2.1 Isotope and % abundance practice questions

Front

What is an isotope?

Back

An isotope is a variant of a chemical element that has the same number of protons but a different number of neutrons, resulting in a different atomic mass.

Front

How do you determine the percent abundance of an isotope?

Back

Percent abundance can be calculated using the formula: (mass of isotope / average atomic mass) x 100.

Front

What is the significance of isotopes in chemistry?

Back

Isotopes are important for understanding atomic structure, nuclear reactions, and applications in medicine and dating techniques.

Front

What does the notation 'Carbon-14' signify?

Back

'Carbon-14' indicates a carbon isotope with 6 protons and 8 neutrons, giving it an atomic mass of 14.

Front

How many protons and neutrons are in Hydrogen-3?

Back

Hydrogen-3 has 1 proton and 2 neutrons.

Front

What is the average atomic mass of an element?

Back

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

Front

If an element has two isotopes, how do you find the more abundant one?

Back

The more abundant isotope will typically have a mass closer to the average atomic mass of the element.

Front

What is the atomic mass of Chromium?

Back

The atomic mass of Chromium is approximately 52.996 amu.

Front

What is the relationship between protons, neutrons, and atomic mass?

Back

The atomic mass of an atom is approximately equal to the sum of its protons and neutrons.

Front

What is the percent abundance of an isotope if it is equal to another isotope?

Back

If two isotopes are equal in abundance, each will have a percent abundance of 50%.