The positions of all the electrons in phosphorus (p, atomic number 15) can be specified in three different ways using electron notation. (8 points) i. give the complete electron configuration of the phosphorus (p) atom. (2 points) 1s22s22p63s23p3 ii. give the noble gas configuration of the phosphorus (p) atom. (2 points) [ne] 3s2 3p3iii. give the orbital configuration of the phosphorus (p) atom.

i) 1s²2s²2p⁶3s²3p³

ii) [Ne]3s²3p³

iii) ↑↓       ↑↓    ↑↓  ↑↓  ↑↓       ↑↓   ↑ ↑ ↑

    1s²      2s²         2p⁶             3s²    3p³    

Explanation:

i) The phosphorus, with atomic number (Z) 15, has the following  electron configuration:

Z=15 → Number of electrons = 15

1s²2s²2p⁶3s²3p³  

ii) The noble gas configuration of the phosphorus is the next:

[Ne]3s²3p³  

Neon is the noble gas that precedes phosphorus, its atomic number is 10. Therefore, the first ten electrons in the electronic configuration of P correspond to the noble gas Ne.  

iii) The orbital configuration of the P is given by the spins of the electrons in each orbital:

   ↑↓            

1   s²

   ↑↓      ↑↓  ↑↓  ↑↓

2  s²             p⁶  

   ↑↓        ↑ ↑ ↑

3  s²           p³  

Where ↑ and ↓ represents electron spins.

We can consider every orbital as a box that contains the electrons, and using the Pauli exclusion principle we can fill the boxes with the electrons.

So, following that principle, we have that every box will have a maximum of two electrons, which are represented as ↑↓, when they are paired up, and ↑ when they are not paired up.          

In phosphorous case, every s orbital contain 2 electrons represented as ↑↓, and every p orbital has three orbitals: , and , for a total of 6 electrons (two electrons for each orbital), except for the 3p orbital, which has only 3 electrons, represented as ↑ ↑ ↑.                                  

I hope it helps you!