Chemistry Class-11: Chapter –2. Structure of Atom – Part-7

Atom / Ion

Electronic configuration

(i)

(a)

(ii)

(b)

(iii)

(c)

(iv)

(d)

(e)

Quantum number

Information

(i)

Principal quantum number

(a)

Orientation of the orbital

(ii)

Azimuthal quantum number

(b)

Energy and size of orbital

(iii)

Magnetic quantum number

(c)

Spin of electron

(iv)

Spin quantum number

(d)

Shape of the orbital

Rules

Statements

(i)

Hund’s Rule

(a)

No two electrons in an atom can have the same set of four quantum numbers.

(ii)

Aufbau Principle

(b)

Half-filled and completely filled orbitals have extra stability.

(iii)

Pauli Exclusion Principle

(c)

Pairing of electrons in the orbitals belonging to the same subshell does not take place until each orbital is singly occupied.

(iv)

Heisenberg’s Uncertainty Principle

(d)

It is impossible to determine the exact position and exact momentum of a subatomic particle simultaneously.

(e)

In the ground state of atoms, orbitals are filled in the order of their increasing energies.

(i)

X-rays

(a)

(ii)

UV

(b)

(iii)

Long radio waves

(c)

(iv)

Microwave

(d)

(i)

Photon

(a)

Value is 4 for N shell

(ii)

Electron

(b)

Probability density

(iii)

(c)

Always positive value

(iv)

Principal quantum number n

(d)

Exhibits both momentum and wavelength

Column I

Column II

(i)

(a)

(ii)

(b)

(iii)

(c)

(iv)

(d)

(e)