Consider two electronic configuration of $K$ (Potassium)
(I) $K = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$
(II) $K = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{1}$
Find the effective nuclear charge experienced by the last electron in (I) and (II).

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Solution

Effective nuclear change $z e f f = z - 5$
$z =$ Atomic number $5 =$ shielding electron
$(i) z e f f = z - 5$
$= 19 - 18 = 1 +$
$(i i) z e f f = 2 - 5$
$= 19 - 10 = 9 +$

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Similar questions

Q. Calculate the effective nuclear charge of the last electron in an atom whose configuration is

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}

Q. Due to inter electronic repulsion, an electron experiences less nuclear charge. It is, therefore, said that inner electronic shells electrons shield the nucleus. The actual nuclear charge experienced by an electron is called effective nuclear charge. If the electrons in K-shell shields the nucleus to the extent of 0.5 (say) each. What will be the wave number of the spectral line arising out of n=4 to n = 2 transition in He atom?

Q. Two electronic configuration of an element 'A' are given below.
(Symbols not real)

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

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

(a) Identify the correct electronic configuration.
(b) Write the period in which the element is present in the periodic table.
(c) Consider another element 'C' with sub-shell configuration

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

. In which among the atoms A and C, the attraction of the nucleus towards the outermost electron is more? Give reason.

Q. Arrange

s, p

and

d

sub-shells of a shell in the increasing order to effective nuclear charge

(Z_{e f f})

experienced by the electron present in them.

Question 22

Arrange s, p and d subshells of a shell in the increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electron present in them.

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Consider two electronic configuration of K (Potassium)(I) K=1s22s22p63s23p64s1(II) K=1s22s22p63s23p63d1Find the effective nuclear charge experienced by the last electron in (I) and (II).

Effective nuclear change zeff=z−5z= Atomic number 5= shielding electron(i)zeff=z−5=19−18=1+(ii)zeff=2−5=19−10=9+

Consider two electronic configuration of $K$ (Potassium)
(I) $K = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$
(II) $K = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{1}$
Find the effective nuclear charge experienced by the last electron in (I) and (II).

Effective nuclear change $z e f f = z - 5$
$z =$ Atomic number $5 =$ shielding electron
$(i) z e f f = z - 5$
$= 19 - 18 = 1 +$
$(i i) z e f f = 2 - 5$
$= 19 - 10 = 9 +$