Chapter 8 Chemistry AS

1. 1Group 2 are called the [blank_start]alkali[blank_end] metals.

   1. Aalkali
2. 2Group 2 metals [blank_start]are[blank_end] reactive and aren't found in there element form.

   1. Aare
   2. Baren't
3. 3Group 2 metals tend to be found in compounds.

   1. ATrue
   2. BFalse
4. 4Most metals are oxidised as they lose 2 electrons to gain a stable configuration.

   1. ATrue
   2. BFalse
5. 5Group 2 elements are [blank_start]reducing[blank_end] agents.

   1. Areducing
   2. Boxidising
6. 6All of the group 2 metals react with oxygen to form a metal oxide.

   1. ATrue
   2. BFalse
7. 7When the metals react with [blank_start]water[blank_end] they form hydrogen and alkaline hydroxide.

   1. Awater
   2. Boxygen
8. 8Group 2 metals reactivity decreases down a group.

   1. ATrue
   2. BFalse
9. 9Metals can take part in [blank_start]redox[blank_end] reactions with dilute acids that form hydrogen and a salt.

   1. Aredox
   2. Bdiproportionation
10. 10The total increase and decrease in oxidation numbers should balance each other out in the group 2 metals.

    1. ATrue
    2. BFalse

11. 11Due to ionization energy decreasing down a group, elements become more reactive and [blank_start]stronger[blank_end] reducing agents down a group.

    1. Astronger
    2. Bweaker
12. 12The oxides of the group 2 elements form hydroxides when [blank_start]water[blank_end] is added, forming alkaline solutions.

    1. Awater
    2. Boxygen
    3. Cacid
13. 13Hydroxides aren't soluble in water.

    1. ATrue
    2. BFalse
14. 14When a solution becomes saturated, any further metal and hydroxide ions will form a [blank_start]solid precipitate[blank_end].

    1. Asolid precipitate
    2. Bgas
15. 15Solubility of hydroxides [blank_start]increases[blank_end] down a group.

    1. Aincreases
    2. Bdecreases
16. 16The more alkaline a solution is (more OH- ions) the more soluble it is in water.

    1. ATrue
    2. BFalse
17. 17Group 2 oxides, hydroxides and carbonates are used as bases to neutralise acids. Some of their uses are:

    1. ATo neutralise soils (Ca(OH)2) to form neutral water.
    2. BFor making alcohol.
    3. CTo treat acid digestion problems e.g. heart burn by turning the acid to neutral water.
18. 18Group 2 metals [blank_start]add[blank_end] electrons to other species so are good reducing agents.

    1. Aadd
    2. Bgain
19. 19Group 17 (the halogens) are the most reactive non-metal group.

    1. ATrue
    2. BFalse
20. 20On earth halogens occur as stable [blank_start]halide[blank_end] ions dissolved in sea water or combined with sodium or potassium.

    1. Ahalide
    2. Bunstable
21. 21At RTP, the halogens are all diatomic molecules e.g. Cl2

    1. ATrue
    2. BFalse
22. 22The halogens are all in the same state.

    1. ATrue
    2. BFalse
23. 23Gas is at the [blank_start]top[blank_end] of group 17 and [blank_start]solid[blank_end] at the bottom of the group.

    1. Atop
    2. Bbottom
    3. Csolid
    4. Dliquid
24. 24Down the halogen group:

    1. ABoiling point increases.
    2. BBoiling point decreases.
    3. CStronger london forces
    4. DWeaker london forces
    5. EMore energy needed to break intermolecular forces
    6. FLess energy needed to break intermolecular forces.
25. 25Halogens are [blank_start]reduced[blank_end]

    1. Areduced
    2. Boxidised
26. 26Halogens are [blank_start]oxidising[blank_end] agents.

    1. Aoxidising
    2. Breducing
27. 27Reactivity of halogens decreases down a group.

    1. ATrue
    2. BFalse
28. 28If a halogen is added and is more reactive than the halide ion it is added to then:

    1. Aa reaction takes place
    2. Bthe halogen displaces the halide from solution
    3. Cthe solution doesn't change colour
    4. Dthe solution changes colour
29. 29If solutions show a similar colour, the non-polar organic solvent [blank_start]cyclohexane[blank_end] can be added and shaken in the mixture.

    1. Acyclohexane
30. 30Non-polar halogens dissolve much more in cyclohexane than water so shows a significant colour difference.

    1. ATrue
    2. BFalse
31. 31Fluorine is a pale yellow gas that is very reactive.

    1. ATrue
    2. BFalse
32. 32Astanine is the least reactive halogen but radioactive and rapidly decays so never been seen.

    1. ATrue
    2. BFalse
33. 33Fluorine is the strongest oxidising agent of the halogens as it gains electrons more easily as it's more reactive.

    1. ATrue
    2. BFalse
34. 34The halogens become [blank_start]weaker[blank_end] oxidising agents down the group.

    1. Aweaker
    2. Bstronger
35. 35[blank_start]Disproportionation[blank_end] reaction is where the same element is both oxidised and reduced.

    1. ADisproportionation
36. 36A disproportionation reaction occurs when chlorine is added to water.

    1. ATrue
    2. BFalse
37. 37Chlorine has a [blank_start]low[blank_end] solubility in water but if the water contains dissolved sodium [blank_start]hydroxide[blank_end] much more chlorine dissolves. This now forms a stronger bleach.

    1. Alow
    2. Bhigh
    3. Chydroxide
    4. Dcarbonate
38. 38Chlorine isn't a toxic gas

    1. ATrue
    2. BFalse
39. 39Chlorine can kill [blank_start]bacteria[blank_end] but can also be a respiratory irritant.

    1. Abacteria
40. 40Chlorine has links to cancer due to it reacting with the organic compound, methane which is produced when digesting vegetation.

    1. ATrue
    2. BFalse
41. 41In the displacement reaction between halides and halogens, the halogen [blank_start]gained[blank_end] electrons so they are [blank_start]oxidising[blank_end] agents.

    1. Agained
    2. Blost
    3. Coxidising
    4. Dreducing
42. 42Titrations are [blank_start]quantitative[blank_end] experiments.

    1. Aquantitative
    2. Bqualititive
43. 43To test for carbonates, you add dilute [blank_start]nitric[blank_end] acid to the solution and test for effervesce of [blank_start]carbon dioxide[blank_end].

    1. Anitric
    2. Bhydrochloric
    3. Csulfuric
    4. Dcarbon dioxide
    5. Eoxygen
    6. Fnitrogen
44. 44The carbonate ion has a [blank_start]2-[blank_end] charge.

    1. A2-
    2. B1-
    3. C2+
45. 45To test for the production of carbon dioxide you add limewater and see if it goes cloudy/forms a white precipitate.

    1. ATrue
    2. BFalse
46. 46Most sulphates are very [blank_start]soluble[blank_end] in water but [blank_start]barium[blank_end] sulphate is very insoluble.

    1. Asoluble
    2. Binsoluble
    3. Cbarium
    4. Dcopper
47. 47A [blank_start]white[blank_end] precipitate forms is a sulphate is present.

    1. Awhite
    2. Byellow
48. 48You can also use barium nitrate or [blank_start]chloride[blank_end] for the sulphate test but there is and addition of chloride ions making the halide test ineffective.

    1. Achloride
    2. Bsulphate
49. 49Most halides are soluble in water but [blank_start]silver[blank_end] halides are insoluble.

    1. Asilver
    2. Bcopper
    3. Cgold
50. 50In a halide test, aqueous silver ions react with aqueous [blank_start]halide ions[blank_end] to form precipitates or silver halides.

    1. Ahalide ions
    2. Bchloride ions
51. 51After the addition of silver nitrate to test for halides, the silver precipitates are different colours. Silver chloride is white, siver iodide is [blank_start]yellow[blank_end] and silver [blank_start]bromide[blank_end] is cream

    1. Ayellow
    2. Bcream
    3. Cwhite
    4. Dbromide
    5. Eiodide
    6. Ffluoride
52. 52Silver halides precipitates can be very similar colours and hard to tell apart.

    1. ATrue
    2. BFalse
53. 53You can add [blank_start]ammonia[blank_end] to silver halides and test solubility to see the difference. Chloride is soluble in dilute, bromide is if its concentrated and iodide [blank_start]isn't[blank_end].

    1. Aammonia
    2. Bbarium
    3. Cisn't
    4. Dis in dilute
    5. Eis in concentrated
54. 54The order for the anions testing is:

    1. Ahalides, carbonates and sulphates
    2. Bsulphates, halides and carbonates
    3. Ccarbonates, sulphates and halides
55. 55The carbonate test must be first.

    1. ATrue
    2. BFalse
56. 56Sulphate testing produces a white precipitate so must have other testing with white precipitates done separately.

    1. ATrue
    2. BFalse
57. 57The halide test must be last as silver carbonate and silver sulphate will produce a positive reaction for this.

    1. ATrue
    2. BFalse
58. 58If you are given a mixture of solutions, you must carry out the test in the same order but ensure each reaction is [blank_start]fully complete[blank_end] so continue to add nitric acid until the bubbling stops completely.

    1. Afully complete
    2. Bpartially complete
    3. Cnot complete
59. 59You can't use hydrochloric or sulphuric acid as these add chloride and sulphate ions.

    1. ATrue
    2. BFalse
60. 60To continue testing if a solution has other ions, filter out the [blank_start]barium[blank_end] sulphate precipitate.

    1. Abarium
    2. Bsilver
61. 61To test for ammonium ions, you must add [blank_start]NaOH[blank_end] and boil the solution. Add damp indicator [blank_start]paper[blank_end] and test for a blue colour.

    1. ANaOH
    2. BHNO3
    3. Cpaper
    4. Dsolution
62. 62Aqueous ammonium ions and sodium hydroxide react to form the ammonia gas.

    1. ATrue
    2. BFalse
63. 63Ammonia isn't soluble in water.

    1. ATrue
    2. BFalse
64. 64What is HClO [blank_start]...[blank_end]

    1. Ableach

Description

Quiz on Chapter 8 Chemistry AS, created by emilycoral on 19/01/2016.

Author

emilycoral

Language

English

Views

4

Rating

No ratings yet

Rate this quiz

Rate this quiz

More on Group 2: alkaline earth metals