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inorganic sem 2 > lecture 8🅱️ > Flashcards

lecture 8🅱️ Flashcards

1
Q

trends in chemical properties can be understood using

A

lattice enthalpy

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2
Q

down the group of metal carbonates and enthalpy of decomposition

A

down group:
metal = cation ionic radius increases

larger enthalpy of decomposition (more endothermic)

more energy needed to decompose into metal oxide + co2

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3
Q

large anions stabilise what

A

large cations

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4
Q

lattice MO > lattice MO3

A

lattice enthalpy decreases

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5
Q

small cations stabilise

A

small anions

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6
Q

small metal,, small 02,, very stable,,, lattice of MO will be stable ,, larger MO lattice enthalpy bcccc

A

more energy needed to break bonds if its more stable

stability : look at size

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7
Q

dissolution equation

A

MX (s) –> M+ aq + X- aq

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8
Q

hydroation enthalpies are always negtative

A

going from +g -> +aq

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9
Q

solubility = lattice +

A

hydration enthalpy

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10
Q

what makes smt more soluble

A

if the solid contains ions of different size

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11
Q

small cation and small anion

A

very large lattice enthalpy!!

MG lattice is very positive,,, INSOLUBLE

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12
Q

large cation and small anion

A

large lattice MX
large anion hydration
small cation hydration

MX is soluble

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13
Q

large cation means

A

easily hydrated
small number for enthalpy of hydration

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14
Q

small anion

A

hard to hydrate
large number for enthalpy of hydration

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15
Q

small cation and large anion

A

cation: large hydration number
anion: small hydration number

soluble

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16
Q

large cation and large anion

A

cation: small number
anion: small number

MX lattice = very large

insoluble

17
Q

for smt to be soluble,, delta g must be negative

A

aka hydration enthalpies must be LARGE and NEGATIVE to overcome lactice enthalpy

lattice depends on sizes
hydration will always be negative but values depend on sizes.

SOL = LATTICE + HYD + HYD

18
Q

if the size matches,, theyre

A

insolube

19
Q

if the sizes dont match

A

theyre soluble

inorganic sem 2 (16 decks)

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