Isotopic mass

The video tutorial explains isotopes, which are variants of elements with different numbers of neutrons, leading to different relative atomic masses. It highlights that the atomic mass numbers in the periodic table are weighted averages of isotopic masses. Using copper as an example, the video illustrates how its relative atomic mass is calculated based on its two main isotopes, copper 63 and copper 65.

What distinguishes isotopes of the same element from each other?

• Different chemical properties

• Different numbers of protons

• Different numbers of electrons

• Different numbers of neutrons

How is the atomic mass number on the periodic table determined?

• By adding the number of protons and electrons

• By calculating a weighted average of isotopic masses

• By taking the mass of the most common isotope

• By averaging the atomic numbers

Why is copper's relative atomic mass not a whole number?

• It is rounded for simplicity

• It includes the mass of electrons

• It is a theoretical value

• It is an average of its isotopes' masses

Which of the following isotopes is more abundant in copper?

• Copper-63

• Copper-64

• Copper-65

• Copper-66

What is the relative atomic mass of copper as given in the periodic table?

• 64.000

• 65.000

• 63.546

• 63.000