n+l +m for the valence electrons of rb will be (where n,l,m, are prinicipal quantum number azimuthal qunatum number magnetic quantum number respectivley ):

For the principal quantum number n = 2, the possible values of azimuthal quantum number and magnetic quantum number respectively are

For the principal quantum number n = 2, the possible values of azimuthal quantum number and magnetic quantum number respectively are

If m = magnetic quantum number and l = azimuthal quantum number then :-

If m = magnetic quantum number and l = azimuthal quantum number then :-

For the azimuthal quantum number 'I' the total number of magnetic quantum numbers is given by

What are the values of principal quantum number (n) and azimuthal quantum number (l) for a 3d electron ?

What are the values of principal quantum number (n) and azimuthal quantum number (l) for a 3d electron ?

The position and energy of an electron is specified with the help of four quantum numbers namely, principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m_l) and spin quantum number (m_s) . The permissible values of these are : n = 1,2..... l = 0,1,.....(n-1) m_l = -l,......0,......+l m_s = +1/2 and -1/2 for each value of m_l . The angular momentum of electron is given as sqrt(l(l + 1)) cdot h/(2pi) While spin angular momentum is given as sqrt(s(s+1)) cdot (h/(2pi)) where s = 1/2 The electrons having the same value of n, l and m_l are said to belong to the same orbital. According to Pauli's exclusion principle, an orbital can have maximum of two electrons and these two must have opposite spin. Which of the following statements is not correct ?

For azimuthal quantum number l=3, the maximum number of electrons will be