Lewis Structures and Resonance Concepts

The video tutorial explains how to draw the Lewis structure for the SN- ion. It begins by counting the valence electrons of sulfur, nitrogen, and oxygen, considering the extra electron due to the negative charge. The tutorial then demonstrates forming chemical bonds and completing octets. It discusses resonance structures and the importance of calculating formal charges to determine the most favorable structure. The video concludes by identifying the most likely Lewis structure based on electronegativity, emphasizing that the negative charge should be on the more electronegative element, oxygen.

What is the total number of valence electrons in SN-?

• 19

• 17

• 16

• 18

Which group does sulfur belong to in the periodic table?

• Group 15

• Group 14

• Group 16

• Group 17

How many valence electrons are initially placed between atoms to form bonds?

• 6

• 2

• 8

• 4

What is the purpose of using double or triple bonds in the Lewis structure?

• To change the element type

• To satisfy the octet rule

• To increase the number of atoms

• To decrease the number of electrons

What are resonance structures?

• Structures with different arrangements of electrons

• Structures with different elements

• Structures with different numbers of electrons

• Structures with different atoms

Which element in SN- is more electronegative?

• Oxygen

• Nitrogen

• Sulfur

• Hydrogen

Why is the negative charge placed on oxygen in the most favorable Lewis structure?

• Oxygen is larger in size

• Oxygen has more protons

• Oxygen is less electronegative

• Oxygen is more electronegative

What is the formal charge on sulfur in the most favorable Lewis structure?

• +2

• -1

• 0

• +1

How does the actual SN- molecule exist in terms of resonance structures?

• As a completely different structure

• As a single structure

• As a combination of resonance structures

• As a non-resonant structure

What is the formal charge on oxygen when it is double-bonded in the Lewis structure?

• -1

• 0

• +2

• +1