lecture 7🅱️ Flashcards

1
Q

enthalpy change

A

the amount of heat evolved or absorbed for a reaction

under constant pressure

H

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2
Q

standard enthalpy change refers to what

A

enthalpy change when all reactants are in standard states and done in standard conditions

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3
Q

standard temp

A

25*C

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4
Q

standard pressure

A

1 bar

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5
Q

standard conc

A

1 mol dm-3

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6
Q

enthalpy change of formation

A

enthalpy change for a reation where 1 mol of product is formed from its reactants in their standard states

at standard conditions

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7
Q

enthalpy of atomisation

A

enthalpy change that occurs from going from a solid to a gas

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8
Q

ionisationenthalpy

A

enthalpy needed to remove electron from element

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9
Q

electron affinity

A

enthalpy change when an electron is added to an element

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10
Q

bond dissociation enthalpy

A

enthalpy change when bonds dissociate

eg: Cl2g -> 2Cl g

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11
Q

bde value can also be

A

2 x atomisation enthalpy

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12
Q

lattice enthalpy

A

enthalpy change when 1 ol of solid is converted to one mol of gas ions

endothermic (needs energy) to overcome strong electrostatic forces of attraction

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13
Q
  • lattice enthalpy issss
A

exothermicccc

refers to the enthalpy of 1 mol of gaseous ions forming 1 mol of solid

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14
Q

lattice enthalpy +

A

solid to gas

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15
Q

lattice enthalpy -

A

gas to solid

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16
Q

hess cycle steps for NaCl

A
  • write equation: Na(s) + 1/2Cl2g -> NaCl(s)
  • atomisation from S -> G
  • bde for Cl2 -> 2Cl
  • ionise Na
  • electron affinity for Cl
  • gas to solid ( lattice enthalpy - )
17
Q

hess law definition

A

total enthalpy change is independednt of route taken

total enthalpy is the sum of the enthalpy for individual steps

if the states remain the same for pro and rea

18
Q

born haber cycle can be written in 2 ways — its a diagram of individual step reactions

A

hess law cycle : the new thing

enthalpy level diagram: alevel one

19
Q

bde is going from a diatomic to 2 monatomics so what do we need to do to the dbe value if we only need 1 monatomic (eg: Cl in NaCl)

A

u need to divide the dbe by 2

or multiply bde by 1/2

20
Q

experimental lattice enthalpy

A

use hess cycle or haber born cycle

21
Q

delta H formation =

A

atom + bde + ie + ea - lattice

22
Q

lattice =

A

atom + bde + ie + ea - formatioon

23
Q

lattice is normally

A

solid to gassss
endothermic

24
Q

solid to gas

A

endothermic
+ lattice enthalpy

25
gas to solid
exothermic - lattice enthalpy
26
experimental lattice enthalpies
born harber cycle hess cycle
27
theoretical lattice enthalpy
use of ionic model - ions = hard sphere character - defined ionic radius - ions are sep by internuclear distance 'r' - consider total electrostatic attractions to find lattice energy - difference in potential energy between free ions and ions bound together in solid.
28
madelung constant
accounts for repulsive and attractive forces between ions in a solid, A depends on structure type
29
if we use madelung constant we also need
avo constant 6.022 x 10^23
30
what else is wrong
ions arent point charges,, their ion charge can overlap we use born exponent , n. to account for this.
31
n for 2 elements of the same exponent group
n = just that singular number
32
n for 2 elements from different exponent groups
add both then divide by 2 basically just get an average of the 2.
33
born lande equation
gives theoretical lattice enthalpy
34
z+. z-
multiply the ion charges
35
what is r
interionic distance distance from nuc to nuc radius + radius
36
difference between theoretical (BL) and experimental (HB HC)
BL is based on ionic model,, this is flawed. - no compound is 100% ionic - e- cloud can be polarised if large and negative (low charge) - small and high charge ion (+ ions) can polarise the e- cloud. - this gives higher covalent character
37
what can born lande be used for
assessing how ionic a compound is if theoretical ( BL) and experimental (HB HC) are similar = ionic character big difference = some covalent character present.. describe this quantitatively!! find the %difference.
38
born mayer equation
better born lande one takes ion ion repulsions into account p is constant but in pm,, so interionic distance must also be converted into pm
39
kapustinskii equation
no knowledge of crystal structure needed,, A or r lattice energy in kj mol-1 must be in pm