Atomic Structure Questions

Dalton's Atomic theory could not explain which of the following?

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

The energies $E_1$ and $E_2$ of two radiations are $25\text{eV}$ and $50\text{eV}$ respectively. The relation between their wavelengths i.e. ${\lambda }_1$ and ${\lambda }_2$ will be:

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

Consider the following sets of quantum numbers

Which of the following sets of quantum number is not possible?

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

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

Two electrons occupying the same orbital are distinguished by:

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

${\text{Be}}^{2+}$ is isoelectronic with which of the following ions?

Calculate the energy in joule corresponding to light of wavelength $45\text{nm}$: (Planck constant $h=6.63\times 10^{-34}\text{Js}$, speed of light $c=3\times 10^8{\text{ms}}^{-1}$)

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

Based on the equation $E=-2.178\times 10^{-18}\text{J}\left(\frac{Z^2}{n^2}\right)$, which of the following conclusions is not correct?

What is the maximum number of electrons that can be associated with the following set of quantum numbers: $n=3,l=1,m=-1$?

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:

According to the Bohr Theory, which transition in the hydrogen atom will give rise to the least energetic photon?

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

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

The energy absorbed by each molecule ($A_2$) of a substance is $4.4\times 10^{-19}\text{J}$ and bond energy per molecule is $4.0\times 10^{-19}\text{J}$. The kinetic energy of the molecule per atom will be:

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

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

If the uncertainty in position and momentum of a particle are equal, then the uncertainty in its velocity is:

The orientation of an atomic orbital is governed by :

Given : The mass of electron is $9.11\times 10^{-31}\text{kg}$ plank constant is $6.626\times 10^{-34}\text{Js}$, the uncertainty involved in the measurement of velocity within a distance of $0.1\text{A˚}$ is :

Assertion : First ionization energy for nitrogen is lower than oxygen.Reason : Across a period effective nuclear charge decreases.

The most probable radius (in $\text{pm}$) for finding the electron in ${\text{He}}^{+}$ is: