SRS 1 - Module 1.2

1. I Module. The main classes of inorganic compounds. Basic concepts and laws of chemistry.

 

Section I. Complex classes of inorganic compounds.

       1.1. Theoretical questions.

 

  1. What binary compounds are called oxides?
  2. What types of oxides are known to you? Please help.
  3. What substances are formed during the reaction of basic oxides with water, acid oxides, acids?
  4. What substances are formed during the reaction of acid oxides with water, basic oxides, bases?
  5. What substances do amphoteric oxides react with??
  6. What substances are formed by the interaction of acid oxides with water?
  7. Which oxides have strong basic properties:

а)

BeO or CaO

b)

ZnO or CdO

c)

As2O3 or Bi2O3

d)

MnO or Mn2O7

e)

FeO or Fe2O3

f)

CuO or Cu2O

1.               What is the basis?

2.               What substances are formed by the interaction of bases with acids and oxides?

3.               What is alkali??

4.               Which hydroxides have the strongest basic properties:

а)

Fe(OH)2 or Fe(OH)3

b)

Sn(OH)2 or Sn(OH)4

c)

Cu(OH)2 or Ba(OH)2

d)

As(OH)3 or Bi(OH)3

5.               What is acid?

6.               What classes of acids react? What is formed as a result?

7.               What is salt?

8.               Salt types?

9.               Acid salt? (give an example).

10.           Base salt? (give an example).

11.           Medium salt? (give an example).

12.           SO3 reacts with any of the following substances:?

а) Mn2O7       b) N2O5                c) SO2           d) Mn2O7           е) Cl2O.  

13.           Which of the following oxides reacts with water to form an alkali??

а) Mn2O7           b) CuO                c) K2O           d) SO2           е) H2O3.

14.           What is the name of the KHSO4 salt?

15.           What reaction can be used to get the base?

a) NaOH+HCl                     b) Na2O+CO2

c) CO2+H2O                        d) FeCl3+KOH  

16.                      What is the name of the (MgOH)3PO4 salt?

17.           Which oxide reacts with hydrochloric acid?

а) CO2           b) CO                c) Na2O           d) N2O           е) P2O5.

18.           What salt is called potassium orthophosphate?

а) KH2 PO4           b) K3P O4                c) K2 HPO4           d) KH2PO3          е) K2HPO3.

19.           Which of the following acids forms an acid salt??

а) HCl           b) H3ASO4                c) HMnO4           d) HNO3           е) CH3 COO3.

20.           What is an acid salt or hydrochloride salt? Give an example, name.

21.           What is a basic salt or hydroxyl salt? Give an example, name

22.           How to find the oxidation state of an acid-forming element and how to write the structural formula of acidity?

23.           How to find the validity of an acid and the laws of acid residue?

24.           What salts are called normal or medium salts?

 

1.2. Write the form of the upper oxides of the indicated elements and the corresponding form of the hydroxide:

 

1.

Lithium, arsenic.

2.

Sodium, molybdenum.

3.

Potassium, selenium.

4.

Rubidium, manganese.

5.

Cesium, antimony.

6.

Beryllium, chrome.

7.

Calcium, niobium.

8.

Magnesium, tantalum.

9.

Zinc, tungsten

10.

Cadmium, gallium.

11.

Mercury, phosphorus.

12.

Strontium, chlorine.

13.

Barium, nitrogen.

14.

Aluminum, rhenium.

15.

Copper, germanium

16.

Silver, tin

17.

Scandium, carbon.

18.

Titanium, silicon.

19.

Aluminum, germanium.

20.

Tellurium, sulfur.

21.

Vanadium, gold.

22.

Bromine, strontium.

23.

Manganese, potassium.

24.

Gallium, nitrogen.

25.

Indium, arsenic.

 

 

 

1.3. Write down the structural formula of acids. Indicate the oxidation state of the acid-forming element and the charge of the acid residue by name..

1.

Nitric acid

2.

Boric acid

3.

Carbonic acid

4.

Orthophosphoric acid

5.

Sulphuric acid

6.

Perchloric acid

7.

Metaphosphoric acid

8.

Orthomic acid

9.

Selenic acid

10.

Meta-silicic acid

11.

Manganese acid

12.

Metamisiacetic acid

13.

Sulphuric acid

14.

Telluric acid

15.

Nitric acid

16.

Bromic acid

17.

Chlorinated acid

18.

Perchloric acid

19.

Telluric acid

20.

Orthochromic acid

21.

Metachromic acid

22.

Orthoacetic acid

23.

Manganese acid

24.

Tungstic acid

25.

Chromic acid

 

 

 

1.4. Define еquations:

 

1.

HMnO4+NaOH®

HMnO4+Na2O®

Mn2O7+NaOH®

Mn2O7+Na2O®

2.

H2SiO3+KOH®

SiO2+KOH®

H2SiO3+K2O®

SiO2+K2O®

3.

Fe(OH)3+H2SO4®

Fe2O3+H2SO4®

Fe(OH)3+SO3®

Fe2O3+SO3®

4.

H3PO4+KOH®

H3PO4+K2O®

P2O5+KOH®

P2O5+K2O®

5.

H2CO3+Ca(OH)2®

CO2+Ca(OH)2®

H2CO3+CaO®

CO2+CaO®

6.

H2CrO4+NaOH®

H2CrO4+Na2O®

CrO3+NaOH®

CrO3+Na2O®

7.

Ca(OH)2+HVO3®

CaO+HVO3®

Ca(OH)2+V2O5®

CaO+V2O5®

8.

CsOH+H2MnO4®

CsOH+MnO3®

Cs2O+H2MnO4®

Cs2O+MnO3®

9.

H3SbO4+NaOH®

H3SbO4+Na2O®

Sb2O5+NaOH®

Sb2O5+Na2O®

10.

Ca(OH)2+HNO3®

Ca(OH)2+N2O5®

CaO+HNO3®

CaO+N2O5®

11.

H2MoO4+KOH®

H2MoO4+K2O®

MoO3+KOH®

MoO3+K2O®

12.

Sr(OH)2+H2TeO4®

Sr(OH)2+TeO3®

SrO+H2TeO4®

SrO+TeO3®

13.

H3AsO4+KOH®

H3AsO4+K2O®

As2O5+KOH®

As2O5+K2O®

14.

Ba(OH)2+H2SnO3®

Ba(OH)2+SnO2®

BaO+H2SnO3®

BaO+SnO2®

15.

HAsO3+NaOH®

HAsO3+Na2O®

As2O5+NaOH®

As2O3+Na2O®

16.

H2GeO3+KOH®

H2GeO3+K2O®

GeO2+KOH®

GeO2+K2O®

17.

H2BeO2+NaOH®

H2BeO2+Na2O®

BeO+NaOH®

BeO+Na2O®

18.

H2WO4+KOH®

H2WO4+K2O®

WO3+KOH®

WO3+K2O®

19.

Sr(OH)2+H2SO4®

Sr(OH)2+SO3®

SrO+H2SO4®

SrO+SO3®

20.

Ba(OH)2+HBrO®

Ba(OH)2+Br2O®

BaO+HBrO®

BaO+Br2O®

21.

HReO4+LiOH®

HReO4+Li2O®

Re2O+LiOH®

Re2O7+Li2O®

22.

HClO3+NaOH®

Cl2O5+NaOH®

HClO3+Na2O®

Cl2O5+Na2O®

23.

H3NbO4+NaOH®

H3NbO4+Na2O®

Nb2O5+NaOH®

Nb2O5+Na2O®

24.

HNO2+Ca(OH)2®

HNO2+CaO®

N2O3+Ca(OH)2®

N2O3+CaO®

25.

H3AsO3+CsOH®

H3AsO3+Cs2O®

As2O3+CsOH®

As2O3+Cs2O®

 

 

 

1.5. Write the reaction equations:

 

1.

Ba®BaO®BaCl2®Ba(NO3)2®BaSO4

2.

Mg®MgSO4®Mg(OH)2®MgO®MgCl2

3.

MnO®MnCl2®Mn(OH)2®MnSO4

4.

P2O5®H3PO4®Na3PO4®Ca3(PO4)2

5.

NiO®NiSO4®Ni(OH)2®NiCl2

6.

CO2®MgCO3®Mg(HCO3)2®MgCl2

7.

SO3®H2SO4®Na2SO4®BaSO4

8.

Fe2O3®FeCl3®Fe(OH)3®Fe(OH)2NO3®Fe(NO3)3

9.

P2O5®H3PO4®NaH2PO4®Na3PO4®Ba3(PO4)2

10.

Zn®ZnCl2®Zn(OH)2®ZnOHCl®ZnCl2

11.

CaCO3®CaO®Ca(OH)2®Ca(HCO3)2®CaCO3

12.

Mg®MgSO4®Mg(OH)2®MgOHCl®MgCl2

13.

Na2O®NaOH®NaHCO3®Na2CO3®CaCO3

14.

Fe2O3®Fe2(SO4)3®Fe(OH)3®FeOHSO4®Fe2(SO4)3

15.

ZnO®ZnCl2®Zn(OH)2®Na2ZnO2®ZnCl2

16.

Al2(SO4)3®Al(OH)3®Na3AlO3®AlCl3

17.

CuO®Cu(NO3)2®Cu(OH)2®CuOHCl®CuCl2

18.

Zn®ZnSO4®Zn(OH)2®(ZnOH)2SO4®ZnSO4

19.

H3PO4®K2HPO4®K3PO4®Ca3(PO4)2

20.

CaO®Ca(OH)2®CaCO3®Ca(HCO3)2®CaCO3

21.

Al2O3®AlCl3®Al(OH)3®AlOHSO4®Al2(SO4)3

22.

K2O®KOH®KHSO3®K2SO3®CaSO3

23.

SnO®Sn(OH)2®SnOHNO3®Sn(NO3)2

24.

NaO®NaOH®NaHCO3®Na2CO3

25.

CuO®CuSO4®Cu(OH)2®CuOHCl®CuCl2

 

Section II. Basic concepts and laws of chemistry

 

2.1. Theoretical questions.

 

1.      Identify atoms, molecules, elements and simple things?

2.      What is allotropy?

3.      The law of compositional stability of a substance?

4.      What is a mole?

5.      What is molar mass and relative molecular mass?

6.      Specify the unit of molar mass

а) G            b) mole                 c) g / mole

7.      Avogadro's law?

8.      What parameters determine the physical state of the gas?

9.      What is the molar volume of a gas under normal conditions??

10.  Mendeleev - Clapeyron equation?

11.  What is a universal gas constant??

12.  Relative density?

13.  What is the equivalent of an element?

14.  What is the equivalent of the substance?

15.  Molar mass equivalent?

16.  What is the law of equivalence?                                                                                

17.  Mass conservation law?

18.  Composition stability law?

19.  Mass conservation law?

20.  What is the equivalent of things?

21.  Basic principles of Avogadro's law?

22.  Equivalence law formula?

23.  The laws of gaseous matter?                                                                                                  

24.  Gay is Lussac's Law?

25.  Boyle-Marriott law.?

 

2.2. Gotta calculate: а) mass of a given number of moles of gas: b) the number of molecules in a given number of moles of gas; c) volume of given moles of gas

 

1.

0.5 mol of hydrogen sulfide;

2.

2.5 mol of ammonia;

3.

1.2 mol of nitrogen;

4.

5.4 moles of carbon dioxide;

5.

0.8 mol hydrogen;

6.

1.5 moles of chlorine;

7.

3 moles of nitrogen;

8.

7.5 mol fluorine;

9.

8.5 mol of nitric oxide (IV)

10.

3 moles of ammonia;

11.

1.6 mol hydrogen fluoride;

12.

12.2 mol hydrogen;

13.

5.4 moles of oxygen;

14.

3.5 mol of sulfur (IV) oxide

15.

2.8 mol of hydrogen sulfide;

16.

C2H2 mol of acetylene;

17.

2.6 mol CH4 methane;

18.

4.4 mol of hydrogen chloride;

19.

5.2 mol of nitric oxide (II);

20.

1.2 mol of sulfur (IV) oxide;

21.

0.8 mol oxygen;

22.

4 moles of carbon monoxide (II);

23.

0.1 mol of ammonia;

24.

3.2 moles of carbon dioxide;

25.

6.0 mol of nitrogen.

 

 

 

2.3. Calculate the molar mass of a gas with a given relative density:

 

1.

= 14;

2.

=0,503;

3.

= 19,0;

4.

= 1,1;

5.

= 1,51;

6.

= 2,45;

7.

= 38;

8.

= 2,218;

9.

= 23;

10.

= 2,375;

11.

= 1,31;

12.

= 2,620;

13.

= 8,5.

14.

= 3,12;

15.

= 31;                

   

16.

= 2,42;

17.

= 7,1;

18.

= 1,32;

19.

= 28;

20.

=5,1;

21.

= 1,96;

22.

= 1,8;

23.

= 19;

24.

= 3,41;

25.

= 21;

26.

= 5,322;

 

 

 

 

 

2.4. Find the molar mass equivalent of acids, bases, salts in reactions:

 

1.

Ba(OH)2+2H2CO3=Ba(HCO3)2+2H2O

2.

Ba(OH)2+H2CO3=BaCO3+2H2O.

3.

Fe(OH)3+HCl=Fe(OH)2Cl+H2O.

4.

Fe(OH)3+2HCl=FeOHCl2+2H2O.

5.

Fe(OH)3+3HCl=FeCl3+3H2O.

6.

H3PO4+KOH=KH2PO4+H2O.

7.

H3PO4+2KOH=K2HPO4+2H2O.

8.

H3PO4+3KOH=K3HPO4+3H2O.

9.

2Al(OH)3+3H2SO4=Al2(SO4)3+6H2O.

10.

Al(OH)3+H2SO4=AlOHSO4+2H2O.

11.

2Al(OH)3+H2SO4=[Al(OH)2]2SO4+2H2O.

12.

Al(OH)3+3H2SO4=Al(HSO4)3+3H2O.

13.

Ca(OH)2+H3PO4=CaHPO4+2H2O.

14.

Ca(OH)2+2H3PO4=Ca(H2PO4)2+2H2O.

15.

3Ca(OH)2+2H3PO4=Ca3(PO4)2+4H2O.

16.

3HNO3+Bi(OH)3=Bi(NO3)3+3H2O.

17.

2HNO3+Bi(OH)3=BiOH(NO3)2+2H2O.

18.

HNO3+Bi(OH)3=Bi(OH)2NO3+H2O.

19.

Cu(OH)2+HCl=CuOHCl+H2O.

20.

Cu(OH)2+2HCl=CuCl2+2H2O.

21.

Cr(OH)3+3H2SO4=Cr2(SO4)3+6H2O.

22.

Cr(OH)3+3H2SO4=Cr(HSO4)3+3H2O.

23.

Cr(OH)3+HF=Cr(OH)2F+H2O.

24.

Ni(OH)2+2HNO3=Ni(NO3)2+2H2O.

25.

Ni(OH)2+HNO3=NiОHNO3+H2O.

 

 

2.5. Find the molar mass of a metal equivalent by the mass of the metal and the volume of hydrogen displaced:

 

 

Metal weight, g

Hydrogen volume, l

 

 

 

1.

0,10

0,560

2.

0,22

0,560

3.

0,40

0,224

4.

0,45

0,336

5.

0,30

0,224

6.

0,85

0,560

7.

0,34

0,224

8.

0,52

0,336

9.

0,44

0,112

10.

0,20

0,112

11.

1,4

0,560

12.

1,2

1,12

13.

2,4

0,150

14.

0,15

0,112

 

2.6. Make a report:

 

1.      One gas contains 82.35% nitrogen and 17.65% hydrogen. Considering that the density of the gas in relation to hydrogen is 8.5, determine its molecular formula.

2.      When 0.24 g of nitrogen is combined with hydrogen, usually 168 m of nitrogen and 0.27 g of water are formed. Considering that the density of this substance in relation to air is 1.1, determine the molecular formula of organic matter..

3.      The substance contains potassium, chlorine, oxygen. Upon complete decomposition of 1.02 grams of this substance, 0.62 g of potassium chloride is formed. Create a simple formula for the substance to be decomposed.

4.      The substance contains potassium, sulfur and oxygen. 0.87 grams of this substance is released as sulfur and oxygen in barium sulfate. Considering that the mass of the resulting barium sulfate is 1.167 g, determine the simple formula for the starting material.

5.      Sodium nitrate, potassium nitrate, calcium nitrate, ammonium nitrate are used as fertilizers to increase the amount of nitrogen in the soil. Which of these salts contains the most nitrogen and what percentage?

6.      From 14.4 g of the sulfur-containing substance, 23.3 g of barium sulfate are obtained. Determine the percentage of sulfur in the test substance.

7.      Heating 200 g of crystalline soda Na2CO10*10H2O gives 63.6 g of anhydrous sodium carbonate. What percentage of the obtained crystalline soda contains impurities.

8.      How many grams of phosphorus / V / oxide is formed when 8 moles of phosphorus are burned in oxygen?

9.      6.02.1024 How many moles of iron / III / oxide are formed during the decomposition of iron hydroxide / III /?  

10.  How many liters of hydrogen are usually formed when 0.5 mol of sodium gyroxide reacts with water?

11.  As a result of the interaction of iron sulfate and potassium hydroxide, 1.07 g of iron (III) hydroxide is formed. How many moles of potassium hydroxide were involved in this reaction?.

12.  Typically, 22.4 ml of hydrogen is used to reduce copper / II oxide. How many water molecules are formed as a result of this reaction?

13.  For the reaction, 10 g of sulfuric acid was added to a vessel containing 5.6 g of potassium hydroxide. What compound is used in excess.

14.  Under normal conditions 10 g of calcium hydroxide and 2.24 liters of carbon monoxide reacted. As a result of this reaction, what substance is left in excess and how much calcium carbonate is formed.

15.  Calculate the volume of air with a mass of 5 kg at a pressure of 101.325 * 103 Pa and a temperature of 170 ° C.

 

 

2. Module II. Nuclear construction. Chemical bond. 

 

Section I. Atomic construction.

1.1. Theoretical questions.

  1. Rutherford's planetary model of the atom. What are the disadvantages of this model?
  2. Explain why the spectrum of the hydrogen atom is linear?
  3. Explain the physical meaning of the wave function of an electron, "potential density", orbital.
  4. What quantum numbers describe the energy state of an electron in an atom??
  5. Calculate the number of levels of energy level IV, where the value of the principal quantum number n = 4?
  6. If the number of the main quantum is n = 4, what are the values ​​of the additional and magnetic quantum numbers? The magnetic quantum number indicates what characteristics of a given orbital?
  7. What is the meaning of the Pauli principle? Could there be neutrons p7, d12, p4, d3 at the levels of the atom??  
  8. Give the first and current definition of the law of the period. Which of the two is correct??
  9. What are isotopes? Can atoms of different elements have the same mass? What do you call these atoms?
  10. If a) the ordinal number of the atom in the periodic table; b) period number; c) If the group number is known, what characteristics of this element can be determined?
  11. Construct a sequence of filling the bonds of atoms according to Klechkovsky's rules..
  12. What is the binding energy of electrons? How the oxidizing properties of non-metals change in the period and group in ascending order of the number of elements in the periodic table?
  13. What is ionization energy? In what units is it measured? How do the redox properties of S and P elements change in the ascending group of elements of the periodic table?
  14. What is electrical conductivity? As the ordinal number of elements in the periodic table increases, how does the electrical resistance change in the period and group of P-elements?
  15. Can different items weigh the same?
  16. Write electronic and electronic graphic formulas of atoms of elements and determine to which electronic types they belong. (S, P, D, f).

 

  1. Sodium, selenium, californium, tantalum.
  1. Lithium, chlorine, osmium, thulium.
  1. Calcium, tin, tungsten, erbium.
  1. Beryllium, argon, rhenium, holmium.
  1. Potassium, niobium, antimony, samarium.
  1. Magnesium, bromine, hafnium,              americium.
  1. Strontium, zinc, iodine, gadolinium..
  1. Barium, bismuth, cobalt, uranium.
  1. Cesium, xenon, manganese, neodymium..
  1. Neon, calcium, nickel, thorium.
  1. Rubidium, indium, iron, cerium..
  1. Francium, tin, zirconium, lanthanum.
  1. Radium, nitrogen, vanadium, neodymium..
  1. Fluorine, strontium, niobium, promethium.
  1. Sulfur, barium, ruthenium, europium..
  1. Oxygen, rubidium, palladium, europium
  1. Phosphorus, cesium, cadmium, dysprosium
  1. Селен, магний, серебро, нептуний
  1. Krypton, sodium, chromium, holmium.
  1. Lead, calcium, gold, plutonium.
  1. Iodine, lithium, tantalum, thulium..
  1. Indium, hydrogen, copper, ytterbium.
  1. Helium, bismuth, rhodium, terbium..

24.  Barium, carbon, technetium, cerium.
  1. Xenon, calcium, cobalt, gadolinium

 

                        

1.3. If the arrangement of electrons in the outer electron shell is as follows, in which group and period the element is located (write electron-graphic formulas and determine the valence electrons in the normal and excited states).

 

1.

2s2p3

2.

3s23p4

3.

3d104s2

4.

3d34s2

5.

2p63s1

6.

3p64s1

7.

2s22p4

8.

3d104p1

9.

3d74s2

10.

3d104s24p3

11.

3d54p1

12.

3d84s2

13.

5s25p1

14.

4d15s2

15.

4d95s2

16.

2s22p5

17.

4d105s2

18.

3s23p5

19.

4d25s2

20.

3d104p2

21.

4p65s2

22.

2s22p2

23.

3s23p4

24.

4d105p2

25.

4d105p5

 

 

 

 

 

1.4.   Write the electronic formula of elements for a given oxidation state:

 

1.

Fe(+3)

2.

Na(+1)

3.

Mo(+4)

4.

S(-2)

5.

Mg(+2)

6.

Cl(-1)

7.

Ca(+2)

8.

K(+1)

9.

O(-2)

10.

Fe(+6)

11.

S(+6)

12.

Mo(+6)

13.

Sb(+5)

14.

Cu(+2)

15.

Nb(+3)

16.

Nb(+5)

17.

W(+6)

18.

Cr(+3)

19.

N(+5)

20.

V(+5)

21.

Mn(+7)

22.

Mn(+2)

23.

As(+5)

24.

Ni(+2)

25.

N(-3)

 

 

 

 

 

 

Section II. Chemical bond.

 

2.1. Теоретические вопросы

 

1.      Explain the nature of chemical bonds and the distribution of energy when atoms form a molecule..

2.      Basic principles of the theory of valence bonds.

3.      What is a covalent bond?

4.      Depending on which covalent bond?

5.      What covalent bond is called _, _ bond? Indicate the types of orbitals formed by these connections.

6.      What is the most important reason for the hybridization of atomic orbitals sp, sp, sp What is the spatial arrangement of the hybridized orbitals relative to the central atom?

7.      What chemical bond is an ionic bond? What is the mechanism of its formation?

8.      Indicate the spatial configuration (location) of CH4 (109.50), NH3 (107.30), H2O (104.50) molecules, compare their bond angles and explain their change..

9.      Which molecule: BF3 and NH3 has a dipole moment of 0? Why?

10.  What is the electrical moment of a dipole? Which of the molecules - HCl, HBr, Hl - has the highest dipole moment?

11.  Basic principles of the MO-AOSK theory.

12.  What are the rules for the arrangement of valence electrons of atoms at the levels of energy diagrams of molecules?

13.  What is Electric Dipole Moment?

14.  Write down the electronic configuration of the molecule by the MO method?

15.  How to arrange the order of bonds in a molecule using the MO method?

16.  What is a paramagnetic molecule?

17.  How the MO method explains the paramagnetic properties of a molecule?

 

2.2. Consider the formation of a molecule by the valence bond method. Specify connection types.  

 

1.

HCl

2.

H2S

3.

PCl3

4.

NH3

5.

BeCl2

6.

CH4

7.

BeF2

8.

SiH4

9.

H2Se

10.

ZnCl2

11.

HF

12.

PCl5

13.

BF3

14.

H2O

15.

NF3

16.

SF6

17.

PF5

18.

BCl4

19.

H2Te

20.

CCl4

21.

PCl3

22.

Cl2

23.

N2

24.

BH3

25.

HgCl2

 

 

 

 

 

 

 

2.3. Show the scheme of energy formation of a molecule by the MO method. Write an electronic formula. Determine the magnetic properties and contact order.

 

1.

Li2

2.

O2-

3.

H2+

4.

B2

5.

He2+

6.

H2

7.

O2

8.

N2

9.

NO

10.

NO-

11.

Cl2

12.

C2

13.

F2

14.

He2

15.

S2

16.

Br2

17.

P2

18.

CO

19.

F2+

20.

O22-

21.

Na2

22.

N2+

23.

K2

24.

O22+

25.

Ne2+

 

 

 

 

 

 

 

 

1. I Module. The main classes of inorganic compounds. Basic concepts and laws of chemistry.

 

Section I. Complex classes of inorganic compounds.

       1.1. Theoretical questions.

 

  1. What binary compounds are called oxides?
  2. What types of oxides are known to you? Please help.
  3. What substances are formed during the reaction of basic oxides with water, acid oxides, acids?
  4. What substances are formed during the reaction of acid oxides with water, basic oxides, bases?
  5. What substances do amphoteric oxides react with??
  6. What substances are formed by the interaction of acid oxides with water?
  7. Which oxides have strong basic properties:

а)

BeO or CaO

b)

ZnO or CdO

c)

As2O3 or Bi2O3

d)

MnO or Mn2O7

e)

FeO or Fe2O3

f)

CuO or Cu2O

1.               What is the basis?

2.               What substances are formed by the interaction of bases with acids and oxides?

3.               What is alkali??

4.               Which hydroxides have the strongest basic properties:

а)

Fe(OH)2 or Fe(OH)3

b)

Sn(OH)2 or Sn(OH)4

c)

Cu(OH)2 or Ba(OH)2

d)

As(OH)3 or Bi(OH)3

5.               What is acid?

6.               What classes of acids react? What is formed as a result?

7.               What is salt?

8.               Salt types?

9.               Acid salt? (give an example).

10.           Base salt? (give an example).

11.           Medium salt? (give an example).

12.           SO3 reacts with any of the following substances:?

а) Mn2O7       b) N2O5                c) SO2           d) Mn2O7           е) Cl2O.  

13.           Which of the following oxides reacts with water to form an alkali??

а) Mn2O7           b) CuO                c) K2O           d) SO2           е) H2O3.

14.           What is the name of the KHSO4 salt?

15.           What reaction can be used to get the base?

a) NaOH+HCl                     b) Na2O+CO2

c) CO2+H2O                        d) FeCl3+KOH  

16.                      What is the name of the (MgOH)3PO4 salt?

17.           Which oxide reacts with hydrochloric acid?

а) CO2           b) CO                c) Na2O           d) N2O           е) P2O5.

18.           What salt is called potassium orthophosphate?

а) KH2 PO4           b) K3P O4                c) K2 HPO4           d) KH2PO3          е) K2HPO3.

19.           Which of the following acids forms an acid salt??

а) HCl           b) H3ASO4                c) HMnO4           d) HNO3           е) CH3 COO3.

20.           What is an acid salt or hydrochloride salt? Give an example, name.

21.           What is a basic salt or hydroxyl salt? Give an example, name

22.           How to find the oxidation state of an acid-forming element and how to write the structural formula of acidity?

23.           How to find the validity of an acid and the laws of acid residue?

24.           What salts are called normal or medium salts?

 

1.2. Write the form of the upper oxides of the indicated elements and the corresponding form of the hydroxide:

 

1.

Lithium, arsenic.

2.

Sodium, molybdenum.

3.

Potassium, selenium.

4.

Rubidium, manganese.

5.

Cesium, antimony.

6.

Beryllium, chrome.

7.

Calcium, niobium.

8.

Magnesium, tantalum.

9.

Zinc, tungsten

10.

Cadmium, gallium.

11.

Mercury, phosphorus.

12.

Strontium, chlorine.

13.

Barium, nitrogen.

14.

Aluminum, rhenium.

15.

Copper, germanium

16.

Silver, tin

17.

Scandium, carbon.

18.

Titanium, silicon.

19.

Aluminum, germanium.

20.

Tellurium, sulfur.

21.

Vanadium, gold.

22.

Bromine, strontium.

23.

Manganese, potassium.

24.

Gallium, nitrogen.

25.

Indium, arsenic.

 

 

 

1.3. Write down the structural formula of acids. Indicate the oxidation state of the acid-forming element and the charge of the acid residue by name..

1.

Nitric acid

2.

Boric acid

3.

Carbonic acid

4.

Orthophosphoric acid

5.

Sulphuric acid

6.

Perchloric acid

7.

Metaphosphoric acid

8.

Orthomic acid

9.

Selenic acid

10.

Meta-silicic acid

11.

Manganese acid

12.

Metamisiacetic acid

13.

Sulphuric acid

14.

Telluric acid

15.

Nitric acid

16.

Bromic acid

17.

Chlorinated acid

18.

Perchloric acid

19.

Telluric acid

20.

Orthochromic acid

21.

Metachromic acid

22.

Orthoacetic acid

23.

Manganese acid

24.

Tungstic acid

25.

Chromic acid

 

 

 

1.4. Define еquations:

 

1.

HMnO4+NaOH®

HMnO4+Na2O®

Mn2O7+NaOH®

Mn2O7+Na2O®

2.

H2SiO3+KOH®

SiO2+KOH®

H2SiO3+K2O®

SiO2+K2O®

3.

Fe(OH)3+H2SO4®

Fe2O3+H2SO4®

Fe(OH)3+SO3®

Fe2O3+SO3®

4.

H3PO4+KOH®

H3PO4+K2O®

P2O5+KOH®

P2O5+K2O®

5.

H2CO3+Ca(OH)2®

CO2+Ca(OH)2®

H2CO3+CaO®

CO2+CaO®

6.

H2CrO4+NaOH®

H2CrO4+Na2O®

CrO3+NaOH®

CrO3+Na2O®

7.

Ca(OH)2+HVO3®

CaO+HVO3®

Ca(OH)2+V2O5®

CaO+V2O5®

8.

CsOH+H2MnO4®

CsOH+MnO3®

Cs2O+H2MnO4®

Cs2O+MnO3®

9.

H3SbO4+NaOH®

H3SbO4+Na2O®

Sb2O5+NaOH®

Sb2O5+Na2O®

10.

Ca(OH)2+HNO3®

Ca(OH)2+N2O5®

CaO+HNO3®

CaO+N2O5®

11.

H2MoO4+KOH®

H2MoO4+K2O®

MoO3+KOH®

MoO3+K2O®

12.

Sr(OH)2+H2TeO4®

Sr(OH)2+TeO3®

SrO+H2TeO4®

SrO+TeO3®

13.

H3AsO4+KOH®

H3AsO4+K2O®

As2O5+KOH®

As2O5+K2O®

14.

Ba(OH)2+H2SnO3®

Ba(OH)2+SnO2®

BaO+H2SnO3®

BaO+SnO2®

15.

HAsO3+NaOH®

HAsO3+Na2O®

As2O5+NaOH®

As2O3+Na2O®

16.

H2GeO3+KOH®

H2GeO3+K2O®

GeO2+KOH®

GeO2+K2O®

17.

H2BeO2+NaOH®

H2BeO2+Na2O®

BeO+NaOH®

BeO+Na2O®

18.

H2WO4+KOH®

H2WO4+K2O®

WO3+KOH®

WO3+K2O®

19.

Sr(OH)2+H2SO4®

Sr(OH)2+SO3®

SrO+H2SO4®

SrO+SO3®

20.

Ba(OH)2+HBrO®

Ba(OH)2+Br2O®

BaO+HBrO®

BaO+Br2O®

21.

HReO4+LiOH®

HReO4+Li2O®

Re2O+LiOH®

Re2O7+Li2O®

22.

HClO3+NaOH®

Cl2O5+NaOH®

HClO3+Na2O®

Cl2O5+Na2O®

23.

H3NbO4+NaOH®

H3NbO4+Na2O®

Nb2O5+NaOH®

Nb2O5+Na2O®

24.

HNO2+Ca(OH)2®

HNO2+CaO®

N2O3+Ca(OH)2®

N2O3+CaO®

25.

H3AsO3+CsOH®

H3AsO3+Cs2O®

As2O3+CsOH®

As2O3+Cs2O®

 

 

 

1.5. Write the reaction equations:

 

1.

Ba®BaO®BaCl2®Ba(NO3)2®BaSO4

2.

Mg®MgSO4®Mg(OH)2®MgO®MgCl2

3.

MnO®MnCl2®Mn(OH)2®MnSO4

4.

P2O5®H3PO4®Na3PO4®Ca3(PO4)2

5.

NiO®NiSO4®Ni(OH)2®NiCl2

6.

CO2®MgCO3®Mg(HCO3)2®MgCl2

7.

SO3®H2SO4®Na2SO4®BaSO4

8.

Fe2O3®FeCl3®Fe(OH)3®Fe(OH)2NO3®Fe(NO3)3

9.

P2O5®H3PO4®NaH2PO4®Na3PO4®Ba3(PO4)2

10.

Zn®ZnCl2®Zn(OH)2®ZnOHCl®ZnCl2

11.

CaCO3®CaO®Ca(OH)2®Ca(HCO3)2®CaCO3

12.

Mg®MgSO4®Mg(OH)2®MgOHCl®MgCl2

13.

Na2O®NaOH®NaHCO3®Na2CO3®CaCO3

14.

Fe2O3®Fe2(SO4)3®Fe(OH)3®FeOHSO4®Fe2(SO4)3

15.

ZnO®ZnCl2®Zn(OH)2®Na2ZnO2®ZnCl2

16.

Al2(SO4)3®Al(OH)3®Na3AlO3®AlCl3

17.

CuO®Cu(NO3)2®Cu(OH)2®CuOHCl®CuCl2

18.

Zn®ZnSO4®Zn(OH)2®(ZnOH)2SO4®ZnSO4

19.

H3PO4®K2HPO4®K3PO4®Ca3(PO4)2

20.

CaO®Ca(OH)2®CaCO3®Ca(HCO3)2®CaCO3

21.

Al2O3®AlCl3®Al(OH)3®AlOHSO4®Al2(SO4)3

22.

K2O®KOH®KHSO3®K2SO3®CaSO3

23.

SnO®Sn(OH)2®SnOHNO3®Sn(NO3)2

24.

NaO®NaOH®NaHCO3®Na2CO3

25.

CuO®CuSO4®Cu(OH)2®CuOHCl®CuCl2

 

Section II. Basic concepts and laws of chemistry

 

2.1. Theoretical questions.

 

1.      Identify atoms, molecules, elements and simple things?

2.      What is allotropy?

3.      The law of compositional stability of a substance?

4.      What is a mole?

5.      What is molar mass and relative molecular mass?

6.      Specify the unit of molar mass

а) G            b) mole                 c) g / mole

7.      Avogadro's law?

8.      What parameters determine the physical state of the gas?

9.      What is the molar volume of a gas under normal conditions??

10.  Mendeleev - Clapeyron equation?

11.  What is a universal gas constant??

12.  Relative density?

13.  What is the equivalent of an element?

14.  What is the equivalent of the substance?

15.  Molar mass equivalent?

16.  What is the law of equivalence?                                                                                

17.  Mass conservation law?

18.  Composition stability law?

19.  Mass conservation law?

20.  What is the equivalent of things?

21.  Basic principles of Avogadro's law?

22.  Equivalence law formula?

23.  The laws of gaseous matter?                                                                                                  

24.  Gay is Lussac's Law?

25.  Boyle-Marriott law.?

 

2.2. Gotta calculate: а) mass of a given number of moles of gas: b) the number of molecules in a given number of moles of gas; c) volume of given moles of gas

 

1.

0.5 mol of hydrogen sulfide;

2.

2.5 mol of ammonia;

3.

1.2 mol of nitrogen;

4.

5.4 moles of carbon dioxide;

5.

0.8 mol hydrogen;

6.

1.5 moles of chlorine;

7.

3 moles of nitrogen;

8.

7.5 mol fluorine;

9.

8.5 mol of nitric oxide (IV)

10.

3 moles of ammonia;

11.

1.6 mol hydrogen fluoride;

12.

12.2 mol hydrogen;

13.

5.4 moles of oxygen;

14.

3.5 mol of sulfur (IV) oxide

15.

2.8 mol of hydrogen sulfide;

16.

C2H2 mol of acetylene;

17.

2.6 mol CH4 methane;

18.

4.4 mol of hydrogen chloride;

19.

5.2 mol of nitric oxide (II);

20.

1.2 mol of sulfur (IV) oxide;

21.

0.8 mol oxygen;

22.

4 moles of carbon monoxide (II);

23.

0.1 mol of ammonia;

24.

3.2 moles of carbon dioxide;

25.

6.0 mol of nitrogen.

 

 

 

2.3. Calculate the molar mass of a gas with a given relative density:

 

1.

= 14;

2.

=0,503;

3.

= 19,0;

4.

= 1,1;

5.

= 1,51;

6.

= 2,45;

7.

= 38;

8.

= 2,218;

9.

= 23;

10.

= 2,375;

11.

= 1,31;

12.

= 2,620;

13.

= 8,5.

14.

= 3,12;

15.

= 31;                

   

16.

= 2,42;

17.

= 7,1;

18.

= 1,32;

19.

= 28;

20.

=5,1;

21.

= 1,96;

22.

= 1,8;

23.

= 19;

24.

= 3,41;

25.

= 21;

26.

= 5,322;

 

 

 

 

 

2.4. Find the molar mass equivalent of acids, bases, salts in reactions:

 

1.

Ba(OH)2+2H2CO3=Ba(HCO3)2+2H2O

2.

Ba(OH)2+H2CO3=BaCO3+2H2O.

3.

Fe(OH)3+HCl=Fe(OH)2Cl+H2O.

4.

Fe(OH)3+2HCl=FeOHCl2+2H2O.

5.

Fe(OH)3+3HCl=FeCl3+3H2O.

6.

H3PO4+KOH=KH2PO4+H2O.

7.

H3PO4+2KOH=K2HPO4+2H2O.

8.

H3PO4+3KOH=K3HPO4+3H2O.

9.

2Al(OH)3+3H2SO4=Al2(SO4)3+6H2O.

10.

Al(OH)3+H2SO4=AlOHSO4+2H2O.

11.

2Al(OH)3+H2SO4=[Al(OH)2]2SO4+2H2O.

12.

Al(OH)3+3H2SO4=Al(HSO4)3+3H2O.

13.

Ca(OH)2+H3PO4=CaHPO4+2H2O.

14.

Ca(OH)2+2H3PO4=Ca(H2PO4)2+2H2O.

15.

3Ca(OH)2+2H3PO4=Ca3(PO4)2+4H2O.

16.

3HNO3+Bi(OH)3=Bi(NO3)3+3H2O.

17.

2HNO3+Bi(OH)3=BiOH(NO3)2+2H2O.

18.

HNO3+Bi(OH)3=Bi(OH)2NO3+H2O.

19.

Cu(OH)2+HCl=CuOHCl+H2O.

20.

Cu(OH)2+2HCl=CuCl2+2H2O.

21.

Cr(OH)3+3H2SO4=Cr2(SO4)3+6H2O.

22.

Cr(OH)3+3H2SO4=Cr(HSO4)3+3H2O.

23.

Cr(OH)3+HF=Cr(OH)2F+H2O.

24.

Ni(OH)2+2HNO3=Ni(NO3)2+2H2O.

25.

Ni(OH)2+HNO3=NiОHNO3+H2O.

 

 

2.5. Find the molar mass of a metal equivalent by the mass of the metal and the volume of hydrogen displaced:

 

 

Metal weight, g

Hydrogen volume, l

 

 

 

1.

0,10

0,560

2.

0,22

0,560

3.

0,40

0,224

4.

0,45

0,336

5.

0,30

0,224

6.

0,85

0,560

7.

0,34

0,224

8.

0,52

0,336

9.

0,44

0,112

10.

0,20

0,112

11.

1,4

0,560

12.

1,2

1,12

13.

2,4

0,150

14.

0,15

0,112

 

2.6. Make a report:

 

1.      One gas contains 82.35% nitrogen and 17.65% hydrogen. Considering that the density of the gas in relation to hydrogen is 8.5, determine its molecular formula.

2.      When 0.24 g of nitrogen is combined with hydrogen, usually 168 m of nitrogen and 0.27 g of water are formed. Considering that the density of this substance in relation to air is 1.1, determine the molecular formula of organic matter..

3.      The substance contains potassium, chlorine, oxygen. Upon complete decomposition of 1.02 grams of this substance, 0.62 g of potassium chloride is formed. Create a simple formula for the substance to be decomposed.

4.      The substance contains potassium, sulfur and oxygen. 0.87 grams of this substance is released as sulfur and oxygen in barium sulfate. Considering that the mass of the resulting barium sulfate is 1.167 g, determine the simple formula for the starting material.

5.      Sodium nitrate, potassium nitrate, calcium nitrate, ammonium nitrate are used as fertilizers to increase the amount of nitrogen in the soil. Which of these salts contains the most nitrogen and what percentage?

6.      From 14.4 g of the sulfur-containing substance, 23.3 g of barium sulfate are obtained. Determine the percentage of sulfur in the test substance.

7.      Heating 200 g of crystalline soda Na2CO10*10H2O gives 63.6 g of anhydrous sodium carbonate. What percentage of the obtained crystalline soda contains impurities.

8.      How many grams of phosphorus / V / oxide is formed when 8 moles of phosphorus are burned in oxygen?

9.      6.02.1024 How many moles of iron / III / oxide are formed during the decomposition of iron hydroxide / III /?  

10.  How many liters of hydrogen are usually formed when 0.5 mol of sodium gyroxide reacts with water?

11.  As a result of the interaction of iron sulfate and potassium hydroxide, 1.07 g of iron (III) hydroxide is formed. How many moles of potassium hydroxide were involved in this reaction?.

12.  Typically, 22.4 ml of hydrogen is used to reduce copper / II oxide. How many water molecules are formed as a result of this reaction?

13.  For the reaction, 10 g of sulfuric acid was added to a vessel containing 5.6 g of potassium hydroxide. What compound is used in excess.

14.  Under normal conditions 10 g of calcium hydroxide and 2.24 liters of carbon monoxide reacted. As a result of this reaction, what substance is left in excess and how much calcium carbonate is formed.

15.  Calculate the volume of air with a mass of 5 kg at a pressure of 101.325 * 103 Pa and a temperature of 170 ° C.

 

 

2. Module II. Nuclear construction. Chemical bond. 

 

Section I. Atomic construction.

1.1. Theoretical questions.

  1. Rutherford's planetary model of the atom. What are the disadvantages of this model?
  2. Explain why the spectrum of the hydrogen atom is linear?
  3. Explain the physical meaning of the wave function of an electron, "potential density", orbital.
  4. What quantum numbers describe the energy state of an electron in an atom??
  5. Calculate the number of levels of energy level IV, where the value of the principal quantum number n = 4?
  6. If the number of the main quantum is n = 4, what are the values ​​of the additional and magnetic quantum numbers? The magnetic quantum number indicates what characteristics of a given orbital?
  7. What is the meaning of the Pauli principle? Could there be neutrons p7, d12, p4, d3 at the levels of the atom??  
  8. Give the first and current definition of the law of the period. Which of the two is correct??
  9. What are isotopes? Can atoms of different elements have the same mass? What do you call these atoms?
  10. If a) the ordinal number of the atom in the periodic table; b) period number; c) If the group number is known, what characteristics of this element can be determined?
  11. Construct a sequence of filling the bonds of atoms according to Klechkovsky's rules..
  12. What is the binding energy of electrons? How the oxidizing properties of non-metals change in the period and group in ascending order of the number of elements in the periodic table?
  13. What is ionization energy? In what units is it measured? How do the redox properties of S and P elements change in the ascending group of elements of the periodic table?
  14. What is electrical conductivity? As the ordinal number of elements in the periodic table increases, how does the electrical resistance change in the period and group of P-elements?
  15. Can different items weigh the same?
  16. Write electronic and electronic graphic formulas of atoms of elements and determine to which electronic types they belong. (S, P, D, f).

 

  1. Sodium, selenium, californium, tantalum.
  1. Lithium, chlorine, osmium, thulium.
  1. Calcium, tin, tungsten, erbium.
  1. Beryllium, argon, rhenium, holmium.
  1. Potassium, niobium, antimony, samarium.
  1. Magnesium, bromine, hafnium,              americium.
  1. Strontium, zinc, iodine, gadolinium..
  1. Barium, bismuth, cobalt, uranium.
  1. Cesium, xenon, manganese, neodymium..
  1. Neon, calcium, nickel, thorium.
  1. Rubidium, indium, iron, cerium..
  1. Francium, tin, zirconium, lanthanum.
  1. Radium, nitrogen, vanadium, neodymium..
  1. Fluorine, strontium, niobium, promethium.
  1. Sulfur, barium, ruthenium, europium..
  1. Oxygen, rubidium, palladium, europium
  1. Phosphorus, cesium, cadmium, dysprosium
  1. Селен, магний, серебро, нептуний
  1. Krypton, sodium, chromium, holmium.
  1. Lead, calcium, gold, plutonium.
  1. Iodine, lithium, tantalum, thulium..
  1. Indium, hydrogen, copper, ytterbium.
  1. Helium, bismuth, rhodium, terbium..

24.  Barium, carbon, technetium, cerium.
  1. Xenon, calcium, cobalt, gadolinium

 

                        

1.3. If the arrangement of electrons in the outer electron shell is as follows, in which group and period the element is located (write electron-graphic formulas and determine the valence electrons in the normal and excited states).

 

1.

2s2p3

2.

3s23p4

3.

3d104s2

4.

3d34s2

5.

2p63s1

6.

3p64s1

7.

2s22p4

8.

3d104p1

9.

3d74s2

10.

3d104s24p3

11.

3d54p1

12.

3d84s2

13.

5s25p1

14.

4d15s2

15.

4d95s2

16.

2s22p5

17.

4d105s2

18.

3s23p5

19.

4d25s2

20.

3d104p2

21.

4p65s2

22.

2s22p2

23.

3s23p4

24.

4d105p2

25.

4d105p5

 

 

 

 

 

1.4.   Write the electronic formula of elements for a given oxidation state:

 

1.

Fe(+3)

2.

Na(+1)

3.

Mo(+4)

4.

S(-2)

5.

Mg(+2)

6.

Cl(-1)

7.

Ca(+2)

8.

K(+1)

9.

O(-2)

10.

Fe(+6)

11.

S(+6)

12.

Mo(+6)

13.

Sb(+5)

14.

Cu(+2)

15.

Nb(+3)

16.

Nb(+5)

17.

W(+6)

18.

Cr(+3)

19.

N(+5)

20.

V(+5)

21.

Mn(+7)

22.

Mn(+2)

23.

As(+5)

24.

Ni(+2)

25.

N(-3)

 

 

 

 

 

 

Section II. Chemical bond.

 

2.1. Теоретические вопросы

 

1.      Explain the nature of chemical bonds and the distribution of energy when atoms form a molecule..

2.      Basic principles of the theory of valence bonds.

3.      What is a covalent bond?

4.      Depending on which covalent bond?

5.      What covalent bond is called _, _ bond? Indicate the types of orbitals formed by these connections.

6.      What is the most important reason for the hybridization of atomic orbitals sp, sp, sp What is the spatial arrangement of the hybridized orbitals relative to the central atom?

7.      What chemical bond is an ionic bond? What is the mechanism of its formation?

8.      Indicate the spatial configuration (location) of CH4 (109.50), NH3 (107.30), H2O (104.50) molecules, compare their bond angles and explain their change..

9.      Which molecule: BF3 and NH3 has a dipole moment of 0? Why?

10.  What is the electrical moment of a dipole? Which of the molecules - HCl, HBr, Hl - has the highest dipole moment?

11.  Basic principles of the MO-AOSK theory.

12.  What are the rules for the arrangement of valence electrons of atoms at the levels of energy diagrams of molecules?

13.  What is Electric Dipole Moment?

14.  Write down the electronic configuration of the molecule by the MO method?

15.  How to arrange the order of bonds in a molecule using the MO method?

16.  What is a paramagnetic molecule?

17.  How the MO method explains the paramagnetic properties of a molecule?

 

2.2. Consider the formation of a molecule by the valence bond method. Specify connection types.  

 

1.

HCl

2.

H2S

3.

PCl3

4.

NH3

5.

BeCl2

6.

CH4

7.

BeF2

8.

SiH4

9.

H2Se

10.

ZnCl2

11.

HF

12.

PCl5

13.

BF3

14.

H2O

15.

NF3

16.

SF6

17.

PF5

18.

BCl4

19.

H2Te

20.

CCl4

21.

PCl3

22.

Cl2

23.

N2

24.

BH3

25.

HgCl2

 

 

 

 

 

 

 

2.3. Show the scheme of energy formation of a molecule by the MO method. Write an electronic formula. Determine the magnetic properties and contact order.

 

1.

Li2

2.

O2-

3.

H2+

4.

B2

5.

He2+

6.

H2

7.

O2

8.

N2

9.

NO

10.

NO-

11.

Cl2

12.

C2

13.

F2

14.

He2

15.

S2

16.

Br2

17.

P2

18.

CO

19.

F2+

20.

O22-

21.

Na2

22.

N2+

23.

K2

24.

O22+

25.

Ne2+