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29 Cards in this Set
- Front
- Back
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What is a ionic solid made up off? |
A metal and a non-metal |
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What are metallic solids made up of? |
Metal |
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What is molecular solids made up of? |
Non-metals |
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Do metals become positively charged or negatively charged in ionic compounds? |
Positively |
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Do the non-metals become positively or negatively charged in ionic compounds? |
Negativly |
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What is the structure of ionic compounds? |
Rigid 3D lattice structure (Therefore shatters) |
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What are the attractive forces in ionic compounds? |
Electrostatic attraction (Due to oppositely charged ions) |
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What kind of bonding in ionic compounds? |
Ionic bonding |
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What is the strength of the ionic bonds and what does this mean? |
Ionic bonds are strong and therefore they have high melting and boiling points |
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When can ionic solids conduct electricity and when? |
Ionic bonds hold ions in a fixed position and therefore there are no free moving charged particles to carry the charge. Ionic compounds are soluble so therefore they dissolve in water and in liquid form they can conduct electricity |
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Are ionic compounds soluble? |
Ionic solids are soluble in water as the ions are separated from the lattice due to the attraction towards the polar water molecules which is strong enough to pull the ions from the lattice. |
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What kind of bonding for metallic solids? |
Metallic bonding |
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Describe the structure of a metallic solid |
Non-directional bonding in a 3D lattice structure because the valence electrons become delocalised and therefore it is ductile and malleable |
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Are metallic solids able to conduct electricity? |
Since the valence electrons are delocalised they are able to carry a charge |
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Are metallic solids soluble? |
Metals are not soluble in water, as the metallic bonds are too strong to be broken by the attraction to the polar water molecules |
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Do metallic solids have a high or low melting and boiling point and why? |
Due to the strong attraction between the valence electrons and the nuclei, metallic solids have high melting and boiling points due to the higher energy needed to overcome the bonds. |
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What kind of particle makes up a metallic solid? |
Atoms |
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What makes up molecular solids? |
Molecules |
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Describe the bonds and structure of molecular solids? |
Intermolecular bonds are random and weak |
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Do molecular solids have low or high melting and boiling points and why? |
Intermolecular bonds are random and weak which is why it takes less energy to overcome the bonds, giving lower melting point. |
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Do molecular solids conduct electricity? |
Molecular compounds can not conduct electricity in any state because they do not contain free moving charges particles |
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How many times can B be bonded? |
3 |
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How many times can Be be bonded |
2 |
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Is trigonal planar symmetrical? |
Yes |
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What kind of bonding in covalent network |
Covalent bonding |
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What is melting and boiling point of covalent networks? |
The covalent bonds are strong and therefore require a lot of heat energy to overcome the bonds and therefore a high melting and boiling point. |
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Describe the structure of diamond |
Each carbon atom is bonded to 4 other carbon atoms in a tetrahedral arrangement |
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Is diamond able to conduct electricity? |
Each carbon is bonded to 4 other carbon atoms which means there are no free moving charged particles to carry a charge. |
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Describe the structure of graphite |
- the weak attraction between the layers of atoms in graphite are easily broken. Therefore, graphite is soft and slippery and layers slide off easily. - Each carbon is bonded to 3 other carbon atoms with one unbounded pair which becomes delocalised |
