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CC13H SC17H
Pearson GCSE Combined and Separate Chemistry Higher
| Question | Answer |
|---|---|
| Describe how lithium reacts with cold water. | Lithium floats and bubbles vigorously |
| Why does the reactivity of Group 1 metals increase down the group? | When metals react they lose their outer electrons. Further down the group there are more shells of electrons so the outer electrons are less attracted to the nucleus and easier to remove |
| Describe the colour and state of Chlorine, Bromine and Iodine | Cl2. A pale green gas. Br2. A red-brown liquid. I2. A shiny purple-black solid |
| Complete and balance this equation for the reaction of lithium with bromine. Li + Br2 --> | 2Li + Br2 --> 2LiBr |
| What is the test for Chlorine Gas? | Chlorine gas turns damp blue litmus red then quickly bleaches it white |
| Explain why the reactivity of group VII elements increases as you go up the group. | When non-metals react they complete their outer shells. Further up the group the elements have fewer shells so the nucleus attracts electrons more strongly |
| Complete the Word Equation for this reaction. Fluorine + Sodium Iodide --> | Fluorine + Sodium Iodide à Iodine + Sodium Fluoride |
| What is the name given to the non-metals in Group 0? | The Noble Gases |
| Explain why Group 0 elements do not react at all | Their atoms have complete outer shells |
| Why is Helium used to fill airships? | It is inert and has very low density |
| Why is Neon used in lighting? | It glows when electricity is passed through it |
| Write and balance this equation for the reaction of sodium with water | 2Na + 2H2O --> 2NaOH + H2 |
| Why does the reactivity of Group 1 metals increase down the group? | When metals react they lose their outer electrons. Further down the group there are more shells of electrons so the outer electrons are less attracted to the nucleus and easier to remove |
| Write a balanced chemical equation for the reaction of Hydrogen and Bromine | H2 + Br2 --> 2HBr |
| What is produced whey Hydrogen Chloride gas dissolves in water | Hydrochloric Acid |
| What is the test for Chlorine Gas? | Chlorine gas turns damp blue litmus red then quickly bleaches it white |
| Complete the Word Equation for this reaction. | Chlorine + Sodium Iodide à Iodine + Sodium Chloride |
| Chlorine + Sodium Iodide, Complete and balance this ionic equation for the reaction of Fluoride ions with Chlorine molecules | F2 + 2Cl- --> 2F-+ Cl2 |
| Why are chloride ions oxidised when they react with Fluorine molecules? | They lost electrons |
| Why are fluorine molecules reduced when they react with chloride ions? | They gain electrons |
| Explain why Group 0 elements do not react at all | Their atoms have complete outer shells |
| Why is Argon used to fill fire extinguishers? | Because it is inert and denser than air |
| Why is Neon used in lighting? | It glows when electricity is passed through it |
| In terms of electrons, what do group 1 elements have in common? | 1 electron in the outer shell |
| In terms of electrons, what do group 7 elements have in common? | 7 electrons in the outer shell |
| In terms of electrons, what do group 0 elements have in common? | Full outer shell |
| What is more reactive, lithium or sodium? | Sodium |
| What is more reactive, chlorine or bromine? | Chlorine |
| Define inert | Un-reactive |
| Explain why the noble gases are inert | They have full outer shells, so do not need to gain or lose electrons |
| State the trend in the melting points of the alkali metals | Gets lower down the group |
| What state are fluorine, chlorine, bromine and iodine at room temperature? | Gas, gas, liquid, solid |
| Balance the equation: Li + H₂O → LiOH + H₂ | 2Li + 2H₂ → 2LiOH + H₂ |
| State the trend in melting and boiling points for the halogens as you go down the group. Predict what state astatine will be. | As you go down the group melting point increases. F2 and Cl2 are gases, Br2 is a liquid, I2 is a solid. At2 will be a solid |
| How can chlorine be tested for? | Bleaches damp litmus paper white |
| Explain why the group 1 elements are called alkali metals | They are metals that form alkalis when they react with water |
| What is a displacement reaction? | A reaction in which a more reactive element takes the place of a less reactive element in a compound |
| Explain why the following reaction does not proceed: KBr + I₂ | Iodine is less reactive than bromine so cannot displace it |
| Balance the below equation and explain why it is a displacement reaction: KBr + Cl₂ → KCl + Br₂ | 2KBr + Cl₂ → 2KCl + Br₂ , chlorine has displaced bromine as it is more reactive |
| Explain why fluorine is more reactive than chlorine | Fewer shells/electrons, less shielding (or stronger attraction from nucleus), easier to gain electrons |
| Explain why potassium is more reactive than lithium (3 marks) | More shells/electrons, less shielding (or weaker attraction from nucleus), easier to lose electrons |
| How do halogens react with magnesium? | Mg (s) + Cl2 → MgCl2 (s) |
| What happens with halogens react with hydrogen? What is the pH when the product dissolves in water? | H2 (g) + Cl2 (g) → 2HCl (g) - pH will be low as forms an acid |
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Davenant Foundation School
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