Metallic bonding- page 25

?
  • Created by: emj790
  • Created on: 20-03-17 19:37
What does Metallic bonding involve?
Delocalised electrons
1 of 33
What do metals consist of?
Giant structures
2 of 33
What are delocalised?
The electrons in the outer shell of the metal atoms
3 of 33
What does delocalised mean?
Free to move around
4 of 33
What is between the positive metal ions and shared negative electrons?
Strong forces of electrostatic attraction
5 of 33
Where are there forces of electrostatic attraction?
Between the positive metals ions and shared negative electrons
6 of 33
What do the forces of attraction do?
They hold the atoms together
7 of 33
How do they hold them together?
In a regular structure
8 of 33
What is it known as?
Metallic bonding
9 of 33
What is the strength of metallic bonding? (strong or weak?)
It is strong
10 of 33
What compounds are held together by metallic bonding?
Metallic elements and alloys
11 of 33
What in the metallic bonds produces all of the properties of metals?
The delocalised electrons
12 of 33
Due to the strength of the electrostatic forces, what is needed?
A lot of energy to break it
13 of 33
Due to this energy, what do most copmpounds have
High melting and boiling points
14 of 33
What do they tend to be at room temperature? (adjective and state)
Shiny solid
15 of 33
What are they in water?
Insoluble
16 of 33
What are metals compared to non-metals?
More dense
17 of 33
Why?
The ions in the metallic structure are packed close together
18 of 33
What can the layers of atoms in a pure metal do?
Slide over each other
19 of 33
What does this make the metal?
Malleable
20 of 33
What does this mean the metal can be?
Hammered or rolled into flat sheets
21 of 33
What are metals good conductors of?
Electricity and heat
22 of 33
Why are they this?
The delocalised electrons carry electricity current and thermal (heat) energy through the material
23 of 33
Metallic bonding in metals causes them to have what?
Similar basic physical materials
24 of 33
Why do non-metals not exhibit the same properties as metals?
They don't have metallic bonding
25 of 33
Non-metals form a variety of what?
Different structures
26 of 33
What does this mean non-metals have?
A wide range of chemical and physical properties
27 of 33
What do non-metals tend to be?
Dull looking, more brittle, have lower boiling points, don't really conduct electricity and often have a lower density
28 of 33
What do metals and non-metals also have that are different?
Chemical properties
29 of 33
What do non-metals tend to do when they are trying to get a full outer shell?
Tend to gain electrons
30 of 33
What do metals do?
Lose electrons to gain full outer shells
31 of 33
Copper is a metallic element. State what property of copper makes it suitable for using in electrical circuits and explain why it has this property. [2 marks]
Copper is a good electrical conductor [1 mark] as it contains delocalised electrons which are able to carry an electrical current [1 mark]
32 of 33
Thomas has samples of two solids, A and B. One of the samples is a metal. Solid A is shiny and conducts electricity as a solid. Solid B is a white powder that only conducts electricity when dissolved in water. Which one is the metal?long answer [3]
Sample A is likely to be the metal[1]. Metals can conduct electricity as a solid as the the metallic structure contains delocalised/free electrons that are able to carry a charge[1]. Metals are also generally shiny[1].
33 of 33

Other cards in this set

Card 2

Front

What do metals consist of?

Back

Giant structures

Card 3

Front

What are delocalised?

Back

Preview of the front of card 3

Card 4

Front

What does delocalised mean?

Back

Preview of the front of card 4

Card 5

Front

What is between the positive metal ions and shared negative electrons?

Back

Preview of the front of card 5
View more cards

Comments

No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all Metallic Bonding resources »