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Which type of overlapping is shown by p (px,py and pz) - orbitals?
- a)Two end to end and one sidewise overlap
- b)Two sidewise and one end to end overlap
- c)Three sidewise overlaps
- d)Three end to end overlaps
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
Which type of overlapping is shown by p (px,py and pz) - orbitals?a)Tw...
pz orbital by convention undergoes end to end overlapping and pxpy undergo sidewise overlapping.
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Which type of overlapping is shown by p (px,py and pz) - orbitals?a)Tw...
Explanation:
1. Introduction:
In chemistry, orbitals are regions of space where an electron is likely to be found. Orbitals can overlap with each other to form molecular orbitals, which are responsible for chemical bonding. The type of overlapping between orbitals determines the nature and strength of the bond formed.
2. Overlapping of p-orbitals:
The p-orbitals are dumbbell-shaped and can overlap in different ways to form bonds. There are three p-orbitals: px, py, and pz. Let's consider the overlapping possibilities for these orbitals.
3. Two sidewise and one end to end overlap:
Option B states that the overlapping of p-orbitals involves two sidewise overlaps and one end to end overlap. This means that two p-orbitals overlap sideways, while the third p-orbital overlaps end to end with the other two.
4. Sidewise overlap:
In sidewise overlap, the lobes of the p-orbitals align parallel to each other. This results in the formation of a pi (π) bond, which is a type of bond that occurs in double and triple bonds. The pi bond is weaker than the sigma (σ) bond formed by end to end overlap.
5. End to end overlap:
In end to end overlap, the lobes of the p-orbitals align along the internuclear axis. This results in the formation of a sigma (σ) bond, which is a strong bond formed by the head-on interaction of orbitals.
6. Conclusion:
Based on the explanation above, option B is the correct answer. The overlapping of p-orbitals involves two sidewise overlaps and one end to end overlap. This type of overlapping leads to the formation of sigma and pi bonds, which play a crucial role in the structure and properties of molecules.
1. Introduction:
In chemistry, orbitals are regions of space where an electron is likely to be found. Orbitals can overlap with each other to form molecular orbitals, which are responsible for chemical bonding. The type of overlapping between orbitals determines the nature and strength of the bond formed.
2. Overlapping of p-orbitals:
The p-orbitals are dumbbell-shaped and can overlap in different ways to form bonds. There are three p-orbitals: px, py, and pz. Let's consider the overlapping possibilities for these orbitals.
3. Two sidewise and one end to end overlap:
Option B states that the overlapping of p-orbitals involves two sidewise overlaps and one end to end overlap. This means that two p-orbitals overlap sideways, while the third p-orbital overlaps end to end with the other two.
4. Sidewise overlap:
In sidewise overlap, the lobes of the p-orbitals align parallel to each other. This results in the formation of a pi (π) bond, which is a type of bond that occurs in double and triple bonds. The pi bond is weaker than the sigma (σ) bond formed by end to end overlap.
5. End to end overlap:
In end to end overlap, the lobes of the p-orbitals align along the internuclear axis. This results in the formation of a sigma (σ) bond, which is a strong bond formed by the head-on interaction of orbitals.
6. Conclusion:
Based on the explanation above, option B is the correct answer. The overlapping of p-orbitals involves two sidewise overlaps and one end to end overlap. This type of overlapping leads to the formation of sigma and pi bonds, which play a crucial role in the structure and properties of molecules.
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Which type of overlapping is shown by p (px,py and pz) - orbitals?a)Tw...
pz orbital by convention undergoes end to end overlapping and pxpy undergo sidewise overlapping.
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Which type of overlapping is shown by p (px,py and pz) - orbitals?a)Two end to end and one sidewise overlapb)Two sidewise and one end to end overlapc)Three sidewise overlapsd)Three end to end overlapsCorrect answer is option 'B'. Can you explain this answer?
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