Add lone pairs where needed to give octets and determine the shape around each indicated atom. If no lone pairs need to be added, please check the box below. Cl3H3 where do i add the ione pairs
To determine where to add lone pairs in Cl3H3 and the shape around each indicated atom, we need to draw the Lewis structure.
The Lewis structure for Cl3H3 would be:
Cl Cl Cl
| | |
H - C - C - C - H - C
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Cl Cl Cl
In this structure, each chlorine (Cl) atom has 7 valence electrons, and hydrogen (H) has 1 valence electron. Carbon (C) has 4 valence electrons.
We distribute the electrons around the atoms, giving each atom an octet except for the central carbon atom.
Cl Cl Cl
| | |
H - C - C - C - H - C
| | |
Cl Cl Cl
Now, let's check the octet for each atom. The central carbon atom has only 6 valence electrons, so we need to add 2 lone pairs to that carbon atom. This will give it a full octet.
Cl Cl Cl
| | |
H - C - C - C - H - C
| | |
Cl Cl Cl
The shape around each indicated atom is as follows:
- Chlorine (Cl) atoms: Trigonal pyramidal since they have 3 bonded pairs and 1 lone pair.
- Hydrogen (H) atoms: Linear since they have 2 bonded pairs and no lone pairs.
- Central carbon (C) atom: Tetrahedral since it has 4 bonded pairs (with chlorine atoms) and 2 lone pairs.
Therefore, the only place where lone pairs need to be added is at the central carbon atom.