The maximum number of emission lines obtained when the excited electron of the H atom jumps from n = 6 to the ground state is -

1. 30

2. 21

3. 15

4. 28

Subtopic:  Hydrogen Spectra |
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The ionization energy for H atom in the ground state is 2.18 x 10-18 J. The process energy requirements will be: \(( He^+(g) \rightarrow He^{2+}(g) + e^- )\)
1. 8.72 x 10-18 J
2. 7.54 x 10-18 J
3. 5.67 x 10-17 J
4. 2.18 x 10-17 J

Subtopic:  Hydrogen Spectra |
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The wavelength of light emitted when the electron in a H atom undergoes the transition from an energy level with n = 4 to an energy level with n = 2, is 

1. 586 mm

2. 486 nm

3. 523 nm

4. 416 pm

Subtopic:  Hydrogen Spectra |
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The energy associated with the fifth orbit of a hydrogen atom is 

1. -2.18 × 10-18 J2. -8.72 × 10-20 J3. -3.88 × 10-21 J4. -8.72 × 10-19 J

Subtopic:  Hydrogen Spectra |
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The wave number for the longest wavelength transition in the Balmer series of atomic hydrogen would be -

1. 1.52 × 106 m-12. 3.14 × 106 cm-13. 15.2 × 106 m-14. 1.52 × 106 cm-1

Subtopic:  Hydrogen Spectra |
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The energy of an electron in H - atom is given by En = (2.18 × 10-18 )n2 J.  The shortest wavelength of light that can be used to remove an electron completely from n = 2 orbit will be

1. 3647 A°2. 5132 A°3. 3017 A°4. None of these

Subtopic:  Hydrogen Spectra |
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Emission transitions in the Paschen series end at orbit n = 3 and start from orbit n and can be represented as v = 3.29 × 1015 (Hz)132- 1n2The value of n if the transition is observed at 1285 nm is
1. 6
2. 5
3. 8
4. 9

Subtopic:  Hydrogen Spectra |
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The transition in the hydrogen spectrum that would have the same wavelength as Balmer transition from n = 4 to n = 2 of He+ spectrum is -

1. n1 = 3 to n2 = 4

2. n2  = 3 to n1 = 2

3. n2  = 3 to n1 = 1

4. n2  = 2 to n1 = 1

Subtopic:  Hydrogen Spectra |
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