1406324
Description
Flashcards by rachelouise01, updated more than 1 year ago
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Created by rachelouise01
about 10 years ago
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| Question | Answer |
| Ionic (Profile) | Metal and Non Metal Particles: Ions Bonding: Electrostatic Forces Example: NaCl |
| Molecular (Profile) | Non Metal Particles: Molecules Bonding: Intermolecular Forces Example: S8 |
| Metallic (Profile) | Metal Particles: Atoms Bonding: Metallic Bonds Example: Ag |
| Covalent Network | Group 14 Particles: Atoms Bonding: Covalent Bonds Example: Diamond, Silica, Graphite |
| Ionic (Definition) | -Made up of a 3-D lattice of positive and negative ions -Held together by strong electrostatic forces between the positive and negative ions |
| Molecular (Definition) | -Made up of discrete molecules with strong intramolecular covalent bonds and weak intermolecular forces -Held together by weak intermolecular forces |
| Metallic (Definition) | -Made up of positive metal nuclei surrounded by a sea of delocalised electrons -Held together by moderately strong metallic bonds created by electrostatic attractions between the metal nuclei and valence electrons of neighbouring atoms |
| Covalent Network (Definition) | -Made up of giant extended (*) lattices made up of atoms with strong covalent bonds to neighbouring atoms -Held together by extremely strong covalent bonds to neighbouring atoms * 3-D (Diamond and Silica), 2-D (Graphite) |
| Melting Point Ranking (lowest to highest required) | Molecular Metallic Ionic Covalent Order due to bond strength |
| Electrical Conductivity - States | Metallic - solid and liquid (delocalised electrons) Ionic - liquid and aqueous (lattice is broken, ions can move) Molecular - none (charged electrons but can't move) Covalent - only graphite in solid (free electrons between 2-D layers) |
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