$$ \leftarrow $$ $$ \mathrm{COF}_{2} $$ is a highly toxic compound that was used as a chemical weapon in Worlo War I. of 31 Draw the Lewis structure of $$ \mathrm{CF}_{2} \mathrm{O} $$

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1. **Count the valence electrons:**  
   - Carbon: $$4$$ electrons  
   - Each Fluorine: $$7$$ electrons (total for two: $$2\times7=14$$)  
   - Oxygen: $$6$$ electrons  
     
   Total electrons:  
   $$
   4 + 14 + 6 = 24 \text{ electrons}
   $$

2. **Choose the skeletal structure:**  
   Carbon is the least electronegative atom, so it is the central atom.  
   Connect Carbon to two Fluorine atoms and to Oxygen.  
     
   An appropriate initial skeletal structure is:  
   $$
   \mathrm{F} - \mathrm{C} - \mathrm{O} \quad \text{with another } \mathrm{F} \text{ attached to } \mathrm{C}
   $$

3. **Assign bonds and electrons:**  
   To satisfy the octet rule for all atoms, it is best to form a double bond between Carbon and Oxygen.  
   - Carbon–Oxygen double bond uses $$4$$ electrons  
   - Two Carbon–Fluorine single bonds use $$2 \times 2 = 4$$ electrons  
     
   Total electrons used in bonding:  
   $$
   4 + 4 = 8 \text{ electrons}
   $$  
     
   Remaining electrons for lone pairs:  
   $$
   24 - 8 = 16 \text{ electrons}
   $$

4. **Complete the octets with lone pairs:**  
   - **Fluorine atoms:** Each Fluorine is single bonded to Carbon, so it has $$2$$ bonding electrons and needs $$6$$ more electrons (i.e., $$3$$ lone pairs) to complete its octet. For two Fluorines, that uses $$2\times6=12$$ electrons.  
   - **Oxygen atom:** Oxygen is double bonded to Carbon (receiving $$4$$ bonding electrons) and needs $$4$$ additional electrons (i.e., $$2$$ lone pairs) to complete its octet. This uses $$4$$ electrons.  
     
   Total electrons assigned as lone pairs:  
   $$
   12 + 4 = 16 \text{ electrons}
   $$

5. **Final Lewis Structure:**

The final Lewis dot structure for $$\mathrm{CF}_{2}\mathrm{O}$$ is:

$$
   \begin{array}{rcl}
   &&\ :\!:\quad \
   &&\quad | \
   \mathrm{F}&:&\cdot\!\cdot \
   &&\quad | \
   &&\ \ \ \ \, \, \, \, \, \ \, \, \, \, \, \, \, \, \, \, \
   &&\quad \mathrm{C} \
   &&\diagdown\quad\diagup \
   \mathrm{F} & & \mathrm{O} \, \, \, (\text{with a double bond})\
   &&\quad \,\,\,: \!:\, 
   \end{array}
   $$
   
   A clearer representation is:

$$
   \begin{array}{ccccccc}
       & & \ddots & & \
       & & :\!\!F & & \
       & & | & & \
   :\!F & - & \mathrm{C} & = & \mathrm{O} \
       & & | & & \
       & & :\!\!F & & \
       & & \ddots & & \
   \end{array}
   $$

More conventionally, draw the structure as:

$$
   \begin{array}{rcl}
      &&\text{F with three lone pairs} \
      &&\quad \vdots \
      \quad &\quad &\mathrm{F}\[6mm]
   \mathrm{:F} & - & \mathrm{C} = \mathrm{O}\[4mm]
       &&\quad \vdots \quad \text{(Oxygen with two lone pairs)}
   \end{array}
   $$

Where:  
   - Each $$\mathrm{F}$$ has $$3$$ lone pairs  
   - $$\mathrm{O}$$ has $$2$$ lone pairs  
   - $$\mathrm{C}$$ is the central atom with a double bond to $$\mathrm{O}$$ and single bonds to each $$\mathrm{F}$$.

This structure satisfies the octet rule for all atoms and uses exactly $$24$$ valence electrons.
The Lewis structure of $$ \mathrm{CF}_{2}\mathrm{O} $$ is: $$ \begin{array}{rcl} &&\text{F with three lone pairs} \ &&\quad \vdots \ \quad &\quad &\mathrm{F}\[6mm] \mathrm{:F} & - & \mathrm{C} = \mathrm{O}\[4mm] &&\quad \vdots \quad \text{(Oxygen with two lone pairs)} \end{array} $$ Each fluorine has three lone pairs, oxygen has two lone pairs, and carbon has a double bond to oxygen and single bonds to each fluorine.

is a highly toxic compound that was used as a chemical weapon in Worlo
War I. of 31
Draw the Lewis structure of

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