Atomic Radius and Periodic Trends

The video tutorial compares the atomic radii of aluminum (Al) and magnesium (Mg) using the periodic table. It explains that atomic radius increases down a group due to added energy levels and decreases across a period due to increased nuclear charge. The tutorial concludes that magnesium has a larger atomic radius than aluminum.

What is the main question being addressed in the video?

• What is the atomic number of aluminum?

• What is the electron configuration of aluminum?

• Which element has a larger atomic radius, aluminum or magnesium?

• How many protons does magnesium have?

Where are aluminum and magnesium located on the periodic table?

• Next to each other

• In the same group

• In the noble gases section

• In the transition metals section

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

• It increases

• It fluctuates

• It decreases

• It remains the same

How does the atomic radius change as you move across a period from left to right?

• It doubles

• It remains constant

• It decreases

• It increases

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

• Because of the loss of electrons

• Because of the addition of energy levels

• Due to the increase in effective nuclear charge

• Due to the decrease in atomic mass

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

• Magnesium

• It cannot be determined

• Aluminum

• Both have the same atomic radius

What is the reason for magnesium having a larger atomic radius than aluminum?

• Magnesium is heavier

• Magnesium has fewer protons

• Magnesium has a lower effective nuclear charge

• Magnesium is a noble gas