Lithium Nitrate and Ionic Compounds

The video tutorial explains how to write the Lewis structure for lithium nitrate (LiNO3). It begins by introducing the components of LiNO3, highlighting lithium as a metal and nitrate as a polyatomic ion. The tutorial details the ionic bonding process, where lithium loses a valence electron to the nitrate ion, resulting in a positive lithium ion and a negative nitrate ion. The video further illustrates the electron transfer process and the resulting charges. It concludes by showing the final Lewis structure for LiNO3 and explaining the concept of formula units in a crystal lattice.

What are the components of lithium nitrate?

• Lithium and nitrate

• Lithium and hydrogen

• Lithium and nitrogen

• Lithium and oxygen

Why is lithium nitrate considered ionic?

• Because nitrate loses electrons to lithium

• Because lithium loses electrons to nitrate

• Because lithium gains electrons from nitrate

• Because lithium shares electrons with nitrate

What happens to lithium when it loses its valence electron?

• It becomes positively charged

• It becomes negatively charged

• It becomes a nonmetal

• It remains neutral

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

• It loses electrons to nitrate

• It gains electrons from nitrate

• It shares electrons with nitrate

• It remains unchanged

What is the charge of the nitrate ion after gaining an electron?

• Neutral

• Double negative

• Positive

• Negative

Why are brackets used in the Lewis structure of the nitrate ion?

• To indicate it is a molecule

• To show it is an ion

• To separate it from lithium

• To highlight its valence electrons

What is a formula unit in the context of lithium nitrate?

• A single molecule of lithium nitrate

• A repeating unit in a crystal lattice

• A pair of lithium and nitrate ions

• A single lithium ion

How are formula units arranged in a crystal of lithium nitrate?

• Randomly scattered

• In a linear pattern

• In a regularly repeating pattern

• In a circular pattern