Understanding Mercury Isotopes and Atomic Structure

This video tutorial explains how to determine the protons, neutrons, electrons, and mass number for mercury isotopes. It covers the atomic number, which remains constant at 80 for all isotopes, and explains that in a neutral element, the number of protons equals the number of electrons. The video also demonstrates how to calculate the mass number and the number of neutrons for different isotopes of mercury using hyphen notation. Finally, it discusses the concept of average atomic mass based on the abundance of naturally occurring isotopes.

What is the atomic number of mercury?

• 82

• 81

• 80

• 79

How many protons does mercury have?

• 81

• 79

• 80

• 78

In a neutral atom of mercury, how many electrons are present?

• 78

• 79

• 80

• 81

What does the mass number of an isotope represent?

• Only the number of protons

• Only the number of neutrons

• The sum of protons and neutrons

• The sum of electrons and neutrons

If an isotope of mercury is represented as mercury-199, what is its mass number?

• 198

• 199

• 200

• 201

How many neutrons are in mercury-199?

• 120

• 119

• 118

• 121

For mercury-200, how many neutrons are present?

• 119

• 120

• 122

• 121

What is the neutron count for mercury-202?

• 123

• 120

• 121

• 122

How can you find the mass number if not given directly?

• By adding protons and electrons

• By subtracting electrons from protons

• By rounding the atomic number

• By rounding the atomic mass from the periodic table

What does averaging the isotopes of mercury based on abundance provide?

• The number of neutrons

• The average atomic mass

• The atomic number

• The mass number