States Of Matter Gases And Liquids L-2 States of matter
→ \rightarrow → → \rightarrow → States of matter → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Matter
State of matter
Intermolecular forces (Ion - ion interaction)
Ion - ion interaction -
NaCl V ∝ 1 r \quad V \propto \frac{1}{r} V ∝ r 1
→ \rightarrow → → \rightarrow → Matter → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Ion- dipole interaction
States of matter → \rightarrow → → \rightarrow → Ion- dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Ion- dipole interaction
O − H → O-H {\rightarrow} O − H →
Matter → \rightarrow → → \rightarrow → Ion- dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Ion - dipole interaction
V i d V_{id} V i d ∝ \propto ∝ 1 r 2 \frac{1}{r^2} r 2 1 V e s ( i − i ) V_{es(i-i)} V es ( i − i ) ∝ \propto ∝ 1 r \frac{1}{r} r 1 V i d = k r 2 V i i = k r V_{id}= \frac{k}{r^2} \quad V_{ii}=\frac{k}{r} V i d = r 2 k V ii = r k
Ion- dipole interaction → \rightarrow → → \rightarrow → Ion - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Ion - dipole interaction
1 r n → \frac{1}{r^n} \rightarrow r n 1 → n n n
1 r → \frac{1}{r} \rightarrow r 1 →
1 r n → \frac{1}{r^n} \rightarrow r n 1 →
NaCl/LiF → H 2 O \rightarrow H_2O → H 2 O
Ion- dipole interaction → \rightarrow → → \rightarrow → Ion - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Hydration enthalpy
Hydration enthalpy of a series of ions M n + ( g ) + H 2 O → M n + ( a q ) M^{n+}(g)+H_2O \rightarrow M^{n+}(aq) M n + ( g ) + H 2 O → M n + ( a q )
Ion \text{ Ion } Ion Ionic radius/pm \text{Ionic radius/pm } Ionic radius/pm Δ H 0 hydr / k J m o l − \Delta \mathrm{H^0} \text {hydr}/kJ ~ mol^- Δ H 0 hydr / k J m o l −
L i + Li^+ L i + 76
-538
N a + Na^+ N a + 102
-424
K + K^+ K + 138
-340
M g 2 + Mg^{2+} M g 2 + 72
-1963
A l 3 + Al^{3+} A l 3 + 54
-4741
Ion - dipole interaction → \rightarrow → → \rightarrow → Hydration enthalpy → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Problem
In which mixture do you expect higher ion-dipole forces between solute & solvent
C H 3 O H CH_3OH C H 3 O H C a ( N O 3 ) 2 Ca(NO_3)_2 C a ( N O 3 ) 2
Ion - dipole interaction → \rightarrow → → \rightarrow → Problem → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Intermolecular forces
Ion - ion
Ion - dipole
Dipole - dipole
Dipole - induced dipole
Induced - induced dipole
Hydration enthalpy → \rightarrow → → \rightarrow → Intermolecular forces → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Dipole - dipole interaction
Molecule
Molecular mass
Boiling point
N 2 N_2 N 2 28
77K
O 2 O_2 O 2 32
90K
N O NO NO 30
121K
Problem → \rightarrow → → \rightarrow → Dipole - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Dipole - dipole interaction
N ≡ N N \equiv N N ≡ N O = O O=O O = O N − O → \overrightarrow{N-O} N − O Electron negativity difference
Higher boiling point of NO over N 2 N_2 N 2 O 2 O_2 O 2
V = μ 1 μ 2 K r 3 V = \frac{\mu_1\mu_2}{Kr^3} V = K r 3 μ 1 μ 2
Intermolecular forces → \rightarrow → → \rightarrow → Dipole - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Dipole - dipole interaction
V d d V_{dd} V dd ∝ \propto ∝ 1 r 6 \frac{1}{r^6} r 6 1 V i i V_{ii} V ii ∝ \propto ∝ 1 r \frac{1}{r} r 1 V i d V_{id} V i d ∝ \propto ∝ 1 r 2 \frac{1}{r^2} r 2 1 V d d V_{dd} V dd ∝ \propto ∝ 1 r 6 \frac{1}{r^6} r 6 1
Dipole - dipole interaction → \rightarrow → → \rightarrow → Dipole - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Dipole - dipole interaction
HCl in water
C H 3 C l \mathrm {CH_3Cl} C H 3 Cl C H 2 C l 2 \mathrm {CH_2Cl_2} C H 2 C l 2 C H C l 3 \mathrm {CHCl_3} CHC l 3
Dipole - dipole interaction → \rightarrow → → \rightarrow → Dipole - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Dipole - dipole interaction
− v e [ 1 r , 1 r 2 , 1 r 6 ] → attractive -\mathrm {ve} \left[\frac{1}{r},\frac{1}{r^2}, \frac{1}{r^6}\right] {\rightarrow} \text { attractive } − ve [ r 1 , r 2 1 , r 6 1 ] → attractive + v e ← 1 r 12 → repulsive + \mathrm {ve } \leftarrow \frac{1}{r^{12}}\rightarrow \text { repulsive } + ve ← r 12 1 → repulsive
Dipole - dipole interaction → \rightarrow → → \rightarrow → Dipole - dipole interaction → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Boiling point of hydrides
Molecule
Molecular mass/amu
Boiling point/o C ^oC o C
C H 4 \mathrm {CH_4} C H 4 16 16 16 − 161.5 -161.5 − 161.5
S i H 4 \mathrm{SiH_4} Si H 4 32 32 32 − 111.9 -111.9 − 111.9
S n H 4 \mathrm{SnH_4} Sn H 4 122 122 122 − 51.9 -51.9 − 51.9
P b H 4 \mathrm{PbH_4} Pb H 4 211 211 211 − 13 -13 − 13
Dipole - dipole interaction → \rightarrow → → \rightarrow → Boiling point of hydrides → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Boiling point of hydrides
Molecule
Molecular mass/amu
Boiling point/o C ^oC o C
N H 3 \mathrm {NH_3} N H 3 17 17 17 − 33.33 -33.33 − 33.33
P H 3 \mathrm {PH_3} P H 3 34 34 34 − 87.75 -87.75 − 87.75
A s H 3 \mathrm {AsH_3} As H 3 78 78 78 − 62.5 -62.5 − 62.5
S b H 3 \mathrm {SbH_3} Sb H 3 125 125 125 − 17.0 -17.0 − 17.0
H 2 O \mathrm {H_2O} H 2 O 18 18 18 ∼ 100 \sim 100 ∼ 100
H 2 S \mathrm {H_2S} H 2 S 34 34 34 − 60 -60 − 60
H 2 S e \mathrm {H_2Se} H 2 Se 81 81 81 − 41 -41 − 41
H 2 T e \mathrm {H_2Te} H 2 Te 130 130 130 − 2 -2 − 2
Dipole - dipole interaction → \rightarrow → → \rightarrow → Boiling point of hydrides → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Boiling point due to hydrogen bonding
Boiling point of hydrides → \rightarrow → → \rightarrow → Boiling point due to hydrogen bonding → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Problem bassed on boiling point
Boiling point of hydrides → \rightarrow → → \rightarrow → Problem bassed on boiling point → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Kevlar
Boiling point due to hydrogen bonding → \rightarrow → → \rightarrow → Kevlar → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Intermolecular forces
Ion - ion interaction
Hydrogen bond
Ion - dipole interaction
Dipole - dipole interaction
Dipole - induced dipole
Induced - induced dipole
Problem bassed on boiling point → \rightarrow → → \rightarrow → Intermolecular forces → \rightarrow → → \rightarrow →
States Of Matter Gases And Liquids L-2 Thank you
Kevlar → \rightarrow → → \rightarrow → Thank you → \rightarrow → → \rightarrow →
Resume presentation
States Of Matter Gases And Liquids L-2 States of matter $\rightarrow$ $\rightarrow$ States of matter $\rightarrow$ Matter $\rightarrow$ Ion- dipole interaction
