To draw the Lewis structure for Co(BASF6), we need to identify the total number of valence electrons and the arrangement of atoms.
Step 1: Count the Valence Electrons
Cobalt (Co) is in group 9 of the periodic table, contributing 9 valence electrons. Each fluorine (F) atom, of which there are 6, contributes 7 valence electrons, giving us a total of 42 from fluorine. Therefore, the total valence electrons from all the elements are:
- Co: 9
- F: 6 × 7 = 42
This gives us a total of 9 + 42 = 51 valence electrons.
Step 2: Identify the Central Atom
Cobalt is the central atom in this molecule. It will bond with the six fluorine atoms surrounding it.
Step 3: Connect Atoms with Single Bonds
Place a single bond between the cobalt atom and each of the six fluorine atoms. Each bond accounts for 2 electrons, so we will use 6 bonds × 2 electrons = 12 electrons.
Step 4: Distribute Remaining Electrons
After using 12 electrons for the bonds, we have 51 – 12 = 39 electrons remaining. Each fluorine needs 6 electrons to complete its octet, and since each bond already has 2 of those electrons, we need 4 more for each fluorine. With 6 fluorine atoms, we require 6 × 4 = 24 electrons. That leaves us with 39 – 24 = 15 electrons.
Step 5: Complete the Octet for Cobalt
Since cobalt can expand its octet, we can distribute the remaining electrons to the cobalt atom. By adding these electrons, we can represent cobalt with an expanded octet. Therefore, Cobalt will have a total of 9 from its own valence and an additional 6 from bonding with six fluorine atoms.
Final Structure
The final Lewis structure shows the cobalt atom at the center with six fluorine atoms surrounding it, each satisfying their octet. The structure will look like a central Co atom bonded to six F atoms with single bonds.
This completes the drawing of the Lewis structure for Co(BASF6).