Select a table from above

OH ^-

NO₃^-

F ^-

CI ^-

Br ^-

I ^-

S ^2-

SO₃^2-

SO₄^2-

CO₃^2-

SiO₃^2-

PO₄^3-

CrO₄^2-

Ac ^2-

H ²⁺

H ⁺

Li ⁺

NH₄⁺

K ⁺

Na ⁺

Ag ⁺

Ba ²⁺

Ca ²⁺

Mg ²⁺

Zn ²⁺

Mn ²⁺

Cu ²⁺

Cu ⁺

Hg ⁺

Hg ²⁺

Pb ²⁺

Fe ²⁺

Al ³⁺

Cr ³⁺

Bi ³⁺

Sn ²⁺

Sr ²⁺

*

Litmus

The colourant of natural origin - one of the first and most well known acid-base (ph) indicators.

[H+] > [OH-] PH = 0

[H+] = [OH-] PH = 7

[OH-] > [H+] PH = 14

Phenolphthalein

Triphenylmethane dyes - acid-base (ph) indicator that changes color from colorless to red-violet (raspberry).

[H+] > [OH-] PH = 0

[H+] = [OH-] PH = 7

[OH-] > [H+] PH = 14

Methyl-orange

Known acid-base (ph) indicator a syhtnetic organic dye of the azo group

[H+] > [OH-] PH = 0

[H+] = [OH-] PH = 7

[OH-] > [H+] PH = 14

Universal

Indicator for the variability of the edges of polymer strips, which determines the acidity of solutions.

[H+] > [OH-] PH = 0

[H+] = [OH-] PH = 7

[OH-] > [H+] PH = 14

The electron configuration is the formula for the location of electrons in the various electron shells of an atom of a chemical element or molecule. The electron configuration is usually written for atoms in their ground state.

The following rules exist for determining the electronic configuration of an element.

1. The Principles of Filling

According to the filling principle, electrons in the ground state of an atom fill the orbitals in the sequence of increasing orbital energy levels.

2. Pauli's Inhibition Principle

According to this principle, no more than two electrons can be on any orbital.

3. The Hund Principle

According to this rule, the filling of the orbitals of one subshell begins with single electrons, and only after the single electrons occupy all the orbitals can the final filling of the orbitals with electron pairs take place.