Zinc and Nitrate Compounds

The video tutorial explains how to write the chemical formula for zinc nitrate. It begins by identifying zinc on the periodic table and recognizing nitrate as a polyatomic ion. The tutorial discusses the ionic nature of the compound, emphasizing the need to balance charges. Zinc, a transition metal, typically has a 2+ charge, while nitrate has a 1- charge. The crisscross method is used to balance these charges, resulting in the formula Zn(NO3)2. The tutorial concludes by verifying the formula to ensure a net charge of zero.

What is the chemical symbol for zinc?

• Z

• ZnO

• Zc

• Zn

Which of the following is a polyatomic ion?

• NO3-

• O2

• Zn

• H2O

What charge does the nitrate ion (NO3-) carry?

• 2+

• 1-

• 2-

• 1+

Why is zinc considered an exception among transition metals?

• It forms covalent bonds

• It is non-metallic

• It has a variable charge

• It is always 2+

What is the charge of zinc in zinc nitrate?

• 2+

• 0

• 1+

• 3+

What method is used to balance the charges in zinc nitrate?

• Cross-multiplication

• Balancing method

• Crisscross method

• Substitution method

Why do we use parentheses around the nitrate ion in the formula?

• To show it is a metal

• To highlight it is a liquid

• To denote it is a gas

• To indicate it is a polyatomic ion

How many nitrate ions are needed to balance the charge of one zinc ion?

• Two

• One

• Four

• Three

What is the final formula for zinc nitrate?

• Zn(NO3)2

• Zn2(NO3)

• Zn2(NO3)2

• Zn(NO3)

What is the net charge of zinc nitrate?

• 1+

• 0

• 3+

• 2-