Lewis Structures and Valence Electrons

This video tutorial explains how to draw the Lewis structure for IF6+. It begins by counting the valence electrons of iodine and fluorine, considering the positive charge of the ion. The tutorial then demonstrates how to distribute these electrons to complete the octets for each fluorine atom and discusses the expanded octet for iodine. Finally, it shows how to represent the ion with brackets and a positive sign.

What is the first step in drawing the Lewis structure for IF6+?

• Identify the central atom

• Draw the skeletal structure

• Count the valence electrons

• Determine the molecular shape

How many valence electrons does iodine contribute in IF6+?

• 8

• 7

• 6

• 5

What is the total number of valence electrons in IF6+?

• 48

• 42

• 54

• 60

How many valence electrons are initially placed between iodine and each fluorine atom?

• 2

• 3

• 4

• 1

What is the next step after placing electrons between iodine and fluorine atoms?

• Add lone pairs to iodine

• Check for resonance structures

• Calculate formal charges

• Complete the octets for fluorine atoms

How many electrons does each fluorine atom have after completing its octet?

• 8

• 7

• 9

• 6

Why is it acceptable for iodine to have more than an octet in IF6+?

• Iodine is highly electronegative

• Iodine can form double bonds

• Iodine is a noble gas

• Iodine can have an expanded octet

What should be added to the Lewis structure of IF6+ to indicate it is an ion?

• A negative sign

• A double bond

• Brackets and a positive sign

• A resonance arrow

What is the final step in completing the Lewis structure for IF6+?

• Add lone pairs to fluorine

• Draw the molecular geometry

• Check for resonance

• Place brackets and indicate charge