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24 Cards in this Set
- Front
- Back
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What is an ionic bond? |
A bond where metals pass their electrons on to nonmetals and become charged ions. |
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When metals lose their electrons, they become .......... charged |
Positively |
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What keeps ions stuck together? |
An electrostatic attraction between positive and negative ions |
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Describe the layout of giant ionic structures. |
A regular, repeat lattice structure without gaps that alternates between positive and negative ions. |
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What charge do ionic compounds have? |
Neutral- the charges of the ions cancel each other out when forming a compound. |
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Give 3 properties of ionic compounds |
Any from -high melting points -hard but brittle -uniform repeat structure -unreactive when solid -dissolve in water -conduct electricity when dissolved in solution |
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What's a covalent bond? |
A bond where two nonmetals share their electrons in pairs, creating intermolecular forces of attraction. |
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Why is graphite soft and slippery? |
The carbon atoms in graphite are covalently bonded with three other atoms, the fourth electron free to move throughout the structure, creating weak intermolecular forces which are easily broken, meaning the atoms can slide over each other easily. |
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Name 3 properties of graphite. |
-high melting point -soft -conducts electricity |
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Why are diamonds so strong? |
All four electrons in carbon's outer shell are used for covalent bonding, meaning that there are no free moving electrons or intermolecular forces. There are many bonds to break. |
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Give 3 properties of diamond |
Very high melting point Very strong Non conductor of electricity |
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Give 3 properties of covalent bonding |
Low melting points Can be very reactive Volatile Soft and brittle (normally) Small finite structures Solids, liquids and gases at room temp |
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Name 3 properties of giant covalent structures |
Extremely high melting points Extremely hard and brittle Uniform repeat structure Unreactive when solid Normally do not conduct electricity Do not dissolve in water |
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Why is the name of the type of structure diamond takes? |
Tetrahedral |
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What is a metallic bond? |
A bond of electrostatic attraction between a lattice of positive ions and delocalised electrons |
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Why can metals conduct electricity? |
They have a sea of delocalised electrons which are free to move and carry charge |
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Why has aluminium got a higher melting point that sodium? |
It has more electrons in the outer shell to donate to the electron cloud and therefore makes it denser and stronger |
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Why is metal malleable? |
The delocalised electrons allow atoms to slide over each other without the interference of strong repulsive forces between ions |
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What is an alloy? |
A mixture of two or more different metals |
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Give three differences between alloys and metals |
Alloys are stronger, more corrosion resistant and less malleable |
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What's a fullerene? |
A large hollow structure consisting of carbon atoms in many different shapes. |
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Give 3 uses for nanotubes |
Delivering medicine (radiation to cancer cells) Lubricants Catalysts |
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What is graphene? |
One layer of carbon atoms bonded in hexagonal rings one atom thick |
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Give 3 properties of graphene |
Good thermal and electrical conductor Low density Very strong |
