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inorganic sem 2 > topic 1🅱️ > Flashcards

topic 1🅱️ Flashcards

1
Q

solid

A

state of matter
particles are arranged in a way that makes their shape + volume stable

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2
Q

what is solid state chem

A

it’s about making/ preparing solids
structure of solids
properties of solids

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3
Q

ionic bonding

A

regular arrays of positively and negatively charged ions

electrostatic forces of interaction

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4
Q

covalent bonding

A

atoms in the compound share electrons in order to obtain an octet figuration.

lewis model + MO bonding theory

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5
Q

why do we use the terms ionic and covalent character

A

bc bonding is a spectrum.

it’s never either the 2 extremes but a combo of both

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6
Q

types of solid: molecular solid

A
  • solid made up of molecules
  • bonds are covalent (strong)
  • intermolecular bonds are weaker (H, DD, VDW
  • soft materials
  • low melting points (only the intermolecular need to be broken to change state)
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7
Q

in molecular solids,, what interaction needs to be broken in order for them to change state

A

intermolecular interaction!!!
HYDROGEN, DIPOLE DIPOLE,, VDW

the covalent bonding (intra) doesn’t need to be broken

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8
Q

types of molecular solids

A

Iodine
I2 = covalently bonded

I2 —- I2 (van der waals interactions)

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9
Q

describe iodine solid

A

covalent between I and I
VDW between I2
VDW = strong enough for iodine to be solid at room temp. (lots of e-)
- solid sublimes easily into vapour
- low 113.7* melting point

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10
Q

sublimation // sublimes meaning

A

going from solid to gas // vapour
doesn’t go through the liquid phase // state

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11
Q

another example for a molecular solid

A

sulfur

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12
Q

describe sulfur

A
  • solid in ambient conditions
  • contains S8 ring molecules
  • covalent S and S
  • VDW // dispersion between S8
  • soft, bright, yellow at room temp
  • low mp of 115.2*
  • sublimes easily
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13
Q

what are covalent network solids

A
  • covalently bonded atoms that form a continuous infinite network
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14
Q

what can form covalent network solids

A

elements (C)
compounds (SiO2)

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15
Q

describe covalent network solids

A

high melting + boiling points
hard
brittle (covalent bonds must be broken to change state)

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16
Q

examples of covalent network solids

A

graphite
diamond
quartz
a-crietobalite

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17
Q

further examples of covalent network solids

A

carbon!!
it has many allotropes

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18
Q

what’s an allotrope

A

different solid stage structures of the same element

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19
Q

describe C,, CNS : graphite

A
  • layers of sp2 hybrid C
  • high mp (covalent within layers)
  • pencils + lubricants (VDW between layers - slips)
  • conductive ( delocalised e- between layers)
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20
Q

CNS: C : diamond

A
  • sp3 hybrids (single bonds)
  • 4 covalent bonds each (hard solid + high mp)
  • no delocalised e- : not conductive
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21
Q

CNS: C : graphene

A

single sheet of graphite
similar properties to graphite (high mp, conductive )
very strong
very light

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22
Q

CNS : C : fullerenes

A

nanotubes
rolled sheet of graphite
strong, light, conductive

buckyballs: lower mp ( VDW between spheres)

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23
Q

difference between fullerenes and graphene

A

graphene is a flat sheet of graphite
fullerene is a rolled sheet of graphite

fullerenes can also include nanotubes or buckyballs

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24
Q

CNS: SiO2 (silicone dioxide)

A
  • covalent bonds between Si and O
  • many diff know structures (polymorphs)
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25
Q

what is a polymorph

A

different solid stage structures of the same compound

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26
Q

what are the 2 polymorphs of SiO2

A

quartz
a-cristobalite

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27
Q

describe quartz : CNS (SiO2)

A

most common polymorph
natural mineral
most common mineral on the earth

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28
Q

describe a-cristobalite : CNS: SiO2

A

common polymorph of SiO2
also has its own polymorphs at high and low temperatures

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29
Q

describe a metallic solid

A
  • cations in a sea of delocalised electrons
  • interactions between cations and e- = strong metallic bonding
  • hard solids + mp + bp due to strong metallic bonding
  • only valence e- contribute to the bonding + are delocalised
  • conductive in solid + molten form
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30
Q

ionic solid type of solid

A
  • cations and anions
  • electrostatic forces between oppositely charged ions holds them together
  • high melting + bp
  • hard and brittle (strong ionic bonds)
  • conductive when molten or dissolved in aq solution
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31
Q

what elements are more likely to form ionic compounds

A

those that are more easily ionised
more readily ionised

aka lower ionisation energies.

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32
Q

example of an ionic solid

A

NaCl
sodium chloride
Na+ and Cl-

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33
Q

what is a crystal

A

a crystalline solid

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34
Q

what is a crystal or a crystalline solid

A

solid consisting of a regular and repeating array of atoms, molecules, ions.

extend in 3 dimensions to give an ordered structure

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35
Q

what type of symmetry does a crystal have

A

translational symmetry

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36
Q

what is translational symmetry

A

a movement, shift or slide in a specific direction by a specific distance without rotation or reflection

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37
Q

what is a unit cell in a crystal

A

the smallest repeating unit of a crystal

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38
Q

how many parameters is a unit cell described with

A

6

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39
Q

what 6 parameters are used to describe a unit cell

A

3 vector lengths : a b c
3 angles : a B y

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40
Q

what the relationship between the crystal parameters in a cubic unit cell

A

a = b = c
a = B = y = 90*

41
Q

how is a full crystal structure generated

A

when the unit cell is translated in 3 directions

when translational symmetry occurs me

42
Q

what are the 4 other basic crystal symmetry

A
  • mirror symmetry
  • inversion symmetry
  • rotational symmetry
  • rotary inversion symmetry
43
Q

combo of what allows us to build up an entire crystal structure

A

combo of all the symmetries
- mirror
- rotation
- translation
- inversion
- rotary inversion

44
Q

1 fold in rotational symmetry

A

360*

45
Q

2 fold in rotational symmetry

A

180

46
Q

4 fold in rotatory symmetry

A

90

47
Q

how can we determine the crystal structure // the structure of crystalline solids

A

analytical technique
- x ray crystallography

48
Q

how does the analytical technique of x ray crystallography determine the solid structure of crystalline solids

A
  • x ray beam is shone on crystal
  • diffraction occurs as x ray beam wavelength is similar to the order of gaps between atoms
  • detector is used to identify the diffraction pattern which is mathematically related to the structure of a crystal
49
Q

close packing + atoms :: what will always be present

A

small gaps will always be present no matter how tightly u pack the atoms together

50
Q

what is the most efficient way for atoms to pack together to minimise the amount of space between them

A

close packing
it minimises the amount of space between them

51
Q

close packing : A

A

looks like a bunch of flower heads

each atom is in contact with 6 atom neighbours

one close packed layer

52
Q

close packing AB

A

spheres in layer 2 sit between the first layers gaps

2 close packed layers

53
Q

3 close packed sphere layers

A

2 options:
- ABA : spheres in 3 sits directly above layer 1 ( hexagonal close packing) flower up front,, gaps go all the way through

  • ABC : spheres in layer 3 sit directly above layer one gaps (cubic close packing) (no spheres are directly above each other,, all layers are different,, no straight through gaps)
54
Q

what repeats does cubic close packing (ccp) aka the triangle top shape have

A

ABCABCABCABCABCABCABC

cubic for c!! each layer is different,, no atoms are directly above other atoms,, no straight through gaps.

55
Q

what repeat does hexagonal close packing have (aka the flower on top)

A

ABABABABABABABABABAB

56
Q

most common close packing arrangements

A

CCP

HCP

57
Q

in how many directions must a unit cell be translated in order to general the full crystal structure

A

must be translated into three directions

58
Q

what is the ‘cubic’ is ccp referring to

A

the cubic symmetry of its structure
- a=b= c
- a = B = y = 90*

59
Q

how else can the ccp unit cell be called

A

face centred cubic (fcc)

60
Q

what are other important cubic cell units called

A

body centred cubic (bcc)
primitive cubic (pc)

61
Q

are bcc or pc close packed

A

nope!!
neither of them are close packed

62
Q

what is face centred cubic (fcc)

A

atoms are on all cube vertices and in the centre of the faces

63
Q

what is body centred cubic (bcc)

A

atoms are on all vertices of the cube
1 atom in the centre of the cube

64
Q

what is primitive cubic

A

atoms are seen on all vertices of the cube only

65
Q

what does the hexagonal in hcp stand for

A

the hexagonal symmetry of the structure

66
Q

what conditions are seen in the unit cell or a hexagonal structure

A
  • vectors: a=b NOT c
  • angles: y=120
67
Q

what elements can adopt the CCP HCP BCC

A

metallic elements!!
phase transitions can occur between different structures under ambient temp and pressure

68
Q

what structure does metallic Cu^0 adopt

A

CCP
FCC

69
Q

what structure does metallic Ti ^0 adopt

A

hcp

70
Q

what structure does metallic Iron m,, Fe^0 adopt

A

bcc

71
Q

make it known!! ccp is

A

cubic close packing
also known as face centred cubic

72
Q

ccp is

A

cubic close packing

73
Q

ccp can also be called

A

fcc

74
Q

what is fcc

A

face centred cubic

also known as cubic close packing

75
Q

what is hexagonal close packing

A

ABABABAB

76
Q

ccp is called,,, and how many different ones are there

A

cubic close packing
also known as face centred cubic

  • body centred cubic
  • primitive cubic
77
Q

which structures are closely packed

A

cubic close packing ABC
(face centred cubic)

hexagonal close packing ABAB

78
Q

which structures arent closely packed

A

body centred cubic
primitive cubic

79
Q

which holes can u see all the way through

A

hexagonal closed packing
ababababa

H exagonal for Holes
3 above and 3 below

80
Q

which holes can u not see all the way through

A

cubic close packing

3 above
1 below

C ubic for ABC

81
Q

coordination number of an atom in hcp

A

12

3 above
6
3 above

82
Q

coordination number of atoms in a ccp

A

12

3 above
6
3 above

83
Q

bcc coordination number

A

8

84
Q

primitive coordination number

A

6

85
Q

primitive cubic can also be called what

A

simple cubic

atoms on corners only

86
Q

what is packing efficacy

A

percentage of the structure that is filled by atoms

87
Q

for a bcc: packing efficacy

A

u need to put a bit more effort in.

first find x by doing
L2 + L2 = X2

then do X2 + L2 = 4r2

then do the whole atom volume thing

and do L3 to find the volume

88
Q

number of atoms in ccp

A

4

89
Q

number of atoms in hcp

A

2

90
Q

number of atoms in bcc

A

2

91
Q

number of atoms in primitive cubic // simple cubic

A

1

92
Q

packing effficacy of hcp and ccp

A

74%

93
Q

packing efficacy of bcc

A

68%

94
Q

packing efficacy of primitive

A

52.4%

95
Q

close packed structures intersitital sites

A

tetrahedral
octahedral

96
Q

how many octahedral sites per atom

A

1

site is bonded to 6 atoms

3 below
3 above

can see through

97
Q

how many tetrahdral sites per atom

A

2

site is bonded to 4 atoms

3 above
1 below

cant see through

98
Q

length of ccp/fcc

A

8 1/2 r

cube this to get volume

99
Q
A

inorganic sem 2 (16 decks)

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