Exploring Average Atomic Mass Concepts

The video tutorial covers isotopes and how to calculate the average atomic mass of elements. It explains isotopes as atoms of the same element with different masses due to varying numbers of neutrons. The tutorial details the calculation of average atomic mass using relative abundance and isotopic mass, with examples using nitrogen and chlorine isotopes. It emphasizes the importance of using parentheses in calculations and rounding significant figures at the end.

What distinguishes isotopes of the same element from each other?

• Number of atoms

• Number of neutrons

• Number of electrons

• Number of protons

Where can you find the average atomic mass of an element on the periodic table?

• On the left side of each square

• In the middle of each square

• At the bottom of each square

• At the top of each square

What is the unit used for atomic mass?

• Atomic Mass Unit (amu)

• Kilograms

• Milligrams

• Grams

Which isotope of nitrogen is more abundant in nature?

• Nitrogen-13

• Nitrogen-15

• Nitrogen-12

• Nitrogen-14

What is the first step in calculating the average atomic mass of an element?

• Add the masses of all isotopes

• Multiply the relative abundance by the mass of each isotope

• Divide the total mass by the number of isotopes

• Subtract the mass of the least abundant isotope

Why is it important to use parentheses when entering calculations into a calculator?

• To simplify the calculation

• To avoid using decimals

• To ensure the correct order of operations

• To make the calculation look neat

What should you do if the mass of an isotope is not given in a problem?

• Use the atomic number

• Use the number of electrons

• Use the mass number

• Use the number of protons

What is the final step in calculating the average atomic mass?

• Round to the nearest whole number

• Add the products of the relative abundances and masses

• Subtract the smallest mass from the largest mass

• Divide by the number of isotopes

What is the average atomic mass of chlorine if chlorine-35 has an abundance of 74.8% and chlorine-37 has an abundance of 25.2%?

• 35.5 amu

• 36.0 amu

• 35.0 amu

• 37.0 amu

Why might the calculated average atomic mass not be as close to the more abundant isotope when using mass numbers?

• Because mass numbers are not exact

• Because mass numbers are always rounded

• Because mass numbers are not used in calculations

• Because mass numbers do not account for electrons