Final answer:
Elements at the right end of the p-block are smaller in size and have a higher ionization energy compared to those at the left end, and they form stronger covalent bonds.
Step-by-step explanation:
Compared with the elements at the left end of the p-block element group, the elements at the right end:
- b. Are smaller in size
- c. Have higher ionization energy
- d. Form stronger, not weaker, covalent bonds
The atomic radius generally decreases across a period because the effective nuclear charge experienced by the electrons increases, pulling the electrons closer to the nucleus. As such, the elements at the right end of the p-block are smaller in size compared to those at the left. This effective nuclear charge also contributes to a higher ionization energy for the elements at the right end as it becomes more difficult to remove an electron from an atom. Contrary to option 'd', these elements actually form stronger covalent bonds due to increased electronegativity and the possession of more tightly held valence electrons.