1s and 2s orbitals are spherical in shape.
The probability of finding the electron is maximum near the nucleus.
The probability of finding the electron at a given distance is equal in all directions.
The probability density of electrons for 2s orbital decreases uniformly as distance from the nucleus increases.
It is a negatively charged particle.
The mass of electron is equal to the mass of neutron.
It is a basic constituent of all atoms.
It is a constituent of cathode rays.
They have same atomic number but different mass number.
They have same number of electrons but different number of neutrons.
They have same number of neutrons but different number of electrons.
Sum of the number of protons and neutrons is same but the number ofprotons is different.
Pauli’s exclusion principle.
Heisenberg’s uncertainty principle.
Hund’s rule of maximum multiplicity.
N and l
N and m
M and s
Alpha particle (He 2+)
3s, 3p, 4s, 3d, 4p
3s, 3p, 3d, 4s, 4p
3s, 3p, 4s, 4p, 3d
3s, 3p, 3d, 4p, 4s
Angular momentum is an integral multiple of h/ 2π
The electron stationed in the orbit is stable.
The path of an electron is circular.
The change in the energy levels of electrons is continuous.
Pauli's exclusion principle
Principal and Azimuthal quantum number
Principal and magnetic Quantum number
Azimuthal and Magnetic Quantum number
Principal, Azimuthal and Magnetic quantum number
Ml gives information on the energy of the electron in a given orbital
L gives an idea about the shape of an orbital
N gives information on the size of the orbital
S gives the direction of spin of the electron in the orbital
N = 5 to n = 1
N = 5 to n = 3
N = 5 to n = 4
N = 5 to n = 2
N = 1, l = 2
N = 2, m = 1
N = 3, l = 0
N = 4, l = 2
The energy is not absorbed or emitted in whole number or multiples of quantum
Radiation is associated with energy.
Radiation is not emitted or absorbed.continuously but in the form of small packets called quanta.
Magnitude of energy associated with quantum is proportional to the frequency.
Only (i) and (ii)
Only (ii) and (iii)
Only (ii) and (iv)
(ii), (iii) and (iv)
Here's an interesting quiz for you.