Chromium Isotopes and Atomic Structure

This video tutorial explains how to determine the number of protons, neutrons, and electrons in chromium isotopes using the periodic table. It covers the atomic number, which equals the number of protons, and explains that in neutral elements, the number of protons equals the number of electrons. The video also discusses how to calculate the number of neutrons using the mass number, which is the sum of protons and neutrons. It highlights the most common isotope, chromium-52, and explains how to use the average atomic mass to estimate the mass number when not given specific values.

What is the first step in finding the protons, neutrons, and electrons for chromium?

• Measure the isotope

• Count the electrons

• Look at the periodic table

• Check the atomic mass

What does the atomic number of an element represent?

• The mass number

• The number of neutrons

• The number of protons

• The number of electrons

What is the relationship between protons and electrons in a neutral atom?

• Protons are double the electrons

• Protons equal electrons

• Electrons are double the protons

• Protons are half the electrons

How do you determine the number of neutrons in an isotope?

• Subtract the atomic number from the mass number

• Divide the mass number by the atomic number

• Add the atomic number to the mass number

• Multiply the atomic number by the mass number

How many neutrons does chromium 50 have?

• 28

• 24

• 30

• 26

Which isotope of chromium is the most common?

• Chromium 50

• Chromium 52

• Chromium 56

• Chromium 54

What percentage of chromium atoms are chromium 52?

• 50%

• 60%

• 84%

• 90%

What is the mass number of chromium 54?

• 54

• 50

• 52

• 56

If not given, how can you estimate the mass number of an element?

• Count the protons and electrons

• Round the average atomic mass to the nearest whole number

• Use the atomic number

• Use the number of neutrons

What is the significance of the average atomic mass?

• It is an average of all isotopes based on abundance

• It is the mass of the most common isotope

• It represents the heaviest isotope

• It is the lightest isotope