Unit 1: Isotopes

Front

What is an isotope?

Back

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses.

Front

How do you calculate the number of neutrons in an isotope?

Back

To find the number of neutrons, subtract the atomic number (number of protons) from the mass number (total number of protons and neutrons).

Front

What is the mass number of an isotope?

Back

The mass number is the total number of protons and neutrons in the nucleus of an atom.

Front

What is the average atomic mass?

Back

The average atomic mass is the weighted average of the masses of an element's isotopes, taking into account their relative abundances.

Front

How do you find the average atomic mass of an element with two isotopes?

Back

Multiply the mass of each isotope by its relative abundance (as a decimal), then sum the results.

Front

What is the significance of isotopes in chemistry?

Back

Isotopes are important for understanding chemical reactions, dating materials, and in medical applications.

Front

What is the atomic number of an element?

Back

The atomic number is the number of protons in the nucleus of an atom, which determines the element's identity.

Front

How many neutrons are in Carbon-14?

Back

Carbon-14 has 8 neutrons (14 - 6 protons = 8 neutrons).

Front

What is the most abundant isotope of lead?

Back

The most abundant isotope of lead is lead-207.

Front

What is the formula to calculate the average atomic mass of an element with multiple isotopes?

Back

Average Atomic Mass = (mass1 * abundance1) + (mass2 * abundance2) + ...