Mangan Nickel

Mangan Nickel

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All chemical compounds are colored, and in some cases it is distinctive or useful for identification. The study of the chemical structure through the adsorption and release of energy is generally known as spectroscopy.
Theory

The UV-vis spectrum for a compound that appears orange in dimethylformamide
All chemicals, including atoms, are capable of absorbing and releasing energy. The amount (s) of energy (quanta) absorbed and released is determined by the quantum structure of chemistry. The release of energy visible to humans extends through the eye of the wavelength between 380 nm and 760 nm and is commonly referred to as the color. The relationship between energy and the wavelength is determined by the equation:

where E is the energy of quanta (photons), h is Planck's constant,? is the wavelength and c is the speed of light. The relationship between structure chemistry and energy can be understood by atomic orbitals, molecular orbital or ligand field theory. In organic compounds the color can be determined by the difference between the highest occupied molecular orbital and lowest unoccupied molecular orbital. The energy absorbed and / or released, not a direct correlation with humans perceive as color. The absorption of a specific wavelength of light less effective from the full visible spectrum, and what we see is the complementary color, formed by the other visible wavelengths. Beta-carotene has an absorption maximum at 454 nm (blue) which consequently remains visible light is orange.
Colors by the wavelength
Below is a table of wavelengths about the colors and complementary colors.
Wavelength (nm)
Color
Complementary color
400-424
Violeta
Green-yellow
424-491
Blue
Yellow
491-570
Green
Red
570-585
Yellow
Blue
585-647
Orange
Green-Blue
647-700
Red
Green
Examples
Ions in aqueous solution
Name
Formula
Color
The alkali metals
M +
None
Alkali metals
M2 +
None
Scandium (III)
Sc3 +
None
Titanium (III)
Ti3 +
Violeta
Titanium
TiO2 +
None
Vanadium (II)
V2 +
Lavender
Vanadium (III)
V3 +
Dark gray / green
Vanadyl
VO2 +
Blue
Pervanadyl
VO2 +
Yellow
Metavanadate
VO3 --
None
Orthovanadate
VO43 --
None
Chromate
CrO4 2 --
Colorless or yellow (sometimes)
Dichromate
Cr2O72 --
Orange
Manganese (II)
Mn2 +
Light Pink
Manganate (VII) (permanganate)
MnO4 --
Deep Purple
Manganate (VI)
MnO42 --
Dark green
Manganese (V)
MnO43 --
Deep blue
Iron (II)
Fe2 +
Light blue
Iron (III)
Fe3 +
Yellow / brown
Cobalt (II)
CO2 +
Red light
Nickel (II)
Ni2 +
Green light
Nickel-ammonium complex
Ni (NH3) 62 +
Lavender / blue
Copper (II)
Cu 2 +
Blue
Copper-ammonium complex
Cu (NH3) 42 +
Royal Blue
Zinc (II)
Zn2 +
None
Silver
Ag +
None
It is important to note, however, that the basic colors will vary depending on what which are a complex, often, and its chemical status. An example with vanadium (III); VCl3 has a distinctive reddish Hue, while V2O3 is black.
Sales
Predicting the color of a compound can be extremely complicated. Examples include cobalt chloride is pink or blue, depending on the state of hydration (blue dry, pink water) so it is used as a moisture indicator silica gel. Zinc oxide is white, but at higher temperatures becomes yellow, turning to white as it cools.
Name
Formula
Color
Picture
Copper (II) sulfate
CuSO4
Blue
Copper (II) sulfate pentahydrate
CuSO4 5H2O
Blue
Cobalt (II)
CoCl2
Deep blue
Cobalt (II) hexahydrate
CoCl2 6H2O
Deep Magenta
Manganese (II) Chloride tetrahydrate
MnCl2 4H2O
Pink
Copper (II) chloride
CuCl2 2H2O
Blue-green
Nickel (II) hexahydrate
NiCl2 6H2O
Green
Oxidation Metals
Flame tests on alkali cations and alkaline earth metals
Name
Formula
Color
Potassium
K
Lilac / Purple
Sodium
Na
Yellow
Lithium
Li
Red
Cesium
Cs
Blue
Calcium
Ca
Red / Orange
Strontium
Sr
Red
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