constructing born haber cycles Flashcards

1
Q

2 factors that effect strength of ionic bonding

A

size of ions and charge of ions

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2
Q

when does ionic bond strength increase

A

when ions smaller and have higher charges

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3
Q

what happens if ionic bonding is stronger

A

the lattice enthalpy is more exothermic

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4
Q

lattice enthalpy definition

A

enthalpy change when one mole of an ionic solid is formed from its constituent ions in the gas state

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5
Q

first step of alternative route for lattice enthalpies hess cycle

A

separation
-negative of enthalpy formation

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6
Q

second stage in hess law alternative route to

A

atomisation
-element in its standard state
-1/2cl2 —>CL

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7
Q

enthalpy change of separation

A

enthalpy change when one mole of an ionic compound is separated into its constituent ions in their gas phase

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8
Q

when can you link enthalpy of atomisation and bond dissociation

A

when elements in standard states are gaseous
-when they are covalently bonded

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9
Q

third step in alternative route in lattice enthalpies

A

electron affinity calculated using ionisation energies

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10
Q

fourth and last step of alternative route lattice enthalpies

A

adding electrons
electron affinities

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11
Q

is lattice enthalpy exo or endo

A

exothermic

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12
Q

equation for calculating lattice enthalpy

A

formation= everything else added together
then rearrange for lattice enthalpy

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13
Q

equation when lattice dissociation is used

A

formation+ lattice dissociation = everything else

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14
Q

perfect ionic model

A

all ions perfectly spherical and all bonding ionic

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15
Q

what does theoretical values not account for

A

covalent character in bonding

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16
Q

what suggest if something has larger covalent character or not

A

the difference between theoretical and experimental values

17
Q

what happens to anion as it bonds with cation

A

its electron cloud distorts and it becomes polarised by the cation

18
Q

what makes ion more polarising

A

small and higher charge

19
Q

which ions have highest polarising power

A

small
high charge
have positive charge

20
Q

polarisability

A

larger and more highly charges ions

21
Q

factors that affect polarisation

A

polarising power of cation
polarisability of anion

22
Q

whats an exception exam question to polarization rules

A

silver halides

23
Q

example of comparing bonding

A

NaCl has larger difference in theoretical and experimental lattice enthalpies
-NaCl has a larger amount og covalent character
-NaCl has larger amount of polarisation
-since anions comparing both Na- this mean Ag+ must have higher polarising power than Na+

24
Q

how to answer silver halides question on polarization

A

AgBr has a larger difference in the theoretical and experimental lattice enthalpies
-AgBr has a larger amount of covalent character

25
what are hydrated ions held together by
ion dipole forces
26
enthalpy of solution
when one mole of a solute in its standard state dissolves in water to form aqueous ions
27
enthalpy of hydration
when one mole of gaseous ions are converted to aqueous ions
28
factors that determine strength between ions and polar water molecules
magnitude of ions charge and size of ion
29