Ionic Compounds and Iron Chemistry

The video tutorial explains how to write the chemical formula for Iron(II) Hydroxide. It begins by identifying the elements involved: iron (Fe) and hydroxide (OH-), a polyatomic ion. The tutorial discusses the ionic nature of the compound and the importance of charge balancing to achieve a neutral compound. The crisscross method is introduced to determine the correct subscripts for the formula, resulting in Fe(OH)2. The video concludes with a verification of the formula to ensure the net charge is zero.

What is the element symbol for iron?

• I

• Ir

• In

• Fe

Which of the following is a polyatomic ion?

• Fe

• OH-

• O2

• H2

What charge does iron have in iron(II) hydroxide?

• 0

• 3+

• 2+

• 1+

Why is it important to balance charges in ionic compounds?

• To make them colorful

• To ensure they are neutral

• To increase their weight

• To make them dissolve in water

What method is used to determine the subscripts in the formula for iron(II) hydroxide?

• Addition method

• Crisscross method

• Substitution method

• Balancing method

Why are parentheses used around hydroxide in the formula for iron(II) hydroxide?

• To indicate it is a metal

• To show it is a polyatomic ion

• To highlight its color

• To denote its charge

What is the net charge of iron(II) hydroxide?

• 1-

• 2+

• 3-

• 0

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

• FeOH

• Fe(OH)2

• Fe2OH

• FeO2H