Name: de Broglie Hypothesis
Uploaded: 2019-07-19
Duration: 11 min 28 s
Description: The De Broglie hypothesis proposes that all matter exhibits wave-like properties and relates the observed wavelength of matter to its momentum. Let's learn.

Question

Match the following species with their corresponding ground state electronic configuration.

Atom/Ion		Electronic Configuration
(i)	$Cu$	(a)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10}$
(ii)	${Cu}^{2 +}$	(b)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2}$
(iii)	${Zn}^{2 +}$	(c)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$
(iv)	${Cr}^{3 +}$	(d)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9}$
		(e)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{3}$

Accepted Answer

(a) $Cu$ has atomic number $29$ , therefore its electronic configuration is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$ .

Atom/Ion Electronic configuration

(i) $Cu$ (c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$

(b) ${Cu}^{+ 2}$ has two electrons less than the ground state copper atom, therefore it electronic configuration is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9}$

Atom/Ion Electronic configuration

(i) ${Cu}^{+ 2}$ (d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9}$

(c) ${Zn}^{+ 2}$ has two electrons less than the ground state zinc $(30)$ atom; therefore its electronic configurations is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10}$ .

Atom/Ion Electronic configuration

(i) ${Zn}^{+ 2}$ (a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10}$

(d) ${Cr}^{+ 3}$ has three electrons less than the ground state chromium $(24)$ atom; therefore, its electronic configuration is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{3}$

Atom/Ion Electronic configuration

(i) ${Cr}^{+ 3}$ (e) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{3}$

Atom/Ion		Electronic Configuration
(i)	$Cu$	(c)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$
(ii)	${Cu}^{2 +}$	(d)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9}$
(iii)	${Zn}^{2 +}$	(a)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10}$
(iv)	${Cr}^{3 +}$	(e)	$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{3}$

Quantum Number		Information Provided
(a)	Principal quantum number	(p)	orientation of the orbital
(b)	Azimuthal quantum number	(q)	energy and size of orbital
(c)	Magnetic quantum number	(r)	spin of electron
(d)	Spin quantum number	(s)	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

NCERT Solutions for Chapter: Structure of Atom, Exercise 1: Matching Type

NCERT Chemistry Solutions for Exercise - NCERT Solutions for Chapter: Structure of Atom, Exercise 1: Matching Type

Questions from NCERT Solutions for Chapter: Structure of Atom, Exercise 1: Matching Type with Hints & Solutions

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(i)	X-rays	(a)	$v = 10^{0} - 10^{4} Hz$
(ii)	UV	(b)	$v = 10^{10} Hz$
(iii)	Long radio waves	(c)	$v = 10^{16} Hz$
(iv)	Microwave	(d)	$v = 10^{18} Hz$

(i)	Photon	(a)	Value is $4$ for $N$ shell
(ii)	Electron	(b)	Probability density
(iii)	$ψ^{2}$	(c)	Always positive value
(iv)	Principal quantum number $n$	(d)	Exhibits both momentum and wavelength

Column I		Column II
(i)	$Cr$	(a)	$[Ar] 3 d^{8} 4 s^{0}$
(ii)	${Fe}^{2 +}$	(b)	$[Ar] 3 d^{10} 4 s^{1}$
(iii)	${Ni}^{2 +}$	(c)	$[Ar] 3 d^{6} 4 s^{0}$
(iv)	$Cu$	(d)	$[Ar] 3 d^{5} 4 s^{1}$
		(e)	$[Ar] 3 d^{6} 4 s^{2}$