Topic "The structure of the atom"
1 Electronic formula of the external energy level of a sulfur atom
A) 3s 2 3p 2 IN ) 3s 2 3p 4 C) 3s 1 3p 4 D) 4s 2 4p 4 E) 4s 2 4p 4 F) 3s 3 3p 4 G) 4s 2 4p 2 H) 3s 2 3p 6
2. The ordinal number of an element in the Periodic Table indicates
A) h atomic nucleus
C) the number of electronic layers in the atom
D) the value of the electronegativity of the element
F) the value of the atomic mass of the element
G) number of neutrons in an atom
3. A series of numbers 2,8,5 corresponds to the distribution of electrons over the energy levels of the atom
A) aluminum B) phosphorus C) nitrogen D) chlorine E) sulfur F) argon G) silicon H) magnesium
4. The electronic formula of the atom is 1s 2 2s 2 2p 6 3s 2 3p 2. Chemical sign and formula of the hydrogen compound of this element
A) C and CH 4 IN) Si and SiH 4 C) O and H 2 O D) Cl and HCl
E) S and H 2 S F) P and PH 3 G) N and NH 3 H) F and HF
5. A pair of elements with a similar structure of the external and pre-external energy levels:
A) B and Si B) S and Se C) K and Ca D ) Na and K E) Mn and Fe F) G) H)
6. Is
s-element
A) barium
B) manganese C) sulfur D) carbon E) zinc F) silicon G) oxygen H) nitrogen
7. An element with the electronic formula 1s 2 2s 2 2p 6 3s 2 3p 3 forms a higher oxide corresponding to the formula
A) E 2 O B) E 2 O 3 C) EO 2 D) EO E) E 2 ABOUT 5 F) EO 3 G) E 2 O 7 H) EO 4
8. Neon atom Ne, sodium cation Na + and fluorine anion F - have the same
A) number of protons B ) the number of electrons C) value of maximum valence D) number of neutrons E) energy sublevels F) value of maximum oxidation state
G) atomic mass value H) electronegativity value
9. The number of protons, neutrons and electrons in the 40 Ar atom, respectively, is
A ) 18, 22, 18 B) 40, 18, 40 C) 22, 18, 40 D) 18, 40, 18 E) 22, 40, 22 F) 18, 22, 40 G) 40, 22, 18 H) 22,18,18
10. The distribution of electrons in the atom of the fourth period element of the IA group corresponds to a number of numbers
A) 2.8.8.2 B) 2,8,8,1 C) 2.8.18.2 D) 2.8.18.1 E) 2.8.18.3 F) 2.8.18.3 G) 2.8.18.1 H) 2.8 , 18.2
11. The fourth electron layer contains five electrons atom
A) V B) P C ) As D) Sn E) Zr F) Cu G) Sb H) N
12. The same number of electrons and neutrons in
A) Be atom B) S 2 - C ion) F - D ion) Cr E ) atom S F) Ar G) Li H) Na
13 The oxygen atom and the sulfur atom are similar in
A) the number of electrons on the outer layer B) the value of the maximum oxidation state C) the number of energy levels D) the number of neutrons in the nucleus E) the number of electrons in the atom F) the charge of the nucleus
G) atomic mass value H) electronegativity value
14. In the nucleus of an atom of an element with the electronic formula 1s 2 2s 2 2p 6 3s 2 3p 2, the number of protons is
A) 18 B) 10 C ) 14 D) 12 E) 16 F) 24 G) 15 H) 2
15. A metal atom, the highest oxide of which is Me 2 O 3, has the electronic formula of the external energy level
A) ns 2 nр 1 B) ns 2 nр 2 C
) ns
2
np
3
D) ns 2 np E) ns 2 np F) ns 1 np 2 G) ns 0 np 1 H) ns 1 np 2
16. Below is a heavy model of the atom of a chemical element. Specify this item.
A) Mg B) Na C) Al D) Ar E) Cl F) P G) Si H) S
17.
For a sulfur atom, the number of electrons at the external energy level and the charge of the nucleus are equal, respectively
A) 4 and + 16 B) 6 and + 32 C) 4 and + 32 D
) 6 and + 16
E) 4 and 16 F) 16 and +4 G) 3 and +32 H) 3 and +6
18. Particles have the same electronic structure
A) Na 0 and Na + B) Na
+
and F
- C) Na 0 and K 0 D) Cr 2+ and Cr 3+
E) Na 0 and F - F) Na 0 and K + G) K 0 and Cl 0 H) K 0 and Cl -
19. Is
p-element is
A) sodium B
) phosphorus
C) uranium D) calcium E) potassium F) lithium G) rubidium H) cesium
20. The formula of the higher oxide of the element, the electronic formula of which is 1s 2 2s 2 2p 6 3s 2 3p 3
A) B 2 O 3 B) N 2 O 5 C) P 2 O 5 D) Al 2 O 3 E) As 2 O 5 F) SO 3 G) P 2 O 3 H) SiO 3
21. In the fifth electron layer contains four electrons atom
A) V B) Sb C) As D) Sn E) Zr F) Si G) Pb H) Sr
Part B. Wadania with a choice of several correct answers.
Sulfur anion composition
A) protons 32 B) electrons 18 C) neutrons 16 D) electrons 16 E) electrons 32
F ) protons 16 G) electrons 14 H) protons 18
2. Refers to s-elements
A) Zn IN) Na FROM) Mg D) S E) Li F) C G) Zn H) Cu
3. At the external energy level, five electrons have
A) N B) Cl C) Si D) C E) H F) Na G) P H) As
4. Carbon and silicon atoms differ from each other
A) refer to p-elements
C) are non-metals
D) the number of vacant orbitals at the external energy level
E) nuclear charge
G) the value of the maximum valence
5. The ordinal number of an element in the Periodic Table indicates
A) h atomic nucleus
B) the number of electrons in the outer layer of the atom
FROM) number of electrons in the atom
D) the number of neutrons in the atom
E) the number of energy sublevels on the electron layer
F ) the number of protons
G) the maximum valence of the element in compounds with oxygen
H) the number of electronic layers in the atom
6. At the last energy level there are 8 electrons in
AND) a argon volume Ar B) calcium atom C) potassium atom K D ) chlorine anion FROM l -
E) potassium atom K F ) calcium cation Ca 2+
7. The electronic formula 1s 2 2s 2 2p 6 corresponds to
A) a to neon B ) oxygen anion C) oxygen atom D ) fluorine anion
E) fluorine atom F) oxygen atom G) sodium atom H) chlorine anion
8. The atom of a given metal has the electronic formula of the external energy level ns 2 np 1
A
)
IN
B) O C) P D) As E
) AND
l
F) C G)
Ga
H) Si
9. In reactions, an element gives up one electron
AND) Li B) Zn C) Cl D ) Rb E) Na F) Al G) Ca H) F
10. The two-electron outer shell has an ion
A) S 6+ B) S 2- FROM)
Br
5+
D
)
S
4+
E) C
2+
F) Sn 4+ G) C 4+ H) Br -
11. Is a p-element
AND) S B) Na C) Ca D ) P E) O F) K G) Zn H) Li
12. In reactions, an element takes one electron
A) Li B) Zn FROM) Cl D) Rb E) B r F) K G) Ca H) F
13. An atom of an element, the maximum oxidation state of which is + 4, in the ground state can have an electronic configuration of the external energy level:
AND) 3 s 2 3 p 4 IN ) 2 s 2 2 p 2 FROM) 2 s 2 2 p 4 D) 3 s 2 3 p 2 E) 2s 2 2p 6 F) 3s 2 3p 4 G) 4 s 2 4 p 2 H) 2s 2 2p 5
14. Particles in a pair have the same electronic structure
AND) F - and Na +
E) F - and Na F) Mg and Si 4+ G) H) Mg and Si 2+ H ) K and Cl -
15. The s-sublevel contains 2 electrons (ground state) for
A) Ca B) S C) Na D ) Mg E) Li F) K G) Rb H) H
16. Composition of the fluorine anion
A) protons 19
B) electrons 10
C) neutrons 10
D) electrons 16
E) electrons 19
F ) protons 9
G) neutrons 19
H) protons 18
17. Refers to d-elements
AND) Ag IN) Zn C) K D ) Cu E) Na F) C G) S H) Cl
18. At the external energy level, 4 electrons have
A) N B) Cl C) Si D) C E) H F) Na G) P H) Sn
19. Nitrogen and phosphorus atoms differ from each other
A) maximum valence value
B) the number of valence electrons
C) are non-metals
D) the number of vacant orbitals at the external energy level
E) nuclear charge
F) the number of electrons at the last energy level
G) refer to p-elements
H) the number of energy levels
20. The ordinal number of an element in the Periodic Table indicates:
A) the number of neutrons in an atom
IN) s atomic nucleus
FROM) number of electrons in the atom
D ) number of protons
E) the number of energy sublevels on the electron layer
F) the number of electrons in the outer layer of the atom
G) the number of electronic layers in an atom
H) the maximum valence of the element in compounds with oxygen
21. Has 18 electrons
AND) calcium atom B) fluorine atom F C) potassium atom K D ) chlorine anion FROM l -
E) potassium cation K + F ) calcium cation Ca 2+ G) chlorine atom H) fluorine anion F -
22. The electronic formula 1s 2 2s 2 2p 6 3 s 2 3p 6 corresponds to
A) a argon volume B) oxygen anion C) oxygen atom D ) calcium cation
E) fluorine atom F ) potassium cation G) sodium atom H) chlorine atom
23. The atom of this metal has the electronic formula of the external energy level ns 2 np 3
A) B B) O C
)
P
D
)
As
E) Al F)
N
G) Ga H) Si
24. These elements, when interacting, give two electrons
A) Li IN) Zn C) Cl D) Rb E) Mg F) K G) Ca H) F
25. The two-electron outer shell has an ion
A) S 6+ IN)Br
5+
C) S 2- D
)
S
4+
E) C 4+ F) Sn 4+ G)
FROM
2+
H) Br -
26. These chemical elements belong to s - elements
A) S B) P FROM) Ca D) Al E) O F) K G) C H) Li
27. These elements, when interacting, take one electron
A) Li B) Zn FROM) Cl D) Rb E) B r F) K G) Ca H) F
28. An atom of an element, the maximum oxidation state of which is + 4, in the ground state can have an electronic configuration of an external energy level:
AND) 3 s 2 3 p 4 IN ) 2 s 2 2 p 2 FROM) 2 s 2 2 p 4 D) 3 s 2 3 p 2 E) 2s 2 2p 6 F) 3s 2 3p 4 G) 4 s 2 4 p 2 H) 2s 2 2p 5
29. Particles in a pair have the same electronic structure
AND) F - and Na + B) F and Na + C) Mg and Ca D) Mg 2+ and Si 2+
E) F - and Na F) Mg and Si 4+ G) Mg and Si 2+ H ) K and Cl -
30. There is 1 electron on the s-sublevel (ground state)
A) Ca B) S FROM) Na D) Mg E) L i F) Ba G) Rb H) H
Part C. Test tasksfor correlation.
Establish a correspondence between an atom of an element and the number of electrons that it gives or receives to complete the outer electron shell:
Establish a correspondence between the ion and its electronic formula:
| Electronic formula |
|
| A) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4 p 6 5s 1 B) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 C) 1s 2 2s 2 2p 6 3s 2 3p 6 D) 1s 2 2s 2 2p 6 E) 1s 2 2s 2 2p 4 F) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4 p 6 |
Match the element and its electronic formula
Establish a correspondence between the energy sublevel and the number of orbitals on it:
Establish a correspondence between an ion and its electronic formula
8. Establish a correspondence between the atom of an element and the number of electrons that it gives
or takes to terminate the outer shell:
| Part A. Test items with a choice of one answer |
|
| Part B. Tasks with the choice of several correct answers. |
|
| Part C. Test tasksfor correlation. |
|
| 1-B 2-E, 3-C |
|
The chemistry test on the topic "The structure of the atom" is designed to assess the knowledge of students in the course "Chemistry". In the test, correct answers are marked with "+"
1. Atoms of isotopes have a different number:
-: protons
+: neutrons
-: electrons
-: there is no correct answer.
2. The energy level is characterized by a quantum number:
+: main;
-: orbital;
-: magnetic;
-: spin.
3. The energy of the sublevel is characterized by a quantum number:
-: main;
+: orbital;
-: magnetic;
-: spin
4. The proper rotational motion of the electron characterizes the quantum number:
-: the main thing;
-: orbital;
-: magnetic;
+: spin
5. What position indicates that the distribution of electrons in an unexcited atom occurs so that their total energy is minimal:
+: principle of minimum energy;
-: Pauli's principle;
-: Gund's rule
-: there is no correct answer
6. What position states that an atom cannot have two electrons with the same set of values \u200b\u200bfor all four quantum numbers:
-: the principle of minimum energy;
+: Pauli's principle;
-: Gund's rule
-: there is no correct answer
7. What position proves that in unexcited atoms the electrons within a given sublevel occupy the maximum number of free orbitals, while the total spin number is maximum:
-: the principle of minimum energy;
-: Pauli's principle;
+: Gund's rule
-: there is no correct answer
8. In the periodic table, elements with the same structure of the outer electron layer are combined into
-: periods;
+: groups;
-: subgroups
-: there is no correct answer
9. A sequential series of elements whose atoms have the same number of energy levels is:
+: period;
-: Group;
-: subgroup
-: there is no correct answer
10. In groups, atomic radii:
+: increase from top to bottom;
-: increase from bottom to top;
-: differ slightly
-: there is no correct answer
11. The energy of detachment of an electron from an atom of an element with the formation of a cation is:
+: ionization energy;
-: there is no correct answer
12. The energy of attachment of an electron by an atom of an element with the formation of an anion is:
-: ionization energy;
+: energy of electron affinity;
-: relative electronegativity
-: there is no correct answer
13. The quantity characterizing the ability of an atom of an element to attract common electrons in a molecule is:
-: ionization energy;
-: energy of electron affinity;
+: relative electronegativity
-: there is no correct answer
14. In the period from left to right:
-: increased metallic properties;
+: the ionization energy increases;
-: the ionization energy decreases;
-: no correct answer
15.With an increase in the serial number from sodium to chlorine, the elements
-: metallic properties are enhanced;
-: non-metallic properties are reduced;
-: valence in oxygen compounds
decreases;
+: metallic properties are reduced and non-metallic properties are increased
16. In a group from top to bottom
-: enhanced metallic properties;
+: restorative properties are enhanced;
-: the atomic radius decreases;
-: no correct answer
17. Electron affinity in the period from left to right
-: decreases;
+: increases;
-: does not change
-: there is no correct answer
18. In the period from left to right, relative electronegativity
-: decreases;
+: increases;
-: does not change
-: there is no correct answer
19. Electrons in a spherical orbital are
-: d-electrons;
+: s-electrons;
-: f-electrons;
-: p-electrons.
20. Shape of the p-electron orbital
-: spherical;
+: dumbbell;
-: asymmetrical dumbbell;
-: four-leaf flower.
21. The fourth energy level contains maximum
-: 8 electrons;
-: 16 electrons;
-: 32 electrons;
+: 36 electrons.
22. With an increase in the serial number of elements from lithium to neon, the number of electrons in the second energy level
-: ranges from 9 to 18;
-: varies with an even number;
-: remains unchanged;
+: ranges from 1 to 8.
23. The number of lone electron pairs at the valence energy level of the nitrogen atom in the ground state is
24. The ion Sc3 + corresponds to the electronic configuration
-: 1s22s22p63s23p64s23d3
-: 1s22s22p63s23p64s24p3
+: 1s22s22p63s23p6
-: 1s22s22p63s23p64s23d0
25. In the period with an increase in the serial number of elements, metallic properties:
-: vary ambiguously
-: intensified
+: weaken
-: do not change
26. On d-orbitals of the same energy level, there can be a maximum of ____ electrons
27. The greatest mass is ...
-: electron
-: positron
+: neutron
28. The total energy storage of an electron in an atom characterizes the quantum number ...
29. The maximum number of unpaired electrons in p-orbitals is ...
30. At the nodes of the crystal lattice of sodium fluoride are ...
-: NaF molecules
-: sodium atoms and fluorine molecules
+: sodium and fluorine ions
-: sodium and fluorine atoms
31. Methane molecule has ……. structure
-: pyramidal
-: angular
+: tetrahedral
-: linear
32. In a series, the bond strength in molecules ...
-: does not change
-: changes periodically
+: decreases
-: increases
33. Chemical bond, carried out due to one or more electron pairs, strongly interacting with the nuclei of both connected atoms, this
+: covalent bond;
-: ionic bond;
-: metal bond
-: there is no correct answer
34. A chemical bond, which is characterized by a strong interaction of a common electron pair with the nucleus of only one of the connected atoms, is
-: covalent bond;
+: ionic bond;
-: metal bond
-: there is no correct answer
35. A chemical bond, characterized by a weak interaction of common electrons with the nuclei of the connected atoms and the complete delocalization of these electrons between all atoms, is
-: covalent bond;
-: ionic bond;
+: metal bond
-: there is no correct answer
36. Substances with ionic bonds
+: they dissolve well in water, their solutions and melts conduct electric current well;
-: poor electrical conduction,
have a low boiling point;
-: poorly conduct electric current, poorly soluble in water;
-: their solutions and melts conduct electric current well, dissolve poorly in water
37. Ionic bond is characterized by
-: focus;
+: by electrostatic interaction
positive and negative ions;
-: saturation;
-: by overlapping electron clouds
38. The molecules of ionic compounds contain elements
+: with low ionization energy and high electron affinity;
-: with high ionization energy and low electron affinity;
-: with low ionization energy;
-: low electronegativity
39. Substances with a non-polar covalent bond are inherent
-: focus;
+: saturation;
-: insolubility in water;
-: all answers are correct
40. A covalent bond is formed
+: overlapping atomic orbitals;
-: electrostatic interaction of positive and negative ions;
-: in metal molecules;
-: in atoms with low ionization energy
41. In the molecule of which compound a covalent bond is possible by the donor-acceptor mechanism
42. The dissimilarity of all or some of the physical and chemical properties of a substance in different directions is
+: anisotropy;
-: polymorphism;
-: isomorphism
-: there is no correct answer
43. Mp + 7 goes into Mp + 2 in
+: acidic environment;
-: alkaline environment;
-: neutral environment
-: there is no correct answer
44.Mp + 7 goes into Mp + 4 in
-: acidic environment;
-: alkaline environment;
+: neutral environment
-: there is no correct answer
45. Mp + 7 goes into Mp + 6 in
-: acidic environment;
+: alkaline environment;
-: neutral environment
-: there is no correct answer
46. \u200b\u200bThe NF3 molecule has _______ spatial configuration.
-: triangular
-: angular
+: pyramidal
-: linear
47. A molecule of carbon monoxide (IV) contains _______ bonds.
48. The PCl3 molecule, in which the phosphorus atom is in the sp3 hybrid state, has a _______ shape.
+: pyramidal
-: linear
-: angular
-: flat
49. A particle that can be a donor of an electron pair is ...
50. Unpaired electrons are contained in molecular orbitals in a molecule ...
Test work in chemistry, grade 11 (O. Gabrielyan's educational code, basic level)
on the topics "The structure of the atom", "The structure of matter".
Checked content items.
Part A contains 16 tasks with a short answer (basic difficulty level).
A1 - Models of the structure of atoms. DI Mendeleev's periodic law, its formulations.
A2 - The physical meaning of the structural elements of the Periodic Table in the light of the doctrine of the structure of the atom.
A3 - The structure of energy levels and sublevels
A4 - Classification of chemical elements (s, p, d, f)
A5 - Electronic configurations of atoms
A6 - Classification of chemical compounds (oxides and hydroxides)
A7 - Changes in the properties of chemical elements in the period and group
A8 - The relationship between the structure of the atom and the formula of chemical compounds formed by it.
A9 - Isotopes, the composition of their atoms
A10 - Types of chemical bonds
A11 - Types of chemical bonds
A12 - Chemical bond characteristics
A13 - Chemical bond characteristics
A14 - Types of crystal lattices
A15 - Classification of dispersed systems
A16 - Colloidal systems
Part B contains 3 tasks with a detailed answer (increased difficulty level).
B17 - The relationship between the structure of the atom and the composition and properties of the chemical compounds formed by it.
B18 - The relationship between the composition of a chemical compound and the types of bonds and crystal lattice in it.
B19 - Calculation of the mass fraction of a solute in a solution
Option 1
Part A (the answer to tasks 1-16 is one digit)
1) The model of the atom "pudding with raisins" was proposed
AND). N. Borom B). E. Rutherford B). J. Thomson G). D. Chadwig.
2) The ordinal number of an element in the periodic system determines:
AND). Nuclear charge of an atom.
D). The number of neutrons in an atom.
AND). B and Si. B). S and Se. IN). K and Ca. D). Mn and Fe.
4) the s-element is:
AND). Barium. B). Americium. IN). Gallium. D). Vanadium.
5) Electronic configuration ... 3d64s2 corresponds to element:
A). Argon. B). Iron. IN). Krypton. D). Ruthenia
AND). Be (OH) 2. B). H2SiO3. IN). Mg (OH) 2. D). Ba (OH) 2.
AND). Sr-Rb-K. B). Na-K-Ca. IN). Na-K-Cs. D). Al-Mg-Be.
8) Element E with the electronic formula 1s22s22p63s23p3 forms a higher oxide corresponding to the formula:
AND). E2O. B). E2O3. IN). EO2. D). E2O5.
9) An isotope of iron, the nucleus of which contains 28 neutrons, means:
ten). Formula of a substance with a covalent polar bond:
A) Cl2. B). KCl. IN). NH3. D). O2.
11) A substance, between the molecules of which there is a hydrogen bond, is:
AND). Ethanol. B). Methane. IN). Hydrogen. D). Benzene.
12). The number of common electron pairs in a hydrogen molecule:
13) The polarity of the chemical bond increases in a number of compounds, the formulas of which are:
AND). NH3, HI, O2. B). CH4, H2O, HF. IN). PH3, H2S, H2. D). HCl, CH4, Cl2.
14) The crystal lattice of magnesium chloride:
15) Milk is:
16) A spontaneous decrease in the volume of the gel, accompanied by the separation of liquid, is called
Part B
17). Write an electronic formula for the element with atomic number 32 in the Periodic Table. Make a conclusion about the belonging of this element to metals or non-metals. Write down the formulas of its higher oxide and hydroxide, indicate their nature.
18) Draw up schemes for the formation of compounds (electronic and structural formulas), consisting of chemical elements A). Silicon and chlorine. B). Sodium and nitrogen. Indicate the type of chemical bond and the type of crystal lattice in each compound.
19) In 280 g of a 15% zinc chloride solution, 12 g of the same salt was dissolved. What is the mass of zinc chloride in the resulting solution?
Option 2
Part A
1) The planetary model of the atom was proposed
AND). D. Mendeleev. IN). J. Thomson.
B). E. Rutherford. D). D. Chadwig.
2) The period number in the Periodic Table determines:
AND). Nuclear charge of an atom.
B). The number of electrons in the outermost layer of an atom.
IN). The number of electron layers in an atom.
D). The number of electrons in an atom.
3) A pair of elements with a similar structure of external and pre-external energy levels:
AND). S and Cl. B). Be and B. B). Kr and Xe. D). Mo and Se.
4) the p-element is:
AND). Scandium. B). Barium. IN). Arsenic. D). Helium.
5) Electronic configuration ... 3d104s2 corresponds to element:
A). Calcium. B). Krypton. IN). Cadmium. D). Zinc.
6) Amphoteric hydroxide is a substance whose formula is:
AND). Zn (OH) 2. B). Mg (OH) 2. IN). Ca (OH) 2. D). Cr (OH) 2.
7) A number of elements arranged in order to enhance metallic properties:
AND). Mg-Ca-Zn. B). Al-Mg-Ca. IN). Sr-Rb-K. D). Ge-Si-Sb.
8) Element E with the electronic formula 1s22s22p63s23p63d104s24p1 forms a higher oxide corresponding to the formula:
9) Calcium isotope, the nucleus of which contains 22 neutrons, means:
AND). HCl. B). KBr. IN). P4. D). CH3OH.
AND). Potassium oxide. B). Copper. IN). Silicon. D). Magnesium hydroxide.
12). The number of common electron pairs in a nitrogen molecule:
AND). One. B). Two. IN). Three. D). Four
AND). Cl2, H2S, CO2. B). NH3, PH3, SO2. IN). HCl, HBr, HI. D). BH3, NH3, HF.
14) .Crystal lattice of silicon oxide (IV):
AND). Atomic. B). Metallic. IN). Ionic. D). Molecular.
fifteen). Enamel paint is:
AND). Suspension. B). Emulsion. IN). Sol. D). Gel.
sixteen). The adhesion of colloidal particles is
AND). Coagulation. B). Sedimentation. IN). Syneresis. D). Tyndall effect.
Part B(for tasks 17-19, a detailed solution is required)
17). Write an electronic formula for the element with serial number 30 in the Periodic Table. Make a conclusion about the belonging of this element to metals or non-metals. Write down the formulas of its higher oxide and hydroxide, indicate their nature.
18). Make a diagram of the formation of compounds (electronic and structural formulas), consisting of chemical elements A). Nitrogen and Hydrogen. B). Sodium and Chlorine. Indicate the type of chemical bond and the type of crystal lattice in each compound.
19) Mixed 80 g of sodium nitrate solution with a mass fraction of 5% and 200 g of an 8% solution of the same salt. What is the percentage of salt in the resulting solution?
Option 3
Part A(The answer to tasks 1-16 is one letter)
1) The quantum model of the atom was proposed
A) N. Bohr. B) D. Mendeleev. C) H. Moseley. D) D. Chadwig.
2) The group number (for elements of the main subgroups) in the Periodic Table determines:
AND). The number of protons in an atom.
B). The number of electrons in the outermost layer of an atom.
IN). The number of electron layers in an atom.
D). The number of neutrons in an atom.
3) A pair of elements with a similar structure of external and pre-external energy levels:
AND). Ba and K. B). Sb and Bi. IN). Ti and Ge. D). Kr and Fe.
4) The d-element is:
AND). Potassium. B). Silicon. IN). Argon. D). Copper.
5) Electronic configuration ... 3d54s2 corresponds to element:
A). Bromine. B). Calcium. IN). Manganese. D). Chlorine.
6) Amphoteric oxide is a substance whose formula is:
AND). CO. B). Cr2O3. IN). CrO3. D). FeO.
7) A number of elements arranged in order to enhance metallic properties:
AND). Al-Ga-Ge. B). Ca-Sr-Ba. IN). K-Na-Li. D). Mg-Ca-Zn.
8) Element E with the electronic formula 1s22s22p63s23p1 forms a higher oxide corresponding to the formula:
AND). EO. B). E2O3. IN). E2O5. D). EO3.
9) An isotope of iron, the nucleus of which contains 30 neutrons, means:
AND). 54 / 26Fe. B). 56 / 26Fe. IN). 57 / 26Fe. D). 58 / 26Fe.
10) Formula of a substance with a covalent non-polar bond:
AND). MgCl2. B). HF. IN). N2. D) .Al.
eleven). A substance between the molecules of which there is a hydrogen bond is:
AND). Oxygen. B). Ethane. B). Sodium fluoride. D). Ethanal.
12). The number of common electron pairs in a fluorine molecule:
AND). One. B). Two. IN). Three. D). Four
13). The polarity of the chemical bond decreases in a number of compounds, the formulas of which are:
AND). HI, HCl, HF. B). HBr, O2, H2S. B). NH3, H2S, CH4. D). H2O, PH3, HI.
fourteen). Crystal lattice of sucrose:
AND). Atomic. B). Metallic. IN). Ionic. D). Molecular.
fifteen). Blood plasma is:
AND). Suspension. B). Emulsion. IN). Sol. D). Gel.
16). The sedimentation of large colloidal particles under the action of gravity is called
AND). Coagulation. B). Sedimentation. IN). Syneresis. D). Tyndall effect.
Part B(for tasks 17-19, a detailed solution is required)
17). Write an electronic formula for the element with serial number 38 in the Periodic Table. Make a conclusion about the belonging of this element to metals or non-metals. Write down the formulas of its higher oxide and hydroxide, indicate their nature.
18). Make schemes for the formation of compounds (electronic and structural formulas), consisting of chemical elements A). Magnesium and Fluorine. B). Carbon and Oxygen. Specify the type of chemical bond and the type of crystal lattice in each compound.
19) (4 points) Mixed 120 g of a 2.5% sodium sulfate solution and 10 g of a 5% solution of the same salt. What is the mass of sodium sulfate in the resulting solution?
Option 4
Part A(The answer to tasks 1-16 is one letter)
1) "The charge of the nucleus of the atom of each element in the periodic table increases by one in comparison with the charge of the nucleus of the atom of the previous element" - this is the formulation of the law
A) G. Pauli. B). E. Rutherford. C) D. Mendeleev D) G. Moseley
2) The total number of neutrons in the nucleus of an atom of an element is
AND). Nuclear charge.
B). Atomic mass.
C) Differences between atomic mass and serial number.
D). Ordinal number
3) A pair of elements with a similar structure of external and pre-external energy levels:
A) .Na and Li. B). Cl and Br. IN). Zn and Ca. D). Mn and Fe.
4) The d-element is:
AND). Germanium. B). Cadmium. IN). Selenium. D). Uranus.
5) Electronic configuration ... 4s24p6 corresponds to element:
A). Bromine. B). Iron. IN). Neon. D). Krypton.
6) Amphoteric hydroxide is a substance whose formula is:
AND). Ge (OH) 4 B). Mg (OH) 2. IN). LiOH. D). Si (OH) 4.
7) A number of elements arranged in order to enhance metallic properties:
AND). K-Rb-Sr. B). Al-Mg-Be. IN). Be-Li-Cs. D) .Ge-Sn-Sb.
8) Element E with the electronic formula 1s22s22p63s23p63d104s24p4 forms a higher oxide corresponding to the formula:
AND). E2O. B). E2O3. IN). EO2. D). EO3.
9) The isotope of calcium, the nucleus of which contains 24 neutrons, means:
AND). 40 / 20Ca. B). 42 / 20Ca. IN). 44 / 20Ca. D). 48 / 20Ca.
10) Formula of substance with a metal bond:
AND). O2. B). H2O. IN). Ca. D) .NH3.
eleven). Substance with only a covalent polar bond:
AND). Hydrogen fluoride. B). Chlorine. B). Sodium peroxide. D). Sodium fluoride.
12). The number of common electron pairs in a hydrogen bromide molecule:
AND). One. B). Two. IN). Three. D). Four
13). (2 points). The polarity of the chemical bond decreases in a number of compounds, the formulas of which are:
AND). PH3, HCl, HF. B). HF, H2O, NH3. IN). CH4, PH3, H2O. D). H2O, HI, NH3.
fourteen). Crystal lattice of white phosphorus:
AND). Atomic. B). Metallic. IN). Ionic. D). Molecular.
fifteen). Cartilage, tendons are:
AND). Suspension. B). Emulsion. IN). Sol. D). Gel.
16) True solutions include homogeneous systems with a particle size of the phase
AND). More than 100nm. B). Less than 1 nm. IN). 1 to 100 nm D). Size doesn't matter.
Part B(for tasks 17-19, a detailed solution is required)
17). Make the electronic formula of the element with serial number 34 in the Periodic Table. Make a conclusion about the belonging of this element to metals or non-metals. Write down the formulas of its higher oxide and hydroxide, indicate their nature.
18). Make a diagram of the formation of compounds (electronic and structural formulas), consisting of chemical elements A). Sulfur and Hydrogen. B). Sodium and Oxygen. Indicate the type of chemical bond and the type of crystal lattice in each compound.
19) 8% sodium acetate solution weighing 200 g was diluted with 120 ml of water. What is the percentage of salt in the resulting solution?
Option 5
Part A(The answer to tasks 1-16 is one letter)
1) "The properties of chemical elements and the compounds formed by them are periodically dependent on their relative atomic masses" - this is the formulation of the law
A) G. Pauli. B.) E. Rutherford. IN). D. Mendeleeva D) G. Moseley
2) The total number of electrons in an atom of an element is determined using the Periodic System, by the number:
AND). Groups. B). Period. IN). Row. D). Ordinal number.
3) A pair of elements with a similar structure of external and pre-external energy levels:
AND). Sn and Pb. B). As and Se. IN). Zn and Ca. D). Mo and Te.
4) The f-element is:
AND). Germanium. B). Calcium. IN). Samarium. D). Lanthanum
5) Electronic configuration ... 5s25p4 corresponds to element:
A). Zirconium. B). Molybdenum. IN). Tellurium. D). Tin.
6) Amphoteric hydroxide is a substance whose formula is:
AND). Fe (OH) 3. B). Mg (OH) 2. IN). LiOH. D). RbOH.
7) A number of elements arranged in order to enhance metallic properties:
AND). K-Cs-Ba. B). Al-Mg-Be. IN). Be-Li-Al. D) .Ge-Sn-Pb.
8) Element E with the electronic formula 1s22s22p63s23p63d104s24p2 forms a higher oxide corresponding to the formula:
AND). E2O. B). E2O3. IN). EO2. D). EO3.
9) An isotope of titanium, the nucleus of which contains 22 neutrons, means:
AND). 40 / 22Ti. B). 42 / 22Ti. IN). 44 / 22Ti. D). 48 / 22Ti.
10) Formula of substance with ionic bond:
AND). NaCl. B). HBr. IN). P4. D). CH2O.
11) .Metal-bonded substance:
AND). Calcium oxide. B). Mercury. B) Ammonia. D). Aluminum hydroxide.
12) The number of total electron pairs in a water molecule:
AND). One. B). Two. IN). Three. D). Four
13). The polarity of the chemical bond decreases in a number of compounds, the formulas of which are:
AND). Cl2, H2S, SO2. B). AsH3, NH3, PH3,. IN). HF, HCl, HBr ,. D). BH3, NH3, BF3.
fourteen). Cast iron crystal lattice:
AND). Atomic. B). Metallic. IN). Ionic. D). Molecular.
fifteen). Smoke is:
AND). Suspension. B). Emulsion. IN). Sol. D). Spray can.
16). The formation of a luminous cone when a beam of light passes through a colloidal solution is called
AND). Coagulation. B). Sedimentation. IN). Syneresis. D). Tyndall effect.
Part B(for tasks 17-19, a detailed solution is required)
17) .Compose the electronic formula of the element with serial number 37 in the Periodic Table. Make a conclusion about the belonging of this element to metals or non-metals. Write down the formulas of its higher oxide and hydroxide, indicate their nature.
18). Make a diagram of the formation of compounds (electronic and structural formulas), consisting of chemical elements A). Carbon and Chlorine. B). Barium and Oxygen. Indicate the type of chemical bond and the type of crystal lattice in each compound.
19) 200 g of 10% sulfuric acid solution was heated. This evaporated 20 ml of water. What is the percentage of acid concentration in the resulting solution?
Assessment of work.
For the correct answer in part A - 1 point
For the complete correct answer in part B:
B17 - 6 points, B18 - 8 points, B19 - 3 points. Total maximum 33 points.
Evaluation criteria B17:
The electronic formula of the element has been compiled - 1 point;
It was concluded that it belongs to metals or non-metals - 1 point;
Molecular formulas of oxide and hydroxide are written down - 1 point for each;
The nature of the oxide and hydroxide is indicated - 1 point for each; (total 6 points)
Evaluation criteria B18:
An electronic formula of the compound was compiled - 1 point for A and B;
The structural formula of the compound was compiled - 1 point each for A and B;
The types of connection in the connection are indicated - 1 point each for A and B;
The type of crystal lattice is indicated - 1 point for A and B; (total 8 points)
Evaluation criteria B18:
The mass of dissolved substances in the initial solutions was determined - 1 point;
The mass of the resulting solution was determined - 1 point;
The mass / mass fraction of the solute in the resulting solution is determined - 1 point; (3 points in total). * If a computational error is made at any stage of the calculations, but the course of the solution is correct, then 1 point is deducted.
Scale for converting primary points into a mark
Key to verification
| Job No. | Option 1 | Option 2 | Option 3 | Option 4 | Option 5 |
| IN | B | AND | D | IN | |
| AND | IN | B | IN | D | |
| B | IN | B | B | AND | |
| AND | IN | D | B | IN | |
| B | D | IN | D | IN | |
| AND | AND | B | AND | AND | |
| IN | B | B | IN | D | |
| D | B | B | D | IN | |
| AND | B | B | IN | IN | |
| IN | B | IN | IN | AND | |
| AND | B | D | AND | B | |
| AND | IN | AND | AND | B | |
| B | IN | IN | B | IN | |
| IN | AND | D | D | B | |
| B | AND | IN | D | D | |
| IN | AND | B | B | D | |
| ... 3d104s24p2 metal, GeO2, Ge (OH) 4 - amphoteric | ... 3d104s2 metal, ZnO, Zn (OH) 2 - amphoteric | ... 4d105s2 metal, SrO, Sr (OH) 2 - basic | ... 3d104s24p4 non-metal, SeO3, H2SeO4 - acidic | ... 4d105s1 metal, Rb2O, RbOH - basic |
|
| A (SiCl4) -covalent polar, molecular; B (Na3N) - ionic, ionic | A (NH3) -covalent polar, molecular; B (NaCl) - ionic, ionic | A (MgF2) -ionic, ionic B (CO2) - covalent polar, molecular; | A (H2S) -covalent polar, molecular; B (Na2O) - ionic, ionic | A (СCl4) -covalent polar, molecular; B (BaO) - ionic, ionic |
|
| 280 * 0.05 +12 \u003d 54g | (80*0,05 + 200*0,08)/ (200+80)=7,14% | 120 * 0.025 + 10 * 0.05 \u003d 3.5g | 200*0,08/(200+ 120)=5% | 200*0,01/(200-20*1)=11% |
Test questions on the topic:
The structure of the atom. Periodic law and periodic system of elements D.I. Mendeleev (grade 8)
How the radii of atoms change in the period:
a) increase
b) decrease
c) do not change
How the radii of atoms in the main subgroups change:
a) increase
b) decrease
c) do not change
How to determine the number of energy levels in an atom of an element:
a) by the ordinal number of the element
b) by group number
c) by row number
d) by period number
How is the place of a chemical element in the periodic system determined by D.I. Mendeleev:
a) the number of electrons at the external level
b) the number of neutrons in the nucleus
c) the charge of the atomic nucleus
d) atomic mass
How many energy levels does a scandium atom have:
What determines the properties of chemical elements:
a) the value of the relative atomic mass
b) the number of electrons on the outer layer
c) the charge of the atomic nucleus
d) the number of valence electrons
How do the chemical properties of elements change during the period:
a) strengthened metal
b) non-metallic
c) metal weaken
d) non-metallic
Indicate the element that heads the large period of the periodic table of elements:
Which element has the most pronounced metallic properties:
a) Magnesium
b) Aluminum
c) Silicon
10. Which element has the most pronounced non-metallic properties:
a) Oxygen
11. What is the main reason for the change in the properties of elements in periods:
a) in an increase in atomic masses
b) in a gradual increase in the number of electrons at the external energy level
c) in an increase in the number of electrons in an atom
d) in increasing the number of neutrons in the nucleus
12. Which element heads the main subgroup of the fifth group:
a) vanadium
c) phosphorus
d) arsenic
13. What is the formula of the higher oxide formed by an element of the sixth group:
14. Which element forms a volatile hydrogen compound:
15. What is an orbital:
a) a certain energy level at which the electron is located
b) the space around the nucleus where the electron is
c) the space around the nucleus, where the probability of finding an electron is greatest
d) the trajectory along which the electron moves
16. In which orbital the electron has the highest energy:
17. Determine which element is 1s 2 2s 2 2p 1:
18. Determine the lowest valence of bromine on the periodic table:
19. What element has the structure of the outer electron layer ... 3s 2 p 6:
20. Based on the incomplete electronic formula, determine what properties the element 1s 2 2s 2 2p 5 has:
a) metal
b) non-metal
c) amphoteric element
d) inert element