C2 quiz

1. 1The mass number is the total number of [blank_start]protons and neutrons[blank_end] in an atom.

   1. Aprotons and neutrons
2. 2The atomic number is the total number of [blank_start]protons[blank_end] in an atom.

   1. Aprotons
3. 3Isotopes are [blank_start]different[blank_end] atomic forms of the [blank_start]same[blank_end] element which have the same number of [blank_start]protons[blank_end] but a different number of [blank_start]neutrons[blank_end].

   1. Asame
   2. Bdifferent
   3. Csame
   4. Ddifferent
   5. Eprotons
   6. Fneutrons
   7. Gprotons
   8. Hneutrons
4. 4In ionic bonding, atoms [blank_start]lose or gain[blank_end] electrons to form [blank_start]charged[blank_end] particles (ions) which are then [blank_start]strongly[blank_end] attracted to each other.

   1. Alose or gain
   2. Bcharged
   3. Cstrongly
5. 5Ionic bonding is between

   1. Aa metal and a non-metal
   2. Btwo metals
   3. Ctwo non-metals
6. 6Ionic bonding normally happens between group 1 or 2( which [blank_start]lose[blank_end] one or two electrons) and group 6 or 7 (which [blank_start]gain[blank_end] one or two electrons).

   1. Alose
   2. Bgain
7. 7Describe the structure of an ionic compound.

   1. Agiant ionic lattice
   2. Bclosely packed regular arrangement
   3. Cparticles can easily slide over each other
   4. Dstrong forces of attraction between particles
   5. Eweak forces of attraction between particles
   6. Fsame structure as a noble gas
   7. Gsame structure as halogens
8. 8There are very strong [blank_start]electrostatic[blank_end] forces of attraction between [blank_start]oppositely[blank_end] charged ions in all directions, which is why particles in ionic bonds are strongly attracted.

   1. Aelectrostatic
   2. Boppositely
9. 9Ionic compounds have [blank_start]high[blank_end] melting points and [blank_start]high[blank_end] boiling points because it takes a large amount of energy to overcome the strong attraction between the ions. When ionic compounds melt they [blank_start]can[blank_end] carry electric current. They [blank_start]do[blank_end] dissolve easily in water so easily carry electric current in the solution.

   1. Ahigh
   2. Bhigh
   3. Ccan
   4. Ddo
10. 10Group 1/2 is [blank_start]positively[blank_end] charged.
    
    Group 6/7 is [blank_start]negatively[blank_end] charged.

    1. Apositively
    2. Bnegatively
    3. Cnegatively
    4. Dpositively

11. 11Atoms that have lost or gained an electron are called [blank_start]ions[blank_end].

    1. Aions
12. 12Group 1 and 2 elements are [blank_start]metals[blank_end] and they [blank_start]lose[blank_end] electrons to form [blank_start]positive[blank_end] ions. Group 6 and 7 elements are [blank_start]non-metals[blank_end] and they [blank_start]gain[blank_end] electrons to form [blank_start]negative[blank_end] ions.

    1. Ametals
    2. Bnon-metals
    3. Close
    4. Dgain
    5. Epositive
    6. Fnegative
    7. Gnon-metals
    8. Hmetals
    9. Igain
    10. Jlose
    11. Knegative
    12. Lpositive
13. 13+ or - symbols tell you what type of ion the atom will form in a chemical reaction i.e. Sodium metal, Na, is neutral so + ions will only appear if the sodium metal reacts with something like water or chlorine (loses one or more electrons)

    1. ARichtig
    2. BFalsch
14. 14Covalent bonds are formed when atoms [blank_start]share[blank_end] electrons.

    1. Ashare
15. 15IN COVALENT BONDING:
    
    Hydrogen atoms share [blank_start]one[blank_end] electron.
    Chlorine atoms share [blank_start]one[blank_end] electron.
    In methane CH4, carbon shares [blank_start]four[blank_end] electrons with hydrogen.
    In Hydrogen Chloride HCl, hydrogen and chlorine share [blank_start]one[blank_end] electron.
    In Ammonia NH3, Nitogen makes [blank_start]three[blank_end] covalent bonds (shares [blank_start]three[blank_end] electrons) with hydrogen.
    In water H2O, Oxygen atoms share [blank_start]two[blank_end] electrons with hydrogen atoms.
    In Oxygen O2, [blank_start]two[blank_end] electrons are shared and a [blank_start]double[blank_end] covalent bond is formed.

    1. Aone
    2. Bone
    3. Cfour
    4. Done
    5. Ethree
    6. Fthree
    7. Gtwo
    8. Htwo
    9. Idouble
16. 16Covalent bonds are between

    1. Aa metal and non-metal
    2. Ba metal and metal
    3. Ca non-metal and non-metal
17. 17Substances bonded covalently are [blank_start]molecules[blank_end].

    1. Amolecules
18. 18Covalent bonds form simple molecular substances.
    
    Describe the structure and properties of a simple molecular substance.

    1. Aatoms formed very strong covalent bonds to form small molecules of several atoms.
    2. Batoms formed very weak covalent bonds to form small molecules of one atom.
    3. Cforces of attraction between molecules are very weak.
    4. Dforces of attraction between molecules are very strong.
    5. Elow melting and boiling points
    6. Fdon't conduct electricity
    7. Ghigh melting and boiling point.
    8. Hintermolecular forces break when simple molecular substances melt or boil.
    9. Icovalent bonds break when simple molecular substances melt or boil.
    10. Jmost molecular substances are gases or liquids at room temperature but they can be solids
19. 19Covalent bonds form giant covalent structures called macromolecules.
    
    Describe the structure and properties of a macromolecule.

    1. Aatoms bonded by strong covalent bonds.
    2. Batoms bonded by weak covalent bonds.
    3. Chigh melting and boiling points
    4. Ddon't conduct electricity (graphite does when molten)
20. 20Which macromolecule is this:
    -four rigid covalent bonds
    -hardest natural substance
    -used for drill tips

    1. Adiamond
    2. Bsilicon dioxide
    3. Cgraphite
21. 21Which macromolecule is this:
    -makes sand
    

    1. Adiamond
    2. Bsilicon dioxide
    3. Cgraphite
22. 22Which macromolecule is this?
    -carbon atoms which each only form three covalent bonds
    -layers which are free to slide over each other: therefore soft and slippery
    -layers are held together loosely so can be rubbed off due to weak intermolecular forces between the layers
    -non-metal which is a good conductor of heat and electricity due to each carbon atom having one delocalised electron

    1. Adiamond
    2. Bsilicon dioxide
    3. Cgraphite
23. 23Metallic bonding is between

    1. Aa metal and non-metal
    2. Ba metal and metal
    3. Ca non-metal and non-metal
24. 24Describe the structure and properties of metallic structures.

    1. Aevery metal atom's outer shell has a delocalised electron
    2. Bgood conductors of heat and electricity
    3. Cpoor conductors of heat and electricity
    4. Dfree electrons hold atoms together in a regular structure
    5. Efree electrons cause structure to be random
    6. Fstrong forces of electrostatic attraction between positive metal ions and negative electrons
    7. Glayers can slide over each other and bend
    8. Hvery rigid
25. 25[blank_start]Alloys[blank_end] are formed when two or more metals are mixed together. They have desired properties.

    1. AAlloys, alloy, an alloy
26. 26Alloys are [blank_start]harder[blank_end] than pure metals.

    1. Aharder
    2. Bsofter
    3. Cmore bendy
27. 27The following are properties of a substance:
    
    -very low melting and boiling points
    -poor electrical conductor
    
    Which substance is it?

    1. Agiant ionic
    2. Bsimple molecular
    3. Cgiant covalent
    4. Dgiant metallic
28. 28The following are properties of a substance:
    
    -high melting and boiling points
    -good electrical conductor
    
    Which substance is it?

    1. Agiant ionic
    2. Bsimple molecular
    3. Cgiant covalent
    4. Dgiant metallic
29. 29The following are properties of a substance:
    
    -high melting and boiling points
    -poor electrical conductor
    
    Which substance is it?

    1. Agiant ionic
    2. Bsimple molecular
    3. Cgiant covalent
    4. Dgiant metallic
30. 30The following are properties of a substance:
    
    -high melting and boiling points
    -conduct electricity when molten
    
    Which substance is it?

    1. Agiant ionic
    2. Bsimple molecular
    3. Cgiant covalent
    4. Dgiant metallic
31. 31Smart materials behave differently depending on the [blank_start]conditions[blank_end], such as temperature. [blank_start]Shape memory[blank_end] alloys can be bent out of shape but will always go back to how they were before. For example, nitinol can be bent and twisted like rubber when cool, but then heated it goes back to its original shape. They are used in braces and in glasses frames.
    

    1. Aconditions
    2. BShape memory
32. 32Nanoparticles contain fullerenes which are molecules of [blank_start]carbon[blank_end], shaped like hollow balls. The carbon atoms are arranged in [blank_start]hexagonal[blank_end] rings. Different fullerenes contain [blank_start]different[blank_end] numbers of atoms. Fullerenes can be joined together to form [blank_start]nanotubes[blank_end] which are tiny hollow carbon tubes. Covalent bonds make carbon nanotubes very [blank_start]strong[blank_end] so can be used to reinforce graphite in tennis rackets.
    

    1. Acarbon
    2. Bhexagonal
    3. Cdifferent
    4. Dnanotubes
    5. Estrong
33. 33How can nanoparticles be used?

    1. Ahuge surface area to volume ratio so could help make new industrial catalysts
    2. Bsensors to detect water purity
    3. Cstronger, lighter building materials
    4. Dcosmetics that don't leave white marks on the skin
    5. Enano medicine wherein fullerenes are absorbed more easily into the body so drugs are delivered right into the cells where theyre needed
    6. Flubricant coatings developed for artificial joints and gears
    7. Gtiny electric circuits for computer chips as nanotubes conduct electricity
34. 34Nanoparticles include fullerenes.
    
    What is meant by the term fullerenes?

    1. Amolecules of hydrogen shaped like hollow balls or closed tubes, all arranged in hexagonal rings
    2. Bmolecules of graphite shaped like hollow balls or closed tubes, all arranged in hexagonal rings
    3. Cmolecules of carbon shaped like hollow balls or closed tubes, all arranged in hexagonal rings
35. 35All plastic-no matter its properties-is a [blank_start]polymer[blank_end].

    1. Apolymer
36. 36[blank_start]Strong[blank_end] covalent bonds hold the atoms together in [blank_start]long[blank_end] chains. The bonds between different molecule chains determine the properties of the plastic.

    1. AStrong
    2. Blong
37. 37polymers with weak forces of attraction:

    1. Aare called thermosoftening polymers
    2. Bare called thermosetting polymers
    3. Cdon't have cross-linking between chains
    4. Dhave crosslinks which hold the chains together in a solid structure
    5. Ethe forces between chains are really easy to overcome so it's easy to melt the plastic-when it cools, the polymer hardens into a new shape so they can be melted and remoulded a lot
    6. Fdon't soften when heated
    7. Gare strong, hard and rigid
38. 38The starting materials and reaction conditions will both affect the properties of a polymer.

    1. ARichtig
    2. BFalsch
39. 39Low density polythene is made by heating ethene to about 200ºC under [blank_start]high[blank_end] pressure. It's [blank_start]flexible[blank_end] and is used for bags/bottles.
    High density polythene is made at a lower temperature under [blank_start]low[blank_end] pressure using a catalyst. It's more [blank_start]rigid[blank_end] and is used for water tanks and drain pipes.

    1. Ahigh
    2. Bflexible
    3. Clow
    4. Drigid
40. 40Relative atomic mass is the same as the [blank_start]mass number[blank_end] in an element.

    1. Amass number
41. 41Relative formula mass of a compound is found by adding each [blank_start]relative atomic mass[blank_end] together.

    1. Arelative atomic mass
42. 42One mole of a substance is equal to its [blank_start]relative formula mass in grams[blank_end].

    1. Arelative formula mass in grams
43. 43Number of moles=

    1. Amass in g of element or compound/relative formula mass of element or compound
    2. Brelative atomic mass of element/relative formula mass of element or compound
    3. Cmass in kg of element or compound/relative formula mass of element or compound
44. 44percentage mass of an element in a compound=

    1. A(relative atomic mass x number of atoms of that element/relative formula mass of compound) x 100
    2. Brelative formula mass/relative atomic mass
45. 45To find the empirical formula:
    
    1) [blank_start]list all elements in compound[blank_end]
    2) [blank_start]write experimental masses or percentages[blank_end]
    3) divide [blank_start]each mass/percentage by element's Ar[blank_end]
    4)[blank_start]make ratio[blank_end]
    
    5) [blank_start]simplify[blank_end]

    1. Alist all elements in compound
    2. Bwrite experimental masses or percentages
    3. Ceach mass/percentage by element's Ar
    4. Deach mass by element's Ar
    5. Eeach percentage by element's Ar
    6. Feach mass or percentage by Mr
    7. Geach mass by Mr
    8. Heach percentage by Mr
    9. Imake ratio
    10. Jsimplify
46. 46To find the mass in a reaction:
    
    1) [blank_start]write out balanced equation[blank_end]
    
    2) [blank_start]work out the Mr for what you need[blank_end]
    3) [blank_start]divide to get one, multiply to get all[blank_end]

    1. Awrite out balanced equation
    2. Bwork out the Mr for what you need
    3. Cdivide to get one, multiply to get all
47. 47Yields are always [blank_start]less than 100%.[blank_end]

    1. Aless than 100%.
48. 48A reversible reaction is hen the [blank_start]products of the reaction[blank_end] keep reacting to [blank_start]produce the original reactants[blank_end].

    1. Aproducts of the reaction
    2. Bproduce the original reactants
49. 49Which three things may cause product to be lost during a reaction?

    1. Afiltering a liquid
    2. Breversible reactions
    3. Cunexpected reactions
    4. Dincorrect equipment
    5. Etoo much of a reactant
50. 50Artificial colours can be separated using [blank_start]paper chromatography[blank_end].

    1. Apaper chromatography
51. 51When using paper chromatography, what should you do?

    1. Adraw the baseline in pen
    2. Bdraw the baseline in pencil
    3. Cuse filter paper
    4. Duse solvent and a food sample to extract colour
    5. Emake sure the baseline is below the solvent
52. 52Three advantages of using machines to analyse unknown substances are that they're very sensitive, very fast and very accurate.

    1. ARichtig
    2. BFalsch
53. 53Gas chromatography can be used to identify substances. How does gas chromatography work?
    
    1) a gas carries substances through a column packed with [blank_start]solid[blank_end] material
    
    2) the substances travel through the tube at different [blank_start]speeds[blank_end], so they're separated
    
    3) the [blank_start]retention time[blank_end] is used to identify these substances.
    
    4) the recorder draws a [blank_start]gas chromatograph[blank_end]
    
    5) the [blank_start]number[blank_end] of peaks show the different compounds in the sample
    
    6) the [blank_start]position[blank_end] of the peaks show each substance's retention time.
    
    7) gas chromatography column can be linked to a mass spectrometer (GC-MS) in order to work out each substance's [blank_start]relative molecular mass[blank_end] by reading from the molecular ion peal.

    1. Asolid
    2. Bliquid
    3. Cgas
    4. Dspeeds
    5. Etimes
    6. Fretention time
    7. Ggas chromatograph
    8. Hnumber
    9. Iposition
    10. Jrelative molecular mass
    11. Krelative atomic mass
54. 54The rate of reaction depends on

    1. Atemperature
    2. Bconcentration of liquid
    3. Cgas pressure
    4. Dcatalyst
    5. Esurface area of solid pieces
55. 55rate of reaction=

    1. Aamount of reactant used or around of product formed/time
    2. Bamount of reactant used or around of product formed x time
    3. Ctime/amount of reactant used or around of product formed
56. 56The rate of reaction can be measured by
    
    a) [blank_start]precipitation[blank_end]-how long it takes for a mark through a solution to disappear as gas clouds form
    D: [blank_start]subjective[blank_end], [blank_start]only for see-through reactions[blank_end]
    
    b) [blank_start]change in mass[blank_end]-metal balanced used to measure decreasing mass as more gas is produced
    [blank_start]A: most accurate[blank_end] D[blank_start]: gas is released straight into the room[blank_end]
    c) [blank_start]volume of gas given off[blank_end]-using a gas syringe
    [blank_start]A: very accurate[blank_end] D: [blank_start]vigorous reactions will[blank_end] [blank_start]blow the plunger out of the syringe[blank_end]

    1. Aprecipitation
    2. Bsubjective
    3. Conly for see-through reactions
    4. Dchange in mass
    5. EA: most accurate
    6. F: gas is released straight into the room
    7. Gvolume of gas given off
    8. HA: very accurate
    9. Ivigorous reactions will
    10. Jblow the plunger out of the syringe
57. 57The reaction of Hydrochloric Acid and marble chips demonstrates...

    1. Ahow increased concentration affects the rate of reaction
    2. Bhow surface area affects the rate of reaction
    3. Chow catalysts affect the rate of reaction
58. 58The reaction of magnesium metal with dilute HCl demonstrates

    1. Ahow concentration affects the rate of reaction
    2. Bhow temperature affects the rate of reaction
    3. Chow surface area affects the rate of reaction
59. 59the reaction of sodium thiosulfate and hydrochloric acid demonstrates...

    1. Ahow temperature and concentration affect the rate of reaction
    2. Bhow concentration and catalysts affect the rate of reactions
    3. Chow catalysts and temperature affect the rate of reaction
60. 60the decomposition of hydrogen peroxide demonstrates...
    
    

    1. Ahow catalysts affect the rate of reaction
    2. Bhow surface area affects the rate of reaction
    3. Chow temperature affects the rate of reaction
61. 61Describe a practical which demonstrates the effect of surface area on the rate of reaction.
    
    Reaction: [blank_start]Hydrochloric acid and marble chips[blank_end]
    
    1) measure the [blank_start]volume of gas produced[blank_end] using a [blank_start]gas syringe[blank_end] and take readings at regular intervals.
    2) repeat with same volumes but [blank_start]more crunched up chips[blank_end] until [blank_start]the mass is powdered chalk[blank_end]

    1. AHydrochloric acid and marble chips
    2. BMagnesium metal+dilute hydrochloric acid
    3. CSodium thiosulfate+hydrochloric acid
    4. DThe decomposition of hydrogen peroxide
    5. Egas syringe
    6. Fmass balance
    7. Gblack mark
    8. Hvolume of gas produced
    9. Itime it takes for the mark to disappear
    10. Jloss in mass
    11. Kmore crunched up chips
    12. Lmore concentrated acid solutions
    13. Mat different temperatures
    14. Ndifferent volumes of catalyst
    15. Othe mass is powdered chalk
    16. Pthe loss in mass plateaus
    17. Qthe temperature is dangerously high
62. 62Describe a practical which tests the effect of concentration on the rate of reaction.
    
    Reaction: [blank_start]magnesium metal+dilute hydrochloric acid[blank_end]
    
    1) combine reactants and measure [blank_start]the volume of hydrogen gas given off[blank_end] using a mass balance
    2) repeat with the same volume of [blank_start]acid[blank_end] but [blank_start]increased concentration[blank_end]

    1. Amagnesium metal+dilute hydrochloric acid
    2. Bdecomposition of hydrogen peroxide
    3. Chydrochloric acid+marble chips
    4. Dsodium thiosulphate+hydrochloric acid
    5. Ethe volume of hydrogen gas given off
    6. Fthe time it takes for mark to disappear
    7. Gthe volume of gas produced
    8. Hthe volume of oxygen gas given off
    9. Iacid
    10. Jmarble chips
    11. Kincreased concentration
    12. Lcrushing them up more
    13. Mat different temperatures
    14. Nincreased volume of catalysts
63. 63Describe a practical that tests the effect of concentration or temperature on the rate of reaction.
    
    Reaction: [blank_start]sodium thiosulphate+hydrochloric acid[blank_end]
    
    1) combine reactants and measure the time it takes for the [blank_start]sulfur precipitate formed[blank_end] [blank_start]to cover the black mark[blank_end]
    2) repeat at different temperatures or with different concentrations

    1. Asodium thiosulphate+hydrochloric acid
    2. Bhydrochloric acid+marble chips
    3. Cmagnesium metal+dilute hydrochloric acid
    4. Dthe decomposition of hydrogen peroxide
    5. Esulfur precipitate formed
    6. Fvolume of gas produced to fill
    7. Gto cover the black mark
    8. Hthe gas syringe
64. 64Describe a practical that tests the effect of catalysts on the rate of reaction.
    
    Reaction: [blank_start]decomposition of hydrogen peroxide[blank_end]
    1) combine the reactants and measure how long it takes [blank_start]for oxygen gas to be given off[blank_end] (plot volume against time)
    2) [blank_start]add manganese oxide and measure again[blank_end]
    3) repeat increasing the [blank_start]mass of the catalyst[blank_end]

    1. Adecomposition of hydrogen peroxide
    2. Bsodium thiosulphate+hydrochloric acid
    3. Cmagnesium metal+dilute hydrochloric acid
    4. Dhydrochloric acid+marble chips
    5. Efor oxygen gas to be given off
    6. Ffor hydrogen gas to be given off
    7. Gfor the black mark to disappear
    8. Hadd manganese oxide and measure again
    9. Iplot on graph
    10. Jmass of the catalyst
    11. Kconcentration
    12. Ltemperature
    13. Mcrunched up chips
65. 65More collisions increases the rate of reaction. Factors that increase collisions are:
    
    1) [blank_start]higher temperature[blank_end]-particles move quicker
    2) [blank_start]higher concentration/pressure[blank_end]-more reactant particles
    3) [blank_start]larger surface area[blank_end]-more exposed particles

    1. Ahigher temperature
    2. Bhigher concentration/pressure
    3. Clarger surface area
66. 66The [blank_start]activation energy[blank_end] is the minimum amount of energy needed by the particles to react.

    1. Aactivation energy
67. 67A [blank_start]catalyst[blank_end] is a substance which speeds up a reaction without being changed or used up in the reaction.

    1. Acatalyst
68. 68Tick what is correct about catalysts.

    1. Athey reduce costs in industrial reactions
    2. Bthey allow reactions to work at lower temperatures
    3. Cthey are very cheap
    4. Dthey are very expensive
    5. Ethey can be reused
    6. Fthey can only be used once
    7. Gdifferent reactions use different catalysts
    8. Himpurities can cause the catalyst to stop working so they need to be kept clean

Beschreibung

GCSE chemistry Quiz am C2 quiz, erstellt von Tess Brockway am 04/04/2016.

Autor

Tess Brockway

Sprache

English

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chemistrygcse

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