13366846
Description
Flashcards by I Shouldn't be awake, updated more than 1 year ago
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Created by I Shouldn't be awake
over 6 years ago
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| Question | Answer |
| Trend in bpt | Increase down group as: ^e- = more dipoles = stronger London forces More E to break IM forces |
| Trends in Reactivity | In redox X2 gains 1 electron Decreases down a group Atomic radius ^ Shielding ^ Ability to attract electron decrease |
| Halogen molecule state at RTP colour in hexane | F2 - Pale yellow gas Cl2 - Pale green gas - pale green Br2 - Red-brown liquid - orange I2 - Shiny grey/black solid - Violet |
| E config | s2p6 |
| Role in redox reactions | Reduced gain an e- to get full OSE config. |
| Displacement | More reactive halogen will displace a less reactive halogen in a solution if its halide ions. i.e. Cl2 + 2Br- -> 2Cl- + Br2 |
| How to differentiate between displaced halogens | Dissolve in hexane Cl2 -> pale green Br2 -> Orange I2 -> Violet |
| Disproportionation | Element is R and O in the same redox reaction |
| Cl2 disproportionation reactions (2) | + H2O + NaOH (cold, dilute) |
| Cl2+H2O | HClO + HCl |
| Cl2+ 2NaOH | NaClO + NaCl + H2O |
| Why use NaOH? | Cl2 LIMITED by low sol. of Cl2 in H2O. If water contains NaOH then much more will dissolve. |
| Dangers | Chlorinated HC Chlorine gas |
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