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(a).Taking example of ethene molecule Sp^2 hybridisation.
(b). NH3 has higher boiling point than PH3, why?
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Answers
Explanation:
a)Learning Objective
Recognize the role of sp2 hybridized atoms in sigma and pi bonding.
Key Points
For boron to bond with three fluoride atoms in boron trifluoride (BF3), the atomic s- and p-orbitals in boron’s outer shell mix to form three equivalent sp2 hybrid orbitals.
In an ethene molecule, a double bond between carbons forms with one sigma and one pi bond.
The sigma bond in the C=C for ethene forms between two sp2 hybrid orbitals of two carbon atoms, and a pi bond for between two p orbitals.
Terms
sp2 hybridizationthe 2s orbital mixes with only two of the three available 2p orbitals
hybridizationmixing atomic orbitals into new hybrid orbitals, suitable for pairing electrons to form chemical bonds in valence bond theory
b)The boiling point of NH3 is higher than that of PH3 due to hydrogen bonding in the former. Unlike NH3, PH3molecules are not associated through hydrogen bonding in liquid state. That is why the boiling point of NH3is higher than
Answer:
In an ethene molecule, a double bond between carbons forms with one sigma and one pi bond.
The sigma bond in the C=C for ethene forms between two Sp² hybrid orbitals of two carbon atoms, and a pi bond for between two p orbitals.
Explanation:
Sp² hybridization:
The 2s orbital mixes with only two of the three available 2p orbitals hybridization mixing atomic orbitals into new hybrid orbitals, suitable for pairing electrons to form chemical bonds in valence bond theory.
Ethene (C2H4) has a double bond between the carbons. In this case, carbon will sp² hybridize; in sp² hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp hybrid orbitals with one p-orbital remaining. The three hybridized orbitals explain the three sigma bonds that each carbon forms.
sp² hybridization in etheneIn sp² hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp² orbitals with one p-orbital remaining.
The two carbon atoms form a sigma bond in the molecule by overlapping two sp2 orbitals. Each carbon atom forms two covalent bonds with hydrogen by s–sp² overlap, all with 120° angles. The pi bond between the carbon atoms perpendicular to the molecular plane is formed by 2p–2p overlap.
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