Manganese. Manganese compounds Hydrogen compound of manganese
IN 1. Establish a correspondence between the formula of a substance and the value of the oxidation state of sulfur in it:
FORMULA OF THE SUBSTANCE OXIDATION DEGREE
A) NaHSO3 1) -2
B) SO3 2) -1
B) MgS 3) 0
D) CaSO3 4) +4 5) +6
IN 2. Establish a correspondence between the name of the substance and the type of bond between the atoms in it: NAME OF THE SUBSTANCE TYPE OF COMMUNICATION
A) calcium fluoride 1) covalent non-polar
B) silver 2) covalent polar
C) carbon monoxide (IV) 3) ionic
D) chlorine 4) metal
IN 3. Establish a correspondence between the electronic configuration of the external energy level of the atoms of a chemical element and the formula of its volatile hydrogen compound:
ELECTRONIC FORMULA FORMULA OF A VOLATILE HYDROGEN COMPOUND
A) ns2np2 1) HR
B) ns2np3 2) RH3
B) ns2np4 3) H2R
D) ns2np5 4) RH4
C1. What mass of precipitate is formed when 448 liters of carbon dioxide (N.O.) are passed through an excess of calcium hydroxide solution?
1) EO3
2) E2O7
3) E2O3
4)EO2
2. Valency of arsenic in a volatile hydrogen compound:
1) II
2) III
3)V
4) I
3. The most pronounced metallic properties are expressed in the element:
1) II group, secondary subgroup, 5 periods.
2) II group, main subgroup, 2 periods
2) Group I, main subgroup, 2 periods
4) Group I, main subgroup, 3 periods.
4. A series in which the elements are arranged in ascending order of electronegativity is:
1) AS,N,P
2) P,Si.Al
3) Te, Sc, S
4) F, Cl, Br
hydrogen compound and hydroxide. What properties (basic, acidic or amphoteric) do they have? Make up its graphical formula and determine the valence possibilities of an atom of this chemical element
Please help me paint the element, according to the plan :) Sr1) the name of the chemical element, its symbol
2) Relative atomic mass (round to the nearest whole number)
3) serial number
4) the charge of the nucleus of an atom
5) the number of protons and neutrons in the nucleus of an atom
6) total number of electrons
7) the number of the period in which the element is located
8) group number and subgroup (main and secondary) in which the element is located
9) diagram of the structure of the atom (distribution of electrons over electronic layers)
10) electronic configuration of an atom
11) chemical properties of a simple substance (metal or non-metal), comparison of the nature of properties with neighbors by subgroup and period
12) maximum oxidation state
13) the formula of the higher oxide and its nature (acidic, amphoteric, basic), characteristic reactions
14) the formula of the higher hydroxide and its nature (acidic, amphoteric, basic), characteristic reactions
15) minimum oxidation state
16) the formula of a volatile hydrogen compound
2. Three particles: Ne0, Na+ u F- - have the same:
A) the number of protons;
B) the number of neutrons;
B) mass number;
D) the number of electrons.
3. The ion has the largest radius:
4. From the following electronic formulas, select the one that corresponds to the d-element of the 4th period: a) ..3s23p64s23d5;
B)..3s23p64s2;
C) ... 3s23p64s23d104s2;
D)..3s23p64s23d104p65s24d1.
5. The electronic formula of the atom is 5s24d105p3. The formula for its hydrogen compound is:
6. From the following electronic formulas, select the one that corresponds to the element that forms the highest oxide of the composition R2O7:
B)..3s23p64s23d5;
D)..4s23d104p2.
7. A number of elements, arranged in order of strengthening non-metallic properties:
A) Mg, Si, Al;
8. The most similar physical and chemical properties are simple substances formed by chemical elements:
9. The nature of oxides in the series P2O5 - SiO2 - Al2O3 - MgO changes:
A) from basic to acidic;
B) from acidic to basic;
C) from basic to amphoteric;
D) from amphoteric to acidic.
10. The nature of higher hydroxides formed by elements of the main subgroup of group 2 changes with increasing serial number:
A) from acidic to amphoteric;
B) from basic to acidic;
C) from amphoteric to basic;
D) from acidic to basic.
Manganese is a hard gray metal. Its atoms have an outer shell electron configuration
Metal manganese interacts with water and reacts with acids to form manganese (II) ions:
In various compounds, manganese detects oxidation states. The higher the oxidation state of manganese, the greater the covalent nature of its corresponding compounds. With an increase in the oxidation state of manganese, the acidity of its oxides also increases.
Manganese(II)
This form of manganese is the most stable. It has an external electronic configuration with one electron in each of the five -orbitals.
In an aqueous solution, manganese (II) ions are hydrated, forming a pale pink hexaaquamanganese (II) complex ion. This ion is stable in an acidic environment, but forms a white precipitate of manganese hydroxide in an alkaline environment. Manganese (II) oxide has the properties of basic oxides.
Manganese (III)
Manganese (III) exists only in complex compounds. This form of manganese is unstable. In an acidic environment, manganese (III) disproportionates into manganese (II) and manganese (IV).
Manganese (IV)
The most important manganese(IV) compound is the oxide. This black compound is insoluble in water. It has an ionic structure. The stability is due to the high lattice enthalpy.
Manganese (IV) oxide has weakly amphoteric properties. It is a strong oxidizing agent, for example displacing chlorine from concentrated hydrochloric acid:
This reaction can be used to produce chlorine in the laboratory (see section 16.1).
Manganese(VI)
This oxidation state of manganese is unstable. Potassium manganate (VI) can be obtained by fusing manganese (IV) oxide with some strong oxidizing agent, such as potassium chlorate or potassium nitrate:
Manganate (VI) potassium has a green color. It is stable only in alkaline solution. In an acidic solution, it disproportionates into manganese (IV) and manganese (VII):
Manganese (VII)
Manganese has such an oxidation state in a strongly acidic oxide. However, the most important manganese(VII) compound is potassium manganate(VII) (potassium permanganate). This solid dissolves very well in water, forming a dark purple solution. Manganate has a tetrahedral structure. In a slightly acidic environment, it gradually decomposes, forming manganese (IV) oxide:
In an alkaline environment, potassium manganate (VII) is reduced, forming first green potassium manganate (VI), and then manganese (IV) oxide.
Potassium manganate (VII) is a strong oxidizing agent. In a sufficiently acidic environment, it is reduced, forming manganese(II) ions. The standard redox potential of this system is , which exceeds the standard potential of the system, and therefore the manganate oxidizes the chloride ion to chlorine gas:
Oxidation of the chloride ion manganate proceeds according to the equation
Potassium manganate (VII) is widely used as an oxidizing agent in laboratory practice, for example
to obtain oxygen and chlorine (see ch. 15 and 16);
for carrying out an analytical test for sulfur dioxide and hydrogen sulfide (see Ch. 15); in preparative organic chemistry (see Ch. 19);
as a volumetric reagent in redox titrimetry.
An example of the titrimetric application of potassium manganate (VII) is the quantitative determination of iron (II) and ethanedioates (oxalates) with it:
However, since potassium manganate (VII) is difficult to obtain in high purity, it cannot be used as a primary titrimetric standard.
] interpreted it as a 0-0 transition band associated with the ground state of the molecule. He attributed the weaker bands 620nm (0-1) and 520nm (1-0) to the same electronic transition. Nevin [42NEV, 45NEV] performed an analysis of the rotational and fine structure of the 568 and 620 nm (5677 and 6237 Å) bands and determined the type of the 7 Π - 7 Σ electronic transition. Later works [48NEV/DOY, 52NEV/CON, 57HAY/MCC] analyzed the rotational and fine structure of several more bands of the 7 Π - 7 Σ (A 7 Π - X 7 Σ +) transition of MnH and MnD.
Methods of high-resolution laser spectroscopy made it possible to analyze the hyperfine structure of lines in the 0-0 band A 7 Π - X 7 Σ + , due to the presence of a nuclear spin in the manganese isotope 55 Mn (I=2.5) and proton 1 H (I=1/2) [ 90VAR/FIE, 91VAR/FIE, 92VAR/GRA, 2007GEN/STE].
The rotational and fine structure of several MnH and MnD bands in the near-IR and violet spectral regions was analyzed in [88BAL, 90BAL/LAU, 92BAL/LIN]. It has been established that the bands belong to four quintet transitions with a common lower electronic state: b 5 Π i - a 5 Σ + , c 5 Σ + - a 5 Σ + , d 5 Π i - a 5 Σ + and e 5 Σ + - a 5 Σ + .
The vibrational-rotational spectrum of MnH and MnD was obtained in the works. The analysis of the rotational and fine structure of vibrational transitions (1-0), (2-1), (3-2) in the ground electronic state X 7 Σ + is performed.
The spectra of MnH and MnD in a low-temperature matrix were studied in [78VAN/DEV, 86VAN/GAR, 86VAN/GAR2, 2003WAN/AND]. The vibrational frequencies of MnH and MnD in solid argon [78VAN/DEV, 2003WAN/AND], neon and hydrogen [2003WAN/AND] are close to ΔG 1/2 in the gas phase. The value of the matrix shift (maximum in argon for MnH ~ 11 cm–1) is typical for molecules with a relatively ionic nature of the bond.
The electron paramagnetic resonance spectrum obtained in [78VAN/DEV] confirmed the symmetry of the 7 Σ ground state. The hyperfine structure parameters obtained in [78VAN/DEV] were refined in [86VAN/GAR, 86VAN/GAR2] by analyzing the electron-nuclear double resonance spectrum.
The photoelectron spectrum of MnH - and MnD - anions was obtained in [83STE/FEI]. The spectrum identified transitions both to the ground state of a neutral molecule and those excited with energies T 0 = 1725±50 cm -1 and 11320±220 cm -1 . For the first excited state, a vibrational progression from v = 0 to v = 3 was observed, vibrational constants w e = 1720±55 cm -1 and w e x e = 70±25 cm -1 . The symmetry of the excited states has not been determined, only assumptions have been made based on theoretical concepts [83STE/FEI, 87MIL/FEI]. The data obtained later from the electronic spectrum [88BAL, 90BAL/LAU] and the results of the theoretical calculation [89LAN/BAU] unambiguously showed that the excited states in the photoelectron spectrum are a 5 Σ + and b 5 Π i .
Ab initio calculations of MnH were performed by various methods in [ 73BAG/SCH, 75BLI/KUN, 81DAS, 83WAL/BAU, 86CHO/LAN, 89LAN/BAU, 96FUJ/IWA, 2003WAN/AND, 2004RIN/TEL, 2005BAL/PET, 2006FUR/ PER, 2006KOS/MAT]. In all works, the parameters of the ground state were obtained, which, in the opinion of the authors, are in good agreement with the experimental data.
The following were included in the calculation of thermodynamic functions: a) the ground state X 7 Σ + ; b) experimentally observed excited states; c) states d 5 Δ and B 7 Σ + calculated in [89LAN/BAU]; d) synthetic (estimated) states, taking into account other bound states of the molecule up to 40000 cm -1 .
The vibrational ground state constants of MnH and MnD were obtained in [52NEV/CON, 57HAY/MCC] and with very high accuracy in [89URB/JON, 91URB/JON, 2005GOR/APP]. In table. Mn.4 values are from [ 2005GOR/APP ].
The ground state rotational constants MnH and MnD were obtained in [ 42NEV, 45NEV, 48NEV/DOY, 52NEV/CON, 57HAY/MCC, 74PAC, 75KOV/PAC, 89URB/JON, 91URB/JON, 92VAR/GRA, 2005GOR/APP, 2007GEN /STE]. Differences in B0 values lie within 0.001 cm -1 , Be within 0.002 cm -1 . They are due to different measurement accuracy and different methods of data processing. In table. Mn.4 values are from [ 2005GOR/APP ].
The energies of the observed excited states are obtained as follows. For the state a 5 Σ +, the value T 0 from [ 83STE/FEI ] is adopted (see above). For other quintet states in Table. Mn.4 are the energies obtained by adding to T 0 a 5 Σ + the values T = 9429.973 cm -1 and T = 11839.62 cm -1 [ 90BAL/LAU ], T 0 = 20880.56 cm -1 and T 0 = 22331.25 cm -1 [ 92BAL/LIN ]. For state A 7 Π shows the value of Te from [ 84HUG/GER ].
State energy d 5 D calculated in [89LAN/BAU] is reduced by 2000 cm -1 , which corresponds to the difference between the experimental and calculated energy of the state b 5 Π i . The energy B 7 Σ + is estimated by adding to the experimental energy A 7 Π energy differences of these states on the graph of potential curves [ 89LAN/BAU ].
The vibrational and rotational constants of the excited states of MnH were not used in the calculations of thermodynamic functions and are given in Table Mn.4 for reference. Vibrational constants are given according to [ 83STE/FEI ] (a 5 Σ +), [ 90BAL/LAU ] ( c 5 Σ +), [ 92BAL/LIN ] ( d 5 Π i , e 5 Σ +), [ 84HUG/HER ] ( A 7a). The rotational constants are given according to [90BAL/LAU] ( b 5 Π i , c 5 Σ +), [ 92BAL/LIN ] (a 5 Σ + , d 5 Π i , e 5 Σ +), [ 92VAR/GRA ] ( B 0 and D 0 A 7 Π) and [ 84HUG/GER ] (a 1 A 7a).
The ionic model Mn + H - was used to estimate the energies of the unobserved electronic states. According to the model, below 20,000 cm -1 the molecule has no other states than those already taken into account, i.e. those states that were observed in the experiment and/or obtained in the calculation [89LAN/BAU]. Above 20000 cm -1, the model predicts a large number of additional electronic states belonging to three ionic configurations: Mn + (3d 5 4s)H - , Mn + (3d 5 4p)H - and Mn + (3d 6)H - . These states compare well with the states calculated in [2006KOS/MAT]. The state energies estimated from the model are somewhat more accurate, since they take into account experimental data. Due to the large number of estimated states above 20000 cm -1 , they are combined into synthetic states at several energy levels (see note in Table Mn.4).
The thermodynamic functions of MnH(g) were calculated using equations (1.3) - (1.6) , (1.9) , (1.10) , (1.93) - (1.95) . Values Q ext and its derivatives were calculated by equations (1.90) - (1.92) taking into account fourteen excited states under the assumption that Q no.vr ( i) = (p i /p X)Q no.vr ( X) . The vibrational-rotational partition function of the X 7 Σ + state and its derivatives were calculated using equations (1.70) - (1.75) by direct summation over energy levels. The calculations took into account all energy levels with values J< J max ,v , where J max ,v was found from conditions (1.81) . The vibrational-rotational levels of the state X 7 Σ + were calculated using equations (1.65) , the values of the coefficients Y kl in these equations were calculated using relations (1.66) for the isotopic modification corresponding to the natural mixture of hydrogen isotopes from the 55 Mn 1 H molecular constants given in Table. Mn.4 . Coefficient values Y kl , as well as the quantities v max and J lim are given in Table. Mn.5 .
The main errors in the calculated thermodynamic functions MnH(g) are due to the calculation method. Errors in the values of Φº( T) at T= 298.15, 1000, 3000 and 6000 K are estimated at 0.16, 0.4, 1.1 and 2.3 J× K -1 × mol -1 , respectively.
The thermodynamic functions of MnH(r) were previously calculated without taking into account excited states up to 5000 K in [74SCH] and taking into account excited states up to 6000 K in [
D° 0 (MnH) = 140 ± 15 kJ × mol -1 = 11700 ± 1250 cm -1.
general review
Manganese is an element of the VIIB subgroup of the IVth period. The electronic structure of the atom is 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2, the most characteristic oxidation states in compounds are from +2 to +7.
Manganese belongs to fairly common elements, making up 0.1% (mass fraction) of the earth's crust. It occurs in nature only in the form of compounds, the main minerals are pyrolusite (manganese dioxide MnO2.), gauskanite Mn3O4 and brownite Mn2O3.
Physical properties
Manganese is a silvery white hard brittle metal. Its density is 7.44 g/cm 3 , melting point 1245 o C. Four crystalline modifications of manganese are known.
Chemical properties
Manganese is an active metal, in a number of voltages it is between aluminum and zinc. In air, manganese is covered with a thin oxide film, which protects it from further oxidation even when heated. In a finely divided state, manganese oxidizes easily.
3Mn + 2O 2 \u003d Mn 3 O 4- when calcined in airWater at room temperature acts on manganese very slowly, when heated - faster:
Mn + H 2 O \u003d Mn (OH) 2 + H 2It dissolves in dilute hydrochloric and nitric acids, as well as in hot sulfuric acid (in cold H2SO4 it is practically insoluble)
Mn + 2HCl \u003d MnCl 2 + H 2 Mn + H 2 SO 4 \u003d MnSO 4 + H 2Receipt
Manganese is obtained:
1. solution electrolysis MnSO 4. In the electrolytic method, the ore is reduced and then dissolved in a mixture of sulfuric acid and ammonium sulfate. The resulting solution is subjected to electrolysis.
2. recovery from its oxides by silicon in electric furnaces.
Application
Manganese is used:
1. in the production of alloy steels. Manganese steel containing up to 15% manganese has high hardness and strength.
2. manganese is part of a number of alloys based on magnesium; it increases their resistance to corrosion.
Magranz oxides
Manganese forms four simple oxides - MNO, Mn2O3, MnO2 and Mn2O7 and mixed oxide Mn3O4. The first two oxides have basic properties, manganese dioxide MnO2 amphoteric, and the higher oxide Mn2O7 is an anhydride of permanganic acid HMnO 4. Derivatives of manganese (IV) are also known, but the corresponding oxide MnO3 not received.
Manganese(II) compounds
+2 oxidation states correspond to manganese (II) oxide MNO, manganese hydroxide Mn(OH) 2 and manganese(II) salts.
Manganese(II) oxide is obtained in the form of a green powder by reducing other manganese oxides with hydrogen:
MnO 2 + H 2 \u003d MnO + H 2 Oor during thermal decomposition of manganese oxalate or carbonate without air access:
MnC 2 O 4 \u003d MnO + CO + CO 2 MnCO 3 \u003d MnO + CO 2Under the action of alkalis on solutions of manganese (II) salts, a white precipitate of manganese hydroxide Mn (OH) 2 precipitates:
MnCl 2 + NaOH = Mn(OH) 2 + 2NaClIn air, it quickly darkens, oxidizing to brown manganese (IV) hydroxide Mn (OH) 4:
2Mn(OH) 2 + O 2 + 2H 2 O \u003d 2 Mn(OH) 4Oxide and hydroxide of manganese (II) exhibit basic properties, easily soluble in acids:
Mn(OH)2 + 2HCl = MnCl 2 + 2H 2 OSalts with manganese (II) are formed by dissolving manganese in dilute acids:
Mn + H 2 SO 4 \u003d MnSO 4 + H 2- when heatedor by the action of acids on various natural manganese compounds, for example:
MnO 2 + 4HCl \u003d MnCl 2 + Cl 2 + 2H 2 OIn solid form, manganese (II) salts are pink in color, solutions of these salts are almost colorless.
When interacting with oxidizing agents, all manganese (II) compounds exhibit reducing properties.
Manganese(IV) compounds
The most stable compound of manganese (IV) is dark brown manganese dioxide MnO2. It is easily formed both in the oxidation of lower and in the reduction of higher compounds of manganese.
MnO2- amphoteric oxide, but both acidic and basic properties are very weakly expressed in it.
In an acidic environment, manganese dioxide is a strong oxidizing agent. When heated with concentrated acids, the following reactions take place:
2MnO 2 + 2H 2 SO 4 = 2MnSO 4 + O 2 + 2H 2 O MnO 2 + 4HCl \u003d MnCl 2 + Cl 2 + 2H 2 Omoreover, in the first stage, in the second reaction, unstable manganese (IV) chloride is first formed, which then decomposes:
MnCl 4 \u003d MnCl 2 + Cl 2When fused MnO2 with alkalis or basic oxides, manganites are obtained, for example:
MnO 2 + 2KOH \u003d K 2 MnO 3 + H 2 OWhen interacting MnO2 with concentrated sulfuric acid, manganese sulfate is formed MnSO 4 and oxygen is released
2Mn(OH) 4 + 2H2SO 4 = 2MnSO 4 + O 2 + 6H 2 OInteraction MnO2 with stronger oxidizing agents leads to the formation of manganese (VI) and (VII) compounds, for example, when fused with potassium chlorate, potassium manganate is formed:
3MnO 2 + KClO 3 + 6KOH = 3K2MnO 4 + KCl + 3H 2 Oand under the action of polonium dioxide in the presence of nitric acid - manganese acid:
2MnO 2 + 3PoO 2 + 6HNO 3 = 2HMnO 4 + 3Po(NO 3) 2 + 2H 2 OApplication of MnO 2
As an oxidizing agent MnO2 used in the production of chlorine from hydrochloric acid and in dry galvanic cells.
Manganese(VI) and (VII) compounds
When manganese dioxide is fused with potassium carbonate and nitrate, a green alloy is obtained, from which dark green crystals of potassium manganate can be isolated. K2MnO4- salts of very unstable permanganic acid H2MnO4:
MnO 2 + KNO 3 + K 2 CO 3 = K 2 MnO 4 + KNO 2 + CO 2in an aqueous solution, manganates spontaneously transform into salts of permanganic acid HMnO4 (permanganates) with the simultaneous formation of manganese dioxide:
3K 2 MnO 4 + H 2 O = 2KMnO 4 + MnO 2 + 4KOHin this case, the color of the solution changes from green to crimson and a dark brown precipitate is formed. In the presence of alkali, manganates are stable; in an acidic medium, the transition of manganate to permanganate occurs very quickly.
Under the action of strong oxidizing agents (for example, chlorine) on a solution of manganate, the latter is completely converted into permanganate:
2K 2 MnO 4 + Cl 2 = 2KMnO 4 + 2KClPotassium permanganate KMnO 4- the most famous salt of permanganic acid. It is a dark purple crystals, moderately soluble in water. Like all compounds of manganese (VII), potassium permanganate is a strong oxidizing agent. It easily oxidizes many organic substances, converts iron (II) salts into iron (III) salts, oxidizes sulfurous acid into sulfuric acid, releases chlorine from hydrochloric acid, etc.
In redox reactions KMnO 4(and he MnO4-) can recover to varying degrees. Depending on the pH of the medium, the reduction product may be an ion Mn2+(in an acidic environment), MnO2(in a neutral or slightly alkaline medium) or an ion MnO4 2-(in a strongly alkaline environment), for example:
KMnO4 + KNO 2 + KOH = K 2 MnO 4 + KNO 3 + H 2 O- in a highly alkaline environment 2KMnO 4 + 3KNO 2 + H 2 O = 2MnO 2 + 3KNO 3 + 2KOH– in neutral or slightly alkaline 2KMnO 4 + 5KNO 2 + 3H 2 SO 4 = 2MnSO 4 + K 2 SO 4 + 5KNO 3 + 3H 2 O- in an acidic environmentWhen heated in dry form, potassium permanganate already at a temperature of about 200 o C decomposes according to the equation:
2KMnO 4 \u003d K 2 MnO 4 + MnO 2 + O 2Corresponding to permanganates, free permanganic acid HMnO 4 in the anhydrous state has not been obtained and is known only in solution. The concentration of its solution can be brought up to 20%. HMnO 4- a very strong acid, completely dissociated into ions in an aqueous solution.
Manganese oxide (VII), or manganese anhydride, Mn2O7 can be obtained by the action of concentrated sulfuric acid on potassium permanganate: 2KMnO 4 + H 2 SO 4 \u003d Mn 2 O 7 + K 2 SO 4 + H 2 O
Manganese anhydride is a greenish-brown oily liquid. It is very unstable: when heated or in contact with combustible substances, it decomposes with an explosion into manganese dioxide and oxygen.
As an energetic oxidizing agent, potassium permanganate is widely used in chemical laboratories and industries, it also serves as a disinfectant. The thermal decomposition reaction of potassium permanganate is used in the laboratory to produce oxygen.
binary connections.
"Bi" means two. Binary compounds consist of two CE atoms.
Oxides.
Binary compounds consisting of two chemical elements, one of which oxygen in the oxidation state - 2 ("minus" two) are called oxides.
Oxides are a very common type of compound found in the earth's crust and throughout the universe.
The names of oxides are formed according to the scheme:
The name of the oxide = "oxide" + the name of the element in the genitive case + (the degree of oxidation is a Roman numeral), if variable, if constant, then do not set.
Examples of oxides. Some have trivial (historical) title.
1. H 2 O - hydrogen oxide water
CO 2 - carbon monoxide (IV) carbon dioxide (carbon dioxide)
CO - carbon monoxide (II) carbon monoxide (carbon monoxide)
Na 2 O - sodium oxide
Al 2 O 3 - aluminum oxide alumina
CuO - copper(II) oxide
FeO - iron(II) oxide
Fe 2 O 3 - iron oxide (III) hematite (red iron ore)
Cl 2 O 7 - chlorine oxide (VII)
Cl 2 O 5 - chlorine oxide (V)
Cl 2 O- chlorine(I) oxide
SO 2 - sulfur oxide (IV) sulfur dioxide
SO 3 - sulfur oxide (VI)
CaO - calcium oxide quicklime
SiO 2 - silicon oxide sand (silica)
MnO - manganese(II) oxide
N2O- nitric oxide (I) "laughing gas"
NO- nitric oxide (II)
N2O3- nitric oxide (III)
NO2- nitric oxide (IV) "fox tail"
N2O5- nitric oxide (V)
The indices in the formula are placed taking into account the degree of oxidation of CE:
Write down the oxides, arrange the oxidation states of ChE. Know how to write by name oxide formula.
Other binary compounds.
Volatile hydrogen compounds.
At the bottom of the PS there is a horizontal line "Volatile hydrogen compounds".
The formulas are listed there: RH4 RH3 RH2 RH
Each formula belongs to its own group.
For example, write the formula of the volatile hydrogen compound N (nitrogen).
We find it in the PS and see which formula is written under the V group.
It's RH3. We substitute the element nitrogen for R, it turns out ammonia NH3.
Since up to "8" nitrogen needs 3 electrons, it draws them from three hydrogens, the oxidation state of nitrogen is -3, and hydrogen has +
SiH4 - silane colorless gas with an unpleasant odor
PH3 - phosphine poisonous gas with the smell of rotten fish
AsH 3 - arsine poisonous gas with a garlic smell
H2S - hydrogen sulfide poisonous gas with the smell of rotten eggs
HCl - hydrogen chloride a gas with a pungent odor that smokes in the air; its solution in water is called hydrochloric acid. In small concentrations found in gastric juice.
NH3 ammonia a gas with a pungent irritating odour.
Its solution in water is called ammonia.
metal hydrides.
Houses: paragraph 19, ex. 3.4 writing. Formulas, how they are formed, the names of binary compounds from the abstract to know.
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