Chemistry > d and f Block Elements > 3.0 General Trends in properties of First Row Elements
d and f Block Elements
1.0 General Introduction and Electronic Configuration
2.0 Occurrence and General Characteristics of Transition Elements
3.0 General Trends in properties of First Row Elements
3.1 Ionisation Enthalpy
3.2 Oxidation State
3.3 Atomic and Ionic Radii
3.4 Colour
3.5 Catalytic properties
3.6 Magnetic Properties
3.7 Formation of Interstitial Compounds
3.8 Alloy Formation
4.0 Potassium dichromate
5.0 Potassium permanganate
5.1 Properties of potassium permanganate
5.2 Structure of manganate ion and permanganate ion
5.3 Disproportion of an oxidation state
5.4 Uses
6.0 F-Block Elements - Introduction
7.0 Lanthanoid Series
7.1 Position of Lanthanoid Series
7.2 Electronic configuration of lanthanoids
7.3 Oxidation States
7.4 Chemical Reactivity of Lanthanides
8.0 Lanthanoid Contraction and its consequence
9.0 Actinoids Series
9.1 Position of Actinoids in periodic table
9.2 Electronic Configuration of actinoids
9.3 Oxidation states of actinoids
10.0 Comparison between lanthanoids and actinoids
3.3 Atomic and Ionic Radii
3.2 Oxidation State
3.3 Atomic and Ionic Radii
3.4 Colour
3.5 Catalytic properties
3.6 Magnetic Properties
3.7 Formation of Interstitial Compounds
3.8 Alloy Formation
5.2 Structure of manganate ion and permanganate ion
5.3 Disproportion of an oxidation state
5.4 Uses
7.2 Electronic configuration of lanthanoids
7.3 Oxidation States
7.4 Chemical Reactivity of Lanthanides
9.2 Electronic Configuration of actinoids
9.3 Oxidation states of actinoids
- In $3d$ Series atomic radii decreases from $Sc$ to $Cr$ then they are constant upto copper and then increases.
- Due to addition of electrons in penultimate $d$-subshell effective nuclear charge increases and atomic radii are constant.
- Increase in nuclear charge and screening effect balance each other and atomic radii are constant.
- At the end of series number of paired electrons in d-orbital increases the repulsive interaction between them and leads to the expansion of atoms.
- Ionic Radii decreases with increase in the oxidation state.
- A particular oxidation state of their ionic radii decreases with increase in nuclear charge in a given transition series.
- The ionic radii of $+2$ oxidation state decreases from $T{i^{ + 2}}$ to $C{a^{ + 2}}$.
