Choose Lewis dot structure for the hypothetical molecule shown below, using the correct number of valence electrons for each atom.

Question

A hypothetical compound that has the following structure: H O C H 2 C H O. The last oxygen atom (from left to right) is attached to its carbon by a double bond.

The Lewis dot structure for the hypothetical compound H O C H 2 C H O, where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is shown as a pair of dots. Every oxygen atom has two additional pairs of dots. The double bond between the carbon and the oxygen atom is illustrated as two pairs of dots.
The Lewis dot structure for the hypothetical compound H O C H 2 C H O, where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is represented by a pair of dots. The double bond between the carbon and the oxygen atom is illustrated as two pairs of dots.
The Lewis dot structure for the hypothetical compound H O C H 2 C H O, where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is represented by one dot. The double bond between the carbon and the oxygen atom is illustrated as two dots.
The Lewis dot structure for the hypothetical compound H O C H 2 C H O, where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is represented by a pair of dots. Every oxygen atom has two additional pairs of dots. Every hydrogen atom has one additional dot. The double bond between the carbon and the oxygen atom is illustrated as two pairs of dots.

GPT-4o mini · Answer

To draw the Lewis dot structure for the molecule \( H - O - C - H_2 - C - H - O \) with the specified structure where the last oxygen is double-bonded to the last carbon, we need to follow these steps:

Count Valence Electrons:
- Hydrogen (H) has 1 valence electron; there are 4 H atoms: \( 4 \times 1 = 4 \).
- Oxygen (O) has 6 valence electrons; there are 2 O atoms: \( 2 \times 6 = 12 \).
- Carbon (C) has 4 valence electrons; there are 2 C atoms: \( 2 \times 4 = 8 \).
Total = 4 (H) + 12 (O) + 8 (C) = 24 valence electrons.
Draw the Skeleton Structure: The structure of the molecule is:
```
H - O - C - H2 - C = O
```
Place Electrons in Bonds:
- Each bond between atoms will use 2 electrons (1 from each atom).
- For the skeleton structure, the first bond is between \( H \) and \( O \), then from \( O \) to \( C \), followed by two bonds from the first \( C \) to two \( H \) atoms, and the second \( C \) is bonded to the other \( H \) atom and has a double bond with the last \( O \).
Complete the Octets:
- Each O atom needs to have a complete octet, so we add lone pairs of electrons around oxygen.
- The first O (attached to the first C) gets 2 additional lone pairs of electrons (4 electrons total).
- The second O (attached to the second C via a double bond) will have 2 bonds with the second C and will also get 2 additional lone pairs (4 electrons total).
Final Structure: Now we can identify the correct description of the Lewis dot structures as specified in your options.

From your descriptions:

The option that states "The Lewis dot structure for the hypothetical compound \( H - O - C - H_2 - C - H - O \), where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is represented by a pair of dots. The double bond between the carbon and the oxygen atom is illustrated as two pairs of dots" seems to be the most accurate.

Thus, the correct choice is: The Lewis dot structure for the hypothetical compound H O C H 2 C H O, where the last oxygen atom, from left to right, is attached to its carbon by a double bond. Every covalent bond is represented by a pair of dots. The double bond between the carbon and the oxygen atom is illustrated as two pairs of dots.