Chemistry AS Chapter 7

1. 1[blank_start]Mendeleev[blank_end] left gaps for elements that he believed to come due to his arrangements.

   1. AMendeleev
2. 2The periodic table has 115 elements

   1. ATrue
   2. BFalse
3. 3The positioning of elements is due to their physical and [blank_start]chemical[blank_end] properties.

   1. Achemical
4. 4Elements are arranged from left to right in increasing atomic number order. Each successive atom has one more proton.

   1. ATrue
   2. BFalse
5. 5Each element in a group has atoms with the same number of outer-shell [blank_start]electrons[blank_end] and similar properties.

   1. Aelectrons
6. 6Horizontal rows in the periodic table are called [blank_start]periods[blank_end]

   1. Aperiods
   2. Brows
   3. Cgroups
7. 7The number of the period gives the number of [blank_start]the highest energy electron shel[blank_end]l in an element's atom.

   1. Athe lowest energy electron shell
   2. Bthe highest energy electron shell
   3. Cthe number of outer electrons
8. 8The repeating trend across a period is called [blank_start]periodicity[blank_end].

   1. Aperiodicity
9. 9Going across a period, the sub-shells that fill are [blank_start]s[blank_end] and p.

   1. As
   2. Bd
   3. Cf
10. 10Groups tend to have similar chemistry.

    1. ATrue
    2. BFalse

11. 11Blocks are sections in the periodic table that are corresponding to elements highest energy level.

    1. ATrue
    2. BFalse
12. 12Group 7 elements are called the [blank_start]halogens[blank_end].

    1. Ahalogens
13. 13The transition metals are just group 3

    1. ATrue
    2. BFalse
14. 14Ionisation energy measures how easily an atom [blank_start]loses[blank_end] electrons to form a positive ions.

    1. Aloses
15. 15The first ionisation energy is the energy needed to remove [blank_start]one[blank_end] electron from each atom in one [blank_start]mole[blank_end] of gaseous atoms of an element to form one mole of gaseous +1 ions.

    1. Aone
    2. Bmole
16. 16Many factors affect first ionisation energy. The first electron lost will be in the [blank_start]highest[blank_end] energy shell and will experience the [blank_start]least[blank_end] attraction from the nucleus.

    1. Ahighest
    2. Blowest
    3. Cmost
    4. Dleast
17. 17Electrons are held in their shells due to attraction from the nucleus.

    1. ATrue
    2. BFalse
18. 18The factors that affect the attraction between the nucleus and electrons are and therefore the ionisation energy are:

    1. Aatomic radius
    2. Bnuclear charge
    3. Catoms around it or are bonded to
    4. Delectron shielding
19. 19The higher the atomic radius (size) the [blank_start]less[blank_end] attraction for the electron to the nucleus.

    1. Aless
    2. Bmore
20. 20Nuclear attraction is higher when there are [blank_start]more[blank_end] protons in the nucleus creating a [blank_start]bigger[blank_end] attraction.

    1. Amore
    2. Bbigger
21. 21Electrons are [blank_start]negatively[blank_end] charged so inner shell electrons can [blank_start]repel[blank_end] outer shell electrons.

    1. Anegatively
    2. Bpositively
    3. Cattract
    4. Drepel
22. 22The repulsion from inner electrons to outer electrons is called the [blank_start]shielding[blank_end] effect and [blank_start]reduces[blank_end] the attraction between the nucleus and outer electrons.

    1. Ashielding
    2. Brepulsion
    3. Creduces
    4. Dincreases
23. 23Elements have as many successive ionsiation energies as they have electrons.

    1. ATrue
    2. BFalse
24. 24the second [blank_start]ionisation[blank_end] energy is the energy required to remove [blank_start]one[blank_end] electron from each atom in 1 mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions.

    1. Aone
    2. Btwo
    3. Cthree
    4. Dionisation
    5. Echarge
25. 25Successive ionisation energies are what provide evidence for different electron energy levels in an atom.

    1. ATrue
    2. BFalse
26. 26Successive ionisation energy allows predictions for:

    1. AThe number of electrons in the outer shell
    2. BThe amount of neutrons
    3. CThe period of the element
    4. DThe group of the element
    5. EThe identity of an element
27. 27There is a general [blank_start]increase[blank_end] in first ionisation energies across each period.

    1. Aincrease
    2. Bdecrease
28. 28There is a sharp increase in first ionisation energy between the end of one period and the start of the next.

    1. ATrue
    2. BFalse
29. 29First ionisation energies [blank_start]decrease[blank_end] down a group.

    1. Adecrease
30. 30Noble gasses tend to have the highest first ionisation energies.

    1. ATrue
    2. BFalse
31. 31First ionisation energy [blank_start]decreases[blank_end] down every group for the same reason.

    1. Adecreases
    2. Bincreases
32. 32Down a group [blank_start]atomic radius[blank_end] increases which effects the first ionistaion energy but is outweighed by the increased [blank_start]radius[blank_end] and shielding.

    1. Aatomic radius
    2. Bnuclear charge
    3. Cradius
    4. Dcharge
33. 33The trends down the group are: (The first ionsiation energy decreases)

    1. Aatomic radius decrease
    2. Batomic radius increases
    3. Cnuclear charge increases
    4. Dnuclear charge decreases
    5. Eincreased shielding
    6. Fdecreased shielding
34. 34The general trends in first ionisation energies across a period are:

    1. ANuclear charge increase
    2. BNuclear charge decrease
    3. CIncreased shielding
    4. DNo effect from shielding
    5. EAtomic radius decrease
    6. FAtomic radius increase
35. 35First ionisation energy falls twice across a period in the same places.

    1. ATrue
    2. BFalse
36. 36The 2p sub shell has [blank_start]higher[blank_end] energy than the 2s sub shell. This means the 2p electron is [blank_start]easier[blank_end] to remove than a 2s electron.

    1. Alower
    2. Bhigher
    3. Ceasier
    4. Dharder
37. 37The second fall in first ionisation energy is due to electron pairing in the P orbitals of the P sub shell.

    1. ATrue
    2. BFalse
38. 38In nitrogen and oxygen the highest energy shell is 2p

    1. ATrue
    2. BFalse
39. 39In oxygen the paired electrons in one of the 2p orbitals [blank_start]repel[blank_end] one another making it easier to remove an electron than nitrogen. So the first ionisation energy is [blank_start]less[blank_end] for oxygen than nitrogen.

    1. Arepel
    2. Battract
    3. Cmore
    4. Dless
40. 40Elements such as boron and silicon can be known as metalloids or semi-metals as they sit on the metal/non-metal divide.

    1. ATrue
    2. BFalse
41. 41There are [blank_start]92[blank_end] metals and [blank_start]22[blank_end] non-metals

    1. A92
    2. B91
    3. C87
    4. D20
    5. E22
    6. F23
42. 42At room temperature all metal elements are solid.

    1. ATrue
    2. BFalse
43. 43Metals have a range of properties e.g. strong, light ,soft and dense.

    1. ATrue
    2. BFalse
44. 44All [blank_start]metals[blank_end] can conduct electricity.

    1. Ametals
45. 45In each metal structure, each atom has donated its negative outer electrons to a shared pool of electrons which are called [blank_start]delocalised[blank_end] electrons.

    1. Adelocalised
46. 46[blank_start]Metallic[blank_end] bonding is the strong [blank_start]electrostatic[blank_end] attraction between cations and delocalised electrons.

    1. Aelectrostatic
    2. BMetallic
47. 47The [blank_start]cations[blank_end] are in a fixed position and the delocalised electrons are [blank_start]mobile[blank_end].

    1. Amobile
    2. Bstill
    3. Ccations
    4. Danions
    5. Edelocalised electrons
48. 48For a 2+ cation, there are twice as many delocalised electrons.

    1. ATrue
    2. BFalse
49. 49Metallic bonding results in a giant [blank_start]metallic lattice[blank_end]

    1. Aionic lattice
    2. Bmetallic lattice
    3. Ccovalent structure
50. 50Most metals have the properties:

    1. Ahigh melting and boiling points
    2. Blow melting and boiling points
    3. Cstrong metallic bonds (between positive ions and delocalised electrons)
    4. Dlow electrical conductivity
    5. Ehigh electrical condictivity
51. 51Metals can conduct electricity as a solid or a liquid

    1. ATrue
    2. BFalse
52. 52When voltage is applied to a metal the [blank_start]delocalised electrons[blank_end] can move through the strucutre carrying the [blank_start]charge[blank_end].

    1. Adelocalised electrons
    2. Belectrons
    3. Cions
    4. Dcharge
    5. Evibration
    6. Fenergy
53. 53Ionic structure have mobile ions in their solid state.

    1. ATrue
    2. BFalse
54. 54Group 1 metals have the lowest melting a boiling points of the metals.

    1. ATrue
    2. BFalse
55. 55The melting point depends on the [blank_start]strength[blank_end] of the metallic bonding holding together the atoms in the [blank_start]giant[blank_end] metallic lattice.

    1. Astrength
    2. Bsize
    3. Cgiant
    4. Dsmall
56. 56Most metals need [blank_start]high[blank_end] temperatures to melt as a large amount of energy is needed to break the [blank_start]electrostatic[blank_end] attraction between the cations and electrons.

    1. Ahigh
    2. Belectrostatic
57. 57Metals can dissolve

    1. ATrue
    2. BFalse
58. 58Non-metallic elements can exist as simple bonded molecules. When [blank_start]solid[blank_end] these form a simple molecular lattice which has [blank_start]weak[blank_end] intermolecular forces meaning it has low melting and boiling points.

    1. Asolid
    2. Bweak
59. 59What 3 elements exist as a giant covalent structure?

    1. ABoron
    2. BAluminium
    3. CSilicon
    4. DCarbon
    5. EArsenic
60. 60Giant covalent structures have strong covalent bonds.

    1. ATrue
    2. BFalse
61. 61Carbon (in it's diamond form) and silicon have [blank_start]4[blank_end] outer shell electrons which are what form [blank_start]covalent[blank_end] bonds to other carbon or silicon atoms.

    1. A5
    2. B4
    3. C3
    4. Dcovalent
    5. Emetallic
    6. Fionic
    7. Gintermolecular
62. 62Carbon and silicon form giant covalent strucutres. Their structure is tetrahedral.

    1. ATrue
    2. BFalse
63. 63Carbon and silicons bond angles are [blank_start]109.5[blank_end]

    1. A109.5
    2. B120
    3. C90
64. 64Giant covalent lattices have [blank_start]high[blank_end] melting and boiling points as covalent bonds are [blank_start]strong[blank_end].

    1. Ahigh
    2. Blow
    3. Cweak
    4. Dstrong
65. 65Giant covalent lattices are [blank_start]insoluble[blank_end] in most solvents.

    1. Ainsoluble
    2. Bsoluble
66. 66Giant covalent lattices are [blank_start]non-conductors[blank_end] of electricity. Apart from [blank_start]graphite[blank_end] and grapheme which are forms of carbon.

    1. Agraphite
    2. Bsilicon
    3. Caluminium
    4. Dnon-conductors
    5. Econductors
67. 67Carbon can conduct electricity as it forms several structures where one electron is left available to conduct the electricity.

    1. ATrue
    2. BFalse
68. 68Carbon and silicon can't conduct electricity because all [blank_start]4[blank_end] electrons are used in covalent bonding so [blank_start]none[blank_end] are available to carry the charge.

    1. A4
    2. Bnone
69. 69All of carbons giant covalent structures are based on planar hexagonal layers.

    1. ATrue
    2. BFalse
70. 70Graphene and graphite have bond angles of [blank_start]120[blank_end]

    1. A120
71. 71Graphene is a [blank_start]single[blank_end] layer of carbon which is composed by hexagonally arranged atoms that are linked by [blank_start]strong[blank_end] covalent bonding.

    1. Asingle
    2. Bdouble
    3. Cweak
    4. Dstrong
72. 72Graphene has the properties:

    1. Aelectrical conductivity
    2. Bstrong
    3. Csoluble
    4. Dthin
    5. Ethick
73. 73Covalent bonds are what hold together layers of grapheme.

    1. ATrue
    2. BFalse
74. 74Across periods 2 and 3, melting point [blank_start]increases[blank_end] from group 1 to 14

    1. Aincreases
    2. Bdecreases
75. 75There is a sharp decrease in melting point between group 14 and 15

    1. ATrue
    2. BFalse
76. 76Melting points are3 higher from group 15-18

    1. ATrue
    2. BFalse
77. 77The trend in melting points across periods 2 and 3 also happens to period 4 downwards but just in s and p blocks as it doesn't apply to d block (transition metals).

    1. ATrue
    2. BFalse

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Quiz on Chemistry AS Chapter 7, created by emilycoral on 04/01/2016.

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