chemistry-class-11-unit-04-chapter-01-chemical-bonding-molecular-structure-l-1-7-ipu0vumwze0

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Chemical bonds </primary>
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- Bonding in $CO_2$
 - $:\ddot O = C =\ddot{O} {:}$
- Electrostatic potential energy model
 - $E_{e l} \propto \frac{Q_1 \times Q_2}{d}$
- $E_{e l}$ becomes negative as the particles approach each other  
- If $A^{+}$ is approaching $B^{-}$ , there is attraction between them and the energy is decreased

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<footer style = "font-size: 18px"> $\rightarrow$ Chemical bonding and molecular structure $\rightarrow$ <span style = "color:blue"> Chemical bonds </span> $\rightarrow$ Chemical bonds $\rightarrow$ Covalent bond </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Covalent bond </primary>
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- Distance between two hydrogen atom is 74pm

- $\ H_A \frac{74 p m}{} H_B $

- $74 \mathrm{pm}$ is called bond length

- Energy is $-432 \mathrm{~kJ} / \mathrm{mol}$

- $432 \mathrm{~kJ} / \mathrm{mol}$ of energy is to be given to cleave the $\mathrm{H}_2$

- $432 \mathrm{~kJ} /$ mol is the bond energy of the bond in $\mathrm{H}-H$ molecule

- $\ H_A \frac{74 p m}{} H_B $  this bond is called covalent bond

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<footer style = "font-size: 18px">Chemical bonds $\rightarrow$ Chemical bonds $\rightarrow$ <span style = "color:blue"> Covalent bond </span> $\rightarrow$ Types of bond $\rightarrow$ Lewis structures </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Types of bond </primary>
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- **Covalent bond -** Sharing of pair of electrons between two atoms

- **Ionic bond -** Type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound such a bond forms when the valence (outermost) electrons of one atom are transferred permanently to another atom

- **Metallic bond -** Shared electrons are delocalized

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<footer style = "font-size: 18px">Chemical bonds $\rightarrow$ Covalent bond $\rightarrow$ <span style = "color:blue"> Types of bond </span> $\rightarrow$ Lewis structures $\rightarrow$ Lewis symbol </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Lewis structures </primary>
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- $G \cdot N$. Lewis proposed octet rule means eight
- For second row elements, n = 2 , s(2$e^-$) & p(6$e^-$) orbitals - 8$e^-$
- Closed shell configuration for nobel gases
- Single bond (means $2 e^{-}$) shared between two atoms
- Double bond (means $4 e^{-}$) shared between two atoms

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<footer style = "font-size: 18px">Covalent bond $\rightarrow$ Types of bond $\rightarrow$ <span style = "color:blue"> Lewis structures </span> $\rightarrow$ Lewis symbol $\rightarrow$ Drawing Lewis structures </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Drawing Lewis structures </primary>
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- **Step 1 -** Determine the number of valence electrons
- $H_2{O}$
 - 2 $\times$ H+ 0 = 0
 - 2 $\times$ 1 + 6 = $8{e^-}$
 - Total electrons = 8
- **Step 2 -** Determine the central atom
 - Central atom is the one has the greatest bonding capacity
- $\dot{.B.}$  $\quad$  $:C:$

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<footer style = "font-size: 18px">Lewis structures $\rightarrow$ Lewis symbol $\rightarrow$ <span style = "color:blue"> Drawing Lewis structures </span> $\rightarrow$ Drawing lewis structures $\rightarrow$ Drawing lewis structures </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Drawing lewis structures </primary>
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- **Step 3 -** Subtract the number of electrons consumed for forming single bonds from the total  valence $e^-$
- **Step 4 -** Distribute the remaining valence electrons as pairs around each terminal atom so that each atom attains octet of $e^-$
- H requires duet or duplet of $e^-$

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<footer style = "font-size: 18px">Lewis symbol $\rightarrow$ Drawing Lewis structures $\rightarrow$ <span style = "color:blue"> Drawing lewis structures </span> $\rightarrow$ Drawing lewis structures $\rightarrow$ Lewis structures </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Drawing lewis structures </primary>
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- **Step 5 -** Match the number af electrons distributed to the number of valence electron counted in step 1
- **Step 6 -** Complete the octet on the cental atom

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<footer style = "font-size: 18px">Drawing Lewis structures $\rightarrow$ Drawing lewis structures $\rightarrow$ <span style = "color:blue"> Drawing lewis structures </span> $\rightarrow$ Lewis structures $\rightarrow$ Lewis structures </footer>

### <Success style="font-size:25px"> Chemical Bonding Molecular Structure L-1 </Success>
### <primary style="font-size:24px"> Lewis structures </primary>
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- **Example (1)** $\mathrm{CHCl}_3$  
  - Valence electrons
  - $C+H+3 Cl$
  - 4+1 $+$ $\underbrace{3 \times 7}_{21}$
  - $26 V e^{-}$
  - 4 Single bonds = 4 $\times$ 2 = 8$e^{-}$ 
  - 26 - 8 = 18$e^{-}$
  - 4 Single bonds
  - 9 Lone pairs

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<footer style = "font-size: 18px">Drawing lewis structures $\rightarrow$ Drawing lewis structures $\rightarrow$ <span style = "color:blue"> Lewis structures </span> $\rightarrow$ Lewis structures $\rightarrow$ Thank you </footer>