Lewis Structures and Valence Electrons

This video tutorial explains how to draw the Lewis structure for ClF4+. It begins by counting the valence electrons using the periodic table, considering the positive charge of the ion. The tutorial then guides the placement of chlorine and fluorine atoms, forming chemical bonds, and completing the octet for fluorine. It discusses the concept of an expanded octet for chlorine, allowing it to hold more than eight electrons. The video concludes by finalizing the structure with brackets and a positive charge to indicate the ion.

What is the first step in drawing the Lewis structure for ClF4+?

• Determine the molecular shape

• Count the valence electrons

• Identify the central atom

• Draw the skeletal structure

How many valence electrons does chlorine have?

• 6

• 5

• 8

• 7

What does the positive charge in ClF4+ indicate?

• An extra electron is present

• An electron has been lost

• A proton has been added

• A neutron has been lost

Why is chlorine placed at the center of the ClF4+ Lewis structure?

• It has fewer valence electrons

• It is less electronegative

• It is a larger atom

• It is more electronegative

What is formed when a pair of electrons is placed between atoms?

• An ionic bond

• A covalent bond

• A metallic bond

• A hydrogen bond

How many total valence electrons are used in the ClF4+ structure before considering extra electrons?

• 28

• 30

• 32

• 34

Why can't extra electrons be placed around fluorine in ClF4+?

• Fluorine is too small

• Fluorine can have an expanded octet

• Fluorine can only have an octet

• Fluorine is too electronegative

What allows chlorine to have an expanded octet?

• It is a transition metal

• It is in period 2

• It is in period 3

• It is a noble gas

How many valence electrons does chlorine have in the expanded octet of ClF4+?

• 8

• 9

• 10

• 11

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

• A negative sign

• Both brackets and a positive sign

• A positive sign

• Brackets