Fluorine has low electron affinity than chlorine because of
Bigger radius of fluorine, less density
Smaller radius of chlorine, high density
Smaller radius of fluorine, high density
Smaller radius of chlorine, less density
Electron affinity depends on
Atomic size
Nuclear charge
Atomic number
Both atomic size and nuclear charge
If 'x' denotes the number of valence electrons of an element, its valency equals
X
x-8
8-x
either (a) or (c)
Al3+has lower ionic radius than Mg2+ because
Al3+ has higher nuclear charge than Mg2+
Mg has less number of neutrons than Al
Al has lower ionization potential than Mg atom
Their electro negativities are different
The element which has greatest difference between first and second ionization energy is
Na
Mg
Si
P
The element forming an acidic oxide is
C
Ca
Zn
On the basis of group valencies the formula of the compound formed between tin and fluorine is
SnF3
SnF4
SnF6
SnF
The electronic configuration of d- block elements is
(n-1) d1-10 ns2p4
(n-1) s2n d1-10
(n-1) d 1-10 ns2
(n-1) p4ns2
The incorrect statement among the following is
The ionisation potential of 'Be' is greater than that of 'B'.
The electro negativity of 'F' is greater than that of 'Cl'.
The ionisation potential of 'N' is greater than that of 'O'.
The electron affinity of 'F' is greater than that of 'Cl'
Number of liquid elements present in the periodic table is
2
3
14
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