13 Questions
Which element shows six different oxidation states due to its 5 unpaired d electrons?
Manganese
What happens when transition elements lose one 4s electron?
Formation of M ion
What trend is observed in the atomic radii of the elements of the transition series from left to right?
Decrease gradually
What happens as the number of unpaired electrons in 3d orbitals increases?
The number of oxidation states shown by the element also increases
Why do d electrons offer smaller screening effect compared to other electrons?
$n-1$d subshell is less penetrating or more diffused
What happens to the oxidation states of transition elements as the number of unpaired electrons in 3d orbitals increases?
The number of oxidation states shown by the element also increases
What happens to the atomic radii of transition elements as we move across a transition series from left to right?
The atomic radii decrease gradually
Which element in the first transition series shows oxidation states from -2 to +7?
Manganese
What happens when a transition element loses two 4s electrons?
$M^{2+}$ ion is formed
Why do d electrons offer smaller screening effect compared to other electrons?
D orbitals in an atom are less penetrating or more diffused
Match the following oxidation states with their corresponding electron loss:
Loss of one 4s electron = M² ion Loss of two 4s electrons = M^{3^{+}} ion Loss of unpaired 3d and 4s electrons = M ion
Match the following elements with the number of oxidation states they show:
Scandium = Only one unpaired electron Manganese = -2 to +7 oxidation states
Match the following trends with the atomic radii of d block elements:
Atomic radii decrease gradually from left to right = Trend in atomic radii Nuclear charge increases from left to right = Trend in atomic radii D orbitals offer smaller screening effect = Trend in atomic radii D electrons enter a penultimate (n-1)d subshell = Trend in atomic radii
Learn about the great variety of oxidation states displayed by transition elements in their compounds, as well as the progressive loss of 4s and 3d electrons leading to the formation of ions.
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