nt. Element with electronic configuration 1s2 is placed in (1) s-block (2) p-block (3) Group 3 (4) d-blockn

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Helium's subshell electron configuration is 1s². But why helium not included on S Block elements?

M^{3 +}

ion has its electronic configuration as

[A r] 3 d^{10} 4 s^{2}

. The element lies in:

Q. The general electronic configuration of d-block elements is
[ Noble gas]

(n - 1) d^{1 - 10} n s^{1 - 2}

(i) Comprehension given below is followed by some multiple choice questions. Each question has one correct option. Choose the correct option. In the modern periodic table, elements are arranged in order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz s, p, d, and f.
The modern periodic table consists of 7 periods and 18 groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle, the seven periods (1 to 7 ) have 2, 8, 8, 18, 18, 32, and 32 elements respectively.
The seventh period is still incomplete. To avoid the periodic table being too long , the two series of f-block elements, called lanthanoids and actionoids are placed at the bottom of the main body of hte periodic table
The element with atomic number 57 belongs to
(a) s- block ( b) p-block (c) d- block (d) f- block

(ii) The last element of the p - block in 6th period is represented by the outermost electronic configuration.
(a) $7 s^{2} 7 p^{6}$ (b) $5 f^{14} 6 d^{10} 7 s^{2} 7 p^{0}$
(c) $4 f^{14} 5 d^{10} 6 s^{2} 6 p^{6}$ (d) $4 f^{14} 5 d^{10} 6 s^{2} 6 p^{4}$

(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?
(a) 107 (b) 118 (c) 126 (d) 102

(iv) The electronic configuration of the element which is just above the element with atomic number 43 in the same group is .....
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{2}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{3} 4 p^{6}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{6} 4 s^{2}$
(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{7} 4 s^{2}$

(v) The elements with atomic numbers 35, 53 and 85 are all ..
(a) noble gases (b) halogens (c) heavy metals (d) light metals

Q. The group of the element with electronic configurations:

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{2}

is 2. If true enter 1, else enter 0.

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