8.13 Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
8.13 Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
-
1 Answer
-
8.13 The oxidation states displayed by the first half of the first row of transition metals are given in the table below.
METALS
Sc ( [Ar] 3d14s2)
Ti ( [Ar]
3d24s2)
V ( [Ar] 3d34s2 )
Cr ( [Ar] 3d54s1)
Mn ( [Ar] 3d54s2)
OXIDATION STATES
+2
+2
+2
+2
+3
+3
+3
+3
+3
+4
+4
+4
+4
+5
+5
+6
+6
+7
Except for Sc, all others metals display +2 oxidation state. This is because as the atomic number increases, the number of electrons in the valence shell increases. +2 oxidation state is attained by the loss of the two 4s electrons by these metals. As the number of electron increases, the possibility of an ion with +2 oxidation state being stable (by attaining half-filled structure) also increases. Finally, Mn2+ ions have half-filled structure and are very stable.
Similar Questions for you
K2Cr2O7 + H2O2 + H2SO4->
Oxidation state of chromium = +6.
Potassium permanganate in alkaline medium oxidise lodide to lodate.
Compound A is
KMnO4 decomposes upon heating at 513 K and forms K2MnO4 and MnO2.
2KMnO4
The colour changes due to change in pH not due to its reaction with water.
Taking an Exam? Selecting a College?
Get authentic answers from experts, students and alumni that you won't find anywhere else
Sign Up on ShikshaOn Shiksha, get access to
- 65k Colleges
- 1.2k Exams
- 688k Reviews
- 1800k Answers