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Chemistry > Lattice Energy > Flashcards

Lattice Energy Flashcards

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1
Q

definition of lattice energy

A

enthalpy change when one mole of ionic compound is formed from its gaseous ions under standard conditions

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2
Q

enthalpy change of lattice energy

A

exothermic

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3
Q

Na+(g) + Cl-(g) → NaCl (s) is an example of

A

lattice energy

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4
Q

what does large exothermic value for lattice energy mean

A

more stable and strong ionic bonding

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5
Q

suggest reason for difference in LE between calcium oxide and iron (II) oxide

A

iron has smaller ionic radius = high charge density

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6
Q

key words for mentioning lattice energy difference (4)

A

ionic radius
charge density
electrostatic attraction between cation and anion
charge on ion

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7
Q

definition of enthalpy change of atomisation

A

enthalpy change when one mole of gaseous atoms are formed from its element under standard conditions

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8
Q

enthalpy change of atomisation

A

endothermic

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9
Q

why is enthalpy change of atomisation endothermic

A

energy must be supplied to break the bonds holding atom together

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10
Q

Li(s) –> Li(g) is an example of

A

enthalpy change of atomisation

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11
Q

definition of enthalpy change of hydration

A

the enthalpy change when one mole of gaseous ions dissolves in sufficient water to form an infinitely dilute solution

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12
Q

enthalpy change of hydration

A

exothermic

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13
Q

trends in enthalpy change of hydration

A

more exothermic with smaller ions

high charge density makes stronger bonds with water molecule

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14
Q

definition of enthalpy change of solution

A

the energy absorbed or released when one mole of an ionic solid dissolves in sufficient amount of water to form an infinitely dilute solution

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15
Q

enthalpy change of solution (aq)

A

exo/endo (little changes)

large values are insoluble

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16
Q

definition of first ionisation energy

A

enthalpy change when one electron is removed from each atom in one mole of gaseous atoms under standard conditions

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17
Q

enthalpy change of first ionisation energy

A

endothermic

18
Q

why is first ionisation eneergy endothermic

A

energy needed to overcome the force of attraction between outer electrons and nucleus

19
Q

why is first ionisation energy of calcium less positive than its second ionisation energy

A

electron lost is closer to the nucleus
electron lost from positive ion
outer electron more firmly attracted to the nucleus

20
Q

definition of first electron affinity

A

enthalpy change when one mole of electrons is added to one mole of gaseous atoms to form one mole of gaseous 1- ions under standard conditions

21
Q

enthalpy change of first electron affinity

A

exothermic

22
Q

why is first electron affinity exothermic

A

electron experience attraction to the nucleus, energy absorbed to overcome repulsion

23
Q

Cl(g) + e → Cl- (g) is an example of

A

first electron affinity

24
Q

definition of second electron affinity

A

enthalpy change when one mole of electrons is added to one mole of gaseous 1- ions to form one mole of gaseous 2- ions under standard conditions

25
Q

enthalpy change of second electron affinity

A

endothermic

26
Q

why is second electron affinity endothermic

A

ion and electron both negative + energy required to overcome repulsion

27
Q

O- (g) + e → O2-(g) is an example of

A

second electron affinity

28
Q

factors affecting electron affinity

A

nuclear charge
distance
shielding from electrons
(shielding + distance offsets)

29
Q

what does low electron affinity mean

A

more wanting to give up its electron and has weak pull on valence of electrons

30
Q

trend of electron affinity with halogens

A

becomes less negative (further away from outer shell = less energy released)

31
Q

why is fluorine a less exothermic value than chlorine

A

very small and pushing in electron require some energy - crowded speace = less energy released

32
Q

look at born haber cycle ok

A

ok

33
Q

definition of enthalpy change of formation

A

enthalpy change when ionic compound formed from its elements under standard conditions

34
Q

enthalpy change of what (2) in born haber cycle

A

formation

lattice

35
Q

factors affecting lattice energy

A

ion size

charge on ions

36
Q

definition of polarising power

A

ability of cation to attract e and distort an anion

37
Q

describe ion polarisaion

A

small cation has high charge density and able to distort large anion

38
Q

describe trend of thermal stability of group 2 carbonates/nitrates

A

increasing stability
increasing ionic size = low charge density
polarising ability on nitrate decreases

39
Q

trend of solubility of sulphates

A

less soluble down the group
lattice energy and hydration energy both decrease
hydration decreases more
enthalpy of solution more endothermic

40
Q

equation for E.sol

A

E.latt - E.hyd

41
Q

trend of solubility of hydroxides

A

more soluble
lattice and hydration energy both decrease
lattice energy decreases more
enthalpy change of solution less endothermic

Chemistry (15 decks)

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