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34 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Define first ionisation energy |
The first ionisation energy is the energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms. |
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Which factors affect ionisation energy? |
• Nuclear charge - The more protons there are in the nucleus, the more positively charged the nucleus is. • Atomic radius - An electron further away is less atteracted to the nucleus. • Shielding - Outer electrons feel less attracted when there more shells between them and the nucleus. |
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Show the second ionisation energy of oxygen. |
O^+(g) -> O^2+(g) + e^- |
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How would you draw the first ionisation of Sodium? |
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Name examples of giant covalent lattices (macromolecular stuctures). |
Carbon and Silicon |
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What are the three carbon allotropes? |
Graphite, diamond and graphene. |
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How are the carbon atoms in grahite held together? |
They are covalently bonded with three bonds each. The forth outer electron of each carbon atom is delocalised, which allows them to be held by induced dipole-dipole interactions. |
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What properties does graphite have due to it's structure? |
• The weak forces between layers of graphite are easily broken so the sheets can slide over each other. • The delocalised electrons in graphite are free to move, so am electric current can flow. • The layers are far apart compared to the covalent bonds, so graphite has a low density. • Because of the covalent bonds they have a very high melting point. • Graphite is insoluble in any solvent. |
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Define sublime |
It changes straight from a solid to a gas, skipping the liquid stage. |
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What is diamond made up of? |
They are made up of carbon atoms that are covalently bonded to 4 other carbon atoms in a tetrahedral shape. |
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Why does having strong covalent bonds help the structure of diamond? |
• High melting point - sublime over 3800K. • Hard - used in saws etc. • Good thermal conductor - vibrations travel easily through a stiff lattice. • Can't conduct electricity - all outer electrons are involved in bonds. • Diamond doesn't dissolve. |
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What is graphene? Give a property and how it can be used. |
One layer of graphite - it's a sheet of carbon atoms. It is transparent it can be used as touchscreens on phones etc. |
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What are giant metallic lattice structures made up of? |
They are a lattice of metal ions surrounded by a 'sea' of delocalised electrons. |
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How are the following affected by metallic structures: • Melting and Boiling points • Ability to be shaped • Conductivity • Solubility |
• Melting and boiling points - the number of delocalised electrons per atom affects the melting and Boiling points. The more they are, the higher the the melting and boiling points are. • Ability to be shaped - metal ions can slide over each other when the structure is pulled. • Conductivity - Delocalised electrons can pass on kinetic energy, which makes theme good thermal conductors. • Solubility - Metals are insoluble because of the strength of the metallic bonds. |
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In group 2, what happens to reactivity down the group? |
It increases because it's easier to lose electrons, so it is more reactive. |
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How do group 2 elements react, in terms of oxidation? |
M -> M^2+ 2e^- |
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How group 2 elements react with the following: • Water • Oxygen • Dilute acids |
• Water - they form to make a metal hydroxide and hydrogen. The metal hydroxide can dissolve in water to form hydroxide ions. • Oxygen - they form to make solid white oxides. These oxides would dissolve in water to for hydroxide ions. • Dilute acids - they form metal chloride/sulfate and hydrogen. |
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Name 2 uses of group 2 compounds. |
• Calcium hydroxide is used in agriculture to neutralise acid soils. • Magnesium hydroxide and calcium carbonate are used in some indigestion tablets as they neutralise excess stomach acids. |
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Give the formula, colour, physical state and electronic structure of the halogens. |
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Explain the trend of boiling points in the halogens. As well as volatility. |
It increases as you go down the group, as there is increasing Trentham due to the induced dipole-dipole forces as the no. of electrons increase. Volatility is high when there's a low boiling point, so volatility decreases down the group. |
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How do halogens react? |
By gaining an electron in their outer shell, this means they are reduced. So halide ions are formed. They're oxidising agents. X + e^- -> X^- |
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What happens when a halogen is dissolved in an organic solvent? |
A colour is formed: • A violet/pink shows the presence of iodine. • An oranage/red colours shows bromine. • A very pale yellow/green shows chlorine. |
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How could you test for a halogen? |
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What should happen to the halogens when they are mixed with ammonia? |
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Define disproptionation |
When a a single element is simultaneously oxidised and reduced. The halogens undergo disproptionation when they react with cold dilute alkali solutions. |
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How can you make bleach? |
When you mix a metal hydroxide with chlorine it forms to make a chlorate ion, which is known as bleach. |
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How does chlorine and water undergo disproptionation? |
Chlorine mixes with water and forms hydrochloric acid and chloric acid. |
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How is chlorine involved in water treatment? |
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What other alternatives are there to chlorine? In terms of water. |
• Ozone (O3) is a strong oxidising agent that is great at killing microorganisms. It is expensive to produce and isn't permanent. • Ultraviolet light kills microorganisms by damaging their DNA. Same weaknesses as Ozone. |
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How would you test for carbonate ions? |
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Which order should an unknown substance be tested? |
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How would you test for sulfates? |
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How would you test for Ammonium ions? |
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How would you test for halides? |
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