Structure of Atom

For a hydrogen atom, the ionization energy is the energy required to move an electron from:

Bohr's model violates which principle that was developed later?

What is the relationship between the energy ($E$) and the radius ($r$) of an orbit in Bohr's model?

The Brackett series of hydrogen spectrum lines is produced by electron transitions ending in which shell?

The kinetic energy of an electron in the $2^{nd}$ orbit of a Hydrogen atom is:

Which transition in $He^+$ will have the same wave number as the $n=2$ to $n=1$ transition in Hydrogen?

The ratio of the area of the second Bohr orbit to the first Bohr orbit of a Hydrogen atom is:

Which of the following is true regarding the total energy ($E$) and kinetic energy ($K$) of an electron in a Bohr orbit?

An electron makes a transition from $n=4$ to $n=2$ in a $Li^{2+}$ ion. The wavelength of the emitted photon is (where $R$ is Rydberg constant):

What is the ratio of the velocity of an electron in the $3^{rd}$ orbit of $Li^{2+}$ to the velocity of an electron in the $4^{th}$ orbit of $Be^{3+}$?

Orbitals belonging to the same subshell and having the same energy are called:

What is the maximum number of electrons that can be held in the $n=1$ shell?

The subshell with $n=3$ and $l=0$ is called:

Which quantum number is not derived from the Schrödinger wave equation directly?

The orientation of an atomic orbital is determined by its:

Which of the following is the correct formula for calculating the total number of nodes in an orbital?

How many electrons in an atom of Sulphur ($Z=16$) have $l = 1$?

The total number of nodes for a $6d$ orbital is:

For which of the following ions is the magnetic moment approximately 4.90 BM?

Identify the element with the ground state electronic configuration $[Ar] 3d^5 4s^1$.

For $n=1$, the only possible subshell is:

How many electrons are in the $d$-subshell of a neutral Zinc atom ($Z=30$)?

Which principle or rule prevents two electrons in the same orbital from having the same spin?

The total number of electrons in a neutral Nitrogen atom ($Z=7$) is:

In the ground state of an Iron atom ($Z=26$), the number of electrons in the $d$-subshell is:

How many electrons can have the quantum numbers $n=3, l=2, m_{l}=0$ in an atom?

The electronic configuration of $Sc^{3+}$ ($Z=21$) is:

Calculate the orbital angular momentum of an electron in a $2s$ orbital.

Which of the following electronic transitions in a $He^+$ ion will have the same wavelength as the $n=2$ to $n=1$ transition in a Hydrogen atom?

Which of the following is the ground state configuration of the $Cr^{2+}$ ion ($Z=24$)?

Which of the following is NOT a characteristic of a photon?

The product of the uncertainty in position and the uncertainty in velocity is given by:

The emission of electrons from a metal surface when light of suitable frequency falls on it is called:

If the mass of a particle is doubled and its velocity remains the same, its de Broglie wavelength will:

If the stopping potential for a metal surface is $1.5 V$, what is the maximum kinetic energy of the emitted photoelectrons?

In the context of the dual nature of matter, which property is primarily associated with the particle nature of electromagnetic radiation?

The de Broglie wavelength of a neutron at $27^{\circ}C$ is $\lambda$. What will be its wavelength at $927^{\circ}C$?

The uncertainty in position of a $0.25\,kg$ ball is $10^{-5}\,m$. The uncertainty in its velocity is ($h = 6.6 \times 10^{-34}\,Js$):

In the context of the Davisson-Germer experiment, if the accelerating voltage is increased, the de Broglie wavelength of the electrons will:

Two radiations of photon energies $1\,eV$ and $2.5\,eV$ successively illuminate a photosensitive metallic surface of work function $0.5\,eV$. The ratio of the maximum speeds of the emitted photoelectrons is: