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GCSE Science Edexcel 2016 Onwards > Chemistry - Topic 2 - Structure and Bonding > Flashcards

Chemistry - Topic 2 - Structure and Bonding Flashcards

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1
Q

Definition of a compound

A

Two or more elements which are chemically combined

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2
Q

Definition of Covalent Bonding

A

Shared pair of electrons

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3
Q

Definition of Ionic Bonding

A

(electrostatic) attraction between oppositely charged ions

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4
Q

Describe the structure of NaCl

A
  • Giant ionic lattice (structure)
  • electrostatic attraction
  • Between Na+ and Cl-
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5
Q

Type of bonding in graphite

A

Covalent

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6
Q

Describe the structure of diamond

A

Giant covalent structure where each carbon has 4 bonds

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7
Q

Describe the structure of graphite

A

Giant covalent structure where each carbon has 3 bonds. It is arranged in layers.

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8
Q

Definition of Metallic Bonding

A

(electrostatic) attraction between positive metal ions and the delocalised electrons

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9
Q

Type of bonding in CO2

A

Covalent

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10
Q

Describe the structure of CO2

A

Simple molecular

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11
Q

Identify the bonding in H2O and describe its structure

A
  • Covalent
  • Simple molecular
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12
Q

Identify the type of bonding in copper and describe its structure

A
  • Metallic
  • Giant metallic lattice
  • Positive ions surrounded by delocalised electrons
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13
Q

Identify the type of bonding in sodium chloride and describe its structure

A
  • Ionic
  • Giant ionic lattice
  • Electrostatic attraction between positive ions and negative ions
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14
Q

Identify the type of bonding in Ca(OH)2 and describe its structure

A
  • Ionic
  • Giant ionic lattice
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15
Q

Identify the type of bonding in SiO2 and describe its structure

A
  • Covalent
  • Giant covalent lattice/structure (giant molecular)
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16
Q

Graphite, diamond, nanotubes and fullerenes are all _________________ of carbon

A

allotropes

17
Q

Explain why NaCl is a solid at room temperature

A
  • It has a giant ionic lattice
  • It is held together by ionic bonds which are very strong
  • and require a lot of energy to break
  • Therefore it has a high melting point
18
Q

Explain why oxygen is a gas at room temperature

A
  • It has a simple molecular structure
  • It is held together by weak intermolecular forces
  • which require little energy to overcome
  • Therefore it has a low melting point
19
Q

Explain why iron is a solid at room temperature

A
  • It has a giant metallic structure
  • It is held together by strong metallic bonds
  • Therefore it has a high melting point
20
Q

Explain why iron conducts electricity as a solid and liquid

A

It has delocalised electrons which are free to move throughout the metal structure

21
Q

Explain why graphite conducts electricity

A
  • Each carbon has only 3 bonds.
  • This leaves one delocalised electron
  • Which is free to move throughout the structure
22
Q

Explain why diamond doesn’t conduct electricity

A

Each carbon has 4 bonds.It has no free electrons

23
Q

Explain why sodium chloride doesn’t conduct electricity as a solid

A

The ions can’t move and carry the charge

24
Q

Explain why sodium chloride conducts electricity when dissolved

A

The ions are free to move and carry the charge

25
Q

Explain why carbon dioxide doesn’t conduct electricity

A

Its electrons aren’t free to move and carry the charge

26
Q

Explain why molten magnesium chloride can conduct electricity

A

The ions are free to move and carry the charge

27
Q

Explain why methane is a gas at room temperature

A
  • It is a simple molecular substance
  • It is held together by weak intermolecular forces
  • which require little energy to break
  • Therefore it has a low melting point
28
Q

Explain why graphite has a very high melting point

A
  • It has a giant covalent structure
  • which is held together by strong covalent bonds
  • which require a lot of energy to break
29
Q

What property makes diamond useful for sharpening knives

A

It is very hard

30
Q

Explain why diamond is so hard

A
  • It is arranged in a giant lattice
  • Each carbon has 4 bonds
  • the covalent bonds are strong
31
Q

Explain why copper is used to make wires rather than graphite

A
  • Copper and graphite both conduct electricity
  • Copper and graphite both have a high melting point
  • Graphite is soft and brittle
  • Copper is strong and ductile
32
Q

Name properties you would expect of an ionic compound?

A
  • High melting point
  • Doesn’t conduct electricity when solid
  • Conducts electricity when molten or in solution
33
Q

Name properties you’d expect of a simple covalent solid

A
  • Low melting point
  • Brittle
  • Dull
  • Soft
34
Q

Name properties you’d expect of a metal

A
  • High melting point
  • Conducts heat and electricity
  • Hard
  • Lustrous (shiny)
  • Malleable (can be hammered into shape)
  • Ductile ( can be drawn into wires)
35
Q

What is meant by the term diatomic?

A

molecule containing two atoms

36
Q

Name the diatomic elements

A

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine(I Bring Clay For Our New House)(Have NO Fear Ice Cold Beer)

GCSE Science Edexcel 2016 Onwards (11 decks)

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