Arsenic Fluoride Lewis Structure Concepts

The video tutorial explains the Lewis structure for the AsF6- ion. It begins by calculating the total valence electrons, placing arsenic at the center, and surrounding it with six fluorine atoms. Single bonds are formed between arsenic and fluorine, and the octets for fluorine are filled. The tutorial ensures all 48 valence electrons are used, and checks that formal charges are zero. The structure is completed by adding brackets to indicate the ion, concluding with a review of the hexafluoroarsinate ion's Lewis structure.

How many total valence electrons are present in the AsF6- ion?

• 42

• 48

• 50

• 54

Which element is placed at the center of the AsF6- Lewis structure?

• Oxygen

• Fluorine

• Arsenic

• Nitrogen

How many single bonds are formed between arsenic and fluorine in the AsF6- structure?

• 7

• 6

• 4

• 5

What is the total number of valence electrons used to complete the octets for all fluorine atoms in AsF6-?

• 36

• 24

• 12

• 48

Why is it acceptable for arsenic to have more than 8 valence electrons in AsF6-?

• Arsenic is highly electronegative.

• Arsenic is in period 4 of the periodic table.

• Arsenic is in period 3 of the periodic table.

• Arsenic is a noble gas.

What is the purpose of adding brackets around the AsF6- Lewis structure?

• To denote the charge distribution

• To indicate it is a molecule

• To show it is an ion

• To highlight the central atom