Valence Electrons and Lewis Structures

This video tutorial explains how to draw the Lewis structure for SbF4-. It begins by counting the valence electrons of antimony and fluorine, considering the extra electron due to the negative charge. The tutorial then guides viewers through placing the atoms and electrons to form bonds and complete octets. It addresses the concept of expanded octets for antimony, which allows for more than eight electrons. Finally, the video shows how to finalize the structure with brackets and a negative sign to indicate the ion.

How many total valence electrons are there in SBF4-?

• 34

• 32

• 38

• 36

How many valence electrons does antimony contribute in the SBF4- structure?

• 3

• 5

• 7

• 9

What group is fluorine in, and how many valence electrons does it have?

• Group 16, 6 electrons

• Group 18, 8 electrons

• Group 15, 5 electrons

• Group 17, 7 electrons

Which atom is placed at the center of the SBF4- Lewis structure?

• Fluorine

• Antimony

• Boron

• Sulfur

What is the primary role of electrons placed between atoms in a Lewis structure?

• To show polarity

• To indicate charge

• To complete octets

• To form chemical bonds

How many valence electrons are used to complete the octets of the fluorine atoms?

• 24

• 28

• 32

• 34

What is the significance of the remaining two valence electrons in the SBF4- structure?

• They are shared with another molecule

• They are unused

• They form a new bond

• They expand the octet of antimony

Why can antimony have an expanded octet in the SBF4- structure?

• It is in period 2

• It is a noble gas

• It is in period 3

• It is below period 3

What should be added to the Lewis structure to indicate that SBF4- is an ion?

• A lone pair

• A positive sign

• A double bond

• A negative sign