QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
Draw the best Lewis structure for $\mathrm{CH}_{2} \mathrm{O}$. Based on the Lewis structure for $\mathrm{CH}_{2} \mathrm{O}$, consider the following.
1. The electronic geometry about the carbon atom is Select an answer
2. What is the strongest intermolecular force this molecule would exhibit?
- Iondon dispersion (LDF)
- dipole-dipole
- hydrogen bonding
3. The molecular geometry about the carbon atom is Select an answer
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Step 1:: Draw the Lewis structure for CH^2O.
To draw the Lewis structure, we need to follow these steps:
Step 2:
Count the total number of valence electrons in the molecule. For CH^2O, there are 6 valence electrons from Carbon (C), 2 valence electrons from each Hydrogen atom (H), and 6 valence electrons from the Oxygen atom (O). This gives us a total of 14 valence electrons.
Step 3:
Place the atoms in a reasonable arrangement. Generally, Oxygen and other highly electronegative atoms prefer to be surrounded by less electronegative atoms. So, arrange CH^2O in a linear shape with O at one end, C in the middle, and two H atoms bonded to C.
Step 4:
Draw a skeleton structure by adding bonds between the atoms. Each single bond contains 2 electrons, so we've used up 4 electrons (2 bonds) in the CH^2O molecule.
Step 5:
Distribute the remaining electrons around the atoms to complete their octets. For CH^2O, we have 10 electrons left. Place these electrons as lone pairs on the O and C atoms to complete their octets. The final Lewis structure for CH^2O is: H:::C:::O: (where each colon represents a pair of electrons in the bond or as lone pairs)
Step 6:: Determine the electronic geometry about the carbon atom.
The electronic geometry about the carbon atom is tetrahedral. Although it appears linear in the Lewis structure, the lone pairs on the carbon atom occupy space and create a tetrahedral geometry with bonded atoms and lone pairs.
Step 7:: Identify the strongest intermolecular force this molecule would exhibit.
The molecular dipole moment of CH^2O points from the positive end (the Hydrogen atoms) to the negative end (the Oxygen atom). Therefore, the strongest intermolecular force this molecule would exhibit is dipole-dipole.
Step 8:: Determine the molecular geometry about the carbon atom.
The molecular geometry about the carbon atom is linear, as the two Hydrogen atoms and the Oxygen atom are all bonded in a straight line.
Final Answer
1. The electronic geometry about the carbon atom is tetrahedral. 2. The strongest intermolecular force this molecule would exhibit is dipole-dipole. 3. The molecular geometry about the carbon atom is linear.
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