(D) The energy of an orbital in a hydrogen-like atom is given by $E_n = -13.6 \times \frac{Z^2}{n^2} \text{ eV}$.As the principal quantum number $n$ i

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(D) The energy of an orbital in a hydrogen-like atom is given by $E_n = -13.6 \times \frac{Z^2}{n^2} \text{ eV}$.As the principal quantum number $n$ increases,the value of $E_n$ becomes less negative,meaning the total energy of the orbital increases.Therefore,the Assertion is incorrect.The Reason states that energy is required to move a negatively charged electron away from a positively charged nucleus,which is correct because work must be done against the electrostatic force of attraction.Thus,the Assertion is wrong,but the Reason is correct.The correct option is $(D)$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

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Choose the correct option regarding: Assertion: Energy of the orbital decreases with increase of $n$.
Reason: Energy is required in shifting away the negatively charged electron from the positively charged nucleus.

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A
Assertion and Reasoning are correct statements and Reason is the correct explanation for Assertion
B
Assertion and Reasoning are correct statements and Reason is not the explanation for Assertion
C
Assertion is correct,Reason is wrong
D
Assertion is wrong,Reason is correct

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Structure of Atom

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Atomic models and Planck's quantum theory

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The work function of sodium metal is $4.41 \times 10^{-19} \ J$. If photons of wavelength $300 \ nm$ are incident on the metal,the kinetic energy of the ejected electrons will be $\left( \dots \right) \times 10^{-21} \ J$. (Given: $h = 6.63 \times 10^{-34} \ J \cdot s; c = 3 \times 10^{8} \ m/s$)

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If the velocity of an electron in the $1^{st}$ orbit of the $H$ atom is $V$,then what will be the velocity in the $4^{th}$ orbit of $Be^{3+}$?

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What is the energy in joules,required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state?
The ground state electron energy is $-2.18 \times 10^{-11} \ erg$.

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Choose the correct option regarding: Assertion: Energy of the orbital decreases with increase of $n$.Reason: Energy is required in shifting away the negatively charged electron from the positively charged nucleus.

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Total number of spectral lines when an electron jumps from the $8^{th}$ orbit to the $2^{nd}$ orbit is:

In Rutherford's experiment,generally the thin foil of heavy atoms,like gold,platinum etc. have been used to be bombarded by the $\alpha$-particles. If the thin foil of light atoms like Aluminium etc. is used,what difference would be observed from the above results?

The work function of sodium metal is $4.41 \times 10^{-19} \ J$. If photons of wavelength $300 \ nm$ are incident on the metal,the kinetic energy of the ejected electrons will be $\left( \dots \right) \times 10^{-21} \ J$. (Given: $h = 6.63 \times 10^{-34} \ J \cdot s; c = 3 \times 10^{8} \ m/s$)

If the velocity of an electron in the $1^{st}$ orbit of the $H$ atom is $V$,then what will be the velocity in the $4^{th}$ orbit of $Be^{3+}$?

What is the energy in joules,required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state?The ground state electron energy is $-2.18 \times 10^{-11} \ erg$.

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Choose the correct option regarding: Assertion: Energy of the orbital decreases with increase of $n$.
Reason: Energy is required in shifting away the negatively charged electron from the positively charged nucleus.

What is the energy in joules,required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state?
The ground state electron energy is $-2.18 \times 10^{-11} \ erg$.