# How do you find the percent abundance of copper isotopes?

Category:
science
chemistry

**Copper**has two

**isotopes**:

**Cu**-63 (

**abundance**= 69.2%, mass = 62.930 amu) and

**Cu**-65 (

**abundance**= 30.8%, mass = 64.928 amu). Calculate the (average) atomic mass of

**copper**. 3. Three magnesium

**isotopes**have atomic masses and

**relative abundances**of 23.985 amu (78.99%), 24.986 amu (10.00%), and 25.982 (11.01%).

People also ask, how do you find the percent abundance of copper?

When it comes to the actual calculation, it's easier to use decimal **abundances**, which are simply **percent abundances** divided by 100 . So, you know that **copper** has two naturally occurring isotopes, **copper**-63 and **copper**-65. This means that their respective decimal **abundance** must add up to give 1 .

**calculate**the

**average atomic mass**, multiply the fraction by the

**mass**number for each

**isotope**, then add them together. Whenever we do

**mass**calculations involving elements or compounds (combinations of elements), we always use

**average atomic masses**.

Also to know is, how do you calculate the atomic mass of relative abundance of an isotope?

Change each percent **abundance** into decimal form by dividing by 100. Multiply this value by the **atomic mass** of that **isotope**. Add together for each **isotope** to get the average **atomic mass**.

The relative **abundance of an isotope** is the **percentage** of atoms with a specific atomic mass found in a naturally occurring sample of an element.