Advertisements
Advertisements
Question
Account for the following:
In case of transition elements, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number.
Advertisements
Solution
In case of transition elements, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number. As the new electron enters a d orbital each time the nuclear charge increases by unity. The shielding effect of a d electron is not that effective, hence the net electrostatic attraction between the nuclear charge and the outermost electron increases and the ionic radius decreases.
APPEARS IN
RELATED QUESTIONS
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Which element has the highest m.p?
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Which element is a strong oxidising agent in +3 oxidation state and why?
Which of the 3d series of the transition metals exhibits the largest number of oxidation states and why?
The \[\ce{E^{\circ}_{(M^{2+}/M)}}\] value for copper is positive (+0.34 V). What is possible reason for this? (Hint: consider its high ΔaH° and low ΔhydH°)
Give reasons for the following:
The transition metals generally form coloured compounds.
In lake test for Al3+ ions, there is the formation of coloured ‘floating lake’. It is due to ______.
Electronic configuration of a transition element X in +3 oxidation state is [Ar]3d5. What is its atomic number?
A solution of \[\ce{KMnO4}\] on reduction yields either a colourless solution or a brown precipitate or a green solution depending on pH of the solution. What different stages of the reduction do these represent and how are they carried out?
Answer the following question:
Which element of the first transition series has highest third ionisation enthalpy?
Explain the magnetic properties of d-block (or transition) elements.
