Why does metal become ionic will show different colors

This is not something that can be explained in one or two sentences, so I will briefly talk about it. 1. The valence state of the ions is different, the color is different, the valency is different, the energy of the ions is different, and the colors displayed are different, such as ferric iron is green in water, and trivalent iron is yellow 2. 3. The state of the ions is related, the copper ions in the solid copper oxide are black, while the copper ions in the aqueous solution are blue.

4. The environment in which ions exist is related, for example, chromate is yellow under alkaline conditions and orange under acidic conditions. Beg.

When it becomes an ion, the energy of each valence state is different, and the macroscopic reaction is also different.

1. In the molecules (ions, atoms) that make up matter, electrons move within a certain orbital range, and this movement is not.

It is very stable, because the electrons in different orbitals have different energies, and the electrons may absorb energy from the lower energy orbitals at any time.

into a high-energy orbital, or emitting energy from a high-energy orbital into a low-energy orbital, this electronic transition in the energy changes to electromagnetic waves.

The form is manifested and further manifested as the color.

2. There are several reasons for the color difference of common transition metal ions:

1. There are different types of metal atoms.

2. The metal atoms are of the same type but have different valences.

3. The ligands of metal ions are different.

4. The coordination mode of metal ions is different.

5. Form metallic bonds.

For example, common iron ions and copper ions have abundant colors because the d orbital is not filled and there is an electron transition phenomenon; The zinc ion is a 3d10 structure and has no electronic transition, so it is often colorless.

Common ions and colors are as follows:

1. Permanganate ion MNO purple.

2. Manganate ion MNO green.

3. Chromic acid. Root ion cro yellow.

4. Dichromate ion cr o orange.

5. Copper ion cu blue.

6. Cuprous ion Cu: red.

7. Iron ions.

Fe brown.

8. Ferrous ion FE light green.

9. Cobalt ion co pink.

10. Manganese ion mn pale pink.

11. Bromine ion br: light yellow.

Features:

Ions are the elementary particles that make up ionic compounds.

Ionic compounds in any state (crystalline, molten state.

vapor state or solution) are in the form of ionic-liquid differences. Therefore, the properties of ions largely determine the ionic compounds.

nature. That is, the properties of ions, that is, the three important characteristics of ions: the charge of ions, the semi-diameter of ions, and the electron shell of ions.

The type of structure (referred to as the electron configuration of the ion) is the fundamental reason that determines the commonality and characteristics of ionic compounds.

The above content reference: Encyclopedia - Ion.

Colored ions are charged ions, some of which can absorb certain wavelengths of light, and the reflected or transmitted light has color. Here are some of the common colored ions:

1.Copper ions: Cu2+ ions are blue-green in color.

2.Iron ions: Fe3+ ions are yellow-brown or reddish-brown, Fe2+ ions are green.

3.Manganese ions: Mn2+ ions are pink and MnO4- ions are purple.

4.Cadmium ions: CD2+ ions are yellow in color.

5.Nickel ions: Ni2+ ions are green.

6.Chromium ions: Cr3+ ions are dark green, CR4- ions are yellow, and Cr2O7- ions are orange-red.

7.Cobalt ions: CO2+ ions are red or pink in color.

It should be noted that the color of the ion depends not only on the structure and composition of the ion itself, but also on the environment in which the ion is located, so the same ion will exhibit different colors in different compounds or mixed reed chain bends.

Many ions have colors. This is due to the arrangement of electrons inside their molecular structure. The following are some of the common dispersal ions of the Yan Chong Qi color and their descriptions:

1.Copper ion (Cu2+): Copper ion is a blue-green ion commonly found in copper salts.

2.Iron ions (Fe2+ and Fe3+): Iron ions come in different colors, Fe2+ is green and Fe3+ is yellow, and they can be converted in different chemical reactions.

3.Cadmium ion (CD2+): Cadmium is an orange ion that is commonly found in cadmium salts.

4.Chromium Ionizer Brigade (Cr3+ and Cr6+): Chromium ions come in different colors, Cr3+ is green and Cr6+ is orange, both of which are commonly found in chromium salts.

5.Manganese ion (mn2+): Manganese ion is a pink ion that is commonly found in manganese salts.

6.Cobalt ion (CO2+): Cobalt ion is a pink ion that is commonly found in cobalt salts.

In conclusion, many ions have colors and this is because they have different electronic structures. These colors can be used not only for analysis and testing in chemical laboratories, but also for the manufacture of dyes and pigments.

Many ions have colors, here are some examples:

1.Copper ion (Cu2+): blue-green.

2.Iron ions (Fe2+ or Fe3+): light green or yellowish brown.

3.Manganese ion (Mn2+): pink.

4.Cadmium ion (CD2+) deficit: yellow.

5.Chromium ion (CR3+): dark green.

6.Cobalt ion (CO2+): Pink.

The color of these ions is mainly due to the high cost of light they absorb at different wavelengths in a transparent medium. Specifically, the color they absorb is related to factors such as the position of the electrons in the molecule, the molecular structure, and the surrounding environment.

For example, the ferric ion is yellow, the copper ion is blue, and the permanganate ion is purple.

Common colored ions are:

Cu Copper Ion – Blue.

Fe ferrous ions – light green.

Fe Iron ion - light purple (usually brownish-yellow in solution).

mn manganese ion – light pink.

Cobalt ion – Pink.

Ni Nickel Ion – Green.

CR chromium ion – blue-green.

CR chromium ion – green.

cd cadmium ion – blue-green.

AU Gold Ion – Golden yellow.

MNO permanganate ion – fuchsia.

MNO manganate ion – dark green.

CRO4 - chromate ion - yellow.

Common metal ions are copper ions, ferrous ions, iron ions, sodium ions, and potassium ions.

The color of each ion is:

1. Copper ions, blue, the solution containing copper ions is blue;

2. Ferrous ions, light green medium mold, in the solution, add NaOH solution, produce a white early slow color gelatinous precipitation, quickly turn green;

3. Iron ions, yellow, yellow in solution;

4. Sodium ion, yellow, flame color reaction, flame color yellow;

5. Potassium ions, showing purple, flame color reaction, flame through the blue cobalt glass color file is purple.

Common metal ions include copper ions, ferrous ions, iron ions, sodium ions, and potassium ions.

The color of each ion is:

1. Copper ions, blue, the solution of cracked branches containing copper ions is blue;

2. Ferrous ions, light green, in the solution, add NaOH solution to produce a white gelatinous precipitate, which quickly turns green;

3. Iron ions, yellow, yellow in solution;

4. Sodium ion, yellow, flame color reaction, flame color yellow;

5. Potassium ions, purple, flame color reaction, flame through blue cobalt glass color purple.

Whether an ion can develop color is related to whether it can absorb visible light, and whether it can absorb visible light depends on the electronic shell structure of the ion. If the electron sublayers outside the nucleus are in a full state, that is, when there are no unpaired electrons, the structure is relatively stable, it is not easy to accept the excitation of light energy, it is not easy to absorb visible light, and it is colorless. The electro-layer structure of the transition metal ions mentioned above is less stable and generally contains an unfilled D sublayer with an unequal number of unpaired electrons.

These unstable electrons are susceptible to light excitation and undergo a transition, that is, the absorption and reflection of certain wavelengths of visible light, showing different colors.

For example, Mn2+ in solution is light pink, but Mn(OH)2 is white, and FeO and FeS are black. Generally speaking, the larger the radius of the negative ion, the more relaxed the peripheral electrons, and the darker the color of the compound or atomic cluster formed.

In addition to negative ions that can affect the color development of transition metal ions, water molecules also have a certain effect. The crystal or solution of copper sulfate appears beautiful blue, but when we put the blue copper sulfate crystal in the test tube and heat, the beautiful blue color will gradually disappear, and at the same time, the resulting water vapor will become liquid when it is cold, and then drip from the mouth of the test tube, like tears shed for the loss of beautiful color. At this point, all that is left in the tube is white powder.

Not only does the presence of water molecules affect the display of color, but the number of water molecules also plays a significant role. For example, cobalt chloride crystals, at room temperature, are pink; When heated to more than 52 and lost water, it becomes purple-red CoCl2·2H2O. Continue to heat to 90 to turn blue-purple CoCl2·H2O, and then reheat will lose all water and become blue CoCl2.

1.Typical ionic compounds generally do not absorb light in the visible region of the spectrum (generally ultraviolet light) and therefore appear white or colorless when exposed to white light.

2.When the chemical bonds between metal and non-metal atoms become more covalent, the electron density gradually shifts from anion to cation, and the charge transition is easier, and less energy is required. The absorbable band is shifted to the visible region.

At this time, the white light that was originally completely emitted is partially absorbed, and the reflected or transmitted light emitted at this time will be colored.

3.The depth of color rendering can determine the covalentity of the chemical bonds of metal atoms (excessive elements) with non-metal atoms... This is what the old man said about the electronic sublayer (spdfg......).

In essence, this is caused by the transition of electrons, according to the classical Maxwell's theory, electrons will be at a higher energy level after getting energy, from the principle of lowest energy, it can be seen that the electrons after absorbing energy are unstable and then transition, so as to reach a stable low-energy orbit, and the energy will be released in the form of electromagnetic waves, different particles absorb different energy, so after the transition, electromagnetic waves of different wavelengths are emitted, one of which is in the visible region, so it is what we call the flame color reaction.