Drawing Lewis Structures for Polyatomic Ions

This video tutorial explains how to draw Lewis structures for various polyatomic ions, including hydroxide (OH-), ammonium (NH4+), cyanide (CN-), nitrate (NO3-), and sulfate (SO4 2-). It covers the process of counting valence electrons, forming chemical bonds, and considering resonance structures and formal charges. The tutorial emphasizes the importance of understanding these structures to simplify chemistry learning.

What is a polyatomic ion?

• An ion with no charge

• An ion with a positive charge only

• An ion with only one type of atom

• An ion with multiple types of atoms

What is the charge of the hydroxide ion (OH-)?

• 2-

• 1-

• 2+

• 1+

How many valence electrons are there in the hydroxide ion (OH-)?

• 8

• 9

• 7

• 6

What is the central atom in the ammonium ion (NH4+)?

• Carbon

• Oxygen

• Hydrogen

• Nitrogen

How many valence electrons are there in the ammonium ion (NH4+)?

• 8

• 9

• 10

• 7

What type of bond is formed between carbon and nitrogen in the cyanide ion (CN-)?

• No bond

• Triple bond

• Double bond

• Single bond

How many valence electrons are there in the cyanide ion (CN-)?

• 11

• 9

• 10

• 8

How many resonance structures can be drawn for the nitrate ion (NO3-)?

• 1

• 2

• 3

• 4

What is the total number of valence electrons in the sulfate ion (SO4 2-)?

• 36

• 34

• 32

• 30

What concept is used to determine the most favorable Lewis structure for the sulfate ion (SO4 2-)?

• Molecular geometry

• Formal charge

• Electronegativity

• Bond length