The bond distance of H-H bond is
1.44 Å
1.98 Å
0.74 Å
2.28 Å
The scale which is based on an empirical relation between the energy of a bond and the electro negativities of bonded atoms is
Pauling scale
Mulliken’s scale
Sanderson’s scale
Alfred and Rochow’s scale
On moving down the group, the radius of an ion
Decreases
Increases
No change
None of these
Electron affinity is expressed in
kJ
J
kJ mol
kJ mol-1
Among the following which has the maximum ionisation energy
Alkali elements
Alkaline elements
Halogens
Noble gases
When XA>>XB, A–B bond is
Covalent
Non-polar covalent
Ionic
Metallic
Across the period, electron affinity
decreases
increases
decrease and then increases
increase and then decreases
Electronegativity of an atom is
Directly proportional to its nuclear charge
directly proportional to its atomic radii
inversely proportional to its nuclear charge
independent
Effective nuclear charge (Z*) can be calculated using the formula
Z* = Z-S
Z* = Z + S
Z* = S – Z
Z = Z* – S
The electron affinity of an atom
is directly proportional to its size
is inversely proportional to its size
is independent of its size
none of these
