Structure of Atom

Which of the following was a major drawback of Rutherford's nuclear model?

The mass of a neutron is approximately:

How many protons and neutrons are there in $^{235}_{92}U$?

What property of oil drops was used by Millikan to calculate the charge on an electron?

Thomson's model of the atom failed to explain which of the following?

Which sub-atomic particle was the first to be characterized by its $e/m$ ratio?

The mass of a neutron is slightly greater than that of a proton. By what approximate factor?

In Rutherford's model, what prevents the electrons from 'falling' into the nucleus due to electrostatic attraction?

Which of the following particles has the highest specific charge?

If an atom has 11 protons and 12 neutrons, and it loses one electron, what is the charge on the resulting ion in Coulombs?

The bounce-back of $\alpha$-particles in Rutherford's experiment can be compared to which of the following scenarios?

What keeps the atom as a whole electrically neutral in the Rutherford model?

In Thomson's model, the large sphere that makes up the bulk of the atom is considered to be ______.

What was the approximate thickness of the gold foil used in Rutherford's scattering experiment in scientific notation?

The scattering experiment performed by Geiger and Marsden was done under the guidance of:

Why did Rutherford's model fail to explain the stability of the atom based on classical electromagnetism?

According to Rutherford's model, the mass of the atom is primarily contributed by:

According to Rutherford, the force $F$ between the alpha particle and the nucleus varies with distance $r$ as $1/r^2$. The work done by this force as the alpha particle moves from infinity to the distance of closest approach $r_0$ is:

In the Rutherford model, if the radius of the orbit of an electron decreases, its kinetic energy:

The probability of an $\alpha$-particle being scattered at an angle $\theta$ is $P$. If the atomic number of the target foil is doubled, the probability becomes:

The Lyman series of the Hydrogen spectrum lies in the:

In Bohr's formula for the radius of an orbit, if $Z$ increases for a fixed $n$, the radius:

The Bohr model could not explain the dual nature of matter, which was proposed by:

Which shell has the highest energy among K, L, M, and N shells?

What is the ratio of the energy of a photon emitted during the transition from $n=2$ to $n=1$ in Hydrogen to that in $Be^{3+}$?

The wavelength of the third line of the Balmer series for Hydrogen corresponds to the transition:

The ionization potential of the Hydrogen atom is $13.6 \text{ V}$. What is the ionization potential of $Li^{2+}$?

Which of the following represents the correct sequence of increasing orbital radius?

The ratio of the difference in energy between $n=2$ and $n=1$ ($E_2 - E_1$) to the difference in energy between $n=3$ and $n=2$ ($E_3 - E_2$) for a Hydrogen atom is:

An electron in a Bohr orbit of Hydrogen has a total energy of $-3.4$ eV. The angular momentum of this electron is:

In the quantum mechanical model, what is the region around the nucleus where the probability of finding an electron is high?

Which rule states that degenerate orbitals are filled singly before pairing begins?

When $l=2$, what are the possible values for $m_l$?

How many $f$-orbitals are present in the $f$-subshell?

Two electrons in the same orbital are distinguished by which quantum number?

If the kinetic energy of an electron is increased nine times, its de Broglie wavelength becomes:

Which quantum number provides information about the orientation of the electron's spin?

What is the total number of nodes (radial + angular) for the $6d$ orbital?

According to the Pauli Exclusion Principle, what is the maximum number of electrons that can be accommodated in a subshell for which $l = 3$?

The nodes in the $2s$ orbital occur at a distance $r$ from the nucleus where the radial wave function $\psi$ becomes zero. For Hydrogen, this occurs at $r$ equal to:

In the photoelectric effect, if the frequency of light is less than the threshold frequency, then:

Wavenumber is defined as the:

The value of $1$ electron-volt ($eV$) in Joules is:

The wave nature of an electron is used in the construction of which device?

Calculate the wavelength of a photon whose momentum is the same as that of an electron moving with a speed of $10^5 \text{ m/s}$.

According to Einstein's photoelectric equation, the graph between the maximum kinetic energy of photoelectrons and the frequency of incident radiation is a:

Which of the following values of Planck's constant ($h$) is used in SI units?

The threshold frequency $\nu_0$ for a metal is $7.0 \times 10^{14} \text{ s}^{-1}$. If light of frequency $\nu = 1.0 \times 10^{15} \text{ s}^{-1}$ hits the metal, the maximum kinetic energy of the photoelectrons is:

The de Broglie wavelength of a ball of mass $150 \text{ g}$ moving at $30 \text{ m/s}$ is of the order of:

An electron is moving with a kinetic energy of $4.55 \times 10^{-25} \text{ J}$. Its de Broglie wavelength is: (Mass of electron = $9.1 \times 10^{-31} \text{ kg}$)

What is the primary reason the uncertainty principle is ignored in classical mechanics?

The uncertainty in position of an electron is $10^{-10}$ m. If the uncertainty in momentum is very high, the electron behaves more like a:

If $\Delta x$ is measured in meters and $\Delta p$ in $kg \cdot m/s$, what is the unit of the constant $h$?

The concept of 'Orbitals' as opposed to 'Orbits' is a result of:

The uncertainty in position of a proton is $10^{-11}$ m. If the mass of a proton is 1836 times that of an electron, the uncertainty in its velocity is:

For a particle with $\Delta x = 10^{-10}$ m and $\Delta p = 10^{-24}$ kg m/s, the product $\Delta x \cdot \Delta p$ is $10^{-34}$ kg m$^2$/s. Is this measurement possible?

Calculate the uncertainty in velocity of a ball of mass $150$ g if the uncertainty in its position is $1$ \AA ($10^{-10}$ m).

Which of the following describes the relationship between the Heisenberg Principle and the Bohr radius ($a_0$)?

If the uncertainty in the momentum of a particle is $10^{-24}$ kg m/s, what is the minimum uncertainty in its position?

If the uncertainty in the position of an electron is $10^{-12}$ m, what is the minimum uncertainty in its velocity?

Which subshell notation corresponds to $n = 3$ and $l = 2$?

What is the total number of orbitals in the first shell ($n = 1$)?

The orbital angular momentum of an electron is calculated using which quantum number?

Which of the following is NOT a valid value for the magnetic quantum number $m_l$ if $l = 1$?

If $n=2$, the possible values of $m_l$ across all subshells are:

The total number of electrons that can be accommodated in all the orbitals having $l=2$ and $n=3$ is:

Which subshell corresponds to $n=4$ and $l=1$?

For a principal quantum number $n=4$, how many orbitals have $l=2$ and $m_l = +1$?

In the ground state of Rubidium ($Z=37$), the valence electron has the following quantum numbers:

How many radial nodes are present in the $4f$ orbital?

Which of the following sets of quantum numbers is NOT allowed?

The ground state electronic configuration of Copper ($Z=29$) is:

If the principal quantum number $n=2$, the possible values of the azimuthal quantum number $l$ are:

Which orbital has a dumbbell shape?

Which of the following ions is diamagnetic in its ground state?

Which of the following is the correct order of filling of electrons in the subshells of the 6th period?

What is the value of the total spin multiplicity ($2S+1$) for the ground state of Carbon ($Z=6$)?

Which of the following quantum number sets represents an electron in a $3d$ orbital?

A subshell with $n=5$ and $l=3$ can accommodate a maximum of how many electrons?

Calculate the total number of electrons in $Mo$ ($Z=42$) which have $l=2$. (Ground state config is $[Kr] 4d^5 5s^1$)

If an electromagnetic wave has a frequency of $10^{15}\ Hz$, in which region does it lie?

Which of these scientists won the Nobel Prize for explaining the photoelectric effect?

The spectrum produced by the sun is an example of:

As the orbit number ($n$) increases in a hydrogen atom, the energy of the level:

The spectrum produced by the white light from the sun after passing through a prism is:

Calculate the frequency of yellow light having wavelength 580 nm.

Which of the following is correct regarding the velocity of light, X-rays, and Radio waves in vacuum?

Calculate the ionization energy of a $Li^{2+}$ ion in its first excited state ($n=2$).

The number of photons emitted per second by a medium wave transmitter of $10\text{ kW}$ power, emitting radio waves of wavelength $500\text{ m}$, is of the order of:

Given the work functions of four metals: A ($2.0\text{ eV}$), B ($2.5\text{ eV}$), C ($3.0\text{ eV}$), and D ($4.0\text{ eV}$). Which metal will NOT show the photoelectric effect for light of $400\text{ nm}$?