The nuclear charge can be defined as the net positive charge that acts on an electron in the orbital of an atom that has more than 1 electrons. It is inversely proportional to the distance between the orbital and the nucleus.
(i) Electrons that reside in the 2s orbital are closer to the nucleus than those residing in the 3s orbital and will, therefore, experience greater nuclear charge.
(ii) 4d orbital is closer to the nucleus than 4f orbital and will, therefore, experience greater nuclear charge.
(iii) 3p will experience greater nuclear charge (since it is closer to the nucleus than the 3f orbital).
Answered by Pragya Singh | 1 year agoAnswer the following questions:-
(a) How many sub-shells are associated with n = 4?
(b) How many electrons will be present in the sub-shells having ms value of \(- \dfrac{1}{2}\) for n = 4?
Indicate the number of unpaired electrons in:
(a) P
(b) Si
(c) Cr
(d) Fe
(e) Kr
The unpaired electrons in Al and Si are present in 3p orbital. Which electrons will experience more effective nuclear charge from the nucleus?
The bromine atom possesses 35 electrons. It contains 6 electrons in 2p orbital, 6 electrons in 3p orbital and 5 electrons in 4p orbital. Which of these electron experiences the lowest effective nuclear charge?
The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists:
1. n = 4, l = 2, \( m_l\) = –2 , ms = \( -\dfrac{1}{2}\)
2. n = 3, l = 2, \( m_l\)= 1 , ms = \( +\dfrac{1}{2}\)
3. n = 4, l = 1, \( m_l\) = 0 , ms = \( +\dfrac{1}{2}\)
4. n = 3, l = 2, \( m_l\)= –2 , ms = \( -\dfrac{1}{2}\)
5. n = 3, l = 1, \( m_l\) = –1 , ms= \( +\dfrac{1}{2}\)
6. n = 4, l = 1, \( m_l\) = 0 , ms = \( +\dfrac{1}{2}\)