Advertisements
Advertisements
Question
Silver atom has completely filled d orbitals (4d10) in its ground state. How can you say that it is a transition element?
Advertisements
Solution
Silver (Z = 47) can also show a +2 oxidation state, in which its 4d orbitals are incompletely filled; hence, it is a transition element.
APPEARS IN
RELATED QUESTIONS
Explain giving reasons:
Transition metals and many of their compounds show paramagnetic behaviour.
Write down the electronic configuration of Cr3+.
Write down the electronic configuration of Pm3+.
Write down the electronic configuration of Cu+.
Write down the electronic configuration of Ce4+.
Write down the electronic configuration of Lu2+.
Write down the electronic configuration of Th4+.
Account for the following:
Mn2+ is more stable than Fe2+ towards oxidation to +3 state.
Which transition metal of 3d series has positive E° (M2+/M) value and why?
Out of Cr3+ and Mn3+, which is a stronger oxidising agent and why?
Which among the following is not considered as a part of transition elements?
The electronic configuration of \[\ce{Cu(II)}\] is 3d9 whereas that of \[\ce{Cu(I)}\] is 3d10. Which of the following is correct?
Which of the following compounds is expected to be colored?
The element with electronic configuration [xe]544f145d16S2 belongs to
Name the element of 3d series which exhibits the largest number of oxidation states. Give reason.
Give reason for the following statements:
Scandium (Z = 21) is a transition element but Zn (Z = 30) is not.
Define transition metals.
Assertion (A) : Copper is a non-transition element.
Reason (R) : Copper has completely filled d-orbitals in its ground state.
Match the properties with the elements of 3d series:
| (i) | lowest enthalpy of atomisation | (p) | Sc |
| (ii) | shows maximum number of oxidation states | (q) | Mn |
| (iii) | transition metal that does not form coloured compounds |
(r) | Zn |
| (s) | Ti |
