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Chemistry (P2)
Groups in the Periodic Table
| Question | Answer |
|---|---|
| What are elements in group 1 called? | Alkali Metals |
| What are elements in group 7 called? | Halogens |
| What are elements in group 0 called? | Noble gases |
| Give 2 properties of alkali metals. | They are soft, have relatively low melting points |
| When we react an alkali metal with water, what does it produce? | Hydrogen gas + hydroxide of the metal |
| How does lithium react with water? | Move around the surface, fizzing furiously |
| How do Sodium and Potassium react with water? | Do the same but also melt in the heat of the reaction |
| How does Potassium differ from Sodium in the reaction? | It gets hot enough to ignite the hydrogen gas |
| What is the reactivity trend with water with the alkali metals? | Elements get more reactive as you go down the group |
| Describe this trend by talking about electronic configurations. | Get more reactive as you go down, outer electron more easily lost because it's further from the nucleus so requires less energy |
| What is the colour and physical state of chlorine in room temperature? | Green gas |
| What is the colour and physical state of bromine in room temperature? | Red-brown liquid that gives off an orange vapour |
| What is the colour and physical state of iodine in room temperature? | Dark grey crystalline solid that gives off a purple vapour when heated |
| Describe the pattern of physical properties in the halogens as they go down. | Melting point increases and colours get darker |
| What is the test for chlorine? | Hold a piece of damp blue litmus paper over a gas, Chlorine will bleach it white |
| What happens when we react halogens with metals and give an example. | They form metal halides (Sodium + Chlorine → Sodium Chloride) |
| What happens when we react halogens with hydrogen and give an example. | They form hydrogen halides that dissolve in water to form acidic solutions. (Hydrogen + Chlorine → Hydrogen Chloride) |
| In terms of displacement, how do the halogens work? | The higher ones can displace the lower ones |
| In terms of these being redox reactions, what 2 things happen? | Halogens gain electrons (reduction) and Halide ions lose electrons (Oxidation) |
| Explain reactivity in terms of electronic configuration for halogens. | It gets harder to attract the extra electron to fill the outer shell when further from the nucleus, therefore it gets less reactive |
| Why are the noble gases chemically inert? | They have a full outer shell and do not give up or gain electrons easily |
| Why do we use Argon in light bulbs? | It is non flammable, stopping filament burning away |
| What do we use in flash photography? | Argon, krypton and xenon to stop flash filament burning |
| Why do we use Argon and helium when metals are being welded? | Inert atmosphere stops hot metals reacting with oxygen |
| Why is helium used in airships and party balloons? | Lower density than air and non flammable |
| What is the pattern of properties of the noble gases? | As you go down, boiling point, melting point and density all increase |
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