In the periodic table, with the increase in atomic number, the metallic character of an element
decrease in a period and increases in a group
increases in a period and decreases in a group
increases in a period as well as in the group
decreases in a period and also in the group
The ions are isoelectronic. Their ionic radii show
an increases from O2- to F- and then decrease from Na+ to Al3+
a decrease from O2- to F- and then increase from Na+ to Al3+
a significant increase from O2- to Al3+
a significant decrease from O2- to Al3+
One of the characteristic properties of non-metals is that they
are reducing agents
form basic oxides
form cations by electron gain
are electronegative
With which of the following electronic configuration an atom has the lowest ionisation enthalpy ?
1s2 ,2s2 2p5
1s2 ,2s2 2p3
1s2 ,2s2 2p5 3s1
1s2 ,2s2 2p6
The electronic configuration of Cu (atomic number 29) is
1s2,2s2,2p6,3s2,3p6, 4s2,3s9
1s2,2s2,2p6,3s2,3p6, 3d10,4s1
1s2,2s2,2p6,3s2,3p6, 4s2,4p6, 5s2,5p1
1s2,2s2,2p6,3s2,3p6, 4s2,4p6, 3d3
The horizontal columns in a periodic table are known as
group
period
class
block
Amongst the elements with following electronic configuration, which one may have the highest ionisation energy ?
Which one of the following arrangements does not truly represent the property indicated against it ?
Br2 < Cl2 < F2 : Oxidising power
The electronic configuration of four elements are given below. Which element does not belong to the same family as others ?
[Xe] 4f14 ,5d10 ,6s2
[Kr] 4d10 ,5s2
[Ne] 3s2 ,3p5
[Ar] 3d10 ,4s2
Ionic radii are
inversely proportional to effective nuclear charge
inversely proportional to square of effective nuclear charge
directly proportional to effective nuclear charge
directly proportional to square of effective nuclear charge
