Atomic Structure — JEE Main PYQs

The correct statement about probability density (except at infinite distance from nucleus) is:

Consider the hypothetical situation where the azimuthal quantum number, l, takes values $0,1,2,\dots \dots .\mathrm{n}+1$, where n is the principal quantum number. Then, the element with atomic number:

In the sixth period, the orbitals that are filled are:

The difference between the radii of $3^{\text{rd}}$ and $4^{\text{th}}$ orbits of $\mathrm{Li}{}^{2+}$ in $\Delta R_1$. The difference between the radii of $3^{\text{rd}}$ and $4^{\text{th}}$ orbits of $\mathrm{He}{}^{+}$ is $\Delta R_2$. Ratio $\Delta R_1:\Delta R_2$ is:

The region in the electromagnetic spectrum where the Balmer series lines appear is:

The shortest wavelength of H atom in the Lyman series is ${\lambda }_1$. The longest wavelength in the Balmer Series of ${\mathrm{He}}^{+}$is:

The quantum number of four electrons are given below:
I. $\mathrm{n}=4,\mathrm{I}=2,{\mathrm{m}}_{\mathrm{l}}=-2,{\mathrm{m}}_{\mathrm{s}}=-1/2$
II. $\mathrm{n}=3,\mathrm{I}=2,{\mathrm{m}}_{\mathrm{l}}=1,{\mathrm{m}}_8=+1/2$
III. …

If p is the momentum of the fastest electron ejected from a metal surface after the irradiation of light having wavelength $\lambda$, then for $1.5p$ momentum of the photoelectron, the wavelength of the light should be:
(Assume kinetic energy of ejected photoelectron to be very h …

For any given series of spectral lines of atomic hydrogen, let $\Delta \overline{\mathrm{V}}=\Delta {\overline{\mathrm{V}}}_{\text{max }}-\Delta {\overline{\mathrm{V}}}_{\text{min }}$ be the difference in maximum and minimum frequencies in ${\mathrm{cm}}^{-1}$. the ration …

Which of the graphs shown below does not represent the relationship between incident light and the electron ejected from metal surface?

The de Broglie wavelength ( $\lambda$ ) associated with a photoelectron varies with the frequency (v) of the incident radiation as, [ ${\mathrm{v}}_0$ is threshold frequency]:

The electrons are more likely to be found:

The ratio of the shortest wavelength of two spectral series of hydrogen spectrum is found to be about 9 . The spectral series are:

Heat treatment of muscular pain involves radiation of wavelength of about 900 nm. Which spectral line of H-atom is suitable for this purpose? …

What is the work function of the metal if the light of wavelength $4000\stackrel{\circ }{A}$ generates photoelectrons of velocity $6\times 10^5{\mathrm{ms}}^{-1}$ from it?
(Mass of electron $=9\times 10^{-31}\mathrm{kg}$
Velocity of light …

Among the following, the energy of 2s orbital is lowest in:

If the de Brogile wavelength of the electron in ${\mathrm{n}}^{\text{th }}$ Bohr orbit in a hydrogenic atom is equal to $1.5\pi {\mathrm{a}}_0$ ( ${\mathrm{a}}_0$ is Bohr radius), then the value of $\mathrm{n}/\mathrm{z}$ is :

Which one of the following about an electron occupying the 1s orbital in a hydrogen atom is incorrect? (The Bohr radius is represented by ${\mathrm{a}}_0$)

Which of the following combination of statements is true regarding the interpretation of the atomic orbitals?
(1) An electron in an orbital of high angular momentum stays away from the nucleus than an electron in the orbital of lower angular momentum.
(2) For a given value of the …

For emission line of atomic hydrogen from ${\mathrm{n}}_{\mathrm{i}}=8$ to ${\mathrm{n}}_{\mathrm{f}}=\mathrm{n}$, the plot of wave number $(\overline{\mathrm{v}})$ against $\left(\frac{1}{{\mathrm{n}}^2}\right)$ will be (The Rydberg constant, ${\mathrm{R}}_{\mathrm{H}}$ is in wave num …

The graph between $|\psi {|}^2$ and r(radial distance) is shown below. This represents:

The isoelectronic set of ions is

The radius of the second Bohr orbit for hydrogen atom is :
(Planck's Const. $\mathrm{h}=6.6262\times 10^{-34}\mathrm{Js}$; mass of electron $=9.1091\times 10^{-31}\mathrm{kg}$; charge of electron $\mathrm{e}=1.60210\times 10^{-19}\mathrm{C}$; permittivity of vacuum …

The group having isoelectronic species is :

A stream of electrons from a heated filament was passed between two charged plates kept at a potential difference $V$ esu. If $e$ and $m$ are charge and mass of an electron, respectively, then the value of $h/\lambda$ (where $\lambda$ is wavelength associated with electron wave …

Which of the following is the energy of a possible excited state of hydrogen?

The correct set of four quantum numbers for the valence electrons of rubidium atom (Z = 37) is:

Energy of an electron is given by $E=-2.178\times 10^{-18}\frac{Z^2}{n^2}$ J. Wavelength of light required to excite an electron in an hydrogen atom from level $\mathrm{n}=1$ to $\mathrm{n}=2$ will be ( $\mathrm{h}=6.62\times 10^{-34}$ Js and $\mathrm{c}=3.0\times 10^8$ …

The electrons identified by quantum numbers n and I :
(a) $n=4,I=1$
(b) $\mathrm{n}=4,\mathrm{I}=0$
(c) $n=3$, I $=2$
(d) $n=3,I=1$

Can be placed in order of increasing energy as :

A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emissions is at 680 nm , the other is at :

The energy required to break one mole of $\mathrm{Cl}-\mathrm{Cl}$ bonds in $\mathrm{Cl}{}_2$ is $242{\text{ kJ mol}}^{-1}$. The longest wavelength of light capable of breaking a single $\mathrm{Cl}-\mathrm{Cl}$ bond is
($c=3\times 10^8{\text{ ms}}^{-1}$ and $N_{\text{A}}=6.02\times 10^{23}{\text{ mol}}^{-1}$)

Ionisation energy of $\mathrm{He}{}^{+}$ is $19.6\times 10^{-18}{\text{ J atom}}^{-1}$. The energy of the first stationary state $(n=1)$ of $\mathrm{Li}{}^{2+}$ is

In an atom, an electron is moving with a speed of $600\mathrm{m}/\mathrm{s}$ with an accuracy of $0.005\%$. Certainity with which the position of the electron can be located is $(\mathrm{h}=6.6\times 10^{-34}\mathrm{kg}{\mathrm{m}}^2{\mathrm{s}}^{-1}$, …

Calculate the wavelength (in nanometer) associated with a proton moving at $1.0\times 10^3{\mathrm{ms}}^{-1}$ (Mass of proton $=1.67\times 10^{-27}\mathrm{kg}$ and $\mathrm{h}=6.63\times 10^{-34}\mathrm{Js}$ ) :

Which one of the following constitutes a group of the isoelectronic species?

The ionization enthalpy of hydrogen atom is $1.312\times 10^6{\mathrm{Jmol}}^{-1}$. The energy required to excite the electron in the atom from $\mathrm{n}=1$ to $\mathrm{n}=2$ is

Which of the following sets of quantum numbers represents the highest energy of an atom?

According to Bohr's theory, the angular momentum of an electron in $5^{\text{th}}$ orbit is

Uncertainty in the position of an electron (mass $=9.1\times 10^{-31}\mathrm{kg}$ ) moving with a velocity $300{\mathrm{ms}}^{-1}$, accurate upto $0.001\%$, will be
( $\mathrm{h}=6.63\times 10^{-34}\mathrm{Js}$ )

Which one of the following sets of ions represents a collection of isoelectronic species?

In a multi - electron atom, which of the following orbitals described by the three quantum numbers will have the same energy in the absence of magnetic acid and electric fields?
(a) $n=1,I=0,m=0$
(b) $n=2,I=0,m=0$
(c) $n=2,I=1,m=1$
(d) $n=3,I=2,m=1$
(e) …

Which of the following statements in relation to the hydrogen atom is correct?

Which of the following sets of quantum numbers is correct for an electron in 4 f orbital?

Consider the ground state of Cr atom $(Z=24)$. The number of electrons with the azimuthal quantum numbers $l=1$ and 2 are respectively

The wavelength of the radiation emitted, when in hydrogen atom electron falls from infinity to stationary state 1, would be (Rydberg constant $=1.097\times 10^7{\mathrm{m}}^{-1}$)

Which one the following sets of ions represents the collection of isoelectronic species?