Test
C4 - Part 3
Este test tiene tipos de pregunta que se abren en el reproductor de siempre.
Preguntas del test (30)
1There are five non - metals in Group 7 and they are known as the [blank_start]halogens[blank_end]. They all have [blank_start]seven[blank_end] [blank_start]electrons[blank_end] in their outer shell which means that they have [blank_start]similar[blank_end] chemical properties. The four important halogens are [blank_start]fluorine[blank_end], [blank_start]chlorine[blank_end], b[blank_start]romine[blank_end] and i[blank_start]odine[blank_end].
- Ahalogens
- Bseven
- Celectrons
- Dsimilar
- Efluorine
- Fromine
- Godine
- Hchlorine
2At room temperature:
Chlorine is a [blank_start]green[blank_end] [blank_start]gas[blank_end]
Bromine is an [blank_start]orange[blank_end] [blank_start]liquid[blank_end]
Iodine is a [blank_start]grey[blank_end] [blank_start]solid[blank_end]- Agreen
- Bgas
- Corange
- Dliquid
- Egrey
- Fsolid
3Iodine is used as an [blank_start]antiseptic[blank_end] to [blank_start]sterilise[blank_end] [blank_start]wounds[blank_end].
The most commonly used group 7 halogen is [blank_start]chlorine[blank_end]. It is used to [blank_start]sterilise[blank_end] [blank_start]water[blank_end] and to make pe[blank_start]sticides[blank_end] and pl[blank_start]astics[blank_end].- Aantiseptic
- Bsterilise
- Cwounds
- Dchlorine
- Esterilise
- Fwater
- Gsticides
- Hastics
4Halogens react vigorously with [blank_start]alkali[blank_end] [blank_start]metals[blank_end] to form [blank_start]metal[blank_end] [blank_start]halides[blank_end].
Lithium + Chlorine --------> [blank_start]Lithium[blank_end] [blank_start]Chloride[blank_end]
2Li + Cl2 --------> 2LiCl
Sodium + Bromine -----> [blank_start]Sodium[blank_end] [blank_start]Bromide[blank_end]
2Na + Br2 -----> 2NaBr
Potassium + Iodine ------> [blank_start]Potassium[blank_end] [blank_start]Iodide[blank_end]
2K + I2 --------> 2KI- Aalkali
- Bmetals
- Cmetal
- Dhalides
- ELithium
- FChloride
- GSodium
- HBromide
- IPotassium
- JIodide
5As we go down group seven, the halogens become [blank_start]less[blank_end] reactive and their melting and boiling points [blank_start]increase[blank_end].
[blank_start]Fluorine[blank_end] is the most reactive halogen.
[blank_start]Iodine[blank_end] in the least reactive halogen.- Aless
- Bincrease
- CFluorine
- DIodine
6A more reactive halogen will displace a [blank_start]less[blank_end] reactive [blank_start]halogen[blank_end] from an aqueous [blank_start]solution[blank_end] of its metal [blank_start]halide[blank_end].
For example, chlorine will displace brom[blank_start]ide[blank_end]s and iod[blank_start]ide[blank_end]s as chlorine is more reactive than bromine and iodine but their halides are bromide and iodide.
Bromine is more reactive than iodine so it will displace iod[blank_start]ide[blank_end]s.- Aless
- Bhalogen
- Csolution
- Dhalide
- Eide
- Fide
- Gide
7If chlorine gas is passed through an aqueous solution of potassium bromide, [blank_start]bromine[blank_end] is formed due to the displacement reaction taking place
- Abromine
8Potassium Bromide + Chlorine ---> [blank_start]Potassium[blank_end] Choride + [blank_start]Bromine[blank_end]
Potassium Iodide + Chlorine ---> [blank_start]Potassium[blank_end] [blank_start]Chloride[blank_end] + [blank_start]Iodine[blank_end]
Potassium Iodide + Bromine ---> [blank_start]Potassium[blank_end] [blank_start]Bromide[blank_end] + [blank_start]Iodine[blank_end]- APotassium
- BBromine
- CIodine
- DChloride
- EPotassium
- FPotassium
- GBromide
- HIodine
9The most reactive element in group seven is [blank_start]Fluorine[blank_end], as the reactivity of the elements in group seven [blank_start]decreases[blank_end] as you go down the group. As [blank_start]Fluorine[blank_end] is the most reactive element in group seven it will [blank_start]displace[blank_end] all the other halogens from an aqueous solution of their [blank_start]metal[blank_end] [blank_start]halides[blank_end].
- AFluorine
- Bdecreases
- CFluorine
- Ddisplace
- Emetal
- Fhalides
10Astatine is the [blank_start]fifth[blank_end] element in Group 7. It is a [blank_start]semi[blank_end] - metallic, [blank_start]radioactive[blank_end] element and only very [blank_start]small[blank_end] amounts of it exist naturally. Even so, it is the [blank_start]least[blank_end] reactive of the halogens and, theoretically, would be unable to [blank_start]displace[blank_end] any of the other halogens from an [blank_start]aqueous[blank_end] solution of their [blank_start]metal[blank_end] [blank_start]halides[blank_end].
- Afifth
- Bsemi
- Cradioactive
- Dsmall
- Eleast
- Fdisplace
- Gaqueous
- Hmetal
- Ihalides
11The physical properties of the halogens alter as we go down the group. The melting and boiling points of the halogens [blank_start]increas[blank_end]e going down the group. The density also [blank_start]increase[blank_end]s going down the group, but the reactivity [blank_start]decrease[blank_end]s.
- Aincreas
- Bincrease
- Cdecrease
12Astatine is estimated to have the [blank_start]highest[blank_end] melting point, boiling point and density. The figure for density in the table is [blank_start]estimated[blank_end] by looking at the trend of differences in between each member of the group and adding that difference onto the value of [blank_start]iodine[blank_end], as iodine is the element above astatine in group seven. Accurate figures for astatine are not known because astatine is a very [blank_start]unstable[blank_end] element.
- Ahighest
- Bestimated
- Ciodine
- Dunstable
13The halogens have similar properties as when they react, an atom gains [blank_start]one[blank_end] [blank_start]electron[blank_end] to form a [blank_start]negative[blank_end] ion with a stable electronic structure (full [blank_start]outer[blank_end] [blank_start]shell[blank_end])
Fluorine is the most reactive as it is easiest for it to [blank_start]gain[blank_end] the extra [blank_start]electron[blank_end].
The halogens get [blank_start]less[blank_end] reactive further down the group as they outer [blank_start]shell[blank_end] gets further away from the influence of the [blank_start]nucleus[blank_end], making it harder for the atom to [blank_start]gain[blank_end] an [blank_start]electron[blank_end].- Aone
- Belectron
- Cnegative
- Douter
- Eshell
- Felectron
- Ggain
- Helectron
- Igain
- Jless
- Kshell
- Lnucleus
14[blank_start]Transition[blank_end] [blank_start]metals[blank_end] are the big section on the periodic table between group 2 and 3
- ATransition
- Bmetals
15Transition metals have the typical properties of [blank_start]metals[blank_end]:
1.) Compounds of transition metals are often [blank_start]coloured[blank_end]:
Copper compounds = [blank_start]blue[blank_end]
iron (II) compounds = [blank_start]grey[blank_end]-[blank_start]gree[blank_end]n
iron (III) compounds = [blank_start]orang[blank_end]e-[blank_start]brown[blank_end]
2.) Many transition metals and their compounds can be used as [blank_start]catalysts[blank_end] in [blank_start]chemical[blank_end] reactions:
iron used in [blank_start]haber[blank_end] [blank_start]process[blank_end]
nickel used in the manufacture of [blank_start]margarine[blank_end]- Ametals
- Bcoloured
- Cblue
- Dgree
- Egrey
- Forang
- Gbrown
- Hcatalysts
- Ichemical
- Jhaber
- Kprocess
- Lmargarine
16[blank_start]Thermal[blank_end] [blank_start]decomposition[blank_end] is a reaction in which a substance is broken down, via heat, into simpler substances.
When transition metal [blank_start]carbonates[blank_end] are heated, a [blank_start]colour[blank_end] change occurs and they decompose to form a [blank_start]metal[blank_end] [blank_start]oxide[blank_end] and [blank_start]carbo[blank_end]n [blank_start]dioxide[blank_end].
Eg. [blank_start]Blue[blank_end]-[blank_start]gree[blank_end]n copper carbonate is heated to produce [blank_start]black[blank_end] [blank_start]copper[blank_end] [blank_start]oxide[blank_end] and [blank_start]carbon[blank_end] [blank_start]dioxide[blank_end].- AThermal
- Bdecomposition
- Ccarbonates
- Dcolour
- Emetal
- Foxide
- Gcarbo
- Hdioxide
- IBlue
- Jgree
- Kcopper
- Lblack
- Moxide
- Ncarbon
- Odioxide
17Metal compounds in solution contain [blank_start]metal[blank_end] [blank_start]ions[blank_end], some of which form [blank_start]precipitates[blank_end] ( [blank_start]Insoluble[blank_end] substances) that come out of solution when [blank_start]sodium[blank_end] [blank_start]hydroxide[blank_end] is added to them.
The reaction between the transition metal ions and sodium hydroxide solution is called a [blank_start]precipitation[blank_end] reaction.- Ametal
- Bions
- Cprecipitates
- DInsoluble
- Esodium
- Fhydroxide
- Gprecipitation
18[blank_start]Copper[blank_end] (II) forms a blue precipitate
[blank_start]Iron[blank_end] (II) forms a grey-green precipitate
[blank_start]Iron[blank_end] (III) forms an orange-brown precipitate.- ACopper
- BIron
- CIron
19Metals are very useful because of their physical properties. They:
1.) are [blank_start]lustrous[blank_end] e.g. gold is used in [blank_start]jewellery[blank_end]
2.) are [blank_start]hard[blank_end] and have a high [blank_start]density[blank_end] e.g [blank_start]steel[blank_end] is made to make [blank_start]drill[blank_end] parts
3.) have high [blank_start]tensile[blank_end] [blank_start]strength[blank_end] (able to bear loads) e.g. [blank_start]steel[blank_end] is used to make [blank_start]girders[blank_end]
4.) have [blank_start]high[blank_end] melting and boiling points e.g. [blank_start]tungsten[blank_end] is used to make [blank_start]light[blank_end] [blank_start]bulb[blank_end] [blank_start]filaments[blank_end]
5.) are good [blank_start]conductors[blank_end] of heat electricity e.g. [blank_start]copper[blank_end] is used to make saucepans and [blank_start]wiring[blank_end].- Alustrous
- Bhard
- Cdensity
- Dtensile
- Estrength
- Fsteel
- Gsteel
- Hhigh
- Ilight
- Jbulb
- Kfilaments
- Lgirders
- Mjewellery
- Ndrill
- Otungsten
- Pconductors
- Qcopper
- Rwiring
20Metal atoms are packed so close together that the [blank_start]outer[blank_end] [blank_start]electron[blank_end] shells [blank_start]overlap[blank_end] and form [blank_start]metallic[blank_end] [blank_start]bonds[blank_end]. The [blank_start]overlap[blank_end] allows [blank_start]electrons[blank_end] to [blank_start]move[blank_end] about [blank_start]freely[blank_end]. The structure is closely packed [blank_start]metal[blank_end] [blank_start]ions[blank_end] in a sea of [blank_start]delocalised[blank_end] [blank_start]electrons[blank_end]. The free movement of the [blank_start]delocalised[blank_end] [blank_start]electrons[blank_end] allows the metal to [blank_start]conduct[blank_end] [blank_start]electricity[blank_end] (e.g. in wiring). The metal is held together by [blank_start]strong[blank_end] forces ( the electrostatic attraction between the [blank_start]metal[blank_end] [blank_start]ions[blank_end] and [blank_start]delocalised[blank_end] e[blank_start]lectrons[blank_end]) which is why metals have [blank_start]high[blank_end] melting and boiling points, as lot of [blank_start]energy[blank_end] is needed to overcome these forces.
Packed together, the metal atoms build a structure of [blank_start]crystals[blank_end].- Aouter
- Belectron
- Coverlap
- Dmetallic
- Ebonds
- Ffreely
- Goverlap
- Helectrons
- Imove
- Jdelocalised
- Kelectrons
- Lmetal
- Mions
- Ndelocalised
- Oelectrons
- Pconduct
- Qelectricity
- Rstrong
- Smetal
- Tions
- Udelocalised
- Vlectrons
- Whigh
- Xenergy
- Ycrystals
21At low [blank_start]temperatures[blank_end], some metals can become [blank_start]super[blank_end] [blank_start]conductors[blank_end]. A super conductor has little to no [blank_start]resistance[blank_end] to the flow of [blank_start]electricity[blank_end]. Very low [blank_start]resistance[blank_end] is useful when you require:
1.) A powerful [blank_start]electro[blank_end][blank_start]magnet[blank_end] e.g. inside [blank_start]medical[blank_end] [blank_start]scanners[blank_end]
2.) Very [blank_start]fast[blank_end] electronic [blank_start]circuits[blank_end] e.g. in a [blank_start]super[blank_end] [blank_start]computer[blank_end]
3.) [blank_start]Power[blank_end] transmission that does not [blank_start]lose[blank_end] [blank_start]energy[blank_end]- Asuper
- Bconductors
- Ctemperatures
- Dresistance
- Eelectricity
- Fresistance
- Gelectro
- Hmagnet
- Imedical
- Jscanners
- Kfast
- Lcircuits
- Msuper
- Ncomputer
- OPower
- Plose
- Qenergy
22The majority of super conductors currently work at temperatures below [blank_start]-[blank_end] [blank_start]200[blank_end] degrees. The low temperature is costly to [blank_start]maintain[blank_end] and [blank_start]impractical[blank_end] for [blank_start]large[blank_end] scale uses. People are trying to find a super conductor that will work at [blank_start]room[blank_end] [blank_start]temperature[blank_end] ( [blank_start]20[blank_end] degrees)
- A200
- B-
- Cmaintain
- Dimpractical
- Elarge
- Froom
- Gtemperature
- H20
23The four main sources of water are:
R[blank_start]ivers[blank_end]
[blank_start]Lakes[blank_end]
Re[blank_start]servoirs[blank_end]
[blank_start]Aquifiers[blank_end] ( [blank_start]wells[blank_end] and [blank_start]bore[blank_end] [blank_start]holes[blank_end])- Aivers
- BLakes
- Cservoirs
- DAquifiers
- Ewells
- Fbore
- Gholes
24The [blank_start]chemical[blank_end] industry used large amounts of water for [blank_start]cooling[blank_end], as a [blank_start]solvent[blank_end] and as a [blank_start]cheap[blank_end] [blank_start]raw[blank_end] material.
In some parts of Britain the [blank_start]demand[blank_end] for water is higher than the [blank_start]supply[blank_end], so it's important not to [blank_start]waste[blank_end] water.- Achemical
- Bcooling
- Csolvent
- Dcheap
- Eraw
- Fdemand
- Gsupply
- Hwaste
25Water has to be purified to make sure it is safe to drink. Untreated ( raw ) water can contain:
1.) [blank_start]Insoluble[blank_end] particles
2.) [blank_start]Pollutants[blank_end]
3.) M[blank_start]icrobes[blank_end]
4.) Dissolved [blank_start]salts[blank_end] and m[blank_start]inerals[blank_end]- AInsoluble
- BPollutants
- Cicrobes
- Dsalts
- Einerals
26Water purification stages:
1.) [blank_start]Sedimentation[blank_end] - the water settles to allow the [blank_start]insoluble[blank_end] particles to [blank_start]sink[blank_end]
2.) [blank_start]Filtration[blank_end] - to remove the very [blank_start]fine[blank_end] particles
3.) [blank_start]Chlorination[blank_end] - to kill the [blank_start]microorganisms[blank_end] in the water- ASedimentation
- Binsoluble
- Csink
- DFiltration
- Efine
- FChlorination
- Gmicroorganisms
27Tap water is [blank_start]impure[blank_end]. It contains [blank_start]soluble[blank_end] materials that are not removed in the normal water treatment process. There is the possibility that some of the materials may be poisonous and in that case extra steps must be taken to remove them. Water must be [blank_start]distilled[blank_end] to ensure it is completely [blank_start]pure[blank_end]. [blank_start]Distillation[blank_end] uses a lot of [blank_start]energy[blank_end] so it is very [blank_start]expensive[blank_end].
Huge amounts of expensive [blank_start]energy[blank_end] would be needed to distill [blank_start]sea[blank_end] water. [blank_start]Sea[blank_end] water is quite [blank_start]corrosive[blank_end] so the [blank_start]equipment[blank_end] needed would be very [blank_start]expensive[blank_end] also. Therefore, we are prevented from drinking [blank_start]sea[blank_end] water as the [blank_start]cost[blank_end] is too high- Aimpure
- Bsoluble
- Cdistilled
- DDistillation
- Epure
- Fenergy
- Gexpensive
- Henergy
- Isea
- JSea
- Kcorrosive
- Lequipment
- Mexpensive
- Nsea
- Ocost
28The pollutants found in water supplies include [blank_start]nitrates[blank_end] from the run - off of [blank_start]fertilisers[blank_end], [blank_start]lead[blank_end] compounds from old [blank_start]pipes[blank_end] in plumbing, and [blank_start]pesticides[blank_end] from spraying [blank_start]crops[blank_end] near to the [blank_start]water[blank_end] supply. These are hard to [blank_start]remove[blank_end] from the water.
- Anitrates
- Bfertilisers
- Clead
- Dpipes
- Epesticides
- Fcrops
- Gwater
- Hremove
29A precipitation reaction occurs when an [blank_start]insoluble[blank_end] [blank_start]solid[blank_end] is made from mixing two solutions together.
The dissolved ions of some salts are easy to identify as they undergo [blank_start]precipitation[blank_end] [blank_start]reactions[blank_end].
[blank_start]Sulfates[blank_end] can be detected using [blank_start]barium[blank_end] [blank_start]chloride[blank_end] solution : a [blank_start]white[blank_end] precipitate of [blank_start]barium[blank_end] [blank_start]sulfate[blank_end] forms.- Ainsoluble
- Bsolid
- Cprecipitation
- Dreactions
- ESulfates
- Fbarium
- Gchloride
- Hwhite
- Ibarium
- Jsulfate
30[blank_start]Silver[blank_end] [blank_start]nitrate[blank_end] solution is used to detect halide ions: ( [blank_start]Halide[blank_end] ions are the ions made by the [blank_start]Halogens[blank_end] - group 7 )
C[blank_start]hlorides[blank_end] form a [blank_start]white[blank_end] precipitate
B[blank_start]romides[blank_end] form a [blank_start]cream[blank_end] precipitate
I[blank_start]odides[blank_end] from a [blank_start]yellow[blank_end] precipitate.- ASilver
- Bnitrate
- CHalogens
- DHalide
- Ehlorides
- Fwhite
- Gromides
- Hcream
- Iodides
- Jyellow
Información
- Descripción
- GCSE Chemistry Test sobre C4 - Part 3, creado por Verity Cartwright el 19/03/2017.
- Autor
- Verity Cartwright
- Idioma
- English
- Visitas
- 2
- Etiquetas
- Valoración
- Aún sin valoraciones Valora este test