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The order of basic character of given oxides is:
(a) According to their metallic character which decreases from Na to Cu.
higher the metallic character, higher the basic nature of their oxide.
the lightest metal in the periodic table is:
Mass no. of metal increases along the period and down the group also.
Which electronic configurations represent to a transition element?
The differentiating electron enters in d-sub-shell.
Low melting point of manganese in the 1st transition series is due to:
(b) Due to d5 configuration, metallic bonds are weak. d5 orbital is half filled as a result of that 3d electrons are more tightly held by the nucleus and this reduces the de-localization of electrons resulting in weaker metallic bonding.
Most common oxidation state of cerium (Ce) is :
E.C of Ce is [Xe]4f15d16s2,
The common stable oxidation state of all the lanthanides is +3. The oxidation states of +2 and +4 are also exhibited and these oxidation states are only stable in those cases where stable 4f0, 4f7 or 4f14 configurations are achieved. Ce4+ is stable due to 4f0 configuration.
Which of the electronic configuration of an atom has the lowest ionization enthalpy?
I.E is inversly proportional to size ..
and valance electron should be lesser.
A common trend to both groups I and II elements in the periodic table, as the atomic number increases are:
Atomic radii increases down the group.
The difference between ions and atoms is of:
The basic differences in an ion and its atom
On going down a main subgroup in the periodic table (example Li to Cs in IA or Be to Ba in IIA) the expected trend of change in atomic radius is a :
(b) Atomic radii increase down the group
An element R forms the highest oxide R2O5. R belongs to:
(b) R has five valency electrons like N.
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