Question

explain how the four isotopes of chromium, atomic number 24, differ from one another, and then calculate the average atomic mass of chromium using its isotopic composition shown in the table. chromium isotope data

Explanation:

Step1: Convert percentage to decimal

For Cr - 50: \(4.35\%=0.0435\), for Cr - 52: \(83.79\% = 0.8379\), for Cr - 53: \(9.50\%=0.095\), for Cr - 54: \(2.36\%=0.0236\)

Step2: Calculate weighted - mass for each isotope

For Cr - 50: \(0.0435\times49.946 = 2.172651\)
For Cr - 52: \(0.8379\times51.941=43.5926439\)
For Cr - 53: \(0.095\times52.941 = 5.029395\)
For Cr - 54: \(0.0236\times53.939=1.2729604\)

Step3: Sum up the weighted - masses

\(2.172651+43.5926439 + 5.029395+1.2729604=52.0676503\approx52.07\)

Answer:

The four isotopes of chromium (atomic number \(Z = 24\)) have the same number of protons (\(Z = 24\)) but different numbers of neutrons. The average atomic mass of chromium is approximately \(52.07\) amu.