topic 2🅱️ Flashcards

1
Q

coordination number

A

number of atoms or ions immediately surrounding a central atom in a complex or crystal

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2
Q

coordination number of ccp or fcc and hcp structures

A

12!!

3 above, 3 below, 6 on the same level

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3
Q

bcc coordination number

A

8
not closed packed
cubic geometry

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4
Q

primitive cubic structure coordination number

A

6
octahedral geometry.
the atom is part of a few unit cells

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5
Q

what’s an interstitial site

A

gaps between closed packed structures

atoms,, even when closely packed,, have gaps between them,, they aren’t packed with 100% efficacy

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6
Q

can interstitial sites be occupied by other atoms

A

yes!!!

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7
Q

most efficient way of packing

A

being closely packed
reduces the interstitial sites between them.

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8
Q

how can interstitial sites be categorised

A

categorised by their geometry

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9
Q

2 close packed type of interstitial site
HCP + CCP can have which interstitial sites

A
  • octahedral site
  • tetrahedral site
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10
Q

octahedral interstitial site

A

between 2 triangles above + below.
between 6 atoms

can see all the way through the structure

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11
Q

tetrahedral interstitial site

A
  • between a triangle above + a single atom below
    (can’t see all the way through the structure)

between 4 atoms

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12
Q

amount of octahedral sites in a close packed structure issss

A

‘N’
where N is the amount of atoms in host

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13
Q

number of tetrahedral interstitial sites in a close packed structure

A

2N

N is the number of atoms in a host

tetrahedral: between 4 atoms

double the amount of octahedral sites

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14
Q

how can we draw a unit cell diagram

A
  • space filling diagram
  • ball and stick diagram
  • cell projection diagram
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15
Q

what is a cell projection diagram

A

a 2D diagram of the unit cell,, viewed from above

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16
Q

what is lost when drawing a cell projection diagram

A

info on the Z axis!! aka how tall the unit cell is + where the diff atoms are placed on the z axis

17
Q

how can we show where the atoms are in a cell projection diagram

A

draw the atoms in diff environments :: code them with either 0,1 or 1/2 to show where they’re located

18
Q

when drawing a cell projection diagram,, what must we do

A

look at the diff atom environments
code each different environment
give them a number to show where they are on the Z axis

19
Q

are close packing structures 100% efficient

A

no!! they have interstitial sites aka gaps between atoms in a close packed structure

20
Q

how can we measure how efficient a close packed structure is in terms of packing

A

find the packing efficiency

21
Q

what is the packing efficiency

A

the percent of the structure that is filled by the atoms // ions

22
Q

packing efficiency equation

A

volume of atoms in a unit cell // total volume of the unit cell

x100

23
Q

what must we find to figure out the packing efficiency

A

we must know the volume of the atoms + the volume of the unit cell

24
Q

how do we figure out the total number of atoms in the unit cell

A
  • find how many atoms there are + if they’re on a vertices or a face
  • find their contribution eg: 1/ how many other unit cells they’re present in
  • contribution x total amount of them in ONE unit cell
25
how do we find the total volume of atoms in a unit cell
- u have the total amount of atoms - number of atoms x volume of one atom
26
what is the equation for the volume of one atom assuming it has hard sphere behaviour
V = 4/3 nr3 n = pi r = atomic radius
27
how do we find the total volume of the unit cell cell
length = 4 radii use Pythagoras to find a side (if it’s cubic : a=b=c) so volume is a3 pythag will give one a 🫶
28
what’s an intensive property
a bulk property they’re independent on the size of the system density is an example 🫶
29
equation for density
density = mass / volume
30
to find the density of the unit cell what to we need
the volume of the unit cell total number of atoms so we can find the total mass of unit cell.
31
what do we multiply the mass by to find the mass of the unit cell
not the total amount of atoms. but the total amount found by their contributions.
32
converting pm into cm
x 10-10
33
to convert amu to grams
amu / avogadros number
34
unit for density
g/cm3 or kg/m3
35
amu to grams
divide ➗ by avogadro
36
pm to m
x10 ^ -12
37
common density units
g/cm3 kg/m3
38
density of unit cell steps
density = mass // vol (mass in amu / avo) x number of atoms in unit cell vol = volume of unit cell grams and cm3 kg and m3 mass/volume