Multiple Choice
What is the electron configuration of the transition metal zirconium (Zr) in the compound ZrCl3?
553
views
24. Transition Metals and Coordination Compounds
Electron Configurations of Transition Metals
Multiple Choice
Which of the following is true about the atomic size of transition metals?
A
The atomic radius decreases from left to right as the number of protons increases.
B
The atomic radius remains relatively constant because electrons are added to an (n − 1) orbital.
C
The atomic radius increases from left to right as electrons are added to an outer orbital.
D
The atomic radius decreases from left to right as Zeff increases.
Verified step by step guidance1
Understand the concept of atomic radius: Atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons. It generally decreases across a period due to increasing nuclear charge.
Identify the role of transition metals: Transition metals are elements found in the d-block of the periodic table, where electrons are added to the (n-1)d subshell.
Analyze the effect of electron addition in transition metals: As electrons are added to the (n-1)d orbital, the increase in nuclear charge is somewhat offset by electron-electron repulsions within the d subshell, leading to a relatively constant atomic radius.
Consider the effective nuclear charge (Zeff): The effective nuclear charge is the net positive charge experienced by valence electrons. In transition metals, Zeff increases, but the added electrons in the (n-1)d orbital provide some shielding, maintaining a relatively constant atomic size.
Conclude the trend for transition metals: Unlike main group elements, the atomic radius of transition metals remains relatively constant across a period because the added electrons enter the (n-1)d orbital, which does not significantly increase the atomic size.
Related Videos
Related Practice
