diff --git a/education/chemistry/1.html b/education/chemistry/1.html index f11372e..dee43bf 100644 --- a/education/chemistry/1.html +++ b/education/chemistry/1.html @@ -2,7 +2,7 @@ title: 1 description: published: true -date: 2026-02-11T15:38:17.754Z +date: 2026-02-11T15:42:38.277Z tags: editor: ckeditor dateCreated: 2026-02-11T14:58:54.870Z @@ -40,14 +40,13 @@ dateCreated: 2026-02-11T14:58:54.870Z

 

+

Element

Protons = Electrons ⇒ Atom. Neutral.

Protons ≠ Electrons ⇒ Ion. Charged.

Electrons are surrounding the nucleus, consisting of protons and neutrons.

 

-

Element

Mass number are the number of protons and neutrons in the nucleus.

Atomic number are the number of protons in nucleus.

-

 

For example, 42He, where mass number is written on top left, and atomic number on bottom left.

 

Periodic Table

@@ -130,8 +129,8 @@ dateCreated: 2026-02-11T14:58:54.870Z g 9 18 -   -   +   +   @@ -175,9 +174,9 @@ dateCreated: 2026-02-11T14:58:54.870Z ⇡⇣ -   +   ⇡⇣ -   +   ⇡⇣ ⇡⇣ ⇡⇣ @@ -190,13 +189,13 @@ dateCreated: 2026-02-11T14:58:54.870Z 1s -   +   2s -   +   2p -   +   3s -   +   3p @@ -205,27 +204,27 @@ dateCreated: 2026-02-11T14:58:54.870Z

 

Aufbau principle

The lowest energy subshell or orbital will be filled first

-

1s < 2s < 2p < 3s < 3p < 4s < 3d
 

+

1s < 2s < 2p < 3s < 3p < 4s < 3d
 

Imagine drawing a line from right to left.

-

You should be able to find out that 4s subshell has a lower energy than 3d subshell this way.
 

+

You should be able to find out that 4s subshell has a lower energy than 3d subshell this way.
 

- - - + + + - - - - - + + + + + - + @@ -235,67 +234,67 @@ dateCreated: 2026-02-11T14:58:54.870Z - + - + - + - + - + - - + + - + - + - + - - - - - + + + + + - + - + - + - - + + - - - - - + - - - + + + + + + + - + - + - + @@ -303,13 +302,13 @@ dateCreated: 2026-02-11T14:58:54.870Z - + - + - + - + @@ -317,61 +316,61 @@ dateCreated: 2026-02-11T14:58:54.870Z - + - + - + - + - + - + - + - + - + - + - + - + - + - + - + - - + + - + - + - + - + - - - + + +
n       1            
       ⁄        
1   1s   2   3        
   ⁄    ⁄    ⁄           
2   2s   2p    4   5    
 ⁄  ⁄    ⁄    ⁄     ⁄  ⁄    
3   3s   3p    3d   67
   ⁄    ⁄    ⁄    ⁄    ⁄ 
4   4s   4p    4d   4f   8
   ⁄    ⁄    ⁄    ⁄    ⁄   
5   5s   5p    5d   5f    
   ⁄    ⁄    ⁄    ⁄       

 

-

Pauli's Exclusion principle

+

Pauli's exclusion principle

Each orbital can be occupied by no more than 2 electrons.

If 2 electrons occupy the same orbital, they must have opposite spins.