Answer:
(a) (i) Cu,
because the electronic configuration of Cu is .
So, second electron needs to be removed from completely filled d-orbital which
is very difficult.
(ii) Zinc, because
of electronic configuration of and Zn2'1'
= which is fully filled and hence is
very stable. Removal of third electron requires very high energy.
(iii) Zinc,
because of it has completely filled 3d subshell and no unpaired electron is available
for metallic bonding.
(b) (i)
Carbonyl is
According to
EAN rule, the effective number of a metal in a metal carbonyl is equal to the
atomic number of nearest inert gas EAN is calculated as
EAN =number
of electrons in metal +2 x (CO)
=atomic
number of nearest inert gas
In = x + 2 x (5) = 36 (Kr is the
nearest inert gas)
x = 26
(atomic number of metal)
So, the
metal is Fe (iron).
(ii)
In
Let us
assume that oxidation state of M is x
X + 3 x (-2)
+ (-1) = 0
Or, x = + 7 i.e., M
is in +7 oxidation state of +7. Hence, the given compound is .
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