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Which of the following hydrocarbons has the lowest dipole moment?
- a)cis-2-butene
- b)2-butyne
- c)1-butyne
- d)H2C = CH−C ≡ CH
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
Which of the following hydrocarbons has the lowest dipole moment?a)ci...
CH3−C≡C−CH3 : symmetric
The given molecule has linear shape and symmetric from both side, So, it will have zero dipole moment. The remaining three option will have non-zero dipole moment.
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Which of the following hydrocarbons has the lowest dipole moment?a)ci...
Explanation:
The dipole moment of a molecule is a measure of its polarity. It is the product of the magnitude of the charge and the distance between the charges. A molecule with a dipole moment will have a positive and negative end, while a molecule with no dipole moment will have an equal distribution of charge.
To determine the dipole moment of each hydrocarbon, we need to examine the molecular structure and the electronegativity of the atoms involved.
a) cis-2-butene:
Cis-2-butene has a double bond between two carbon atoms. The carbon-carbon double bond is formed by the overlap of sp2 hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the double bond is fairly symmetrical. As a result, cis-2-butene does not have a significant dipole moment.
b) 2-butyne:
2-Butyne has a triple bond between two carbon atoms. The carbon-carbon triple bond is formed by the overlap of sp hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the triple bond is fairly symmetrical. As a result, 2-butyne does not have a significant dipole moment.
c) 1-butyne:
1-Butyne also has a triple bond between two carbon atoms. The carbon-carbon triple bond is formed by the overlap of sp hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the triple bond is fairly symmetrical. As a result, 1-butyne does not have a significant dipole moment.
d) H2C = CH−C ≡ CH:
This molecule is a cumulene, which has alternating double and triple bonds between carbon atoms. The carbon-carbon double bond and triple bond are formed by the overlap of sp2 and sp hybrid orbitals, respectively. The electronegativity of carbon is relatively low, so the electron distribution in the double and triple bonds is fairly symmetrical. As a result, H2C = CH−C ≡ CH does not have a significant dipole moment.
Conclusion:
Out of the given hydrocarbons, 2-butyne has the lowest dipole moment. This is because the electron distribution in the triple bond is fairly symmetrical, resulting in a molecule with no significant dipole moment.
The dipole moment of a molecule is a measure of its polarity. It is the product of the magnitude of the charge and the distance between the charges. A molecule with a dipole moment will have a positive and negative end, while a molecule with no dipole moment will have an equal distribution of charge.
To determine the dipole moment of each hydrocarbon, we need to examine the molecular structure and the electronegativity of the atoms involved.
a) cis-2-butene:
Cis-2-butene has a double bond between two carbon atoms. The carbon-carbon double bond is formed by the overlap of sp2 hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the double bond is fairly symmetrical. As a result, cis-2-butene does not have a significant dipole moment.
b) 2-butyne:
2-Butyne has a triple bond between two carbon atoms. The carbon-carbon triple bond is formed by the overlap of sp hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the triple bond is fairly symmetrical. As a result, 2-butyne does not have a significant dipole moment.
c) 1-butyne:
1-Butyne also has a triple bond between two carbon atoms. The carbon-carbon triple bond is formed by the overlap of sp hybrid orbitals. The electronegativity of carbon is relatively low, so the electron distribution in the triple bond is fairly symmetrical. As a result, 1-butyne does not have a significant dipole moment.
d) H2C = CH−C ≡ CH:
This molecule is a cumulene, which has alternating double and triple bonds between carbon atoms. The carbon-carbon double bond and triple bond are formed by the overlap of sp2 and sp hybrid orbitals, respectively. The electronegativity of carbon is relatively low, so the electron distribution in the double and triple bonds is fairly symmetrical. As a result, H2C = CH−C ≡ CH does not have a significant dipole moment.
Conclusion:
Out of the given hydrocarbons, 2-butyne has the lowest dipole moment. This is because the electron distribution in the triple bond is fairly symmetrical, resulting in a molecule with no significant dipole moment.
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Which of the following hydrocarbons has the lowest dipole moment?a)cis-2-buteneb)2-butynec)1-butyned)H2C = CH−C ≡ CHCorrect answer is option 'B'. Can you explain this answer?
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