QQuestionChemistry
QuestionChemistry
Draw the Lewis structure of chloroform, also called trichloromethane, $\left(\mathrm{CHCl}_{3}\right)$ and then determine the ideal bonding angle(s) of the central atom.
A) $180^{\circ}$
B) $90^{\circ}$ and $120^{\circ}$
C) $109.5^{\circ}$
D) $120^{\circ}$
E) $135^{\circ}$
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Answer
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Step 1:: Draw the Lewis structure of chloroform, $\left(\mathrm{CHCl}_{3}\right)$.
To draw the Lewis structure, we need to follow these steps:
Step 2:
Count the total number of valence electrons for the molecule. Chlorine (Cl) has 7 valence electrons, and hydrogen (H) has 1 valence electron. The central atom, carbon (C), has 4 valence electrons. So, the total number of valence electrons is: \text{Total valence electrons} = 4 \text{(C)} + 1 \text{(H)} + 7 \times 3 \text{(Cl)} = 28 \text{ valence electrons}
Step 3:
Place the central atom in the structure and add all the other atoms around it. In this case, the central atom is carbon, and it is bonded to one hydrogen atom and three chlorine atoms: \mathrm{H}-\mathrm{C}-\mathrm{ClClCl}
Step 4:
Add electron pairs to form bonds between atoms. In this case, we need to add single bonds between carbon and each of the other atoms: \mathrm{H}-\mathrm{C}-\mathrm{ClClCl} \qquad \text{(8 electrons used)}
Step 5:
Distribute the remaining electrons as lone pairs on the outer atoms. In this case, we have 20 electrons left, which should be distributed as 5 lone pairs on the chlorine atoms: \mathrm{H}-\mathrm{C}\left(\mathrm{Cl} : : \mathrm{Cl}\right)\left(\mathrm{Cl} : : \mathrm{Cl}\right) \qquad \text{(28 electrons used)}
Step 6:: Determine the ideal bonding angle(s) of the central atom.
Therefore, the ideal bonding angle(s) of the central atom is $109.5^{\circ}$.
In the Lewis structure, the central carbon atom is bonded to three chlorine atoms and one hydrogen atom.
Final Answer
So, the correct answer is option (C).
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