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What are the hybridization and shapes of the following molecules?
(i) CH3F
(ii) HC ≡ N
(i) CH3F
(ii) HC ≡ N
- a)(i) sp2, trigonal planar; (ii) sp3, tetrahedral
- b)(i) sp3, tetrahedral; (ii) sp, linear
- c)(i) sp, linear; (ii) sp2, trigonal planar
- d)(i) sp2, trigonal planar, (ii) sp2, trigonal planar
Correct answer is option 'B'. Can you explain this answer?
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What are the hybridization and shapes of the following molecules?(i) C...
CH3F - sp3 hybridised carbon, tetrahedral shape
(ii) HC = N - sp hybridised carbon, linear shape.
(ii) HC = N - sp hybridised carbon, linear shape.
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What are the hybridization and shapes of the following molecules?(i) C...
(i) CH3F:
The central atom in CH3F is carbon, which has the electron configuration 1s2 2s2 2p2. Carbon forms four covalent bonds in this molecule.
To determine the hybridization, we count the number of regions of electron density around the central atom. In this case, we have one single bond to each hydrogen atom, one single bond to the fluorine atom, and one lone pair on carbon. This gives us a total of four regions of electron density.
The hybridization of an atom with four regions of electron density is sp3. Therefore, the carbon atom in CH3F is sp3 hybridized.
The shape of the molecule can be determined by looking at the arrangement of the regions of electron density. In this case, the lone pair and the three bond pairs are arranged in a tetrahedral geometry. However, the presence of a lone pair causes a distortion in the shape.
The lone pair occupies more space than the bond pairs and exerts a stronger repulsion. As a result, the bond angle between the three hydrogen atoms and the fluorine atom is slightly less than 109.5 degrees.
Therefore, the shape of CH3F is trigonal pyramidal.
(ii) HC:
The central atom in HC is carbon, which has the electron configuration 1s2 2s2 2p2. Carbon forms one covalent bond in this molecule.
To determine the hybridization, we count the number of regions of electron density around the central atom. In this case, we have one single bond to the hydrogen atom. This gives us a total of one region of electron density.
The hybridization of an atom with one region of electron density is sp. Therefore, the carbon atom in HC is sp hybridized.
The shape of the molecule can be determined by looking at the arrangement of the regions of electron density. In this case, there is only one bond pair, so there is no specific shape associated with HC. However, the bond angle between the carbon and hydrogen atoms is approximately 180 degrees.
Therefore, the shape of HC is linear.
The central atom in CH3F is carbon, which has the electron configuration 1s2 2s2 2p2. Carbon forms four covalent bonds in this molecule.
To determine the hybridization, we count the number of regions of electron density around the central atom. In this case, we have one single bond to each hydrogen atom, one single bond to the fluorine atom, and one lone pair on carbon. This gives us a total of four regions of electron density.
The hybridization of an atom with four regions of electron density is sp3. Therefore, the carbon atom in CH3F is sp3 hybridized.
The shape of the molecule can be determined by looking at the arrangement of the regions of electron density. In this case, the lone pair and the three bond pairs are arranged in a tetrahedral geometry. However, the presence of a lone pair causes a distortion in the shape.
The lone pair occupies more space than the bond pairs and exerts a stronger repulsion. As a result, the bond angle between the three hydrogen atoms and the fluorine atom is slightly less than 109.5 degrees.
Therefore, the shape of CH3F is trigonal pyramidal.
(ii) HC:
The central atom in HC is carbon, which has the electron configuration 1s2 2s2 2p2. Carbon forms one covalent bond in this molecule.
To determine the hybridization, we count the number of regions of electron density around the central atom. In this case, we have one single bond to the hydrogen atom. This gives us a total of one region of electron density.
The hybridization of an atom with one region of electron density is sp. Therefore, the carbon atom in HC is sp hybridized.
The shape of the molecule can be determined by looking at the arrangement of the regions of electron density. In this case, there is only one bond pair, so there is no specific shape associated with HC. However, the bond angle between the carbon and hydrogen atoms is approximately 180 degrees.
Therefore, the shape of HC is linear.
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What are the hybridization and shapes of the following molecules?(i) CH3F(ii) HC ≡ Na)(i) sp2, trigonal planar; (ii) sp3, tetrahedralb)(i) sp3, tetrahedral; (ii) sp, linearc)(i) sp, linear; (ii) sp2, trigonal planard)(i) sp2, trigonal planar, (ii) sp2, trigonal planarCorrect answer is option 'B'. Can you explain this answer?
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What are the hybridization and shapes of the following molecules?(i) CH3F(ii) HC ≡ Na)(i) sp2, trigonal planar; (ii) sp3, tetrahedralb)(i) sp3, tetrahedral; (ii) sp, linearc)(i) sp, linear; (ii) sp2, trigonal planard)(i) sp2, trigonal planar, (ii) sp2, trigonal planarCorrect answer is option 'B'. 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 What are the hybridization and shapes of the following molecules?(i) CH3F(ii) HC ≡ Na)(i) sp2, trigonal planar; (ii) sp3, tetrahedralb)(i) sp3, tetrahedral; (ii) sp, linearc)(i) sp, linear; (ii) sp2, trigonal planard)(i) sp2, trigonal planar, (ii) sp2, trigonal planarCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for What are the hybridization and shapes of the following molecules?(i) CH3F(ii) HC ≡ Na)(i) sp2, trigonal planar; (ii) sp3, tetrahedralb)(i) sp3, tetrahedral; (ii) sp, linearc)(i) sp, linear; (ii) sp2, trigonal planard)(i) sp2, trigonal planar, (ii) sp2, trigonal planarCorrect answer is option 'B'. Can you explain this answer?.
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