Draw Lewis structures for each of the following ion: CO3 (2-)
I tried this method below, i do not know where am i going wrong, please help me understand this concept for ions.
Valence Electrons 4e- + 18e- = 22e-
Noble gas Config 8e- + 24e- = 32e-
Total 32e- 22e- = 10e-
Covalent bonds 10e-/2 = 5
Non-Bonding Pairs 22e- - 10e- = 12e-
C has 4 electrons, O has 6 electrons + -2 charge adds 2 more electrons
4 + (3 * 6) + 2 = 24 electrons
4 atoms * 8 electrons per atom = 32 electrons
32 – 24 = 8 electrons
8 electrons ÷ 2 electrons per bond = 4 bonds
24 – 8 = 16 electrons
16 electrons = 8 pairs of non-bonding electrons
The carbonate ion, CO32-, has 1 C atom bonded to 3 O atoms with 4 bonds.
2 C – O bonds and 1 C = O bond, using 4 pair of bonding electrons.
To draw the Lewis structure for the carbonate ion (CO3 2-), follow these steps:
1. Determine the total number of valence electrons:
- Carbon (C) has 4 valence electrons.
- Oxygen (O) has 6 valence electrons each.
- The charge of CO3 2- is 2-, meaning it gained 2 extra electrons. Add 2 electrons to the total.
Total valence electrons = (4 for C) + (3 x 6 for O) + 2 extra electrons = 24
2. Arrange the atoms in the Lewis structure:
Carbon is the central atom because it is least electronegative. Surround it with three oxygen atoms.
O
|
O - C - O
|
3. Connect the atoms with single bonds:
Carbon in the center forms a single bond with each oxygen atom.
O
|
O = C = O
|
4. Distribute the remaining electrons:
Use the remaining 12 electrons to satisfy the octet rule of each atom. Place these electrons as lone pairs on the atoms.
O
|
O = C = O
| |
Each oxygen atom now has 8 electrons (a full octet) and carbon has 8 electrons.
5. Check if each atom has a complete octet:
In this case, all atoms have satisfied the octet rule.
So, the Lewis structure for the carbonate ion (CO3 2-) is O = C = O with a double bond between carbon and each oxygen atom, and one lone pair on each oxygen atom.