chemistry-class-11-unit-05-chapter-03-states-of-matter-gases-and-liquids-l-3-8-fcay8q-legi

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-3 </Success>
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- **Problem -** Which of the following molecule have a dipole - dipole interaction ?
- (a) $\mathrm{CO}_2$
- (b) $\mathrm{CH}_2 \mathrm{Cl}_2$
- (C) $\mathrm{CH}_4$

- **Ans** 
- Structure of the molecule
- Qualitative idea about the electronegative of elements
- Vectorial additon 
- Molecule that have a dipole - dipole interaction is 
- (b) $\mathrm{CH}_2 \mathrm{Cl}_2$

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<footer style = "font-size: 18px">Intermolecular forces $\rightarrow$ Intermolecular forces $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ Problem $\rightarrow$ Dipole - induced dipole interaction </footer>

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- **Problem -** predict the relative boiling point of $\mathrm{CH}_3 \mathrm{COOH}$ and $\mathrm{CH}_3 \mathrm{OH}$
- Boiling point of acetic acid is higher than methanol

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<footer style = "font-size: 18px">Intermolecular forces $\rightarrow$ Problem $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ Dipole - induced dipole interaction $\rightarrow$ Polarizability </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-3 </Success>
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- Water - life (fishes)

- ${O}_2$ and ${N}_2$ is dissolved in water

- $O=O$ is non polar and has no dipole

- $O=O \rightarrow$ induced dipole

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<footer style = "font-size: 18px">Problem $\rightarrow$ Problem $\rightarrow$ <span style = "color:blue"> Dipole - induced dipole interaction </span> $\rightarrow$ Polarizability $\rightarrow$ Polarizability </footer>

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- $\alpha$ measures the size of the induced dipole
- $\mu_{\text {ind }} = \alpha E$
- Larger the $\alpha $ , larger is the induced dipole

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|          | Polarizability/$10^{-25}cm^3$ |  Molar mass/amu | Boiling point/K |
| -------- | --------                      | --------        | --------        |
| $H_2$    | $7.9$                         | $2$               | $20k$         |
| $O_2$    | $16$                          | $32$              | $90k$         |
| $N_2$    | $17.6$                       | $28$              | $77k$         |
| $CH_4$   | $26$                          | $16$              | $109k$        |

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<footer style = "font-size: 18px">Problem $\rightarrow$ Dipole - induced dipole interaction $\rightarrow$ <span style = "color:blue"> Polarizability </span> $\rightarrow$ Polarizability $\rightarrow$ Polarizability and london dispersion force </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-3 </Success>
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- $CH_4-C_2H_6-C_3H_8-C_4H_{10}$
 - $\alpha$ increases 
 - Boiling point increases

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|           | Polarizability/$10^{-25}cm^3$ |  Molar mass/amu | Boiling point/K |
| --------  | --------                      | --------        | --------        |
| $C_2H_6$  | $44.7$                        | $30$            | $185k$          |
| $C_3H_6$  | $62.9$                        | $44$            | $231k$          |
| $CCl_4$   | $105$                         | $154$           | $350k$          |
| $Cl_2$    | $246$                         | $71$            | $238k$          |

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<footer style = "font-size: 18px">Dipole - induced dipole interaction $\rightarrow$ Polarizability $\rightarrow$ <span style = "color:blue"> Polarizability </span> $\rightarrow$ Polarizability and london dispersion force $\rightarrow$ Interaction in molecule </footer>

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- Fritz london
- $H_3C$ - $CH_2$-$CH_2$-$CH_3$
- n - Butane has higher boiling point
- Straight chain (larger the molecule) more polarizable - higher boiling point 
- Then , dipole - induced dipole interactions are higher

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<footer style = "font-size: 18px">Polarizability $\rightarrow$ Polarizability $\rightarrow$ <span style = "color:blue"> Polarizability and london dispersion force </span> $\rightarrow$ Interaction in molecule $\rightarrow$ Problem </footer>

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- Dipole - induced dipole
- Liquid $O_2$ 
 - $O=O$ no permanent dipole moment
- Electron density is symmetric at equilibrium 
- Instantaneous dipole - asymmetric electron density
- All molecules show dispersion forces

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<footer style = "font-size: 18px">Polarizability $\rightarrow$ Polarizability and london dispersion force $\rightarrow$ <span style = "color:blue"> Interaction in molecule </span> $\rightarrow$ Problem $\rightarrow$ London dispersion forces </footer>

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- **Problem** - The bp of propane , $\mathrm {n-}$ butane , $\mathrm {n-}$pentane , and $\mathrm {n-}$ hexane are respectively , $[-42.1^o\mathrm {c} , 0.5^o\mathrm {c},36.1^o\mathrm {c} \text { and } 68.7^o\mathrm {c}]$ explain this trend

|   Molecule     | $\text {Molecule mass}$ | $\text {BP}$ |
| --------          | --------            | --------     |
| $CH_3~ CH_2~ CH_3$| $44$                | $\downarrow$ |
| $n-C_4~ H_{10}$   | $58$                | $\downarrow$ |
| $n-C_5~ H_{12}$   | $72$                |   $\downarrow$  |
| $n-C_6~ H_{14}$   | $86$                |  $\downarrow$    |

- **Ans**

- London - dispersion forces 
- Dipole - induced dipole
- Induced dipole - induced dipole

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<footer style = "font-size: 18px">Polarizability and london dispersion force $\rightarrow$ Interaction in molecule $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ London dispersion forces $\rightarrow$ Interaction in molecules </footer>

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- **Problem -** Identify intermolecular interaction present in $\mathrm{CH}_3 \mathrm{CH}_3 , \mathrm{CH}_3 \mathrm{OH} , \mathrm{CH}_3 \mathrm{CH}_2 \mathrm{OH}$ 
- **What do we know -** Structure of the molecules functional groups (polar) , molar mass
- **Strategy -** Determine the type of interaction in each molecule follow the chart

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<footer style = "font-size: 18px">London dispersion forces $\rightarrow$ Interaction in molecules $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ Problem $\rightarrow$ Problem </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-3 </Success>
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- **Problem -** Rank the following in order of increasing strength of intermolecular forces in the pure substance
- (a) $\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{CH}_2 \mathrm{CH}_3$
- (b) $\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{OH}$
- (C) He 
- **Solution**
- **What do we know?** Structure , functional groups
- **Strategy ?** Flow chart \& know the relative sizes of various intermolecular interaction

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<footer style = "font-size: 18px">Interaction in molecules $\rightarrow$ Problem $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ Problem $\rightarrow$ Problem </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-3 </Success>
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- **Problem -** In each spare of ionic compounds. which is more likely to have the more negative enthalpy of, hydration ? Briefly explain your reasoning
- (a) $LiCl$ or $\mathrm{Cs} Cl$
- (b) $\mathrm{NaNO}_3 \hspace{1mm} or \hspace{1mm} \mathrm{Mg}\left(\mathrm{NO}_3\right)_2$
- (c) $\mathrm{RbCl} \hspace{1mm} or \hspace{1mm} \mathrm{NiCl_2}$

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<footer style = "font-size: 18px">Problem $\rightarrow$ Problem $\rightarrow$ <span style = "color:blue"> Problem </span> $\rightarrow$ Problem $\rightarrow$ Intermolecular Interaction </footer>