(D) For the first orbit of a monopositive $He^{+}$ ion,the atomic number $Z = 2$ and the orbit number $n = 1$.The energy of an electron in the $n^{th}

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(D) For the first orbit of a monopositive $He^{+}$ ion,the atomic number $Z = 2$ and the orbit number $n = 1$.The energy of an electron in the $n^{th}$ orbit is given by the formula:$E_n = -2.18 \times 10^{-18} \left( \frac{Z^2}{n^2} \right) \ J$Substituting the values $Z = 2$ and $n = 1$:$E_1 = -2.18 \times 10^{-18} \left( \frac{2^2}{1^2} \right) \ J$$E_1 = -2.18 \times 10^{-18} \times 4 \ J$$E_1 = -8.72 \times 10^{-18} \ J$

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

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What is the amount of energy associated with the first orbit of a monopositive helium ion? $[R_{H} = 2.18 \times 10^{-18} \ J]$

MHT CET 2024 All MHT CET

A
$-1.9 \times 10^{-18} \ J$
B
$-4.36 \times 10^{-18} \ J$
C
$-6.54 \times 10^{-18} \ J$
D
$-8.72 \times 10^{-18} \ J$

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Structure of Atom

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Atomic models and Planck's quantum theory

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What is the amount of energy associated with the first orbit of a monopositive helium ion? $[R_{H} = 2.18 \times 10^{-18} \ J]$

Similar Questions

For a $H$ atom,the energy transition from $n = 1$ to $n = 2$ is $10.2 \ eV$. What will be the energy for the same transition in $Be^{3+}$ ion?

For a $H$ atom,the wavelength for the highest energy transition is $91.2 \ nm$. Calculate the corresponding wavelength for $He^{+}$ in $nm$.

If the wavelength of an electromagnetic radiation is $2000 \ \text{Å}$, what is its energy in ergs?

What is the ratio of the wave number of the first line (lowest energy line) of the Balmer series of the $H$ atomic spectrum to the first line of its Brackett series?

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