1.5 Metals Flashcards Preview

GCSE Chemistry 2.1 Structure and Bonding > 1.5 Metals > Flashcards

Flashcards in 1.5 Metals Deck (17)
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1
Q

What happens to the electrons in the highest energy levels?

A

They delocalise and can move freely between atoms

2
Q

What does delocalise mean?

A

They can move freely around the atoms

3
Q

What does delocalised electrons cause?

A

A lattice of positive ions in a sea of moving electrons

4
Q

Why are metallically bonded atoms always positively charged?

A

They lose their electrons when they become delocalised so they have more protons than electrons

5
Q

How do the positive ions stay together in metallic bonding?

A

The delocalised electrons strongly attract the positive ions and hold them together

6
Q

What forces hold metal ions in their place in their giant structures?

A

Electrostatic forces between positive metal ions and delocalised electrons

7
Q

Why can metals conduct electricity?

A

They are metallically bonded so their delocalised electrons can move quickly so a current can flow

8
Q

Why can’t magnesium oxide conduct electricity?

A

It is ionically bonded so it’s electrons are all tied up holding the compound together

9
Q

Why doesn’t magnesium oxide dissolve in water?

A

Magnesium oxide is charged 2+ whereas water is only charged 1- so it is not strong enough to pull the magnesium oxide apart

10
Q

Explain the physical appearance before, during and after bonding magnesium and oxygen

A

Before: silver, shiny, sturdy, metal
During: shining, blindingly bright, on fire, white light, energy given out
After: White, crumbling, breaks easily, chalk like, powder

11
Q

Why isn’t silicon dioxide soluble in water?

A

It is covalently bonded so it has no charge

12
Q

What is silicon dioxide?

A

Sand

13
Q
Fact file for copper: 
Appearance: 
Hardness: 
Conduct electricity as a solid:
Conducts electricity as a water solution: 
Soluble in water: 
Melting point: 
Boiling point: 
Structure: 
Bonding:
A
  • bronzey brown
  • malleable
  • yes
  • no
  • no
  • medium high
  • medium high
  • giant lattice structure
  • metallic bond
14
Q
Fact file for sodium chloride:
Appearance: 
Hardness: 
Conduct electricity as a solid:
Conducts electricity as a water solution: 
Soluble in water: 
Melting point: 
Boiling point: 
Structure: 
Bonding:
A
  • white powder
  • solid but soft
  • no
  • yes
  • no
  • medium high
  • medium high
  • lattice
  • ionic bond
15
Q
Fact file for sulphur:
Appearance: 
Hardness: 
Conduct electricity as a solid:
Conducts electricity as a water solution: 
Soluble in water: 
Melting point: 
Boiling point: 
Structure: 
Bonding:
A
  • yellow powder
  • solid but soft, fluffy
  • no
  • no
  • no
  • quite low
  • quite low
  • covalent structure
  • covalent bond/no charge
16
Q
Fact file for silicon dioxide: 
Appearance: 
Hardness: 
Conduct electricity as a solid:
Conducts electricity as a water solution: 
Soluble in water: 
Melting point: 
Boiling point: 
Structure: 
Bonding:
A
  • brown powder
  • grainy
  • no
  • yes
  • no
  • really high
  • really high
  • giant covalent structure
  • covalent bond
17
Q

What structures are formed by metallic bonding?

A

Giant layered structures in which layers of atoms are arranged in regular patterns as they are all the same size