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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 because
- a)Oxygen atom does not have d-orbitals
- b)Oxygen atom has two unpaired electrons in its valence shell
- c)Oxygen can form a double bond with another oxygen atom
- d)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small size
Correct answer is option 'A'. Can you explain this answer?
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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 o...
Oxygen does not have a d-orbital thereby not exceeding its covalency beyond 2. Whereas sulphur has vacant d-orbitals hence can exceed its covalency to +4 or +6.
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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 o...
Answer:
Oxygen atom does not have d-orbitals
The correct answer for why the covalency of oxygen cannot exceed 2 is option A, which states that oxygen atom does not have d-orbitals. This means that the oxygen atom does not have any available d-orbitals to participate in bonding. Let's delve into this explanation further.
Valence shell electronic configuration of oxygen
The atomic number of oxygen is 8, which means it has 8 electrons. The electronic configuration of oxygen is 1s² 2s² 2p⁴. In its valence shell (2s² 2p⁴), there are a total of 6 electrons.
Formation of covalent bonds
Oxygen has a valency of 2, which means it can form 2 covalent bonds. In a covalent bond, two atoms share electrons to achieve a stable electronic configuration. Oxygen has a tendency to gain 2 electrons to complete its octet.
Lack of d-orbitals in oxygen
The d-orbitals are present in the third shell (n=3) and beyond. Oxygen, being in the second period, does not have any d-orbitals. It only has 2s and 2p orbitals available for bonding. Therefore, the covalency of oxygen is limited to a maximum of 2.
Comparison with sulphur
Sulphur, on the other hand, is in the third period and has access to the d-orbitals. Hence, it can exhibit a covalency of 4 or even 6. The electronic configuration of sulphur is 1s² 2s² 2p⁶ 3s² 3p⁴ 3d⁰.
Formation of multiple bonds by oxygen
Although oxygen cannot exceed a covalency of 2, it can form a double bond with another oxygen atom. In this case, oxygen shares two pairs of electrons with another oxygen atom, resulting in a double bond. The double bond helps oxygen achieve a stable electronic configuration.
Limitation due to small size
The small size of the oxygen atom also plays a role in its limited covalency. The small size restricts the possibility of promoting its electrons to higher energy levels, such as the d-orbitals. The promotion of electrons to higher energy levels requires a larger atomic size, which oxygen lacks.
In conclusion, the covalency of oxygen cannot exceed 2 because it does not have d-orbitals available for bonding, and its small size prevents the promotion of electrons to higher energy levels.
Oxygen atom does not have d-orbitals
The correct answer for why the covalency of oxygen cannot exceed 2 is option A, which states that oxygen atom does not have d-orbitals. This means that the oxygen atom does not have any available d-orbitals to participate in bonding. Let's delve into this explanation further.
Valence shell electronic configuration of oxygen
The atomic number of oxygen is 8, which means it has 8 electrons. The electronic configuration of oxygen is 1s² 2s² 2p⁴. In its valence shell (2s² 2p⁴), there are a total of 6 electrons.
Formation of covalent bonds
Oxygen has a valency of 2, which means it can form 2 covalent bonds. In a covalent bond, two atoms share electrons to achieve a stable electronic configuration. Oxygen has a tendency to gain 2 electrons to complete its octet.
Lack of d-orbitals in oxygen
The d-orbitals are present in the third shell (n=3) and beyond. Oxygen, being in the second period, does not have any d-orbitals. It only has 2s and 2p orbitals available for bonding. Therefore, the covalency of oxygen is limited to a maximum of 2.
Comparison with sulphur
Sulphur, on the other hand, is in the third period and has access to the d-orbitals. Hence, it can exhibit a covalency of 4 or even 6. The electronic configuration of sulphur is 1s² 2s² 2p⁶ 3s² 3p⁴ 3d⁰.
Formation of multiple bonds by oxygen
Although oxygen cannot exceed a covalency of 2, it can form a double bond with another oxygen atom. In this case, oxygen shares two pairs of electrons with another oxygen atom, resulting in a double bond. The double bond helps oxygen achieve a stable electronic configuration.
Limitation due to small size
The small size of the oxygen atom also plays a role in its limited covalency. The small size restricts the possibility of promoting its electrons to higher energy levels, such as the d-orbitals. The promotion of electrons to higher energy levels requires a larger atomic size, which oxygen lacks.
In conclusion, the covalency of oxygen cannot exceed 2 because it does not have d-orbitals available for bonding, and its small size prevents the promotion of electrons to higher energy levels.
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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer?
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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer?.
Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer?.
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Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 becausea)Oxygen atom does not have d-orbitalsb)Oxygen atom has two unpaired electrons in its valence shellc)Oxygen can form a double bond with another oxygen atomd)Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small sizeCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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