Structure Of Atom MCQ - 1 (Advance) - JEE MCQ

Select the correct statement(s) :

Choose the incorrect statement(s) :

Select the correct curve(s) :

If v = velocity of electron in Bohr's orbit.

r = Radius of electron in Bohr's orbit.

P.E. = Potential energy of electron in Bohr's orbit.

K.E. = Kinetic energy of electron in Bohr's orbit.

Which is/are correct statement.

It is a data sufficiency problem in which it is to be decided on the basis of given statements whether the given question can be answered or not. No matter whether the answer is yes or no.

Question : Is the orbital of hydrogen atom 3p_x?

Statement - 1 : The radial function of the orbital is R(r) =

Statement - 2 : The orbital has 1 radial node & 0 angular node.

Statement - 1 : Energy emitted when an electron jump from 5 → 2 (energy level) is less than when an electron jump from 2 → 1 in all `H' like atom.

Statement - 2 : The |total energy difference| between 1st & 2nd energy level is greater than that of any two energy level provided level `1' is not part of those two energy levels

Statement - 1 : Emitted radiations will fall in visible range when an electron jump from higher level to n = 2 in Li⁺² ion.

Statement - 2 : Balmer series radiations belong to visible range in all H - like atoms.

Assertion : The fraction of total number of electrons in p-sub levels of Mg is 50%

Reason : The fraction of total number of electron in p-sub levels of Be is 40%

Assertion : Energy of an electron is determined by its principal quantum number.

Reason : Principal quantum number is a measure of the most probable distance of finding the electrons around the nucleus.

Assertion : Cathode rays do not travel in straight lines.

Reason : Cathode rays can penetrate through a thick metal sheet.

Assertion : Energy of radiation is large if its wavelength is large.

Reason: Energy = hv (v = frequency, v = )

Match the column
Column - I and Column - II contain data on Schrondinger Wave - Mechanical model, where symbols have
their usual meanings. Match the columns.

Match the column

The French physicist Louis de-Broglie in 1924 postulated that matter, like radiation, should exhibit a dual behaviour. He proposed the following relationship between the wavelength λ of a material particle, its linear momentum p and planck constant h.

The de Broglie relation implies that the wavelength of a particle should decreases as its velocity increases. It also implies that for a given velocity heavier particles should have shorter wavelength than lighter particles. The waves associated with particles in motion are called matter waves or de Broglie waves.
These waves differ from the electromagnetic waves as they,
(i) have lower velocities
(ii) have no electrical and magnetic fields and
(iii) are not emitted by the particle under consideration.
The experimental confirmation of the de–Broglie relation was obtained when Davisson and Germer, in 1927, observed that a beam of electrons is diffracted by a nickel crystal. As diffraction is a characteristic property of waves, hence the beam of electron behaves as a wave, as proposed by de–Broglie.
Werner Heisenberg considered the limits of how precisely we can measure properties of an electron or other microscopic particle like electron. He determined that there is a fundamental limit of how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also ture. This is summed up in what we now call the “Heisenberg uncertainty principle : It is impossible to determine simultaneously and precisely both the momentum and position of a particle. The product of undertainty in the position, Δx and the uncertainity in the momentum Δ(mv) must be greater than or equal to h/4π. i.e.

Q.

The correct order of wavelength of Hydrogen (₁H¹), Deuterium (₁H²) and Tritium (₁H³) moving with same kinetic energy is :

The French physicist Louis de-Broglie in 1924 postulated that matter, like radiation, should exhibit a dual behaviour. He proposed the following relationship between the wavelength λ of a material particle, its linear momentum p and planck constant h.

The de Broglie relation implies that the wavelength of a particle should decreases as its velocity increases. It also implies that for a given velocity heavier particles should have shorter wavelength than lighter particles. The waves associated with particles in motion are called matter waves or de Broglie waves.
These waves differ from the electromagnetic waves as they,
(i) have lower velocities
(ii) have no electrical and magnetic fields and
(iii) are not emitted by the particle under consideration.
The experimental confirmation of the de–Broglie relation was obtained when Davisson and Germer, in 1927, observed that a beam of electrons is diffracted by a nickel crystal. As diffraction is a characteristic property of waves, hence the beam of electron behaves as a wave, as proposed by de–Broglie.
Werner Heisenberg considered the limits of how precisely we can measure properties of an electron or other microscopic particle like electron. He determined that there is a fundamental limit of how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also ture. This is summed up in what we now call the “Heisenberg uncertainty principle : It is impossible to determine simultaneously and precisely both the momentum and position of a particle. The product of undertainty in the position, Δx and the uncertainity in the momentum Δ(mv) must be greater than or equal to h/4π. i.e.

Q.

The transition, so that the de - Broglie wavelength of electron becomes 3 times of its initial value in He⁺ ion will be :

The French physicist Louis de-Broglie in 1924 postulated that matter, like radiation, should exhibit a dual behaviour. He proposed the following relationship between the wavelength λ of a material particle, its linear momentum p and planck constant h.

The de Broglie relation implies that the wavelength of a particle should decreases as its velocity increases. It also implies that for a given velocity heavier particles should have shorter wavelength than lighter particles. The waves associated with particles in motion are called matter waves or de Broglie waves.
These waves differ from the electromagnetic waves as they,
(i) have lower velocities
(ii) have no electrical and magnetic fields and
(iii) are not emitted by the particle under consideration.
The experimental confirmation of the de–Broglie relation was obtained when Davisson and Germer, in 1927, observed that a beam of electrons is diffracted by a nickel crystal. As diffraction is a characteristic property of waves, hence the beam of electron behaves as a wave, as proposed by de–Broglie.
Werner Heisenberg considered the limits of how precisely we can measure properties of an electron or other microscopic particle like electron. He determined that there is a fundamental limit of how closely we can measure both position and momentum. The more accurately we measure the momentum of a particle, the less accurately we can determine its position. The converse is also ture. This is summed up in what we now call the “Heisenberg uncertainty principle : It is impossible to determine simultaneously and precisely both the momentum and position of a particle. The product of undertainty in the position, Δx and the uncertainity in the momentum Δ(mv) must be greater than or equal to h/4π. i.e.

Q. If the uncertainty in velocity & position is same, then the uncertainty in momentum will be :

The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to  . For examle, in the case of n = 4, number of lines produced is 6. (4 → 3, 4 → 2, 4 → 1, 3 → 2, 3 → 1, 2 → 1). When an electron returns from n₂ to n₁ state, the number of lines in the spectrum will be equal to 
If the electron comes back from energy level having energy E₂ to energy level having energy E₁, then the difference may be expressed in terms of energy of photon as :

Since h and c are constants, ΔE corresponds to definite energy; thus each transition from one energy level to another will produce a light of definite wavelength. This is actually observed as a line in the spectrum of hydrogen atom.
Wave number of line is given by the formula 

where R is a Rydberg’s constant
(R = 1.1 × 10⁷ m^-1)

Q.

The energy photon emitted corresponding to transition n = 3 to n = 1 is [h = 6 × 10^-34 J - sec]

The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to . For examle, in the case of n = 4, number of lines produced is 6. (4 → 3, 4 → 2, 4 → 1, 3 → 2, 3 → 1, 2 → 1). When an electron returns from n₂ to n₁ state, the number of lines in the spectrum will be equal to 
If the electron comes back from energy level having energy E₂ to energy level having energy E₁, then the difference may be expressed in terms of energy of photon as :

Since h and c are constants, ΔE corresponds to definite energy; thus each transition from one energy level to another will produce a light of definite wavelength. This is actually observed as a line in the spectrum of hydrogen atom.
Wave number of line is given by the formula 

where R is a Rydberg’s constant
(R = 1.1 × 10⁷ m^-1)

Q.

In a collection of H–atom, electrons make transition from 5th excited state to 2nd excited state then maximum number of different types of photons observed are :

The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to . For examle, in the case of n = 4, number of lines produced is 6. (4 → 3, 4 → 2, 4 → 1, 3 → 2, 3 → 1, 2 → 1). When an electron returns from n₂ to n₁ state, the number of lines in the spectrum will be equal to 
If the electron comes back from energy level having energy E₂ to energy level having energy E₁, then the difference may be expressed in terms of energy of photon as :

Since h and c are constants, ΔE corresponds to definite energy; thus each transition from one energy level to another will produce a light of definite wavelength. This is actually observed as a line in the spectrum of hydrogen atom.
Wave number of line is given by the formula 

where R is a Rydberg’s constant
(R = 1.1 × 10⁷ m^-1)

Q.

The difference in the wavelength of the 1^st line of Lyman series and 2nd line of Balmer series in a hydrogen atom is :

The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth and fifth orbits from higher energy orbits respectively. Maximum number of lines produced when an electron jumps from nth level to ground level is equal to . For examle, in the case of n = 4, number of lines produced is 6. (4 → 3, 4 → 2, 4 → 1, 3 → 2, 3 → 1, 2 → 1). When an electron returns from n₂ to n₁ state, the number of lines in the spectrum will be equal to 
If the electron comes back from energy level having energy E₂ to energy level having energy E₁, then the difference may be expressed in terms of energy of photon as :

Since h and c are constants, ΔE corresponds to definite energy; thus each transition from one energy level to another will produce a light of definite wavelength. This is actually observed as a line in the spectrum of hydrogen atom.
Wave number of line is given by the formula 

where R is a Rydberg’s constant
(R = 1.1 × 10⁷ m^-1)

Q.

The wave number of electromagnetic radiation emitted during the transition of electron in between two levels of Li²⁺ ion whose principal quantum numbers sum is 4 and difference is 2 is :

A single electron atom has a nuclear charge +Ze where Z is the atomic number and ‘e’ is the electronic charge. It requires 47.2ev to excite the electron from 2^nd Bohr’s orbit to 3rd Bohr’s orbit from above given data solve the following question:

Q.

The atomic no. of the element is:

A single electron atom has a nuclear charge +Ze where Z is the atomic number and ‘e’ is the electronic charge. It requires 47.2ev to excite the electron from 2^nd Bohr’s orbit to 3^rd Bohr’s orbit from above given data solve the following question:

Q. The energy required for transition of electron from third to fourth Bohr’s orbit is: