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14 Cards in this Set
- Front
- Back
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Define an ionic bond |
The attraction between a positive and negative ion. |
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What determines strength of ionic bond |
The size of charge and size of ion Higher charge and smaller ion = greater force of attraction |
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What are the electrons in a covalent bond attracted to |
The electrons are attracted to the nuclei of both atoms |
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What determines strength of covalent bond |
Shorted bond length, stronger bond |
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Simple molecular 1) Melting and boiling point 2) what makes it higher 3) conductivity |
1) low 2) when it’s a bigger molecule 3) Not conductive |
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Giant covalent 1) mp and bp 2) what makes it higher 3) conductivity |
1) very high 2) when there’s shorter covalent bonds 3) not conductive except graphite |
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Ionic bonding 1) mp and bp 2) what makes it higher 3) conductivity |
1) High 2) Higher density 3) Molten or in solvent |
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Metallic 1) mp and bp 2) what makes it higher 3) conductivity |
1) high 2) higher charge density 3) always but not as gas |
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What is a metallic bond |
The attraction between positive metal ions and the delocalised electrons |
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What determines strength of metallic bond |
The higher the density of the charge, the higher the number of electrons and the higher the strength of the bond. |
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Which electrons become delocalised in a metallic bond |
The outer electrons from the metal ion become delocalised |
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What shape does diamond make |
Tetrahedron |
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What is a dative covalent bond |
Both electrons came from the same atom |
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How did the dative covalent bond from ammonia form |
Nitrogen has a lone pair of electrons when it forms NH3 (ammonia) it donates both of its electrons to a new H+ ion to form NH4 (ammonium) |
