Final answer:
To find the elements linked to the given average atomic masses, we convert the masses from grams to amu and compare with the periodic table. The elements corresponding to the atomic masses of 30.98 amu and 14.01 amu are Phosphorus (P) and Nitrogen (N), respectively.
Step-by-step explanation:
To identify the elements with atoms that have an average mass of 5.143 x 10-23 g and 2.326 x 10-23 g, we need to convert these masses from grams to atomic mass units (amu), since the periodic table lists the average atomic mass in amu.
One atomic mass unit (1 amu) is equal to 1.66 x 10-24 g. Therefore, we can calculate the atomic mass in amu by dividing the given mass by the mass of 1 amu:
- For the average mass of 5.143 x 10-23 g:
- 5.143 x 10-23 g ÷ 1.66 x 10-24 g/amu = 30.98 amu
- For the average mass of 2.326 x 10-23 g:
- 2.326 x 10-23 g ÷ 1.66 x 10-24 g/amu = 14.01 amu
By looking up these atomic mass values on the periodic table:
- The element with an atomic mass of approximately 30.98 amu is Phosphorus (P).
- The element with an atomic mass of approximately 14.01 amu is Nitrogen (N).