# Emission and Absorption Spectra

## Trending Questions

**Q.**How many spectral line will be observed when an electron jumps from n = 5 to n = 1 in the visible line spectra of H spectrum?

- 10
- 3
- 6
- 8

**Q.**

Which of the following is the correct order of increasing field strength of ligands to form coordination compounds?

${\mathrm{CN}}^{-}<{\mathrm{C}}_{2}{\mathrm{O}}_{2}^{-4}<{\mathrm{SCN}}^{-}<{\mathrm{F}}^{-}$

${\mathrm{SCN}}^{-}<{\mathrm{F}}^{-}<{\mathrm{CN}}^{-}<{\mathrm{C}}_{2}{\mathrm{O}}_{2}^{-4}$

${\mathrm{F}}^{-}<{\mathrm{SCN}}^{-}<{\mathrm{C}}_{2}{\mathrm{O}}_{2}^{-4}<{\mathrm{CN}}^{-}$

${\mathrm{SCN}}^{-}<{\mathrm{F}}^{-}<{\mathrm{C}}_{2}{\mathrm{O}}_{2}^{-4}<{\mathrm{CN}}^{-}$

**Q.**The shortest and the longest wavelength in Balmer series of hydrogen spectrum are:

Rydberg constant, RH=109678 cm−1

- 911.7 oA and 1215.7 oA
- 3647 oA and 6565 oA
- 6565oA and 3647 oA
- 911.7 oA and 6565 oA

**Q.**

What will be the correct order for the wavelengths of absorption in the visible region for the following:

[Ni(NO_{2})_{6}]^{4−}, [Ni(NH_{3})_{6}]^{2+},
[Ni(H_{2}O)_{6}]^{2+}

**Q.**The shortest and the longest wavelength in Lyman series of hydrogen spectrum are:

Rydberg constant , RH=109678 cm−1

- 911.7 oA and 1215.7 oA
- 566.4 oA and 788.6 oA
- 1015.6 oA and 1438.8 oA
- 863.1 oA and 1215.7 oA

**Q.**

A body of mass $10mg$ is moving with a velocity of $100m{s}^{-1}$. The wavelength of the de-Broglie wave associated with it would be (Note:$h=6.63\times {10}^{-34}Js$)

**Q.**

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

**Q.**The number of possible lines of Paschen series when an electron jumps from the 7th excited state to the ground state in a hydrogen like atom is:

- 2
- 5
- 4
- 3

**Q.**The wavelength of Hα line of the Balmer series is 6500 oA. The wavelength of the Hβ line of Balmer series is:

- 4814.8 oA
- 1625.3 oA
- 6500.5 oA
- 5428.7 oA

**Q.**

The work function of sodium metal is $4.41\times {10}^{\u201319}J$. If photons of wavelength $300nm$ are incident on the metal, the kinetic energy of the ejected electrons will be ($h=6.63\times {10}^{\u201334}Js;c=3\times {10}^{8}\raisebox{1ex}{$m$}\!\left/ \!\raisebox{-1ex}{$s$}\right.$) __________ .

**Q.**For which of the species is Bohr's theory not applicable?

- Be3+
- Li2+
- He2+
- H

**Q.**In a sample of hydrogen atoms, transition of electrons take place from the 5th excited state to the ground state producing all possible types of photons. The number of lines in the infrared region is:

- 4
- 5
- 6
- 3

**Q.**Calculate the wavelength of the spectral line, when an electron in the hydrogen atom undergoes a transition from the energy level 4 to energy level 2.

RH=109678 cm−1

- 486 nm
- 386 nm
- 427 nm
- 554 nm

**Q.**Calculate the wavelength of radiation emitted when an electron falls from third excited state to ground state in the Lyman series of Hydrogen atom.

(RH=1.1×107m−1)

- λ=1.83×10−7m
- λ=0.97×107m
- λ=0.97×10−7m
- λ=1.83×10−8m

**Q.**How many spectral lines will be observed when an electron jumps from the 5th excited state to the ground state in the visible line spectra of H-spectrum?

- 4
- 5
- 3
- 6

**Q.**The spectral line of the shortest wavelength in Balmer series of atomic hydrogen will be:

- 6.215×10−5 cm
- 1.437×10−5 cm
- 5.942×10−5 cm
- 3.647×10−5 cm

**Q.**

Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen.

**Q.**

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

- n = 2 to n = 3
- n = 1 to n = 2
- n = 3 to n = 5
- n = 1 to n = 2

**Q.**What is the maximum wavelength line in the Lyman series for He+ ion?

- 3R
- 13R
- 44R
- None of these

**Q.**Find the maximum number of spectral lines in Balmer series when an electron returns from the 7th orbit to the 1st orbit in a sample of hydrogen atoms.

- 5
- 6
- 21
- 15

**Q.**The maximum kinetic energy of the photoelectrons ejected from a metal when it is irradiated with a radiation of frequency 2×1014s−1 is 6.63×10−20J. The thereshold frequency of the metal is:

- 2 ×10−14 s−1
- 1 ×1014 s−1
- 2×1014 s−1
- 3 ×1014 s−1

**Q.**Assume that 2×10−17 J of light energy is needed by the interior of the human eye to see an object. How many photons of yellow light with λ=595.2 nm are needed to generate this minimum energy?

- 6
- 30
- 45
- 60

**Q.**What is maximum wavelength of line of Balmer series of Hydrogen spectrum (RH = 1.1 × 107 m−1) :

- 400 nm
- 654 nm
- 486 nm
- 434 nm

**Q.**

Calculate the wavelength for the emission transition if it starts from the orbit having radius 1.3225 nm and ends at 211.6 pm. Name the series to which this transition belongs and the region of the spectrum.

**Q.**

When the electrons of a sample of hydrogen atoms jump from the 4th orbit to the ground state, the maximum number of spectral lines observed is:

- 15
- 6
- 3
- 4

**Q.**In a collection of H-atoms, all the electrons jump from n=5 to the ground level (directly or indirectly) without emitting any line in the Balmer series. The number of different possible radiations is:

- 10
- 8
- 7
- 6

**Q.**Calculate the wave number for the shortest wavelength transition in Brackett series for atomic hydrogen.

- 6.5×106 m−1
- 6.75×104 m−1
- 6.85×105 m−1
- 6.9×107 m−1

**Q.**An electron makes a transition from 7th excited state to 2nd energy level in a H-atom sample. Find the maximum spectral lines observed.

- 15
- 21
- 23
- 17

**Q.**An electron in an h atom in its ground state absorbs 1.5 times as much energy as the minimum required for its escape(13.6ev) from the atom .what is the wavelength of the emitted electron?

**Q.**

Which has maximum internal energy at 290K

(a) Neon gas (b) Nitrogen gas

(c) Ozone gas (d) Equal for all