chemistry-class-11-unit-05-chapter-01-states-of-matter-gases-and-liquids-l-1-8-fugr2b7nghu

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-1 </Success>
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- **Exception to this characterization**
  - Glass - appearance of a  solid (super cooled liquid)
- **Principal characteristics**
  - Compressibility

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<footer style = "font-size: 18px">States of matter $\rightarrow$ States of matter $\rightarrow$ <span style = "color:blue"> States of matter </span> $\rightarrow$ States of matter $\rightarrow$ States of matter </footer>

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- **Principal characteristics**
- **Rigidity**
  - Constant volume
  - Changes the shape
- **Viscosity**
  - Measure of resistance that a system has to change of shape taking place at finite speeds

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- **Molecules are structureless circle**
- Solid
  - Fixed positions
  - Small empty space
  - Molecules vibrate about fixed positions

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- **Liquid**
  - Random position
  - Small empty space 
  - Not compressible
  - Viscosity is slightly higher

- **Gas**
  - compresses easily
  - Lot of empty space

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- Why do different compounds exist in different states	
- $\text { Ice (s) } $
- $H_2O(s) \rightarrow H_2O(l) \rightarrow H_2O(s) \rightarrow H_2O$(g)

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- **Force of attraction between molecules**
- Intermolecular forces of attraction between molecules holds them together
- Temperature - thermal energy 
 - **RT**  
 - R $\rightarrow$ gas constant
 - T $\rightarrow$ kelvin 
 - $8.314 {JK}^{-1} {mol}^{-1} \times 300 {K}$
 - $2.5 {kJ} / {mol}$ at 300 ${K}$

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- ${Cl_2(g)} \longrightarrow {2Cl(g)}$
- Bond enthalpy $(\Delta H) = 242.4 KJ mol^{-1}$
- Typical covalent bond energy
- ${Cl_2(l)} \rightarrow {Cl_2(g)}$
- $\Delta H = 20.4 {kJ} / {mol}$
- It explains that intermolecular forces are smaller than typical covalent bond energy

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- List the types of intermolecular forces
- Identify in a molecule/series of molecules the kind of intermolecular force that predominate
- Given a list of molecules. to arrange them in the correct order of same physical properties which depend on the intermolecular forces

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- Ion-ion  600-1000 kj $mol^{-1}$
- Hydrogen bond  10 - 40 kj mole {-1}
- Ion-dipole  15 kj $mol^{-1}$
- Dipole-dipole  2 kj$ mol^{-1}$
- Dipole-induced dipole < 2kj $mol^{-1}$
- Induced dipole - induced dipole < 2kg $mol^{-1}$
- Induced dipole - induced dipole$\rightarrow$ London Dispersion

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- ${NaCl} \rightarrow {Na}^{+} \stackrel{r}{\longleftrightarrow} {Cl}^{-}$

- Electron negativity of Na = 0.9

- Electron negativity of Cl = 3.0

- $V = \frac {q_1 q_2} {k r}$

- $PbSo_4 \rightarrow Pb^{2+} \quad So_4^{2-}$

- Lattice energy  $\rightarrow$ melting point

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- As we move down in the table ion - ion interaction decreasing

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| molecules                       | $mp/^0C$ | 
| --------                      | -------- | 
| Lithium fluoride     | 848.2    | 
| Lithium chloride     | 610      | 
| Lithium bromide      | 550      | 
| Lithium iodide       | 469      |

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- Match the lattice enthalpies given in the right column with the compounds in the left hand column

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| $\text {Compounds}$ | $$\Delta H^o_{\text {lattice}} {\text {/kJ mol }} ^{-1}$$ |
| --------            | --------                                                  |
| LiCl           | 2153                                                    |
| KBr            | 2524                                                    |
| $MgCl_2$         | 852                                                     |
| $Sr ~ Cl_2$         | $689$                                                     |

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- Repulsion force - short range 
 
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- $ Ion-dipole$
 
- NaCl  in $H_2O$

- NaCl(s) $\rightarrow \quad$ NaCl(aq)

$\quad \quad$$\downarrow \quad \quad \quad \quad \quad \downarrow$

- Lattice energy $\quad$ $Na{^+}Cl^{-}$
 
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