According to the text, why does the simple rule for determining valence electrons from the group number not apply to transition metals?
1 point
Transition metals have a complex electron configuration that cannot be easily predicted.
Transition metals have variable valencies, meaning they can have different numbers of valence electrons.
Transition metals are not part of the periodic table.
Transition metals do not participate in chemical reactions.
Answer (1)
Answer:The correct answer is: Transition metals have a complex electron configuration that cannot be easily predicted. Here's why: - The Simple Rule: For main group elements, the number of valence electrons generally matches the group number on the periodic table. This is because their valence electrons are located in the s and p orbitals of the outermost shell.- Transition Metals: Transition metals have their valence electrons in the d orbitals, which are located in the second-to-last shell. This means their electron configurations are more complex and don't follow the simple pattern of main group elements. Why the other options are incorrect: - Transition metals have variable valencies: While true, this is a consequence of their complex electron configurations, not the reason why the simple rule doesn't apply.- Transition metals are not part of the periodic table: This is incorrect. Transition metals occupy the central block of the periodic table.- Transition metals do not participate in chemical reactions: This is also incorrect. Transition metals are known for their diverse and often catalytic roles in chemical reactions. In summary: The simple rule for determining valence electrons from the group number doesn't work for transition metals because their electron configurations are more complex due to the involvement of d orbitals.
