Atomic Radius Trends and Comparisons

The video tutorial explains how to determine which of the two atoms, magnesium (Mg) or phosphorus (P), has a larger atomic radius. By examining the periodic table, it is shown that atomic radii decrease across a period. Since Mg and P are in the same period, phosphorus is smaller, making magnesium the larger atom. The tutorial concludes with Dr. B confirming that magnesium has a larger atomic radius than phosphorus.

What is the main question being addressed in the video?

• How many electrons does phosphorus have?

• What is the atomic mass of magnesium?

• What is the melting point of magnesium?

• Which atom has a larger atomic radius, magnesium or phosphorus?

What is the general trend of atomic radii as you move across a period in the periodic table?

• Atomic radii decrease

• Atomic radii fluctuate randomly

• Atomic radii increase

• Atomic radii remain constant

Why is magnesium larger than phosphorus in terms of atomic radius?

• Phosphorus has more electrons

• Phosphorus is a non-metal

• Magnesium is located to the left of phosphorus in the same period

• Magnesium has more protons

Which element is found to the right of magnesium in the same period?

• Aluminum

• Sodium

• Sulfur

• Phosphorus

What conclusion is drawn about the atomic radius of magnesium compared to phosphorus?

• Magnesium is smaller than phosphorus

• Magnesium is larger than phosphorus

• Magnesium and phosphorus have the same atomic radius

• Phosphorus is larger than magnesium

What is the significance of the periodic table trends in determining atomic size?

• They help predict chemical reactivity

• They allow comparison of atomic sizes across periods

• They determine the color of elements

• They are used to calculate atomic mass