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Bohr's Model of Atom

Which of the ...

Question

Which of the following electron transitions will require the largest amount of energy in a hydrogen atom?

A

From

n = 1

to

n = 2

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B

From

n = 2

to

n = 3

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C

From

n = \infty

to

n = 1

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D

From

n = 3

to

n = 5

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Solution

The correct option is A From $n = 1$ to $n = 2$

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Similar questions

Q. Radiation coming from transitions

n = 2

n = 1

of hydrogen atoms fall on

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Q. Consider the following two electronic transition possibilities in a hydrogen atom as pictured below:
(a) The electron drops from third Bohr orbit to second Bohr orbit followed with the next transition from second to first Bohr orbit.
(b) The electron drops from third Bohr orbit to first Bohr orbit directly. Show that the sum of energies for the transitions

n = 3

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n = 2

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is equal to the energy of transition for

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.

Q. Consider the following two electronic transition possibilities in hydrogen atom as:

(1)

The electron drops from third Bohr's orbit to second Bohr's orbit followed with the next transition from second to first Bohr's orbit.

(2)

The electron drops from third Bohr's orbit to first Bohr's orbit directly.
Then the statement :
"The sum of the energies for the transitions

n = 3

n = 2

n = 2

n = 1

= the energy of transition for

n = 3

n = 1

1

if true, else enter

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Q. In which of the following transitions will the wavelength be minimum?

(a) n = 5 to n = 4
(b) n = 4 to n = 3
(c) n = 3 to n = 2
(d) n = 2 to n = 1

Q. Electron transition in

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n_{2}

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2 n_{2} + 3 n_{1} = 18

2 n_{2} - 3 n_{1} = 6

What will be the total number of photons emitted when electrons transit to

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