Draw the Lewis dot structure of 2-(chlorite ion) ?and answer the following:
Only Lewis structures that obey the octet rule (or duet for ) ?will be counted as correct in this class.
Number of total valence electrons = ?valence electrons
Describe the Lewis structure around the central atom, ?? ?:
Describe the Lewis structure around each oxygen atom (both should be the same):
The Correct Answer and Explanation is :
Let’s break down the Lewis structure of the chlorite ion ((ClO_2^-)).
Step 1: Determine the total number of valence electrons.
- Chlorine (Cl) is in Group 17 (Halogens), so it has 7 valence electrons.
- Oxygen (O) is in Group 16, so each oxygen atom has 6 valence electrons.
- There are two oxygen atoms, so (2 \times 6 = 12) valence electrons from the oxygen atoms.
- The negative charge on the ion adds one additional electron.
So, the total number of valence electrons is:
[
7 (\text{Cl}) + 12 (\text{O}) + 1 (\text{negative charge}) = 20 \text{ valence electrons}
]
Step 2: Draw the skeleton structure.
The central atom will be chlorine (Cl), with the two oxygen atoms bonded to it. The chlorite ion has a bent shape, with oxygen atoms on each side.
- Chlorine will be the central atom because it is less electronegative than oxygen.
- Each oxygen atom will form a single bond with the chlorine.
Step 3: Distribute the electrons.
- Start by drawing a single bond between chlorine and each oxygen. Each bond counts as 2 electrons.
- After drawing the single bonds, there are (20 – 4 = 16) electrons left to be placed.
- Distribute the remaining electrons to complete the octet for the oxygen atoms. Since each oxygen is attached by a single bond, it will need 6 more electrons to complete its octet.
- After completing the oxygen octets, the remaining electrons go on chlorine.
Step 4: Check for resonance.
The chlorite ion has resonance structures, which means the electrons are delocalized. The negative charge can be placed on either of the oxygen atoms.
Final structure:
- Chlorine has 3 lone pairs of electrons and shares one pair of electrons with each oxygen.
- Each oxygen has 3 lone pairs and shares one bond with chlorine.
- The negative charge resides on one of the oxygen atoms, and the structure is represented as a resonance hybrid of the two possible configurations.
Step 5: Answer the questions.
Number of total valence electrons = 20 valence electrons
Describe the Lewis structure around the central atom (Chlorine):
The chlorine atom is in the center, forming single bonds with each of the two oxygen atoms. It has 3 lone pairs of electrons, and each oxygen atom is attached by a single bond. Chlorine does not fulfill the octet rule, as it can accommodate more than 8 electrons in its valence shell (it can hold up to 12 electrons).
Describe the Lewis structure around each oxygen atom:
Each oxygen atom has 3 lone pairs of electrons and forms a single bond with chlorine. Each oxygen atom needs 6 electrons to complete its octet, so these are provided as lone pairs of electrons. One of the oxygen atoms carries a negative charge.
Now, I’ll generate the image of the Lewis structure for you.
Here is the Lewis structure of the chlorite ion ((ClO_2^-)) showing the central chlorine atom, two oxygen atoms, and the lone pairs of electrons. The structure also includes the delocalized negative charge, which can be shared between the two oxygen atoms in resonance.
Let me know if you need further details or explanations!
