Lewis structure of [(CH3)3O]+. Be sure to show all atoms, bonds, lone pairs, and formal charges.
Convert CH3CH(Cl)CH(OH)CH3 into a skeletal structure.
If you could explain it, it would help. Or somehow do some of it here and explain. Im having a lot of trouble with this question. Thank you.
To draw the Lewis structure of [(CH3)3O]+, you need to first determine the total number of valence electrons.
The formula [(CH3)3O]+ suggests that you have three methyl groups (CH3) and one oxygen atom (O) with a positive charge (+). Each carbon atom contributes four valence electrons, the three hydrogen atoms contribute one valence electron each, and the oxygen atom contributes six valence electrons. Since there are three methyl groups, the total number of valence electrons is:
3 × (4 + 1) + 6 + 1 = 21
Now, let's draw the Lewis structure step by step:
1. Start by placing the oxygen atom (O) in the center and connect it to each of the three methyl groups (CH3).
H H H
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H C - O - C - C H
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H H H
2. Next, distribute the remaining electrons to satisfy the octet rule for each atom. Hydrogen atoms (H) only need two valence electrons to complete their shells, so each hydrogen atom will have two electrons.
H H H
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H - C - O - C - C - H
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H H
3. The oxygen atom (O) has six valence electrons, so it needs two more to complete its octet. Since it carries a positive charge, it lacks two electrons. We can place these two electrons in the form of a lone pair of electrons on the oxygen atom.
H H H
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H - C - O - C - C - H
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H . H
4. Carbon atoms (C) also need four more electrons to complete their octets. Each carbon atom should form one bond and have three lone pairs of electrons.
H H H
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H - C - O - C - C - H
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H . H
5. Finally, assign the formal charges. To do this, we need to compare the number of valence electrons each atom has in the Lewis structure with the number it would normally have.
The oxygen atom has six valence electrons (2 from the lone pair and 4 from the bonds) compared to its normal six valence electrons. Therefore, the oxygen atom has a formal charge of +1.
The carbon atoms, with four valence electrons in the Lewis structure (one from a bond and three lone pairs), also have four valence electrons in their normal state. They have no formal charge.
The final Lewis structure of [(CH3)3O]+ is:
H H H
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H - C - O - C - C - H
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H . H
Formal charge: +1
(Note: The dot (.) represents a lone pair of electrons)
To determine the Lewis structure of [(CH3)3O]+, let's break it down step-by-step:
1. Count the total number of valence electrons:
Carbon (C) has 4 electrons.
Hydrogen (H) has 1 electron.
Oxygen (O) has 6 electrons.
Positive charge means we remove one electron.
The molecular formula [(CH3)3O]+ contains one carbon atom (C), three hydrogen atoms (H), and one oxygen atom (O).
2. Determine the central atom:
In this case, the central atom is oxygen (O) since it is less electronegative than carbon (C).
3. Connect the atoms:
Connect the three methyl groups (CH3) to the oxygen atom (O) by single bonds. Each carbon (C) atom will be bonded to the oxygen (O) atom.
4. Place the remaining electrons around the atoms:
Start by placing the electrons in pairs (lone pairs) around the atoms. Oxygen (O) will have 6 electrons placed around it since it is group 6A (Group 16) element.
5. Calculate the formal charges:
Formal charge (FC) is the hypothetical charge that an atom would possess if all the shared electrons were divided equally between the bonded atoms. Formal charge can be calculated using the formula:
FC = Group number (valence electrons) - 1/2 (shared electrons) - unshared electrons
6. Adjust the formal charges:
Rearrange the electrons to achieve a more stable structure by minimizing formal charges. Try to place the negative charge on the more electronegative atom.
Here is the step-by-step process for the Lewis structure of [(CH3)3O]+:
Step 1: Determine the total number of valence electrons:
Carbon (C) = 4 valence electrons x 3 atoms = 12 electrons
Hydrogen (H) = 1 valence electron x 3 atoms = 3 electrons
Oxygen (O) = 6 valence electrons
Positive charge: -1 electron
Total valence electrons = 12 + 3 + 6 - 1 = 20 electrons.
Step 2: Determine the central atom:
Oxygen (O) is less electronegative than carbon (C), so oxygen will be the central atom.
Step 3: Connect the atoms:
Connect each carbon (C) atom to the oxygen (O) atom by single bonds.
H H H
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H - C - C - C - O
Step 4: Place the remaining electrons:
Place 6 lone pair electrons on the oxygen (O) atom.
H H H
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H - C - C - C = O
Step 5: Calculate formal charges:
To calculate the formal charges, we need to distribute the electrons as follows:
Carbon initially has 4 valence electrons, and it gains one electron from each of the three sigma bonds with the hydrogen atoms.
Oxygen initially has 6 valence electrons, and it gains two electrons from each of the carbon-oxygen bonds.
Formal charges:
Carbon (C1) = 4 - 4/2 - 0 = 0
Carbon (C2) = 4 - 4/2 - 0 = 0
Carbon (C3) = 4 - 4/2 - 0 = 0
Oxygen (O) = 6 - 4/2 - 4 = 0
Step 6: Adjust the formal charges:
In this case, all atoms have a formal charge of 0, which is the most stable configuration.
The final Lewis structure of [(CH3)3O]+ is:
H H H
| | |
H - C - C - C = O
Note: The positive charge is indicated by the "+" sign.