Flashcards
Metallic bonding
Cards in this deck (12)
- 1Describe the structure of a pure metalThe atoms in a pure metal are in tightly - packed layers which form a regular lattice structure
- 2What happens to the electrons in the outer shells, that have been lost from the metal atom?They separate from the atoms and create a sea of delocalised electrons.
- 3What is a metallic bond?The positive cations (+) are attracted to the sea of electrons (-), this attraction is called a metallic bond
- 4Why do metals have high boiling and melting pointsThe metallic bond is very strong so they need a lot of heat energy to break the bonds meaning they have high boiling and melting points
- 5Why do metals conduct electricity?The sea of electrons are free charges that allow the metals to conduct electricity
- 6What is the definition of metallic bonding?Metallic bonding is the strong attraction between closely packed positive metal ions (+) and a 'sea' of delocalised
electrons (-) - 7Why are metals malleable and ductile?because the layers of positive cations slide over each other
- 8how do delocalized electrons in metallic bonding allow metals to conduct heat and electricity?for example, when a metal is heated, the delocalised electrons gain kinetic energy, these electrons then move faster so they gain energy throughout the metal, this makes the hear transfer in metals very efficient
- 9What does ductile mean?It means that the metal can be stretched into a wire.
- 10What does ductile mean?It means the metal can be shaped
- 11What does lustrous mean?It means shiny
- 12Why are metals lustrous?Light hits the free electrons and is reflected off them
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- Flashcards on Metallic bonding, created by Miss C Rodgers on 27/03/2018.
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- Miss C Rodgers · Mar 2018
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- Mar 27, 2018
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- Created by anna.a.graysmith · May 13, 2014
- Copied by Miss C Rodgers · Mar 27, 2018
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