Which of the following properties generally decreases across a period from left to right, but shows an anomalous increase at Group 15 elements compared to Group 14 and 16 elements?
Ionization enthalpy
Atomic radius
Electronegativity
Electron gain enthalpy
Related Questions
An element X belongs to group 14 and period 3 of the periodic table. What is the number of valence electrons in X?
2
4
6
8
An element 'X' has the highest third ionization enthalpy in the 3d series. Which of the following is most likely to be 'X'?
Cr
Mn
Fe
Cu
Oxygen is divalent, but sulphur exhibits variable valency of , because:
Sulphur is less electronegative than oxygen
Sulphur is bigger atom than oxygen
Ionisation potential of sulphur is more than oxygen
Of the presence of -orbitals in sulphur
Oxygen is divalent, but sulphur exhibits variable valency of , because:
Sulphur is less electronegative than oxygen
Sulphur is bigger atom than oxygen
Ionisation potential of sulphur is more than oxygen
Of the presence of -orbitals in sulphur
Which element in the fourth period exhibits the lowest second ionization enthalpy?
Potassium (K)
Calcium (Ca)
Gallium (Ga)
Krypton (Kr)
Among the correct order of increasing atomic radii is:
An element has the electronic configuration [Ar] 4s 3d 4p. In which block and group of the periodic table is this element located?
s-block, Group 2
d-block, Group 10
p-block, Group 15
f-block, Group 3
An element has E.C. predict their period, group and block
period = 3, block = p, group = 15
period = 5, block = s, group = 1
period = 3, block = p, group = 10
period = 4, block = d, group = 12
Elements of group 1 and group VI in the periodic table have one thing common. That is with the increasing atomic number, the:
Maximum valency increases
Reactivity increases
Atomic radius increases
Oxidizing power increases
