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A molecule contains two σ- and two π-bonds and one lone pair of electrons in the valence shell of central atom. The arrangement of lone pair as well as bond pairs is
- a)square planar
- b)trigonal planar
- c)linear
- d)tetrahedral
Correct answer is option 'B'. Can you explain this answer?
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A molecule contains twoσ-and twoπ-bonds and one lone pair of ...
Since there are three sigma bond equivalents, therefore hybridisation should be sp2 (lone pair = 1 sigma bond equivalent, and two sigma bonds). So, the structure should be trigonal planar, but bond angle will be a little contracted due to lone pair and bond pair repulsion.
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A molecule contains twoσ-and twoπ-bonds and one lone pair of ...
Trigonal Planar Arrangement
- The molecule described in the question has two sigma bonds and two pi bonds, which indicate a total of four bond pairs around the central atom.
- Additionally, there is one lone pair of electrons present in the valence shell of the central atom.
- In a trigonal planar arrangement, the central atom is surrounded by three electron pairs (either bonding pairs or lone pairs) that are arranged in a flat, triangular shape.
- The lone pair of electrons will occupy one of the positions in the trigonal planar arrangement, while the remaining three positions will be occupied by the bonding pairs.
- This arrangement results in a trigonal planar molecular geometry, which is the most stable configuration for the given set of electron pairs in the molecule.
- Therefore, the correct arrangement of the lone pair as well as bond pairs in the molecule is trigonal planar.
By following the rules of valence shell electron pair repulsion (VSEPR) theory, we can determine the most likely molecular geometry for a molecule based on the number of bond pairs and lone pairs present around the central atom. In this case, the trigonal planar arrangement best fits the description provided in the question.
- The molecule described in the question has two sigma bonds and two pi bonds, which indicate a total of four bond pairs around the central atom.
- Additionally, there is one lone pair of electrons present in the valence shell of the central atom.
- In a trigonal planar arrangement, the central atom is surrounded by three electron pairs (either bonding pairs or lone pairs) that are arranged in a flat, triangular shape.
- The lone pair of electrons will occupy one of the positions in the trigonal planar arrangement, while the remaining three positions will be occupied by the bonding pairs.
- This arrangement results in a trigonal planar molecular geometry, which is the most stable configuration for the given set of electron pairs in the molecule.
- Therefore, the correct arrangement of the lone pair as well as bond pairs in the molecule is trigonal planar.
By following the rules of valence shell electron pair repulsion (VSEPR) theory, we can determine the most likely molecular geometry for a molecule based on the number of bond pairs and lone pairs present around the central atom. In this case, the trigonal planar arrangement best fits the description provided in the question.
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A molecule contains twoσ-and twoπ-bonds and one lone pair of electrons in the valence shell of central atom. The arrangement of lone pair as well as bond pairs isa)square planarb)trigonal planarc)lineard)tetrahedralCorrect answer is option 'B'. Can you explain this answer?
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