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!

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!

Explanation:

The Electronic Configuration of the elements is the arrangement of all electrons of an element in energy levels and sub-levels (orbitals).  

There are 7 energy levels, numbered from 1 to 7, and in which electrons are distributed, logically in order according to their energy level. Each level is divided into sub-levels. These sub-levels into which each level is divided can be up to 4, called: s, p, d, f. In the sub-level s there can only be a maximum of 2 electrons, in p there can be a maximum of 6 electrons, in the sub-level d 10 electrons and finally in the sub-level f there can be a maximum of 14 electrons.

In level 1 there is only one sub-level, which will be the s. In level 2 there are 2 sub-levels, the s and the p. At level 3 there are 3 sub-levels s, p and d. And at level 4 there are 4 sub-levels, the s, the p, the d and the f.

Aufbau's principle is a principle of atomic physics, which explains how electrons are accommodated in their orbits around the nucleus of the atom. This principle states that the filling of these orbitals occurs in increasing order of energy, that is, from the orbitals of lower energy to those of higher energy.

The simplest of the sub-levels is 1s. If you fill the 1s you can start filling the 2s. After the 2s sub-level is satisfied, the 2p can begin to fill and so on.  

The atomic number Z of the element represents the number of protons of the element, and in a neutral atom it also indicates the number of electrons.  

So, given that the atomic number of the phosphorus is 15, and everything that has been said before, it is possible to say that the electrons that it has in the orbitals will be placed as follows:

1s² 2s² 2p⁶ 3s² 3p³

Finally, the orbital configuration of the phosphorus atom (P) will be as the image shows.

1) The full electron configuration for phosphorus is 1s²2s²2p⁶3s²3p

2) Phosphorus is paramagnetic

Explanation:

1) To write the electron configuration, we follow the electron filling order, that is starting from 1s, to 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4f, 5s, 5p, 5d, 6s till the electrons are all accounted for (up to 58)

We note that the s orbitals can each take two electrons while the p orbital can take 6 electrons and the d orbital can take 10 electrons

The electron configuration chart for phosphorus, P, is given as follows;

1s²2s²2p⁶3s²3p.

2) Diamagnetism is the temporary magnetism is the magnetism of a material that exists in the presence of a magnetic field due to a a change in the atomic electron orbital motion

Paramagnetism is a magnetism in which a material is weakly attracted by an applied external magnetic field such that there is induced magnetism in the applied magnetic field direction

Paramagnetic materials have have unpaired electrons that give them permanent magnetic moments in the absence of an applied magnetic field as such unpaired electrons are termed paramagnetic electrons and atoms that have one or more unpaired electrons are paramagnetic

Phosphorus, with the 3 partially filled p orbitals have 3 unpaired electrons in their outermost shell giving them the overall properties of a paramagnetic materials.

1) The full electron configuration for phosphorus is 1s²2s²2p⁶3s²3p

2) Phosphorus is paramagnetic

Explanation:

1) To write the electron configuration, we follow the electron filling order, that is starting from 1s, to 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4f, 5s, 5p, 5d, 6s till the electrons are all accounted for (up to 58)

We note that the s orbitals can each take two electrons while the p orbital can take 6 electrons and the d orbital can take 10 electrons

The electron configuration chart for phosphorus, P, is given as follows;

1s²2s²2p⁶3s²3p.

2) Diamagnetism is the temporary magnetism is the magnetism of a material that exists in the presence of a magnetic field due to a a change in the atomic electron orbital motion

Paramagnetism is a magnetism in which a material is weakly attracted by an applied external magnetic field such that there is induced magnetism in the applied magnetic field direction

Paramagnetic materials have have unpaired electrons that give them permanent magnetic moments in the absence of an applied magnetic field as such unpaired electrons are termed paramagnetic electrons and atoms that have one or more unpaired electrons are paramagnetic

Phosphorus, with the 3 partially filled p orbitals have 3 unpaired electrons in their outermost shell giving them the overall properties of a paramagnetic materials.

The correct configuration is -

Explanation:

Diamagnetism is an extremely week type of attraction that is incited by an adjustment in the orbital movement of electrons because of an applied attractive field. This attraction is nonpermanent and continues due to the presence of an external field.

The magnetic properties of a substance can be controlled by analyzing its electron configuration. If it has unpaired electrons in its outer orbital, at that point the substance is paramagnetic, and in the event that all electrons are found paired, the substance is then diamagnetic.

The electron configuration of the phosphorus is -

. As it is clear that the outer shell of P has 3 unpaired electron it is paramagnetic.

Electronic Configuration can be defined as the electron distribution of an atom or molecule in an atomic or molecular orbit. The atomic orbit consists of the s, p and d orbitals.

The Atomic number of Phosphorus is 15.

Thus, the Electronic configuration of Phosphorus is 1s² 2s² 2p6 3s² 3p³.

Read more:

What do u mean by electronic configuration? What are basic requirements while writing electronic configuration of an ele...

link

₁₅P = 1s² 2s² 2p⁶ 3s² 3p³

Explanation:

Phosphorus is the second element of group (v) with atomic number 15 and the electrons per shell are arrange as thus; 2, 8, 5.

The electronic configuration of phosphorus is

₁₅P = 1s² 2s² 2p⁶ 3s² 3p³

Or

₁₅P [Ne] 3s² 3p³

In its first shell I.e 1s shell, it has 2 electrons filling it to s-orbital requirement. In its second shell, electrons fill it in 2s² 2p⁶ filling the second orbital and attaining an octet configuration. The third shell contains 5 electrons filling 3s² 3p³ orbital.