Здравствуйте, Уважаемые Студенты! Обращаю Ваше внимание на то, что не все ФИ идентифицированы, поэтому пожалуйста подписывайтесь. Что же Вас ожидает сегодня.... 1. Grammar Test 4 - материалы предоставляются на занятии, позже публикуются в Вашем блоге. 2. Pronunciation - http://usefulenglish.ru/phonetics/practice-consonant-contrast 3. Lecture - https://studfiles.net/preview/5708252/page:19/ * Составьте 20 вопросов по тексту лекции. 4. Speaking - https://learnenglish.britishcouncil.org/advanced-c1-listening/tech-addiction Выразите своё мнение по данной теме 15-20 предложений, не забывайте воспользоваться словарём! Keys to punctuation task: Nobody seemed to care about Mary . She was born in India , where her father was a British official . He was busy with his work , and her mother , who was very beautiful , spent all her time going to parties . So an Indian woman , Kamala , was paid to take care of the little girl . Mary was not a pretty child . ...
1. a. Atomic radius decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase. b. Atomic radius increases from top to bottom within group. There is an increase in the positive nuclear charge. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels.
ОтветитьУдалить2. a. Ionization energy increases from left to right across a period. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required. b. Ionization energy decreases from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom.
3. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Halogens have the highest electronegativities. b. Alkali metals have the lowest electronegativities
6. d
7. b
8. a. P b. O c. Li d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na b. Br c. Ca2+ d. the same
11. a. F b. S c. Be d. Al
12. c
13. Al Na K Cs
14. P N O F
15. Na+ ion is likely to form because of formation of stable noble gas configuration, therefore Na2+ ion is unlikely to form.
Вахрушева Дарья
1. a. Atomic radius decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase. b. Atomic radius increases from top to bottom within group. There is an increase in the positive nuclear charge. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels.
ОтветитьУдалить2. a. Ionization energy increases from left to right across a period. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required. b. Ionization energy decreases from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom.
3. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Halogens have the highest electronegativities. b. Alkali metals have the lowest electronegativities
6. d
7. b
8. a. P b. O c. Li d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na b. Br c. Ca2+ d. the same
11. a. F b. S c. Be d. Al
12. c
13. Al Na K Cs
14. P N O F
15. Na+ ion is likely to form because of formation of stable noble gas configuration, therefore Na2+ ion is unlikely to form.
Grammar test 2: 87%
ОтветитьУдалитьGrammar test 2- 86%
ОтветитьУдалитьGrammar test 87%
ОтветитьУдалитьGrammar test 2-85%
ОтветитьУдалитьGrammar test 2 - 77%
ОтветитьУдалить1.a)Atomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge. Since the force of attraction between the nuclei and electrons increases, the size of the atoms decreases. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase.
ОтветитьУдалитьb)The atomic radius of atoms generally increases from top to bottom within a group. As the atomic number increases down a group, there is again an increase in the positive nuclear charge. However, there is also an increase in the number of occupied principal energy levels. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels. This effect outweighs the increase in nuclear charge, so atomic radius increases down a group.
2.a)The ionization energy of atoms generally increases from left to right across each row of the periodic table. The reason for this increase in ionization energy is the increase in nuclear charge. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required.
b)The ionization energies of the representative elements generally decrease from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom. The attractive force between the valence electron and the nucleus weakens as the distance between them increases, resulting in a lower ionization energy for the larger atoms within a group.
3.Thee second ionization energy of an element is always higher than the first, the third is always higher than the second, and so on. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4.The energy change that occurs when a neutral atom gains an electron is called its electron affinity. When energy is released in a chemical reaction or process, that energy is expressed as a negative number.
5.a)The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities.
b) In general, electron affinities increase (become more negative) from left to right across a period and decrease (become less negative) from top to bottom down a group.
6.a)K b)S c)Br d)Cs
ОтветитьУдалить7.b
8.a)P b)O c)Li d)Ne
9.This is because after two ionizations, a stable positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a third electron is therefore more difficult.
10.a)Na b)Br- c)Ca 2+ d)O 2-
11.a)F b)S c)Be d) Al
12.a
13.Al,Na,K,Cs
14.P,N,O,F
15.As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Grammar test 1 - 83%
ОтветитьУдалитьa. Atomic radius decreases from left to right across a period. b. Atomic radius increases from top to bottom within group.
Удалить2. a. Ionization energy increases from left to right across a period.
b. Ionization energy decreases from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group.
3. Second ionization energy is larger than the first one because after one ionization, a positively charged ion is formed. Because of that, there is a greater overall attractive force on the remaining electrons, so removing a second electron is therefore more difficult.
4.The most electron affinities are negative numbers, because the process of gaining electrons is accompanied by a process of releasing energy. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the
5. a. Halogens have the highest electronegativities. b. Alkali metals have the lowest electronegativities
6. d
7. b
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na
b. Br
c. Ca2+
d. Equal
11. a. F
b. S
c. Be
d. Al
12. c
13. Al Na K Cs
14. P N O F
15. Na2+ ion is unlikely to form, because Na has the most stable formation as an ion being Na+ as it has a stable noble gas configuration.
Reading/Translating Test -- 93%
ОтветитьУдалитьGrammar test 95%
ОтветитьУдалитьАлимханова Лилия
Алимханова Лилия
ОтветитьУдалить1. a. Atomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.
b. Atomic radius of atoms generally increases from top to bottom within a group.
2. a. Ionization energy of atoms generally increases from left to right across each row of the periodic table.
b. Ionization energies of the representative elements generally decrease from top to bottom within a group.
3. After one ionization, a positively charged ion is formed. There is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Halogens have the highest electronegativities.
b. Alkali metals have the lowest electronegativities.
6. a. K
b. S
c. Br
d. Cs
7. b
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na
b. Br-
c. Ca2+
d. The same
11. a. F
b. S
c. Be
d. Al
12. a
13. Al, Na, K, Cs
14. P, N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Grammar test 2 - 74%
УдалитьGrammar test 2 76%
ОтветитьУдалитьReading/Translating Test - 88%
ОтветитьУдалитьGrammar test 2- 77%
ОтветитьУдалитьReading/Translating Test -87%
ОтветитьУдалитьReading/translating test 83%
ОтветитьУдалитьGrammar test 2 - 81%
ОтветитьУдалитьReading/translating - 87%
УдалитьGrammar test 2 - 80%
ОтветитьУдалитьМамонтова Мария
1. a. Atomic radius decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge. Since the force of attraction between the nuclei and electrons increases, the size of the atoms decreases. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase.
ОтветитьУдалить1. b. The atomic radius of atoms generally increases from top to bottom within a group. As the atomic number increases down a group, there is again an increase in the positive nuclear charge. However, there is also an increase in the number of occupied principal energy levels. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels. This effect outweighs the increase in nuclear charge, so atomic radius increases down a group.
2. a. The ionization energy of atoms generally increases from left to right across each row of the periodic table. The reason for this increase in ionization energy is the increase in nuclear charge. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required.
b. The ionization energies of the representative elements generally decrease from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom. The attractive force between the valence electron and the nucleus weakens as the distance between them increases, resulting in a lower ionization energy for the larger atoms within a group. Although the nuclear charge is increased for larger atoms, the shielding effect also increases due to the presence of a larger number of inner electrons. This is particularly easy to see in the alkali metals, where the single valence electron is shielded by all of the inner core electrons.
3. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
@
Мамонтова Мария.
часть 2.
Удалить5. a. Halogens have the highest electronegativities.
b. Alkali metals have the lowest electronegativities.
6.
a. K
b. S
c. Br
d. Cs
7. b.
8.
a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10.
a. Na
b. Br-
c. Ca2+
d. The same
11.
a. F
b. S
c. Be
d. Al
12. с.
13. Al, Na, K, Cs
14. P, N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
@
Мамонтова Мария.
1. a. Atomic radius decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase. b. Atomic radius increases from top to bottom within group. There is an increase in the positive nuclear charge. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels.
ОтветитьУдалить2. a. Ionization energy increases from left to right across a period.
b. Ionization energy decreases from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group.
3.Thee second ionization energy of an element is always higher than the first, the third is always higher than the second, and so on. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4.The most electron affinities are negative numbers, because the process of gaining electrons is accompanied by a process of releasing energy. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the
5. a. Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Halogens have the highest electronegativities. b. Alkali metals have the lowest electronegativities
6.
a. K
b. S
c. Br
d. Cs
7. b.
8.
a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10.a)Na b)Br- c)Ca 2+ d)O 2-
11.a)F b)S c)Be d) Al
12.a
13.Al,Na,K,Cs
14.P,N,O,F
15. Na+ ion is likely to form because of formation of stable noble gas configuration, therefore Na2+ ion is unlikely to form.
1. a. Atomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.
ОтветитьУдалитьb. Atomic radius of atoms generally increases from top to bottom within a group.
2. a. Ionization energy of atoms generally increases from left to right across each row of the periodic table.
b. Ionization energies of the representative elements generally decrease from top to bottom within a group.
3. After one ionization, a positively charged ion is formed. There is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Halogens have the highest electronegativities.
b. Alkali metals have the lowest electronegativities.
6. a. K
b. S
c. Br
d. Cs
7. b
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na
b. Br-
c. Ca2+
d. The same
11. a. F
b. S
c. Be
d. Al
12. a
13. Al, Na, K, Cs
14. P, N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Grammar Test 2-77%
ОтветитьУдалить1. а) Аtomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.
ОтветитьУдалитьb) Atomic radius increases from top to bottom within group. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge. Since the force of attraction between the nuclei and electrons increases, the size of the atoms decreases. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase.
2. a)The ionization energy of atoms generally increases from left to right across each row of the periodic table. The reason for this increase in ionization energy is the increase in nuclear charge. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required.
b) The ionization energies of the representative elements generally decrease from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom. The attractive force between the valence electron and the nucleus weakens as the distance between them increases, resulting in a lower ionization energy for the larger atoms within a group. Although the nuclear charge is increased for larger atoms, the shielding effect also increases due to the presence of a larger number of inner electrons. This is particularly easy to see in the alkali metals, where the single valence electron is shielded by all of the inner core electrons.
3. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a) Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Halogens have the highest electronegativities.
b)Alkali metals have the lowest electronegativities.
6. a) K
b) S
c) Br
d) Cs
7. b)
8. a) P
b) O
c) Li
d) Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a) Na
b) Br
c) Ca2+
d) Equal
11. а) F
b) S
c) Be
d) Al
12. с)
13. Al, Na, K, Cs
14. Р,N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Панкова
Grammar test 2 - 76%
ОтветитьУдалитьГорохова Виктория
ОтветитьУдалитьGrammar test: 87%
Горохова Виктория
ОтветитьУдалитьReading test:
1. a) Atomic radius generally decreases from left to right across a period.
b) Atomic radius increases from top to bottom within a group.
2. a) Ionization energy generally increases from left to right across the period.
b) Ionization energy decreases from top to bottom within a group.
3. The second ionization energy is always higher than the second because after one ionization, a positively charged ion is formed.
4. When energy is released in a chemical reaction that energy is expressed as a negative number.
5. a) Halogens have the highest electronegativities.
b) Alkali metals have the lowest electronegativities.
6. a) P
b) S
c) Br
d) Cs
7. b
8. a) P
b) O
c) Li
d) Ne
10. a) Na
b) Br
c) Ca 2+
d) the same
11. a) F
b) S
c) Be
d) Al
12. c
13. Al, Na, K, Cs
14. P, N, O, F
Grammar test - 82%
ОтветитьУдалитьМария Виноградова
ОтветитьУдалить1. a. Atomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.
b. Atomic radius of atoms generally increases from top to bottom within a group.
2. a. Ionization energy of atoms generally increases from left to right across each row of the periodic table.
b. Ionization energies of the representative elements generally decrease from top to bottom within a group.
3. After one ionization, a positively charged ion is formed. There is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Halogens have the highest electronegativities.
b. Alkali metals have the lowest electronegativities.
6. a. K
b. S
c. Br
d. Cs
7. b
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na
b. Br-
c. Ca2+
d. The same
11. a. F
b. S
c. Be
d. Al
12. a
13. Al, Na, K, Cs
14. P, N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Reading/Translating Test 86%
ОтветитьУдалить1. a. Atomic radius decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen. The effect lessens as one moves farther to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase. b. Atomic radius increases from top to bottom within group. There is an increase in the positive nuclear charge. Higher principal energy levels consist of orbitals that are larger in size than the orbitals from lower energy levels.
ОтветитьУдалить2. a. Ionization energy increases from left to right across a period. A nucleus containing more protons has a larger total positive charge, which results in a greater attractive force being applied to each electron. If the valence electrons are held more tightly to the nucleus by this stronger force, they are more difficult to remove, and more ionization energy is required. b. Ionization energy decreases from top to bottom within a group. This trend is explained by the increase in size of the atoms within a group. The valence electron that is being removed is farther from the nucleus in the case of a larger atom.
3. This is because after one ionization, a positively charged ion is formed. At this point, there is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Electronegativities generally increase from left to right across a period. This is due to an increase in nuclear charge. Halogens have the highest electronegativities. b. Alkali metals have the lowest electronegativities
6. a. K
b. S
c. Br
d. Cs
7. b.
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10.a)Na b)Br- c)Ca 2+ d)O 2-
11.a)F b)S c)Be d) Al
12.a
13.Al,Na,K,Cs
14.P,N,O,F
15. Na+ ion is likely to form because of formation of stable noble gas configuration, therefore Na2+ ion is unlikely to form.
Ковалишин Михаил
ОтветитьУдалить1. a. Atomic radius generally decreases from left to right across a period, although there are some small exceptions to this trend, such as the relative radii of oxygen and nitrogen.
b. Atomic radius of atoms generally increases from top to bottom within a group.
2. a. Ionization energy of atoms generally increases from left to right across each row of the periodic table.
b. Ionization energies of the representative elements generally decrease from top to bottom within a group.
3. After one ionization, a positively charged ion is formed. There is a greater overall attractive force on the remaining electrons because the protons now outnumber the electrons. Removing a second electron is therefore more difficult.
4. When energy is released in a chemical reaction or process, that energy is expressed as a negative number. The elements of the halogen group (Group 17) gain electrons most readily, as can be seen from their large negative electron affinities. The outer configuration of all halogens is ns2np5. The addition of one more electron gives the halide ions the same electron configuration as a noble gas, which we have seen is particularly stable.
5. a. Halogens have the highest electronegativities.
b. Alkali metals have the lowest electronegativities.
6. a. K
b. S
c. Br
d. Cs
7. b
8. a. P
b. O
c. Li
d. Ne
9. The difference between the second and third ionization energies (IE2 and IE3) of calcium so much larger than the difference between its first and second ionization energies, because calcium has only 2 valence electrons. And if calcium loses 2 electrons, it will have a stable noble gas electron configuration.
10. a. Na
b. Br-
c. Ca2+
d. The same
11. a. F
b. S
c. Be
d. Al
12. a
13. Al, Na, K, Cs
14. P, N, O, F
15. As an alkali metal, its first ionization energy is very low. After it loses its valence electron (the 2s electron), it becomes a sodium ion, Na+, which has an electron configuration of 1s2. This is the electron configuration of the noble gas neon. The second ionization energy of sodium shows an extremely large jump compared to the first because the removal of a second electron requires breaking apart the noble gas electron configuration.
Ковалишин Михаил
ОтветитьУдалитьGrammar test 2 - 80%