Draw the Lewis structure for COCl2, including lone pairs.
What is the molecular shape of COCl2? The C - Cl ...

Question

Draw the Lewis structure for COCl2, including lone pairs.
What is the molecular shape of COCl2? The C - Cl bond in COCl2 is polar or nonpolar?

What is the Cl - C - Cl bond angle? The molecule COCl2 is polar or nonpolar?

CramX · Accepted Answer

Step 1: : Draw the Lewis structure for COCl2.. To draw the Lewis structure, first count the total number of valence electrons for the molecule. Carbon (C) is in the 4th group, so it has 4 valence electrons. Oxygen (O) is in the 6th group, so it has 6 valence electrons. Chlorine (Cl) is also in the 7th group, so it has 7 valence electrons. The molecule contains one carbon atom, one oxygen atom, and two chlorine atoms, so the total number of valence electrons is: 	ext{Total valence electrons} = 4 	ext{(C)} + 6 	ext{(O)} + 7 	ext{(Cl)} + 7 	ext{(Cl)} = 24 Now, subtract the number of electrons used to form bonds. In this case, there are two single bonds (each using 2 electrons) between carbon and chlorine atoms, and one double bond (using 4 electrons) between carbon and oxygen atoms. Therefore, the number of electrons used to form bonds is: 	ext{Bonding electrons} = 2 	ext{(C-Cl bonds)} + 4 	ext{(C=O bond)} = 8 The remaining electrons are non-bonding electrons (lone pairs). In this case, we have: 	ext{Lone pairs} = 	ext{Total valence electrons} - 	ext{Bonding electrons} = 24 - 8 = 16 Distribute the valence electrons around the molecule, ensuring that each atom has 8 electrons in its outer shell. The resulting Lewis structure for COCl2 is: \mathrm{O} : \underbrace{\overbrace{\boxed{\cdot \mathrm{C} \cdot}}^{	ext{double bond}} : \mathrm{Cl}}_{	ext{single bond}} : \mathrm{Cl} Step 2: : Determine the molecular shape of COCl2.. The molecular shape is determined by the central atom's bonded and non-bonded electron pairs. In this case, the central atom is carbon, which has two bonded chlorine atoms and one double-bonded oxygen atom. The electron pairs around the central carbon atom form a linear geometry. Therefore, the molecular shape of COCl2 is linear. Step 3: : Determine if the C - Cl bond in COCl2 is polar or nonpolar.. The C - Cl bond is polar because chlorine is more electronegative than carbon. Step 4: : Determine the Cl - C - Cl bond angle.. Since the molecular shape of COCl2 is linear, the bond angle between the two chlorine atoms is 180 degrees. Step 5: : Determine if the molecule COCl2 is polar or nonpolar.. The molecule is polar because the C - Cl bond is polar and the bond angle is 180 degrees, which does not allow the dipole moments to cancel out. Final Answer: 1. The Lewis structure for COCl2 is: $ \mathrm{O} : \underbrace{\overbrace{\boxed{\cdot \mathrm{C} \cdot}}^{	ext{double bond}} : \mathrm{Cl}}_{	ext{single bond}} : \mathrm{Cl} $ 2. The molecular shape of COCl2 is linear. 3. The C - Cl bond in COCl2 is polar. 4. The Cl - C - Cl bond angle is 180 degrees. 5. The molecule COCl2 is polar.

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Step 1:
: Draw the Lewis structure for COCl^2.

Step 2:
: Determine the molecular shape of COCl^2.

Step 3:
: Determine if the C - Cl bond in COCl^2 is polar or nonpolar.

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