Calculating Atomic Mass and Compounds

Miss Stover introduces the mole concept, focusing on counting atoms in chemical formulas. She explains how to determine the number of atoms in compounds like ammonium phosphate and sodium chlorate. The lesson progresses to calculating the formula mass of compounds using atomic masses from the periodic table. Students are guided through example calculations to reinforce their understanding of these concepts.

What is the primary focus of the mole concept lecture?

• Understanding chemical reactions

• Counting atoms in chemical formulas

• Learning about isotopes

• Balancing chemical equations

In the compound Al2(SO4)3, how many sulfur atoms are present?

• Three

• Two

• Four

• Six

How many total atoms are in the compound Zn(HCO3)2?

• Nine

• Eleven

• Thirteen

• Fifteen

What is the first step in calculating the mass of a compound?

• Finding the number of molecules

• Identifying the chemical formula

• Using the periodic table to find atomic masses

• Balancing the chemical equation

What is the atomic mass of carbon used in the calculation of CO2's formula mass?

• 16.00

• 14.01

• 18.02

• 12.01

How many oxygen atoms are in a molecule of CO2?

• One

• Two

• Four

• Three

What is the formula mass of carbon dioxide?

• 32.00 AMU

• 48.00 AMU

• 28.01 AMU

• 44.01 AMU

How many nitrogen atoms are in the compound (NH4)3PO4?

• Four

• One

• Two

• Three

What is the atomic mass of hydrogen used in the ammonium phosphate calculation?

• 1.010

• 1.009

• 1.008

• 1.007

What is the total formula mass of ammonium phosphate?

• 149.18 AMU

• 150.00 AMU

• 149.09 AMU

• 151.01 AMU