Physical and chemical properties of zinc oxide. The use of zinc oxide in cosmetology and medicine
Zinc oxide ZnO - semiconductor connection. Zinc oxide - compound white color, which sublimates at 2000 K, melts at 2250 K, exhibits both basic and acidic properties, and dissolves in acids and alkalis.
The most common crystalline modification is the hexagonal wurtzite type. A rarer cubic sphalerite type is also known.
Zinc oxide can be obtained by burning or oxidizing zinc, by roasting zinc sulfide in air, by calcining
salts, precipitation with ammonia from a boiling aqueous solution of zinc nitrate.
Compact samples of zinc oxide (zincite) are obtained by pressing blanks from a powdered compound and their subsequent sintering. Preliminary sintering is carried out at 1100 K. Final sintering is carried out at 1700...1800 K. Heating is carried out either in special high-temperature furnaces or by direct current passing through the samples after they have been preheated to a temperature at which sufficient electrical conductivity occurs. At a final sintering temperature of 1700...1800 K, coarse-grained samples with crystals up to 2 mm are formed. To obtain a finer-grained structure, the sintering temperature is reduced to 1300...1400 K. Zinc oxide single crystals are grown by the hydrothermal method and from the gas phase.
Thin films of zinc oxide ZnO can be obtained by evaporation and condensation of zinc on a substrate in a vacuum, followed by oxidation of the metal film when heated in an oxygen atmosphere or reactive two-electrode ion sputtering Zn in an Ar + O 2 atmosphere.
ZnO thin films exhibit the piezoelectric effect.
Main properties of zinc oxide
Molecular weight 81.38
Crystal structure G
Permanent crystal lattice, nm:
A 0.3250
C 0.5206
Density, Mg / m 3 5.67
Temperature, K:
melting point 2250
boiling 2000
Specific heat capacity, J/(kg× K) 495
Temperature coefficient of linear expansion for
single crystal, α× I 0 6 , K -1 5.7 || a
5.2 || With
Resistivity, Ohm× cm 10 8 …10 9
Thermal conductivity coefficient, W/(m× K) 15…30
Mohs hardness 4.0…5.0
Refractive index 1.96
Dielectric constant 8.5
The use of zinc oxide.
Zinc oxide is used in radio electronics for the manufacture of self-activated phosphor ZnO:Zn. This phosphor is obtained by calcination ZnO in a weakly reducing atmosphere of carbon monoxide at 1270 K - The color of the glow of the phosphor is blue-green, the radiation is characterized by two maxima., attributable to wavelengths of 0.385 microns (ultraviolet region) and 0.505 microns (blue-green region of the spectrum). This phosphor has a very short afterglow, about 2 μs.
Zinc oxide has found its main application in the production of varistors, devices whose electrical resistance is highly dependent on the applied voltage. On the basis of varistors, surge arresters (SPDs) are created that suppress surges in power networks.
This is due to a special property of varistors - the nonlinearity of the current-voltage characteristic. Silicon carbide also has a non-linear current-voltage characteristic, but the non-linearity coefficient of varistors based on zinc oxide is 1-1.5 orders of magnitude higher.
For the manufacture of varistors, ZnO powder of submicron size, oxides of other metals ~5% (bismuth, cobalt, antimony, manganese, chromium) and inorganic binders are mixed, molded under a pressure of ~10 4 ... 10 6 MPa and fired for several hours at temperatures from 1200 to 1600 °C. During the reaction interaction, the material is transferred through the liquid phase from zinc oxide grains with a high surface energy to grains with a lower surface energy. The material is compacted during sintering, and as a result a new polycrystalline structure is obtained.
A zinc oxide varistor is a polycrystalline semiconductor material whose individual grains are in electrical contact with each other. At the contact points of zinc oxide grains, there are thin insulating regions, which cause the nonlinearity of the current-voltage characteristic. The mechanism of non-linearity of varistors is not well understood. Most likely, the nonlinearity is due to the phenomena at grain boundaries, and additional additives in the composition of varistors also have a decisive influence.
- Designation - Zn (Zincum);
- Period - IV;
- Group - 12 (IIb);
- Atomic mass - 65.39;
- Atomic number - 30;
- Radius of an atom = 138 pm;
- Covalent radius = 125 pm;
- Electron distribution - 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 ;
- melting point = 419.88°C;
- boiling point = 907°C;
- Electronegativity (according to Pauling / according to Alpred and Rochov) = 1.65 / 1.66;
- Oxidation state: +2, 0;
- Density (n.a.) \u003d 7.13 g / cm 3;
- Molar volume = 9.2 cm 3 / mol.
Zinc was used by people even before our era in the form of its alloy with copper - brass. For the first time, pure zinc was isolated by the Englishman William Champion in the 18th century.
V earth's crust zinc contains 8.3 10 -3% by weight. A lot of zinc is found in thermal springs, from which zinc sulfides, which are of great industrial importance, precipitate. Zinc plays an active role in the life of animals and plants, being an important biogenic trace element.
Rice. The structure of the zinc atom.
The electronic configuration of the zinc atom is 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 (see Electronic structure of atoms). The penultimate electron layer of the zinc atom is completely filled, and on outer layer there are two s-electrons, which interact with other elements, therefore, the oxidation state +2 is manifested in zinc compounds. (see Valency). Zinc has a high chemical activity.
Physical properties of zinc:
- bluish white metal;
- fragile at n. y.;
- when heated above 100°C, it is well forged and rolled;
- has good thermal and electrical conductivity.
Chemical properties of zinc:
- in air, it quickly oxidizes, becoming covered with a thin film of zinc oxide, which protects the metal from further reaction;
- when heated, it reacts with oxygen, chlorine, sulfur, forming oxides, chlorides, sulfides, respectively:
2Zn + O 2 = 2ZnO; Zn + Cl 2 \u003d ZnCl 2; Zn + S = ZnS. - reacts with dilute sulfuric acid and non-oxidizing acid solutions, displacing hydrogen from them:
Zn + H 2 SO 4 (rzb.) \u003d ZnSO 4 + H 2; Zn + 2HCl \u003d ZnCl 2 + H 2; - reacts with nitric and concentrated sulfuric acid, reducing nitrogen or sulfur, respectively:
Zn + H 2 SO 4 (knc.) \u003d ZnSO 4 + SO 2 + 2H 2 O; - reacts when heated with alkali solutions, forming hydrozincates: Zn + 2NaOH + 2H 2 O \u003d Na 2 + H 2;
- displaces less active metals (see the electrochemical series of metal voltages) from solutions of their salts: Zn + CuCl 2 = ZnCl 2 + Cu.
Getting zinc:
- pure zinc is obtained by electrolysis of its salts;
- Zinc is obtained industrially from sulfide ores:
- at the first stage, zinc oxide is obtained by subjecting the ore to oxidative roasting: 2ZnS + 3O 2 = 2ZnO + 2SO 2;
- at the second stage, zinc oxide is reduced with coal at a high temperature: ZnO + C = Zn + CO.
Applications of zinc:
- as an anticorrosive coating of metal products (galvanizing);
- for the manufacture of alloys widely used in mechanical engineering;
- in batteries and dry cells;
- in the paint and varnish industry (production of zinc white);
- as a reducing agent in organic synthesis reactions.
Topic 28
Group IIB elements: zinc, cadmium, mercury
General characteristics.
The elements of this subgroup are complete electronic analogues of each other, each in its period is the last element of the d-family, they have completed d- electronic configuration, valence electrons (n-1)d 10 ns 2 . On the outside electron shell contains 2 electrons and 18 electrons on the previous shell. Zinc and its analogs differ from d-elements and show more similarity with p-elements of large periods.
For zinc, cadmium and mercury atoms, as well as for copper atoms, the (n-1)d-sublevel is completely filled and quite stable. Removing electrons from it requires a very large expenditure of energy. Therefore, the elements under consideration exhibit the maximum oxidation state +2 in their compounds. Only mercury forms compounds in which its oxidation state is +1.
characteristic feature elements is their tendency to complex formation (c.h. = 4; 6).
In contrast to the elements of the main subgroups, the elements of the zinc subgroup are more difficult to oxidize, exhibit less reactivity, and exhibit weaker metallic properties.
In the subgroup from top to bottom: the atomic radius increases, the melting and boiling points decrease, the electronegativity and electrode potential increase. The minimum ionization energy is observed for cadmium (8.99 eV), since. the properties of mercury are affected by lanthanide compression, as a result of which its ionization energy increases to 10.43 eV (for zinc, 9.39 eV).
Distribution and main minerals.
ZnS - zinc blende,
HgS - cinnabar,
ZnCO 3 - galmei,
CdS is greenockite.
Natural zinc compounds are part of polymetallic sulfide ores, which contain pyrite FeS 2 , galena PbS, chalcopyrite CuFeS 2 , and less ZnS. Mercury is a rare element and occurs naturally.
Metallic zinc, its production, properties and application.
Silver-white soft metal, covered with an oxide film in air. It has no polymorphic modifications, it is diamagnetic. The external electronic configuration of the Zn atom is 3d 10 4s 2 . The oxidation state in compounds is +2. The normal redox potential of 0.76 V characterizes Zinc as an active metal and an energetic reducing agent.
To isolate zinc, the ZnS concentrate obtained after enrichment is subjected to roasting, and the resulting oxide is reduced with coal:
2ZnS + 3O 2 = 2ZnO + 2SO 2
ZnO + C = Zn + CO
Another way is that the ore containing ZnS is roasted and then treated with dilute sulfuric acid:
ZnO + H 2 SO 4 \u003d ZnSO 4 + H 2 O
The resulting solution of zinc sulfate is subjected to electrolysis.
In terms of chemical activity, the zinc subgroup is inferior to alkaline earth metals. In a subgroup with increasing atomic mass chemical activity metal decreases, as evidenced by the values of the standard electrode potentials (see above). Zinc is a reactive metal, easily soluble in acids and, when heated, in alkalis:
Zn + 2HCl \u003d ZnCl 2 + H 2 Zn + H 2 SO 4 (solution) \u003d ZnSO 4 + H 2
These reactions are slow because the resulting atomic hydrogen coats the surface of the zinc.
Zn + 2H 2 SO 4 (conc.) = ZnSO 4 + SO 2 + H 2 O
4Zn + 10HNO 3 = 4Zn(NO 3) 2 + NH 4 NO 3 + 3H 2 O
Zn + 2NaOH + 2H 2 O \u003d Na 2 + H 2
Metallic zinc displaces less active metals and reduces H2CrO4, HMnO4, iron (III) and tin (IV) salts:
5Zn + 2KMnO 4 + 8H 2 SO 4 (p - p) \u003d 2MnSO 4 + 5ZnSO 4 + K 2 SO 4 + 8H 2 O
Zn + CuSO 4 \u003d ZnSO 4 + Cu
The use of zinc is varied. An alloy is prepared from zinc with aluminum, copper, magnesium, which are of industrial importance. A significant part of the zinc is used for coating iron and steel products, which protect the base metal from corrosion.
Zinc oxide and hydroxide.
zinc oxide- loose white powder, turning yellow when heated, but turning white again when cooled, a semiconductor. Zinc oxide amphoterene - reacts with acids to form salts; when interacting with alkali solutions, it forms complex tri-tetra- and hexahydroxy zincates (Na 2, Ba 2):
ZnO + 2HCl \u003d ZnCl 2 + H 2
ZnO + 2NaOH + 2H 2 O Na 2 + H 2
Zinc oxide dissolves in aqueous solution ammonia, forming complex ammonia:
ZnO + 4NH 3 + H 2 O - (OH) 2
When fused with alkalis and metal oxides, zinc oxide forms zincates:
ZnO + 2NaOH Na 2 ZnO 2 + H 2 O
ZnO + CoO CoZnO 2
When fused with oxides of boron and silicon, zinc oxide forms vitreous borates and silicates:
ZnO + B 2 O 3 Zn(BO 2) 2
ZnO + SiO 2 ZnSiO 3
At temperatures above 1000 ° C, it is reduced to metallic zinc with carbon, carbon monoxide and hydrogen:
ZnO + C = Zn + CO
ZnO + CO = Zn + CO 2
ZnO + H 2 \u003d Zn + H 2 O
Does not react with water. When interacting with non-metal oxides, it forms salts, where it is a cation:
2ZnO + SiO 2 = Zn 2 SiO 4
ZnO + B 2 O 3 \u003d Zn (BO 2) 2
Obtained by burning zinc metal:
2Zn + O 2 = 2ZnO
at thermal decomposition salts:
ZnCO 3 \u003d ZnO + CO 2
Zinc oxide is used for the manufacture of white oil paint (zinc white), in medicine and cosmetics (for the manufacture of various ointments); a significant portion of zinc oxide is used as a rubber filler.
Zinc hydroxide- a colorless crystalline or amorphous substance. At temperatures above 125°C decomposes:
Zn(OH) 2 = ZnO + H 2 O
Zinc hydroxide exhibits amphoteric properties, easily soluble in acids and alkalis:
Zn(OH) 2 + H 2 SO 4 (conc) = ZnSO 4 + 2H 2 O
Zn(OH) 2 + 2NaOH \u003d Na 2
also readily soluble in aqueous ammonia to form tetraamminzinc hydroxide:
Zn (OH) 2 + 4NH 3 \u003d (OH) 2
It is obtained in the form of a white precipitate when zinc salts react with alkalis:
ZnCl 2 + 2NaOH = Zn(OH) 2 + 2NaCl
Ministry of Education and Science of the Russian Federation
federal state budgetary educational institution
higher professional education
PETROZAVODSK STATE UNIVERSITY
Faculty of Medicine
Abstract on the discipline "Pharmaceutical chemistry"
Topic: Zinc oxide. zinc sulfate.
The work was done by a 4th year student
Specialty: Pharmacy
Correspondence department
Group: 73Z42
Rigoeva Anna Sergeevna
Work checked
Teacher:
Ermakova Galina Vladimirovna
Petrozavodsk 2012
Zinc is an element of a side subgroup of the second group, the fourth period of the periodic system chemical elements D. I. Mendeleev, with atomic number 30.
It is designated by the symbol Zn (lat. Zincum).
A simple substance zinc under normal conditions is a brittle transition metal of a bluish-white color (it tarnishes in air, becoming covered with a thin layer of zinc oxide).
A typical example of a metal that forms amphoteric compounds. Zinc compounds ZnO and Zn(OH)2 are amphoteric. The standard electrode potential is −0.76 V, in the series of standard potentials it is located before iron.
In air, zinc is covered with a thin film of ZnO oxide. When heated strongly, it burns out with the formation of amphoteric white oxide ZnO:
Zinc oxide reacts both with acid solutions:
and alkalis:
Zinc of ordinary purity actively reacts with acid solutions:
and alkali solutions: forming hydroxo-zincates. Very pure zinc does not react with solutions of acids and alkalis. The interaction begins with the addition of a few drops of a solution of copper sulfate CuSO4.
When heated, zinc reacts with halogens to form ZnHal2 halides. With phosphorus, zinc forms phosphides Zn3P2 and ZnP2. With sulfur and its analogues - selenium and tellurium - various chalcogenides, ZnS, ZnSe, ZnSe2 and ZnTe.
Zinc does not directly react with hydrogen, nitrogen, carbon, silicon and boron. Nitride Zn3N2 is obtained by the reaction of zinc with ammonia at 550-600 °C.
In aqueous solutions, zinc ions Zn2+ form aquacomplexes 2+ and 2+.
zinc sulfate
ZnSO4, colorless crystals. Dissolves in water. ZnSO4 7H2O crystallizes from solutions - zinc vitriol. It is used in the production of viscose, glazes, to protect wood from decay.
ZINC SULFATE
ZINC SULPHATE (zinc sulfate) Zinci sulfas, ZnSO4. ZnSO4 · 7H2O - zinc vitriol - crystallizes from solutions. It is used in the production of viscose, glazes, to protect wood from decay.
Characteristic:
Colorless transparent crystals or fine crystalline powder, astringent taste, odorless. It vanishes in the air. Very easily soluble in water, practically insoluble in ethanol, slowly soluble in glycerin (1:10). Aqueous solutions are acidic.
Zinc sulfate has an antimicrobial, astringent, drying and local anti-inflammatory effect.
Application:
Conjunctivitis, laryngitis, urethritis, vaginitis - locally; the need to induce vomiting - inside in high doses; zinc deficiency in the body with violations of anabolic, immunological and other processes (prevention and treatment) - inside; hypogonadism, alopecia areata, cerebral palsy, liver disease, diabetes mellitus, diffuse connective tissue diseases, etc. (as part of complex therapy) - inside.
Contraindications:
Hypersensitivity.
Side effects:
Nausea, vomiting, diarrhea (when taking high doses orally).
Zinc sulfate, zinc sulfate, ZnSO4 - zinc salt of sulfuric acid.
Colorless crystals, density 3.74 g/cm³. Solubility in water (%): 29.4 (0°C), 37.7 (99°C). ZnSO4 7H2O (zinc vitriol) crystallizes from solutions at temperatures below 38.8 °C, ZnSO4 6H2O crystallizes in the range from 38.8 °C to 70 °C, and ZnSO4 H2O monohydrate forms above 70 °C. The latter is dehydrated at 238°C. Zinc sulfate in the range of 600-900 °C decomposes into ZnO and SO3. Weak solutions of zinc sulfate become cloudy during hydrolysis due to the precipitation of 3Zn(OH)2 ZnSO4 4H2O.
Receipt
Zinc vitriol is obtained by evaporation and crystallization from solutions (along with the production of zinc). Zn+H2SO4=ZnSO4+H2
Application
It is used in the production of viscose, mineral paints, glazes, in metallurgy (flotation agent) and in medicine.
Active-active substance / beginning: zinc (zinc sulfate, picolinate, asparaginate)
Bio-zinc; Solgar zinc picolinate; zinc sulfate; Zinc aspartate; Zinc picolinate; zinc sulfate; Zincite; Zincteral.
It is used for liver diseases (cirrhosis), enteritis, enteropathic dermatitis, psoriasis, collagenosis (rheumatoid arthritis, lupus erythematosus), cerebral palsy, frequent colds. Topically used for conjunctivitis, laryngitis, urethritis, vaginitis.
Zinc (zinc sulfate, picolinate, aspartate).
Dosage forms:
Effervescent tablets.
Eye drops.
Solution for external use.
Zinc (zinc sulfate, picolinate, aspartate)
Properties / Action:
Zinc is an essential trace element. It is an integral part of more than 90 different enzymes that synthesize DNA and participate in metabolic processes. Zinc stimulates the synthesis of nucleic acids, proteins, tissue regeneration, promotes weight gain. Zinc is necessary for the functioning of insulin, hormones of the gonads, maintains the stability of cell membranes, limiting the release of histamine from mast cells. It limits free radical reactions, prevents damage cell membranes. Zinc is necessary for the normal activity of lymphoid tissue, alkaline phosphatase, carboxypeptidases, alcohol dehydrogenase.
Zinc increases resistance to infectious diseases, promotes wound healing, accelerates growth, increases efficiency, improves memory, and prevents hair loss.
Certain populations, such as pregnant women, breastfeeding mothers, teenagers, athletes, and consistent vegetarians, have an increased need for zinc. Zinc deficiency can be caused by insufficient intake or malnutrition, unbalanced diets, impaired absorption of zinc (for example, with intestinal diseases), or increased excretion of zinc, for example, with alcoholism, taking laxatives or other medications.
Indications:
Elimination of hypozincemia, incl. with violations of anabolic, immunological and other processes, which can occur with liver diseases (especially with cirrhosis), steatorrhea, enteritis, helminthic invasion, enteropathic acrodermatitis, psoriasis, with kidney diseases, hypovitaminosis D, with burns.
Prophylactically in the following conditions: diabetes mellitus, collagenosis (rheumatoid arthritis, lupus erythematosus), hypogonadism, alopecia areata, cerebral palsy, frequent colds, glucocorticoids, pregnancy and lactation.
Locally (zinc sulfate):
Conjunctivitis, laryngitis, urethritis, vaginitis.
Dosage and administration:
On an empty stomach, in dragee or effervescent tablets. For the prevention of hypozincemia 10 mg of zinc 1-2 times a day. WITH therapeutic purpose- 20-50 mg 2-3 times a day.
Locally (zinc sulfate):
With conjunctivitis - eye drops of 0.1-0.5%, with laryngitis - lubrication or spraying with a 0.25-0.5% solution, with urethritis and vaginitis - douching with a 0.1-0.5% solution.
Overdose:
Possible when taken orally: fever, impaired lung function, dehydration, plasma electrolyte imbalance, lethargy, muscle movement disorders, renal failure.
Contraindications:
active autoimmune processes, especially immune encephalitis;
acute renal failure, severe parenchymal lesions of the kidneys.
Use during pregnancy and lactation:
Application is possible only with a proven deficiency of zinc in the body.
Side effect:
Appears when taking large doses. At the same time, dyspeptic disorders (nausea, vomiting, diarrhea), dehydration, imbalance of electrolytes in blood plasma, lethargy, and renal failure are observed.
When used in therapeutic doses, complications are extremely rare.
Storage conditions:
At room temperature no higher than 25C.
Keep out of the reach of children.
Expiry dates are indicated on the packaging. The drug cannot be used after the expiration date.
Vacation from the pharmacy: without a doctor's prescription.
zinc oxide (Zincioxidum)
White or white with a yellowish tint amorphous powder, odorless. Absorbs carbon dioxide from the air .
Practically insoluble in water and alcohol, soluble in alkali solutions, diluted mineral acids, and also in acetic acid.
When heated, the substance changes color: white at room temperature, zinc oxide becomes yellow. This is explained by a decrease in the band gap and a shift of the edge in the absorption spectrum from the UV region to blue.
Zinc oxide amphoterene - reacts with acids to form salts, when interacting with alkali solutions, it forms complex tri-tetra- and hexahydroxy zincates (Na2, Ba2):
OH-2-
Zinc oxide dissolves in an aqueous solution of ammonia, forming complex ammonia:
ZnO + 4NH3 + H20 - (OH)2
When fused with alkalis and metal oxides, zinc oxide forms zincates:
ZnO + 2NaOH Na2ZnO2 + H2O
ZnO + CoO CoZnO2
When fused with oxides of boron and silicon, zinc oxide forms vitreous borates and silicates:
ZnO + B2O3 Zn(BO2)2
ZnO + SiO2 ZnSiO3
Receipt
natural mineral zincite
combustion of zinc vapor in oxygen ("French process")
thermal decomposition of compounds:
acetate Zn(CH3COO)2
hydroxide Zn(OH)2
carbonate ZnCO3
nitrate Zn(NO3)2
oxidative roasting of ZnS sulfide
hydrothermal synthesis
extraction from dust and sludge from metallurgical plants, especially those that work on scrap metal as a raw material (it contains a significant proportion of galvanized iron).
extraction from the ternary phase equilibrium system "zinc nitrate-amine nitrate-water" (with pyridine and quinoline nitrate, the particle size is about 5-10 nm up to 75%)
Application
vulcanization activator of some rubbers
vulcanizing agent for chloroprene rubbers
methanol synthesis catalyst
white pigment in the production of paints and enamels (currently (2007) replaced by non-toxic titanium dioxide TiO2)
filler and pigment in production:
plastics
perfumery and cosmetics
In medicine, in the form of powders and as part of ointments as an antiseptic.
animal feed additive
in the production of glass and paints based on liquid glass
as one of the rust converter components
It is also known that zinc oxide has photocatalytic activity, which is used in practice to create self-cleaning surfaces, bactericidal coatings for walls and ceilings in hospitals, etc. Zinc oxide is not currently used for industrial-scale photocatalytic water purification.
In addition, zinc oxide powder is a promising material as a working medium for powder lasers. Based on zinc oxide, a blue LED was created. Thin films and other nanostructures based on zinc oxide can be used as sensitive gas and biological sensors.
The properties of zinc oxide make it widely used in the pharmaceutical industry. Zinc oxide has found wide application in the creation of abrasive toothpastes and cements in therapeutic dentistry, in sunscreens and cosmetic procedures, in the production of electrical cables, artificial leather and rubber products. In addition, the application is widespread in the tire, paint and varnish, oil refining industries. Zinc oxide is involved in the production of glass and ceramics.
Zinc oxide preparations are anti-inflammatory dermatotropic agents with a drying effect for external use. Zinc oxide also has an adsorbing, astringent and antiseptic effect; forms albuminates and denatures proteins. Reduces the phenomena of exudation, inflammation and irritation of tissues, forms a protective barrier against the action of irritating factors. Softens irritated skin. It is used as a remedy with a protective effect in eczema (in the acute stage), dermatitis (diaper dermatitis, contact dermatitis), diaper rash, prickly heat, bedsores, superficial wounds, cuts, scratches, burns, ulcerative skin lesions, herpes simplex, streptoderma, trophic ulcers.
Active active ingredient:
Zinc oxide / Zinc oxide.
Dosage forms:
Liniment.
zinc oxide
Properties / Action:
Zinc oxide exhibits a weak astringent effect and is used as a protective agent for eczema and skin flaking.
Indications:
intertrigo;
dermatitis, incl. diaper dermatitis (diaper rash in infants), contact dermatitis;
bedsores;
superficial wounds, cuts, scratches;
burns (thermal, solar);
ulcerative skin lesions;
eczema in the acute stage;
simple herpes;
streptoderma;
trophic ulcers.
Dosage and administration:
Zinc oxide preparations are used externally, in the form of an ointment, paste, liniment.
Wash and dry the affected area. Apply to cleansed and dried skin.
Zinc oxide preparations are applied in a thin layer to the affected areas of the skin 4-6 times a day.
The course of treatment is up to 1 month.
The amount of the drug applied depends on the extent of the lesion.
Minor thermal and sunburns, cuts, scratches, wounds - apply a thin layer on the affected surface, if necessary, apply a gauze bandage.
Diaper rash in children - if the first signs of hyperemia, diaper rash or minor skin irritation appear, the ointment is applied 3 or more times a day, if necessary, during each diaper change; prophylactically treat areas of the body that are in prolonged contact with wet linen.
Contraindications:
individual intolerance (including history of hypersensitivity) to zinc oxide.
Side effects:
Allergic reactions (skin itching, hyperemia, skin rash).
Special instructions and precautions:
For external use only. Avoid contact with eyes.
The ointment is applied only to superficial and non-infected lesions and is not used to treat pustular skin lesions. Not intended for prescribing treatment without the participation of a doctor.
The drug is not contraindicated during pregnancy and lactation.
Drug interaction:
Not described.
Storage conditions:
At temperatures up to 30°C, away from heat sources and direct sunlight.
The shelf life is indicated on the packaging.
Vacation from a pharmacy - without a doctor's prescription.
Structural formula
Russian name
Latin name for zinc oxide
Zinci oxydum ( genus. Zinci oxydi)Gross formula
ZnOPharmacological group of the substance Zinc oxide
Nosological classification (ICD-10)
CAS code
1314-13-2Characteristics of the substance Zinc oxide
Anti-inflammatory agent for local use. White or white with a yellowish tint amorphous powder, odorless. Absorbs from the air carbon dioxide. Practically insoluble in water and ethanol, soluble in dilute mineral acids and acetic acid, in alkali solutions.
Pharmacology
pharmachologic effect- antiseptic, astringent, drying.Forms albuminates and denatures proteins. When applied to the affected skin surface, it reduces the severity of exudative processes, eliminates local manifestations of inflammation and irritation; has an adsorbing effect, forms a protective coating on the skin, which reduces the impact of irritating factors on it. Applied externally in the form of powder, ointment, paste, liniment.
Application of the substance Zinc oxide
Dermatitis, including diaper dermatitis (treatment and prevention), diaper rash, prickly heat; superficial wounds and burns (including sunburns, cuts, scratches), ulcerative skin lesions (including trophic ulcers), bedsores; eczema in the acute stage, herpes simplex, streptoderma.
Contraindications
Hypersensitivity.
Routes of administration
Outwardly.
Substance precautions Zinc oxide
Avoid contact with eyes.
Interactions with other active substances
Trade names
| Name | The value of the Wyshkovsky Index ® |
