Iron(II) Nitrate and Nitrate Ions

The video tutorial explains how to write the chemical formula for iron(II) nitrate. It begins by identifying iron and nitrate, noting that nitrate is a polyatomic ion with a one-minus charge. The tutorial then discusses the ionic charges of iron and nitrate, emphasizing the need for a neutral compound. The crisscross method is introduced to balance the charges, resulting in the formula Fe(NO3)2. The video concludes by verifying the formula and ensuring the charges add up to zero.

What is the chemical symbol for iron as found on the periodic table?

• I

• Ir

• In

• Fe

Which of the following is a polyatomic ion not found on the periodic table?

• Chloride

• Nitrate

• Sulfide

• Oxide

What is the charge of the nitrate ion?

• 2+

• 1+

• 2-

• 1-

Why is it important for the charges in an ionic compound to add up to zero?

• To make the compound reactive

• To ensure the compound is stable

• To ensure the compound is neutral

• To make the compound colorful

What method is used to balance the charges in the formula for iron(II) nitrate?

• Substitution method

• Cross-multiplication method

• Crisscross method

• Addition method

In the crisscross method, what happens to the charges of the ions?

• They are added together

• They are ignored

• They are subtracted

• They are swapped and used as subscripts

How many nitrate ions are needed to balance the charge of one iron(II) ion?

• One

• Two

• Three

• Four

What is the final formula for iron(II) nitrate?

• FeNO3

• Fe(NO3)2

• Fe2(NO3)3

• Fe(NO3)3

What is the total charge of two nitrate ions?

• 1-

• 1+

• 2-

• 2+

What is the significance of the Roman numeral in iron(II) nitrate?

• It indicates the number of nitrate ions

• It shows the charge of the iron ion

• It represents the atomic number of iron

• It denotes the mass of the compound