d and f BLOCK ELEMENTS

What is the primary reason for the increase in ionization enthalpy across a period (from left to right)?

• Decrease in atomic radius.
• Increase in effective nuclear charge.
• Decrease in electron shielding.
• Increase in the number of electron shells.

Why do elements in the same group of the periodic table have similar chemical properties?

• They have the same atomic mass.
• They have the same number of electron shells.
• They have the same number of valence electrons.
• They are all metals.

Which of the following statements correctly describes the relationship between atomic size and ionization enthalpy?

• Generally, as atomic size decreases, ionization enthalpy decreases.
• Generally, as atomic size decreases, ionization enthalpy increases.
• There is no relationship between atomic size and ionization enthalpy.
• Ionization enthalpy depends only on nuclear charge.

An element has the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹. In which block and group of the periodic table would you place this element?

• s-block, Group 1
• s-block, Group 2
• p-block, Group 1
• d-block, Group 1

Which of the following best describes the trend in metallic character as you move down a group in the periodic table?

• Metallic character decreases.
• Metallic character remains constant.
• Metallic character increases.
• Metallic character first increases then decreases.