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2 cards from this section. Quick, good the night before a test.
What is electron configuration?
Think about how many electrons fit in different orbitals.
What is the general configuration for first-row transition metals?
Consider the noble gas that precedes these metals in the periodic table.
What is the general electron configuration of first-row transition metals?
Remember, transition metals are defined by their d shell configuration.
True or False: Electrons in the 4s sublevel are always lost before those in the 3d sublevel.
Think about the order of filling and energy levels.
Given the electron configurations of various transition metals, categorize them based on predicted oxidation states and explain how these states relate to their electron configurations.
Look for the stability in half-filled or fully filled conditions.
Calculate the energy levels of electrons as they fill in transition metals and explain how this affects their reactions with ligands in coordination complexes.
Consider how ligand type affects the energy of d orbitals.
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