Exploring Isotopes and Average Atomic Mass

The video tutorial covers isotopes, atomic structure, and average atomic mass. It explains the differences between isotopes, their role in determining atomic mass, and their real-world applications like carbon dating. The tutorial also demonstrates how to calculate average atomic mass using isotopes and their abundance.

Which subatomic particles are located in the nucleus of an atom?

• Protons and electrons

• Neutrons and electrons

• Protons and neutrons

• Electrons only

What defines the atomic number of an element?

• Number of protons

• Number of neutrons

• Number of electrons

• Sum of protons and neutrons

How do isotopes of the same element differ?

• Number of protons

• Number of electrons

• Number of neutrons

• Atomic number

What is the mass number of an isotope?

• Sum of protons and neutrons

• Number of neutrons

• Number of electrons

• Number of protons

Why are isotopes important in carbon dating?

• They are used to measure temperature

• They change the atomic number

• They decay at a specific rate

• They have different numbers of electrons

What does the average atomic mass on the periodic table represent?

• Mass of the heaviest isotope

• Average mass of all isotopes

• Sum of all isotopes' masses

• Mass of the most common isotope

Which two numbers are needed to calculate the average atomic mass?

• Atomic number and mass number

• Isotope mass and abundance

• Number of protons and neutrons

• Number of electrons and protons

How should percentages be converted for calculations in average atomic mass?

• Into fractions

• Into whole numbers

• Into ratios

• Into decimals

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

• Adding the isotopes' masses

• Multiplying isotope mass by its abundance

• Dividing the total mass by the number of isotopes

• Subtracting the atomic number from the mass number

What unit is used for average atomic mass?

• Moles

• Atomic mass units (amu)

• Kilograms

• Grams