Home
Class 10
CHEMISTRY
Explain Pauli's exclusion principle ....

Explain Pauli's exclusion principle .

Text Solution

Verified by Experts

According to Pauli's exclusion principle, no two electrons of the same atom can have all four quantum numbers the same.
Promotional Banner

Topper's Solved these Questions

  • STRUCTURE OF ATOM

    VGS PUBLICATION-BRILLIANT|Exercise CREATIVE QUESTIONS FOR NEW MODEL EXAMINATION ( SECTION - III 2 MARKS QUESTIONS )|38 Videos

  • STRUCTURE OF ATOM

    VGS PUBLICATION-BRILLIANT|Exercise CREATIVE QUESTIONS FOR NEW MODEL EXAMINATION ( SECTION - IV 4 MARKS )|32 Videos

  • STRUCTURE OF ATOM

    VGS PUBLICATION-BRILLIANT|Exercise CREATIVE QUESTIONS FOR NEW MODEL EXAMINATION ( SECTION - I 1/2 MARK QUESTIONS)|96 Videos

  • REFLECTION AND REFRACTION

    VGS PUBLICATION-BRILLIANT|Exercise EXERCISE|24 Videos

  • SUMMATIVE ASSESSMENT

    VGS PUBLICATION-BRILLIANT|Exercise SUMMATIVE ASSESSMENT|28 Videos

Similar Questions

Explore conceptually related problems

Explain Paulis exclusion principle .

Which of the following is violation of Pauli's exclusion principle ?

Electronic configuration of multielectron atoms can be written by the use of four quantum numbers and also by following certain principles. Pauli's exclusion principle suggests that maximum capacity of an atomic orbital is two. Auf bau principle suggests that the lower energy orbitals are filled first and hence stability can be attained. Hunds rule of maximum multiplicity suggests that pairing occurs with one electron. The arrangement of electrons in the space around the nucleus can be understood only after writing the electronic configuration. Thus writing electronic configuration is more important in the structure of an atom. Auf-bau principle is first violated for the element with atomic numbers

Electronic configuration of multielectron atoms can be written by the use of four quantum numbers and also by following certain principles. Pauli's exclusion principle suggests that maximum capacity of an atomic orbital is two. Auf bau principle suggests that the lower energy orbitals are filled first and hence stability can be attained. Hunds rule of maximum multiplicity suggests that pairing occurs with one electron. The arrangement of electrons in the space around the nucleus can be understood only after writing the electronic configuration. Thus writing electronic configuration is more important in the structure of an atom. Six unpaired electrons are present in the ground state electronic configuration of the element

Electronic configuration of multielectron atoms can be written by the use of four quantum numbers and also by following certain principles. Pauli's exclusion principle suggests that maximum capacity of an atomic orbital is two. Auf bau principle suggests that the lower energy orbitals are filled first and hence stability can be attained. Hunds rule of maximum multiplicity suggests that pairing occurs with one electron. The arrangement of electrons in the space around the nucleus can be understood only after writing the electronic configuration. Thus writing electronic configuration is more important in the structure of an atom. The set of quantum numbers not possible for electrons present in potassium atom in its ground state

The electrons in atoms occupy atomic orbitals (AO_(s)) that are represented as theregions around the nuclei where there is a high probability of finding the electrons. ln the so-called LCAO (linear combitaks) approach, as pioneered by Hund and Mulliken, when AOs come close together, they overlap forming MOs (molecular orbitals). Two AO s can overlap to form two MOs, one of which lies at a lower energy level (BMO) than the other at a higher energy level and is called an antibonding molecular orbital (ABMO). Each MO can hold one or two electrons in accordance with Pauli's exclusion principle. MOT can explain the paramagnetism of molecules such as O_(2) and NO and other spectral features. In a molecule number of electrons in bonding MO is more as compared to antibonding MO, hence

The electrons in atoms occupy atomic orbitals (AO_(s)) that are represented as theregions around the nuclei where there is a high probability of finding the electrons. ln the so-called LCAO (linear combitaks) approach, as pioneered by Hund and Mulliken, when AOs come close together, they overlap forming MOs (molecular orbitals). Two AO s can overlap to form two MOs, one of which lies at a lower energy level (BMO) than the other at a higher energy level and is called an antibonding molecular orbital (ABMO). Each MO can hold one or two electrons in accordance with Pauli's exclusion principle. MOT can explain the paramagnetism of molecules such as O_(2) and NO and other spectral features. Bond strength increases with

The maximum number of unpaired electrons which can exist in an orbital according to Pauli’s exclusion principle