Isotopes-unit 1 review playlist

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 calculate the average atomic mass of an element with multiple isotopes?

Back

To calculate the average atomic mass, multiply the mass of each isotope by its relative abundance (as a decimal), then sum these values.

Front

What is the significance of the number of neutrons in an isotope?

Back

The number of neutrons determines the isotope's mass and can affect the stability of the nucleus.

Front

If an isotope has 29 protons and 34 neutrons, what is its mass number?

Back

The mass number is the sum of protons and neutrons, so 29 + 34 = 63.

Front

What is the average atomic mass of an element with isotopes of 4 amu (30%), 5 amu (20%), and 3 amu (50%)?

Back

The average atomic mass is approximately 4 amu.

Front

Which isotope of calcium is most abundant if the isotopes have masses of 35.00 amu, 41.00 amu, and 40.00 amu?

Back

The most abundant isotope is 40.00 amu.

Front

How do you express the abundance of an isotope as a percentage?

Back

To express abundance as a percentage, divide the number of atoms of the isotope by the total number of atoms and multiply by 100.

Front

What is the average mass of an element with isotopes of 75.23 amu (24.1%), 74.61 amu (48.7%), and 75.20 amu (27.2%)?

Back

The average mass is 74.92 amu.

Front

What is the notation for isotopes?

Back

Isotopes are often denoted by the element's name followed by the mass number, e.g., Copper-63.

Front

How does the presence of isotopes affect the atomic mass of an element on the periodic table?

Back

The atomic mass listed on the periodic table is a weighted average of all the isotopes of that element.