To build the Lewis structure of SeCl3+, we first need to determine the total number of valence electrons. Selenium (Se) has 6 valence electrons, and each chlorine (Cl) has 7 valence electrons. Since there are three chlorine atoms, we have:
6+3×7=27 valence electrons
However, because the molecule has a positive charge, we subtract one electron:
27−1=26 valence electrons
Next, we draw the skeletal structure with selenium (Se) as the central atom and three chlorine (Cl) atoms bonded to it. Each bond represents 2 electrons.
After placing the bonds, we distribute the remaining electrons to satisfy the octet rule for each atom. Each Se-Cl bond uses 2 electrons, so:
3×2=6 electrons used in bonds
Subtracting these from the total valence electrons:
26−6=20 electrons remaining
Each chlorine atom needs 8 electrons to complete its octet. Since each Cl already has 2 electrons from the bond, each needs 6 more electrons:
3×6=18 electrons for Cl atoms
Subtracting these from the remaining electrons:
20−18=2 electrons remaining
The remaining 2 electrons are placed on the selenium atom.
Finally, we check the formal charges to ensure the structure is correct. The formal charge is calculated as:
Formal charge=Valence electrons−Non-bonding electrons−2Bonding electrons
For selenium:
6−2−26=6−2−3=+1
For each chlorine:
7−6−22=7−6−1=0
The positive charge is on the selenium atom, which matches the given SeCl3+.
The Lewis structure of SeCl3+ is:
Cl∣Cl−Se+−Cl
Lewis structure of SeCl3+ is correct