Which of the following statements correctly describes the trend in atomic radius across a period in the periodic table?

Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements.

Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium. Predict the relative densities of these two metals. Look up the densities in a reference book, periodic table, or on the Internet to check if your predictions are correct.

Which of the following correctly arranges the atoms and ions in order of increasing atomic radius: Se, Se2-, Te2-?

Which atom in each group has the smallest atomic radius? Na, Si, Cl; Be, Mg, Ca?

Which of the following elements has the smallest atomic radius?

Which of the following elements has a larger atomic radius than sulfur (S)?

Which of the following is an observed trend in atomic radii across the periodic table?

Which factor would be most likely to decrease the atomic radius of an atom?