# Oxygen Atomic Number

Atomic Number is the amount of electrons in an atom, it is also the amount of protons in the nucleus of an atom.Example:Oxygen (O) has the atomic number, 8. Which means that there are 8 protons in. Oxygen is an element displayed by the symbol O, and atomic number 8. It is an essential element for human survival. Decreased oxygen levels may be treated with medical oxygen therapy. Treatment with oxygen serves to increase blood oxygen levels and also exerts a secondary effect of decreasing blood flow resistance in the diseased lung, leading to decreased cardiovascular workload in an attempt. Element Oxygen (O), Group 16, Atomic Number 8, p-block, Mass 15.999. Sources, facts, uses, scarcity (SRI), podcasts, alchemical symbols, videos and images. Name: Oxygen: Symbol: O Atomic Number: 8: Atomic Mass: 15.999 atomic mass units: Number of Protons: 8: Number of Neutrons: 8: Number of Electrons: 8: Melting Point.

### An oxygen atom has a total of 8 elections. How do you write the 4 quantum numbers for each of the 8 electrons in the ground state ?

Uses of Oxygen: Forms almost 21% of atmosphere. Used in steel making, welding, water purification, cement. It is also required for supporting life and combustion. Additional Notes: Oxygen is the most abundant element on the surface of the earth. Oxygen Page One. Overview of Oxygen; Oxygen's Name in Other Languages; Atomic Structure.

You know that a neutral oxygen atom has 8 electrons.

It's always helpful to write the electron configuration for an element before trying to assign quantum numbers for each individual electron . As you can see in the image above, the electron configuration for neutral oxygen is

$' O ' : 1 {s}^{2} 2 {s}^{2} 2 {p}^{4}$

Assuming you know the basics behind quantum numbers, you can write the unique 4-number set for each electron belonging to oxygen like this

The first energy level:

$' n = 1 '$, $' l = 0 '$, $' m {'}_{l} ' = 0 '$, $' m {'}_{s} ' = - \frac{1}{2} '$$\to$ the electron located in the 1s-orbital, spin-down;
$' n = 1 '$, $' l = 0 '$, $' m {'}_{l} ' = 0 '$, $' m {'}_{s} ' = + \frac{1}{2} '$$\to$ the electron located in the 1s-orbital, spin-up;

The second energy level:

$' n = 2 '$, $' l = 0 '$, $' m {'}_{l} ' = 0 '$, $' m {'}_{s} ' = - \frac{1}{2} '$$\to$ the electron lcoated in the 2s-orbital, spin-down;
$' n = 2 '$, $' l = 0 '$, $' m {'}_{l} ' = 0 '$, $' m {'}_{s} ' = + \frac{1}{2} '$$\to$ the electron located in the 2s-orbital, spind-up;

$' n = 2 '$, $' l = 1 '$, $' m {'}_{l} ' = - 1 '$, $' m {'}_{s} ' = - \frac{1}{2} '$$\to$ the electron located in the $' 2 p {'}_{x} ' - \mathmr{and} b i t a l '$, spin-down;
$' n = 2 '$, $' l = 1 '$, $' m {'}_{l} ' = - 1 '$, $' m {'}_{s} ' = + \frac{1}{2} '$$\to$ the electron located in the $' 2 p {'}_{x} ' - \mathmr{and} b i t a l '$, spin-up;
$' n = 2 '$, $' l = 1 '$, $' m {'}_{l} ' = 0 '$, $' m {'}_{s} ' = + \frac{1}{2} '$$\to$ the electron located in the $' 2 p {'}_{y} ' - \mathmr{and} b i t a l '$, spin-up;
$' n = 2 '$, $' l = 1 '$, $' m {'}_{l} ' = 1 '$, $' m {'}_{s} ' = + \frac{1}{2} '$$\to$ the electron located in the $' 2 p {'}_{z} ' - \mathmr{and} b i t a l '$, spin-up;

First, you must know the rules for quantum numbers.

#### Explanation:

Then you use the Aufbau Principle, the Pauli Exclusion Principle, and Hund's Rule to assign the quantum numbers.

The rules for quantum numbers are:

#n = 1, 2, 3… ∞#.
#l = 0, 1, 2… n – 1#
#m_l = -l… -1, 0, 1… l#
#m_s = ±1/2#

No two electrons can have the same set of four quantum numbers.

According to the Aufbau Principle, electrons fill orbitals starting at the lowest possible energy levels.

So the first two electrons have the quantum numbers

$\left.\begin{matrix}\boldsymbol{n} & \boldsymbol{l} & {\boldsymbol{m}}_{l} & {\boldsymbol{m}}_{s} \\ 1 & 0 & \textcolor{w h i t e}{i} 0 & + \frac{1}{2} \\ 1 & 0 & \textcolor{w h i t e}{i} 0 & - \frac{1}{2}\end{matrix}\right.$

The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of four quantum numbers.

So the next two electrons have the quantum numbers

$\left.\begin{matrix}\boldsymbol{n} & \boldsymbol{l} & {\boldsymbol{m}}_{l} & {\boldsymbol{m}}_{s} \\ 2 & 0 & \textcolor{w h i t e}{i} 0 & + \frac{1}{2} \\ 2 & 0 & \textcolor{w h i t e}{i} 0 & - \frac{1}{2}\end{matrix}\right.$

Now Hund's Rule comes into effect.

### Atomic Model Oxygen

Hund's Rule states that if two or more orbitals of equal energy are available, electrons will occupy them singly and with the same spin before filling them in pairs.

The next four electrons have the quantum numbers

$\left.\begin{matrix}\boldsymbol{n} & \boldsymbol{l} & {\boldsymbol{m}}_{l} & {\boldsymbol{m}}_{s} \\ 2 & 1 & - 1 & + \frac{1}{2} \\ 2 & 1 & \textcolor{w h i t e}{X} 0 & + \frac{1}{2} \\ 2 & 1 & + 1 & + \frac{1}{2} \\ 2 & 1 & - 1 & - \frac{1}{2}\end{matrix}\right.$

### Atomic Mass For Oxygen

And now you have the quantum numbers for the eight electrons in an oxygen atom.