The electronic configuration $1s^2, 2s^2 2p^5, 3s^1$ represents:

The atomic number of an element is $35$. What is the total number of electrons present in all the $p-$ orbitals of the ground state atom of that element?

For $3d_{z^2}$ calculate the value of $n, \ell, m$ and $s$.

The quantum number which explains the line spectra observed as doublets in the case of hydrogen and alkali metals,and doublets and triplets in the case of alkaline earth metals is:

In a multielectron atom,which of the following orbitals described by three quantum numbers will have the same energy in the absence of electric and magnetic fields?
$A: n=1, \ell=0, m_{\ell}=0$
$B: n=2, \ell=0, m_{\ell}=0$
$C: n=2, \ell=1, m_{\ell}=1$
$D: n=3, \ell=2, m_{\ell}=1$
$E: n=3, \ell=2, m_{\ell}=0$
Choose the correct answer from the options given below:

The atom of the element having atomic number $14$ should have: