and dense because each carbon is bonded to four others in a rigid tetrahedral structure.
It is used in cutting tools (e.g., drills) due to its hardness.
Diamond is brittle – hard but can be smashed with a hammer.
It does not conduct electricity (no delocalised electrons).

Properties & Uses of Graphite

Graphite is slippery – layers can slide over each other due to weak intermolecular forces.
Used in pencils and as an industrial lubricant because of its slipperiness.
Graphite conducts electricity – used in electrodes.
Pencil 'lead' is actually graphite, not the metal lead.

Graphite — giant covalent structure (layers)

Metallic Bonding

Metals consist of a giant lattice of positive metal ions surrounded by a 'sea of delocalised electrons'.
Metallic bond is the strong electrostatic attraction between positive ions and delocalised electrons.
Delocalised electrons are free to move throughout the structure.
Metal alloys are mixtures of metals with the same bonding type.

Metallic bonding

Properties of Metals

Most metals have high melting and boiling points due to strong metallic bonds.
Metals are good conductors of heat and electricity because delocalised electrons carry charge and energy.
Metals are malleable (can be hammered into shape) and ductile (can be drawn into wires) because layers of ions can slide over each other.
Conduction in metals is by free electrons; in molten/ aqueous ionic compounds it is by free ions.

Malleability of metals

Slide

Step through every slide for this topic — plus flashcards and revision notes — with a free account.

ĐĂNG KÝ — MIỄN PHÍ ĐĂNG NHẬP

Câu hỏi luyện tập

Xem trước miễn phí — 8 trên 56 câu hỏi. Đăng ký để xem tất cả.

1.What type of structure does graphite have?
Easy
- AGiant ionic structure
- BGiant covalent structure
- CSimple molecular structure
- DMetallic structure
2.Why does graphite conduct electricity?
Easy
- AIt has free ions
- BIt has delocalised electrons
- CIt has a giant ionic lattice
- DIt has strong covalent bonds
3.State one use of diamond that relies on its hardness.
Easy
4.Diamond conducts electricity.
Easy
True or false?
5.Complete the sentence.
Easy
In graphite, each carbon atom is bonded to ____ other carbon atoms.
6.How many carbon atoms is each carbon atom bonded to in diamond?
Easy
- A3
- B4
- C6
- D5
7.Arrange the following substances in order of increasing electrical conductivity: diamond, graphite, copper.
Medium
- diamond
- graphite
- copper
8.Match each property to the correct carbon allotrope.
Medium
- Conducts electricity
- Very hard
- Slippery layers
- Diamond
- Graphite
- Both

Thêm câu hỏi

9.Which statement explains why metals are malleable?
Medium
- AThe atoms are held together by strong covalent bonds
- BThe layers of positive ions can slide over each other
- CThe delocalised electrons are free to move
- DThe metal ions are arranged in a rigid lattice
10.Name the type of bond that holds the positive metal ions and delocalised electrons together in a metal.
Easy
11.Graphite has a high melting point because of strong covalent bonds between carbon atoms.
Medium
True or false?
12.Which of the following is NOT a property of diamond?
Easy
- AVery high melting point
- BConducts electricity
- CExtremely hard
- DDense
13.What is the structure of graphite?
Easy
- AEach carbon atom is bonded to four others forming a tetrahedral structure
- BEach carbon atom is bonded to three others forming layers of hexagons
- CEach carbon atom is bonded to two others forming chains
- DEach carbon atom is bonded to five others forming a pentagonal structure
14.Which property allows graphite to be used as a lubricant?
Easy
- AIt conducts electricity
- BIt has a high melting point
- CIts layers can slide over each other
- DIt is very hard
15.Diamond is the hardest naturally occurring mineral.
Easy
True or false?
16.Why does graphite have a high melting point?
Medium
- AIt has weak intermolecular forces between layers
- BIt contains strong covalent bonds that require a lot of energy to break
- CIt has delocalised electrons
- DIt is a giant ionic structure
17.Which of the following are properties of diamond? (Select all that apply)
Medium
- AConducts electricity
- BVery high melting point
- CExtremely hard and dense
- DSlippery
18.Metals are good conductors of electricity because they have delocalised electrons.
Easy
True or false?
19.Match each property to the correct carbon allotrope (diamond or graphite).
Medium
- Conducts electricity
- Very hard
- Slippery layers
- Does not conduct electricity
- Diamond
- Graphite
- Diamond
- Graphite
20.Arrange the following substances in order of increasing electrical conductivity (lowest to highest): diamond, graphite, copper.
Medium
- diamond
- graphite
- copper
21.Which of the following are properties of graphite? (Select all that apply)
Medium
- AConducts electricity
- BHas a high melting point
- CIs very hard
- DSlippery
22.Arrange the following in order of increasing melting point: graphite, copper, diamond.
Medium
- copper
- graphite
- diamond
23.Which property of graphite allows it to be used as a lubricant?
Medium
- AIt has delocalised electrons.
- BIt has strong covalent bonds within layers.
- CThe layers can slide over each other due to weak intermolecular forces.
- DIt has a high melting point.
24.Diamond can conduct electricity because it has delocalised electrons.
Easy
True or false?
25.A substance has a high melting point, does not conduct electricity, and is very hard. What is it most likely to be?
Medium
- AGraphite
- BDiamond
- CCopper
- DSalt (sodium chloride)
26.In an experiment to compare the electrical conductivity of diamond, graphite, and copper, a student sets up a circuit with a battery, a bulb, and the sample. Which sample(s) will cause the bulb to light up?
Easy
- Adiamond only
- Bgraphite only
- Ccopper only
- Dgraphite and copper
27.Which statement about the structure of graphite is correct?
Medium
- AEach carbon atom is bonded to four other carbon atoms.
- BThe layers are held together by strong covalent bonds.
- CEach carbon atom has one delocalised electron.
- DGraphite has a simple molecular structure.
28.A student is investigating the properties of a substance. It has a very high melting point, does not conduct electricity, and is extremely hard. Which substances could it be? (Select all that apply)
Medium
- Adiamond
- Bgraphite
- Ccopper
- Dsilicon dioxide (silica)
- Esodium chloride (solid)
29.Graphite is a good lubricant because the layers of carbon atoms can slide over each other due to weak intermolecular forces between the layers.
Easy
True or false?
30.Match each property to the correct structure (diamond or graphite).
Medium
- Has delocalised electrons
- Each carbon atom bonded to four others
- Layers can slide over each other
- Extremely hard
- Diamond
- Graphite
- Diamond
- Graphite
31.A student is given three solid samples: A, B, and C. A is very hard and does not conduct electricity. B is slippery and conducts electricity. C is malleable and conducts electricity. What are A, B, and C most likely to be?
Medium
- AA = diamond, B = graphite, C = copper
- BA = graphite, B = diamond, C = copper
- CA = diamond, B = copper, C = graphite
- DA = copper, B = graphite, C = diamond
32.In graphite, each carbon atom is bonded to four other carbon atoms.
Easy
True or false?
33.Which type of structure do diamond and graphite have?
Easy
- AGiant covalent structure
- BGiant ionic structure
- CSimple molecular structure
- DMetallic structure
34.Graphite conducts electricity because it has delocalised electrons.
Easy
True or false?
35.What type of bonding occurs in metals?
Easy
- AIonic bonding
- BCovalent bonding
- CMetallic bonding
- DIntermolecular bonding
36.Diamond is a good conductor of electricity.
Easy
True or false?
37.Which property of graphite makes it useful as a lubricant?
Easy
- AIt has a high melting point
- BIt conducts electricity
- CThe layers can slide over each other
- DIt is very hard
38.Metals are malleable because the layers of atoms can slide over each other when force is applied.
Easy
True or false?
39.Why does diamond have a very high melting point?
Medium
- AIt has weak intermolecular forces
- BIt has strong covalent bonds that require lots of energy to break
- CIt has delocalised electrons
- DIt has a simple molecular structure
40.Which statement explains why diamond is extremely hard?
Medium
- AEach carbon atom is bonded to three others, forming layers that can slide.
- BEach carbon atom is bonded to four others in a tetrahedral structure with strong covalent bonds.
- CThere are weak intermolecular forces between the layers of carbon atoms.
- DDiamond contains delocalised electrons that hold the structure together.
41.Graphite conducts electricity because it has delocalised electrons that are free to move between the layers.
Easy
True or false?
42.Match each substance to its correct electrical conductivity property.
Medium
- Diamond
- Graphite
- Copper
- Does not conduct electricity
- Conducts electricity due to delocalised electrons
- Conducts electricity due to delocalised electrons in a metallic lattice
43.Arrange the following substances in order of increasing electrical conductivity (lowest to highest).
Medium
- Diamond
- Graphite
- Copper
44.State one use of graphite that relies on its slipperiness.
Easy
45.In diamond, each carbon atom is bonded to how many other carbon atoms?
Easy
46.In a sample of graphite, if there are 6.02 × 10²³ carbon atoms, how many delocalised electrons are present? (Assume each carbon atom contributes one delocalised electron.)
Medium
47.Complete the sentences about the structure of graphite.
Medium
In graphite, each carbon atom is bonded to ____ other carbon atoms, and there is one ____ electron per carbon atom.
48.Complete the sentence about metallic bonding.
Medium
In metallic bonding, the positive metal ions are held together by a '____ of electrons' formed from ____ outer electrons.
49.Explain why graphite can conduct electricity.
Medium
50.Complete the sentences about the properties of metals.
Easy
Metals are ____ because the layers of atoms can slide over each other when a force is applied. They are good conductors of electricity because they have ____ electrons.
51.Explain why graphite has a high melting point.
Medium
52.Explain why diamond has a very high melting point.
Medium
53.Explain why metals are malleable.
Medium
54.Explain why graphite has a high melting point and why it can conduct electricity. Refer to the structure and bonding in your answer.
Hard
55.In diamond, each carbon atom is bonded to how many other carbon atoms?
Easy
- A5
- B6
- C3
- D4
56.In a sample of graphite, if there are 6.02 × 10²³ carbon atoms, how many delocalised electrons are present? (Assume each carbon atom contributes one delocalised electron.)
Easy
- A6.622e+23 electrons
- B5.418e+23 electrons
- C6.02e+23 electrons
- D7.224000000000001e+23 electrons

Thẻ ghi nhớ

What is a giant covalent structure?

A giant covalent structure contains billions of non-metal atoms, each joined to adjacent atoms by covalent bonds forming a giant lattice structure.

What are allotropes?

Allotropes are different structural forms of the same element, such as diamond and graphite for carbon.

Describe the structure of graphite.

Each carbon atom in graphite is bonded to three others forming layers of hexagons, with one free electron per carbon atom that becomes delocalised. The layers are held together by weak intermolecular forces.

Why does graphite conduct electricity?

Graphite conducts electricity because each carbon atom has one delocalised electron that is free to move between the layers and carry charge.

Why does graphite have a high melting point?

Graphite has a high melting point because it has a giant covalent structure with strong covalent bonds between carbon atoms that require a lot of energy to break.

Why is graphite slippery?

Graphite is slippery because its layers are held together by weak intermolecular forces, allowing them to slide over each other.

What are two uses of graphite based on its properties?

Graphite is used in pencils and as an industrial lubricant because its layers can slide over each other.

Describe the structure of diamond.

In diamond, each carbon atom bonds with four other carbons, forming a tetrahedron. All covalent bonds are identical and very strong, with no intermolecular forces.

Why does diamond not conduct electricity?

Diamond does not conduct electricity because all outer shell electrons are held in the four covalent bonds around each carbon atom, so there are no free-moving charged particles.

Why does diamond have a very high melting point?

Diamond has a very high melting point because it has a giant covalent structure with strong covalent bonds that require a lot of energy to break.

Why is diamond extremely hard?

Diamond is extremely hard because each carbon atom is bonded to four other carbon atoms by strong covalent bonds, forming a rigid tetrahedral structure.

What is a common use of diamond based on its hardness?

Diamond is used in cutting tools like drills because of its extreme hardness.

What is the difference between hard and strong?

Hard means resistant to scratching or indentation, while strong means able to withstand force without breaking. Diamond is hard but brittle.

What is metallic bonding?

Metallic bonding is the strong electrostatic attraction between positive metal ions and delocalised electrons in a giant metallic lattice.

Describe the structure of a metal.

Metals consist of a giant lattice of positive metal ions surrounded by a 'sea' of delocalised electrons that are free to move.

Why do most metals have high melting and boiling points?

Metals have high melting and boiling points because strong electrostatic forces between positive ions and delocalised electrons require a lot of energy to overcome.

Why are metals good conductors of electricity?

Metals conduct electricity because delocalised electrons are free to move and carry charge through the structure.

Why are metals malleable?

Metals are malleable because their atoms are arranged in layers that can slide over each other when force is applied.

Why are metals ductile?

Metals are ductile because their atoms are arranged in layers that can slide over each other, allowing them to be pulled into wires.

What is the difference between conduction in metals and in molten ionic compounds?

Metals conduct electricity via free electrons, while molten or aqueous ionic compounds conduct via free ions.

What are delocalised electrons?

Delocalised electrons are electrons that are not associated with a particular atom and are free to move throughout the structure, as seen in graphite and metals.

Unlock all 56 questions, flashcards & more

Tạo tài khoản miễn phí để xem mọi câu hỏi, slide, thẻ ghi nhớ và ghi chú ôn tập cho chủ đề này.

ĐĂNG KÝ — MIỄN PHÍ ĐĂNG NHẬP

Đề thi cũ

Luyện đề thi cũ cho chủ đề này sắp ra mắt.

Sắp ra mắt