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18 Cards in this Set
- Front
- Back
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What are Ions? |
Atoms that have different numbers of electrons and protons |
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What causes and atom to become an ion? |
The atom has lost or gained electron(s), which has caused the atom to become positively (loss of electrons) or negatively (gain of electrons) charged |
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What is Oxidation? |
Oxidation is the loss of electrons (OILRIG) |
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What is Reduction? |
Reduction is the gain of electrons (OILRIG) |
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How do you draw a Covalent Compound? |
Dot and Cross Diagram |
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How do you draw an Ionic Compound? |
Draw the elements with their electron configuration and shells around the element symbol, then an arrow, and then the elements with a full outer shell, and their charges to the top left of the atom (Same for the configuration), except O2 becomes 2x O^2- |
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What is an ionic bond? |
When two or more elements of different charges are bonded by strong forces of electrostatic attraction |
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Why do ionic compounds have high melting and boiling points? |
Because they have very strong electrostatic bonds, and strong inter molecular forces of attraction, so more energy is required to break the bonds. |
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What configuration are ionic solids in? |
A three dimensional lattice of a regular order, with each ion being surrounded by 6 oppositely charged ions, held together by the electrostatic attraction |
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What are covalent bonds? |
Bonds where two or more atoms share 1 or more pairs of electrons, to form a full outer shell |
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What causes the bonds to hold the two atoms together? |
The shared pair(s) of electrons are attracted to both nuclei, so the atoms are held together |
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Why do simple covalent compounds have low melting and boiling points? |
Because the intermolecular bonds are much weaker than ionic bonds, which means that less energy is required for a liquid or moulten state of matter |
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What are Giant Covalent structures? |
Diamond, Graphite, Buckministerfullerene (C60) which are all carbon based, and Silicone Dioxide are all giant covalent structures, with a regular lattice and many strong covalent bonds |
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Why do giant covalent structures have high melting and boiling points? |
Because there are lots of strong covalent bonds that need to be broken, which collectively take a lot of energy to break. Usually, there would only be intermolecular forces to overcome (Eg Graphite, which has a low melting point), however is giant covalent structures with only covalent bonds, very high temperatures are required |
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What can metals be referred to as? |
Giant metallic crystals with positive metal ions surrounded by a sea of delocalised electrons |
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What are the properties of ionic compounds? |
High Melting and boiling points, Hard but Brittle, generally soluble in water, conduct electricity in moulten / liquid form |
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How are the ions from an ionic compound arranged in liquid and gaseous state? |
They are separated, and free to move around each other (This allows the flow of electric charge) |
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How are atoms from a covalent compound arranged in liquid and gaseous state? |
The separate covalent molecules remain bonded, however the weak intermolecular forces have been broken, so the separate molecules do not attach together |
