The outer electronic configuration of some elements are:
$(a) 3 s^{2} 3 p^{4}$
$(b) 3 d^{10} 4 s^{2}$
$(c) 3 s^{2} 3 p^{6} 4 s^{2}$
$(d) 6 s^{2} 4 f^{3}$
State to which block of elements in the periodic table each of these belongs?

p, d, p, s

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p, d, s, f

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s, d, p, s

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p, p, f, s

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Solution

The correct option is B $p, d, s, f$
The general outer electronic configuration of s block elements is $n s^{(1 - 2)}$ .

The general outer electronic configuration of p block elements is $n s^{2} n p^{(1 - 6)}$ .

The general outer electronic configuration of d block elements is $(n - 1) d (^{1 - 10)} n s^{(0 - 2)}$ .

The general outer electronic configuration of f− block elements is $(n - 2) f^{(0 - 14)} (n - 1) d^{(0 - 1)} n s^{2}$ .

$A = 3 s^{2} 3 p^{4}$ belongs to $p$ block as last electron enters in $p$ subshell.
$B = 3 d^{10} 4 s^{2}$ belongs to $d$ block as last electron enters in $d$ subshell.
$C = 3 s^{2} 3 p^{6} 4 s^{2}$ belongs to $s$ block as last electron enters in $s$ subshell.
$D = 6 s^{2} 4 f^{3}$ belongs to $f$ block as last electron enters in $f$ subshell.

Option B is correct.

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(ii) The last element of the p - block in 6th period is represented by the outermost electronic configuration.
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(iii) Which of the elements whose atomic numbers are given below, cannot be accommodated in the present set up of the long frm of the periodic table?
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(iv) The electronic configuration of the element which is just above the element with atomic number 43 in the same group is .....
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(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{3} 4 p^{6}$
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(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{7} 4 s^{2}$

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B, P, S

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The outer electronic configuration of some elements are:(a) 3s23p4(b) 3d104s2(c) 3s23p64s2(d) 6s24f3State to which block of elements in the periodic table each of these belongs?

The outer electronic configuration of some elements are:
$(a) 3 s^{2} 3 p^{4}$
$(b) 3 d^{10} 4 s^{2}$
$(c) 3 s^{2} 3 p^{6} 4 s^{2}$
$(d) 6 s^{2} 4 f^{3}$
State to which block of elements in the periodic table each of these belongs?