Question

you can use this periodic table during the quiz. however, as stated in the course outline, and in the orientation session, this quiz is not open book. you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc. question 1 (1 point) which of the following has the lowest number of unshared electrons around the central atom? xef4 so2 clf3 h2o sf6

Explanation:

Step1: Determine valence - electrons of central atoms

Use the group number of the central atom in the periodic table to find valence - electrons.

Step2: Calculate bonding and non - bonding electrons for each compound

• For \(XeF_4\):
• \(Xe\) is in Group 18, has 8 valence electrons. It forms 4 bonds with \(F\) atoms. So the number of unshared electrons \(=8 - 4\times1= 2\) lone pairs (4 unshared electrons).
• For \(SO_2\):
• \(S\) is in Group 16, has 6 valence electrons. It forms 2 double - bonds with \(O\) atoms. So the number of unshared electrons \(=6-4 = 1\) lone pair (2 unshared electrons).
• For \(ClF_3\):
• \(Cl\) is in Group 17, has 7 valence electrons. It forms 3 bonds with \(F\) atoms. So the number of unshared electrons \(=7 - 3\times1=2\) lone pairs (4 unshared electrons).
• For \(H_2O\):
• \(O\) is in Group 16, has 6 valence electrons. It forms 2 bonds with \(H\) atoms. So the number of unshared electrons \(=6 - 2\times1 = 2\) lone pairs (4 unshared electrons).
• For \(SF_6\):
• \(S\) is in Group 16, has 6 valence electrons. It forms 6 bonds with \(F\) atoms. So the number of unshared electrons \(=6-6\times1 = 0\) lone pairs (0 unshared electrons).

Answer:

\(SF_6\)