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chemistry 11b > The Solid State: Lattice Structure > Flashcards

The Solid State: Lattice Structure Flashcards

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1
Q

Giant covalent structures such as

A

graphite, diamond, sio2, graphene allotropes of carbon

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2
Q

structure and geometry of graphite

A

layered structure, geometrically planar. within planar layers, hexagonal C atoms.

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3
Q

C atoms in graphite

A

each C atom joined to adjacent 3 other by strong covalent bonds. sideways overlap of p orbitals, occupied by the 4th electron of each C atom in each planar layer form clouds of delocalised electrons above and below the plane of C rings and join up forming an extended delocalised rings of electrons.

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4
Q

colour and transparency of graphite

A

black-coloured, opaque

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5
Q

imf of graphite

A

layers of C atoms having weak van der waals’ forces

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6
Q

physical properties of graphite

A

high mp, high bp, soft, tender, slippery, good electrical conductor, insoluble in water

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7
Q

3 uses of graphite

A

pencils, lubricants, batteries

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8
Q

structure and geometry of diamond

A

C atoms arranged around each other regularly giving a crystalline structure and are geometrically tetrahedral

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9
Q

In diamond, each C atom bonded to

A

4 adjacent C atoms

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10
Q

colour and transparency of diamond

A

when pure, colourless and transparent

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11
Q

physical properties of diamond

A

high mp, high bp, the hardest natural substance on earth, good electrical insulator, insoluble in all solvents

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12
Q

3 uses of diamonds

A

gemstones, industrial abrasives, heat sinks

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13
Q

colour and transparency of sio2

A

they are colorless transparent crystals

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14
Q

physical properties of sio2

A

high mp, high bp, hard, good electrical insulator

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15
Q

3 uses of sio2

A

glass, ceramics, abrasives

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16
Q

shape of sio2

A

tetrahedral arrangement in which each Si atom bonded to 4 O atoms and each O atom bonded to 2 Si atoms

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17
Q

structure and geometry of graphene

A

it is a single isolated layer of graphite. hexagonally arranged sheet of C atoms

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18
Q

to what extent is the hardness of graphene

A

the hexagonally arranged sheet of C atoms is not completely rigid and can be distorted

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19
Q

reactivity of graphene

A

it is the most chemically reactive form of C

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20
Q

physical properties of graphene

A

high mp but burn at very low temperatures, good electrical and heat conductor (better than that of graphite)

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21
Q

3 uses of graphene

A

tiny transistors, touchscreens, solar cells

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22
Q

simple molecular structures such as

A

iodine and fullerene allotropes of C like C60 and nanotubes

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23
Q

distance between the nuclei of NEIGHBOURING iodine molecules … distance between the nuclei WITHIN the iodine molecule

A

>

24
Q

structure of iodine

A

regular packing of the molecules in a lattice structure

25
Q

physical properties of iodine

A

low mp, low bp, is a semiconductor in the plane of its crystalline layers and an insulator in the perpendicular direction

26
Q

disinfectants, printing inks, animal feed supplements, are 3 examples of uses of

A

iodine

27
Q

in fullerene allotropes of C, each C atom is bonded to

A

3 adjacent other C atoms

28
Q

other name of C60

A

buckminsterfullerene

29
Q

explain the shape of C60

A

football shaped. C atoms arranged at the corners of 20 hexagons and 12 pentagons.

30
Q

in C60, bond length between hexagons … between hexagons and pentagons

A

shorter than

31
Q

Although both have each C atom bonded to 3 adjacent other C atoms, the extent of delocalised electrons in C60 is … than in graphite

A

lesser

32
Q

physical properties of C60

A

low sublimation point, soft, poor electrical conductor, slightly soluble in solvents like carbon disulfide and methylbenzene

33
Q

explain the reactivity of C60

A

more reactive than graphite or diamond. because it has a high electron density in certain parts.

34
Q

antiviral treatment against HIV, cages for drug delivery in the body, are examples of uses of

A

C60

35
Q

structure or geometry of nanotubes

A

hexagonally arranged C atoms like a single layer of graphite bent into the form of a cylinder

36
Q

a simple molecular structure that is synthesized artificially

A

nanotubes

37
Q

physical properties of nanotubes

A

very high melting points, very high tensile strength, high electrical conductivity, and better thermal conductivity than diamond

38
Q

3 examples of uses of nanotubes

A

electrodes in paper-thin batteries, for added strength in clothing and sports equipment, used in the treatment of certain types of cancer

39
Q

ionic substances are hard, but they are also brittle. explain the brittle property of ionic substances.

A

ionic crystals are split apart when hit in the same direction as layers of ions. this is because layers of ions are displaced by the force of the blow, then ions with the same charge come together, and repulsions between thousand of ions in the layers, all with the same charge, cause the crystals to split along these cleavage planes.

40
Q

why is the metallic substance mercury a liquid at room temperature?

A

because some of the electrons in a mercury atom are bound MORE TIGHTLY than usual to the nucleus, WEAKENING the metallic bonds between atoms.

41
Q

explain the heat conductivity property of metallic substances

A

they are good conductors of heat. their conduction of heat is partly due to the movement of delocalized electrons and partly due to the vibrations passed on from one metal ion to the next.

42
Q

how do delocalised electrons move

A

they are free to move in a given direction, towards a positive charge or a more electronegative atom

43
Q

explain the high tensile strength and hardness of metallic substances

A

in a metallic bond, the attractive forces between metal ions and delocalized electrons act in all directions.

44
Q

explain the malleability and ductility of metallic substances

A

when layers slide, new metallic bonds reform easily between ions in new lattice positions and the delocalized electrons, which continue to hold ions in the lattice together.

45
Q

explain the density of ice compared to water

A

in ice, there is a more open arrangement due to long hydrogen bonds, allowing h2o molecules to be slightly further apart than in the liquid, resulting in the density of ice being less than that of water.

46
Q

structure of ice

A

three-dimensional hydrogen-bonded network of h2o molecules. a rigid lattice. each O atom surrounded by a tetrahedron of H atoms.

47
Q

Allotrope

A

different crystalline or molecular forms of the same element. e.g. graphite and diamond are allotropes of carbon.

48
Q

liquid state, vaporisation

A

the change in state when a liquid changes to vapour

49
Q

liquid state, vapour pressure

A

the pressure exerted by a vapour in equilibrium with a liquid

50
Q

explain the low sublimation point of C60

A

weak van der waals forces between each molecule and no continuous layered giant structure as in graphite

51
Q

explain the softness of C60

A

does not require much energy to overcome the weak imf van der waals

52
Q

explain high mps and bps in giant molecular lattices

A

a lot of energy needed to break strong covalent bonding between C atoms and separate the atoms throughout the structure

53
Q

explain the hardness in diamond

A

difficult to break the three-dimensional network of strong covalent bonds between C atoms

54
Q

explain the softness in graphite

A

it is easily scratched. the forces between layers of C atoms are weak. layers of graphite can slide over each other when a force is applied. the layers readily flake off.

55
Q

explain the hardness of ionic lattices

A

takes a lot of energy to scratch the surface because of the strong attractive forces keeping ions together.

56
Q

explain the high mp high bp of ionic lattices

A

the attraction between large numbers of oppositely charged ions in the lattice acts in all directions and bonds them strongly together.

57
Q

explain the trend in mp bp with ions

A

the mp bp increase with the charge density on the ions. e.g. Mg2+ O2- magnesium oxide has higher melting point than Na+Cl- sodium chloride. this is because there is a greater electrostatic attraction between doubly charged ions than singly charged ions of similar size.

chemistry 11b (10 decks)

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