Atomic Radius Comparisons and Trends

The video tutorial discusses the comparison of atomic sizes between magnesium (Mg) and sodium (Na). It explains that as you move down a group in the periodic table, atomic radius increases due to the addition of energy levels. Conversely, as you move across a period, atomic radius decreases due to increasing effective nuclear charge. The tutorial concludes that sodium has a larger atomic radius than magnesium because it is positioned to the left of magnesium in the same period, where atomic size decreases.

Which two elements are being compared for their atomic sizes in the video?

• Sodium and Chlorine

• Magnesium and Sodium

• Sodium and Potassium

• Magnesium and Calcium

What happens to the atomic radius as you move down a group in the periodic table?

• It decreases

• It remains the same

• It increases

• It fluctuates

Why does the atomic radius decrease as you move across a period?

• Due to the removal of electrons

• Due to adding more energy levels

• Due to increasing nuclear charge

• Due to decreasing nuclear charge

Which element has a larger atomic radius, sodium or magnesium?

• Sodium

• It depends on the isotope

• Magnesium

• Both have the same size

What is the main reason sodium is larger than magnesium?

• Sodium is to the left of magnesium in the period

• Sodium has fewer electrons

• Sodium is further down the group

• Sodium has more protons