Ionic Compounds and Lithium Chemistry

The video tutorial explains how to draw the Lewis structure for lithium carbonate (Li2CO3). It begins by identifying lithium as a metal and carbonate as a polyatomic ion, forming an ionic compound. The tutorial details how lithium transfers its valence electrons to carbonate, resulting in a positive charge for lithium and a negative charge for carbonate. This electron transfer leads to the formation of ionic bonds. The video also explains the concept of a formula unit and how these units form a crystal structure in ionic compounds.

What type of compound is lithium carbonate?

• Ionic

• Molecular

• Metallic

• Covalent

What is the role of lithium in the formation of lithium carbonate?

• It gains electrons from carbonate.

• It shares electrons with carbonate.

• It transfers electrons to carbonate.

• It does not interact with carbonate.

How many valence electrons does each lithium atom have before bonding?

• Four

• Three

• One

• Two

What charge does lithium acquire after losing an electron?

• Double negative

• Positive

• Neutral

• Negative

What is the charge on the carbonate ion after accepting electrons?

• 2+

• 1-

• 2-

• 3-

What is the overall charge of lithium carbonate?

• Negative

• Double positive

• Positive

• Neutral

What is a formula unit in the context of ionic compounds?

• A single atom

• A group of atoms bonded covalently

• The simplest ratio of ions in a compound

• A molecule with a net charge

How are formula units arranged in an ionic compound?

• Randomly scattered

• In a repeating pattern

• In pairs

• In a single line

What is the significance of a crystal structure in ionic compounds?

• It makes the compound soluble in water.

• It prevents the formation of ions.

• It provides a repeating pattern of formula units.

• It allows for covalent bonding.