Home
Class 12
CHEMISTRY
STATEMENT -1 : Orbital angular momentum ...

STATEMENT -1 `:` Orbital angular momentum is given by `sqrt(l(l+1))(h)/(2pi)`
and
STATEMENT-2 `:` I ( Quantum number ) decides the shape of orbital

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1

B

Statement-1 is True, Statement-2 isTrue, Statement-2 is NOT a correct explanation for Statement-1

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False , Statement-2 isTrue

Text Solution

Verified by Experts

The correct Answer is:
2
Promotional Banner

Topper's Solved these Questions

  • STRUCTURE OF ATOM

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT ( SECTION -F) Matrix - Match Type Questions|4 Videos

  • STRUCTURE OF ATOM

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT ( SECTION -G) Integer Answer Type Questions|4 Videos

  • STRUCTURE OF ATOM

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT ( SECTION -D) Linked Comprehension Type Questions)|9 Videos

  • STRUCTURE OF ATOM

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION -D) Assertion-Reason Type Questions|15 Videos

  • SURFACE CHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment Section - C (Assertion - Reason type questions)|10 Videos

Similar Questions

Explore conceptually related problems

The orbital angular momentum of a p electron is equal to sqrt(2) (h)/(2pi)

STATEMENT-1 : The orbital angular momentum of an e^(-) in 4f atomic orbital is sqrt( 12) ( h)/( 2pi) and STATEMENT-2 : The orbital angualar momentum of an electron is given by sqrt(l(l+1)) ( h)/( 2pi) and for f-subshell, l=3

The orbital angular momentum of an electron in 2s -orbital is

The orbital angular momentum of an electron in 2s -orbital is

STATEMENT-1: The angular momentum of d-orbitals is sqrt6(h)/(2pi) STATEMENT 2 : Angular momentum of electron in orbit is mvr=(nh)/(2pi)

When the azimuthal quantum number l = 1, the shape of the orbital will be

The orbital angular momentum of an electron in 2s orbital is ………

Azimuthal quantum number (l) : It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1) {:("Value of l",0,1,2,3),("subshell",s,p,d,r):} Number of orbitals in a subshell =2l+1 Orbital angular momentum L =h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)] Magnetic quantum number (m) : It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals (p_x ,p_y and p_z) , d-subshell five orbitals (d_"xy", d_"yz",d_(x^2-y^2), d_z^2) and f-subshell has seven orbitals. Spin quantum number (s) : It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis. Spin of the electron produces angular momentum equal to S=sqrt(s(s+1)) h/(2pi) where s=+1/2 Total spin of an atom =+n/2 or -n/2 (where n is the number of unpaired electron ) The magnetic moment of an atom mu_s=sqrt(n(n+2)) B.M. n=number of unpaired electrons B.M. (Bohr magneton) Orbital angular momentum of an electron is sqrt3h/pi then the number of orientations of this orbital in spaces are :

Azimuthal quantum number (l) : It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1) {:("Value of l",0,1,2,3),("subshell",s,p,d,r):} Number of orbitals in a subshell =2l+1 Orbital angular momentum L =h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)] Magnetic quantum number (m) : It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals (p_x ,p_y and p_z) , d-subshell five orbitals (d_"xy", d_"yz",d_(x^2-y^2), d_z^2) and f-subshell has seven orbitals. Spin quantum number (s) : It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis. Spin of the electron produces angular momentum equal to S=sqrt(s(s+1)) h/(2pi) where s=+1/2 Total spin of an atom =+n/2 or -n/2 (where n is the number of unpaired electron ) The magnetic moment of an atom mu_s=sqrt(n(n+2)) B.M. n=number of unpaired electrons B.M. (Bohr magneton) The correct order of the maximum spin of [._25Mn^(4+),._24Cr^(3+), ._26Fe^(3+)] is :

Azimuthal quantum number (l) : It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1) {:("Value of l",0,1,2,3),("subshell",s,p,d,r):} Number of orbitals in a subshell =2l+1 Orbital angular momentum L =h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)] Magnetic quantum number (m) : It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals (p_x ,p_y and p_z) , d-subshell five orbitals (d_"xy", d_"yz",d_(x^2-y^2), d_z^2) and f-subshell has seven orbitals. Spin quantum number (s) : It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis. Spin of the electron produces angular momentum equal to S=sqrt(s(s+1)) h/(2pi) where s=+1/2 Total spin of an atom =+n/2 or -n/2 (where n is the number of unpaired electron ) The magnetic moment of an atom mu_s=sqrt(n(n+2)) B.M. n=number of unpaired electrons B.M. (Bohr magneton) A d-block element has total spin value of +3 or -3 then the magnetic moment of the element is approximately :