Covalent, Ionic and Metallic Bonding Flashcards
Structure between metals?
Giant metallic structure
Bonding between metals?
Metallic bonding
What is metallic bonding?
Electrostatic attraction between positive ions and delocalised electrons in a layered structure
Trend in melting points in metals
Al3+ is stronger than Mg2+ which is stronger than Na+ as it has more protons and more delocalised electrons so a stronger metallic bond
Are metals malleable/ ductile and if yes why?
Yes, because layers of ions can slide over each other
Why are metals electrical conductors?
The delocalised electrons can travel through the layers
Drawing silver as a metal in the mark scheme
6 same sized particles attached , each with a single + in the centre
Group 4 NON-METALS: structure?
Giant macromolecular structure
Group 4 NON-METALS: bonding?
Covalent bonding
What is covalent bonding?
Electrostatic attraction between a shared pair of electrons and a positive nucleus
What is the melting point of group 4 non-metals?
High because very strong covalent bonds must be broken between atoms
Electrical conductivity of silicon dioxide and diamond (group 4)
None as no delocalised electrons or free ions
Electrical conductivity of graphite (group 4)
Can conduct as delocalised electrons between layers can move
Structure of diamond
4 carbon atoms covalently bonded in tetrahedral structure 109.5 degree bond angle
Structure of graphite
3 Carbon atoms covalently bonded in a hexagonal layered structure, 4th electron delocalised between the layers. Bond angle 120 degrees between carbon atoms