Drawing Lewis Structures for Ionic Compounds

Dr. Morris explains how to draw Lewis structures for ionic compounds, using examples like sodium chloride, sodium oxide, and magnesium sulfide. The video highlights the importance of valence electrons and the octet rule in forming stable ionic compounds. It also demonstrates how to predict the ratios in which elements combine to form these compounds.

What is the main focus of this episode of Real Chemistry?

• Covalent bonding

• Lewis structures for ionic compounds

• Molecular geometry

• Chemical reactions

Why are sodium metal and chlorine gas dangerous to ingest?

• They are both highly reactive

• They are both inert gases

• They are both liquids at room temperature

• They are both non-reactive

How many valence electrons does sodium have?

• Two

• Seven

• Eight

• One

What happens to sodium's valence electron when it forms sodium chloride?

• It is lost to oxygen

• It is shared with chlorine

• It is lost to chlorine

• It remains with sodium

What is the charge on chlorine after it gains an electron from sodium?

• Negative

• Positive

• Neutral

• Double positive

How many sodium atoms are needed to combine with one oxygen atom to form sodium oxide?

• Four

• Three

• Two

• One

What is the charge on the oxygen ion in sodium oxide?

• 1-

• 2-

• 1+

• 2+

How many valence electrons does magnesium have?

• Eight

• Two

• One

• Six

How many electrons does sulfur need to achieve an octet?

• One

• Two

• Four

• Three

What is the charge on the magnesium ion in magnesium sulfide?

• 1-

• 2+

• 2-

• 1+