Transcript Slide 1

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A2 034
17-Jul-12
NaCl
Na+ (g) + e- + Cl (g)
H
H ionisation energy/ies
Na (g) + Cl (g)
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Na (s) + ½ Cl2 (g)
H lattice energy
of formation
H formation
NaCl (s)
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17-Jul-12
Na+ (g) + e- + Cl (g)
H
H ionisation energy/ies
Na (g) + Cl (g)
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Na (s) + ½ Cl2 (g)
H lattice energy
of formation
H formation
Ionic compound (s)
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Na+ (g) + e- + Cl (g)
H
H ionisation energy/ies
Na (g) + Cl (g)
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Elements (std states)
H lattice energy
of formation
H formation
Ionic compound (s)
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Na+ (g) + e- + Cl (g)
H
H ionisation energy/ies
Gas atoms (g)
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Elements (std states)
H lattice energy
of formation
H formation
Ionic compound (s)
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Metal ions, e-’s, non-metal atoms (g)
H
H ionisation energy/ies
Gas atoms (g)
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Elements (std states)
H lattice energy
of formation
H formation
Ionic compound (s)
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A2 034
17-Jul-12
Metal ions, e-’s, non-metal atoms (g)
H
H ionisation energy/ies
Gas atoms (g)
H electron affinity/ies
Gas ions (g)
H
atomisation(s)
Elements (std states)
H lattice energy
of formation
H formation
Ionic compound (s)
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A2 034
17-Jul-12
Metal ions, e-’s, non-metal atoms (g)
H
H ionisation energy/ies
Gas atoms (g)
H electron affinity/ies
Gas ions (g)
H
atomisation(s)
Elements (std states)
H lattice energy
of formation
H formation
Ionic compound (s)
Hformation = sum of all other H’s
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NaCl
Na+ (g) + e- + Cl (g)
H
494
H ionisation energy/ies
–364
Na (g) + Cl (g)
109
121
?
H electron affinity/ies
Na+ (g) + Cl- (g)
H
atomisation(s)
Na (s) + ½ Cl2 (g)
H lattice energy
–771
of formation
H formation
NaCl (s)
Hformation = 109 + 121 + 494 – 364 – 771 =
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–
411 kJmol-1
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MgCl2
Mg2+ (g) + 2 e- + 2 Cl (g)
H
736
1450
150
2(121)
–642
H ionisation energy/ies 2(–364) H electron affinity/ies
Mg (g) + 2 Cl (g)
Mg2+ (g) + 2 Cl- (g)
H
atomisation(s)
Mg (s) + Cl2 (g)
?
H lattice energy
of formation
H formation
MgCl2 (s)
= 150 + 2(121) + 736 + 1450 – 2(364) + Hlattice
Hlattice = – 642 – 150 – 2(121) – 736 – 1450 + 2 (364)
= – 2492 kJ mol-1
– 642
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KCl
K+ (g) + e- + Cl (g)
H
418
H ionisation energy/ies
–364 H
K+ (g) + Cl- (g)
K (g) + Cl (g)
90
121
?
electron affinity/ies
H
atomisation(s)
K (s) + ½ Cl2 (g)
– 710
H lattice energy
of formation
H formation
KCl (s)
Hformation = 90 + 121 + 418 – 364 – 710 = – 445 kJ mol-1
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CaBr2
Ca2+ (g) + 2 e- + 2 Br (g)
H
590
1150
193
2(112)
?
H ionisation energy/ies 2(–342) H electron affinity/ies
Ca (g) + 2 Br(g)
Ca2+ (g) + 2 Br- (g)
H
atomisation(s)
Ca (s) + Br2 (l)
–2125
H lattice energy
of formation
H formation
CaBr2 (s)
Hformation = 193 + 2(112) + 590 + 1150 – 2(342) – 2125
= – 652 kJ mol-1
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Al2O3
2 Al3+ (g) + 6 e- + 3 O (g)
H
2(577)
2(1820)
2(2740)
2(314)
3(248)
–1669
H ionisation energy/ies 3(–142) H electron affinity/ies
2 Al (g) + 3 O (g)
3(844)
2 Al3+ (g) + 2 O2- (g)
H
atomisation(s)
2 Al (s) + 3/2 O2 (g)
?
H lattice energy
of formation
H formation
Al2O3 (s)
–1669 = 2(314) + 3(248) + 2(577) + 2(1820) + 2(2740) + 3(-142) + 3(844) + H
H = –1669 – 2(314) – 3(248) – 2(577) – 2(1820) – 2(2740) + 3(142) – 3(844)
= – 15421 kJ mol-1
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CaO
Ca2+ (g) + 2 e- + O (g)
H
590
1150
193
248
–635
H ionisation energy/ies
Ca (g) + O (g)
–142 H
+844
electron affinity/ies
Ca2+ (g) + O2- (g)
H
atomisation(s)
Ca (s) + ½ O2 (g)
?
H lattice energy
of formation
H formation
CaO (s)
= 193 + 248 + 590 + 1150 – 142 + 844 + Hlattice
Hlattice = – 635 – 193 – 248 – 590 – 1150 + 142 – 844
= – 3518 kJ mol-1
– 635
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CaI2
Ca2+ (g) + 2 e- + 2 I (g)
H
590
1150
193
2(107)
–535
H ionisation energy/ies
Ca (g) + 2 I(g)
2X H
electron affinity/ies
Ca2+ (g) + 2 I- (g)
H
atomisation(s)
Ca (s) + I2 (s)
– 2054
H lattice energy
of formation
H formation
CaI2 (s)
= 193 + 2(107) + 590 + 1150 + 2X – 2054
2X = – 535 – 193 – 2(107) – 590 – 1150 – 2054
2X = - 628
X = – 314 kJ mol-1
– 535
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CuO
Cu2+ (g) + 2 e- + O (g)
H
745
1960
X
248
–155
H ionisation energy/ies
Cu (g) + O (g)
–142 H
+844
electron affinity/ies
Cu2+ (g) + O2- (g)
H
atomisation(s)
Cu (s) + ½ O2 (g)
– 4149
H lattice energy
of formation
H formation
CuO (s)
= X + 248 + 745 + 1960 – 142 + 844 – 4149
X = – 155 – 248 – 745 – 1960 + 142 – 844 + 4149
= + 339 kJ mol-1
– 155
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CoCl
Co+ (g) + e- + Cl (g)
H
757
H ionisation energy/ies
–364 H
Co (g) + Cl(g)
427
121
?
electron affinity/ies
Co+ (g) + Cl- (g)
H
atomisation(s)
Co (s) + ½ Cl2 (g)
–700
H lattice energy
of formation
H formation
CoCl (s)
Hformation = 427 + 121 + 757 – 364 – 700
= + 241 kJ mol-1
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CoCl2
Co2+ (g) + 2 e- + 2 Cl (g)
H
757
1640
427
2(121)
?
H ionisation energy/ies 2(–364) H electron affinity/ies
Co (g) + 2 Cl(g)
Co2+ (g) + 2 Cl- (g)
H
atomisation(s)
Co (s) + Cl2 (g)
–2624
H lattice energy
of formation
H formation
CoCl2 (s)
Hformation = 427 + 2(121) + 757 + 1640 – 2(364) – 2624
= – 286 kJ mol-1
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CoCl3
Co3+ (g) + 3 e- + 2 Cl (g)
H
757
1640
3230
427
3(121)
?
H ionisation energy/ies 3(–364) H electron affinity/ies
Co (g) + 3 Cl(g)
Co3+ (g) + 3 Cl- (g)
H
atomisation(s)
Co (s) + 3/
2
Cl2 (g)
–5350
H lattice energy
of formation
H formation
CoCl3 (s)
Hformation = 427 + 3(121) + 757 + 1640 + 3230 – 3(364) – 5350
= – 25 kJ mol-1
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A2 034
17-Jul-12