Control test questions. 1. Where is acid Cn and CM is the same:

 

1. Where is acid Cn and C_M is the same:

1) H₂SO₄ 3) HCl 5) H₂SO₃

2) H₃PO₄ 4) H₂CO₃

2. Mass fraction of a solution consisting of 200 g. of water and 40 g. of glucose, is:

1) 0.32 3) 2.4 5) 4.2

2) 0.16 4) 3.2

3. Where is a base Cn twice larger than C_M:

1) LiOH 3) Ca(OH)₂ 5) Fe(OH)₃

2) Al (OH)3 4) KOH

4. The equation for calculating the molar concentration:

1) C_M = m / M 3) C_M = n / mV 5) C_M = MV / m

2) C_M = n / M ^. V 4) C_M = m / M ^. V

5. The equation for calculating the titer:

1) T = N ^. E / 1000 3) T = N ^. 1000 / E 5) T = N ^. M / 1000

2) T= m_sub / m_sol 4) T = E ^. 1000 / N

6. The weight of potassium permanganate required for the preparation of 50 g 5 % solution:

1) 1.5 g 3) 10 g 5) 25 g

2) 5.1 g 4) 2.5 g

7. The expression for calculating the normal concentration:

1) 3) 5)

2) 4)

8. The mass fraction of the solution consisting of 80 g H₂O and 20 g NaCl:

1) 0.8 3) 0.2 5) 0.02

2) 0.1 4) 0.4

9. The equation for calculating the mass fraction (%)

1) 3) 5)

2) 4)

10. If at this temperature the solute is not soluble, such a solution is:

1) a saturated 3) unsaturated 5) homogeneous

2) diluted 4) supersaturated

11. Mass fraction of solute - is:

1) the ratio of the mass of solute to the total weight of the solution

2) the mass of the solute in solution of 1000 g

3) the mass of the solute in 100 g water

4) The weight of the solute in 100 g solvent

5) the mass of the solute in 1 liter of solution

12. In the 1 liter of solution contained 20 g of NaOH. The molar concentration of this solution is:

1) 0.1 M 3) 0.5 M 5) 2 M

2) 0.2 M 4) 1 M

13. In 250 ml of a solution of 4.9 g of H₂SO₄. Equivalent concentration of this solution is:

1) 0.52 n 3) 1.05 n 5) 0.1 n

2) 0.32 n 4) 0.4 n

14. To prepare 500 g 10% solution of glucose is necessary to take glucose:

1) 60 g 3) 98 g of 5) 25 g

2) 50 g of 4) 40 g

15. How many grams of copper sulfate should be taken to prepare

250 ml of 0.25 M solution:

1) 12 g 3) 25 g 5) 30 g

2) 10 g 4) 15 g

16. To prepare 100 g of a 5% solution of salt is necessary to take:

1) 7.5 g 3) 10.0 g 5) 0.5 g

2) 2.5 g 4) 5.0 g

17. Unit of Titres:

1) mol / ml 3) mol 5) mol / kg

2) g / ml 4) moles / l

18. Unit of measurement equivalent concentration:

1) %  3) mol / l 5) g / mol

2) g / cm³ 4) mol / kg

19. Unit of measurement of the molar concentration:

1) mol / l 3) mol / kg 5) g / mol

2) g / cm³ 4) moles

20. Factor equivalence Ca (NO₃)₂:

1) 1/3 2) 1/2 3) 2 4) 1 5) 1/5

21. To prepare 100 ml of a 0.2 N solution of calcium chloride to take:

1) 4.12 g 2) 1.11 g 3) 0.75 g 4) 10.21 g 5) 7.5 g

22. To prepare 200 ml of a 0.5 N solution of potassium nitrate to take:

1) 24.5 g 2) 16.2 g 3) 54.4 g of 4) 8.5 g of 5) 10 g

23. To prepare 2 liters of a 0.1 N solution of potassium nitrate to take:

1) 20.2 g 2) 6.2 g 3) 4 g 4) 0.1 g 5) 10 g

24. How many moles contained in 250 g of calcium sulphate:

1) 1.8 moles 2) 6 moles 3) 2 moles 4) 3 moles 5) 0.5 mole

25. Normal concentration corresponding to a 1 M solution of H₂SO₄:

1) 1 n 2) 2 n 3) 0,5 n 4) 0,1 n 5) 0,25 n

26. Factor equivalence Al₂ (SO₄) ₃:

1) 1/4 2) 1 3) 1/2 4) 1/6 5) 1/3

27. Expression of molal concentration is:

1) C_m = n_вещ-ва / m _р-ля 3) C_m = n_р-ля / m_вещ-ва 5) C_m = n /V

2) C_m = n _вещ-ва /V 4) C_m = n / М^.m

28. Expression of the normal concentration is:

1) C_Н = m /V 3) C_Н = m / Э ^. V 5) C_Н = n / V

2) C_Н = m₁/m₂ 4) C_Н = n / m

29. Unit of measurement of mass fraction:

1) %  3) moles / l 5) mol / kg

2) g / l 4) g / ml

30. Factor of equivalence H₃PO₄:

1) 1/2 2) 1 3) 1/3 4) 3 5) 1/4

 

 

Theme number 2: Chemical kinetics. Factors affecting the rate of reaction.

 

The purpose of the activity: Cformirovat knowledge about the teachings of the rate and mechanism of chemical reactions, the doctrine of chemical equilibrium (the principle of Le Chatelier-Braun), learn the basic concepts and laws of chemical kinetics, the influence of different factors: the nature and concentration of the reactants, temperature, pressure, catalyst the rate of chemical reactions.

 

The main questions of the theme:

 

1. What is the subject of studying chemical kinetics?

2. What is called the speed of a chemical reaction? As it is expressed for homogeneous and heterogeneous reactions?

3. State the law of mass action (Guldberg and Waage law) and write their mathematical expressions for the rates of the forward and reverse reactions.

4. What is called the order and molecular reactions?

5. Effect of pressure and temperature on the reaction rate.

6. An approximate rule of van't Hoff and his mathematical expression.

7. The activation energy and the Arrhenius equation.

8. Effect of catalysts on the reaction rate. Positive and negative catalysis. Homogeneous and heterogeneous catalysis.

9. The role of catalysis in the vital activity of living organisms. Enzymatic reactions. Meaning enzymes. Michaelis-Menten equation.

10. What is called chemical equilibrium?

11. The equilibrium constant and its physical meaning.

12. State the principle of Le Chatelier - Brown.

13. Effect of temperature, concentration of reactants, and the pressure on the direction of displacement of the chemical equilibrium in reversible reactions.

Methods of teaching and learning: effective formative feedback on the development of competencies, training in small groups SGL.

 

Literature

1. Lenski A.S.Introduction to bioinorganic and biophysical chemistry.- М.: VW, 1989.- 256 page.

2. Glinka N.L.. General chemistry.Edited by V.A. Rabinovich.- L.: Chemistry,1988.- 704 с.

3.Glinka N.L.. exercises and works in chemistry.Edited by A.Rabinovich and X.MRubin.- Chemistry 1985.- 264 page.

4Vasileva Z.G., Granovskaya А.А., Taperova А.А. Laboratorial works in inorganic chemistry.- Chemistry, 1986. - 288 page.

5.Lectures and synopsis.

6.Ahmetov N.B. Genaerally and inorganic chemistry. М.: VW, 1981. – 679 page.

Control test questions:

 

1. With increasing concentration of the reactants the reaction rate:

1) is increased 3) is not changed

2) decreases 4) no correct answer

5) significantly reduced

2. The activation energy determines:

1) the chemical equilibrium

2) the possibility of chemical interaction

3) a chain reaction

4) parallel reactions

5) the order of reaction

3. The temperature coefficient of the reaction (g = 2). When the temperature rises to 20 ° C the reaction rate increases:

1) 3 times 3) 4 times 5) is reduced by 4 times

2) 2 times 4) does not change

4. The temperature coefficient of the reaction (g = 2). When the temperature is lowered to 30 ° C the reaction rate change:

1) decreases by 6 times 3) decreases by 8 times 5) does not change

2) increase of 6 times 4) increase of 8 times

5. To direct the endothermic reaction shifts the equilibrium temperature increase:

1) left 3) does not change

2) right 4) no correct answer

6. The law of mass action:

1) chemical reaction rate is directly proportional to the product of the concentrations of the reactants

2) at increasing temperature every 10 ° C, the reaction rate increases by 2-3 times

3) the rate of a chemical reaction is the change in the amounts of reactants per unit time per unit volume of the system

4) chemical reaction rate is the change amounts of the reactants per unit of time per unit of interfacial surface

5) if the system is in equilibrium, outside influence, the system processes develop, shifts the equilibrium in the direction in which the effect is produced by the impact will be weakened

7. The temperature coefficient of the reaction g = 3. When the temperature rises to 40 ° C, the reaction rate increases:

1) 21 times 3) 81 times 5) 43 times

2) 27 times 4) 12 times

8. With increasing concentration of the reactants equilibrium constant:

1) does not change 3) decreased 5) tends to infinity

2) increase 4) tends to zero

9. Effect of catalyst on the rate of chemical reaction is:

1) to reduce the activation energy

2) to increase the activation energy

3) to increase the number of active molecules

4) active in reducing collisions

5) in the constancy of the activation energy

10. When the temperature rises from 10 ° C to 50 ° C the reaction rate increased by 16 times. The temperature coefficient of this reaction is:

1) 3 3) 2.5 5) 3.5

2) 2 4) 1.5

11. The temperature coefficient is equal to 3. When the reaction temperature rises from 40 ° C to 70 ° C the reaction rate increases:

1) 30 times 2) 18 times 3) 3 times 4) 27 times 5) 21 times

12. As the temperature increases the reaction rate increases, where in:

1) the number of collisions is not changed

2) the average kinetic energy of the molecules decreases

3) the number of active molecules increases

4) the number of active molecules decreases

5) the number of collisions decreases

13. For the reaction 2H₂ (g) + O₂ (g) = 2H₂O (g) the mathematical expression of the law of mass action has the following form:

1) u=k [H₂]^.[O₂]³ 3) u=k [H₂]^2.[O₂]

2) u=k [H₂]^.[O₂] 4) u=k [H₂]

5) u=k [H₂О]²

14. For the reaction Cl₂ + H₂ = 2HCl mathematical expression of the law of mass action has the following form:

1) u=k [Cl₂] + [H₂] 3) u=k [Cl] + [H]³

2) u=k [Cl₂]^.[H₂] 4) u=k [HCl]

5) u=k [Cl₂] - [H₂]

 

15. In the system of N₂ + 3H₂ = 2NH₃ increase in pressure will shift the equilibrium:

1) left 2) right 3) does not change 4) no correct answer

16. The system N₂ + 3H₂ = 2NH₃ with increasing concentration of N₂ equilibrium shift:

1) right 2) left 3) does not change 4) no correct answer

17. The equilibrium constant for the reaction N₂ + 3H₂ = 2NH₃:

1) 3)

 

2) 4) 5)

18. The system 2NO + O₂ ® 2NO₂, if the volume of the reaction vessel 2 times the speed of the direct reaction:

1) decreased by 4 times 3) increased by 4 times 5) increased by 2 times

2) reduced by 8 times 4) increased by 8 times

19. On the basis of the law of mass action expression rate of a chemical reaction 2Fe_(тв) +3Cl_2(г) = 2FeCl_3(тв) has the form:

1 1) u=k [Cl₂]³ 3) u=k [Fe] 5) u=k [Cl₂]

2) u=k [Fe][Cl₂] 4) u=k [Fe] ² [Cl₂]³

 

20. The system CaCO_3(к) Û CaO_(к)+CO_2(г); DH=179 kJ (кДж) at higher temperatures the equilibrium will shift:

1) left 2) right 3) does not change 4) no correct answer

21. When the concentration of NO increased in 4 times the speed of the direct reaction

2NO + Cl₂ Û 2NOCl:

1) increase by 4 times 3) increased by 16 times

2) reduced by 16 times 4) decreases by 12 times

5) decreases by 4 times

22. The system Cl₂ + H₂ = 2HCl with decreasing volume, the balance will shift:

1) left 2) right 3) does not shift 4) no correct answer

23. On the basis of the law of mass action, rate expression for the reaction 2NO + O₂ ® 2NO₂ is:

1) u=k [NO]²[ O₂] 3) u= k[NO₂] 5) u=k [NO₂]²

2) u=k [NO][O₂] 4) u=k [O₂]

 

24. For the reaction 4NH₃+ 5O₂ Û 4NO+ 6H₂O, the equilibrium constant expression is:

1) K = k [NH₃]⁴[O₂]⁵ 3) K = k[NO]⁴[H₂O]⁶ 5)

2) 4)

25. When the pressure in the system 2F_2(г)+2Н₂О_(г)Û 4HF_(г)+O_2(г), the equilibrium will shift:

1) left 2) right 3) does not shift 4) no correct answer

26. When the concentration of hydrogen 3 times N₂ (g) + 3H₂ (g) = 2NH₃ (g) reaction rate:

1) increases by 81 times 3) decrease in 9 times

2) increased by 9 times 4) increase in 5 times 27) is reduced by 27 times

27. In the system of N₂ (g) + 3H₂ (g) = 2NH₃ (g) when the pressure balance will be shifted:

1) toward the reverse reaction

2) in the direction of the direct reaction

3) does not shift

28. By reducing the volume of the reaction vessel at 5 times the rate of reaction

2NO (g) + O₂ (g) = 2NO₂ (g):

1) increases 5 times 3) increase 125 times

2) reduced 5 times 4) is reduced to 75 times 5) is reduced 125 times

29. The temperature coefficient of the reaction is equal to 3.When the temperature rises to 10 ^o C the reaction rate will increase:

1) 33 times 2) in 30 times 3) in 3.3 times 4) 3 times 5) 10 times

30. For the reaction of C (k) + O₂ (g) = CO₂ (g) the expression of the law of mass action has the form:

1) u=k [C] [O₂] 3) u=k [O₂] 5) u=k [C]

2) u=k [CO₂] 4) u=k [O₂] /[CO₂]

 

 

Theme number 3: Acid-base balance in life processes. The ionic product of water. Hydrogen index as a quantitative measure of the active acidity and alkalinity. Buffer systems.

 

The purpose of the activity: Cformirovat knowledge on the theory of electrolytic dissociation, learn the basic definitions and terms on this topic, highlighting the role of electrolytes in the activity of organisms.

 

The main questions of the theme:

 

1. Expand the essence of electrolytic dissociation of Arrhenius. What are the weaknesses of this theory. What are its advantages?

2. Modern physico-chemical theory of solutions of electrolytes (theory and I.A.Kablukova V.A.Kistyakovskogo).

3. Explain the process of solvation and hydration, based on chemical theory of solutions Mendeleev.

4. What substances are called electrolytes? Strong and weak electrolytes. Give examples.

5. What is the degree of electrolytic dissociation? How to change the value of the degree of electrolytic dissociation, depending on the strength of the electrolyte?

6. Formulate Law of dilution and write its mathematical expression.

7. The application of the law of mass action to the processes of dissociation of weak electrolytes. What characterizes the electrolytic dissociation constant and what factors it zavisisit?

8. The theory of strong electrolytes and P.Debaya E.Hyukkelya.

9. What is called the activity and how is it calculated?

10. How is the ionic strength of the solution and the activity coefficient?

11. The electrolytic dissociation of water. What is called the ionic product of water? What did it matter? Output value of the ion product of water.

12. Hydrogen and gidrokislny indicators.

13. What substances are called indicators? Their use in chemical practice.

14. What system called buffer?

15. As classified buffer systems?

16. As the pH buffer system is calculated, a weak acid and a salt of the acid? Give a formula to calculate the pH of this buffer solution?

17. How do you calculate the pH of the buffer system, weak base - salt of this base? Give a formula to calculate the pH of the buffer solution.

18. What is called the buffer capacity? What it depends on, and how can it be calculated?

19. What buffer systems in the human body maintain a constant pH in blood and tissue fluids?

20. What is the value of the buffer systems to the human body?

Methods of teaching and learning: effective formative feedback on the development of competencies, training in small groups SGL, training based on teamwork TBL.

 

Literature

1. Lenski A.S.Introduction to bioinorganic and biophysical chemistry.- М.: VW, 1989.- 256 page.

2. Glinka N.L.. General chemistry.Edited by V.A. Rabinovich.- L.: Chemistry,1988.- 704 с.

3.Glinka N.L.. exercises and works in chemistry.Edited by A.Rabinovich and X.MRubin.- Chemistry 1985.- 264 page.

4Vasileva Z.G., Granovskaya А.А., Taperova А.А. Laboratorial works in inorganic chemistry.- Chemistry, 1986. - 288 page.

5.Lectures and synopsis.

6.Ahmetov N.B. Genaerally and inorganic chemistry. М.: VW, 1981. – 679 page.

Control test questions:

 

1. Mathematical expression law of dilution:

1) 3)

2) 4) 5)

2. Expression of the ion product of water:

1) K_W = [H⁺]^. [OH^-] 2) 3)

4) 5)

3. The equation of the hydroxyl index:

1) pOH = -lg [H⁺] 3) pOH = -lg [OH^-]

4) pOH= - lg[C_кисл.]

2) 5) pOH= 14 + рН

4. The equation of hydrogen index:

1) pH = -lg [H⁺] 2) 3)

4) pH= - lg[C_b] 5) рН = - lg [ОH^-]

 

5. The dissociation constant of hydrocyanic acid:

1) 2) 3)

4) K _д= [H⁺] [CN^-] 5) K _д= [НCN]

6. [H⁺] = 10^-4 mol / l, the pH value is:

1) рН=2 2) рН=10 3) рН=4 4) рН=8 5) рН= 6

7. [H⁺] = 10^-3 mol / l, pOH value is:

1) рОН=9 2) рОН=11 3) рОН=3 4) рОН=13 5) рОН = 7

8. By increasing the pH value per unit concentration of hydrogen ions in solution:

1) decreases by 10 times 3) decreases by 100 times

2) increased 10 times 4) increases 100 times

5) no change

9. When the pH is increased to 3 units, the concentration of hydrogen ions in solution:

1) decreases by times 100 3) increased by 100 times

2) reduced 1000 times 4) increases 1000 times

5) decreases by 3 times

10. [H⁺] = 10^-8 mol / l, the concentration [ОH^-] is:

1) 10^-5 mol / l 3) 10^-6 mol / l 5) 10^-10 mol / l

2) 10^-4 mol / l 4) 10^-8 mol / l

11. Law of dilution is valid for:

1) dilute solutions of weak electrolytes

2) non-electrolyte solutions

3) dilute solutions of electrolytes

4) concentrated solutions of electrolytes

4) solutions of strong electrolytes

12. Expression of the degree of dissociation:

1) a = N_общ / n_дис 2) a =n_дис / N_общ 3) a = N_общ /n_{число ионов}

4) a = n_{число ионов} ^. N_общ 5) a=N_общ – n_дис

 

13. The dissociation constant of CH₃COOH:

1) 3)

2) 4)

5) К_д= [H⁺] ^. [CН₃СОО^-]

14. The dissociation constant of HNO₂:

1) 3)

2) 4) 5) К_д= [H⁺] ^. [NO₂^-]

15. The ionic product of water is equal to:

1) K_w = 10¹⁴ 2) K_w = 10^-10 3) K_w = 10^-14 4) K_w =10^-7 5) K_w =10⁷

16. The concentration of hydrogen ions in solution of 10^-2 mol / l, the pH value of the solution:

1) рН=3 2) рН=2 3) рН=1/2 4) рН=0,2 5) рН= 12

17. Hydrogen ion concentration (mol / l) at pH = 3 is:

1) [H⁺] = 10¹³ 2) [H⁺] = 10³ 3) [H⁺] = 10^-3 4) [H⁺] = 10^-5 5) [H⁺] = 10^-11

18. Hydrogen ion concentration (mol / l) at pOH = 4 is:

1) [H⁺] = 10^-4 2) [H⁺] = 10^-5 3) [H⁺] = 10¹⁰ 4) [H⁺] = 10^-10 5) [H⁺] = 10^-2

19. The concentration of hydroxyl ions (mol / l) at pH = 5 is equal to:

1) [ОH^-] = 1 ^.10^-10 2) [ОH^-] = 1 ^.10⁵ 3) [ОH^-] = 1 ^.10^-9 4) [ОH^-] = 1^.10^-5

5) [ОH^-] = 1 ^.10^-8

20. Weak electrolyte:

1) H₃PO₄ 3) KCl 5) КОН

2) NaCl 4) H₂SO₄

21. Strong electrolyte:

1) NH₄OH 3) Be(OH)₂ 5) СН₃СООН

2) Mg(OH)₂ 4) KOH

22. In dilute solution dissociation occurs reversibly:

1) KOH 3) NaOH 5) НСl

2) NH₄OH 4) Ba(OH)₂

23. pH 0.01 N KOH solution is equal to:

1) 2 2) 0.01 3) 12 4) 14 5) 10

24. The pH of the 0.1 M solution of NH₄OH (a= 0,01) is:

1) 12 2) 2 3) 3 4) 11 5) 8

25. The pH of a 0.1 M solution of acetic acid К_Д = 1,8^. 10^-5 (pK = 4,76) is equal to:

1) 2.88 2) 3.55 3) 1.0 4) 10.5 5) 12

26. The pH of 0.001 M formic acid (a= 0,1) is equal to:

1) 3 2) 6 3) 4 4) 2 5) 7

27. When added to 1 l of water 10^-2 mol NaOH, the pH of the solution:

1) will increase by two units 3) reduced by two units

2) increase by five units 4) decrease by five units

5) decreases by one unit

28. To increase the pH to 2 units, a hydrogen ion concentration is necessary to:

1) reduce to 100 times 3) increased 10 times

2) to reduce to 10 times 4) increase 100 times

5) increased 2 times

 

29. The degree of dissociation of a 0.2 N solution of weak monobasic acid is 0.03. The quantity pOH of this solution equal:

1) 11.78 2) 6.4 3) 3.2 4) 7 5) 3.6

30. The pH value of blood is 7.53, then the concentration of hydrogen ions is:

1) 2,3^. 10^-7 3) 2,95^. 10^-8 5) 8,2^. 10^-3

2) 1,27^. 10^-5 4) 0,01

Theme number 4: The nature of the chemical bond. Biogenic s-, p-, d-elements and their biological role.

 

Session Purpose: To study the chemical properties of biogenic elements (s-, p-, d-, f-elements), to disclose the value of the macro- and micronutrients for the life of the organism.

 

The main questions of the theme:

 

1. The structure of the atom and the four main characteristics of the energy state of an electron in an atom.

2. What characterizes the main, side or orbital magnetic and spin quantum number?

3. State the Pauli exclusion principle.

4. Give the definition of the principle of least energy.

5. Give two formulations Aufbau principle.

6. Formulate Hund's rule.

7. What elements of the Mendeleev periodic table are s-elements? What properties are characteristic of them. Give examples.

8. What elements belong to the p-elements? What properties exhibit p-elements? Give examples.

9. What elements are among the d-elements? What are the chemical properties characteristic of the d-elements?

10. What elements are among the f-elements? Give examples.

11. The concept of the biosphere and biogenic elements. Classification of nutrients. The biological role of the elements in the life of the organism.

Methods of teaching and learning: effective formative feedback on the development of competencies, training in small groups SGL, task-based learning TaskBL.

 

Literature

 

1. Lenski A.S.Introduction to bioinorganic and biophysical chemistry.- М.: VW, 1989.- 256 page.

2. Glinka N.L.. General chemistry.Edited by V.A. Rabinovich.- L.: Chemistry,1988.- 704 с.

3.Glinka N.L.. exercises and works in chemistry.Edited by A.Rabinovich and X.MRubin.- Chemistry 1985.- 264 page.

4Vasileva Z.G., Granovskaya А.А., Taperova А.А. Laboratorial works in inorganic chemistry.- Chemistry, 1986. - 288 page.

5.Lectures and synopsis.

6.Ahmetov N.B. Genaerally and inorganic chemistry. М.: VW, 1981. – 679 page.

Control test questions:

1. The electronic formula of atomic Na:

1) 1s²2s²2p⁶3s¹ 3) 1s²2s²2p⁴3s¹ 5) 1s²2s²2p⁶3s²

2) 1s²2s²2p⁵3s¹ 4) 1s²2s²2p³

2. E-atom formula Mg:

1) 1s²2s²2p⁴3s¹ 3) 1s²2s²2p⁶3s² 5) 1s²2s²2p⁶3s²3p²

2) 1s²2s²2p⁶3s¹ 4) 1s²2s²2p⁴3s²

 

3. Electronic formula atom K:

1) 1s²2s²2p⁶3s⁶4s¹ 3) 1s²2s²2p⁶3s²3p⁴ 5) 1s²2s²2p⁶3s²3p⁵

2) 1s²2s²2p⁶3s²3p⁶4s¹ 4) 1s²2s²2p⁶3s² 3p⁴4s¹

 

4. Refers to the d - elements:

1) P 3) As 5) Hg

2) Rb 4) Ba

5. Refers to the s - elements:

1) Zn 3) Fe 5) Hg 2) Cu 4) Ra

6. Shows amphoteric properties:

1) Zn(OH)₂ 3) Mn(OH)₂ 5) Ca(OH)₂

2) Fe(OH)₂ 4) Cr(OH)₂

7. Electronic formula corresponding atom Zn:

1) 1s²2s²2p⁶3s²3p⁵4s²3d¹⁰ 3) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

2) 1s²2s²2p⁶3s²3p⁶4s² 3d⁷ 4) 1s²2s²2p⁶3s²3p⁶4s²3d⁸

5) 1s²2s²2p⁶3s²3p⁶4s²3d⁹

8. s - elements include:

1) Na, B, C 3) K, Be, Mg 5) N, P, As

2) Li, Pb, Zn 4) Cl, P, Na

9. s - elements include:

1) Ca, Mg, Be 3) Li, H, Cl 5) Cu, Ag, Au

2) Pb, Nb, Mg 4) F, Co, Ni

10. s - elements include:

1) Ag, Au, Cu 3) Zn, Ca, Ge 5) As, Sb, Bi

2) Rb, Cs, Fr 4) Be, B, O

11. d - elements include:

1) Zn, Ca, Ge 3) Ca, K, S 5) F, Cl, Br

2) O, F, Cl 4) Zn, Cu, Ag

12. d - elements include:

1) Zn, Ca, Ge 3) Cr, Mn, Fe 5) F, Cl, Br

2) O, F, Cl 4) C, N, O

13. d - elements include:

1) Sb, Te, I 3) S, Cl, Fe 5) O, Se, I

2) Ru, O, F 4) Hg, Ag, Au

14. Electronic structure of the outer energy level of an atom of Ca:

1) 4s² 3) 4s¹3p⁶ 5) 3s²

2) 4s¹ 4) 4s⁰3p⁸

15. Electronic structure of the outer energy level of an oxygen atom:

1) 2s¹3p⁵ 3) 2s⁰3p⁶ 5) 2s²2p³

2) 2s²2p⁴ 4) 2s²2p⁶

16. Electronic structure of the outer energy level of phosphorus atom:

1) 2s²3p³ 3) 3s²3p³ 5) 2s²2p²

2) 3s²3p⁴ 4) 3s²3p⁵

17. d - elements include:

1) Cu, Zn, Ca 3) Cu, Au, Ag 5) Cl, Br, I

2) Cu, Zn, S 4) K, Zn, Ca

18. p - elements include:

1) Mn, Co, Fe 3) F, Cl, Br 5) K, Rb, Cs

2) B, C, Ni 4) B, Be, Li

19. p - elements include:

1) P, S, C 3) Se, Te, Pd 5) Li, Ca, Ba

2) Ti, V, Cr 4) B, Al, Cu

20. d - elements include:

1) Zn, Nb, Mo 3) Cr, Mn, Cl 5) Cs, Ba, Ra

2) O, F, Cl 4) Al, Si, Li

21. The element with the highest electronegativity:

1) Cl 3) F 5) Ca

2) O 4) N

22. A compound, where in the degree of oxidation of nitrogen is 5:

1) HNO₃ 3) NaNO₂ 5) NO₂

2) NO 4) NH₃

23. A compound, wherein the degree of sulfur oxidation is 4:

1) К₂SO₄ 3) SO₃ 5) Na₂S₂O₃

2) (NH₄)₂SO₃ 4) Na₂S

24. A compound, wherein the degree of oxidation of chlorine is 3:

1) HClO₄ 3) HClO₃ 5) HCl

2) HClO 4) HClO₂

25. The strongest acid:

1) HCl 3) HOCl 5) HClO₂

2) HOBr 4) HBr

26. Electronic structure of the outer energy level of an atom Li:

1) 2s² 2) 1s¹ 3) 2s¹ 4) 2s²2p¹ 5) 2s²2p²

27. With the increase in the number of electrons in the outer energy level of p-elements in periods from left to right their electronegativity:

1) increases 2) is reduced 3) is not changed 4) equals zero

5) there is no right answer

28. With the reduction of the number of electrons in the outer energy level of the p elements in the periods from right to left their electronegativity:

1) increases 2) is reduced 3) is not changed 4) equals zero

5) there is no right answer

29. The element with the highest electronegativity:

1) C 2) B 3) S 4) O 5) N

30. Electronic structure of the outer energy level of an atom of aluminum:

1) 3s²3p¹ 2)3s¹3p⁴ 3) 3s¹3p² 4) 4s¹3p⁶ 5) 3s²3p⁶

 

 

Theme number 5: The complex compounds and their properties. Medical - biological role of complex compounds.

 

The purpose of the activity: to systematize knowledge of the main provisions of the coordination theory, learn the basic types, nomenclature and chemical properties of complex compounds.

 

The main questions of the theme:

1. The main provisions of the coordination theory A.Vernera.

2. Define the following terms: complexing agent (central ion), ligands, the inner coordination sphere, the outer coordination sphere, the coordination number.

3. Methods of establishing coordination complex compounds of formulas.

4. The main types of complex compounds: ammines, aqua complexes, acidocomplexes, cyclic (chelate) complex compounds, chelate compounds.

5. The range of complex compounds.

6. Dissociation of complex compounds in solution. Instability constants and stability constants of complex compounds.

7. Spatial structure and isomerism of complex compounds.

Methods of teaching and learning: effective formative feedback on the development of competencies, training in small groups SGL, training in using peer PAL.

 

Literature

1. Lenski A.S.Introduction to bioinorganic and biophysical chemistry.- М.: VW, 1989.- 256 page.

2. Glinka N.L.. General chemistry.Edited by V.A. Rabinovich.- L.: Chemistry,1988.- 704 с.

3.Glinka N.L.. exercises and works in chemistry.Edited by A.Rabinovich and X.MRubin.- Chemistry 1985.- 264 page.

4Vasileva Z.G., Granovskaya А.А., Taperova А.А. Laboratorial works in inorganic chemistry.- Chemistry, 1986. - 288 page.

5.Lectures and synopsis.

6.Ahmetov N.B. Genaerally and inorganic chemistry. М.: VW, 1981. – 679 page.