Structure of atom practice · Mixed difficulty

Non-directional orbital is

Which particle may be removed from a stable neutral atom with least energy change?

The de-Broglie wavelength associated with a particle of mass $10^{-6} {~kg}$ moving with a velocity of $10 {~ms}^{-1}$ is :

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

For ionizing an ground state hydrogen atom, the energy needed in electron volts will be :

Calculate the energy required for the process $\mathrm{Z}_{\text {eff }}$ $\mathrm{He^{+}(g}) \rightarrow \mathrm{He^{2+}(g)+e}^{-}$. The ionisation energy for the $\mathrm{H}$-atom in the ground state is $2.18 \times 10^{-18} \mathrm{~J ~atom}^{-1}$.

What is the maximum number of electrons in an atom that can have the following quantum numbers $n = 4,\;{m_1} = + 1?$

All types of electromagnetic radiations possess same:

Which set is not correct?

Wave nature of electrons was demonstrated by

In an atom, an electron is moving with a speed of 600 m/s with an accuracy of 0.005%. Certainity with which the position of the electron can be located is $\left( {\begin{array}{cccccccccccccccccccc} {h = 6.6 \times {{10}^{ - 34}}kg\;{\mathrm{m}^2}{\mathrm{s}^{ - 1}},\;}\\ {mass\;of\;electron,\;{e_\mathrm{m}} = 9.1 \times {{10}^{ - 31}}kg} \end{array}} \right)$

In which orbital electron is most tightly bound to the nucleus?

The value of charge on the oil droplets experimentally observed were $- 1.6 \times {10^{ - 19}}$ and $- 4 \times {10^{ - 19}}$ coulomb. The value of the electronic charge, indicated by these results is:

The difference between ions and atoms is of:

Assertion: Ratio of anode rays is different for different gases.
Reason: Proton is the fundamental particle present in gases.

Assertion (A): $s$-orbital electron will be more tightly bound to the nucleus than $p$-orbital electron.
Reason (R): $Z_{\text {eff }}$ experienced by the electron decreases with increase of azimuthal quantum number ($l$).

The last electron placed in the third (n=3) quantum shell for:

In order to designate an orbital n in an atom, the number of quantum number required are:

When atoms are bombarded with α-particles suffer deflections while others pass through undeflected.
This is because :

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

Uncertainty in position of a particle of 25 g in space is ${10^{ - 5}}\mathrm{m}$. Hence, uncertainty in velocity $\left( {\mathrm{m}{\mathrm{s}^{ - 1}}} \right)$ is (Planck’s constant $h = 6.6 \times {10^{ - 34}}\mathrm{Js}$)

If Rutherford would have used $\beta$-particles instead of $\alpha$-particles in his Gold-leaf experiment, which of the following observations would definitely not have been made:

If the ionisation potential for hydrogen atom is 13.6eV, then the wavelength of light required for the ionisation of hydrogen atom would be:

The uncertainty in the momentum of an electron is $1.0 \times {10^{ - 5}}\mathrm{kg\;m}{\mathrm{s}^{ - 1}}$ , The uncertainty in its position will be

The ratio of radius of III and IV Bohr's orbits in hydrogen atom is:

Consider the following statements : 1.Electron density in xy plane in $3{d_{{x^2} - {y^2}}}$ orbital is zero 2.Electron density in xy plane in $3{d_{{z^2}}}$ orbital is zero 3.2s orbital has only one spherical node 4.For $2{p_z}$ orbital yz is the nodal plane The correct statements are

Which one of the following set of quantum numbers is possible for electron in the ground state of an atom with atomic number 19?

The potential energy of electron revolving in the ground state of $\mathrm{H}$ atom is

When photons of energy 4.25eV strike the surface of a metal A, the ejected photoelectrons have maximum kinetic energy, ${T_A}$ (expressed in eV) and de Broglie wavelength ${\lambda _A}.$ The maximum kinetic energy of photoelectrons liberated from another metal B by photons of energy 4.70V is ${T_B} = {T_A} - 1.50\;\mathrm{eV}.$ If the de Broglie wavelength of these photoelectrons is ${\lambda _B} = 2{\lambda _A},$ then which is not correct?

The momentum of a photon is $p,$ the energy associated with photon is given by: