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Студенты: Алимханова Л., Корупаева Е., Масленников А., Тихомиров А., Шишкинская В., Машкова С., Голикова С., Корягина П., Голубева В., Власкина Е., Дёмина Ю., Вахрушева Д., Панкова С., Харитонов А., Горохова В. - зачёт принят автоматом по результатам посещения, выполнения аудиторной работы, а также домашних заданий.
Задания на сегодня:
1) Vocabulary - страница 6 - 20 своих предложений или 20 предложений из Ваших учебников по Химии, в которых употребляются эти фразы и слова.
Студенты: Алимханова Л., Корупаева Е., Масленников А., Тихомиров А., Шишкинская В., Машкова С., Голикова С., Корягина П., Голубева В., Власкина Е., Дёмина Ю., Вахрушева Д., Панкова С., Харитонов А., Горохова В. - зачёт принят автоматом по результатам посещения, выполнения аудиторной работы, а также домашних заданий.
Задания на сегодня:
1) Vocabulary - страница 6 - 20 своих предложений или 20 предложений из Ваших учебников по Химии, в которых употребляются эти фразы и слова.
1. triple covalent bond: A covalent bond formed by
atoms that share three pairs of electrons.
2. electron domain geometry: Geometry based only on the
total number of electron pairs around the central
atom, both bonding pairs and lone pairs.
3. molecular geometry: The three-dimensional
arrangement of atoms in a molecule.
4. valence shell: The outermost electron-occupied shell
of an atom.
5. valence shell electron pair repulsion: A theory for
predicting molecular geometries; it states that electron pairs will repel each other such that the valence
electron-pairs stay as far apart from each other as possible.
6. diatomic element: An element whose natural form is
of a diatomic molecule.
7. dipole: A molecule with two poles, a positive pole
and a negative pole; also called a polar molecule
8. dipole-dipole forces: The attractive forces that
occur between polar molecules; the positive end of one dipole is attracted to the negative end of a neighboring
dipole.
9. hydrogen bond: An intermolecular attractive force in
which a hydrogen atom that is covalently bonded to a
small, highly electronegative atom is attracted to a
lone pair of electrons on an atom in a neighboring molecule.
10. intermolecular forces: Attractive forces that occur
between molecules.
11. London dispersion forces: The intermolecular forces
that occur between all atoms and molecules due to the
random motion of electrons.
12. nonpolar covalent bond: A covalent bond in which the
bonding electrons are shared equally between the two atoms.
13. polar covalent bond: A covalent bond in which the
atoms have an unequal attraction for electrons, and so the sharing is unequal.
14. polar molecule: A molecule in which one end of the
molecule is slightly positive, while the other end is
slightly negative.
15. van der Waals forces: The weakest intermolecular
forces; they consist of dipole-dipole forces and dispersion forces.
16. hybridization: The mixing of the atomic orbitals in
an atom to produce a set of hybrid orbitals.
17. hybrid orbitals: The atomic orbitals obtained when
two or more nonequivalent orbitals from the same atom
combine in preparation for bond formation.
18. pi bond (p): A bond formed by the overlap of
orbitals in a side-by-side fashion with the electron density
concentrated above and below the plane of the nuclei
of the bonding atoms.
19. sigma bond (s): A bond formed by the overlap of
orbitals in an end-to-end fashion, with the electron density concentrated between the nuclei of the bonding atoms.
20. valence bond theory: A theory which states that the
electrons in a molecule are assumed to occupy atomic
orbitals of the individual atoms and that a covalent
bond results from overlap of those orbitals.
3) Text Book - https://www.ck12.org/book/CK-12-Chemistry-Intermediate/section/13.0/ - чтение/перевод/тесты
Алимханова
ОтветитьУдалитьChapter 13
Part 1
1. The particles of a gas may be either atoms or molecules. The distance between the particles of a gas is much, much greater than the distances between the particles of a liquid or a solid. Most of the volume of a gas, therefore, is composed of the empty space between the particles. In fact, the volume of the particles themselves is considered to be insignificant compared to the volume of the empty space.
2. a, d
3. Collisions between gas particles and between particles and the container walls are elastic collisions. An elastic collision is one in which there is no overall loss of kinetic energy.
4. One unit of gas pressure is the millimeter of mercury (mmHg). An equivalent unit to the mmHg is called the torr. The pascal (Pa) is the standard unit of pressure. A pascal is a very small amount of pressure, so a more useful unit for everyday gas pressures is the kilopascal (kPa). Another commonly used unit of pressure is the atmosphere (atm).
5. At sea level, a mercury column will rise a distance of 760 mm. Mercury is commonly used in barometers because its high density means the height of the column can be a reasonable size to measure atmospheric pressure. A barometer using water, for instance, would need to be 13.6 times taller than a mercury barometer to obtain the same pressure difference. This is because mercury is 13.6 times more dense than water.
6. At higher altitudes, the atmospheric pressure is lower, so the column of mercury will not rise as high. Drinking through a straw is slightly more difficult atop a mountain. This is because the reduced atmospheric pressure is less effective in pushing water up into the straw.
7. The temperature of a substance in Kelvin is directly proportional to the average kinetic energy of the particles in that substance. As a sample of matter is continually warmed, the average kinetic energy of its particles increases.
8. a. 1307,96 mm Hg
b. 74,53 kPa
c. 0,9 atm
d. 3,05 atm
9. 772 mm Hg is the pressure of the gas sample in the bulb.
10. 471С
11. The column of water would rise to 10500 mm.
Алимханова
ОтветитьУдалитьChapter 13
Part 2.
1. The primary difference between liquids and gases is that the particles of a liquid are much closer together, and there is very little empty space between them. Liquids are essentially not compressible and are far denser than gases.
2. The heating process results in a greater fraction of the liquid’s molecules having the necessary kinetic energy to escape the surface of the liquid. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and, thus, has a lower vapor pressure. When the liquid in a closed container is heated, more molecules escape the liquid phase and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure.
3. As the acetone evaporates from your skin, it removes heat from its surroundings. In this case, your skin. You feel the transfer of heat away from your skin as cold.
4. In a closed container the rate of evaporation is equal to the rate of condensation.
5. Boiling points are affected by external pressure. At higher altitudes, the atmospheric pressure is lower. With less pressure pushing down on the surface of the liquid, it boils at a lower temperature. This can also be seen from the vapor pressure curves.
6. The boiling point is the temperature at which the vapor pressure of a liquid is equal to the external pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the standard atmospheric pressure of 760 mmHg.
7. a. A
b. B
c. B
8. a. 150 mm Hg
b. 52°C
c. 88°C
d. liquid
9. The boiling point of water is 100°C at sea level, where the atmospheric pressure is close to the standard value. At 3000 m above sea level, the atmospheric pressure is lower, so water boils at about 90°C. On the other hand, water boils at temperatures greater than 100°C if the external pressure is higher than the standard value. Pressure cookers do not allow the water vapor to escape, so the total pressure inside the cooker increases. Since water now boils at a temperature above 100°C, the food cooks more quickly.
Алимханова
ОтветитьУдалитьChapter 13
Part 3.
1. A crystal is a substance in which the particles are arranged in an orderly, repeating, three-dimensional pattern. Particles of a solid crystal may be ions, atoms, or molecules, depending on the type of substance. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice.
2. The melting point is the temperature at which a solid changes into a liquid. The melting point of a solid is the same as the freezing point of the corresponding liquid. At that temperature, the solid and liquid states of the substance are in equilibrium.
3. Water in the clothes will freeze to ice, then sublimate into water vapor, making the clothes dry.
4. Crystals are classified into general categories based on their shapes.
5. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice. A unit cell is the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire crystal.
6. Unit cells occur in many different varieties. As one example, the cubic crystal system is composed of three different types of unit cells: simple cubic, face-centered cubic, and body-centered cubic.
7. a. cubic, rhombohedral
b. tetragonal, cubic, orthorhombic
c. triclinic
8. a. molecular crystal
b. covalent network crystal
c. ionic crystal
d. metallic crystal
9. a. metallic crystal
b. ionic crystal
c. molecular crystal
d. ionic crystal
e. covalent network crystal
f. molecular crystal
g. metallic crystal
h. covalent network crystal
10. Simple-cubic (least)
Body-centered cubic
Face-centered cubic (most)
1.Brass and bronze are the most famous alloys.
ОтветитьУдалить2.You need to be careful while calculating the mass of a diatomic element.
3.Chemists have to know the structural formula to have a better understanding of chemical properties of the substance.
4.The lone pair of electrons of nitrogen in ammonia changes its structure.
5.A double covalent bond is shorter then a single bond.
6.Nonpolar covalent bonds are usually between the same atoms of a diatomic molecule,for example O2.
7.Molecules of a substance stay closed to each other because of different intermolecular forces.
8.A triple covalent bond is harder to destroy then a single covalent bond.
9.A covalent bond usually connects two non-metals.
10.The double helix of the DNA is held together by hydrogen bonds.
11.The existence of several resonance structures explaines the difference in chemical properties.
12.Ionic compaund contain a cation and an anion.
13.Lewis electron dot structure allows the chemist to decide on the kind of bond between different atoms.
14.A dipole can be formed during electrophoresis.
15.Ionic compounds have the highest bond energy.
16.The metallic bond is the reason for hight conductivity in metals.
17.The coordinate covalent bond is really common for chemical complexes.
18.Polar covalent bond holds together two different non-metals.
19.Chemists can see the molecular geometry of the substance in a special program on the computer.
20.The valence shell was invented to explain the properties of electrons.
Test 13.1
ОтветитьУдалить1. The particles of a gas may be either atoms or molecules. The distance between the particles of a gas is much, much greater than the distances between the particles of a liquid or a solid. Most of the volume of a gas, therefore, is composed of the empty space between the particles. In fact, the volume of the particles themselves is considered to be insignificant compared to the volume of the empty space.
2. a, d
3. Collisions between gas particles and between particles and the container walls are elastic collisions. An elastic collision is one in which there is no overall loss of kinetic energy.
4. One unit of gas pressure is the millimeter of mercury (mmHg). An equivalent unit to the mmHg is called the torr. The pascal (Pa) is the standard unit of pressure. A pascal is a very small amount of pressure, so a more useful unit for everyday gas pressures is the kilopascal (kPa). Another commonly used unit of pressure is the atmosphere (atm).
5. At sea level, a mercury column will rise a distance of 760 mm. Mercury is commonly used in barometers because its high density means the height of the column can be a reasonable size to measure atmospheric pressure. A barometer using water, for instance, would need to be 13.6 times taller than a mercury barometer to obtain the same pressure difference. This is because mercury is 13.6 times more dense than water.
6. At higher altitudes, the atmospheric pressure is lower, so the column of mercury will not rise as high. Drinking through a straw is slightly more difficult atop a mountain. This is because the reduced atmospheric pressure is less effective in pushing water up into the straw.
7. The temperature of a substance in Kelvin is directly proportional to the average kinetic energy of the particles in that substance. As a sample of matter is continually warmed, the average kinetic energy of its particles increases.
8. a. 1307,96 mm Hg b. 74,53 kPa c. 0,9 atm d. 3,05 atm
9. 772 mm Hg
10. 471С
11. 10500 mm.
Test 13.2
ОтветитьУдалить1. The primary difference between liquids and gases is that the particles of a liquid are much closer together, and there is very little empty space between them. Liquids are essentially not compressible and are far denser than gases.
2. The heating process results in a greater fraction of the liquid’s molecules having the necessary kinetic energy to escape the surface of the liquid. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and, thus, has a lower vapor pressure. When the liquid in a closed container is heated, more molecules escape the liquid phase and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure.
3. As acetone evaporates from your skin, it removes heat from its surroundings. I You feel the transfer of heat away from your skin as cold.
4. In a closed container the rate of evaporation is equal to the rate of condensation.
5. Boiling points are affected by external pressure. At higher altitudes, the atmospheric pressure is lower. With less pressure pushing down on the surface of the liquid, it boils at a lower temperature. This can also be seen from the vapor pressure curves.
6. The boiling point is the temperature at which the vapor pressure of a liquid is equal to the external pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the standard atmospheric pressure of 760 mmHg.
7. a. a b. b c. b
8. a. 150 mm Hg b. 52°C c. 88°C d. liquid
9. The boiling point of water is 100°C at sea level, where the atmospheric pressure is close to the standard value. At 3000 m above sea level, the atmospheric pressure is lower, so water boils at about 90°C. On the other hand, water boils at temperatures greater than 100°C if the external pressure is higher than the standard value. Pressure cookers do not allow the water vapor to escape, so the total pressure inside the cooker increases. Since water now boils at a temperature above 100°C, the food cooks more quickly.
Test 13.3
ОтветитьУдалить1. A crystal is a substance in which the particles are arranged in an orderly, repeating, three-dimensional pattern. Particles of a solid crystal may be ions, atoms, or molecules, depending on the type of substance. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice.
2. The melting point is the temperature at which a solid changes into a liquid. The melting point of a solid is the same as the freezing point of the corresponding liquid. At that temperature, the solid and liquid states of the substance are in equilibrium.
3. Water in will freeze to ice, then sublimate into water vapor, making clothes dry.
4. Crystals are classified into general categories based on their shapes.
5. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice. A unit cell is the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire crystal.
6. Unit cells occur in many different varieties. For example, the cubic crystal system is composed of three different types of unit cells: simple cubic, face-centered cubic, and body-centered cubic.
7. a. cubic, rhombohedral b. tetragonal, cubic, orthorhombic c. triclinic
8. a. molecular crystal b. covalent network crystal c. ionic crystal d. metallic crystal
9. a. metallic crystal b. ionic crystal c. molecular crystal d. ionic crystal e. covalent network crystal f. molecular crystal g. metallic crystal
h. covalent network crystal
10. simple-cubic ,body-centered cubic, face-centered cubic
Алимханова
ОтветитьУдалить20 предложений
1. Double and triple covalent bonds are stronger than single covalent bonds.
2. For three electron domains, the arrangement of the electron domains is trigonal planar.
3. The molecular geometry can be determined by various spectroscopic methods and diffraction methods.
4. The electron can break free from its associated atom's valence shell; this is ionization to form a positive ion.
5. The Valence-Shell Electron-Pair Repulsion theory assumes that each atom in a molecule will achieve a geometry that minimizes the repulsion between electrons in the valence shell of that atom.
6. Diatomic elements are all gases, and they form molecules because they don't have full valence shells on their own.
7. In electromagnetism, there are two kinds of dipoles.
8. An important type of dipole-dipole forces are hydrogen bonds.
9. Hydrogen bonds can be intermolecular or intramolecular.
10. Intermolecular forces are much weaker than the intramolecular forces of attraction but are important because they determine the physical properties of molecules.
11. The London dispersion force is the weakest intermolecular force.
12. Nonpolar covalent bonds are very strong bonds requiring a large amount of energy to break the bond.
13. In a polar covalent bond, the electrons are not equally shared because one atom spends more time with the electrons than the other atom.
14. The most important polar molecule on Earth is water.
15. Solids that are held together by van der Waals forces characteristically have lower melting points and are softer than those held together by the stronger ionic, covalent, and metallic bonds.
16. Hybridization helps to explain molecule shape.
17. The three sp2 hybrid orbitals are at angles of 120° to each other, so this hybridisation favours trigonal planar molecular geometry with bond angles of 120°.
18. Pi bonds are usually weaker than sigma bonds.
19. The C-C double bond, composed of one sigma and one pi bond, has a bond energy less than twice that of a C-C single bond, indicating that the stability added by the pi bond is less than the stability of a sigma bond.
20. According to valence bond theory, bonding is caused by the overlap of half-filled atomic orbitals.
FCE listening - 94%
ОтветитьУдалитьListening 90%
ОтветитьУдалитьПАВЛЕНКО ПОЛИНА
ОтветитьУдалитьVOCABULARY:
1. Polar molecules attract water molecules, mainly through hydrogen bonding.
2. Van der Waals interactions are a phenomenon where charge fluctuations in one part of a system correlate with fluctuations in another, resulting in an attractive force.
3. Sigma bonding can be a bonding interaction or an antibonding interaction.
4. The valence bond theory states that atoms in a covalent bond share electron density through the overlapping of their valence atomic orbitals.
5. Sigma and pi bonds are formed by the overlap of atomic orbitals.
6. An electrical dipole consists of two opposite charges attached to a molecule and separated by a certain distance.
7. A diatomic element is a molecule of an element consisting of two atoms.
8. The valence shell electron pair repulsionmodel is useful for predicting and visualizing molecular structures.
9. Double and triple covalent bonds are stronger than single covalent bonds and they are characterized by the sharing of four or six electrons between atoms, respectively.
10. Electron domain geometries are one of the five learned so far: linear, trigonal planar, tetrahedral, trigonal bipyramidal, or octahedral.
11. The valence shell is the outermost occupied shell of electrons in an atom.
12. Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
13. The intermolecular forces are in general much weaker than the intramolecular forces.
14. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
15. Nonpolar covalent bonds are a type of bond that occurs when two atoms share a pair of electrons with each other.
16. Orbital hybridisation is the concept of mixing atomic orbitals into new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in valence bond theory.
17. Sigma bonding is most simply defined for diatomic molecules using the language and tools of symmetry groups.
18. Molecular geometry is the 3-dimensional shape that a molecule occupies in space.
19. Nonpolar covalent bonds are a type of bond that occurs when two atoms share a pair of electrons with each other.
20. A polar molecule is a molecule containing polar bonds where the sum of all the bond's dipole moments is not zero.
ПАВЛЕНКО ПОЛИНА
УдалитьTEST:
13.1
1. The particles of a gas may be either atoms or molecules. The distance between the particles of a gas is much, much greater than the distances between the particles of a liquid or a solid. Most of the volume of a gas, therefore, is composed of the empty space between the particles. In fact, the volume of the particles themselves is considered to be insignificant compared to the volume of the empty space.
2. a d
3. Collisions between gas particles and between particles and the container walls are elastic collisions. An elastic collision is one in which there is no overall loss of kinetic energy.
4. One unit of gas pressure is the millimeter of mercury (mmHg). An equivalent unit to the mmHg is called the torr. The pascal (Pa) is the standard unit of pressure. A pascal is a very small amount of pressure, so a more useful unit for everyday gas pressures is the kilopascal (kPa). Another commonly used unit of pressure is the atmosphere (atm).
5. At sea level, a mercury column will rise a distance of 760 mm. Mercury is commonly used in barometers because its high density means the height of the column can be a reasonable size to measure atmospheric pressure. A barometer using water, for instance, would need to be 13.6 times taller than a mercury barometer to obtain the same pressure difference. This is because mercury is 13.6 times more dense than water.
6. At higher altitudes, the atmospheric pressure is lower, so the column of mercury will not rise as high. Drinking through a straw is slightly more difficult atop a mountain. This is because the reduced atmospheric pressure is less effective in pushing water up into the straw.
7. The temperature of a substance in Kelvin is directly proportional to the average kinetic energy of the particles in that substance. As a sample of matter is continually warmed, the average kinetic energy of its particles increases.
8. a) 1307,96 mm Hg; b) 74,53 kPa; c) 0,9 atm d. 3,05 atm
9. 772
10. 471
11. 10500
ПАВЛЕНКО ПОЛИНА
УдалитьTEST:
13.2
1. The primary difference between liquids and gases is that the particles of a liquid are much closer together, and there is very little empty space between them. Liquids are essentially not compressible and are far denser than gases.
2. The heating process results in a greater fraction of the liquid’s molecules having the necessary kinetic energy to escape the surface of the liquid. A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure. A liquid with stronger intermolecular forces does not evaporate easily and, thus, has a lower vapor pressure. When the liquid in a closed container is heated, more molecules escape the liquid phase and evaporate. The greater number of vapor molecules strike the container walls more frequently, resulting in an increase in pressure.
3. As acetone evaporates from your skin, it removes heat from its surroundings. I You feel the transfer of heat away from your skin as cold.
4. In a closed container the rate of evaporation is equal to the rate of condensation.
5. Boiling points are affected by external pressure. At higher altitudes, the atmospheric pressure is lower. With less pressure pushing down on the surface of the liquid, it boils at a lower temperature. This can also be seen from the vapor pressure curves.
6. The boiling point is the temperature at which the vapor pressure of a liquid is equal to the external pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the standard atmospheric pressure of 760 mmHg.
7. a. a b. b c. b
8. a) 150; b)52; c) 88; d) liquid
9. The boiling point of water is 100°C at sea level, where the atmospheric pressure is close to the standard value. At 3000 m above sea level, the atmospheric pressure is lower, so water boils at about 90°C. On the other hand, water boils at temperatures greater than 100°C if the external pressure is higher than the standard value. Pressure cookers do not allow the water vapor to escape, so the total pressure inside the cooker increases. Since water now boils at a temperature above 100°C, the food cooks more quickly.
13.3
1. A crystal is a substance in which the particles are arranged in an orderly, repeating, three-dimensional pattern. Particles of a solid crystal may be ions, atoms, or molecules, depending on the type of substance. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice.
2. The melting point is the temperature at which a solid changes into a liquid. The melting point of a solid is the same as the freezing point of the corresponding liquid. At that temperature, the solid and liquid states of the substance are in equilibrium.
3. Water in will freeze to ice, then sublimate into water vapor, making clothes dry.
4. Crystals are classified into general categories based on their shapes.
5. The three-dimensional arrangement of a solid crystal is referred to as the crystal lattice. A unit cell is the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire crystal.
6. Unit cells occur in many different varieties. For example, the cubic crystal system is composed of three different types of unit cells: simple cubic, face-centered cubic, and body-centered cubic.
7. a) cubic, rhombohedral; b) tetragonal, cubic, orthorhombic; c) triclinic
8. a) molecular crystal; b) covalent network crystal; c) ionic crystal; d) metallic crystal
9. a) metallic crystal; b) ionic crystal; c) molecular crystal; d) ionic crysta;l e) covalent network crystal; f) molecular crystal; g) metallic crystal
h. covalent network crystal
10. Simple-cubic; body-centered cubic; face-centered cubic.
ПАВЛЕНКО ПОЛИНА
УдалитьFCE TEST 4:
Reading:
1. e
2. i
3. a
4. h
5. c
6. d
7. g
8. d
9. c
10. b
11. a
12. d
13. b
14. a
15. a
16. f
17. c
18. h
19. b
20. d
21. g
22. c
23. d
24. a
25. b
26. c
27. c
28. d
29. a
30. b
31. c
32. d
33. a
34. a
35. b
Use of english:
1. c
2. a
3. c
4. a
5. c
6. b
7. c
8. b
9. a
10. c
11. b
12. c
13. a
14. d
15. a
16. a
17. to
18. feel
19. in
20. for
21. -
22. out
23. were
24. and
25. smaller
26. when
27. same
28. other one
29. will
30. and
31. should hang
32. in spite of
33. isn’t necessary
34. suggested
35. didn’t let
36. hadn’t lost
37. will be meet
38. burst with laugh
39. objects
40. rather stay in bed
41. this
42. correct
43. for
44. correct
45. correct
46. in
47. correct
48. correct
49. the
50. the
51. well
52. correct
53. kind
54. a
55. correct
56. hatred
57. delivered by
58. shoppers
59. choice
60. addition
61. throughout
62. accusation
63. argument
64. products
65. combinations
Алимханова Лилия
ОтветитьУдалитьFCE Test 5
Reading 82%
Use of English 87%
Listening 94%