If an electron has spin quantum number of +1/2 and a magnetic quantum number of -1, it cannot be represented in an
Options
(a) s-orbital (b) p-orbital (c) d-orbital (d) f-orbital
Correct Answer: […]
Which one of the following explains light both as stream of particle and as wave motion?
Options
(a) Diffraction (b) Interference (c) λ=h/p (d) Photoelectric effect
Correct Answer:
λ=h/p
Explanation:
λ= h/p = […]
In hydrogen spectrum, the different line of Lyman series are present in
Options
(a) UV field (b) IR field (c) visible field (d) for IR field
Correct Answer:
UV field
Explanation:
According to […]
Which of the following is never true for cathode rays?
Options
(a) They possess kinetic energy (b) They are electromagnetic waves (c) They produce heat (d) They produce mechanical pressure
Correct Answer:
They […]
The two electrons in K-subshell will differ in
Options
(a) principal quantum number (b) azimuthal quantum number (c) magnetic quantum number (d) spin quantum number
Correct Answer:
spin quantum number
Explanation:
The two […]
In the photo-electron emission,the energy of the emitted electron is
Options
(a) greater than the incident photon (b) same as than of the incident photon (c) smaller than the incident photon (d) proportional […]
If electron has spin quantum number +1/2 and magnetic quantum number -1, it cannot be present in
Options
(a) d-orbital (b) f-orbital (c) p-orbital (d) s-orbital
Correct Answer:
s-orbital
Explanation:
No explanation available. […]
If r is the radius of the first orbit, the radius of nth-orbit of H-atom is given by
Options
(a) rn² (b) rn (c) r/n (d) r² n²
Correct Answer:
rn²
Explanation:
Radius […]
What is the packet of energy called?
Options
(a) Electron (b) Photon (c) Positron (d) Proton
Correct Answer:
photon
Explanation:
According to Planck’s quantum theory of radiation, radient energy is emitted or absorbed […]
In a given atom no two electrons can have the same values for all the four quantum numbers.This is called
Options
(a) Hund’s Rule (b) Aufbau principle (c) Uncertainty principle (d) Pauli’s Exclusion […]
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