Structure of Atom

\(\text { Consider the following schematic plots of orbital wavefunction }\left(\psi_r\right) \text { against distance }(r) \text { from the nucleus. }\)

The figure representing two radial nodes in the orbital is

A bulb is rated at 150 watt, converting $8 \%$ energy into light. If energy of one photon is $4.42 \times 10^{-19} \mathrm{~J}$, how many photons are emitted by the bulb per second?

\(\text { Match List I with List II : }\)
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Energy and radius of first Bohr orbit of $\mathrm{He}^{+}$and $\mathrm{Li}^{2+}$ are [Given $\mathrm{R}_{\mathrm{H}}=2.18 \times 10^{-18} \mathrm{~J}, \mathrm{a}_0=52.9 \mathrm{pm}$ ]

The ratio of the wavelengths of the light absorbed by a Hydrogen atom when it undergoes $n=2 \rightarrow n=3$ and $n=4 \rightarrow$ $\mathrm{n}=6$ transitions, respectively, is

Given below are two statements:
Statement I: The Balmer spectral line for H atom with lowest energy is located at \(\frac{5}{36} R_H \mathrm{~cm}^{-1}\).
(\(\mathrm{R}_{\mathrm{H}}=\) Rydberg constant)
Statement II: When the temperature of ...

The quantum numbers of four electrons are given below :
I. \(n=4 ; I=2 ; m_1=-2 ; s=-\frac{1}{2}\)
II. \(n=3 ; I=2 ; m_1=1 ; s=+\frac{1}{2}\)
III. \(n=4 ; I=1 ; m_1=0 ; s=+\frac{1}{2}\)
IV. \(n=3 ; I=1 ; m_1=-1 ; s=+\frac{1}{2}\)
The correc...

Match List I with List II.

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The energy of an electron in the ground state \(\mathrm{(n=1)}\) for \(\mathrm{He}^{+}\) ion is \(\mathrm{-x} \mathrm{~J}\), then that for an electron in \(\mathrm{(n=2)}\) state for \(\mathrm{Be}^{3+}\) ion in \(\mathrm{J}\) is

Given below are two statements:
Statement I : The value of wave function, \(\psi\) depends upon the coordinates of the electron in the atom.
Statement II : The probability of finding an electron at a point within an atom is proportional to...

Incorrect set of quantum numbers from the following is :

The relation between \(\mathrm{n}_{\mathrm{m}},\left(\mathrm{n}_{\mathrm{m}}=\right.\) the number of permissible values of magnetic quantum number \((\mathrm{m})\)) for a given value of azimuthal quantum number \((l)\), is

Select the correct Statements from the following :
A. Atoms of all elements are composed of two fundamental particles.
B. The mass of the electron is \(9.10939 \times 10^{-31} \mathrm{~kg}\).
C. All the isotopes of a given elements show sam...

When electromagnetic radiation of wavelength 300 nm falls on the surface of a metal, electrons are emitted with the kinetic energy of 1.68 \(\times\) 105 J mol\(-\)1. What is the minimum energy needed to remove an electron from the metal?
(...

Match List-I with List-II :

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If radius of second Bohr orbit of the He+ ion is 105.8 pm, what is the radius of third Bohr orbit of Li2+ ion?

Identify the incorrect statement from the following.

From the following pairs of ions which one is not an iso-electronic pair?

A particular station of All India Radio, New Delhi broadcasts on a frequency of 1,368 kHz (kilohertz). The wavelength of the electromagnetic radiation emitted by the transmitter is : [speed of light c = 3.0 \(\times\) 108 ms\(-\)1]

Which of the following series of transitions in the spectrum of hydrogen atom falls in visible region?

4d, 5p, 5f and 6p orbitals are arranged in the order of decreasing energy. The correct option is :

Which one is a wrong statement?

Which one is the wrong statement ?

How many electrons can fit in the orbital for which n = 3 and \(l\) = 1?

Which of the following pairs of d-orbitals will have electron density along the axes ?

Two electrons occupying the same orbital are distinguished by

The number of d-electrons in Fe2+ (Z = 26) is not equal to the number of electrons in which one of the following ?

The angular momentum of electron in 'd' orbital is equal to

Which is the correct order of increasing energy of the listed orbitals in the atom of titanium ? (At. no. Z = 22)

Be2+ is isoelectronic with which of the following ions ?

Calculate the energy in joule corresponding to light of wavelength 45 nm. (Planck,s constant, h = 6.63 \(\times\) 10\(-\)34 J s, speed of light, c = 3 \(\times\) 108 m s\(-\)1)

What is the maximum number of orbitals that can be identified with the following quantum numbers ?
n = 3, l = 1, m1 = 0

The outer electronic configuration of Gd (At. No. 64) is

According to law of photochemical equivalence the energy absorbed (in ergs/mole) is given as (h = 6.62 \(\times\) 10\(-\)27 ergs, c = 3 \(\times\) 1010 cm s\(-\)1, NA = 6.02 \(\times\) 10\(-\)23 mol\(-\)1)

Based on equation E = \(-\) 2.178 \(\times\) 10\(-\)18 J \(\left( {{{{Z^2}} \over {{n^2}}}} \right)\), certain conclusions are written. Which of them is not correct ?

What is the maximum numbers of electrons that can be associated with the following set of quantum numbers ?
n = 3, \(l\) = 1 and m = \(-\) 1

The value of Planck's constant is 6.63 \(\times\) 10\(-\)34 J s. The speed of light is 3 \(\times\) 1017 mm s\(-\)1. Which value is closest to the wavelength in nanometer of a quantum of light with frequency of 6 \(\times\) 1015 s$$-...

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

Maximum number of electrons in a subshell with \(l\) = 3 and n = 4 is

The orbital angular momentum of a p-electron is given as

The total number of atomic orbitals in fourth energy level of an atom is

The energies E1 and E2 of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths i.e., \(\lambda\)1 and \(\lambda\)2 will be

If n = 6, the correct sequence for filling of electrons will be

According to the Bohr theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon ?

A 0.66 kg ball is moving with a speed of 100 m/s. The associated wavelength will be
(h = 6.6 \(\times\) 10\(-\)34 J s)

Which of the following is not permissible arrangement of electrons in an atom ?

Maximum number of electrons in a subshell of an atom is determined by the following

If uncertainty in position and momentum are equal, then uncertainty in velocity is

The measurement of the electron position is associated with an uncertainty in momentum, which is equal to 1 \(\times\) 10\(-\)18 g cm s\(-\)1. The uncertainty in electron velocity is (mass of an electron is 9 \(\times\) 10\(-\)28 g)

Consider the following sets of quantum numbers :

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