1
Q
What is a metals structure?
A
- metals have crystal structures
- held together by metallic bonding (giving all metals the same basic properties)
- this allows the outer electron(s) of each atom to move freely
- creating a sea of delocalised (free) electrons throughout metal which gives rise to many of metals properties
2
Q
What are the properties of most metals?
A
- high melting and boiling point and density
- strong, bendy and malleable
- good conductors of electricity and heat
- hard, dense and lustrous
3
Q
Why do metals have high melting and boiling points?
A
- strong attraction between delocalised electron and the closely packed positive ions causes very strong metallic bonding
- metals have high melting and boiling points because of this, you need lots of energy to break them apart
4
Q
Why are metals strong and flexible and malleable?
A
- metals have a high tensile strength (strong and hard to break)
- but can be hammered into different shapes (malleable)
5
Q
Why are metals good conductors of heat and electricity?
A
-sea of delocalised electrons move freely through metal, carrying electrical current and heat energy
6
Q
What transition metals and their compounds?
A
-mainly everyday metals
7
Q
Why are transition metal compounds colourful?
A
-due to the transition metal ion they contain
8
Q
What are transitional metals used for and where are they on the periodic table?
A
- catalysts
- middle of periodic table
9
Q
How does the strength of metallic bonding decrease?
A
-as atomic radius increases
10
Q
What are some examples of transition metal compounds and their colours?
A
- iron(II) compounds=light green
- iron(III) compounds=orange/brown
- copper compounds=blue
