Color of chemicals

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All chemical compounds have colors, and in some cases these are distinctive or useful for identification. The study of chemical structure by means of energy adsorption and release is generally referred to as spectroscopy.
Theory

The UV-vis spectrum for a compound that appears orange in Dimethylformamide
All chemical compounds, 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 the chemical. The release of energy visible to the human eye spans the wavelengths 380 nm to 760 nm and is commonly referred to as color. The relationship between energy and wavelength is determined by the equation:

where E is the energy of the quanta (photon), h is Planck’s constant, ? is the wavelength and c is the speed of light. The relationship between chemical structure and energy can be understood using atomic orbital, molecular orbital, or Ligand Field Theory. In organic compounds the color can be determined by the difference between the Highest Occupied Molecular Orbital and the Lowest Unoccupied Molecular Orbital. The energy absorbed and/or released does not directly correlate to what humans perceive as color. The absorption of a particular wavelength of light effectively subtracts it from the full visible spectrum, and what we see is the complementary color, made up of the other visible wavelengths. Beta-carotene has maximum absorption at 454 nm (blue light) consequently what visible light remains appears orange.
Colors by wavelength
Below is a rough table of wavelengths, colors and complementary colors.
Wavelength (nm)
Color
Complementary Color
400-424
Violet
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
Alkali metals
M+
None
Alkaline earth metals
M2+
None
Scandium (III)
Sc3+
None
Titanium (III)
Ti3+
Violet
Titanyl
TiO2+
None
Vanadium (II)
V2+
Lavender
Vanadium (III)
V3+
Dark grey/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 violet
Manganate (VI)
MnO42-
Dark green
Manganate (V)
MnO43-
Deep blue
Iron (II)
Fe2+
Light blue
Iron (III)
Fe3+
Yellow/brown
Cobalt (II)
Co2+
Light red
Nickel (II)
Ni2+
Light green
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 elemental colors will vary depending on what they are complexed with, often as well as their chemical state. An example with vanadium(III); VCl3 has a distinctive redish hue, whilst V2O3 appears black.
Salts
Predicting the color of a compound can be extremely complicated. Some examples include: Cobalt chloride is pink or blue depending on the state of hydration (blue dry, pink with water) so it’s used as a moisture indicator in silica gel. Zinc Oxide is white, but at higher temperatures becomes yellow, returning to white as it cools.
Name
Formula
Color
Picture
Copper (II) sulfate
CuSO4
Blue
Copper (II) sulfate pentahydrate
CuSO4 5H2O
Blue
Cobalt (II) chloride
CoCl2
Deep blue
Cobalt (II) chloride hexahydrate
CoCl2 6H2O
Deep magenta
Manganese(II) chloride tetrahydrate
MnCl2 4H2O
Pink
Copper(II) chloride dihydrate
CuCl2 2H2O
Blue-green
Nickel(II) chloride hexahydrate
NiCl2 6H2O
Green
Oxidising Metals
Flame Tests on cations for Alkali and Alkali 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
…(and so on) To get More information , you can visit some products about wall hung toilets, electrode holders, . The Double Desk with Chair products should be show more here!

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