Match the following laws with their correct statements:
Laws Statements $(1)$ Hund's Rule $(A)$ No two electrons in an atom can have the same set of all four quantum numbers. $(2)$ Aufbau Principle $(B)$ Half-filled and fully-filled orbitals have greater stability. $(3)$ Pauli Exclusion Principle $(C)$ Electrons prefer to remain unpaired in degenerate orbitals first. $(4)$ Heisenberg's Uncertainty Principle $(D)$ It is impossible to determine simultaneously the exact position and exact momentum of an electron. $(E)$ In the ground state of atoms,orbitals are filled in the order of increasing energy.
| Laws | Statements |
|---|---|
| $(1)$ Hund's Rule | $(A)$ No two electrons in an atom can have the same set of all four quantum numbers. |
| $(2)$ Aufbau Principle | $(B)$ Half-filled and fully-filled orbitals have greater stability. |
| $(3)$ Pauli Exclusion Principle | $(C)$ Electrons prefer to remain unpaired in degenerate orbitals first. |
| $(4)$ Heisenberg's Uncertainty Principle | $(D)$ It is impossible to determine simultaneously the exact position and exact momentum of an electron. |
| $(E)$ In the ground state of atoms,orbitals are filled in the order of increasing energy. |
(C) The correct matching is: $(1-C, 2-E, 3-A, 4-D)$.
$(1)$ Hund's Rule states that in degenerate orbitals,electrons prefer to remain unpaired with parallel spins as much as possible.
$(2)$ Aufbau Principle states that in the ground state of atoms,electrons fill orbitals in the order of increasing energy.
$(3)$ Pauli Exclusion Principle states that no two electrons in an atom can have the same set of all four quantum numbers.
$(4)$ Heisenberg's Uncertainty Principle states that it is impossible to determine simultaneously the exact position and exact momentum of a microscopic particle like an electron.
$(1)$ Hund's Rule states that in degenerate orbitals,electrons prefer to remain unpaired with parallel spins as much as possible.
$(2)$ Aufbau Principle states that in the ground state of atoms,electrons fill orbitals in the order of increasing energy.
$(3)$ Pauli Exclusion Principle states that no two electrons in an atom can have the same set of all four quantum numbers.
$(4)$ Heisenberg's Uncertainty Principle states that it is impossible to determine simultaneously the exact position and exact momentum of a microscopic particle like an electron.
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Similar Questions
For the given electronic transitions,which of the following statements is correct?
Medium
View SolutionMatch the items in Column-$A$ with the items in Column-$B$.
Column-$A$ Column-$B$ $(1)$ Dalton $(A)$ Photoelectric effect $(2)$ Maxwell $(B)$ Wave theory $(3)$ Huygens $(C)$ Atomic theory $(D)$ Electromagnetic radiation
| Column-$A$ | Column-$B$ |
| $(1)$ Dalton | $(A)$ Photoelectric effect |
| $(2)$ Maxwell | $(B)$ Wave theory |
| $(3)$ Huygens | $(C)$ Atomic theory |
| $(D)$ Electromagnetic radiation |
Easy
View SolutionGiven below are two statements:
Statement $I$: Rutherford's gold foil experiment cannot explain the line spectrum of hydrogen atom.
Statement $II$: Bohr's model of hydrogen atom contradicts Heisenberg's uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:
Statement $I$: Rutherford's gold foil experiment cannot explain the line spectrum of hydrogen atom.
Statement $II$: Bohr's model of hydrogen atom contradicts Heisenberg's uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:
Consider the following:
$I$. The electron spin quantum number describes the orientation of the spin of the nucleus with respect to the magnetic field.
$II$. The orbitals represented by the quantum numbers $n=3, l=2, m=+2$ and $n=3, l=2, m=-2$ have the same energy.
$III$. The energy of a photon is directly proportional to wavelength but inversely proportional to wave number.
$IV$. Lyman series of lines appear in ultra-violet region.
The correct statements are:
$I$. The electron spin quantum number describes the orientation of the spin of the nucleus with respect to the magnetic field.
$II$. The orbitals represented by the quantum numbers $n=3, l=2, m=+2$ and $n=3, l=2, m=-2$ have the same energy.
$III$. The energy of a photon is directly proportional to wavelength but inversely proportional to wave number.
$IV$. Lyman series of lines appear in ultra-violet region.
The correct statements are:
Which one of the following about an electron occupying the $1s$ orbital in a hydrogen atom is incorrect? (Bohr's radius is represented by $a_0$)
DifficultJEE MAIN 2025
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