Multiple Choice
Draw the Lewis Dot Structure for the following ion:PCl4+.
10. Chemical Bonding
Lewis Dot Structures: Ions (Simplified)
Struggling with Introduction to Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Determine the Lewis Dot Structure for the following ion:SCl42+.
A
B
C
D
Verified step by step guidance1
Identify the total number of valence electrons for the SCl4^2+ ion. Sulfur (S) has 6 valence electrons, and each chlorine (Cl) has 7 valence electrons. Since there are four chlorine atoms, the total is 6 + (4 * 7) = 34 valence electrons. However, because the ion has a 2+ charge, we subtract 2 electrons, resulting in 32 valence electrons.
Place the sulfur atom in the center as it is less electronegative than chlorine. Arrange the four chlorine atoms around the sulfur atom.
Distribute the 32 valence electrons around the atoms, starting by forming single bonds between the sulfur and each chlorine atom. This uses up 8 electrons (2 electrons per bond).
Distribute the remaining 24 electrons to complete the octets of the chlorine atoms. Each chlorine atom needs 6 more electrons to complete its octet, using up all 24 remaining electrons.
Check the formal charges to ensure the most stable structure. The formal charge is calculated as: Formal Charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons/2). Adjust the structure if necessary to minimize formal charges, keeping in mind the 2+ charge of the ion.
3:11mWatch next
Master Lewis Dot Structures: Ions (Simplified) Concept 1 with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Lewis Dot Structures: Ions (Simplified) practice set
Problem sets built by lead tutorsExpert video explanations