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
Identify the correct statements from the following:
$A$. Heisenberg uncertainty principle is applicable to electrons.
$B$. The size of $2p_x$ orbital is less than the size of $3p_x$ orbital.
$C$. The energy of $2s$ orbital of $H$ atom is equal to the energy of $2s$ orbital of $Li$.
$D$. The electronic configuration of $Cr$ is $[Ar]3d^5 4s^1$.
$A$. Heisenberg uncertainty principle is applicable to electrons.
$B$. The size of $2p_x$ orbital is less than the size of $3p_x$ orbital.
$C$. The energy of $2s$ orbital of $H$ atom is equal to the energy of $2s$ orbital of $Li$.
$D$. The electronic configuration of $Cr$ is $[Ar]3d^5 4s^1$.
Among the following,the correct statement$(s)$ for electrons in an atom is(are):
$A$. Uncertainty principle rules out the existence of definite paths for electrons.
$B$. The energy of an electron in $2s$ orbital of an atom is lower than the energy of an electron that is infinitely far away from the nucleus.
$C$. According to Bohr's model,the most negative energy value for an electron is given by $n=1$,which corresponds to the most stable orbit.
$D$. According to Bohr's model,the magnitude of velocity of electrons increases with increase in values of $n$.
$A$. Uncertainty principle rules out the existence of definite paths for electrons.
$B$. The energy of an electron in $2s$ orbital of an atom is lower than the energy of an electron that is infinitely far away from the nucleus.
$C$. According to Bohr's model,the most negative energy value for an electron is given by $n=1$,which corresponds to the most stable orbit.
$D$. According to Bohr's model,the magnitude of velocity of electrons increases with increase in values of $n$.
MediumIIT 2024
View SolutionWhich of the following graphs is correct for the kinetic energy $(K.E.)$ of an electron in the $n^{th}$ orbit of a hydrogen-like atom?
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 SolutionWhich 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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