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Flashcards by Miss C Rodgers, updated more than 1 year ago
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| Question | Answer |
| Describe the structure of a pure metal | The atoms in a pure metal are in tightly - packed layers which form a regular lattice structure |
| What 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. |
| What is a metallic bond? | The positive cations (+) are attracted to the sea of electrons (-), this attraction is called a metallic bond |
| Why do metals have high boiling and melting points | The 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 |
| Why do metals conduct electricity? | The sea of electrons are free charges that allow the metals to conduct electricity |
| What is the definition of metallic bonding? | Metallic bonding is the strong attraction between closely packed positive metal ions (+) and a 'sea' of delocalised electrons (-) |
| Why are metals malleable and ductile? | because the layers of positive cations slide over each other |
| how 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 |
| What does ductile mean? | It means that the metal can be stretched into a wire. |
| What does ductile mean? | It means the metal can be shaped |
| What does lustrous mean? | It means shiny |
| Why are metals lustrous? | Light hits the free electrons and is reflected off them |
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